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Chem Unit 2

This document provides examination details for the Pearson Edexcel International Advanced Level Chemistry paper scheduled for January 14, 2021. It includes instructions for candidates, information about the total marks, and a series of questions covering various chemistry topics. Candidates are advised to read the questions carefully and show all workings in calculations.

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0% found this document useful (0 votes)

41 views443 pages

Chem Unit 2

Uploaded by

nyumch07

We take content rights seriously. If you suspect this is your content, claim it here.

Available Formats

Download as PDF, TXT or read online on Scribd

You are on page 1/ 443

Please check the examination details below before entering your candidate information

Candidate surname Other names

Pearson Edexcel Centre Number Candidate Number

International
Advanced Level

Thursday 14 January 2021

Afternoon (1 hour 30 minutes) Paper Reference WCH12/01

Chemistry
International Advanced Subsidiary / Advanced Level
Unit 2: Energetics, Group Chemistry, Halogenoalkanes
and Alcohols
You must have: Total Marks
Scientific calculator, Data booklet, Ruler

Instructions
• Use black ink or black ball-point pen.
• Fill in the boxes at the top of this page with your name,
centre number and candidate number.
• Answer all questions.
• Answer the questions in the spaces provided
– there may be more space than you need.
• Show all your working in calculations and include units where appropriate.
Information
• The total mark for this paper is 80.
• The marks for each question are shown in brackets
– use this as a guide as to how much time to spend on each question.
• toIn the question marked with an asterisk (*) marks will be awarded for your ability
structure your answer logically, showing how the points that you make are
related or follow on from each other where appropriate.
• A Periodic Table is printed on the back cover of this paper.

Advice
• Read each question carefully before you start to answer it.
• Try to answer every question.
• your answers if you have time at the end.
Check

Turn over

P67748A
©2021 Pearson Education Ltd.

1/1/1
*P67748A0128*
SECTION A
Answer ALL the questions in this section.
You should aim to spend no more than 20 minutes on this section.
For each question, select one answer from A to D and put a cross in the box . If you change
your mind, put a line through the box and then mark your new answer with a cross .
1 The energy profile for a reaction is shown.

Energy X products

reactants

Progress of reaction

What is the minimum energy needed for this reaction to occur?

A X
B Y

C X−Y
D X+Y

(Total for Question 1 = 1 mark)

2 Which of these isomers with the formula C8H18 has the lowest boiling temperature?

A CH3CH(CH3)CH2CH2CH(CH3)CH3
B CH3CH(CH3)CH2CH2CH2CH2CH3

C CH3C(CH3)2CH2CH(CH3)CH3

D CH3CH2CH2CH2CH2CH2CH2CH3

(Total for Question 2 = 1 mark)

2
*P67748A0228*
3 Which of these pure compounds has hydrogen bonding in the liquid state?

A 1,1,1-trichloroethane, CH3CCl3

B trimethylamine, (CH3)3N

C hydrogen fluoride, HF
D hydrogen sulfide, H2S

(Total for Question 3 = 1 mark)

4 The hydrogen ion, H+, bonds to a water molecule forming an H3O+ ion.
For H3O+, what shape and H-O-H bond angle are predicted by the
electron-pair repulsion theory?

A trigonal planar 120°

B trigonal planar 117.5°

C trigonal pyramidal 107°

D trigonal pyramidal 104.5°

(Total for Question 4 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

3
*P67748A0328* Turn over
5 The viscosities of four liquid organic compounds are compared by placing the liquids
in separate identical tubes, each with an air bubble at the top.

Air bubble

Liquid

The tubes are inverted, and the times measured for the air bubble to travel the length
of the tube.
For which compound does the air bubble take the longest time?

A
OH
OH
OH
OH

B OH
OH
OH
OH
OH
OH
OH
OH

C
OH
OH
OH
OH
HO
HO
HO
HO OH
OH
OH
OH

D O
OO
O

O
OO
O
O O
OO
O OO
O

O O
OO
O OO
O

(Total for Question 5 = 1 mark)

4
*P67748A0428*
6 This question is about the reaction of potassium iodide with concentrated sulfuric acid.
(a) Which of these would not be seen?
(1)
A misty fumes
B black solid

C yellow solid

D dense white smoke

(b) One of the reaction products is the gas H2S.
What is the change in oxidation number of sulfur as H2S forms?
(1)
A −8

B −6
C −2
D +6

(Total for Question 6 = 2 marks)

7 Iodate(V) ions, IO3−, oxidise dithionate ions, S2O62−, according to the equation

x IO3− + y S2O62− + 4H2O → z SO42− + 8H+ + I2

What are the balancing numbers x, y and z?

x y z

A 2 1 2

B 2 2 4

C 2 5 5

D 2 5 10

(Total for Question 7 = 1 mark)

5
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8 Magnesium reacts with hydrochloric acid.

Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)

Which statement about this reaction is correct?

A magnesium atoms act as oxidising agents

B hydrogen molecules act as reducing agents

C hydrogen ions act as oxidising agents

D chloride ions act as oxidising agents

(Total for Question 8 = 1 mark)

9 Which of these compounds does not produce a colour in a flame test, and produces
an alkaline gas when warmed with sodium hydroxide solution?

A Ca(OH)2
B Mg(OH)2
C NH4Cl

D BeCl2

(Total for Question 9 = 1 mark)

10 Which of these increases as Group 7 is descended?

A oxidising ability of the molecular halogens

B reducing ability of the halide ions

C electrostatic attraction between the nucleus and outer shell of electrons

D electronegativity of the halogen atoms

(Total for Question 10 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

6
*P67748A0628*
11 The table shows the amount of energy released per gram when some alkanes are
burned in excess oxygen under standard conditions.

Energy released
Alkane
/ kJ g−1

methane 55.6

ethane 52.0

propane 50.4

butane 49.6

Which alkane has a standard enthalpy change of combustion of −2877 kJ mol−1?

A methane
B ethane

C propane
D butane

(Total for Question 11 = 1 mark)

12 The enthalpy changes for two reactions are shown.

H+(aq) + OH−(aq) → H2O(l) ΔrH = −57.2 kJ mol−1
CH3COOH(aq) + OH−(aq) → CH3COO−(aq) + H2O(l) ΔrH = −56.0 kJ mol−1

What is the enthalpy change for the dissociation of CH3COOH(aq) into CH3COO−(aq)
and H+(aq) ions, in kJ mol−1?

A +113.2

B +1.2
C −1.2

D −113.2

(Total for Question 12 = 1 mark)

7
*P67748A0728* Turn over
13 What is the skeletal formula of 2-chloro-4,4-dimethylhexane?

A
Cl
Cl
Cl
Cl

Cl
B
Cl
Cl
Cl
Cl

C Cl
Cl
Cl

Cl
Cl
D Cl
Cl

(Total for Question 13 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

8
*P67748A0828*
14 Some alcohols react with concentrated phosphoric(V) acid, H3PO4 , to form alkenes.
(a) What type of reaction occurs?

A addition

B elimination
C hydrolysis

D substitution
(b) The structure of 2-methylpentan-3-ol is shown.
CH₃

H₃C CH₃

This alcohol reacts with concentrated phosphoric(V) acid.

How many different alkenes can form?

A one

B two
C three

D four

(Total for Question 14 = 2 marks)

Use this space for any rough working. Anything you write in this space will gain no credit.

9
*P67748A0928* Turn over
15 Magnesium nitrate decomposes on heating.

2Mg(NO3)2 → 2MgO + 4NO2 + O2

What is the total volume of gas formed at room temperature and pressure (r.t.p.)
when 0.005 mol of magnesium nitrate decomposes completely?
[Molar volume of a gas at r.t.p. = 24 000 cm3 mol−1]

A 600 cm3

B 300 cm3
C 240 cm3

D 120 cm3

(Total for Question 15 = 1 mark)

16 How many moles are there in 15.1 cm3 of liquid propan-1-ol?

[Density of propan-1-ol = 0.80 g cm−3 Mr of propan-1-ol = 60]

A (0.80 × 15.1) ÷ 60
B 0.80 ÷ (60 × 15.1)
C 60 ÷ (0.80 × 15.1)

D (60 × 15.1) ÷ 0.80

(Total for Question 16 = 1 mark)

17 The oxidation of propan-1-ol by acidified potassium dichromate(VI) forms

propanoic acid with a yield of 36 % by mass.
What mass of propan-1-ol is needed to form 37.0 g of propanoic acid in this reaction?
[Mr of propanoic acid = 74 Mr of propan-1-ol = 60]

A 10.8 g

B 36.0 g

C 40.8 g

D 83.3 g

(Total for Question 17 = 1 mark)

10
*P67748A01028*
18 Barium chloride solution, BaCl2(aq), reacts with gallium sulfate solution, Ga2(SO4)3(aq)
to form a precipitate of barium sulfate, BaSO4(s).
What is the minimum volume of 0.100 mol dm−3 barium chloride needed to precipitate
all the sulfate ions in 200 cm3 of 0.05 mol dm−3 gallium sulfate?

A 100 cm3

B 200 cm3

C 300 cm3

D 400 cm3

(Total for Question 18 = 1 mark)

TOTAL FOR SECTION A = 20 MARKS

11
*P67748A01128* Turn over
SECTION B
Answer ALL the questions. Write your answers in the spaces provided.
19 Ethanol can be made in industry by the reaction of ethene with steam, using
a phosphoric(V) acid catalyst.

CH2=CH2(g) + H2O(g) ⇌ CH3CH2OH(g) ΔrH = −45 kJ mol−1

The reaction is carried out at 300°C and 60 atm. An initial yield of 5 % is achieved
when the ethene and steam first pass through the reactor.
*(a) Explain the chemical reasons for the conditions used and why such a
low initial yield is acceptable in the industrial process.
(6)

12
*P67748A01228*
.. .. ... .. ... .. ... .. ... .. ... ... .. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .... .......... .. ........ .......... .......... .......... .......... .......... .......... .......... .......... .......... .......... .......... ...... .............. ..... .................

13
*P67748A01328* Turn over
(b) The product of the reaction is a mixture of ethanol and water.
Explain why ethanol and water mix together fully.
You may find it helpful to draw a diagram.
(3)

(c) Ethanol can be oxidised using a solution of acidified potassium dichromate(VI),

K2Cr2O7(aq).
Ethanoic acid and another organic compound, Y, are both possible products.
(i) Draw the structure of Y.
(1)

(ii) State the conditions needed to maximise the yield of each product.
(2)
Conditions for maximum yield of Y

Conditions for maximum yield of ethanoic acid

(Total for Question 19 = 12 marks)

14
*P67748A01428*
BLANK PAGE

15
*P67748A01528* Turn over
20 The compound DMAA was originally synthesised as a decongestant.
NH2 NH2
DMAA DMAA

A suggested synthetic route for DMAA is shown.

OH Step 1 OHCl Step 2
Step 1 Cl NH2 2
Step

conc. NH3 / heat conc. NH3 / heat

high pressure high pressure
compound A compound A

(a) (i) Give the systematic name of compound A.

(1)

(ii) Identify, by name or formula, a suitable reagent for Step 1.

(1)

(iii) Give the mechanism for the reaction in Step 2.

Include curly arrows, and any relevant dipoles and lone pairs.
(4)

16
*P67748A01628*
(b) DMAA is only slightly soluble in water but dissolves readily in hydrochloric acid to
form an aqueous solution.
NH2 +
NH3
+ HCl −
+ Cl

DMAA
(i) Explain the type of bonding that occurs between the nitrogen atom and the
hydrogen ion, when the positive ion forms.
(3)

(ii) Complete the diagrams to show how the ions formed in the reaction between
DMAA and hydrochloric acid interact with water molecules.
(3)

(Total for Question 20 = 12 marks)

17
*P67748A01728* Turn over
21 This question is about ethanoic acid and some related salts.
(a) A test to confirm the presence of an aqueous acid is adding a small amount of
solid sodium carbonate to the solution.
Describe two observations you would see in this test.
(2)

(b) Sodium ethanoate is a component of reusable hand warmers.

In use, a supersaturated solution of sodium ethanoate recrystallises to form
solid hydrated sodium ethanoate, releasing energy.
CH3COONa(aq) + 3H2O(l) → CH3COONa.3H2O(s) ΔrH = −19.7 kJ mol−1
A hand warmer has a mass of 63.2 g and forms 20.1 g of
hydrated sodium ethanoate on recrystallisation.
Calculate the maximum temperature reached by the hand warmer if its initial
temperature is 5.0°C.
[Specific heat capacity of the hand warmer = 3.0 J °C−1 g−1]
(5)

18
*P67748A01828*
(c) Ammonium ethanoate, CH3COONH4(s), is used to control the pH of foods.
It can be formed by the reaction of pure ethanoic acid, CH3COOH(l), with
ammonium carbonate, (NH4)2CO3(s).
Calculate the standard enthalpy change for this reaction by completing the
Hess cycle and using the data shown.
(5)

Compound Enthalpy change of formation / kJ mol−1

CH3COOH(l) −484.5

(NH4)2CO3(s) −939.9

CH3COONH4(s) −586.3

CO2(g) −393.5

H2O(l) −285.8

19
*P67748A01928* Turn over
(d) Ammonium carbonate, (NH4)2CO3 , is an ingredient in cleaning solutions for
camera lenses.
These are aqueous solutions which contain no more than 1.8 g of
ammonium carbonate in 100 cm3 of solution.
Calculate the maximum concentration, in mol dm−3, of ammonium carbonate in
such a solution.
(2)

(Total for Question 21 = 14 marks)

TOTAL FOR SECTION B = 38 MARKS

20
*P67748A02028*
BLANK PAGE

21
*P67748A02128* Turn over
SECTION C
Answer ALL the questions. Write your answers in the spaces provided.
22 Potassium chlorate(V), KClO3 , is a crystalline solid used in fireworks.
It is produced by the Liebig Process in two stages.
Stage 1 Chlorine gas is passed through hot calcium hydroxide solution forming
calcium chlorate(V), Ca(ClO3)2 .

6Ca(OH)2(aq) + 6Cl2(g) → Ca(ClO3)2(aq) + 5CaCl2(aq) + 6H2O(l)

Stage 2 Potassium chloride solution is then added to form potassium chlorate(V).

Ca(ClO3)2(aq) + 2KCl(aq) → 2KClO3(aq) + CaCl2(aq)

The solution is heated to reduce its volume and then allowed to crystallise.
The crystals are filtered off.
The remaining filtrate is evaporated further to obtain more crystals.
(a) (i) Write the overall equation for the Liebig Process.
State symbols are not required.
(1)

(ii) Calculate the overall atom economy by mass for the production of
potassium chlorate(V), KClO3 , using your equation in (a)(i).
(3)

22
*P67748A02228*
(b) Explain the type of reaction that takes place in Stage 1 of the Liebig Process, using
oxidation numbers.

6Ca(OH)2(aq) + 6Cl2(g) → Ca(ClO3)2(aq) + 5CaCl2(aq) + 6H2O(l)

(3)

(c) The crystals of potassium chlorate(V) formed also contain some

halide ion impurities.
(i) Describe a chemical test on a solution of these crystals to confirm that the
impurities present are chloride ions rather than bromide ions.
Include the expected results.
(3)

23
*P67748A02328* Turn over
(ii) 1.52 g of impure potassium chlorate(V), formed in the Liebig Process, was
heated until the mass of solid remaining was constant at 1.02 g.
The reaction that occurred was

2KClO3(s) → 2KCl(s) + 3O2(g)

The impurities present did not decompose on heating.
Calculate the percentage purity of the sample.
Give your answer to an appropriate number of significant figures.
(5)

24
*P67748A02428*
(d) In fireworks, potassium chlorate(V) decomposes. This thermal decomposition
takes place in two stages with a solid catalyst.

4KClO3 → KCl + 3KClO4

KClO4 → KCl + 2O2

(i) Give the systematic name of KClO4 .

(1)

(ii) A student investigated the role of the catalyst in this reaction.

Procedure

Step 1 Heat a sample of KClO3 , in a test tube, with a known mass of insoluble
catalyst until the mass remains constant.
Step 2 Mix the contents of the test tube with water.
Step 3 Filter the mixture and rinse with deionised water.
Step 4 Dry the remaining solid.
Step 5 Measure the mass of the dry solid.
Explain how each of the steps in this procedure is needed to show that the
catalyst is not used up in this reaction.
(4)

25
*P67748A02528* Turn over
(e) Explain, using the diagram, how a catalyst speeds up a chemical reaction.
(2)

Number of
particles
with
energy, E

Energy, E

(Total for Question 22 = 22 marks)

TOTAL FOR SECTION C = 22 MARKS

TOTAL FOR PAPER = 80 MARKS

26
*P67748A02628*
BLANK PAGE

27
*P67748A02728*
28
*P67748A02828*
Write your name here
Surname Other names

Pearson Edexcel Centre Number Candidate Number

International
Advanced Level

Chemistry
International Advanced Subsidiary/Advanced Level
Unit 2: Energetics, Group Chemistry,
Halogenoalkanes and Alcohols
Sample Assessment Materials for first teaching September 2018 Paper Reference

Time: 1 hour 30 minutes WCH12/01

You must have: Total Marks
Data Booklet, scientific calculator, ruler

Instructions
• Use black ink or black ball-point pen.
• centre
Fill in the boxes at the top of this page with your name,
number and candidate number.
• Answer all questions.
• Answer the questions in the spaces provided
– there may be more space than you need.
• Show all your working in calculations and include units where
appropriate.

Information
• The total mark for this paper is 80.
• The marks for each question are shown in brackets
– use this as a guide as to how much time to spend on each question.
• toIn questions marked with an asterisk (*), marks will be awarded for your ability
structure your answer logically, showing how the points that you make are
related or follow on from each other where appropriate.
• There is a Periodic Table on the back page of this paper.

Advice
• Read each question carefully before you start to answer it.
• Try to answer every question.
• your answers if you have time at the end.
Check
Turn over

S58310A
©2018 Pearson Education Ltd.

1/1/1/
*S58310A0126*
Pearson Edexcel International Advanced Subsidiary/Advanced Level in Chemistry 47
Sample Assessment Materials – Issue 1 – September 2017 © Pearson Education Limited 2017
SECTION A

Answer ALL the questions in this section.

DO NOT WRITE IN THIS AREA

You should aim to spend no more than 20 minutes on this section.

For each question, select one answer from A to D and put a cross in the box .
If you change your mind, put a line through the box and then mark your new answer
with a cross .

1 Which alkane has the highest boiling temperature?

A 2,2-dimethylpropane
B 2-methylbutane
C butane
D pentane

(Total for Question 1 = 1 mark)

DO NOT WRITE IN THIS AREA

2 Which is the order of increasing boiling temperature?

H H H H H H H H

W= H C C C C O H X= H C C C C O H

H O O H H H H H

H H

H H H H H H H H

Y= H C C C C H Z= H C C C C O H

H H H H H H O H

H DO NOT WRITE IN THIS AREA

A YZXW
B YXZW
C WXZY
D XWYZ

(Total for Question 2 = 1 mark)

2
*S58310A0226*
48 Pearson Edexcel International Advanced Subsidiary/Advanced Level in Chemistry
Sample Assessment Materials – Issue 1 – September 2017 © Pearson Education Limited 2017
3 Which statement is not explained by hydrogen bonding?
A all Group 1 hydroxides are soluble in water
DO NOT WRITE IN THIS AREA

B many simple alcohols are soluble in water

C the density of ice is less than the density of liquid water at 0 °C
D the melting temperature of water is abnormally high

(Total for Question 3 = 1 mark)

4 Which compound is hydrolysed most rapidly?

A 1-chloropropane
B 1-chlorobutane
C 2-chloro-2-methylpropane
D 2-chlorobutane

(Total for Question 4 = 1 mark)

DO NOT WRITE IN THIS AREA

5 Give the systematic name for the following molecule.

A E-1-bromo-2-methylbut-2-ene
B E-2-methyl-1-bromobut-1-ene
C E-1-bromo-3-methylpent-2-ene
D E-1-bromo-2-methylbut-1-ene

(Total for Question 5 = 1 mark)

DO NOT WRITE IN THIS AREA

3
*S58310A0326*
Pearson Edexcel International Advanced Subsidiary/Advanced Level in Chemistry 49
Sample Assessment Materials – Issue 1 – September 2017 © Pearson Education Limited 2017
Turn over
6 1-bromobutane reacts with alkali:
CH3-CH2-CH2-CH2Br + OH− → CH3-CH2-CH2-CH2OH + Br−

DO NOT WRITE IN THIS AREA

The mechanism and type of reaction is:
A electrophilic addition
B electrophilic substitution
C nucleophilic addition
D nucleophilic substitution

(Total for Question 6 = 1 mark)

7 Which of the following compounds could be oxidised to a carboxylic acid by refluxing

with potassium dichromate(VI) and dilute sulfuric acid?

CH3

A CH3 C CH CH3

DO NOT WRITE IN THIS AREA

CH3 O H

CH3

B CH3 C O H

CH3

C CH3 CH2 CH CH3

O H

CH3

D CH3 C CH2 O H
DO NOT WRITE IN THIS AREA

CH3

(Total for Question 7 = 1 mark)

4
*S58310A0426*
50 Pearson Edexcel International Advanced Subsidiary/Advanced Level in Chemistry
Sample Assessment Materials – Issue 1 – September 2017 © Pearson Education Limited 2017
8 A student made the following statements about trends going down Group 2.
Which statement is correct?
DO NOT WRITE IN THIS AREA

A the thermal stability of the nitrates decreases

B the thermal stability of the carbonates decreases
C the solubility of hydroxides increases
D the solubility of sulfates increases

(Total for Question 8 = 1 mark)

9 A colourless solid, Q, was warmed with sodium hydroxide solution. A gas was
evolved which turned damp red litmus paper blue. What is solid Q?
A NaNO3
B NH4Cl
C NaCl
D Ca(NO3)2
DO NOT WRITE IN THIS AREA

(Total for Question 9 = 1 mark)

10 Which test is used to show that sodium chloride solution contains chloride ions?
A damp blue litmus paper turns red
B damp blue litmus paper is bleached
C dilute hydrochloric acid followed by silver nitrate solution gives
a white precipitate
D dilute nitric acid followed by silver nitrate solution gives a white precipitate

(Total for Question 10 = 1 mark)

DO NOT WRITE IN THIS AREA

5
*S58310A0526*
Pearson Edexcel International Advanced Subsidiary/Advanced Level in Chemistry 51
Sample Assessment Materials – Issue 1 – September 2017 © Pearson Education Limited 2017
Turn over
11 Compound X gives a red flame test colour and a white precipitate on addition of
dilute hydrochloric acid followed by barium chloride solution. Which compound is X?

DO NOT WRITE IN THIS AREA

A calcium chloride
B lithium sulfate
C potassium sulfate
D strontium chloride

(Total for Question 11 = 1 mark)

12 Which process explains the flame colour produced by the compounds of

Group 1 elements?
A absorption of visible light energy as electrons are promoted to higher energy levels
B absorption of visible light energy as electrons are removed from gaseous atoms
C emission of visible light energy as electrons return to lower energy levels
D emission of visible light energy as electrons are added to gaseous ions

DO NOT WRITE IN THIS AREA

(Total for Question 12 = 1 mark)

13 When chlorine is reacted with hot concentrated potassium hydroxide, the chlorine
undergoes disproportionation.
What are the oxidation states of chlorine in the products?
A –1 and +3
B –1 and +5
C +1 and –1
D +1 and +5

(Total for Question 13 = 1 mark)

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6
*S58310A0626*
52 Pearson Edexcel International Advanced Subsidiary/Advanced Level in Chemistry
Sample Assessment Materials – Issue 1 – September 2017 © Pearson Education Limited 2017
14 What are the gaseous products formed, other than water vapour, when concentrated
sulfuric acid is added to potassium bromide?
DO NOT WRITE IN THIS AREA

A bromine and sulfur dioxide only

B bromine, hydrogen bromide and hydrogen sulfide only
C bromine, hydrogen bromide and sulfur dioxide only
D bromine, hydrogen bromide, sulfur dioxide and hydrogen sulfide only

(Total for Question 14 = 1 mark)

15 Zinc metal reacts with copper(II) sulfate solution. The equation for the reaction is:
Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s) ∆rH = −210 kJ mol–1.
(a) What is the temperature rise, in °C, when excess zinc powder is added to 50 cm3 of
copper(II) sulfate solution containing 0.0025 mol of copper(II) ions?
[Assume the specific heat capacity of the solution is 4.2 J g–1 °C–1].
(1)
DO NOT WRITE IN THIS AREA

A 2.5
B 10.5
C 25.0
D 44.1

(b) The reaction of zinc with copper(II) sulfate is best classified as:
(1)
A disproportionation
B neutralisation
C redox
D thermal decomposition
DO NOT WRITE IN THIS AREA

(Total for Question 15 = 2 marks)

16 Magnesium metal reacts with hydrochloric acid. Which change in condition would
have no effect on the initial rate of this reaction?
A an increase in the volume of acid solution
B a decrease in the temperature of the acid solution
C an increase in the surface area of the magnesium
D a decrease in the concentration of the acid solution

(Total for Question 16 = 1 mark)

7
*S58310A0726*
Pearson Edexcel International Advanced Subsidiary/Advanced Level in Chemistry 53
Sample Assessment Materials – Issue 1 – September 2017 © Pearson Education Limited 2017
Turn over
17 The diagram shows the general shape of a Maxwell-Boltzmann distribution curve for
the particles present in a reaction mixture.

DO NOT WRITE IN THIS AREA

Number of
particles with
energy, E

B
Ea Energy, E

(a) How does the peak change when the temperature of the reaction mixture
is decreased?
(1)

DO NOT WRITE IN THIS AREA

Peak position Peak height
A shifted left higher

B shifted right higher

C shifted left lower

D shifted right lower

(b) The activation energy of an uncatalysed reaction is represented by the vertical

line, Ea, on the horizontal axis. The shaded areas A and B are the areas under the
curve on either side of the line Ea.
How do the two shaded areas change, if at all, when a catalyst is added?
(1)
Area A Area B
DO NOT WRITE IN THIS AREA

A increases decreases
B decreases increases

C no change no change
D increases increases

(Total for Question 17 = 2 marks)

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54 Pearson Edexcel International Advanced Subsidiary/Advanced Level in Chemistry
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18 The equilibrium reaction shown in the equation was studied by placing the
components into a sealed glass container.
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2NO2(g)  N2O4(g)
At equilibrium, which of the following statements is not true?
A the concentrations of the NO2(g) and N2O4(g) both remain constant
B the total number of molecules is constant
C the forward and reverse reactions have both stopped
D the rate of the forward reaction is equal to the rate of the
reverse reaction

(Total for Question 18 = 1 mark)

TOTAL FOR SECTION A = 20 MARKS

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9
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Pearson Edexcel International Advanced Subsidiary/Advanced Level in Chemistry 55
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SECTION B
Answer ALL the questions.

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Write your answers in the spaces provided.
19 2-methylpropan-1-ol has the skeletal formula:

(a) 2-methylpropan-1-ol can be converted to 1-bromo-2-methylpropane.

Give the reagents and conditions used for this reaction.
(2)

Reagents . .... ... .... ... .... . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . ........... ............. ............................ .............. ............. .............. .............. .............. ............. ....... ...................

Conditions .. .... ... ... ... . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . ...... .............. .............. ............. .............. .............. .............. ............. .............. .............. ......... ............ .........

(b) 1-bromo-2-methylpropane can be converted back to 2-methylpropan-1-ol by

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heating with aqueous alkali. A student suggested the following mechanism for
the reaction.

CH3 H CH3 H

CH3 C Cδ– Br δ+ CH3 C C OH + :Br –

H H H H

OH–

Identify and correct the three mistakes in the mechanism shown.

(3)

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56 Pearson Edexcel International Advanced Subsidiary/Advanced Level in Chemistry
Sample Assessment Materials – Issue 1 – September 2017 © Pearson Education Limited 2017
(c) 1-bromo-2-methylpropane can be converted to 2-methylpropene.
Give the reagents and conditions used for this reaction.
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(2)

Reagents .... ... .... ... ... ... . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .... ............. .............. .............. .............. ............. .............. .............. .............. ............. ............. ........ .............

Conditions ... .... ... .... . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . ........ .............. .............. ............. .............. .............. .............. ............. .............. .............. ..................... ........

(Total for Question 19 = 7 marks)

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11
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Pearson Edexcel International Advanced Subsidiary/Advanced Level in Chemistry 57
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20 Ethanedioic acid is a solid diprotic acid. A student used ethanedioic acid in a titration to
find the concentration of a potassium hydroxide solution.

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The equation for the reaction is:
2KOH + (COOH)2 → (COOK)2 + 2H2O
(a) Calculate the mass of ethanedioic acid that should be used to make 1000 cm3 of a
0.0500 mol dm–3 solution in water.
Give your answer to an appropriate number of significant figures.
[Molar mass of ethanedioic acid = 90.0 g mol–1].
(2)

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(b) A student decided to check to see if phenolphthalein was a suitable indicator for
this titration. The student measured 400 cm3 of the 0.0500 mol dm–3 ethanedioic
acid into a beaker and added a few drops of phenolphthalein indicator.
Calculate the minimum mass of solid potassium hydroxide that should be added
to produce a colour change.
(2)

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12
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58 Pearson Edexcel International Advanced Subsidiary/Advanced Level in Chemistry
Sample Assessment Materials – Issue 1 – September 2017 © Pearson Education Limited 2017
*(c) A student used a 0.0500 mol dm–3 solution of ethanedioic acid to find an accurate
concentration of a potassium hydroxide solution which was known to have an
approximate concentration of 0.1 mol dm–3.
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Describe a procedure to obtain reliable titration results using standard laboratory

equipment.
(6)

(Total for Question 20 = 10 marks)

13
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21 Sodium hydrogencarbonate can be decomposed to sodium carbonate by heating to
about 300 °C.

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The equation for the reaction is:
2NaHCO3(s) → Na2CO3(s) + CO2(g) + H2O(l)
(a) Give a reason why it is not possible to measure the enthalpy change for this
reaction directly.
(1)

(b) (i) State what is meant by the standard enthalpy change of formation.
(2)

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(ii) Complete the Hess cycle that you would use to determine the enthalpy
change for this reaction from the standard enthalpy changes of formation.
(2)

2NaHCO3(s) Na2CO3(s) + CO2(g) + H2O(l)

∆rH

∆H1 ∆H2

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60 Pearson Edexcel International Advanced Subsidiary/Advanced Level in Chemistry
Sample Assessment Materials – Issue 1 – September 2017 © Pearson Education Limited 2017
(iii) Calculate the standard enthalpy change for the thermal decomposition of
sodium hydrogencarbonate, using the information in the table and your
completed cycle. Include a sign and units in your answer.
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(4)

Standard enthalpy change of formation,

Compound
∆fH d / kJ mol–1
NaHCO3(s) –950.8
Na2CO3(s) –1130.7
CO2(g) –393.5
H2O(l) –285.8
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(iv) Use your answer to (b)(iii) to draw an enthalpy level diagram for this reaction,
labelling the axes provided.
(2)
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(Total for Question 21 = 11 marks)

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22 Three compounds, A, B and C, each have the same molecular formula C4H10O and are
known to be alcohols.

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(a) The infrared spectra of compounds A, B and C are shown.

Compound A

100

Transmittance
50
(%)

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4000 3000 2000 1500 1000 500
Wavenumber / cm–1

Compound B

100

Transmittance
50
(%)

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0
4000 3000 2000 1500 1000 500

Wavenumber / cm–1

16
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Compound C

100
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Transmittance
50
(%)

0
4000 3000 2000 1500 1000 500
Wavenumber / cm–1
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(i) Identify one feature, common to all three infrared spectra, which shows that
A, B and C are all alcohols.
(1)

(ii) State, giving a reason for your answer, if it is possible to identify each of these
three alcohols on the basis of the infrared spectra alone.
(1)

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(b) The mass spectra of the compounds A, B and C are shown.
Compound A

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100

Relative 60
intensity
40

0
10 20 30 40 50 60 70 80 90
m/z

Compound B

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100

Relative 60
intensity
40

0
10 15 20 25 30 35 40 45 50 55 60 65 70 75 80 85 90
m/z

Compound C
100
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Relative 60
intensity
40

0
10 15 20 25 30 35 40 45 50 55 60 65 70 75 80 85 90
m/z

18
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64 Pearson Edexcel International Advanced Subsidiary/Advanced Level in Chemistry
Sample Assessment Materials – Issue 1 – September 2017 © Pearson Education Limited 2017
(i) Identify one feature common to the mass spectra of compounds A, B and C
which shows that the molecular formula is C4H10O.
(1)
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(ii) Using the fragmentation patterns, a student proposed that:

compound A is butan-2-ol
compound B is butan-1-ol
compound C is 2-methylpropan-2-ol
State how the appearance in the spectra of the following peaks supports the
student’s conclusion.
(3)
the fragment causing the peak at m/z = 45 for compound A

the fragment causing the peak at m/z = 31 for compound B

the fragment causing the peak at m/z = 59 for compound C

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(c) To help with the identification of compounds A and B, the student decided to mix
each of them with potassium dichromate(VI) and dilute sulfuric acid solutions,
and then distil the mixture immediately.

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(i) Identify, by name and structural formula, the organic compound present at
the conclusion of each of these two oxidation reactions.
(3)

Organic
Name of oxidation
compound Structural formula of oxidation product
product
used

A, butan-2-ol

B, butan-1-ol

(ii) To identify A and B, the student decided that one further chemical test should
be used on their oxidation products.

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Give a suitable reagent and expected observations that could be used to
distinguish between the oxidation products of A and B.
(3)

(Total for Question 22 = 12 marks) DO NOT WRITE IN THIS AREA

TOTAL FOR SECTION B = 40 MARKS

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66 Pearson Edexcel International Advanced Subsidiary/Advanced Level in Chemistry
Sample Assessment Materials – Issue 1 – September 2017 © Pearson Education Limited 2017
SECTION C
Answer ALL the questions.
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Write your answers in the spaces provided.

23 Iodine monochloride, ICl, is a covalent compound produced by the reaction of iodine
with chlorine. Iodine monochloride is a dark brown liquid at room temperature.
The equipment shown can be used to pass chlorine over solid iodine to produce
iodine monochloride.

chlorine gas, Cl2

U tube
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iodine solid, I2

When excess chlorine is passed through the U tube, the iodine monochloride reacts
to produce iodine trichloride in an equilibrium reaction.
(a) Write a chemical equation for the reaction of iodine with chlorine to produce
iodine monochloride. Include state symbols.
(2)
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21
*S58310A02126*
Pearson Edexcel International Advanced Subsidiary/Advanced Level in Chemistry 67
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(b) The iodine monochloride molecule has a permanent dipole.
Complete the following table using the electronegativity data from
your Data Booklet and hence show the dipole on the diagram of the

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iodine monochloride molecule.
(1)

Element Electronegativity

I ⎯ Cl

(c) Iodine monochloride reacts with propene to form two isomeric products. This is an
addition reaction that is similar to the reaction of propene with hydrogen halides.
(i) Draw the skeletal formulae of both isomers.
(2)

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(ii) Explain which of these isomers is the major product.
(3)

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68 Pearson Edexcel International Advanced Subsidiary/Advanced Level in Chemistry
Sample Assessment Materials – Issue 1 – September 2017 © Pearson Education Limited 2017
(d) The equation for the reaction between iodine monochloride and chlorine is:

ICl(l) + Cl2(g)  ICl3(s)

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brown liquid yellow solid

(i) State and justify one precaution that must be taken when preparing
iodine trichloride.
(2)

(ii) Give the oxidation number of iodine in both iodine-containing compounds in

the equilibrium.
(1)
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I in ICl . ... ... .... ... .... ... .... . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . ........... ............. .............. .............. .............. ............. .............. .............. .............. ............. ..... .. .................. .

I in ICl3 ... ... .... ... .... ... .... . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . ........... .............. ............. .............. .............. .............. ............. .............. .............. .............. .... ................ .....

(iii) Iodine trichloride can also be made by reacting potassium chlorate(V) with
iodine in hydrochloric acid. The equation for the reaction is

KClO3 + I2 + 6HCl → KCl + 2ICl3 + 3H2O

By considering oxidation numbers for chlorine, explain whether or not this
reaction is a disproportionation.
(2)

23
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(e) Chlorine gas has a molar volume of 24 000 cm3 mol–1 under the conditions used in
this reaction.

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(i) Show that the density of chlorine gas is approximately 3 g dm–3.
(2)

(ii) Air has an average density of 1.25 g dm–3. If the U-tube used in 23(d) is inverted,
as shown in the diagram, the solid yellow iodine trichloride produced in the
equilibrium reaction turns to a brown liquid.

iodine trichloride, ICl3

inverted U tube DO NOT WRITE IN THIS AREA

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Explain this observation.

(3)

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Sample Assessment Materials – Issue 1 – September 2017 © Pearson Education Limited 2017
(f ) A mass of 0.64 g of iodine reacted with fluorine to form 1.31 g of a fluoride of
iodine.
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Calculate the empirical formula of this compound of iodine and fluorine.

(2)
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(Total for Question 23 = 20 marks)

TOTAL FOR SECTION C = 20 MARKS

TOTAL FOR PAPER = 80 MARKS
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25
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26
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72 Pearson Edexcel International Advanced Subsidiary/Advanced Level in Chemistry
Sample Assessment Materials – Issue 1 – September 2017 © Pearson Education Limited 2017
Please check the examination details below before entering your candidate information
Candidate surname Other names

Pearson Edexcel Centre Number Candidate Number

International
Advanced Level

Time 1 hour 30 minutes

Paper
reference WCH12/01
Chemistry
International Advanced Subsidiary / Advanced Level
UNIT 2: Energetics, Group Chemistry,
Halogenoalkanes and Alcohols

You must have: Total Marks

Scientific calculator, Data Booklet, ruler

Instructions
• Use black ink or ball-point pen.
• Fill in the boxes at the top of this page with your name,
centre number and candidate number.
• Answer all questions.
• Answer the questions in the spaces provided
– there may be more space than you need.
• Show all your working in calculations and include units where appropriate.
Information
• The total mark for this paper is 80.
• The marks for each question are shown in brackets
– use this as a guide as to how much time to spend on each question.
• Instructure
the question marked with an asterisk (*) marks will be awarded for your ability to
your answer logically, showing how the points that you make are related or
follow on from each other where appropriate.
• A Periodic Table is printed on the back cover of this paper.

Advice
• Read each question carefully before you start to answer it.
• Try to answer every question.
• Check your answers if you have time at the end.
• Good luck with your examination.
Turn over

P64624A
©2021 Pearson Education Ltd.

1/1/1/1/1/1/1/1
*P64624A0128*
SECTION A
Answer ALL questions. Write your answers in the spaces provided.
You should aim to spend no more than 20 minutes on this section.
For each question, select one answer from A to D and put a cross in the box . If you change
your mind, put a line through the box and then mark your new answer with a cross .
1 Which is the correctly labelled reaction profile for an exothermic reaction?

Enthalpy
Ea
Reactants
A
∆H
Products

Reaction pathway

Enthalpy
∆H
Reactants
B
Ea
Products

Reaction pathway

Enthalpy
Ea
Products
C
∆H
Reactants

Reaction pathway

Enthalpy
∆H
Products
D
Ea
Reactants

Reaction pathway

(Total for Question 1 = 1 mark)

2
*P64624A0228*
2 The equation for a reaction is
2C(s) + O2(g) 2CO(g)
Which is the correct symbol for the enthalpy change for this reaction?

A ∆atH
B ∆cH

C ∆fH

D ∆rH

(Total for Question 2 = 1 mark)

3 The graph shows how the concentration of iodine changes with time in a reaction.
0.30

0.25

0.20

[I2] 0.15
/ mol dm–3
0.10

0.05

0.00
0 2 4 6 8 10 12 14 16
Time / s

What is the value for the rate of reaction, in mol dm−3 s−1, at 8 seconds?

A 0.01

B 0.02
C 0.03

D 0.25

(Total for Question 3 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

3
*P64624A0328* Turn over
4 The solid line on the graph below shows the Maxwell–Boltzmann distribution for an
uncatalysed reaction. Ea is the activation energy of this reaction.

X
Number of
particles with
energy, E Y

W Ea Z

Energy / E

Which row shows the correct Maxwell–Boltzmann curve and activation energy for the
reaction at a higher temperature with a catalyst?

Maxwell-Boltzmann curve Activation energy

A X W

B X Z

C Y W

D Y Z

(Total for Question 4 = 1 mark)

5 What is the oxidation number of chromium in Na2Cr2O7?

A +1

B +2

C +3

D +6

(Total for Question 5 = 1 mark)

4
*P64624A0428*
6 In an oxide of nitrogen, the oxidation number of nitrogen is +4.
Which is the formula of the oxide?

A N2O

B N2O3
C N2O4

D N2O5

(Total for Question 6 = 1 mark)

7 Hydrogen peroxide, H2O2 , breaks down into water and oxygen.

In terms of oxidation and reduction, how do hydrogen and oxygen change
in this reaction?

Hydrogen Oxygen

A oxidised reduced

B oxidised and reduced unchanged

C reduced oxidised

D unchanged oxidised and reduced

(Total for Question 7 = 1 mark)

8 Several factors may affect ionisation energies:

I) the number of protons increases
II) the outer electron is further from the nucleus
III) the amount of shielding increases
IV) the number of unpaired outer electrons increases
Which factors explain the decrease in ionisation energy as Group 1 is descended?

A I and II

B II and III
C III and IV

D I, II, III and IV

(Total for Question 8 = 1 mark)

5
*P64624A0528* Turn over
9 Separate samples of some halogenoalkanes were dissolved in ethanol and a few
drops of silver nitrate solution added. The faster the reaction of the halogenoalkane,
the quicker a precipitate forms.
(a) Which of these halogenoalkanes reacts the fastest?
(1)
A CH3CHICH3

B CH3CHBrCH3

C CH3CHClCH3

D CH3CHFCH3
(b) Which of these halogenoalkanes reacts the fastest?
(1)
A CH3CHBrCH(CH3)CH3

B CH3CH2CBr(CH3)CH3
C CH3CH(CH2Br)CH2CH3
D CH3CH2CH2CH2CH2Br

(Total for Question 9 = 2 marks)

10 What is the structure of 2-bromo-3-chloro-2-methylbutane?

Br Cl
A H3C C C H
CH3 CH3

Cl
B

Br Cl
C H3C C C CH3
CH3 CH3

D
Cl

(Total for Question 10 = 1 mark)

6
*P64624A0628*
11 Which structure represents a primary halogenoalkane?

Cl
B

C
Cl

D
Cl

(Total for Question 11 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

7
*P64624A0728* Turn over
12 Which could be the infrared spectrum of CH2=CHCH2OH?
100

A % Transmittance 50

0
4000 3000 2000 1500 1000 500
Wavenumber / cm–1

100

B % Transmittance 50

0
4000 3000 2000 1500 1000 500
Wavenumber / cm–1

100

C % Transmittance 50

0
4000 3000 2000 1500 1000 500
Wavenumber / cm –1

100

D % Transmittance 50

0
4000 3000 2000 1500 1000 500
Wavenumber / cm–1

(Total for Question 12 = 1 mark)

8
*P64624A0828*
13 The mass spectrum of propanone is shown.

100

60
Relative
intensity
40

0
10 15 20 25 30 35 40 45 50 55 60
m/z

Which fragment is most likely to produce the peak at m / z = 43?

A CH3CH2CH2+
B CH3CO+

C CH2CHO+
D CHCH2O+

(Total for Question 13 = 1 mark)

14 A 4.00 mol dm−3 solution of an acid is used to prepare dilute solutions of the acid.
What volume of water is required to make up 150 cm3 of 0.35 mol dm−3 solution of
the acid?

A 13.1 cm3

B 52.5 cm3

C 97.5 cm3

D 136.9 cm3

(Total for Question 14 = 1 mark)

9
*P64624A0928* Turn over
15 (a) A pellet of sodium hydroxide has a mass of 0.700 g.
Some pellets were dissolved to make 350 cm3 of 0.25 mol dm–3 solution.
[Mr value: NaOH = 40]
How many pellets were dissolved?
(1)
A 4

B 5

C 8
D 125
(b) 25.0 cm3 of the sodium hydroxide solution prepared in (a) was placed in a conical
flask and titrated with sulfuric acid.
2NaOH + H2SO4 Na2SO4 + 2H2O
Calculate the number of moles of sulfuric acid that reacted.
(1)
A 0.0031
B 0.0063
C 0.013

D 0.044
(c) Phenolphthalein indicator was used for the titration in (b).
What was the colour change at the endpoint?
(1)
A colourless pink
B pink colourless

C orange yellow
D yellow orange

(Total for Question 15 = 3 marks)

Use this space for any rough working. Anything you write in this space will gain no credit.

10
*P64624A01028*
16 Which silver halides are soluble in concentrated aqueous ammonia?

A AgBr and AgI

B AgCl and AgI

C AgCl and AgBr

D AgCl only

(Total for Question 16 = 1 mark)

17 What volume, in dm3, of hydrogen gas will be produced when 3.00 g of lithium is
reacted with water at room temperature and pressure (r.t.p.)?
2Li + 2H2O 2LiOH + H2
[Molar volume of gas at r.t.p. = 24.0 dm3 mol–1]

A 0.217

B 0.435
C 5.22
D 10.4

(Total for Question 17 = 1 mark)

TOTAL FOR SECTION A = 20 MARKS

11
*P64624A01128* Turn over
SECTION B
Answer ALL questions.
Write your answers in the spaces provided.
18 1-bromopropane is used for spot removal when ‘dry cleaning’ clothes.
(a) 1-bromopropane does not occur naturally but can be made from propan-1-ol.
Identify the reagent or reagents you would use to make 1-bromopropane
from propan-1-ol.
(1)

(b) Some reactions of 1-bromopropane are shown.

propylamine

ammonia
potassium
hydroxide reaction C
propene 1-bromopropane propan-1-ol

potassium cyanide

product B

(i) Give the conditions for the formation of propene.

(1)

(ii) Give the molecular formula of product B.

(1)

(iii) Name the type and mechanism of the reaction taking place in reaction C.
(2)

12
*P64624A01228*
(iv) Complete the mechanism for the reaction that occurs between ammonia and
1-bromopropane to form propylamine, CH3CH2CH2NH2 .
Include curly arrows, and relevant lone pairs and dipoles.
(4)

H H H

H C C C Br

H H H

(Total for Question 18 = 9 marks)

13
*P64624A01328* Turn over
BLANK PAGE

14
*P64624A01428*
19 Magnesium reacts with sulfuric acid in an exothermic reaction.
(a) Write an equation for the reaction.
Include state symbols in your answer.
(2)

(b) A student carried out an experiment to determine the enthalpy change of

the reaction.
A sample of 0.50 g of magnesium powder was added to
25 cm3 of 0.20 mol dm−3 sulfuric acid.
Calculate the number of moles of magnesium and of sulfuric acid that reacted.
Justify your answer.
(3)

15
*P64624A01528* Turn over
(c) (i) The results obtained are given in the table.
Plot the results on the grid.
(2)

Time Temperature
/ minutes / °C
0 22.2
1 22.0
2 22.0 Mg added
3 39.6
4 41.8
5 40.8
6 40.2
7 39.4
8 38.6

16
*P64624A01628*
(ii) Use your graph to determine the maximum change in temperature.
You must show your working on the graph.
(2)

ΔT = .. .......... .......... ... ............ .................... .....

(d) Calculate the standard molar enthalpy change for the reaction, using your
answers to (b) and (c)(ii).
Include a sign and units in your answer.
[Specific heat capacity of solution = 4.18 J g–1 °C–1]
(4)

(Total for Question 19 = 13 marks)

17
*P64624A01728* Turn over
20 This question is about the forces between molecules and ions.
*(a) Some data for three small molecules are shown.

Boiling temperature
Molecule Mr
/ °C

Fluorine 38.0 −188

Hydrogen chloride 36.5 −85

Methanol 32.0 65

Explain the large variation in boiling temperatures, given the small range in
Mr values.
Detailed descriptions of the forces involved are not required.
(6)

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19
*P64624A01928* Turn over
(b) Calcium chloride is soluble in water.
Complete the diagram to show how water molecules interact with each ion.
You may use to represent a water molecule.
(2)

Ca2+ Cl–

(c) Explain why bromine is a liquid but iodine is a solid at room temperature.
Detailed explanations of the forces involved are not required.
(2)

(Total for Question 20 = 10 marks)

20
*P64624A02028*
21 Magnesium oxalate, MgC2O4 , decomposes on heating to form magnesium carbonate
and carbon monoxide.
MgC2O4(s) → MgCO3(s) + CO(g)
(a) A 6.0 g sample of magnesium oxalate was heated for three minutes but the
decomposition was only 70 % complete.
Calculate the total mass of solid that remains.
(4)

(b) In practice, magnesium carbonate also decomposes on stronger heating.

Describe and explain the trend in the thermal decomposition of Group 2 carbonates.
(3)

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(c) Suggest why a pure sample of magnesium carbonate will not be produced from
the decomposition of magnesium oxalate even if the sample is heated for longer.
(1)

(Total for Question 21 = 8 marks)

TOTAL FOR SECTION B = 40 MARKS

22
*P64624A02228*
SECTION C
Answer all the questions. Write your answers in the spaces provided.
22 Phosgene (COCl2) is a colourless gas used in the pharmaceutical industry.
Phosgene has a boiling temperature of 8 °C and is extremely toxic.
(a) Complete the dot-and-cross diagram to show the bonding in phosgene.
(2)

C
Cl Cl

(b) Phosgene can be formed from carbon monoxide and chlorine, using a catalyst of
activated carbon.
CO(g) + Cl2(g) ⇌ COCl2(g) ΔrH = –107.6 kJ mol–1
(i) State and explain how the reaction conditions could be changed to maximise
the equilibrium yield of phosgene in this reaction.
(4)

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(ii) The standard enthalpy change of formation for phosgene is
Δ f H = –220.1 kJ mol–1.
Complete the Hess cycle and determine the standard enthalpy change of
formation for carbon monoxide. Use the data from (b)(i).
Include state symbols in your cycle.
(4)
CO(g) + Cl2(g) COCl2(g)

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(c) The mass spectrum of a sample of phosgene is shown.
The peak at m / z = 65 has been omitted.
100

60
Relative
intensity
40

0.0
20 40 60 80 100 120
m/z

(i) Give the reason for the ratio of peak heights at m / z values of 102, 100 and 98.
(2)

(ii) Suggest an identity for the peak at m / z = 63.

(1)

(iii) The peak at m / z = 65 has been omitted.

Draw on the mass spectrum the peak at m / z = 65, showing its
relative intensity.
(1)
(d) Use your Data Booklet to suggest the wavenumber of a strong absorbance you
would expect to see in the infrared spectrum for phosgene. Justify your answer.
(2)

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*P64624A02528* Turn over
(e) In UV light, trichloromethane (CHCl3 , boiling temperature 61°C) reacts with
oxygen to form phosgene and hydrogen chloride.
(i) Write an equation for this reaction.
State symbols are not required.
(1)

(ii) In a closed bottle, the rate of this reaction decreases with time.
Give a reason for this.
(1)

(iii) Suggest a precaution that should be taken when opening a

bottle of trichloromethane.
(1)

(iv) Trichloromethane can be used as an anaesthetic.

Suggest whether an old bottle of trichloromethane can still be used for
medical treatment, giving a reason for your answer.
(1)

(Total for Question 22 = 20 marks)

TOTAL FOR SECTION C = 20 MARKS

TOTAL FOR PAPER = 80 MARKS

26
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BLANK PAGE

27
*P64624A02728*
28
*P64624A02828*
Please check the examination details below before entering your candidate information
Candidate surname Other names

Pearson Edexcel Centre Number Candidate Number

International
Advanced Level

Thursday 16 January 2020

Morning (Time: 1 hour 30 minutes) Paper Reference WCH12/01

Chemistry
International Advanced Subsidiary/Advanced Level
Unit 2: Energetics, Group Chemistry, Halogenoalkanes and
Alcohols
Candidates must have: Scientific calculator Total Marks
Data Booklet
Ruler

Information
• The total mark for this paper is 80.
• The marks for each question are shown in brackets
– use this as a guide as to how much time to spend on each question.
• ability
In the question marked with an asterisk (*), marks will be awarded for your
to structure your answer logically, showing how the points that you make
are related or follow on from each other where appropriate.
• A Periodic Table is printed on the back cover of this paper.

Advice
• Read each question carefully before you start to answer it.
• Show all your working in calculations and include units where appropriate.
• Check your answers if you have time at the end.
Turn over

P60464A
©2020 Pearson Education Ltd.

1/1/1/1/1/
*P60464A0128*
SECTION A

Answer ALL the questions in this section.

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You should aim to spend no more than 20 minutes on this section.

For each question, select one answer from A to D and put a cross in the box .
If you change your mind, put a line through the box and then mark your new answer
with a cross .

1 Which equation represents the standard enthalpy change of formation, f H , of

hydrogen iodide?
A H(g) + I(g) → HI(g)
B H2(g) + I2(s) → 2HI(g)
C ½H2(g) + ½I2(g) → HI(g)
D ½H2(g) + ½I2(s) → HI(g)

(Total for Question 1 = 1 mark)

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2 When 50 cm3 of hydrochloric acid of concentration 2.0 mol dm−3 is added to 50 cm3 of
sodium hydroxide solution of concentration 2.0 mol dm−3, the temperature increase is 13.0 C.

HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l)

The experiment is repeated using 25 cm3 of the same hydrochloric acid and 50 cm3 of
the same sodium hydroxide solution.

What is the temperature increase?

A 4.9 C
B 6.5 C
C 8.7 C
D 13.0 C DO NOT WRITE IN THIS AREA

(Total for Question 2 = 1 mark)

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3 Nitrogen reacts with hydrogen to form ammonia.

N2(g) + 3H2(g) 2NH3(g) H = −92 kJ mol−1

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Bond Bond energy / kJ mol−1

N N 945
H H 436

What is the mean bond energy, in kJ mol−1, for the N H bond?

A 246
B 360
C 376
D 391

(Total for Question 3 = 1 mark)

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4 How many moles of CO2 are formed when 3.0 mol of chloroethene, C2H3Cl, is mixed
with 10.0 mol of oxygen and react as shown?

2C2H3Cl + 5O2 → 4CO2 + 2H2O + 2HCl

A 3.0
B 4.0
C 6.0
D 8.0

(Total for Question 4 = 1 mark)

5 Which compounds are arranged in order of decreasing boiling temperature?

A CH3CH2CH2CH3 > CH3CH2CH2CH2CH3 > CH3CH2CH2CH2CH2CH3
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B CH3CH2CH2CH2CH2CH3 > (CH3)2CHCH2CH2CH3 > (CH3)3CCH2CH3

C CH3CH2CH2OH > CH3CHOHCH2OH > CH2OHCHOHCH2OH
D CH3Cl > CH3Br > CH3I

(Total for Question 5 = 1 mark)

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6 Chlorine is added to 2 cm3 of a dilute solution of potassium iodide.
The equation for the reaction between chlorine and iodide ions is

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Cl2(aq) + 2I−(aq) → I2(aq) + 2Cl−(aq)

(a) Which statement is correct?

(1)
A iodide ions oxidise chlorine
B iodide ions reduce chlorine
C chlorine reduces iodide ions
D chlorine is neither oxidised nor reduced

(b) When the reaction is complete, 10 cm3 of cyclohexane (density = 0.79 g cm−3) is added.
The mixture is shaken and left to settle into two layers.
Which description of one of these layers is correct?
(1)

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A the upper layer is purple
B the lower layer is purple
C the upper layer is brown
D the lower layer is brown

(Total for Question 6 = 2 marks)

7 Going from calcium to barium in Group 2, which property changes as stated?

A ionic radius decreases

B first ionisation energy decreases
C melting temperature increases
D reactivity with water decreases
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(Total for Question 7 = 1 mark)

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8 The properties of Group 2 compounds change down the group from magnesium
to barium.
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Which statement is correct?

A solubility of Group 2 sulfates increases
B solubility of Group 2 hydroxides decreases
C thermal stability of Group 2 nitrates increases
D thermal stability of Group 2 carbonates decreases

(Total for Question 8 = 1 mark)

9 Iodine reacts with hot sodium hydroxide solution.

a NaOH(aq) + b I2(aq) → c NaI(aq) + d NaIO3(aq) + e H2O(l)

What are the coefficients (a, b, c, d and e) needed to balance this equation?

a b c d e
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A 2 1 1 1 1

B 4 2 3 1 2
C 4 1 3 1 1

D 6 3 5 1 3

(Total for Question 9 = 1 mark)

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10 Aqueous sodium iodide reacts with aqueous silver nitrate to form a precipitate of
silver iodide.
NaI(aq) + AgNO3(aq) → NaNO3(aq) + AgI(s)

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Mr values: 149.9 169.9 85.0 234.8
(a) Which is correct for silver iodide?
(1)

Solubility in concentrated
Colour of precipitate
aqueous ammonia
A yellow insoluble

B yellow soluble

C cream insoluble

D cream soluble

(b) What is the percentage atom economy by mass for the production of silver iodide
in this reaction?

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(1)
A 29 %
B 37 %
C 50 %
D 73 %

(Total for Question 10 = 2 marks)

Use this space for any rough working. Anything you write in this space will gain no credit.

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11 Ethanol can be prepared by reacting chloroethane with aqueous potassium hydroxide.

(a) What type of reaction occurs in this preparation?

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(1)
A addition
B elimination
C reduction
D substitution

(b) How do the boiling temperatures of ethanol and chloroethane compare, and
what is the reason for the difference?
(1)
Comparison of boiling
Reason for the difference
temperature
A ethanol is higher ethanol molecules form hydrogen bonds

B ethanol is higher ethanol molecules have more atoms

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C ethanol is lower ethanol molecules have fewer electrons

D ethanol is lower ethanol has a lower molar mass

(c) Bromoethane and chloroethane react with aqueous potassium hydroxide at

different rates.
Which is correct?
(1)

Difference in rate Reason for difference

A bromoethane is faster C Br bond is less polar than the C Cl bond

B bromoethane is faster C Br bond is weaker than the C Cl bond

C bromoethane is slower C Br bond is less polar than the C Cl bond

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D bromoethane is slower C Br bond is stronger than the C Cl bond

(Total for Question 11 = 3 marks)

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12 Butanol burns completely in oxygen.

C4H9OH(l) + 6O2(g) → 4CO2(g) + 5H2O(l)

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⎣
⎡ Mr butanol = 74.0 ⎢
⎢ Molar volume of a gas at room temperature and pressure (r.t.p.) = 24.0 dm3 mol–1 ⎡
⎣

7.40 g butanol was burned completely in 16.0 dm3 oxygen and the mixture of gases
produced was cooled to r.t.p.

(a) What is the final volume of the mixture of gases in dm3 at r.t.p.?
(1)
A 9.60
B 11.2
C 21.6
D 23.2

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(b) If the final mixture of gases is passed through a U-tube containing sodium hydroxide,
what is the final volume of gas in cm3?
(1)
A 0.0
B 1600
C 9600
D 12000

(Total for Question 12 = 2 marks)

Use this space for any rough working. Anything you write in this space will gain no credit.

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13 A halogenoalkane is dissolved in aqueous ethanol. When aqueous silver nitrate is
added, a white precipitate forms immediately.
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What is the halogenoalkane?

A 1-chlorobutane
B 2-chlorobutane
C 1-chloro-2-methylpropane
D 2-chloro-2-methylpropane

(Total for Question 13 = 1 mark)

14 Propanal (CH3CH2CHO) and propanone (CH3COCH3) are isomers.

(a) Which m / z peak would not be expected in the mass spectrum of propanone?
(1)
A 15
B 29
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C 43
D 58

(b) Propanal and propanone can be distinguished by chemical tests.

Which pair of observations is correct?
(1)
Observation with Observation
Test
propanal with propanone
A warm with Fehling’s solution no change red precipitate

B add solid phosphorus(V) chloride no change misty fumes

C warm with acidified potassium dichromate(VI) turns green no change
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D add sodium hydrogencarbonate fizzes no change

(Total for Question 14 = 2 marks)

TOTAL FOR SECTION A = 20 MARKS

9
*P60464A0928* Turn over
SECTION B
Answer ALL the questions.

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Write your answers in the spaces provided.

15 This question is about hydrated salts.

(a) The enthalpy change for the conversion of anhydrous copper(II) sulfate, CuSO4 , to
the hydrated form, CuSO4.5H2O, can be found using Hess’s Law.

r H
CuSO4(s) + 5H2O(l) CuSO4.5H2O(s)
A student carried out experiments to determine the value of the enthalpy change, rH.
Known masses of anhydrous and hydrated copper(II) sulfate were dissolved separately
in water in insulated containers, and the temperature changes measured.
The results are shown in the table.

Mass Volume of water used Temperature change soln H

Compound
/g / cm3 / °C / kJ mol−1

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CuSO4.5H2O(s) 12.5 45.5 −3.0 +12.6

CuSO4(s) 8.00 50.0 +16.0

(i) State why different volumes of water are used in the two experiments.
Justify your answer.
(2)

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(ii) Calculate the enthalpy change of solution, H, in kJ mol−1, for the
soln
anhydrous salt, CuSO4 .
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⎣
⎡ Assume: heat capacity of the solution = 4.2 J g−1 °C−1 ⎢
⎢ density of solution = 1.0 g cm−3
⎡
⎣
(3)
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*P60464A01128* Turn over
(iii) Complete the Hess cycle by adding two arrowheads.
(1)

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rH
CuSO4(s) + 5H2O(l) CuSO4.5H2O(s)

H(CuSO4)
soln H(CuSO4.5H2O)
soln

CuSO4(aq)

(iv) Calculate the value for the enthalpy change rH, in kJ mol−1, for the conversion of the
anhydrous salt to the hydrated salt.
Use the value from the table for solnH (CuSO4.5H2O), the value for solnH (CuSO4)
calculated in (a)(ii) and the completed Hess cycle in (a)(iii).
(2)

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*P60464A01228*
(b) The hydration of anhydrous copper(II) sulfate is reversible.

CuSO4(s) + 5H2O(l) CuSO4.5H2O(s)

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The forward reaction is exothermic. The temperature changes for both the
forward and reverse reactions are difficult to measure.
Suggest a reason in each case.
(2)

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*P60464A01328* Turn over
(d) Hydrates of sodium carbonate may be represented by the formula Na2CO3.xH2O.
The value of x can be found by making up a solution of sodium carbonate and

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titrating this with a solution of hydrochloric acid of known concentration.
A known mass of Na2CO3.xH2O was dissolved in water, made up to the mark in a
250.0 cm3 volumetric flask and mixed thoroughly.
25.0 cm3 portions of the solution were titrated with 0.0900 mol dm−3 hydrochloric acid
using methyl orange indicator. The mean titre was 25.60 cm3.
The equation for the neutralisation reaction is

Na2CO3(aq) + 2HCl(aq) 2NaCl(aq) + CO2(g) + H2O(l)

(i) Calculate the amount, in moles, of sodium carbonate in the 250.0 cm3 of solution.
(2)

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*P60464A01428*
(ii) The 250.0 cm3 of solution was prepared by dissolving 3.29 g of Na2CO3.xH2O.
Use this mass and your answer to (d)(i) to determine the value of x.
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Give your answer to the appropriate number of significant figures.

You must show your working.
(4)
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(Total for Question 15 = 18 marks)

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15
*P60464A01528* Turn over
16 This question is about trends in the Periodic Table.
*(a) The boiling temperatures of some isoelectronic hydrides are shown.

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Hydride CH4 NH3 H2O HF
Boiling temperature / K 112 240 373 293

Explain the differences in these boiling temperatures by considering all the

intermolecular forces involved.
Detailed descriptions of the intermolecular forces involved are not required.
(6)

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16
*P60464A01628*
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17
*P60464A01728* Turn over
(b) Compare and contrast the reactions of concentrated sulfuric acid with
solid potassium chloride and with solid potassium bromide.
(4)

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............ .. .. .. .. .. .. .. .. .. . .. .. .. .. .. .. .. .. . .. . . .. . . .. . . .. . . .. . . .. . . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . . .. . . .. ........... ............................................................................................................................... .. .. .. .. ... .. .. ... .. ..

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... .......... .. .. .. .. . .. .. .. .. .. .. .. .. .. .. .. .. .. . .. . . .. . . .. . . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . . .. . . .. . . .. . . .. . . ............ ............................................................................................................................... . .. .. .. ... .. .. ... .. .. .

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(Total for Question 16 = 10 marks)

DO NOT WRITE IN THIS AREA

18
*P60464A01828*
17 This question is about 2-methylbutan-2-ol, C5H11OH, and some related compounds.
(a) Draw the displayed formula of 2-methylbutan-2-ol.
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(1)

(b) 2-methylbutan-2-ol forms two different alkenes in an elimination reaction.

One product is 2-methylbut-2-ene.

H H
DO NOT WRITE IN THIS AREA

C
H
H
C=C
H H
C C
H H H H

(i) Identify by name or formula a reagent for this reaction.

(1)

. .. ........ .. .. .. .. .. . .. .. .. .. .. .. .. .. .. .. ....................................................................... .. . . . . . . .. . ............................................................................................................................... . .. .. .. ... .. .. .. ... .. .

(ii) Draw the displayed formula of the other alkene formed.

(1)
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19
*P60464A01928* Turn over
(iii) Explain whether or not these two alkenes show geometric isomerism.
(2)

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........... .. .. .. .. .. .. .. .. .. . .. .. .. .. .. .. .. .. .. . .. . . .. . . .. . . .. . . .. . . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . . .. . . .. . . ............ ............................................................................................................................... .. .. ... .. .. .. ... .. .. ..

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............. .. .. .. .. .. .. .. .. .. .. .. .. . .. .. .. .. . .. . . .. . . .. . . .. . . .. . . .. . . .. . . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . ............ ............................................................................................................................... . .. .. .. .. ... .. .. ... .. .

............ . .. .. .. .. .. .. .. .. .. .. .. .. .. . .. .. .. ... . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . ............ ............................................................................................................................... . .. .. .. .. ... .. .. ... .. .

............. .. .. .. .. .. .. .. .. .. .. .. .. .. .. .. . .. ... . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . ............ ............................................................................................................................... . .. .. .. .. ... .. .. ... .. .

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(c) When dry hydrogen chloride gas reacts with 2-methylbut-2-ene, two isomeric
chloroalkanes are formed.
Give the structure of the major product and the reason why more of this is formed.

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(2)
Structure

Reason . . . . . . . . . . . . . . . . . . . . . . . . . . ...................................................................... .............................. .............................................................................................................. .. .. .. ... .. .. ... . . ..

............ .. .. . .. .. .. .. .. .. .. .. .. .. .. .. .. .. ... . . .. . . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . . .. . . .. . . .. . . .. . . .. . ............ .................................................................................................................................. .. ... .. .. .. ... .. .. .

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............ .. .. .. .. .. .. .. .. .. .. .. .. .. .. .. .. . .. . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. ............ ................................................................................................................................. ... .. .. .. ... .. .. ... .

20
*P60464A02028*
(d) The major product formed in (c) can also be formed from
2-methylbutan-2-ol (C5H11OH) in one step, using phosphorus(V) chloride.
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(i) Complete the equation for this reaction.

(1)

C5H11OH + PCl5

(ii) Give two reasons why this reaction would produce a greater yield of this
chloroalkane than the combined reactions in (b) and (c).
(2)

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............. .. .. .. .. .. .. .. .. .. .. .. .. . .. .. .. .. . .. . . .. . . .. . . .. . . .. . . .. . . .. . . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . ............ ............................................................................................................................... . .. .. .. .. ... .. .. ... .. .

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(iii) Give the bond and the wavenumber range of its absorption in the infrared spectrum of
2-methylbutan-2-ol which would not be in the infrared spectrum of this chloroalkane.
Use the Data Booklet.
(1)

........ ..... .. .. .. .. .. .. .. . .. .. .. .. .. .. .. .. .. .. . .. . . .. . . .. . . .. . . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . . .. . . .. . . ............ ............................................................................................................................... .. .. ... .. .. .. ... .. .. ..

......... .. .. .. .. .. .. .. .. .. . .. .. .. .. .. .. .. .. ...................................................................... . .. . . . . . . .. ................................................................................................................................ .. ... .. .. ... .. .. .. ...

(e) In the liver, enzymes oxidise some alcohols as part of the process which removes
them from the body. During this process any aldehydes produced are toxic.
Other alcohols are excreted unchanged. Between 1880 and 1950, 2-methylbutan-2-ol
was used as an anaesthetic.
Explain why 2-methylbutan-2-ol was preferred to 2-methylbutan-1-ol.
(2)

........ ..... .. .. .. .. .. .. .. . .. .. .. .. .. .. .. .. .. .. . .. . . .. . . .. . . .. . . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . . .. . . .. . . ............ ............................................................................................................................... .. .. ... .. .. .. ... .. .. ..

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........... .. .. .. .. .. .. .. .. .. . .. .. .. .. .. .. .. .. .. . .. . . .. . . .. . . .. . . .. . . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . . .. . . .. . . ............ ............................................................................................................................... .. .. ... .. .. .. ... .. .. ..

............ . .. .. .. .. .. .. .. .. .. .. . .. .. .. .. .. .. . .. . . .. . . .. . . .. . . .. . . .. . . .. . . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . . .. ............ ............................................................................................................................... .. .. ... .. .. .. ... .. .. ..

............. .. .. .. .. .. .. .. .. .. .. .. .. . .. .. .. .. . .. . . .. . . .. . . .. . . .. . . .. . . .. . . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . ............ ............................................................................................................................... . .. .. .. .. ... .. .. ... .. .

............ . .. .. .. .. .. .. .. .. .. .. .. .. .. . .. .. .. ... . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . ............ ............................................................................................................................... . .. .. .. .. ... .. .. ... .. .

............. .. .. .. .. .. .. .. .. .. .. .. .. .. .. .. . .. ... . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . ............ ............................................................................................................................... . .. .. .. .. ... .. .. ... .. .

(Total for Question 17 = 13 marks)

TOTAL FOR SECTION B = 41 MARKS

21
*P60464A02128* Turn over
SECTION C

Answer ALL the questions.

DO NOT WRITE IN THIS AREA

Write your answers in the spaces provided.

18 Urea (NH2CONH2) and ammonium nitrate (NH4NO3) are nitrogen-rich, water-soluble

fertilisers which are important to the agriculture industry worldwide.
Ammonium nitrate contains 35% nitrogen by mass.
(a) Calculate the percentage by mass of nitrogen in urea.
(2)

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(b) Urea is supplied as solid pellets and is used widely in Africa and Asia, particularly in the
cultivation of crops such as rice which are grown in fields immersed in water.
It hydrolyses to form ammonia and carbon dioxide.

NH2CONH2(s) + H2O(l) 2NH3(g) + CO2(g)

After the urea is applied to the soil, the ammonia formed may escape into the
atmosphere unless it dissolves in water. Crops cannot absorb ammonia or urea
directly but can take up and use dissolved ammonium ions.
Suggest why urea is used as a fertiliser for crops such as rice but not in regions
with unpredictable rainfall patterns.
(2)

........ ..... .. .. .. .. .. .. .. . .. .. .. .. .. .. .. .. .. .. . .. . . .. . . .. . . .. . . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . .. . . . .. . . .. . . ............ ............................................................................................................................... .. .. ... .. .. .. ... .. .. ..

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22
*P60464A02228*
(c) Both urea and ammonium nitrate are made from ammonia.
Ammonia is manufactured in the Haber process in which nitrogen and hydrogen are
passed over an iron catalyst at a temperature of 400 °C and a pressure of 200 atm.
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N2(g) + 3H2(g) 2NH3(g)

(i) Draw on the axes the Maxwell−Boltzmann distribution of molecular energies

of the reactant gases, showing on your diagram the activation energies for the
catalysed and uncatalysed reactions.
(3)

Number of
molecules
with a given
energy
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Energy, E

(ii) Explain, using your diagram, why the addition of a catalyst changes the rate of
the reaction.
(2)

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23
*P60464A02328* Turn over
(iii) Explain the effect of increasing the pressure on the equilibrium yield of ammonia.
(2)

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(d) Urea is also used in reducing harmful emissions from diesel engines which
operate at high temperatures and emit nitrogen monoxide, NO. One way to
decrease these emissions involves two reactions.
A solution of urea is added to the hot exhaust gases, and is hydrolysed.

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Reaction 1 NH2CONH2(aq) + H2O(l) 2NH3(g) + CO2(g)
The ammonia formed reacts with nitrogen monoxide and oxygen to form
harmless products.
(i) State why Reaction 1 is not a redox reaction.
(1)

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(ii) Suggest why it is an advantage to carry out Reaction 1 at a high temperature.

(2)

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(iii) The ammonia produced by the hydrolysis of urea reacts with nitrogen monoxide
and oxygen to produce nitrogen gas and water.
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Reaction 2 4NH3(g) + 4NO(g) + O2(g) 4N2(g) + 6H2O(g)

Explain, using oxidation numbers, why this reaction is a redox reaction but
not a disproportionation reaction.
(3)

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(iv) Give two reasons why it is important to remove nitrogen oxides from the
exhaust gases of diesel engines.
(2)

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(Total for Question 18 = 19 marks)

TOTAL FOR SECTION C = 19 MARKS

TOTAL FOR PAPER = 80 MARKS

25
*P60464A02528*
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*P60464A02628*
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*P60464A02728*
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*P60464A02828*
28
Please check the examination details below before entering your candidate information
Candidate surname Other names

Centre Number Candidate Number

October 2021

Pearson Edexcel International Advanced Level

Time 1 hour 30 minutes
Paper
reference WCH12/01
Chemistry
 

International Advanced Subsidiary/Advanced Level

UNIT 2: Energetics, Group Chemistry,
Halogenoalkanes and Alcohols
You must have: Total Marks
Scientific calculator, Data Booklet

Instructions
• Use black ink or black ball-point pen.
• centrethe
Fill in boxes at the top of this page with your name,
number and candidate number.
• Answer all questions.
• Answer the questions in the spaces provided
– there may be more space than you need.

Information
• The total mark for this paper is 80.
• The marks for each question are shown in brackets
– use this as a guide as to how much time to spend on each question.
• Into the question marked with an asterisk (*) marks will be awarded for your ability
structure your answer logically, showing how the points that you make are
related or follow on from each other where appropriate.
• A Periodic Table is printed on the back cover of this paper.

P67128A
©2021 Pearson Education Ltd.

E:1/1/1/1/1/1/E2/
*P67128A0128*
SECTION A
Answer ALL the questions in this section.
You should aim to spend no more than 20 minutes on this section.
For each question, select one answer from A to D and put a cross in the box .
If you change your mind, put a line through the box and then mark your new answer with
a cross .
1 The infrared spectrum of an organic compound is shown.

100
% Transmittance

0
4000 3000 2000 1500 1000 500
Wavenumber / cm–1

Which of these compounds would give this infrared spectrum?

A hexanal

B hexane
C hexanoic acid
D hexan-1-ol

(Total for Question 1 = 1 mark)

2 Which of these compounds does not react with acidified potassium dichromate(VI)?

A CH3CH2OH

B CH3CHOHCH3
C CH3CH2CHO

D CH3COCH3

(Total for Question 2 = 1 mark)

2
*P67128A0228* 
3 Which of these compounds is a tertiary alcohol?

A 2-methylpropan-2-ol

B 3-methylbutan-2-ol

C 2,2-dimethylpropan-1-ol
D 3,3-dimethylbutan-2-ol

(Total for Question 3 = 1 mark)

4 In a mass spectrum, the molecular ion is the ion which always has the

A greatest abundance

B greatest stability

C highest charge
D highest mass/charge ratio

(Total for Question 4 = 1 mark)

5 Butan-1-ol and butan-2-ol are isomers.

Which m / z value would be expected to have a significant peak in the mass spectrum
of butan-1-ol but not that of butan-2-ol?

A 15
B 29
C 43

D 57

(Total for Question 5 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

3
 *P67128A0328* Turn over
6 Which of these isomers has the highest boiling temperature?

(Total for Question 6 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

4
*P67128A0428* 
7 Organic reactions can be classified in different ways.
(a) How should the reaction shown be classified?
(1)

A addition

B oxidation
C polymerisation

D substitution

(b) How should the reaction shown be classified?

(1)

OH O

A addition

B oxidation
C reduction

D substitution

(Total for Question 7 = 2 marks)

Use this space for any rough working. Anything you write in this space will gain no credit.

5
 *P67128A0528* Turn over
8 Data for some Group 1 and Group 2 cations are shown in the table.

Cation Ionic radius / nm Ionic charge

W 0.100 +2

X 0.138 +1

Y 0.113 +2

Z 0.149 +1

Which cation would be expected to form the nitrate with the greatest
thermal stability?

A W
B X
C Y
D Z

(Total for Question 8 = 1 mark)

9 The equation for the complete combustion of propan-1-ol is shown.

C3H7OH(l) + 4½O2(g) ® 3CO2(g) + 4H2O(l)

2.00 × 10−3 mol of propan-1-ol undergoes complete combustion.

What mass of carbon dioxide is formed?

A 0.0293 g
B 0.0880 g

C 0.132 g

D 0.264 g

(Total for Question 9 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

6
*P67128A0628* 
10 This question is about the reaction shown.

2KMnO4 + xH2C2O4 + yH2SO4 ® 2MnSO4 + K2SO4 + 10CO2 + zH2O

(a) What values of x, y and z are needed to balance the equation?

(1)

x y z

A 5 6 8

B 10 3 4

C 5 3 8

D 10 6 4

(b) What is the reducing agent in the reaction?

(1)

A H+
B C2O42–
C MnO4–

D SO42–

(Total for Question 10 = 2 marks)

11 What is the oxidation number of phosphorus in the phosphate ion, PO43– ?

A –3

B +3

C +5
D +7

(Total for Question 11 = 1 mark)

12 Which reaction is not a redox reaction?

A 4KClO3(s) ® 3KClO4(s) + KCl(s)

B 2HCl(aq) + Ba(OH)2(aq) ® BaCl2(aq) + 2H2O(l)

C Zn(s) + CuSO4(aq) ® ZnSO4(aq) + Cu(s)

D Cl2(g) + H2O(l) ® HCl(aq) + HClO(aq)

(Total for Question 12 = 1 mark)

7
 *P67128A0728* Turn over
13 A student is provided with 25.0 cm3 of 1.00 mol dm–3 hydrochloric acid.
What volume of distilled water should the student add to this solution to make a
0.0500 mol dm–3 solution?

A 25.0 cm3
B 50.0 cm3

C 475 cm3

D 500 cm3

(Total for Question 13 = 1 mark)

14 Which statement about the Group 7 elements chlorine, bromine and iodine is
not correct?

A boiling temperature increases down the group

B reactivity increases down the group

C first ionisation energy decreases down the group
D electronegativity decreases down the group

(Total for Question 14 = 1 mark)

15 When iodine is dissolved in a non-polar organic solvent, the solution formed is

A purple
B orange

C colourless
D brown

(Total for Question 15 = 1 mark)

16 Which row shows the hydrogen halides in order of increasing boiling temperature?

Lowest Highest
A HF HCl HBr HI
B HI HBr HCl HF
C HCl HBr HI HF
D HF HI HBr HCl

(Total for Question 16 = 1 mark)

8
*P67128A0828* 
17 Solid potassium bromide reacts with concentrated sulfuric acid.
Which of these substances does not form?

A bromine

B hydrogen bromide
C hydrogen sulfide

D sulfur dioxide

(Total for Question 17 = 1 mark)

18 10.00 g of hydrated magnesium sulfate, MgSO4.7H2O, is heated to remove the

water of crystallisation.
What mass of anhydrous magnesium sulfate, MgSO4 , is formed?
[ Molar mass of MgSO4.7H2O = 246.4 g mol−1 ]

A 2.84 g
B 4.89 g
C 5.11 g
D 7.16 g

(Total for Question 18 = 1 mark)

TOTAL FOR SECTION A = 20 MARKS

9
 *P67128A0928* Turn over
SECTION B
Answer ALL the questions in this section.
Write your answers in the spaces provided.
19 This question is about enthalpy changes.
(a) An experiment was carried out to determine the enthalpy change of combustion
for ethanol.

C2H5OH(l) + 3O2(g) ® 2CO2(g) + 3H2O(l)

1.19 g of ethanol was burned in a spirit burner. The heat energy from this
combustion raised the temperature of 100 g of water from 21.6 °C to 63.9 °C.
(i) Calculate the number of moles of ethanol in 1.19 g.
[ Molar mass of ethanol = 46.0 g mol−1 ]
(1)

(ii) Calculate the heat energy required to raise the temperature of 100 g of water
from 21.6 °C to 63.9 °C.
[ Specific heat capacity of water = 4.18 J g−1 °C −1 ]
(2)

10
*P67128A01028* 
(iii) Use your answers to (a) (i) and (ii) to calculate a value for the
enthalpy change of combustion of ethanol.
Give your answer to an appropriate number of significant figures
and include a sign and units.
(3)

(iv) The value of the enthalpy change of combustion from this experiment was
very inaccurate.
Give two reasons why this value was so inaccurate, apart from heat loss.
(2)

11
 *P67128A01128* Turn over
(b) Mean bond enthalpies can be used to calculate a value for the enthalpy change of
combustion of a compound.
(i) Give the meaning of the term ‘mean bond enthalpy’.
(2)

(ii) Calculate a value for the enthalpy change of combustion of methanol, using
the information in the table and the equation shown.
(3)
CH3OH + 1½O2 ® CO2 + 2H2O

C–H C–O O–H O=O C=O

Mean bond enthalpy

413 358 464 498 805
/ kJ mol−1

12
*P67128A01228* 
(c) Enthalpy changes of combustion can be used to calculate the enthalpy change of
formation of a compound.

Standard enthalpy change of combustion,

Substance
∆c H / kJ mol−1

C(s,graphite) –394

H2(g) –286

CH3CHO(g) –1167

Complete the Hess cycle and use it to calculate the standard enthalpy change of
formation for ethanal, CH3CHO.
(3)

2C(s, graphite) + 2H2(g) + ½O2(g) ® CH3CHO(g)

(Total for Question 19 = 16 marks)

13
 *P67128A01328* Turn over
20 This question is about halogenoalkanes.
(a) The rates of hydrolysis of 1-chloropropane, 1-bromopropane and 1-iodopropane
in reactions with aqueous silver nitrate solution were compared.
(i) State what would be measured in the experiment to compare
the rates of hydrolysis.
(1)

(ii) State which of these halogenoalkanes would hydrolyse the fastest.

Justify your answer.
(2)

(b) The equation for the hydrolysis of 1-chloropropane by aqueous hydroxide ions
is shown.

CH3CH2CH2Cl + OH− ® CH3CH2CH2OH + Cl−

Give the mechanism for this hydrolysis.

Include curly arrows, and relevant dipoles and lone pairs.
(2)

14
*P67128A01428* 
(c) The boiling temperatures of some halogenoalkanes are shown.

Boiling temperature
Halogenoalkane
/ °C

1-chloropropane 47

1-bromopropane 71

1-iodopropane 103

Explain the trend in boiling temperature of these halogenoalkanes by comparing

the intermolecular forces involved.
Detailed explanations of the forces involved are not required.
(4)

15
 *P67128A01528* Turn over
(d) In another experiment, 2-bromobutane is heated with
ethanolic potassium hydroxide and an elimination reaction occurs.
Draw the skeletal formulae of the three possible organic products, giving
their names.
(3)

Skeletal formula Name

(Total for Question 20 = 12 marks)

16
*P67128A01628* 
21 This question is about Group 1 metals.
(a) When potassium is placed into a beaker of cold water, potassium hydroxide and
hydrogen are formed.
(i) Write the equation for this reaction. Include state symbols.
(2)

(ii) This is a redox reaction.

State which element is oxidised and which is reduced.
Justify your answer by giving the initial and final oxidation numbers of any
element that changes oxidation state.
(2)

(iii) The reaction of potassium with water is very vigorous and a flame is seen.

State the colour of the flame.

(1)

17
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(b) The label has come off a bottle known to contain M, a Group 1 metal which is
stored in oil.
A student carried out an experiment to determine the identity of M.
Procedure
Step 1 A small piece of M was wiped with tissue paper to remove the oil.
The piece of M was weighed and placed in a beaker of distilled water.
Step 2 After the reaction had finished, the contents of the beaker and washings
were transferred to a 250.0 cm3 volumetric flask. The solution was made
up to the mark with distilled water and mixed thoroughly.
Step 3 A pipette was used to transfer 25.0 cm3 portions of this solution to
conical flasks. Each portion was then titrated with hydrochloric acid of
concentration 0.400 mol dm–3 .
Results

Mass of metal, M 0.37 g

Mean titre of hydrochloric acid 12.80 cm3

The reaction taking place is shown.

MOH(aq) + HCl(aq) ® MCl(aq) + H2O(l)

(i) The indicator used was phenolphthalein.

State the colour change at the end-point.
(2)

from . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . ........ ....... ... .......... ........ to ........ .......... .......... .......... .......... .......... .......... .......... ........... ....

18
*P67128A01828* 
(ii) Calculate the relative atomic mass of M and use it to identify the Group 1
metal, M.
(4)

(c) Another student repeated the experiment, using a different sample of metal M,
but did not wipe off the oil before weighing it.
State how this would change the calculated value of the relative atomic mass
of M. Justify your answer.
(2)

(Total for Question 21 = 13 marks)

TOTAL FOR SECTION B = 41 MARKS

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*P67128A02028* 
SECTION C
Answer ALL the questions in this section.
Write your answers in the spaces provided.
22 This question is about ethanol and bioethanol.
The main fuel used as a petrol substitute is bioethanol. Bioethanol is ethanol that
has been produced by fermentation. The starting material is usually some form of
plant material rich in starch, such as wheat, maize or potatoes. Enzymes in yeast
convert this material to simple carbohydrates such as glucose (C6H12O6 ) and then to
ethanol and carbon dioxide.

C6H12O6 ® 2CH3CH2OH + 2CO2

The mixture is left for several days until fermentation is complete.

The percentage of ethanol is never greater than 15 % because higher concentrations
of ethanol kill the yeast.
A common blend of fuel is 95 % petrol and 5 % bioethanol. The engine does not need
to be modified for this mixture.
(a) Give one advantage and one disadvantage of using bioethanol in petrol.
(2)
Advantage

Disadvantage

(b) Suggest why this fermentation must be carried out in the absence of air.
(1)

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(d) Ethanol is hygroscopic, which means it readily absorbs water from the air.
(i) Give a possible reason why ethanol is able to absorb water.
(1)

(ii) Suggest a problem arising from the hygroscopic nature of ethanol when using
this fuel in a motor vehicle.
(1)

(e) Ethanol can also be produced by the hydration of ethene.

CH2 = CH2(g) + H2O(g)  CH3CH2OH(g) ∆H = − 45 kJ mol−1

*(i) Typical conditions are 300 °C and 60 atm with a catalyst of phosphoric acid.
Explain why these conditions are used, by describing the effect of changing
the temperature and pressure on rate of reaction, equilibrium yield and cost.
(6)

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(ii) The rate of this reaction is increased by using a catalyst of phosphoric acid.
Label the axes on the Maxwell–Boltzmann distribution curve and use it to
explain how a catalyst increases the rate of reaction.
(4)

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*P67128A02428* 
(f ) Catalysts such as phosphoric acid are bonded to a support material that contains
lots of pores.

support material

pores

(i) Suggest the advantage of using support materials containing lots of pores.
(1)

(ii) Under these conditions, only about 5 % of the ethene is converted into
ethanol as it passes over the catalyst.
Suggest how the overall yield of this process can be improved to make it
economically viable.
(2)

(Total for Question 22 = 19 marks)

TOTAL FOR SECTION C = 19 MARKS

TOTAL FOR PAPER = 80 MARKS

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*P67128A02828* 
Please check the examination details below before entering your candidate information
Candidate surname Other names

Centre Number Candidate Number

Pearson Edexcel International Advanced Level

Time 1 hour 30 minutes
Paper
reference WCH12/01
Chemistry
 

International Advanced Subsidiary/Advanced Level

UNIT 2: Energetics, Group Chemistry,
Halogenoalkanes and Alcohols
You must have: Total Marks
Scientific calculator, Data Booklet, ruler January 2022

P69501A
©2022 Pearson Education Ltd.

L:1/1/1/
*P69501A0128*
SECTION A

Answer ALL the questions in this section.

You should aim to spend no more than 20 minutes on this section.

For each question, select one answer from A to D and put a cross in the box . If you change
your mind, put a line through the box and then mark your new answer with a cross .

1 Which are correct for the reaction shown?

CH3COOH + KOH → CH3COO−K+ + H2O ΔH = –55.8 kJ mol−1

Type of reaction Type of enthalpy change

A endothermic formation
B endothermic neutralisation

C exothermic formation
D exothermic neutralisation

(Total for Question 1 = 1 mark)

2 Which equation does not represent a standard enthalpy change of atomisation?

A Mg(s) → Mg(g)
B Cl2(g) → 2Cl(g)

C ½O2(g) → O(g)
D Hg(l) → Hg(g)

(Total for Question 2 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

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*P69501A0228*
3 5.20 g of sodium hydrogencarbonate is added to an excess of acid.

The temperature increases and the energy change is calculated to be 1030 J.

What is the enthalpy change per mole of sodium hydrogencarbonate?

[Mr NaHCO3 = 84.0]

A –12.3 kJ mol−1

B –16.6 kJ mol−1

C –63.8 kJ mol−1
D –16 600 kJ mol−1

(Total for Question 3 = 1 mark)

4 The equation for the complete combustion of methanal is shown.

C + O O → O C O + O ΔH = –591 kJ mol−1
H H H H

Some bond enthalpy data are shown.

Bond Bond enthalpy / kJ mol−1

C H 413

O O 498

C O in CO2 805

O H 464

What is the C O bond enthalpy in methanal?

A 623 kJ mol−1

B 678 kJ mol−1

C 805 kJ mol−1
D 1036 kJ mol−1

(Total for Question 4 = 1 mark)

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5 Which sequence shows the molecules in order of increasing boiling temperature?

A H2O < Br2 < Cl2 < CH4

B Br2 < CH4 < Cl2 < H2O

C Cl2 < CH4 < H2O < Br2

D CH4 < Cl2 < Br2 < H2O

(Total for Question 5 = 1 mark)

6 Which is not correct about ice?

A ice has a lower density than water

B H2O molecules are further apart in ice than in water

C the H−O−H bond angle is the same in ice and in water

D H2O molecules in ice are held together by hydrogen bonds

(Total for Question 6 = 1 mark)

7 Which intermolecular forces exist between the molecules of the compound shown?

HO O

A hydrogen bonding and London forces only

B hydrogen bonding and permanent dipole-permanent dipole forces only
C London forces and permanent dipole-permanent dipole forces only

D hydrogen bonding, permanent dipole-permanent dipole forces and

London forces

(Total for Question 7 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

4
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8 This question is about alkanes.

(a) Which of these alkanes has the highest boiling temperature?

(1)
A butane
B hexane

C pentane

D propane

(b) Which of these alkanes has the lowest boiling temperature?

(1)

(Total for Question 8 = 2 marks)

9 Which solvent dissolves the greatest amount of hydrocarbon C35H72 ?

A butan-1-ol
B ethanoic acid

C hexane

D water

(Total for Question 9 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

5
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10 Which reagent would convert an alcohol into an alkene?

A acidified potassium dichromate(VI)

B anhydrous calcium sulfate

C concentrated phosphoric acid

D ethanolic potassium hydroxide

(Total for Question 10 = 1 mark)

11 Which name is correct for the ion SO42− ?

A sulfate(II)

B sulfate(IV)

C sulfate(VI)
D sulfate(VIII)

(Total for Question 11 = 1 mark)

12 In which compound is the oxidation number of nitrogen +5?

A Ca(NO3)2
B Mg3N2

C N2O3
D NaNO2

(Total for Question 12 = 1 mark)

13 In which reaction is the copper species acting as an oxidising agent?

A Cu2+ + 2Ag → 2Ag+ + Cu

B 2Cu+ + O2– → Cu2O

C 3Cu + O2 → Cu2O + CuO

D Cu + Hg2+ → Hg + Cu2+

(Total for Question 13 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

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14 Two half-equations for a reaction are shown.

Cu → Cu2+ + 2e−

NO3− + 4H+ + 3e− → NO + 2H2O

What is the overall ionic equation for this reaction?

A Cu + NO3− + 4H+ → Cu2+ + NO + 2H2O

B 2Cu + NO3− + 4H+ → 2Cu2+ + NO + 2H2O

C 3Cu + 2NO3− + 8H+ → 3Cu2+ + 2NO + 4H2O

D 6Cu + 2NO3− + 8H+ → 6Cu2+ + 2NO + 4H2O

(Total for Question 14 = 1 mark)

15 A titre of 13.25 cm3 was obtained using a 50 cm3 burette.

What is the percentage uncertainty in the titre?
[Each reading of the burette has an uncertainty of ± 0.05 cm3]

A ± 0.38 %
B ± 0.75 %

C ± 1.5 %
D ± 7.5 %

(Total for Question 15 = 1 mark)

16 Barium hydroxide reacts with sulfuric acid as shown.

Ba(OH)2(aq) + H2SO4(aq) → BaSO4(s) + 2H2O(l)

Which is the ionic equation for this reaction?

A Ba2+(aq) + 2OH−(aq) + 2H+(aq) + SO42−(aq) → BaSO4(s) + 2H2O(l)

B Ba2+(aq) + SO42−(aq) → BaSO4(s)

C OH−(aq) + H+(aq) → H2O(l)

D Ba2+(aq) + 2OH−(aq) + 2H+(aq) + SO42−(aq) → Ba2+(s) + SO42−(s) + 2H2O(l)

(Total for Question 16 = 1 mark)

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17 Four tests used to identify ions are shown:
1 flame test
2 addition of acidified barium nitrate solution
3 addition of acidified silver nitrate solution
4 addition of sodium hydroxide solution, then testing any gas with indicator paper
Which tests could be used to positively identify the ions in ammonium chloride?

A 1 and 2

B 1 and 3
C 2 and 4

D 3 and 4

(Total for Question 17 = 1 mark)

18 Which conditions give the highest yield for the forward reaction?

NH4Cl(s)  NH3(g) + HCl(g) ΔH = +176 kJ mol−1

A high temperature, high pressure

B high temperature, low pressure

C low temperature, high pressure

D low temperature, low pressure

(Total for Question 18 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

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19 Nitrogen dioxide and dinitrogen tetroxide exist in equilibrium.

2NO2(g)  N2O4(g)
brown gas colourless gas

When an equilibrium is set up in a gas syringe, the mixture is pale brown.

When the mixture is compressed the colour becomes

A darker

B lighter
C darker and then lighter

D lighter and then darker

(Total for Question 19 = 1 mark)

TOTAL FOR SECTION A = 20 MARKS

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SECTION B

Answer ALL the questions. Write your answers in the spaces provided.

20 Ammonia reacts with 1-chlorobutane.

(a) State the type and mechanism of this reaction.
(2)

(b) A student drew the first step of the mechanism for the reaction.

H H H H H H H H H
+
H C C C C Clδ– H C C C C N H + Cl–

H H H H H H H H H
N

HHH

(i) Identify two omissions in the student’s mechanism.

(2)

(ii) To obtain butylamine, sodium hydroxide solution is added.

Complete the next step of the mechanism to form butylamine,
showing curly arrows, relevant lone pairs and the reaction products.
(3)

H H H H H
+
H C C C C N H

H H H H H

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(c) The reactions of ammonia and of hydroxide ions with halogenoalkanes are similar.
Compare the rate of reaction of ammonia with 1-chlorobutane and with
2-bromo-2-methylpropane.
Justify your answer.
(3)

(Total for Question 20 = 10 marks)

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21 Enthalpy changes of combustion can be determined using calorimetry or calculated
using Hess cycles. Apparatus for a calorimetry experiment is shown.

thermometer

beaker
75 g water

spirit burner
2-methylpropan-2-ol

A sample of 2-methylpropan-2-ol was burned in a spirit burner and used to heat

75 g of water. The results are shown.

At the start At the end Change

Mass of spirit burner / g 267.35 266.78

Temperature of water / °C 19.5 65.3

(a) (i) Complete the table.

(1)
(ii) Calculate the enthalpy change of combustion, Δc H, of 2-methylpropan-2-ol.
Give a sign and units in your answer.
[Specific heat capacity of water = 4.18 J g−1 °C−1 ]
(4)

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(b) The standard enthalpy change of combustion, Δc H d , can be calculated using
standard enthalpy changes of formation.

Compound ∆ f H d / kJ mol−1

2-methylpropan-2-ol –359

carbon dioxide –394

water –286

(i) State why no ∆ f H d value has been given for oxygen.

(1)

(ii) Complete the Hess cycle.

C4H10O(l) + ...................... O2(g) ........ .......... .... CO2(g) + .... .......... ........ H2O(l)

4C(s, graphite) + .......... .......... .. + .. .......... ..........

(2)
(iii) Calculate the standard enthalpy change of combustion of
2-methylpropan-2-ol using the data in the table and the completed
Hess cycle.
(2)

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(c) The value for Δc H obtained in part (a)(ii) is much less exothermic than Δc H d
calculated in (b)(iii).
Suggest two reasons for this other than non-standard conditions.
(2)

(Total for Question 21 = 12 marks)

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*P69501A01428*
22 This question is about the elements in Group 7.
(a) Use your knowledge of the trends in the properties of Group 7 elements to
predict the colour and physical state of astatine at room temperature.
(1)

(b) (i) State the meaning of the term electronegativity.

(1)

(ii) Explain the trend in electronegativity down Group 7.

(2)

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*(c) Compare and contrast the reactions of chlorine with
• water
• cold, dilute aqueous alkali
• hot, concentrated aqueous alkali
Include an equation for each reaction, stating the type of reaction and the
oxidation numbers of the chlorine involved. State symbols are not required.
(6)

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(Total for Question 22 = 10 marks)

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23 Magnesium ethanedioate (MgC2O4) decomposes on gentle heating to form
magnesium carbonate and carbon monoxide.

MgC2O4 → MgCO3 + CO

(a) (i) State why the thermal decomposition of magnesium ethanedioate should be
carried out in a fume cupboard.
(1)

(ii) After heating a 6.0 g sample of magnesium ethanedioate for three minutes,
the decomposition was 70 % complete.
Calculate the total mass of the solid mixture that remains.
(4)

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*P69501A01828* 
(b) Magnesium carbonate undergoes thermal decomposition at a higher
temperature than magnesium ethanedioate.

MgCO3 → MgO + CO2

Explain the trend in the thermal decomposition of Group 2 carbonates going

down the group.
(3)

(Total for Question 23 = 8 marks)

TOTAL FOR SECTION B = 40 MARKS

19
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SECTION C

Answer all the questions. Write your answers in the spaces provided.

24 Some diesel cars contain an extra catalytic converter for the reduction of
nitrogen oxides (NOx) in exhaust gases.
A solution of urea is used for this process.

H C H
N N
urea
H H

(a) Urea has a melting temperature of 133 °C.

Explain why this value is higher than expected for a relatively small molecule.
(3)

(b) A saturated solution of urea has a concentration of 9.07 mol dm–3 at 25 °C.
Calculate the mass of urea in 150 cm3 of a saturated solution.
(2)

20
*P69501A02028* 
(c) State why NOx emissions are harmful to the environment.
(1)

(d) An infrared spectrum of urea is shown.

Refer to your Data Booklet.

100

Transmittance
50
/%

0
4000 3000 2000 1500 1000 500
–1
Wavenumber / cm

(i) Draw a circle around an absorption in the spectrum that could be due to the
stretching of the N H bond.
(1)
(ii) Identify the bond responsible for the absorption at 1683 cm−1.
(1)

(e) In a diesel car exhaust system, the urea reacts with water to form ammonia and
carbon dioxide. The enthalpy change for this reaction is +133 kJ mol−1.
(i) Complete the equation for this reversible reaction.
State symbols are not required.
(1)

(NH2)2CO + H2O . . . . . . . . . . . . . . . . . . . ......... ...... .... .......... .......... .......... .......... .......... .......... .......... .......... ......... . .......... .......... .......... ...

21
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(ii) Sketch the reaction profile for the forward reaction on the axes provided.
Include labels for ΔH and the activation energy (Ea).

Energy

Reaction progress
(3)

(f ) The catalytic converter contains metal oxides. When the exhaust gases pass
through the catalytic converter, ammonia reacts with NOx gases to form nitrogen
and water.
(i) Explain why it is not correct to state that urea is acting as a catalyst in the
reaction.
(1)

22
*P69501A02228* 
(ii) Explain how a catalyst increases the rate of a chemical reaction.
Use the Maxwell-Boltzmann distribution shown and refer to the
collision theory.
(3)

Number of
particles with
energy, E

Ea Energy, E

(g) The catalytic converter works best at a temperature of around 350 °C.
(i) Suggest how the catalytic converter reaches this temperature.
(1)

23
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(ii) The chemical reactions in the exhaust system of a diesel car, using
a catalytic converter, form 89.3 m3 of nitrogen per hour.
Calculate the number of molecules of nitrogen formed per hour.
[Molar volume at 350 °C = 51.1 dm3 mol−1
Avogadro constant, L = 6.02 × 1023 mol−1]
(3)

(Total for Question 24 = 20 marks)

TOTAL FOR SECTION C = 20 MARKS

TOTAL FOR PAPER = 80 MARKS

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 *P69501A02728*
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*P69501A02828* 
Please check the examination details below before entering your candidate information
Candidate surname Other names

Pearson Edexcel Centre Number Candidate Number

International
Advanced Level

Friday 11 October 2019

Morning (Time: 1 hour 30 minutes) Paper Reference WCH12/01

Chemistry
International Advanced Subsidiary Level
Unit 2: Energetics, Group Chemistry, Halogenoalkanes and
Alcohols
Candidates must have: Scientific calculator Total Marks
Data Booklet
Ruler

Information
• The total mark for this paper is 80.
• The marks for each question are shown in brackets
– use this as a guide as to how much time to spend on each question.
• ability
In the question marked with an asterisk (*), marks will be awarded for your
to structure your answer logically, showing how the points that you make
are related or follow on from each other where appropriate.
• There is a Periodic Table on the back cover of this paper.

P61657A
©2019 Pearson Education Ltd.

1/1/1/1/1/1/1/
*P61657A0128*
SECTION A

Answer ALL the questions in this section.

DO NOT WRITE IN THIS AREA

You should aim to spend no more than 20 minutes on this section.

For each question, select one answer from A to D and put a cross in the box .
If you change your mind, put a line through the box and then mark your new answer
with a cross .

1 Lithium carbonate decomposes on heating.

Li2CO3(s) Li2O(s) + CO2(g)

What is the maximum volume, in dm3, measured at room temperature and pressure (r.t.p.),
of gas produced from 3.69 g of lithium carbonate?
[Mr Li2CO3 = 73.8 Molar volume of a gas at r.t.p. = 24.0 dm3 mol−1]
A 24.0
B 12.0

DO NOT WRITE IN THIS AREA

C 1.20
D 0.83

(Total for Question 1 = 1 mark)

2 A sample of 1,2-dichloroethane, CH2ClCH2Cl, contains only the isotopes 1H, 12C, 35Cl and 37Cl.
How many molecular ion peaks are there in its mass spectrum?
A 1
B 2
C 3
D 4 DO NOT WRITE IN THIS AREA

(Total for Question 2 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

2
*P61657A0228*
3 Under certain conditions, graphite burns to form carbon monoxide.
2C(s) + O2(g) 2CO(g) H = −221 kJ mol−1
DO NOT WRITE IN THIS AREA

Which of these is correct?

A c H (carbon) = −221 kJ mol−1
B f H (carbon monoxide) = −221 kJ mol−1
C c H (carbon) = −110.5 kJ mol−1
D f H (carbon monoxide) = −110.5 kJ mol−1

(Total for Question 3 = 1 mark)

4 What are the strongest interactions between molecules in solid hydrogen iodide, HI?
A covalent bonds
B hydrogen bonds
C ionic bonds
DO NOT WRITE IN THIS AREA

D London forces

(Total for Question 4 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.
DO NOT WRITE IN THIS AREA

3
*P61657A0328* Turn over
5 Equations for four reactions of copper or its compounds are shown.
Reaction 1 2Cu2+ + 4I− 2CuI + I2

DO NOT WRITE IN THIS AREA

Reaction 2 Cu + 4HNO3 Cu(NO3)2 + 2NO2 + 2H2O
Reaction 3 2Cu+ Cu + Cu2+
Reaction 4 CuO + H2SO4 CuSO4 + H2O

(a) Which is a disproportionation reaction?

(1)
A Reaction 1
B Reaction 2
C Reaction 3
D Reaction 4

(b) Which is an acid-base reaction?

DO NOT WRITE IN THIS AREA

(1)
A Reaction 1
B Reaction 2
C Reaction 3
D Reaction 4

(Total for Question 5 = 2 marks)

6 Which statement is correct?

A barium carbonate is less stable to heat than magnesium carbonate
B barium hydroxide is less soluble in water than magnesium hydroxide
C barium sulfate is less soluble in water than magnesium sulfate DO NOT WRITE IN THIS AREA

D barium metal is less reactive with water than magnesium metal

(Total for Question 6 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

4
*P61657A0428*
7 Which statement is not correct?
A chlorine is more electronegative than bromine
DO NOT WRITE IN THIS AREA

B chlorine is more reactive than bromine

C chloride ions are stronger reducing agents than bromide ions
D chloride ions are stronger reducing agents than fluoride ions

(Total for Question 7 = 1 mark)

8 A white solid X produces a red colour in a flame test.

When aqueous silver nitrate and nitric acid are added to a solution of X,
a cream precipitate is formed which dissolves in concentrated aqueous ammonia.
What is the formula of X?
A SrBr2
B NaBr
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C LiCl
D BaI2

(Total for Question 8 = 1 mark)

9 Exactly 50.0 cm3 of 2.00 mol dm−3 nitric acid reacts with 50.0 cm3 of 1.00 mol dm−3
barium hydroxide to form a neutral solution of barium nitrate.
(a) What is the concentration, in mol dm−3, of barium nitrate in the solution?
(1)
A 0.05
B 0.50
C 1.00
D 2.00
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(b) The volume of the nitric acid is measured using a burette.

Each burette reading has an uncertainty of ± 0.05 cm3.
What is the percentage uncertainty in measuring 50.00 cm3 of the nitric acid?
(1)
A ± 0.40%
B ± 0.20%
C ± 0.10%
D ± 0.05%
(Total for Question 9 = 2 marks)

5
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10 Which of these products are formed when chlorine is passed through cold, dilute
aqueous sodium hydroxide?

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A NaCl and NaClO
B NaClO and NaClO3
C NaCl and NaClO3
D NaClO and NaClO4

(Total for Question 10 = 1 mark)

11 Potassium iodide reacts with concentrated sulfuric acid.

Which of the following is not a product?
A H2S
B I2
C S

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D SO3

(Total for Question 11 = 1 mark)

12 Sodium thiosulfate solution reacts with hydrochloric acid to produce solid sulfur.
Which change would be expected to increase the time taken for sulfur to appear?
A increasing the concentration of the hydrochloric acid
B decreasing the concentration of the sodium thiosulfate
C increasing the temperature
D adding a catalyst

(Total for Question 12 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.
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6
*P61657A0628*
13 The equation for a reversible reaction is shown.

PCl3(g) + Cl2(g) PCl5(g) H = −88 kJ mol−1

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What effect will each change have on the rate of reaction and the equilibrium yield of
phosphorus(V) chloride?
(a) Increasing the temperature at constant pressure.
(1)

Effect on rate of reaction Effect on yield of PCl5(g)

A increase decrease

B decrease decrease
C increase increase

D decrease increase
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(b) Increasing the pressure at constant temperature.

(1)

Effect on rate of reaction Effect on yield of PCl5(g)

A increase decrease

B decrease decrease
C increase increase

D decrease increase

(Total for Question 13 = 2 marks)

14 A chloroalkane is heated with dilute aqueous sodium hydroxide and the pure organic
product is obtained.
When the organic product is warmed with acidified potassium dichromate(VI) solution,
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there is no change in colour.

The chloroalkane could be
A 1-chlorobutane
B 2-chloro-2-methylpropane
C 1-chloro-2-methylpropane
D 2-chlorobutane

(Total for Question 14 = 1 mark)

7
*P61657A0728* Turn over
15 This question is about two isomeric alcohols and two isomeric carbonyl compounds.

propan-1-ol, CH3CH2CH2OH and propan-2-ol, CH3CH(OH)CH3

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propanal, CH3CH2CHO and propanone, CH3COCH3

(a) Which reaction is possible?

(1)
A reducing propan-1-ol to propanal
B oxidising propan-1-ol to propanal
C reducing propanal to propanone
D oxidising propan-1-ol to propanone

(b) Which compound would be expected to give a significant peak at m / z = 31 in its

mass spectrum?
(1)
A propan-1-ol

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B propan-2-ol
C propanal
D propanone

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*P61657A0828*
(c) The infrared spectrum of one of the four compounds is shown.

100
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Transmittance (%)

0
4000 3000 2000 1500 1000 500
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Wavenumber / cm–1

Identify the compound, using the infrared absorptions from the Data Booklet.
(1)
A propan-1-ol
B propan-2-ol
C propanal
D propanone

(Total for Question 15 = 3 marks)

TOTAL FOR SECTION A = 20 MARKS

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9
*P61657A0928* Turn over
SECTION B

Answer ALL the questions. Write your answers in the spaces provided.

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16 Group 2 hydroxides, M(OH)2 , are used to neutralise acids.
(a) Write an equation for the reaction of calcium with cold water.
State symbols are not required.
(1)

(b) Explain why a saturated solution of calcium hydroxide is more alkaline than a
saturated solution of magnesium hydroxide.
(2)

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(c) A solution was tested for the presence of carbonate ions.

Dilute hydrochloric acid was added to the solution and the gas given off was bubbled
through limewater (aqueous calcium hydroxide). A white precipitate formed.
(i) Write the ionic equation for the formation of the gas.
State symbols are not required.
(1)
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*P61657A01028*
(ii) Write the equation for the formation of the precipitate.
Include state symbols.
(2)
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(d) Magnesium hydroxide can be used to neutralise hydrochloric acid in the stomach
to relieve acid indigestion.

Mg(OH)2 + 2HCl MgCl2 + 2H2O

Calculate the minimum mass of magnesium hydroxide needed to neutralise
0.150 mol of hydrochloric acid.
Give your answer to an appropriate number of significant figures.
(3)
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(Total for Question 16 = 9 marks)

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*P61657A01128* Turn over
17 Biobutanol is a possible alternative to bioethanol as an additive to petrol.
(a) (i) Complete the table for the four isomers of C4H9OH which are alcohols.

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(3)

Boiling
Skeletal formula Name Classification
temperature / °C

OH butan-1-ol primary 117

OH 108

99
OH

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2-methylpropan-2-ol 82

(ii) Explain the difference in boiling temperature between butan-1-ol and

2-methylpropan-2-ol.
(2)

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*P61657A01228*
(iii) The displayed formula of butan-1-ol is shown.
Complete the diagram to show the strongest intermolecular force between
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two molecules of butan-1-ol. Include the intermolecular bond angle.

(2)

H H H H H
H C C C C O
H H H H
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13
*P61657A01328* Turn over
(b) (i) Complete the equation for the combustion of butan-1-ol.
State symbols are not required.
(1)

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H H H H H
H C C C C O + . . .. . . . . . . . . . . . . . .. . . . O O ...................... O C O + ...................... H O H
H H H H

(ii) Calculate a value for the enthalpy change of combustion of butan-1-ol using
the equation in (b)(i) and the mean bond enthalpies in the table.
(3)

Bond C C C O C O C H O H O O

Mean bond enthalpy / kJ mol−1 347 358 805 413 464 498

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*P61657A01428*
(iii) A data book value of the molar enthalpy change of combustion of butan-1-ol
is −2670 kJ mol−1
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Give two reasons for the difference between this value and the value
calculated in (b)(ii).
(2)

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(c) Biobutanol has some advantages over bioethanol.

(i) The combustion of bioethanol releases 23 MJ dm−3 compared to petrol which
releases 32 MJ dm−3.
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Calculate the energy released in MJ dm−3 for the combustion of biobutanol.

Biofuel Formula c H / kJ mol−1 Density / g cm−3

biobutanol C4H9OH −2670 0.810

(2)
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15
*P61657A01528* Turn over
(ii) Biobutanol can be mixed with petrol in any proportion whereas bioethanol cannot.
Petrol is a mixture of liquid alkanes.

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Explain why petrol is more miscible with biobutanol than with bioethanol.
(2)

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(Total for Question 17 = 17 marks)

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*P61657A01628*
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BLANK PAGE

*P61657A01728*
17
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18 Two different processes can be used for the production of chloroethene (CH2 CHCl),
which is the monomer for the manufacture of poly(chloroethene).

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(a) Process A
Ethene, produced from crude oil, reacts with chlorine gas to form 1,2-dichloroethane.
The 1,2-dichloroethane is then thermally cracked to form chloroethene.

Reaction 1
C2H4(g) + Cl2(g) C2H4Cl2(g)

Reaction 2
C2H4Cl2(g) C2H3Cl(g) + HCl(g)

(i) A student wrote a mechanism for Reaction 1.

H H H H H H
δ+
H C C H H C C H H C C H

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Cl – Cl Cl
Cl δ + Cl:

Cl δ –

The mechanism contains two mistakes.

Identify each mistake, giving the correction that should be made.
(2)

Mistake 1. . . .. . . . . . . .. . . . . . . .. . . . . . . . . . .. . . . . . . . . . . . . . .. . . . . . . . . . . . . . . .. . . . . . . . . . . . . . .. . . . . . . . . . . . . .................................... ....................................................................................................... .....................

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Correction . . .. . . . . . .. . . . . . . ....................................................................... . . . . . . . . . . . . . . . . . . . . . . . . .. . . . . . . . . . . . . .................................................................................................... .....................

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Mistake 2. . . .. . . . . . . .. . . . . . . .. . . . . . . . . . .. . . . . . . . . . . . . . .. . . . . . . . . . . . . . . .. . . . . . . . . . . . . . .. . . . . . . . . . . . . .................................... ....................................................................................................... .....................

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Correction . . .. . . . . . .. . . . . . . ....................................................................... . . . . . . . . . . . . . . . . . . . . . . . . .. . . . . . . . . . . . . .................................................................................................... .....................

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18
*P61657A01828*
(ii) Write the overall equation for Process A and use it to calculate the percentage
atom economy by mass for the production of chloroethene.
(3)
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(b) Process B
In an alternative process, chloroethene is obtained by reacting ethyne (HC CH), with
hydrogen chloride. Ethyne is produced from coal. This reaction uses a catalyst of
mercury(II) chloride which is highly toxic.

HC CH(g) + HCl(g) C2H3Cl(g)

The temperature during this reaction is high enough to vaporise the
mercury(II) chloride catalyst.
State how Process A compares to Process B in terms of the percentage atom economy
by mass and environmental impact of each process. No calculation is needed.
(2)

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19
*P61657A01928* Turn over
*(c) Process B involves gas molecules reacting at high temperature in the
presence of a catalyst.

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Explain the effects on the rate of reaction of increasing the temperature and using
a catalyst in Process B, referring to a labelled diagram of
the Maxwell-Boltzmann distribution.
(6)

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20
*P61657A02028*
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(Total for Question 18 = 13 marks)

TOTAL FOR SECTION B = 39 MARKS

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22
SECTION C

Answer ALL the questions. Write your answers in the spaces provided.
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19 Major volcanic eruptions, such as the one in Indonesia in 1815, eject large amounts of
ash and gases into the atmosphere. The gases include carbon dioxide, water vapour,
hydrogen chloride and sulfur dioxide.
(a) (i) Complete the dot-and-cross diagram to show a possible arrangement of the
outer shell electrons in a molecule of sulfur dioxide.
Use dots (•) for the sulfur electrons and crosses (×) for the oxygen electrons.
(2)

O S O
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(ii) Suggest a value for the bond angle.

(1)

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(b) The levels of sulfur dioxide in the atmosphere can be measured by collection and
titration with sodium hydroxide solution.

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One possible method is:
• air containing sulfur dioxide is bubbled through hydrogen peroxide solution
• all the sulfur dioxide reacts to form 40.0 cm3 of dilute sulfuric acid, solution Z

SO2(g) + H2O2(aq) H2SO4(aq)

• a pipette is used to remove 10.0 cm3 portions of solution Z

• each portion is titrated with 0.00500 mol dm−3 sodium hydroxide.
The results are shown in the table.

Titration 1 2 3

Final volume / cm3 21.55 42.70 21.05

Initial volume / cm3 0.00 21.55 0.00

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Titre / cm3 21.55 21.15 21.05

The mean titre is 21.10 cm3

(i) Give a reason why a further titration was not attempted.
(1)

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(ii) Calculate the number of moles of sulfuric acid in the 40 cm3 of solution Z.

2NaOH(aq) + H2SO4(aq) Na2SO4(aq) + 2H2O(aq)

(3)
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(iii) Deduce the number of moles of sulfur dioxide bubbled through the
hydrogen peroxide solution, using the answer from (b)(ii) and the equation
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SO2(g) + H2O2(aq) H2SO4(aq)

(1)

(iv) The air containing sulfur dioxide was bubbled through the hydrogen peroxide
solution at a rate of 10 dm3 min−1 for 30 minutes.
Calculate the concentration of sulfur dioxide in the air in parts per million
(ppm) by volume.
The molar volume of a gas at r.t.p. is 24 dm3 mol−1.
(3)
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(c) (i) During a volcanic eruption, hydrogen chloride gas is also released into the upper
atmosphere, which in turn produces some chlorine free radicals. Chlorine free
radicals react with ozone:

Cl• + O3 ClO• + O2

ClO• + O3 Cl• + 2O2

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Derive the overall equation for this reaction of ozone.

State symbols are not required.
(1)

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(ii) Give two reasons why the presence of a small number of chlorine free radicals in the
upper atmosphere causes a large decrease in the amount of ozone.
(2)

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(d) (i) Sulfur dioxide is converted into sulfur trioxide in the upper atmosphere in the
presence of ultraviolet light.

2SO2(g) + O2(g) 2SO3(g)

Show, by use of all the relevant oxidation numbers, that this is a redox reaction.
(2)

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(ii) Sulfur trioxide reacts with water to produce sulfuric acid.

SO3(g) + H2O(l) H2SO4(aq) r H = −200 kJ mol−1

Draw an enthalpy level diagram to show the enthalpy change for this reaction.
(2)

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Enthalpy

Reaction pathway

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(iii) Droplets of sulfuric acid are formed when sulfur trioxide reacts with water in the
upper atmosphere. These droplets reflect ultraviolet radiation from the Sun back
into space.
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In the volcanic eruption in Indonesia in 1815, large amounts of both carbon dioxide
and sulfur dioxide were released.
During the following year, there were global low temperatures.
Assess the effect of both gases on global temperatures after the volcanic eruption.
(3)

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(Total for Question 19 = 21 marks)

TOTAL FOR SECTION C = 21 MARKS

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TOTAL FOR PAPER = 80 MARKS

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28
Please check the examination details below before entering your candidate information
Candidate surname Other names

Centre Number Candidate Number

Pearson Edexcel International Advanced Level

Time 1 hour 30 minutes
Paper
reference WCH12/01
Chemistry
 

International Advanced Subsidiary/Advanced Level

UNIT 2: Energetics, Group Chemistry,
Halogenoalkanes and Alcohols
You must have: Total Marks
Scientific calculator, Data Booklet, ruler October 2022

Instructions
• Use black ink or ball-point pen.
• centrethe
Fill in boxes at the top of this page with your name,
number and candidate number.
• Answer all questions.
• Answer the questions in the spaces provided
– there may be more space than you need.

Information
• The total mark for this paper is 80.
• The marks for each question are shown in brackets
– use this as a guide as to how much time to spend on each question.
• toIn the question marked with an asterisk (*), marks will be awarded for your ability
structure your answer logically, showing how the points that you make are
related or follow on from each other where appropriate.
• A Periodic Table is printed on the back cover of this paper.

Advice
• Read each question carefully before you start to answer it.
• Show all your working in calculations and include units where appropriate.
• Try to answer every question.
• your answers if you have time at the end.
Check

Turn over

P71861A
©2022 Pearson Education Ltd.

B:1/1/1/1/
*P71861A0124*
SECTION A
Answer ALL the questions in this section.
You should aim to spend no more than 20 minutes on this section.
For each question, select one answer from A to D and put a cross in the box . If you change
your mind, put a line through the box and then mark your new answer with a cross .
1 Hydrogen reacts with oxygen to form steam.

H2(g) + ½O2(g) → H2O(g) ∆H = −242 kJ mol−1

Bond Bond enthalpy / kJ mol−1

H H 436

O O 498

What is the bond enthalpy of the O H bond, in kJ mol−1?

A 221.5
B 463.5

C 588
D 927

(Total for Question 1 = 1 mark)

2 Which equation shows the standard enthalpy change of formation of

sodium chloride?
A Na(s) + ½Cl2(g) → NaCl(s)
B 2Na(s) + Cl2(g) → 2NaCl(s)

C Na(g) + Cl(g) → NaCl(s)

D Na+(g) + Cl−(g) → NaCl(s)

(Total for Question 2 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

2
*P71861A0224* 
3 Some enthalpy changes of combustion are shown.

Substance Enthalpy change of combustion / kJ mol−1

CH3CHO(l) −1167

C(s) −394

H2(g) −286

What is the enthalpy change of formation of ethanal, CH3CHO, in kJ mol−1?

A +765

B −765

C +193
D −193

(Total for Question 3 = 1 mark)

4 What is the mass of carbon formed when 1.80 g of propan-1-ol, C3H7OH, undergoes
incomplete combustion according to the equation shown?

C3H7OH(l) + 2O2(g) → 2C(s) + CO(g) + 4H2O(l)

A 0.18 g
B 0.36 g

C 0.72 g

D 1.08 g

(Total for Question 4 = 1 mark)

5 Which property decreases as Group 2 of the Periodic Table is descended?

A reactivity of the elements

B solubility of the hydroxides

C solubility of the sulfates

D thermal stability of the carbonates

(Total for Question 5 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

3
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6 How many structural isomers with the molecular formula C5H10O react with Benedict’s
or Fehling’s solutions?
A 2

B 3
C 4

D 5

(Total for Question 6 = 1 mark)

7 Butanenitrile can be formed by reacting 1-bromopropane with potassium cyanide.

Which is the correct mechanism and type of reaction that occurs?

A electrophilic addition

B nucleophilic addition
C electrophilic substitution
D nucleophilic substitution

(Total for Question 7 = 1 mark)

8 What produces the colour in a flame test?

Energy change of electrons Movement of electrons

A energy absorbed from ground state to excited state
B energy emitted from ground state to excited state
C energy absorbed from excited state to ground state
D energy emitted from excited state to ground state

(Total for Question 8 = 1 mark)

9 Why is the boiling temperature of hydrogen iodide higher than that of

hydrogen bromide?
A hydrogen iodide has stronger London forces than hydrogen bromide

B hydrogen iodide has a larger permanent dipole than hydrogen bromide

C hydrogen iodide has stronger hydrogen bonds than hydrogen bromide

D the H I bond is stronger than the H Br bond

(Total for Question 9 = 1 mark)

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10 Which nitrate forms oxygen as the only gaseous product on heating?

A LiNO3

B NaNO3

C Mg(NO3)2
D Ca(NO3)2

(Total for Question 10 = 1 mark)

11 Which compound has the highest boiling temperature?

OH
A

B OH

(Total for Question 11 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

5
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12 Which compound does not form hydrogen bonds between its molecules?

A HCl

B H2O

C HF
D NH3

(Total for Question 12 = 1 mark)

13 What is the oxidation number of bromine in BrO3− ?

A +1

B +3

C +5
D +7

(Total for Question 13 = 1 mark)

14 Which reaction is not a disproportionation?

A 3Cl2(g) + 6NaOH(aq) → NaClO3(aq) + 5NaCl(aq) + 3H2O(l)

B 2H2O2(l) → 2H2O(l) + O2(g)

C Cl2(g) + H2O(l) → HCl(aq) + HClO(aq)

D Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s)

(Total for Question 14 = 1 mark)

15 Which trend is not correct as Group 7 is descended?

A atomic radius of the elements increases

B boiling temperature of the elements increases

C electronegativity of the elements decreases

D reactivity of the elements increases

(Total for Question 15 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

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16 The results of an experiment to determine the rate of the reaction between
magnesium and hydrochloric acid are shown.

120

100

80
Volume of hydrogen
/ cm3
60

0
0 20 40 60 80 100 120
Time / s

What is the approximate rate of reaction in cm3 s−1 at 40 seconds?

A 0.75

B 1.3
C 2.2

D 6.0

(Total for Question 16 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

7
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17 A Maxwell-Boltzmann distribution curve for the particles present in a
reaction mixture is shown.

Number of
particles with
energy, E

X Ea
Energy

(a) Which statement is correct?

(1)
A position X represents the mean energy of the particles

B activation energy, Ea , is the mean energy of the particles that react

C the area under the curve to the right of the activation energy, Ea ,
represents the number of particles with enough energy to react
D adding a catalyst moves the activation energy, Ea , to the right

(b) What happens to the distribution curve when the temperature of the gas
is decreased?
(1)

Position of the peak Height of the peak

A shifts to the right lower
B shifts to the right higher
C shifts to the left lower
D shifts to the left higher

(Total for Question 17 = 2 marks)

Use this space for any rough working. Anything you write in this space will gain no credit.

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*P71861A0824* 
18 Part of a reaction mechanism is shown.

H H H H :Br−
1 +
δ+ δ−
H C C Br H C C NH2
3
H H 2 H H H
:NH3 4 :NH3

Which curly arrow in the mechanism is not correct?

A arrow 1
B arrow 2

C arrow 3

D arrow 4

(Total for Question 18 = 1 mark)

19 A student carries out two sets of titrations, one using methyl orange and the other
using phenolphthalein as indicators.
The conical flask contains sodium hydroxide solution and the burette contains
hydrochloric acid.
What are the colour changes at the end-points?

Methyl orange Phenolphthalein

A red to orange colourless to pink

B yellow to orange pink to colourless

C red to orange pink to colourless

D yellow to orange colourless to pink

(Total for Question 19 = 1 mark)

TOTAL FOR SECTION A = 20 MARKS

9
 *P71861A0924* Turn over
SECTION B
Answer ALL the questions. Write your answers in the spaces provided.
20 A student carries out two experiments and uses the results to determine
the enthalpy change when anhydrous copper(II) sulfate forms
hydrated copper(II) sulfate, CuSO4·5H2O.

CuSO4(s) + 5H2O(l) → CuSO4·5H2O(s)

(a) In the first experiment, the student determines the enthalpy change when
hydrated copper(II) sulfate dissolves in water.

CuSO4·5H2O(s) + aq → CuSO4(aq)

10.68 g of hydrated copper(II) sulfate is added to distilled water in a

polystyrene cup to give 55.0 g of solution.
The mixture is stirred and the temperature change determined.
Results
Initial temperature = 21.0 °C
Minimum temperature = 18.5 °C
Calculate the enthalpy change for this reaction.
Give your answer to an appropriate number of significant figures.
Include a sign and units.
Data: Specific heat capacity of the solution = 3.70 J g−1 °C−1
Molar mass CuSO4·5H2O = 249.6 g mol−1
(4)

10
*P71861A01024* 
(b) In the second experiment, the student determined the enthalpy change of the
reaction when anhydrous copper(II) sulfate dissolves in water.

CuSO4(s) + aq → CuSO4(aq) ∆H = −67.4 kJ mol−1

(i) Complete the Hess cycle.

(2)

CuSO4(s) + 5H2O(l) CuSO4 ·5H2O(s)

(ii) Calculate the enthalpy change when anhydrous copper(II) sulfate forms
hydrated copper(II) sulfate. Include a sign and units.
(2)

(Total for Question 20 = 8 marks)

11
 *P71861A01124* Turn over
21 This question is about sulfuric acid.
(a) Sulfuric acid is manufactured in a three-step process.
Step 1 S(s) + O2(g) → SO2(g)
Step 2 2SO2(g) + O2(g)  2SO3(g)
Step 3 SO3(g) + H2O(l) → H2SO4(l)
(i) At room temperature and pressure, sulfur is a solid and oxygen a gas.
Explain why sulfur and oxygen exist in different states by referring to the
intermolecular forces involved.
(2)

(ii) Step 2 is a reversible reaction.

2SO2(g) + O2(g)  2SO3(g) ∆H = −196 kJ mol−1

State the effect on the position of equilibrium when the temperature and
pressure are increased. Justify your answers.
(4)
Increasing temperature at constant pressure

Increasing pressure at constant temperature

12
*P71861A01224* 
(iii) Vanadium(V) oxide, V2O5 , is used to catalyse the reaction in Step 2.
Complete the reaction profile to show both the catalysed and
uncatalysed reactions.
Label the activation energy and the enthalpy change.
Your diagram does not have to be to scale.
(4)

Energy

Progress of reaction

(iv) Explain how the use of a catalyst makes this reaction more sustainable.
(2)

13
 *P71861A01324* Turn over
*(b) Concentrated sulfuric acid reacts with solid potassium chloride and with
solid potassium iodide.
Compare and contrast these reactions to show the difference in reducing ability
of these two halide ions.
In your answer describe what would be observed and identify the
products formed.
(6)

14
*P71861A01424* 
.. .. ... .. ... .. ... .. ... .. ... ... .. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .... .......... .. ........ .......... .......... .......... .......... .......... .......... .......... .......... .......... .......... .......... ...... .............. ..... .................

15
 *P71861A01524* Turn over
(c) Dilute sulfuric acid is used in many laboratories. It is often supplied as
concentrated sulfuric acid and then diluted.
A technician makes 500 cm3 of 1.5 mol dm−3 sulfuric acid by adding
40.5 cm3 of concentrated sulfuric acid to distilled water.
Calculate the concentration of the concentrated sulfuric acid, in mol dm−3 .
(2)

(Total for Question 21 = 20 marks)

16
*P71861A01624* 
22 This question is about the four structural isomers with the formula C4H10O which
are alcohols.
One of the isomers, 2-methylpropan-1-ol, is shown.

CH3 H

H3C C C OH

H H

(a) 2-methylpropan-1-ol is a primary alcohol.

Explain what is meant by the terms alcohol and primary.
(2)

(b) Complete the table for the other three structural isomers of C4H10O which
are alcohols.
(5)

Name butan-2-ol

H H H H
Displayed
H C C C C O H
formula
H H H H

Classification
tertiary
of alcohol

17
 *P71861A01724* Turn over
(c) 2-methylpropan-1-ol can be oxidised to 2-methylpropanoic acid, in a
two-step process.

Step 1 Step 2
(CH3)2CHCH2OH (CH3)2CHCHO (CH3)2CHCOOH

(i) Identify by name or formula the reagents needed to prepare the

oxidising mixture.
(2)

(ii) Write the equation for Step 1 using [O] to represent the oxygen from the
oxidising agent.
(1)

(iii) Infrared spectroscopy provides information on functional groups.

In an experiment, a sample of 2-methylpropan-1-ol was treated with an
oxidising agent.
Show that infrared spectroscopy can be used to show that both the alcohol
and the aldehyde are present in the resulting mixture.
In your answer refer to any relevant wavenumber ranges and bonds
responsible for the infrared spectrum.
Refer to page 7 of the Data Booklet.
(2)

(Total for Question 22 = 12 marks)

TOTAL FOR SECTION B = 40 MARKS

18
*P71861A01824* 
SECTION C
Answer ALL the questions. Write your answers in the spaces provided.
23 This question is about bicycles.
Bicycle frames have been made from steel and aluminium for many years but more
recently titanium has been used.
Titanium is a metal that is extracted from its ore, impure titanium oxide (TiO2) , in a
two-step process.
Step 1
The titanium oxide reacts with chlorine in the presence of carbon to form
titanium(IV) chloride (TiCl4) and carbon monoxide.
Step 2
The titanium(IV) chloride reacts with magnesium.

TiCl4 + 2Mg → Ti + 2MgCl2

(a) (i) Write the equation for Step 1.

State symbols are not required.
(1)

(ii) Explain why Step 2 is a redox reaction.

Refer to relevant oxidation numbers in your answer.
(2)

(b) Titanium(IV) chloride is a liquid that reacts violently with water, producing
white smoke. This reaction has been used to produce naval smoke screens to
hide ships.
Suggest the type of reaction taking place and the compound producing the
white smoke.
(2)
Type of reaction

Compound

19
 *P71861A01924* Turn over
(c) Many bicycles use an inner tube inside the tyre.
A common material used for inner tubes is the addition polymer
formed from 2-methylpropene.

H3C
C CH2
H3C

2-methylpropene

Draw a section of the polymer showing two repeat units.

(2)

(d) A reaction scheme involving 2-methylpropene is shown.

H3C
C CH2
H3C

Reaction 2 Reaction 4

Reaction 3
H3C H3C
OH Cl

CH3 CH3
Reaction 1

20
*P71861A02024* 
(i) For Reaction 1, give the name or formula of a suitable reagent, stating the
conditions for the reaction.
(2)
Reagent

Conditions

(ii) For Reaction 2, give the name or formula of a suitable reagent, stating the
type of reaction taking place.
(2)
Reagent

Type of reaction

(iii) For Reaction 3, give the name or formula of a suitable reagent, writing an
equation for the reaction taking place.
(2)
Reagent

Equation

(iv) For Reaction 4, the reagent used is potassium hydroxide (KOH).

Give the conditions required for this reaction, stating the role of the
hydroxide ions in this reaction.
(2)
Conditions

Role of hydroxide ions

21
 *P71861A02124* Turn over
(e) Many cyclists carry a small cylinder of carbon dioxide to inflate their inner tube if
it is punctured. The carbon dioxide is stored under pressure.

valve carbon dioxide cylinder

(Source: © Douglas Sacha/Getty Images)

A gas cylinder contains 16.0 g of carbon dioxide (CO2).

The cylinder has a volume of 20 cm3 .
Calculate the pressure in the cylinder at 25 °C. Include units in your answer.
Assume that all the CO2 in the cylinder is a gas.
[ pV = nRT R = 8.31 J mol−1 K−1]
(5)

(Total for Question 23 = 20 marks)

TOTAL FOR SECTION C = 20 MARKS

TOTAL FOR PAPER = 80 MARKS
22
*P71861A02224* 
BLANK PAGE

23
 *P71861A02324*
24
*P71861A02424* 
Please check the examination details below before entering your candidate information
Candidate surname Other names

Centre Number Candidate Number

January 2023
Pearson Edexcel International Advanced Level
Time 1 hour 30 minutes
Paper
reference WCH12/01
Chemistry
 

International Advanced Subsidiary/Advanced Level

UNIT 2: Energetics, Group Chemistry,
Halogenoalkanes and Alcohols
You must have: Total Marks
Scientific calculator, Data Booklet, ruler

Instructions
• Use black ink or ball-point pen.
• Fill in theis boxes
If pencil used for diagrams/sketches/graphs it must be dark (HB or B).
• centre number andat candidate
the top of this page with your name,
number.
• Answer all questions.
• – there may
Answer the questions in the spaces provided
be more space than you need.

Information
• The total mark for this paper is 80.
• – usemarks
The for each question are shown in brackets
this as a guide as to how much time to spend on each question.
• toIn the question marked with an asterisk (*), marks will be awarded for your ability
structure your answer logically, showing how the points that you make are
related or follow on from each other where appropriate.
• A Periodic Table is printed on the back cover of this paper.

Advice
• Read each question carefully before you start to answer it.
• Show all your working in calculations and include units where appropriate.
• Checkanswer
Try to every question.
• your answers if you have time at the end. Turn over

P71876A
©2023 Pearson Education Ltd.

J:1/1/1/
*P71876A0128*
SECTION A
Answer ALL the questions in this section.
You should aim to spend no more than 20 minutes on this section.
For each question, select one answer from A to D and put a cross in the box . If you change
your mind, put a line through the box and then mark your new answer with a cross .
1 A student measures the enthalpy change of combustion, ΔcH ,
of methanol, CH3OH , using the apparatus shown.

thermometer

stirrer

copper calorimeter
containing 50.0 cm3
of water

spirit burner
containing methanol

After burning 0.20 g of methanol, the temperature of the water increases by 16.0 °C .
(a) The measurement uncertainty in the thermometer used in the experiment
is 0.5 °C for each reading.
What is the percentage uncertainty in the temperature change of 16.0 °C ?
(1)
A 1.6%

B 3.1%
C 6.3%

D 12.5%

2
*P71876A0228*
(b) The student repeats the experiment but burns 0.30 g of methanol and uses
75.0 cm3 of water in the copper calorimeter.
What is the expected temperature change in this repeat experiment?
(1)
A 7.1 °C
B 10.7 °C

C 16.0 °C

D 36.0 °C

(c) The student’s calculated enthalpy change of combustion of methanol is more

exothermic than a data book value.
What is a possible reason for this?
(1)
A heat loss to the surroundings

B incomplete combustion of methanol

C evaporation of methanol from the wick of the spirit burner
D use of the molar mass of ethanol, C2H5OH , in the calculation

(Total for Question 1 = 3 marks)

2 Which equation represents the standard enthalpy change of atomisation, ΔatH ,

of bromine?

A ½Br2(l) → Br(g)

B ½Br2(g) → Br(g)
C Br2(l) → 2Br(g)

D Br2(g) → 2Br(g)

(Total for Question 2 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

3
*P71876A0328* Turn over
3 The enthalpy change of reaction, ΔrH , for the equation shown can be calculated
using bond enthalpy data.

½H2(g) + ½Cl2(g) → HCl(g)

Bond Bond enthalpy / kJ mol–1

H H 436

Cl Cl 242

H Cl 431

The expression that should be used in the calculation is

A (0.5 × 436 + 0.5 × 242) – 431

B (2 × 431) – (436 + 242)

C 431 – (0.5 × 436 + 0.5 × 242)

D (436 + 242) – (2 × 431)

(Total for Question 3 = 1 mark)

4 Which compound has London forces as the only intermolecular force?

A HF
B OF2
C PF3

D CF4

(Total for Question 4 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

4
*P71876A0428*
5 Which compound has intermolecular hydrogen bonding?

A (CH3)3N

B (CH3)3CF

C (CH3)3COH
D (CH3)3CCHO

(Total for Question 5 = 1 mark)

6 Which sequence shows the hydrogen halides in order of decreasing

boiling temperature?

A HF > HCl > HBr > HI

B HF > HI > HBr > HCl

C HI > HF > HCl > HBr

D HI > HBr > HCl > HF

(Total for Question 6 = 1 mark)

7 Which ion contains vanadium with an oxidation number of +4?

A VO2+

B VO2+
C VO3–
D VO43–

(Total for Question 7 = 1 mark)

8 What is the formula of potassium manganate(VI)?

A KMnO4

B K2MnO4

C K3MnO4

D K6Mn2O6

(Total for Question 8 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

5
*P71876A0528* Turn over
9 Compound Q produces
• a red colour in a flame test
• a white precipitate when aqueous potassium sulfate is added to a solution of
the compound.
What is compound Q?

A LiCl

B NaNO3
C Sr(NO3)2

D BaCl2

(Total for Question 9 = 1 mark)

10 Which reaction produces more than one product?

A Mg + O2 →
B Ca + Cl2 →
C Sr + H2O →
D BaO + H2O →
(Total for Question 10 = 1 mark)

11 Which equation shows a redox reaction that would not be expected to occur, based
on the trend in reactivity of the halogens?

A I2(aq) + 2At–(aq) → At2(aq) + 2I–(aq)

B 2Br–(aq) + Cl2(aq) → 2Cl–(aq) + Br2(aq)

C Cl2(aq) + 2I–(aq) → I2(aq) + 2Cl–(aq)
D 2F–(aq) + At2(aq) → 2At–(aq) + F2(aq)

(Total for Question 11 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

6
*P71876A0628*
12 A fixed amount of concentrated H2SO4 is reacted separately with an excess of four
solid potassium halides.
In which reaction would the greatest number of moles of halide be oxidised?

A 2KF(s) + H2SO4(aq) → K2SO4(aq) + 2HF(g)

B KCl(s) + H2SO4(aq) → KHSO4(aq) + HCl(g)

C 2KBr(s) + 3H2SO4(aq) → 2KHSO4(aq) + Br2(l) + SO2(g) + 2H2O(l)

D 8KI(s) + 9H2SO4(aq) → 8KHSO4(aq) + 4I2(s) + H2S(g) + 4H2O(l)

(Total for Question 12 = 1 mark)

13 Silver nitrate in aqueous ethanol is added separately to four halogenoalkanes.

Which would form a silver halide precipitate in the shortest time?

A (CH3)3CI

B (CH3)3CCl
C CH3CH2CH2CH2I
D CH3CH2CH2CH2Cl

(Total for Question 13 = 1 mark)

14 CH3CH2CHBrCH2CH2CH3 is heated with ethanolic potassium hydroxide.

How many alkene products are possible?

A one

B two
C three

D four

(Total for Question 14 = 1 mark)

15 Which compound is least likely to have a prominent peak at m / z = 43 in its

mass spectrum?

A CH3COCH2CH3
B CH3CH2NHCH3

C CH3CH(CH3)2

D CH3CH2CH2CH3

(Total for Question 15 = 1 mark)

7
*P71876A0728* Turn over
16 Which compound has peaks at 3415 cm–1 and 2250 cm–1 in its infrared spectrum?
Refer to the Data Booklet.

A H2NCH2CH2C N

B CH3CH2CH2COOH
C ClCH2CH2C CH

D HOCH2CH2CH CH2

(Total for Question 16 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

8
*P71876A0828*
17 The distribution of molecular energies for a sample of gas in a sealed container
is shown.

Number of
particles with
energy, E

Energy, E

(a) Why does the distribution of energies start at the origin, (0,0)?
(1)

A some molecules have no energy

B all molecules possess some energy
C the temperature is 0 K
D some molecules do not have enough energy to react

(b) Some of the gas is removed and then the container is resealed and the gas
is cooled.
How does the new distribution of molecular energies compare to the
original sample?
(1)

Area under the curve Position of peak

A does not change shifts to the left

B decreases shifts to the left

C does not change shifts to the right

D decreases shifts to the right

(Total for Question 17 = 2 marks)

TOTAL FOR SECTION A = 20 MARKS

9
*P71876A0928* Turn over
SECTION B
Answer ALL the questions. Write your answers in the spaces provided.
18 Calcium hypochlorite, Ca(ClO)2 , is used for water treatment in swimming pools.
It is produced in the reaction between Ca(OH)2 and Cl2 .

2Ca(OH)2(aq) + 2Cl2(g) → Ca(ClO)2(aq) + CaCl2(aq) + 2H2O(l)

(a) State the type of reaction occurring in the production of Ca(ClO)2 .

Justify your answer using oxidation numbers.
(3)

(b) Calculate the percentage atom economy by mass for the production of Ca(ClO)2
in this reaction.
(2)

10
*P71876A01028*
(c) A swimming pool has the dimensions 50 m × 25 m × 2.0 m.
The water in this swimming pool has a Ca(ClO)2 concentration of 4.2 mg dm–3 .
(i) Calculate the mass, in kg, of Ca(ClO)2 required to treat the water needed to
completely fill this swimming pool.
(3)

(ii) Calculate the volume of Cl2 , at room temperature and pressure, needed to
make the mass of Ca(ClO)2 calculated in (c)(i).
(3)

(Total for Question 18 = 11 marks)

11
*P71876A01128* Turn over
19 This question is about alcohols with the molecular formula C6H14O.
(a) Draw the skeletal formula of each of the three tertiary alcohols with the
formula C6H14O.
(3)

tertiary alcohol 1

tertiary alcohol 2

tertiary alcohol 3

12
*P71876A01228*
(b) Two primary C6H14O alcohols, A and B, are shown.

OH
OH

alcohol A alcohol B

(i) Give the IUPAC name of alcohol A.

(1)

(ii) Explain why alcohol B has a higher boiling temperature than alcohol A.
(2)

(iii) Explain why alcohol B is completely soluble in ethanol but only slightly
soluble in water.
A detailed description of the forces involved is not required.
(3)

13
*P71876A01328* Turn over
(c) Give the structure of the organic product of each reaction shown.
(3)
Reaction 1

K2Cr2O7 , H2SO4
OH
heat under reflux

Reaction 2

K2Cr2O7 , H2SO4

OH heat under reflux

Reaction 3

red phosphorus and iodine

heat under reflux

(Total for Question 19 = 12 marks)

14
*P71876A01428*
20 This question is about the synthesis of propylamine, CH3CH2CH2NH2 .
Three routes for the synthesis of CH3CH2CH2NH2 are shown.

Step X KCN
CH2 CH2 CH3CH2Cl organic compound W

H2(g) , Pt catalyst

CH3CH2CH2NH2

Step Z
H2(g) , Pt catalyst

Step Y
CH3CH2CH2Br CH3CH2CH2N3

(a) Identify, by name or formula, the reagent used in Step X.

(1)

(b) Give the structure of organic compound W.

(1)

15
*P71876A01528* Turn over
(c) The reagent used in Step Y is potassium azide, KN3 .
This is a source of the azide ion, N–3 , which acts as a nucleophile.
(i) Complete a possible dot-and-cross diagram for N–3 .
Show outer electrons only.
(2)

⎡ ⎤ ⎡ ⎤–
⎢ ⎥ ⎢ ⎥
⎢
⎢
⎢
⎥
⎥
⎥
N N N ⎢
⎢
⎢
⎥
⎥
⎥
⎣ ⎦ ⎣ ⎦

(ii) Complete the mechanism for Step Y.

Include curly arrows, and any relevant lone pairs and dipoles.
(3)

CH3CH2 C Br

H
N3–

16
*P71876A01628*
(d) Step Z is carried out by reacting ammonia with 1-bromopropane.
(i) Give the conditions for this reaction.
(2)

(ii) Suggest why the yield of CH3CH2CH2NH2 obtained using Step Z is low.
(1)

(Total for Question 20 = 10 marks)

17
 *P71876A01728* Turn over
*21 Discuss some aspects of the thermal stability of the anhydrous nitrates of the
elements in Groups 1 and 2 of the Periodic Table.
In your answer you should
• explain the trend in thermal stability of the Group 2 nitrates
• describe any differences in the products of thermal decomposition of the
Group 1 nitrates
• give equations for the thermal decomposition of sodium nitrate and of
magnesium nitrate.
(6)

18
*P71876A01828* 
.. .. ... .. ... .. ... .. ... .. ... ... .. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .... .......... .. ........ .......... .......... .......... .......... .......... .......... .......... .......... .......... .......... .......... ...... .............. ..... .................

(Total for Question 21 = 6 marks)

TOTAL FOR SECTION B = 39 MARKS

19
 *P71876A01928* Turn over
SECTION C
Answer ALL the questions. Write your answers in the spaces provided.
22 Ammonium nitrate, NH4NO3 , is used in the manufacture of fertilisers and explosives.
It is produced on a large scale using only methane, water and air.
The process has four stages.
(a) The first two reactions in Stage 1 involve the production of hydrogen.
At temperature T1 , methane reacts with excess steam to give hydrogen.

CH4(g) + H2O(g)  3H2(g) + CO(g) ΔH = +206 kJ mol–1

At a different temperature, T2 , the carbon monoxide reacts with more steam.

CO(g) + H2O(g)  H2(g) + CO2(g) ΔH = –42 kJ mol–1

(i) Give the reason why excess steam is used in the first reaction.
(1)

(ii) Predict which of T1 and T2 is the higher temperature.

Justify your answer.
(1)

(iii) Derive the overall equation for the production of H2 in Stage 1.

State symbols are not required.
(1)

20
*P71876A02028* 
(b) The third reaction in Stage 1 involves the removal of carbon dioxide, using an
aqueous solution of N-methyldiethanolamine, CH3N(CH2CH2OH)2 .

CO2(g) + H2O(l) + 2CH3N(CH2CH2OH)2(aq)  (CH3NH(CH2CH2OH)2)2CO3(aq)

(i) Suggest one reason why CO2 is removed.

(1)

(ii) Name the type of reaction occurring.

(1)

(iii) Draw the displayed formula of N-methyldiethanolamine, CH3N(CH2CH2OH)2 .

(1)

(c) In Stage 2, the hydrogen from Stage 1 reacts with nitrogen (from the air) to
produce ammonia. The conditions for this reaction are:
• a temperature of 700 K
• a pressure in the range 100–200 atm
• an iron catalyst

N2(g) + 3H2(g)  2NH3(g) ΔH = –92 kJ mol–1

Give one advantage and one disadvantage of using a pressure of 200 atm,
compared to a pressure of 100 atm, in Stage 2.
(2)

21
 *P71876A02128* Turn over
(d) The reaction in Stage 2 has an activation energy, Ecat = +70 kJ mol–1 .
The uncatalysed reaction between N2 and H2 has an activation energy,
Ea = +290 kJ mol–1 .
(i) Complete the profile for the catalysed and uncatalysed reactions.
Label the activation energies and the enthalpy change of reaction, ΔH.
Your diagram must match the scale shown for the production of NH3.
(3)

H / kJ mol–1

N2(g) + 3H2(g)

2NH3(g)

Reaction progress

(ii) Suggest why the use of the catalyst makes Stage 2 more sustainable.
(1)

22
*P71876A02228* 
(e) In Stage 3, nitrogen monoxide, NO, is produced in the reaction between
NH3 (from Stage 2) and O2 (from the air). The conditions used are a temperature of
1100 K in the presence of a platinum-rhodium catalyst.

4NH3(g) + 5O2(g)  4NO(g) + 6H2O(g) ΔH = –905 kJ mol–1

(i) Give one reason why a high temperature is needed in this reaction.
(1)

(ii) Suggest why only a small amount of energy is used to maintain the
temperature at 1100 K.
(1)

(f ) The NO from the first reaction in Stage 3 is cooled and then converted to
nitrogen dioxide, NO2 , by reaction with more O2 .

2NO(g) + O2(g)  2NO2(g)

Nitric acid, HNO3(aq), is produced by the addition of water.

3NO2(g) + H2O(l) → 2HNO3(aq) + NO(g)

Explain how adding water in the second reaction affects the yield of NO2 in the
first reaction.
(2)

23
 *P71876A02328* Turn over
(g) In Stage 4, a solution of NH4NO3 is produced by reacting NH3 (from Stage 2) with
HNO3 (from Stage 3).

NH3(g) + HNO3(aq) → NH4NO3(aq)

Data

Species NH3(g) HNO3(l) NH4NO3(s)

Δf H / kJ mol–1 –46.1 –174.1 –365.6

Equation ΔH / kJ mol–1
HNO3(l) + aq → HNO3(aq) –32.6
NH4NO3(s) + aq → NH4NO3(aq) +25.6

(i) Complete the enthalpy cycle.

(2)
Enthalpy cycle

Δr H
NH3(g) + HNO3(aq) NH4NO3(aq)

–32.6 kJ mol–1
.... .......... .......... ....... kJ mol–1

NH4NO3(s)

–220.2 kJ mol–1 .... .......... .......... ....... kJ mol–1

N2(g) + 2H2(g) + 1½O2(g)

(ii) Calculate the enthalpy change, Δr H , in kJ mol–1 , for the reaction of NH3(g)
with HNO3(aq).
(1)

24
*P71876A02428* 
(h) Suggest two reasons why it is more profitable to carry out all four stages
at the same site, instead of using different sites for each stage in the
industrial production of ammonium nitrate.
(2)

(Total for Question 22 = 21 marks)

TOTAL FOR SECTION C = 21 MARKS

TOTAL FOR PAPER = 80 MARKS

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*P71876A02628* 
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27
 *P71876A02728*
28
*P71876A02828* 
Please check the examination details below before entering your candidate information
Candidate surname Other names

Centre Number Candidate Number

Pearson Edexcel International Advanced Level

Monday 15 May 2023
Morning (Time: 1 hour 30 minutes) Paper
reference WCH12/01
Chemistry
 

International Advanced Subsidiary/Advanced Level

UNIT 2: Energetics, Group Chemistry,
Halogenoalkanes and Alcohols
You must have: Total Marks
Scientific calculator, Data Booklet, ruler

Instructions
• Use black ink or ball-point pen.
• IfFillpencil is used for diagrams/sketches/graphs it must be dark (HB or B).
• centrein the boxes at the top of this page with your name,
number and candidate number.
• Answer all questions.
• Answer the questions in the spaces provided
– there may be more space than you need.

Information
• The total mark for this paper is 80.
• – usemarks
The for each question are shown in brackets
this as a guide as to how much time to spend on each question.
• Into the question marked with an asterisk (*), marks will be awarded for your ability
structure your answer logically, showing how the points that you make are
related or follow on from each other where appropriate.
• A Periodic Table is printed on the back cover of this paper.

Advice
• Read each question carefully before you start to answer it.
• Show all your working in calculations and include units where appropriate.
• Try to answer every question.
• Check your answers if you have time at the end. Turn over

P71940A
©2023 Pearson Education Ltd.

N:1/1/1/1/1/
*P71940A0128*
SECTION A
Answer ALL the questions in this section.
You should aim to spend no more than 20 minutes on this section.
For each question, select one answer from A to D and put a cross in the box . If you change
your mind, put a line through the box and then mark your new answer with a cross .
1 The enthalpy level diagram for a reaction is shown.

reactants

Enthalpy ∆H

products

Progress of reaction

Which is represented by this diagram?

A Na(s) → Na(g)
B Na(g) → Na+(g) + e–

C 2Cl(g) → Cl2(g)
D NH4NO3(s) + aq → NH+4 (aq) + NO3–(aq)

(Total for Question 1 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

2
*P71940A0228*
2 Excess zinc powder is added to 50.00 g of 0.500 mol dm–3 copper(II) sulfate solution in
a polystyrene cup.
The mixture is stirred and the maximum temperature change determined.
The enthalpy change for the reaction is calculated to be –185 kJ mol–1.
The data book value for this reaction is –217 kJ mol–1.
(a) The percentage error in this experiment is
(1)
A ±7.37 %

B ±8.65 %
C 14.7 %

D 17.3 %

(b) In the calculation, the specific heat capacity of the liquid is taken to be
4.18 J g–1 °C–1 rather than the true value of 3.85 J g–1 °C–1.
The use of 4.18 J g–1 °C–1 in the calculation
(1)
A is partly responsible for the error in the final value obtained

B lowers the error in the final value obtained

C has a negligible effect on the final value obtained

D has a negligible effect compared with the measurement uncertainties

(Total for Question 2 = 2 marks)

3 The enthalpy changes for two reactions are shown.

2Fe(s) + 1½O2(g) → Fe2O3(s) ΔrH = –824 kJ mol–1

C(s) + ½O2(g) → CO(g) ΔrH = –111 kJ mol–1

What is the enthalpy change for the reaction between iron(III) oxide and carbon?

Fe2O3(s) + 3C(s) → 2Fe(s) + 3CO(g)

A +491 kJ mol–1

B +713 kJ mol–1

C –491 kJ mol–1
D –713 kJ mol–1

(Total for Question 3 = 1 mark)

3
*P71940A0328* Turn over
4 Which of these alkanes would be expected to have the highest boiling temperature?

(Total for Question 4 = 1 mark)

5 The boiling temperature of hexane is 69 °C and that of cyclohexane is 81 °C.

The main reason that cyclohexane has a higher boiling temperature is that
cyclohexane molecules

A have more electrons

B have strong permanent dipole-permanent dipole forces

C have a larger surface area of contact

D form hydrogen bonds

(Total for Question 5 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

4
*P71940A0428*
6 The structures and boiling temperatures of butane and propanal are shown.

Butane Propanal

CH2 O
CH2 CH3 CH3 C
CH3 CH2
H

Tb = 0 °C Tb = 49 °C

The main reason that propanal has a higher boiling temperature is that
propanal molecules

A have more electrons

B have strong permanent dipole-permanent dipole forces

C have a larger surface area of contact

D form hydrogen bonds

(Total for Question 6 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

5
*P71940A0528* Turn over
7 Hydrogen bonds are formed when methanol dissolves in water.
Which structure best represents a hydrogen bond between methanol and water?

H H

A H C O: H O
H
H

H H
O
B H C O: H H

H H H

C O: H C O
H H

H H

D H O: H C O
H
H

(Total for Question 7 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

6
*P71940A0628*
8 In which pair of compounds is the stated element in the same oxidation state?

A chlorine in Cl2O7 and Ca(ClO3)2

B chromium in K2Cr2O7 and K2CrO4

C manganese in K2MnO4 and Mn2O7

D oxygen in K2O and K2O2

(Total for Question 8 = 1 mark)

9 What is the formula of barium(II) ferrate(VI)?

A Ba2FeO3

B BaFeO3

C Ba2FeO4
D BaFeO4

(Total for Question 9 = 1 mark)

10 When lithium reacts with excess oxygen, only lithium oxide is formed.
When sodium reacts with excess oxygen, sodium oxide and sodium peroxide are
both formed.
What is the main reason why sodium peroxide is formed?

A sodium is more reactive than lithium

B sodium has a lower first ionisation energy than lithium

C the sodium ion has a larger ionic radius than the lithium ion

D the sodium ion has a higher charge density than the lithium ion

(Total for Question 10 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

7
*P71940A0728* Turn over
11 A piece of sodium weighing 1.15 g reacts completely with distilled water and the
solution formed is made up to 250.0 cm3.

2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g)

What is the concentration of the sodium hydroxide solution?

A 0.025 mol dm–3

B 0.050 mol dm–3

C 0.100 mol dm–3

D 0.200 mol dm–3

(Total for Question 11 = 1 mark)

12 Magnesium nitrate decomposes on heating.

2Mg(NO3)2(s) → 2MgO(s) + 4NO2(g) + O2(g)

A sample of magnesium nitrate decomposed completely.

The total volume of gas formed was 1200 cm3, measured at
room temperature and pressure (r.t.p.).
What mass of magnesium nitrate was used?
[Mr Mg(NO3)2 = 148.3 Molar volume of gas at r.t.p. = 24 000 cm3 mol–1]

A 1.48 g

B 2.97 g

C 7.42 g

D 14.8 g

(Total for Question 12 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

8
*P71940A0828*
13 When solid sodium chloride is placed in a Bunsen flame, a persistent yellow colour
is observed.
The yellow colour is due to

A electrons being excited to higher energy levels and

emitting yellow light on returning to the ground state
B electrons being excited to higher energy levels and
emitting blue-violet light on returning to the ground state
C electrons being excited to higher energy levels and
absorbing yellow light
D electrons being excited to higher energy levels and
absorbing blue-violet light

(Total for Question 13 = 1 mark)

14 In a series of experiments, the time taken to complete the reaction between

iron(III) sulfate and sodium thiosulfate in aqueous solution is measured.
One drop of a solution of a substance is added to separate reaction mixtures.
The results are shown.

Substance added Reaction time / s

(no substance) 205

copper(II) sulfate 75

lead(II) nitrate 464

sodium nitrate 204

zinc sulfate 202

Which ion speeds up the reaction?

A copper(II)

B lead(II)

C nitrate

D sulfate

(Total for Question 14 = 1 mark)

9
*P71940A0928* Turn over
15 Hydrogen peroxide decomposes in the presence of a catalyst.

2H2O2(aq) → 2H2O(l) + O2(g)

The volume of gas formed is measured at regular time intervals and the data plotted
on a graph.

15
Volume X
of gas
/ cm3
10

0
0 2 4 6 8 10

Time / min

What is the rate of formation of oxygen at point X?

A 1.3 cm3 min–1

B 2.5 cm3 min–1

C 4.4 cm3 min–1

D 25 cm3 min–1

(Total for Question 15 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

10
*P71940A01028*
16 The structures of three bromoalkanes P, Q and R are shown.

Br Br Br

P Q R

Which of these bromoalkanes may be classified as tertiary?

A P only

B Q only

C R only
D Q and R only

(Total for Question 16 = 1 mark)

17 When 1-chlorobutane is mixed with ethanol and aqueous silver nitrate,

a reaction occurs.
Which species is the nucleophile in this reaction?

A ethanol
B nitrate ions
C silver ions

D water

(Total for Question 17 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

11
*P71940A01128* Turn over
18 Propan-1-ol may be converted into propene.

CH3CH2CH2OH → CH3CH CH2 + H2O

(a) Which reagent is used for this reaction?

(1)

A 50 % sulfuric acid

B ethanolic potassium hydroxide

C phosphoric(V) acid
D red phosphorus

(b) The reaction is best classified as

(1)
A elimination
B hydrolysis
C reduction
D substitution

(Total for Question 18 = 2 marks)

TOTAL FOR SECTION A = 20 MARKS

12
*P71940A01228*
SECTION B
Answer ALL the questions. Write your answers in the spaces provided.
19 Some reactions of a halogenoalkane are summarised in the diagram.
All the reactions are of the same type and mechanism.

CH3

H3C C NH2

CH3
Reaction 1

CH3 CH3
Reaction 2
H3C C Br H3C C OH

CH3 CH3

KCN in ethanol
compound M

(a) Name the type and mechanism of these reactions.

(1)

(b) Give the IUPAC name and the structure of compound M.

(2)

(c) State the reagent and conditions required for Reaction 1.

(2)

13
*P71940A01328* Turn over
(d) An incomplete mechanism for Reaction 2 is shown.

CH3 CH3 CH3

H3C C Br H3C C+ + Br– H3C C OH + Br–

CH3 CH3 CH3

–
OH

intermediate J

(i) Complete the mechanism by adding curly arrows, and relevant dipoles and
lone pairs.
(2)
(ii) Describe how intermediate J is formed in the first step, naming the process
that occurs.
(2)

(iii) State the shape of intermediate J. Justify your answer.

(2)

14
*P71940A01428*
(iv) The product of Reaction 2 is shown.

CH3

H3C C OH

CH3

This compound has three isomers that are also alcohols.

Draw the structures of these isomers.
(2)

isomer 1 isomer 2 isomer 3

(e) The reaction of halogenoalkanes with hydroxide ions is often carried out using
sodium hydroxide or potassium hydroxide.
An alternative is ‘moist silver(I) oxide’, which is prepared by adding a few drops of
water to solid silver(I) oxide.
Silver(I) oxide is insoluble in water but produces sufficient hydroxide ions for
the reaction.
(i) Write the ionic equation for the reaction of silver(I) oxide with water.
State symbols are not required.
(2)

(ii) Suggest one advantage of using silver(I) oxide rather than sodium hydroxide
or potassium hydroxide.
(1)

(Total for Question 19 = 16 marks)

15
*P71940A01528* Turn over
20 This question is about fuels.
The enthalpy change of combustion is the maximum amount of heat energy that can
be obtained by the complete combustion of a substance.
Values for the enthalpy change of combustion may be obtained by direct
measurement or from mean bond enthalpies. These data may be used to assess the
efficiency of fuels.
Petrol is a mixture of a large number of different hydrocarbons containing between
four and twelve carbon atoms. Octane, C8H18 , is a typical component of petrol.
(a) The equation for the combustion of octane is shown.

H H H H
H H H H
O
H C C C C H + 12½ O O 8O C O + 9H H
C C C C
H H H H
H H H H

(i) Use mean bond enthalpies to calculate a value for the enthalpy change of
combustion of octane.
(4)

Bond C C C H O H O O C O
Mean bond enthalpy
347 413 464 498 805
/ kJ mol–1

16
*P71940A01628*
(ii) The standard enthalpy change of combustion, ΔcH , of octane is –5470 kJ mol–1.
Give two reasons why this value, measured under standard conditions, is
different from the value obtained using bond enthalpy data.
(2)

(iii) When petrol is used to power a car, the energy available is less than the
theoretical maximum.
When one kilogram of petrol powers a car, the energy used to move the car
is 11 MJ.
Calculate the percentage of the maximum energy that is available to move a
car, assuming that this fuel is pure octane.
Use ΔcH = –5470 kJ mol–1.
(2)

(iv) Give two reasons why the energy used to move the car is less than the
theoretical maximum.
(2)

17
 *P71940A01728* Turn over
*(b) Two alternatives to hydrocarbon fuels are hydrogen and ammonia.
Hydrogen burns to form water as the only product but hydrogen is extremely
hard to liquefy. Ammonia is easily liquefied but it is toxic.
Compare and contrast the intermolecular forces involved when hydrogen and
ammonia liquefy, by describing how these forces are formed.
(6)

18
*P71940A01828* 
.. .. ... .. ... .. ... .. ... .. ... ... .. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .... .......... .. ........ .......... .......... .......... .......... .......... .......... .......... .......... .......... .......... .......... ...... .............. ..... .................

(Total for Question 20 = 16 marks)

19
 *P71940A01928* Turn over
21 Methanal is used in the production of many materials and chemical compounds.
It is manufactured from methanol by reaction with oxygen at 300–400 °C using an
iron-molybdenum oxide catalyst.

CH3OH(g) + ½O2(g) → HCHO(g) + H2O(g)

(a) The Maxwell–Boltzmann distribution for the reaction mixture at 300 °C is shown.

Fraction of
collisions with
energy E

Energy, E

(i) On the diagram, sketch the Maxwell–Boltzmann distribution for this reaction
mixture at a higher temperature.
(1)
(ii) Using the Maxwell–Boltzmann distributions, explain why increasing the
temperature and adding a catalyst both increase the rate of reaction.
(2)

20
*P71940A02028* 
(b) An alternative method for producing methanal uses a silver catalyst at a
temperature of 650 °C. The reaction is shown.

CH3OH(g) → HCHO(g) + H2(g)

Suggest one advantage and one disadvantage of this method, other than the
cost of the silver catalyst.
(2)
Advantage

Disadvantage

(c) Explain how the infrared spectra of methanol and methanal can be used to
distinguish between the two compounds, stating the relevant bond stretching
vibrations and their wavenumber ranges.
(2)

(Total for Question 21 = 7 marks)

TOTAL FOR SECTION B = 39 MARKS

21
 *P71940A02128* Turn over
SECTION C
Answer ALL the questions. Write your answers in the spaces provided.
22 Toilet Cleaners
Products used to clean toilets work in two ways: removing the limescale that collects
in the toilet bowl and disinfecting the bowl.
Limescale contains calcium carbonate which is removed by reaction with acids.
The strongest acid used in toilet cleaners is hydrochloric acid, although weaker acids
such as methanoic acid are also used.
Disinfectants are essentially chlorine dissolved in aqueous sodium hydroxide.
The effective disinfectant in these solutions is the chlorate(I) ion, ClO–.
(a) State one safety precaution that you should take when using a toilet cleaner
containing hydrochloric acid.
(1)

(b) The equation for the reaction of calcium carbonate with hydrochloric acid
is shown.

CaCO3(s) + 2HCl(aq) → CaCl2(aq) + H2O(l) + CO2(g)

(i) Write the ionic equation for this reaction.

State symbols are not required.
(1)

22
*P71940A02228* 
(ii) A 750 cm3 bottle of a toilet cleaner contains 85.0 g of hydrochloric acid.
Calculate the maximum mass of calcium carbonate limescale that could be
removed by 50.0 cm3 of this toilet cleaner.
(4)

(c) Chlorine gas reacts with water.

Cl2(g) + H2O(l)  HClO(aq) + HCl(aq)

(i) State the classification of this reaction. Justify your answer in terms of the
relevant oxidation numbers.
(3)

23
 *P71940A02328* Turn over
(ii) When 5.00 cm3 of a disinfectant reacts with excess hydrogen peroxide, 113 cm3
of oxygen is produced, measured at room temperature and pressure.

H2O2(aq) + NaClO(aq) → H2O(l) + NaCl(aq) + O2(g)

Calculate the concentration, in g dm–3, of sodium chlorate(I) in the disinfectant.

Give your answer to two significant figures.
(4)
[Molar volume of gas at r.t.p. = 24 000 cm3 mol–1]

(iii) Commercial disinfectants are often made more viscous by adding

propane-1,2,3-triol to the aqueous solution.
Suggest how propane-1,2,3-triol makes disinfectants more viscous.
(2)

24
*P71940A02428* 
(d) Toilet cleaners that remove limescale should not be mixed with
chlorine-based disinfectants.
Explain, using the relevant equation, why these two types of toilet cleaner should
not be mixed.
(2)

(e) Borax is another cleaning agent used to remove limescale.

Borax is a compound of sodium, boron and oxygen.
Borax crystals contain water of crystallisation.
The percentage composition by mass of some borax crystals is
H = 5.2 % B = 11.3 % O = 71.4 % Na = 12.1 %
Determine the empirical formula of the borax crystals and hence their formula.
(4)

(Total for Question 22 = 21 marks)

TOTAL FOR SECTION C = 21 MARKS

TOTAL FOR PAPER = 80 MARKS

25
 *P71940A02528*
BLANK PAGE

26
*P71940A02628* 
BLANK PAGE

27
 *P71940A02728*
28
*P71940A02828* 
Please check the examination details below before entering your candidate information
Candidate surname Other names

Centre Number Candidate Number

Pearson Edexcel International Advanced Level

Friday 13 October 2023
Morning (Time: 1 hour 30 minutes) Paper
reference WCH12/01
Chemistry  

International Advanced Subsidiary/Advanced Level

UNIT 2: Energetics, Group Chemistry,
Halogenoalkanes and Alcohols

You must have: Total Marks

Data Booklet, scientific calculator, ruler

Instructions
•• Use black ink or ball-point pen.
If pencil is used for diagrams/sketches/graphs it must be dark (HB or B).
• Fill in the boxes at the top of this page with your name,
centre number and candidate number.
•• Answer all questions.
Answer the questions in the spaces provided
– there may be more space than you need.

Information
•• The total mark for this paper is 80.
The marks for each question are shown in brackets
– use this as a guide as to how much time to spend on each question.
• toIn the question marked with an asterisk (*), marks will be awarded for your ability
structure your answer logically, showing how the points that you make are
related or follow on from each other where appropriate.
• A Periodic Table is printed on the back cover of this paper.
Advice
•• Read each question carefully before you start to answer it.
Show all your working in calculations and include units where appropriate.
•• Try to answer every question.
Check your answers if you have time at the end. Turn over

P75069A
©2023 Pearson Education Ltd.
Z:1/1/1/1/1/
*P75069A0124*
SECTION A
Answer ALL the questions in this section.

DO NOT WRITE IN THIS AREA

You should aim to spend no more than 20 minutes on this section.
For each question, select one answer from A to D and put a cross in the box . If you change
your mind about an answer, put a line through the box and then mark your new answer with
a cross .
1 The mean C–F bond enthalpy is +485 kJ mol–1.
Which process has an enthalpy change of +1940 kJ mol–1?

A C(g) + 4F(g) → CF4(g)

B C(s) + 2F2(g) → CF4(g)

C CF4(g) → C(g) + 4F(g)

D CF4(g) → C(s) + 2F2(g)
(Total for Question 1 = 1 mark)

DO NOT WRITE IN THIS AREA

2 Which expression gives the standard enthalpy change, in kJ mol–1, for the
reaction shown?

BaCO3(s) → BaO(s) + CO2(g)

Δf H d values: BaCO3(s) = –1216 kJ mol–1

BaO(s) = –554 kJ mol–1

CO2(g) = –394 kJ mol–1

A –554 – 394 + 1216

B –554 – 394 – 1216

C 554 + 394 + 1216 DO NOT WRITE IN THIS AREA

D 554 + 394 – 1216

(Total for Question 2 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

2
*P75069A0224* 
3 The standard enthalpy changes of combustion for a series of alkanes are shown.
DO NOT WRITE IN THIS AREA

Alkane formula Δc H d / kJ mol–1

C2H6(g) –1560

C3H8(g) –2219

C4H10(l) –2877

C5H12(l) –3509

Another alkane has an enthalpy change of combustion of –6125 kJ mol–1.

Which is the most likely formula for this alkane?

A C6H14
B C7H16
DO NOT WRITE IN THIS AREA

C C8H18
D C9H20
(Total for Question 3 = 1 mark)

4 Which row in the table shows the forces between the molecules in the liquid state?

Permanent dipole-dipole
Molecule London forces Hydrogen bonding
interaction
A BF3   
B CH4   
C NH3   
D H2S   
DO NOT WRITE IN THIS AREA

(Total for Question 4 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

3
 *P75069A0324* Turn over
5 Which of these isoelectronic compounds would be expected to have the
highest boiling temperature?

DO NOT WRITE IN THIS AREA

A butan-1-ol

B 2-methylpropan-1-ol
C 2-methylpropan-2-ol

D pentane
(Total for Question 5 = 1 mark)

6 What is the value of n in the half-equation shown?

O2(g) + 2H2O(l) + ne– → nOH–(aq)

A 2
B 3

C 4

DO NOT WRITE IN THIS AREA

D 5
(Total for Question 6 = 1 mark)

7 Which equation shows a disproportionation reaction?

A Cu + 4HNO3 → Cu(NO3)2 + 2H2O + 2NO2

B I2 + 5O3 + H2O → 2HIO3 + 5O2
C 2MnO4– + MnO2 + 4OH– → 3MnO42– + 2H2O

D S2O32– + 2H+ → SO2 + S + H2O

(Total for Question 7 = 1 mark)

8 When sodium bromide reacts with concentrated sulfuric acid,

DO NOT WRITE IN THIS AREA

sodium hydrogensulfate is always formed.

What other product(s) are formed in this reaction?

A hydrogen bromide only

B bromine and hydrogen bromide only

C bromine, hydrogen bromide and sulfur dioxide only

D bromine, hydrogen bromide, sulfur dioxide and sulfur only
(Total for Question 8 = 1 mark)

4
*P75069A0424* 
9 Which property decreases as Group 2 is descended?

A atomic radius
DO NOT WRITE IN THIS AREA

B reactivity of the elements

C solubility of the sulfates

D thermal stability of the nitrates
(Total for Question 9 = 1 mark)

10 In a neutralisation reaction, 20.0 cm3 of 0.500 mol dm–3 nitric acid reacts with 10.0 cm3
of 1.00 mol dm–3 aqueous sodium hydroxide.

HNO3(aq) + NaOH(aq) → NaNO3(aq) + H2O(l)

What is the concentration, in mol dm–3, of the sodium nitrate solution produced?

A 0.33

B 0.50
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C 0.67
D 1.0
(Total for Question 10 = 1 mark)

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11 The equation for the reaction of sulfur dioxide with oxygen is shown.

2SO2(g) + O2(g)  2SO3(g) ΔrH = –192 kJ mol–1

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(a) What is the effect of a decrease in temperature?
(1)
A rate increases and yield decreases

B rate increases and yield increases

C rate decreases and yield decreases

D rate decreases and yield increases

(b) What is the effect of an increase in pressure?

(1)
A rate increases and yield decreases
B rate increases and yield increases

C rate decreases and yield decreases

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D rate decreases and yield increases
(Total for Question 11 = 2 marks)

12 A mixture of 1.0 cm3 of 0.20 mol dm–3 potassium chromate(VI) and

5.0 cm3 of 1.0 mol dm–3 sulfuric acid forms the equilibrium shown.

2CrO42–(aq) + 2H+(aq)  Cr2O72–(aq) + H2O(l)

yellow orange

What would be the effect, if any, on the colour of the solution if

5.0 cm3 of 1.0 mol dm–3 sodium hydroxide were added?

A no visible change
B the mixture becomes colourless
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C the mixture becomes more yellow

D the mixture becomes more orange

(Total for Question 12 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

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13 Tertiary alcohols are used in the manufacture of petrol additives.
(a) Which of these is a tertiary alcohol?
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(1)
A 1-methylcyclopentanol
B 2-methylcyclopentanol

C 2-methylbutan-1-ol

D 3-methylpentan-2-ol

(b) Which reagent reacts with tertiary alcohols?

(1)
A acidified aqueous potassium dichromate(VI)

B bromine water
C phosphorus(V) chloride

D sodium carbonate solution

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(Total for Question 13 = 2 marks)

14 Infrared spectra may be used to identify organic compounds.

(a) When propan-2-ol is refluxed with excess acidified potassium dichromate(VI),
the product will show a peak due to
(1)
A O H stretching at 3750 – 3200 cm–1
B C O stretching at 1740 – 1720 cm–1

C C O stretching at 1725 – 1700 cm–1

D C O stretching at 1720 – 1700 cm–1

(b) When propan-1-ol is heated with acidified potassium dichromate(VI),

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the product that is distilled off as it is formed will show a peak due to
(1)
A O H stretching at 3750 – 3200 cm–1

B C O stretching at 1740 – 1720 cm–1

C C O stretching at 1725 – 1700 cm–1

D C O stretching at 1720 – 1700 cm–1

(Total for Question 14 = 2 marks)

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15 Separate solutions of 1-chloropropane and 1-bromopropane in ethanol are warmed
with aqueous silver nitrate.

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Why does the formation of a precipitate take longer with 1-chloropropane?

A 1-chloropropane is less soluble than 1-bromopropane

B the C Cl bond is stronger than the C Br bond

C the C Cl bond is more polar than the C Br bond

D silver chloride is more soluble than silver bromide

(Total for Question 15 = 1 mark)

16 A sample of propane-1,2-diol with a mass of 1.52 g reacts completely with

excess phosphorus(V) chloride.
What is the maximum mass, in grams, of the organic product?
[Ar values: H = 1.0 C = 12.0 O = 16.0 Cl = 35.5]

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A 1.13
B 1.89

C 2.26
D 4.52
(Total for Question 16 = 1 mark)

17 Which compound reacts with ammonia to form CH3CH(NH2)CH3?

A 1-chloropropane

B 2-chloropropane
C propane
D propene
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(Total for Question 17 = 1 mark)

TOTAL FOR SECTION A = 20 MARKS

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SECTION B
Answer ALL the questions. Write your answers in the spaces provided.

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18 This question is about sodium hydroxide.
(a) (i) Write an ionic equation for the neutralisation reaction between
aqueous sodium hydroxide and hydrochloric acid.
State symbols are not required.
(1)

(ii) State what is meant by standard enthalpy change of neutralisation, Δneut H d .

(2)

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(b) A student carried out an investigation to determine the enthalpy change of

neutralisation of aqueous sodium hydroxide by hydrochloric acid.
Method
• separate 25.0 cm3 samples of 0.80 mol dm–3 sodium hydroxide and
0.80 mol dm–3 hydrochloric acid were left to reach room temperature
• after two minutes, the solutions were mixed in a copper calorimeter and the
temperature was noted at 30 s intervals.
(i) Use the graph shown to determine the maximum temperature change, ΔT, in
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this experiment. You must show your working on the graph.

(2)

ΔT ... .......... .......... ... . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

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Temperature
/ °C

24
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20
0 60 120 180 240 300 360
Time / s

(ii) Calculate the enthalpy change of neutralisation using your answers to

(a) and (b)(i). Give a sign and units with your answer.
Assume: no energy is used to heat the container.
the specific heat capacity of the solution = 4.2 J °C–1 g–1.
the densities of the solutions of NaOH and HCl are 1.0 g cm–3.
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(3)

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(iii) Explain how, if at all, the enthalpy change of neutralisation obtained in
(b)(ii) would differ if the heat capacity of the calorimeter was included
in the calculation.

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(2)

(c) Aqueous sodium hydroxide reacts with 1-bromopropane to produce propan-1-ol.

(i) State the type and mechanism of this reaction.

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(1)

(ii) Complete the mechanism for this reaction.

Include curly arrows, and relevant lone pairs and dipoles.
(3)

H H H

H C C C Br

H H H
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(iii) Under different conditions, sodium hydroxide reacts with 1-bromopropane to
form propene.
Name the type of reaction and a suitable solvent.
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(2)
Type of reaction

Suitable solvent

(Total for Question 18 = 16 marks)

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19 This question is about some of the elements in Group 7 of the Periodic Table.
(a) Mixtures of halide salts are found in brine solutions extracted from oil and

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gas wells.
Iodine, which is used as a dietary supplement, may be obtained from
these mixtures.
A brine solution containing 2.49 g of a mixture of potassium iodide and
potassium chloride was analysed.
Procedure
Step 1 Excess aqueous silver nitrate solution was added to the solution to
completely precipitate the halide ions.
Step 2 Excess aqueous ammonia was added to the mixture.
Step 3 The mixture was filtered, and the solid was washed, dried and weighed.
The mass of the dried solid was 0.162 g.
(i) State the colour of the solid in Step 3.
(1)

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(ii) Calculate the percentage by mass of potassium iodide in the mixture.

Give your answer to an appropriate number of significant figures.
[Ar values: Ag = 107.9 K = 39.1 I = 126.9]
(3)

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(b) Chlorine gas may be prepared by heating concentrated hydrochloric acid with
solid manganese(IV) oxide.
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MnO2(s) + 4HCl(aq) → MnCl2(aq) + Cl2(g) + 2H2O(l)

Show, by reference to oxidation numbers, that this is a redox reaction.

(2)

(c) Iodine may be obtained by bubbling chlorine gas through aqueous

potassium iodide.
When the reaction is complete, hexane is added and the mixture shaken.
Two layers are formed.
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State the colour of each layer.

(2)
Aqueous layer

Hexane layer

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*(d) Explain why iodine is more soluble in hexane than in water, by considering the
intermolecular forces in iodine, hexane and water and any intermolecular forces
formed between iodine and the solvents.

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Detailed descriptions of how the intermolecular forces form are not required.
(6)

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(Total for Question 19 = 14 marks)

17
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20 This question is about carbon dioxide.
(a) (i) Carbonate ions may be identified by their reaction with aqueous acid to

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produce carbon dioxide.
Give the ionic equation for this reaction. Include state symbols.
(2)

(ii) Limewater (an aqueous solution of calcium hydroxide) can be used to test for
the presence of gaseous carbon dioxide.
State what would be seen when carbon dioxide is bubbled through
limewater.
(1)

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(b) A student determined the solubility of calcium hydroxide in water by titration
with hydrochloric acid. The equation for the reaction is shown.

Ca(OH)2 + 2HCl → CaCl2 + 2H2O

Procedure
• calcium hydroxide powder was added to distilled water and the mixture was
stirred until no more solid dissolved.
The excess solid was filtered off to leave a saturated solution.
• 25.0 cm3 portions of this solution were titrated with
0.0500 mol dm–3 hydrochloric acid with phenolphthalein as an indicator
until two concordant titres were obtained.
The mean titre was 18.95 cm3.
(i) Calculate the concentration of the saturated solution, in g dm–3.
(4)
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(ii) The student used the same procedure to determine the solubility of
strontium hydroxide.
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Explain whether or not the mean titre value for strontium hydroxide would be
different from that for calcium hydroxide.
(2)

(c) Between 1960 and 2020 the amount of carbon dioxide in the atmosphere rose
from 320 parts per million (ppm) to 420 ppm.
The recent rapid increase in the atmospheric carbon dioxide is affecting the
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chemistry of seawater.
Carbon dioxide dissolves in water to form carbonic acid, H2CO3(aq).
The carbonic acid dissociates in water according to the equilibrium shown.

H2CO3(aq)  H+(aq) + HCO3–(aq)

Explain, in terms of the equilibrium, the effect of the increase in

atmospheric carbon dioxide on the acidity of seawater.
(3)

(Total for Question 20 = 12 marks)

TOTAL FOR SECTION B = 42 MARKS

19
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SECTION C
Answer ALL the questions. Write your answers in the spaces provided.

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21 This question is about some organic molecules which are important in the
production of adhesives and coatings.
(a) Compound X is a liquid containing carbon, hydrogen and oxygen only.
A sample of X, with a mass of 1.92 g, contains 1.08 g carbon and 0.131 g hydrogen.
(i) Use these data to calculate the empirical formula of X.
(3)

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(ii) The mass spectrum of X is shown.

100

Percentage 60
relative
abundance 40 DO NOT WRITE IN THIS AREA

0.0
30 40 50 60 70 80 90
m/z

Deduce the molecular formula of X, using the mass spectrum and

your answer to (a)(i).
(2)

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(iii) Reagents were added to separate samples of X to identify the functional
groups in the molecule.
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Complete Table 1.
(2)
Table 1

Reagent Observation Functional group

bromine water
bromine water
decolourised

aqueous sodium
effervescence
carbonate
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(iv) Using your answer to (a)(iii) and the mass spectrum, complete Table 2.
(2)
Table 2

Peak in mass spectrum Formula of ion

m / z = 41

m / z = 45

(v) X does not show geometric isomerism.

Draw a possible displayed formula of X.
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(1)

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(b) Propenoic acid can be produced industrially from propane-1,2,3-triol,
a by-product of the manufacture of biodiesel.

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The first step is a dehydration reaction to convert gaseous propane-1,2,3-triol to
propenal. This reaction requires a solid catalyst.

CH2OH CHO
CHOH CH + 2H2O
CH2OH CH2

(i) Explain how a catalyst increases the rate of this reaction.

Use the Maxwell–Boltzmann distribution shown and refer to the
collision theory.
(3)

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Number of
particles with
energy, E

Ea Energy, E

(ii) The propenal is then oxidised to propenoic acid.

Write an equation for this reaction using [O] to represent the oxygen from the
oxidising agent.
(1)

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(c) One synthetic route for the production of propenoic acid uses propene, derived
from crude oil, as a starting material.
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propene → propane-1,2-diol → prop-2-en-1-ol → propenoic acid

(i) Suggest suitable reagents and conditions for the conversion of propene to
propane-1,2-diol.
(2)

(ii) Suggest why the production of propenoic acid from propane-1,2,3-triol is

more sustainable than its production from propene.
(2)

(Total for Question 21 = 18 marks)

TOTAL FOR SECTION C = 18 MARKS

TOTAL FOR PAPER = 80 MARKS
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*P75592A02828*
*P75069A02424*
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Please check the examination details below before entering your candidate information
Candidate surname Other names

Centre Number Candidate Number

Pearson Edexcel International Advanced Level

Tuesday 16 January 2024
Morning (Time: 1 hour 30 minutes) Paper
reference WCH12/01
Chemistry  

International Advanced Subsidiary/Advanced Level

UNIT 2: Energetics, Group Chemistry,
Halogenoalkanes and Alcohols

You must have: Total Marks

Scientific calculator, Data Booklet

Instructions
• Use black ink or ball-point pen.
• IfFillpencil is used for diagrams/sketches/graphs it must be dark (HB or B).
• centre number
in the boxes at the top of this page with your name,
and candidate number.
• Answer all questions.
• – there may
Answer the questions in the spaces provided
be more space than you need.
• Show all your working in calculations and include units where appropriate.
Information
• The total mark for this paper is 80.
• – usemarks
The for each question are shown in brackets
this as a guide as to how much time to spend on each question.
• structurequestion
In the marked with an asterisk (*), marks will be awarded for your ability to
your answer logically, showing how the points that you make are related or
follow on from each other where appropriate.
• There is a Periodic Table on the back cover of this paper.
Advice
• Read each question carefully before you start to answer it.
• Try to answer every question.
• your answers if you have time at the end.
Check
Turn over

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You should aim to spend no more than 20 minutes on this section.
For each question, select one answer from A to D and put a cross in the box . If you change
your mind, put a line through the box and then mark your new answer with a cross .

1 Which compound has intermolecular hydrogen bonding?

A HF
B H2Te

C AsH3
D SnH4
(Total for Question 1 = 1 mark)

2 In which process are intermolecular hydrogen bonds broken?

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A H2(g) → 2H(g)

B H2O(l) → H2O(g)

C H2(l) → H2(g)

D H2(g) + ½O2(g) → H2O(g)

(Total for Question 2 = 1 mark)

3 A compound contains
• molecules with non-polar bonds
• permanent dipole-permanent dipole forces between its molecules.
What could be the formula of this compound?
Use the Data Booklet as a source of information.

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A NO

B BeCl2
C PH3

D CI4
(Total for Question 3 = 1 mark)

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4 Which alkane has the strongest London forces in the liquid phase?

A (CH3)4C
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B CH3CH2CH2CH2CH3

C (C2H5)4C
D CH3(CH2)7CH3
(Total for Question 4 = 1 mark)

5 In which liquid solvent would the solubility of lithium chloride (LiCl) be lowest?

A ammonia
B cyclohexane
C methanol

D water
(Total for Question 5 = 1 mark)
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6 Which compound does not contain an element with an oxidation number of –1?

A HF

B NaH
C H2O2

D CH4
(Total for Question 6 = 1 mark)

7 Which reaction involves the oxidation of a Group 7 element?

A Br2 + F2 → 2BrF
B U + 3ClF3 → UF6 + 3ClF
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C 2F2 + 2H2O → 4HF + O2

D KCl + H2SO4 → HCl + KHSO4

(Total for Question 7 = 1 mark)
Use this space for any rough working. Anything you write in this space will gain no credit.

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8 Equal volumes of some 0.01 mol dm–3 solutions were mixed.
Which pair of solutions gave the greatest mass of precipitate?

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A BaCl2 and AgNO3

B BaCl2 and Ag2SO4

C BaCl2 and NaNO3

D BaCl2 and Na2SO4

(Total for Question 8 = 1 mark)

9 Which test reagent could be used to identify an aqueous solution containing

hydrogencarbonate ions, HCO3– ?

A sodium carbonate

B sodium hydroxide

C nitric acid

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D ammonia
(Total for Question 9 = 1 mark)

10 Bromine, Br2(l), can be disposed of safely by reaction with

aqueous sodium thiosulfate, Na2S2O3(aq).

Br2(l) + 2Na2S2O3(aq) → 2NaBr(aq) + Na2S4O6(aq)

What is the minimum volume, in cm3, of 0.5 mol dm–3 Na2S2O3(aq) needed to react
completely with 0.01 mol of Br2(l)?

A 0.01
B 0.04

C 10

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D 40
(Total for Question 10 = 1 mark)
Use this space for any rough working. Anything you write in this space will gain no credit.

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11 What is the mass of nitrogen atoms in 50 cm3 of a 2.0 mol dm–3 solution of
ammonium nitrate, NH4NO3(aq)?
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A 35 g

B 8.0 g
C 2.8 g

D 1.4 g
(Total for Question 11 = 1 mark)

12 Which row shows the correct trends down the group for the elements of Group 7?

Reactivity as
Boiling temperature Electronegativity
oxidising agent
A increases decreases decreases

B decreases increases increases

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C increases decreases increases

D decreases increases decreases

(Total for Question 12 = 1 mark)

13 Which statement best explains why the rate of a chemical reaction increases with
increasing temperature?

A the activation energy decreases

B the number of collisions increases

C the kinetic energy of the particles increases

D the frequency of collisions with E  Ea increases

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(Total for Question 13 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

5
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14 Which statement is not true for a system at dynamic equilibrium?

A the position of equilibrium is affected by temperature,

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by pressure and by catalysts
B the concentration of reactants is constant

C the forward and backward reactions occur at equal rates

D the equilibrium can be reached from either direction
(Total for Question 14 = 1 mark)

15 Silver nitrate, in aqueous ethanol, is added separately to four halogenoalkanes.

Which would form a silver halide precipitate in the shortest time?

A 1-bromobutane

B 1-chlorobutane

C 1-fluorobutane

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D 1-iodobutane
(Total for Question 15 = 1 mark)

16 What is the total number of structural isomers for cyclic alcohols with the molecular
formula C4H8O?

A 2

B 3

C 4

D 5
(Total for Question 16 = 1 mark)
Use this space for any rough working. Anything you write in this space will gain no credit.

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17 Which is a correct equation for the incomplete combustion of butan-1-ol?

A CH3CH2CH2CH2OH + 6O2 → 4CO2 + 5H2O

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B CH3CH2CH2CH2OH + 6½O2 → 4CO2 + 5H2O

C CH3CH2CH2CH2OH + 4O2 → 4CO + 5H2O

D CH3CH2CH2CH2OH + 4½O2 → 4CO + 5H2O
(Total for Question 17 = 1 mark)

18 Which reagent(s) could be used to produce a chloroalkane from a tertiary alcohol?

1 PCl5
2 concentrated HCl
3 concentrated H2SO4 and KCl

A 1, 2 and 3

B 1 and 3 only
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C 2 and 3 only

D 1 only
(Total for Question 18 = 1 mark)

19 What amount, in mol, of [O] is needed to convert 1 mol of pentane-1,3,5-triol into

3-oxopentanedioic acid and water?

OH OH O OH

HO OH O O

pentane-1,3,5-triol 3-oxopentanedioic acid

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A 2

B 3
C 4
D 5
(Total for Question 19 = 1 mark)

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20 Which compound gives this mass spectrum?

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100

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60
Relative
intensity
40

0
10 15 20 25 30 35 40 45 50 55 60

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m/z

A CH3COOH

B CH3COCH3

C CH3CH2CHO
D CH3CH2CH2CH3
(Total for Question 20 = 1 mark)

TOTAL FOR SECTION A = 20 MARKS

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SECTION B
Answer ALL the questions. Write your answers in the spaces provided.

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21 This question is about the element calcium and some of its compounds.
(a) Give the complete electronic configuration, using s, p, d notation, of a
calcium atom in the ground state.
(1)

(b) Calcium reacts with chlorine to form calcium chloride.

Ca(s) + Cl2(g) → CaCl2(s)

(i) Explain, in terms of oxidation numbers, why this is a redox reaction.

(2)

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(ii) Complete the table to indicate the type(s) of bonding and structure in the
species involved in this reaction.
(3)

Species Bonding Structure

Ca(s)
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covalent

giant

(iii) State the expected flame colour when CaCl2 is used in a flame test.
(1)

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(c) A sample of solid anhydrous calcium nitrate, Ca(NO3)2(s), is heated strongly for
several minutes in the apparatus shown.
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Ca(NO3)2(s)

water containing
heat universal indicator

(i) State two observations that would be made.

(2)

1 . . .. . . .. . .. . . .. . . .. . .. . . .. . . . . . . .. ... ... .... ... ... ... ... ... ... ... .... ... ... ... ... ... ... .... ... ................ ..... ..... ..... ..... ..... ..... ..... ..... .... ..... ..... ..... ..... ..... ..... ..... ..... ..... ..... .... ..... ..... ..... ..... ..... .. ... ..... ..... ..... ..... .............

2 . . .. . . .. . .. . . .. . . .. . .. . . .. . . . . . . .. ... ... .... ... ... ... ... ... ... ... .... ... ... ... ... ... ... .... ... ................ ..... ..... ..... ..... ..... ..... ..... ..... .... ..... ..... ..... ..... ..... ..... ..... ..... ..... ..... .... ..... ..... ..... ..... ..... .. ... ..... ..... ..... ..... .............
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(ii) Explain why the observations from (c)(i) would be made more quickly if
the experiment was repeated with solid anhydrous magnesium nitrate,
Mg(NO3)2(s).
(3)

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*(d) Samples of calcium and magnesium are added to separate test tubes of
cold water containing a few drops of universal indicator.

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State and explain the differences in the observations made in each experiment.
Include an equation in your answer.
(6)

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.. . .. . . .. . . .. . .. . . .. . . .. . .. . . .. . . . . . . .. ... ... .... ... ... ... ... ... ... ... .... ... ... ... ... ... ... .... ... ................ ..... ..... ..... ..... ..... ..... ..... ..... .... ..... ..... ..... ..... ..... ..... ..... ..... ..... ..... .... ..... ..... ..... ..... ..... .. ... ..... ..... ..... ..... .............

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(Total for Question 21 = 18 marks)

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22 This question is about enthalpy changes.
A student wanted to use Hess’s Law to determine the enthalpy change, ΔrH1 ,

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in kJ mol–1, for Reaction 1.
Reaction 1 Mg(s) + ½O2(g) → MgO(s) Δ r H1
(a) Explain why ΔrH1 can also be described as an enthalpy change of formation.
(2)

(b) The student carried out an experiment to determine the enthalpy change of
reaction, ΔrH2 , in kJ mol–1, for Reaction 2.
Reaction 2 MgO(s) + 2HCl(aq) → MgCl2(aq) + H2O(l) ΔrH2
0.189 g of solid magnesium oxide was added to excess hydrochloric acid in a

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polystyrene cup and stirred until the reaction was complete.
The total mass of the solution formed was 25.0 g.
During the experiment, the temperature increased from 21.5°C to 28.0°C.
Calculate ΔrH2 , in kJ mol–1, including a sign.
Give your answer to an appropriate number of significant figures.
[ Specific heat capacity of the solution = 4.18 J g–1 °C–1. ]
(4)

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(c) Calculate the enthalpy change of reaction, ΔrH1 , for Reaction 1.
Use your answer to (b), the data provided and the enthalpy cycle shown.
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[If you did not calculate an answer to (b), use a value of –100 kJ mol–1.
This is not the correct answer.]
(2)
Data
Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) ΔrH = –462 kJ mol–1
H2(g) + ½O2(g) → H2O(l) ΔfH = –286 kJ mol–1

Enthalpy cycle

ΔrH1
Mg(s) + ½O2(g) MgO(s)

2HCl 2HCl
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MgCl2(aq) + H2(g) + ½O2(g) MgCl2(aq) + H2O(l)

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(Total for Question 22 = 8 marks)

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16
23 This question is about bromoalkanes with the molecular formula C4H9Br.
(a) (i) Give the IUPAC name of the only C4H9Br tertiary bromoalkane.
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(1)

(ii) Draw the displayed formula of the only C4H9Br secondary bromoalkane.
(1)
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(iii) Draw the skeletal formula of the only branched-chain C4H9Br

primary bromoalkane.
(1)

(b) Give the structure of the C4H9Br bromoalkane that would react fastest with
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aqueous silver nitrate in ethanol.

(1)

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(c) Some reactions of CH3CH2CH2CH2Br are shown.

CH3CH2CH2CH2OH

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R1

R4 R2
CH3CH2CH2CH2CN CH3CH2CH2CH2Br CH3CH2CH CH2

CH3CH2CH2CH2NH2

(i) Complete the table.

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(4)

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Formula
Reaction Name of mechanism of Condition(s)
reagent

R1 nucleophilic substitution

R2 heat in ethanol

R3 NH3

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R4 heat in ethanol

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(ii) Complete the mechanism for reaction R3.
Include curly arrows, and any relevant lone pairs, dipoles and charges.
(4)
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NH3

H H H

H7C3 C Br H7C3 C N H + Br–

H H H

NH3

CH3CH2CH2CH2NH2 + NH4+
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(iii) Give the wavenumber range of an absorption in the infrared spectrum of the
organic product of reaction R4, which is not present in the infrared spectrum
of CH3CH2CH2CH2Br.
Indicate the bond responsible for this absorption.
(2)

Wavenumber range . ... ... .... ... ... ... ... ... ... ... .... ... ... ... .............. .... ..... ..... ..... ..... ..... ..... ..... ..... ..... ..... ..... .... ..... ..... ..... ..... ..... ..... ..... ..... ..... ..... .... ..... ... ... ..... ..... .... ..... ..............

Bond .. . .. . . .. . . .. . .. . . . . . . .. ... ... ... .... ... ... ... ... ... ... .... ... ... ... ... ... ... ... .... .................. ..... ..... ..... ..... ..... ..... ..... .... ..... ..... ..... ..... ..... ..... ..... ..... ..... ..... ..... .... ..... ..... ..... ..... .... . ..... ..... ..... ..... ..... ..........
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(Total for Question 23 = 14 marks)

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TOTAL FOR SECTION B = 40 MARKS

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SECTION C
Answer ALL the questions. Write your answers in the spaces provided.

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24 The elements of Group 7, the halogens, have many important uses.
Fluorine is used to make sulfur hexafluoride, SF6 , a gas which is used
as an insulator in electrical equipment.
Chlorine is used as a bleach and as a disinfectant in water treatment.
Bromine is used to make organic chemicals that are used as fire retardants.
Iodine has been used in the catalyst in the manufacture of ethanoic acid.
(a) SF6 can be made from the reaction of sulfur, S8 , with fluorine.

S8(s) + 24F2(g) → 8SF6(g) ΔrH = –9672 kJ mol–1

The structure of S8(s) is shown.

S S

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S S

S S
S S

Bond enthalpy data

Bond Mean bond enthalpy / kJ mol–1

S S 268

F F 151

(i) Calculate the mean bond enthalpy, in kJ mol–1, for a single S F bond.
(3)

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(ii) Give two reasons why your answer to (a)(i) is unlikely to accurately represent
the true S F bond enthalpy in SF6 .
(2)
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(iii) SF6 is a potent greenhouse gas.

1.00 g of SF6 absorbs the same amount of infrared radiation as 23.9 kg of CO2 .
Calculate the number of molecules of CO2 , to the nearest whole number,
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that absorb the same amount of infrared radiation as one molecule of SF6 in
the atmosphere.
(3)
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(b) Bleach, NaClO(aq), is formed by the reaction of chlorine
with cold, dilute aqueous sodium hydroxide.

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Cl2(g) + 2NaOH(aq) → NaClO(aq) + NaCl(aq) + H2O(l)

The following species and equilibria are present in solutions of NaClO(aq).

Equilibrium 1 HClO(aq)  H+(aq) + ClO–(aq)

Equilibrium 2 HClO(aq) + Cl–(aq) + H+(aq)  Cl2(aq) + H2O(l)

Equilibrium 3 Cl2(aq)  Cl2(g)

Household bleach is stored at a pH between 11 and 13.
Household bleach should not be stored near strong acid.
(i) Give the formula of the chlorine-containing species present at
highest concentration in household bleach at pH 12.
(1)

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(ii) Explain why mixing strong acid with bleach is dangerous.
Justify your answer using the equilibria shown.
(3)

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(iii) On heating, NaClO disproportionates to form sodium chloride and
sodium chlorate(V).
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Give the equation for this disproportionation reaction.

State symbols are not required.
(2)

(c) The structure of a fire retardant is shown.

Br Br
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Br
Br

Calculate the percentage by mass of bromine in this fire retardant.

Give your answer to an appropriate number of significant figures.
(2)
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(d) The industrial manufacture of ethanoic acid first used an iodine-based catalyst.
Explain, with the aid of a labelled Maxwell–Boltzmann distribution, how a catalyst

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increases the rate of a chemical reaction.
(4)

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(Total for Question 24 = 20 marks)

TOTAL FOR SECTION C = 20 MARKS

TOTAL FOR PAPER = 80 MARKS

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28
Please check the examination details below before entering your candidate information
Candidate surname Other names

Centre Number Candidate Number

Pearson Edexcel International Advanced Level

Monday 13 May 2024
Morning (Time: 1 hour 30 minutes) Paper
reference WCH12/01
Chemistry  

International Advanced Subsidiary/Advanced Level

UNIT 2: Energetics, Group Chemistry,
Halogenoalkanes and Alcohols

You must have: Total Marks

Scientific calculator, Data Booklet, ruler

Information
• The total mark for this paper is 80.
• – usemarks
The for each question are shown in brackets
this as a guide as to how much time to spend on each question.
• to structure
In the question marked with an asterisk (*), marks will be awarded for your ability
your answer logically, showing how the points that you make are
related or follow on from each other where appropriate.
• A Periodic Table is printed on the back cover of this paper.
Advice
•• Read each question carefully before you start to answer it.
Show all your working in calculations and include units where appropriate.
•• Try to answer every question.
Check your answers if you have time at the end.
Turn over

Answer ALL the questions in this section.

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You should aim to spend no more than 20 minutes on this section.

For each question, select one answer from A to D and put a cross in the box . If you change
your mind about an answer, put a line through the box and then mark your new answer with
a cross .

1 An enthalpy level diagram for a reaction with an intermediate is shown.

intermediate
B C
D
Enthalpy

A products

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reactants

Progress of reaction

Which arrow shows the enthalpy change for this reaction?

A arrow A

B arrow B

C arrow C
D arrow D

(Total for Question 1 = 1 mark)

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2 Sodium chloride dissolves in water to form a solution because of the interactions

between the sodium chloride and water. What are these interactions?

A dipole-dipole
B hydrogen bonds

C ion-dipole
D London forces

(Total for Question 2 = 1 mark)

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3 Which equation represents the reaction for which the enthalpy change, ΔrH, is the
mean bond enthalpy of the C Cl bond in CCl4?
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A CCl4(g) → C(g) + 4Cl(g)

B ¼CCl4(g) → ¼C(g) + Cl(g)

C C(g) + 4Cl(g) → CCl4(g)

D ¼C(g) + Cl(g) → ¼CCl4(g)

(Total for Question 3 = 1 mark)

4 This question is about boiling temperatures.

(a) Which isomer has the highest boiling temperature?
(1)

A
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(b) Which compound has the highest boiling temperature?

(1)
A pentane
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B cyclopentane

C butan-1-ol
D butane-1,4-diol

(Total for Question 4 = 2 marks)

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5 Steam is passed over heated magnesium.
Which reaction occurs most readily?

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A Mg + H2O → MgO + H2

B Mg + 2H2O → Mg(OH)2 + H2
C 2Mg + H2O → Mg2O + H2

D 2Mg + 2H2O → 2MgOH + H2

(Total for Question 5 = 1 mark)

6 What are the products formed when lithium nitrate and calcium nitrate are
heated separately?

Lithium nitrate Calcium nitrate

A lithium nitrite and oxygen calcium nitrite and oxygen

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B lithium nitrite and oxygen calcium oxide, nitrogen dioxide
and oxygen
lithium oxide,
C calcium nitrite and oxygen
nitrogen dioxide and oxygen
lithium oxide, calcium oxide, nitrogen dioxide
D
nitrogen dioxide and oxygen and oxygen

(Total for Question 6 = 1 mark)

7 Group 2 compounds give different colours in a flame test.

The best explanation is that the cations have different

A gaps between electronic energy levels

B ionic radii

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C ionisation energies

D numbers of electrons
(Total for Question 7 = 1 mark)
Use this space for any rough working. Anything you write in this space will gain no credit.

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8 Two tests were performed on an unknown ionic compound.
Silver nitrate solution was added to an aqueous solution of the compound, forming a
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white precipitate.
A flame test carried out on the ionic compound gave a red flame.
The unknown compound could have been

A calcium iodide

B lithium bromide
C potassium carbonate

D strontium chloride

(Total for Question 8 = 1 mark)

9 Which compound needs exactly nine moles of oxygen (O2) for complete combustion
of one mole of the compound?
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A C5H12

B C6H12O

C C6H14

D C6H14O

(Total for Question 9 = 1 mark)

10 Which solution remains clear on addition to barium chloride solution?

A dilute sulfuric acid

B silver nitrate solution

C sodium nitrate solution

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D sodium sulfate solution

(Total for Question 10 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

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11 In a titration, a conical flask containing 10.00 cm3 of 1.00 mol dm–3 sulfuric acid is fully
neutralised by 25.00 cm3 of 0.80 mol dm–3 potassium hydroxide.

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(a) The titration is carried out using methyl orange as an indicator.
What would be the colour change at the end-point of the titration?
(1)
A orange to red
B red to orange

C orange to yellow
D yellow to orange

(b) What is the concentration, in mol dm–3, of the potassium sulfate solution
produced by this reaction at the end-point, to 2 significant figures?
(1)
A 0.010

B 0.020

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C 0.29

D 0.57

(c) Information about the uncertainties in each reading used to measure the volumes
of the solutions in this titration is shown.

Solution Equipment used Uncertainty / cm3

sulfuric acid pipette ±0.04

potassium hydroxide burette ±0.05

(1)
Which statement is true?

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A the percentage uncertainty of the volume of sulfuric acid is more than

the percentage uncertainty of the volume of potassium hydroxide
B the percentage uncertainty of the volume of sulfuric acid is 0.8 %
C the total percentage uncertainty is 0.8 %

D the percentage uncertainty of the volume of potassium hydroxide

solution is 0.2 %

(Total for Question 11 = 3 marks)

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12 The boiling temperatures of the halogens increase down Group 7 because on
descending the group the
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A bond polarities increase

B covalent bond strengths increase

C electronegativities increase

D number of electrons in the molecule increase

(Total for Question 12 = 1 mark)

13 Bromine and chlorine each have two stable isotopes, 79Br, 81Br, 35Cl and 37Cl.
Which statement is true?

A the atomic radius of 81Br is greater than that of 79Br

B the electronegativity of 35Cl is greater than that of 37Cl

C the first ionisation energy of 37Cl is greater than that of 79Br

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D the mass spectrum of CH2BrCl has two molecular ion peaks

(Total for Question 13 = 1 mark)

14 Cyclohexane (density = 0.78 g cm–3) and aqueous iodine (density > 1.0 g cm–3 ) are
shaken and left to stand.
What colours are the two layers that form?

lower layer upper layer

A brown yellow

B yellow purple

C yellow brown

D purple brown
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(Total for Question 14 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

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15 Four containers of the same dimensions hold samples of a gas.
For Container 1, the diagram of the Maxwell-Boltzmann distribution of molecular

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energy for this gas shows the activation energy, Ea , the mean molecular energy,
Emean , and the most probable molecular energy, Emode .

Number of
particles

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Emode Emean Ea
Energy

(a) For Container 2, the temperature is increased.

For which values would the energy value change?
(1)
A Ea only

B Emode only
C Emode and Emean only

D Ea , Emode and Emean

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(b) For Container 3, at the same temperature as Container 1, the pressure is lower.
For which values would the number of particles at that value change?
(1)
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A Ea only

B Emode only
C Emode and Emean only

D Ea , Emode and Emean

(c) For Container 4, at the same temperature and pressure as Container 1, the walls of
the container act as a catalyst for the reaction of the gas.
For which values would the energy value change?
(1)
A Ea only

B Emode only

C Emode and Emean only

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D Ea , Emode and Emean

(Total for Question 15 = 3 marks)

TOTAL FOR SECTION A = 20 MARKS

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SECTION B

Answer ALL the questions. Write your answers in the spaces provided.

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16 This question is about the reactions of halogenoalkanes.
(a) When halogenoalkanes are heated with potassium hydroxide, the products
depend on the conditions.
(i) State what condition, other than a suitable temperature and concentration
of potassium hydroxide, would give a high yield of but-1-ene and but-2-ene
from 2-chlorobutane.
(1)

(ii) Give the type of reaction occurring in (a)(i).

(1)

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(b) (i) State what condition, other than a suitable temperature and concentration
of potassium hydroxide, would give a high yield of butan-1-ol from
1-chlorobutane.
(1)

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(ii) Complete the mechanism for the reaction of potassium hydroxide with
1-chlorobutane to form butan-1-ol.
Use curly arrows and show relevant dipoles and lone pairs.
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(2)

OH–
H H H H

H C C C C Cl

H H H H
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H H H H

H C C C C OH + Cl–

H H H H

(iii) Give two reasons why, under the conditions used in (b)(ii), the reaction
between potassium hydroxide and 2-iodo-2-methylpropane is faster than the
reaction between potassium hydroxide and 1-chlorobutane.
(2)

(Total for Question 16 = 7 marks)

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17 In a titration between a weak acid and a weak base indicators do not give a distinct
colour change, so other techniques must be used.
One technique is thermometric titration.

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Procedure
Step 1 The temperature of 30.0 cm3 of dilute ethanoic acid in a polystyrene cup
is recorded.
Step 2 Ammonia solution of concentration 1.30 mol dm‒3 is added to the acid in the
polystyrene cup in separate 5.00 cm3 portions.
After each addition the mixture is stirred and the temperature measured.
A student carried out the experiment and plotted the graph shown.

29.0

28.0

27.0

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26.0

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25.0
Temperature
/ °C 24.0

23.0

22.0

21.0

20.0
0.0 5.0 10.0 15.0 20.0 25.0 30.0 35.0 40.0
Volume of added NH3(aq) / cm3

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(a) Find the end-point volume and the maximum temperature by adding appropriate
lines of best fit to the graph.
(3)
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End-point volume = . ... ... ... ... ... .... ... ... ... ... ... ... ... ...................... ..... ..... ..... ..... ..... .... ..... ..... ..... ..... ..... ..... ..... ..... ..... ..... ..... .... ..... ..... ..... ..... ..... ..... ... .. ..... ..... ..... ..... ..............

Maximum temperature = .. ... ... ... .... ... ... ... ... ... ................ ..... ..... ..... ..... ..... ..... ..... ..... .... ..... ..... ..... ..... ..... ..... ..... ..... ..... ..... .... ..... ..... ..... ..... ..... ..... ..... ..... ..... ..... ............

(b) Calculate the number of moles of ammonia added at the end-point.

(1)

(c) The reaction that occurs is shown.

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CH3COOH(aq) + NH3(aq) → CH3COONH4(aq)

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Calculate the enthalpy change of neutralisation for this reaction, in kJ mol‒1.

Give your answer to an appropriate number of significant figures and include a
sign with your answer.
[Assume that the density of all solutions is 1.00 g cm‒3 and that the
specific heat capacity of all solutions is 4.18 J g–1 °C–1]
(5)
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(Total for Question 17 = 9 marks)

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18 Chlorine dioxide, ClO2 , can be used to treat water to make it safe for drinking.
The molecule is a free radical. One suggested structure is shown.

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•
Cl
O O

(a) (i) Complete the dot-and-cross diagram for this structure.

Use dots (•) for oxygen electrons and crosses (×) for chlorine electrons.
(2)

O O

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(ii) Give the reason why chlorine dioxide is not a linear molecule.
(1)

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(b) Chlorine dioxide can be made from potassium chlorate(V), KClO3 , in a
two-step process.
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Step 1 Potassium chlorate(V) reacts with concentrated sulfuric acid to form

compound A.
Step 2 Compound A then undergoes a disproportionation reaction to form
chlorine dioxide and hydrogen chlorate(VII), HClO4.
(i) State the meaning of the Roman numerals in chlorate(V) and chlorate(VII).
(1)

(ii) State the oxidation number of chlorine in chlorine dioxide.

(1)
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(iii) In Step 2, compound A undergoes disproportionation.

Deduce the possible range of oxidation numbers for the chlorine in
compound A. Justify your answer.
(2)

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(iv) Compound A has Mr = 84.5, and a composition by mass of H = 1.18 %,
Cl = 42.01 % and the remainder is oxygen.

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Deduce the molecular formula of compound A, showing all your working.
(4)

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(v) Write an equation for each of the two steps in the formation of
chlorine dioxide, using your answers in (b).
State symbols are not required.
(2)

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(Total for Question 18 = 13 marks)

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19 One industrial preparation of ethanol is by the catalysed hydration of ethene via a
reversible reaction.
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H2O + CH2 CH2  CH3CH2OH ΔrH = ‒42 kJ mol–1

(a) The hydration of ethene requires a catalyst which is coated onto a solid
silicon dioxide support.
Identify, by name or formula, the catalyst used.
(1)

(b) Under these conditions, the conversion of ethene to ethanol is 5 % at equilibrium

but the overall yield of ethanol for the process is 95 %.
Suggest what happens to the equilibrium mixture containing ethanol so that the
overall yield of ethanol becomes 95 %.
(2)
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(c) The temperature used is 300 °C and the pressure used is 7 MPa. These, and the
amount of water present in the reaction mixture, are all compromises.
(i) Explain why the temperature used is a compromise.
(2)

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(ii) Explain why a manufacturer might suggest a pressure of greater than the
compromise pressure of 7 MPa.
(2)

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(iii) At pressures greater than 7 MPa, a waxy solid forms which melts over a range
of temperatures.
Identify, by name or formula, this solid.
(1)

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(iv) Give one other reason for not operating the process at a pressure greater than
7 MPa. Do not include safety considerations in your answer.
(1)

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(v) Increasing the amount of water in the reaction mixture, without changing the
pressure, might also be suggested.
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Suggest one advantage and one disadvantage of increasing the amount

of water.
(2)

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(Total for Question 19 = 11 marks)

TOTAL FOR SECTION B = 40 MARKS

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SECTION C

Answer ALL the questions. Write your answers in the spaces provided.

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20 Terpenes and terpenoids are groups of chemicals found in plants.
They contribute to the smell and taste of the plant, and so are used in flavourings
and perfumes.
Both terpenes and terpenoids have carbon skeletons based on one or more units of
the compound isoprene.

isoprene

Terpenes are made up of two or more isoprene units joined together, while
terpenoids have additional functional groups, often containing oxygen.
Limonene and myrcene are both terpenes composed of two isoprene units.

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Menthol, linalool and citronellol are terpenoids containing an ‒OH group.
(a) (i) Give the IUPAC name for isoprene.
(1)

(ii) The peaks with the highest intensity in the mass spectrum of isoprene are at
m / z = 68 and m / z = 53.
Identify the species responsible for these two peaks.
(2)
m / z = 68

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m / z = 53

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(iii) The infrared spectrum of isoprene is shown.
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R
Transmittance P
Q
/%
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3000 2000 1000

–1
Wavenumber / cm

State the origins of the peaks labelled P, Q and R. You may use a
labelled diagram.
Use the Data Booklet as a source of information.
(3)
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P . . .. . .. . . .. . . .. . .. . . .. . . .. . . . . . . .. .... ... ... ... ... ... ... ... .... ... ... ... ... ... ... .... ... ... ... ................... ..... .... ..... ..... ..... ..... ..... ..... ..... ..... ..... ..... ..... .... ..... ..... ..... ..... ..... ..... ..... ..... ..... ..... .... ..... ..... ..... ..... ..... ..........

Q . .. . .. . . .. . . .. . .. . . .. . . .. . . . . . . .. .... ... ... ... ... ... ... ... .... ... ... ... ... ... ... .... ... ... ... ................... ..... .... ..... ..... ..... ..... ..... ..... ..... ..... ..... ..... ..... .... ..... ..... ..... ..... ..... ..... ..... ..... ..... ..... .... ..... ..... ..... ..... ..... ..........

R . . .. . .. . . .. . . .. . .. . . .. . . .. . . . . . . .. .... ... ... ... ... ... ... ... .... ... ... ... ... ... ... .... ... ... ... ................... ..... .... ..... ..... ..... ..... ..... ..... ..... ..... ..... ..... ..... .... ..... ..... ..... ..... ..... ..... ..... ..... ..... ..... .... ..... ..... ..... ..... ..... ..........

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(b) (i) Show that myrcene and limonene are terpenes by comparing the molecular
and/or empirical formulae of myrcene, limonene and isoprene.

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myrcene limonene isoprene

(2)

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(ii) Both myrcene and limonene can be completely hydrogenated by reaction

with hydrogen.
State the conditions required for hydrogenation of alkenes.
(1)

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(iii) 5 g samples of myrcene and limonene were completely hydrogenated.
Calculate the volume of hydrogen required to hydrogenate each sample.
Include the unit with your answer.
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Assume the volume of 1 mol of hydrogen = 24 000 cm3

(4)
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(iv) Give the IUPAC name of the product formed by complete hydrogenation
of myrcene.
(1)

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*(c) Three students were asked to carry out a single chemical test to unambiguously
identify the presence of the ‒OH group in the three terpenoid compounds,
menthol, linalool and citronellol.

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HO

OH OH

menthol linalool citronellol

The first student tried using acidified potassium dichromate(VI) to oxidise

the alcohols.
The second tried acidified potassium manganate(VII), an oxidising agent similar
to potassium dichromate(VI).

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The third student tried using phosphorus(V) chloride.

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Criticise the three students’ suggestions by linking the expected results, and the
actual observations that would be made, for each test and the structures of the
three alcohols.
(6)

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(Total for Question 20 = 20 marks)

TOTAL FOR SECTION C = 20 MARKS

TOTAL FOR PAPER = 80 MARKS

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28
Please check the examination details below before entering your candidate information
Candidate surname Other names

Centre Number Candidate Number

Pearson Edexcel International Advanced Level

Monday 13 May 2024
WCH12/01R
Morning (Time: 1 hour 30 minutes) Paper
reference

Chemistry  

International Advanced Subsidiary/Advanced Level

UNIT 2: Energetics, Group Chemistry,
Halogenoalkanes and Alcohols

You must have: Total Marks

Scientific calculator, Data Booklet, ruler

Information
•• The total mark for this paper is 80.
The marks for each question are shown in brackets
– use this as a guide as to how much time to spend on each question.
• Into the question marked with an asterisk (*), marks will be awarded for your ability
structure your answer logically, showing how the points that you make are
related or follow on from each other where appropriate.
• A Periodic Table is printed on the back cover of this paper.

Advice
• Read each question carefully before you start to answer it.
•• Show all your working in calculations and include units where appropriate.
Try to answer every question.
• Check your answers if you have time at the end. Turn over

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You should aim to spend no more than 20 minutes on this section.
For each question, select one answer from A to D and put a cross in the box . If you change
your mind, put a line through the box and then mark your new answer with a cross .

1 A Maxwell-Boltzmann distribution of molecular energies is shown.

P
Q

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R S

(a) Which letter represents the mean energy of the molecules?

(1)
A letter P

B letter Q
C letter R

D letter S

(b) What happens to the curve when the temperature is decreased?

(1)
A the peak becomes higher and further to the right
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B the peak becomes higher and further to the left

C the peak becomes lower and further to the right

D the peak becomes lower and further to the left

(Total for Question 1 = 2 marks)

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2 The reaction profile for a reaction is shown.
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X
Products

W
Enthalpy Y

Z
Reactants

Progress of reaction

Which arrow represents the activation energy of the forward reaction?

A letter W
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B letter X
C letter Y

D letter Z
(Total for Question 2 = 1 mark)
Use this space for any rough working. Anything you write in this space will gain no credit.
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3 The reaction between calcium carbonate and hydrochloric acid is investigated.

CaCO3(s) + 2HCl(aq) → CaCl2(aq) + H2O(l) + CO2(g)

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(a) Which change in property will not affect the rate of this reaction?
(1)

A concentration of hydrochloric acid

B particle size of calcium carbonate

C pressure of the system

D temperature of hydrochloric acid

(b) The graph shows the results of one of the experiments.

120

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100

80
Volume of
carbon dioxide / cm3
60

20
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0
0 20 40 60 80 100 120

Time / s

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What is the approximate rate of reaction in cm3 s–1 at 20 seconds?
(1)
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A 0.67

B 0.70

C 1.50
D 3.50
(Total for Question 3 = 2 marks)
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4 Nitrogen reacts with hydrogen to form ammonia.

½N2(g) + 1½H2(g)  NH3(g) ∆fH = –46 kJ mol–1

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Bond Bond enthalpy / kJ mol–1

H H 436

N N 945

What is the bond enthalpy, in kJ mol–1, of the N H bond?

A 360

B 391

C 548

D 1173

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(Total for Question 4 = 1 mark)

5 A gas cylinder contains 2.5 kg of butane.

How many molecules of butane are in the cylinder?
[Molar mass of butane = 58.0 g mol–1 Avogadro constant, L = 6.02 × 1023 mol–1]

A 1.40 × 1022

B 2.59 × 1022
C 1.40 × 1025

D 2.59 × 1025
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Use this space for any rough working. Anything you write in this space will gain no credit.

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6 In an experiment to calculate the enthalpy change of neutralisation, ∆neutH ,
25 cm3 of 0.1 mol dm–3 hydrochloric acid, HCl, was reacted with 25 cm3 of 0.1 mol dm–3
sodium hydroxide solution. The increase in temperature, ∆T, was recorded.
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[Assume the density of the solutions = 1.00 g cm–3

Specific heat capacity of solutions = 4.2 J g–1 °C–1 ]
(a) Which is the correct expression to calculate the enthalpy change of neutralisation
for this reaction, in J mol–1 ?
(1)

ΔT " 4.2 " 50

A
5.0 " 10 !3

ΔT " 4.2 " 25

B
2.5 " 10 !3

!ΔT " 4.2 " 50

C
5.0 " 10 !3
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!ΔT " 4.2 " 50

D
2.5 " 10 !3

(b) The table below shows the measurement uncertainty of some

laboratory apparatus.

Measurement uncertainty
Apparatus
on each reading / cm3

burette +/− 0.05

25 cm3 measuring cylinder +/− 0.5

25 cm3 volumetric flask +/− 0.1

25 cm3 pipette +/− 0.06

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Which piece of apparatus would measure 25 cm3 of hydrochloric acid with the
lowest percentage uncertainty?
(1)

A burette
B measuring cylinder

C volumetric flask

D pipette
(Total for Question 6 = 2 marks)

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7 Which equation shows the reaction that occurs when the standard enthalpy change
of atomisation of iodine is measured?

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A I2(s) → 2I(g)

B ½I2(s) → I(g)

C I2(g) → 2I(g)
D ½I2(g) → I(g)
(Total for Question 7 = 1 mark)

8 Which statement about the elements in Group 7 is not correct?

A they all exist as diatomic molecules

B electronegativity decreases down the group

C reactivity increases up the group

D they all show variable oxidation states in their compounds

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(Total for Question 8 = 1 mark)

9 What are the only products formed when chlorine reacts with
cold aqueous sodium hydroxide?

A sodium chloride, sodium chlorate(I) and water

B sodium chloride, sodium chlorate(V) and water

C sodium chlorate(I) and water

D sodium chloride and sodium chlorate(I)

(Total for Question 9 = 1 mark)

10 Which statement about the reaction between concentrated sulfuric acid and
potassium bromide is correct?
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A bromide ions are reduced

B hydrogen bromide and hydrogen sulfide are formed

C sulfuric acid acts as an oxidising agent

D bromine and hydrogen sulfide are formed

(Total for Question 10 = 1 mark)

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11 Which statement is correct about the solubilities of Group 2 compounds as the group
is descended?
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A the solubility of the hydroxides and sulfates increases for both

B the solubility of the hydroxides and sulfates decreases for both

C the solubility of the hydroxides increases and the solubility of the

sulfates decreases
D the solubility of the hydroxides decreases and the solubility of the
sulfates increases
(Total for Question 11 = 1 mark)

12 Which nitrate does not produce brown fumes when heated?

A LiNO3

B KNO3

C Ca(NO3)2
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D Ba(NO3)2
(Total for Question 12 = 1 mark)

13 Compound X gives a red flame test and a solution of X produces a white precipitate
when added to nitric acid and silver nitrate solution.
Which could be compound X?

A LiCl

B NaCl
C NaBr

D RbBr
(Total for Question 13 = 1 mark)
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14 Which species contains an element with an oxidation number of +4?

A CrO42–

B MnO42–
C H2SO4

D Na2CO3
(Total for Question 14 = 1 mark)

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15 The compounds W, X, Y and Z have different boiling temperatures.

CH3

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CH3CH2CH2CH3 H 3C C CH3

Compound W Compound X

CH3
CH3CH2CH2CH2Br H 3C C CH3

Compound Y Compound Z

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Which is the correct order of increasing boiling temperature?

A X < W < Z < Y

B X < Z < W < Y

C W < X < Y < Z

D X < W < Y < Z
(Total for Question 15 = 1 mark)

16 How many structural isomers are there with the molecular formula C3H6BrI ?

A 4

B 5
C 6
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D 7
(Total for Question 16 = 1 mark)
Use this space for any rough working. Anything you write in this space will gain no credit.

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17 Which alcohol can be oxidised to a carboxylic acid by acidified
potassium dichromate(VI)?
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OH
A

B
OH

C
OH

D OH
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(Total for Question 17 = 1 mark)

TOTAL FOR SECTION A = 20 MARKS

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SECTION B
Answer ALL the questions in this section.

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Write your answers in the spaces provided.
18 This question is about Group 2 carbonates.
Group 2 carbonates decompose on heating to form the corresponding metal oxide
and carbon dioxide. The general equation is shown.

MCO3(s) → MO(s) + CO2(g)

(a) A sample of magnesium carbonate was heated for 4 minutes.

The mass of the sample decreased from 4.17 g to 2.35 g.
Calculate the percentage of magnesium carbonate that has decomposed.
[Molar mass of magnesium carbonate = 84.3 g mol–1]
(3)

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(b) The enthalpy change, ∆rH , for the thermal decomposition of
magnesium carbonate, MgCO3 , can be calculated using the data in the table.
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Enthalpy change of
Substance
formation / kJ mol–1

MgCO3 –1095.8

MgO –601.7

CO2 –393.5

(i) Complete the Hess cycle with two arrows and correct species and state
symbols in the box.
(2)

Δ rH
MgCO3(s) MgO(s) + CO2(g)
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(ii) Calculate the enthalpy change for the thermal decomposition of

magnesium carbonate, ∆rH . Include a sign and units in your answer.
(2)
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(c) Explain how the enthalpy change for the thermal decomposition of
calcium carbonate, CaCO3 , compares to that for magnesium carbonate in (b)(ii).
(3)

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. . . . . .. . . . . ...................... . . . . . . . . .. . . . . . . . . . . .. . . . . . . . . . .. . . . . . . . . . .. . . . . . . . . . .. . . . . . . . . . .. . . .. ... .. .. .. .. .............................................................................................................................. .............. .. ....................

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(Total for Question 18 = 10 marks)

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19 This question is about ozone, O3 .
Ozone is formed by the action of ultraviolet radiation on oxygen molecules.
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3O2(g)  2O3(g) ∆rH = +143 kJ mol–1

Ozone is a pale blue gas and oxygen gas is colourless.

A mixture of oxygen and ozone was placed in a sealed container and left to
reach equilibrium.
(a) (i) Explain what you would see on heating the mixture.
(2)

. . . . . .. . . . . ...................... . . . . . . . . .. . . . . . . . . . . .. . . . . . . . . . .. . . . . . . . . . .. . . . . . . . . . .. . . . . . . . . . .. . . .. ... .. .. .. .. .............................................................................................................................. .............. .. ....................

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. . . . . .. . . . . ...................... . . . . . . . . .. . . . . . . . . . . .. . . . . . . . . . .. . . . . . . . . . .. . . . . . . . . . .. . . . . . . . . . .. . . .. ... .. .. .. .. .............................................................................................................................. .............. .. ....................

(ii) Explain what you would see on increasing the pressure.

(2)

. . . . . .. . . . . ...................... . . . . . . . . .. . . . . . . . . . . .. . . . . . . . . . .. . . . . . . . . . .. . . . . . . . . . .. . . . . . . . . . .. . . .. ... .. .. .. .. .............................................................................................................................. .............. .. ....................

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. . . . . .. . . . . ...................... . . . . . . . . .. . . . . . . . . . . .. . . . . . . . . . .. . . . . . . . . . .. . . . . . . . . . .. . . . . . . . . . .. . . .. ... .. .. .. .. .............................................................................................................................. .............. .. ....................

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(b) Ozone can be used in the treatment of drinking water. As well as killing
bacteria and viruses, ozone also removes other dissolved impurities such
as hydrogen sulfide, H2S. Hydrogen sulfide reacts with ozone to produce

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sulfuric acid.

4O3(g) + H2S(aq) → H2SO4(aq) + 4O2(g)

State the role of the ozone in this redox reaction.

Justify your answer using oxidation numbers.
(3)

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(c) Ozone can also be used in the treatment of water in swimming pools.
A swimming pool has a volume of 375 000 dm3 and contains 15 g of ozone.
Calculate the concentration of ozone in the pool in parts per million (ppm).
[Assume the density of water in the swimming pool = 1.00 g cm–3 ]
(2)

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(Total for Question 19 = 9 marks)

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20 An organic compound, acetoin, is one of the compounds that gives butter its
characteristic flavour.
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(a) Acetoin contains 54.5 % by mass of carbon and 9.1 % by mass of hydrogen.
The remainder is oxygen.
(i) Calculate the empirical formula of acetoin.
You must show all your working.
(3)
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(ii) The molar mass of acetoin is 88.0 g mol–1.

Use this information to calculate the molecular formula of acetoin.
(1)
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(b) Acetoin contains two functional groups.
(i) Some chemical tests were carried out on acetoin. These tests identify one of

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the two functional groups.
Acetoin produced steamy fumes when reacted with PCl5 .
Acetoin did not react with sodium hydrogencarbonate solution.
Acetoin turned hot acidified potassium dichromate(VI) solution from orange
to green.
State what can be deduced from each of these three tests and hence identify
this functional group.
(3)

. . . . . .. . . . . ...................... . . . . . . . . .. . . . . . . . . . . .. . . . . . . . . . .. . . . . . . . . . .. . . . . . . . . . .. . . . . . . . . . .. . . .. ... .. .. .. .. .............................................................................................................................. .............. .. ....................

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. . . . . .. . . . . ...................... . . . . . . . . .. . . . . . . . . . . .. . . . . . . . . . .. . . . . . . . . . .. . . . . . . . . . .. . . . . . . . . . .. . . .. ... .. .. .. .. .............................................................................................................................. .............. .. ....................

(ii) Acetoin also contains the carbonyl group C O, in the form of a ketone not
an aldehyde.
Use page 5 of your Data Booklet to show how infrared spectra data could be
used to prove that acetoin contains a ketone not an aldehyde.
Complete the table.
(3)

Bond Wavenumber range / cm–1

Absorption present in acetoin

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but not in an aldehyde

One absorption present in an

aldehyde but not in acetoin

Another absorption present in

an aldehyde but not in acetoin

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(iii) Part of the mass spectrum of acetoin is shown.

100
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60
Relative intensity
40

0.0
15 30 45 60 75 90
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m/z

Determine a possible structure of acetoin using your answer to part (b)(i), the
information given in (b)(ii) and the mass spectrum.
In your answer, identify the two ions responsible for the two peaks of
highest intensity.
(3)
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(Total for Question 20 = 13 marks)

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21 This question is about halogenoalkanes.
(a) Complete the table by giving the displayed formula and name of

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each halogenoalkane.
(3)

A straight chain primary

A tertiary iodoalkane with the
chloroalkane with the
molecular formula C4H9I
molecular formula C4H9Cl
Displayed
formula

Name

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(b) The two halogenoalkanes in part (a) react with aqueous potassium hydroxide to
produce alcohols.
Give two reasons why the rate of reaction of the iodoalkane is faster than that of
the chloroalkane.
(2)

Reason 1 ....... . . . . . .. . . . . . . . . . .. . . . . . . . . . .. . . . . . . . . . . .. . . . . . . . . . .. . . . . . . . . . .. . . . . . .. .. .. .. .. ... .. ............................................................................................................................................. ....................

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Reason 2 ...... . . . . . .. . . . . . . . . . .. . . . . . . . . . .. . . . . . . . . . . .. . . . . . . . . . .. . . . . . . . . . .. . . . . . .. .. .. .. .. ... .. ............................................................................................................................................. ....................

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(c) Halogenoalkanes react with cyanide ions, CN– , in alcoholic solution to form
nitriles. The cyanide ions act as nucleophiles.
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Complete the mechanism for the formation of butanenitrile, CH3CH2CH2CN .

Include curly arrows, and relevant lone pairs and dipoles.
(3)

H H H

H C C C Br

H H H
CN–
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(Total for Question 21 = 8 marks)

TOTAL FOR SECTION B = 40 MARKS

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SECTION C
Answer ALL the questions in this section.
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Write your answers in the spaces provided.

22 Ammonia, ammonium nitrate and urea are nitrogen-based fertilisers.
The nitrogen in the fertiliser is taken up by the roots of plants and promotes growth.
Ammonia, NH3 , is manufactured by the reaction between nitrogen and hydrogen.
The nitrogen is obtained from the air.
Hydrogen can be obtained by two methods.
Method 1
The hydrogen is usually obtained by reacting methane gas with steam.

CH4 + 2H2O → CO2 + 4H2

Method 2
Hydrogen can also be obtained using solar power to split water into hydrogen
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and oxygen.

2H2O → O2 + 2H2

(a) Evaluate which of these two methods used to obtain hydrogen is

more sustainable.
(3)

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(b) Ammonia can be used directly as a fertiliser or converted to other compounds
such as ammonium nitrate and urea.

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Name of fertiliser ammonia ammonium nitrate urea

Formula NH3 NH4NO3 NH2CONH2

% nitrogen by mass 82.4 46.7

(i) Complete the table by calculating the percentage by mass of nitrogen in

ammonium nitrate.
(1)

(ii) Give one advantage and one disadvantage of applying ammonia directly into

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the soil as a fertiliser.
Use information in the table and your knowledge of ammonia.
(2)
Advantage

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Disadvantage

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(c) Ammonium nitrate, NH4NO3 , can be made by reacting ammonia with nitric acid.
(i) Give the equation for this reaction. State symbols are not required.
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(1)

(ii) Name the type of reaction occurring.

(1)

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*P78392A02432* 
(d) Urea, NH2CONH2 , can also be made from ammonia.
Complete the dot-and-cross diagram for the urea molecule.
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(2)

N N
H H
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H H
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*(e) Both urea and ammonium nitrate are soluble in water.
Discuss the differences in the interactions of water molecules with both urea and

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ammonium nitrate.
Include three diagrams showing these interactions.
(6)

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 *P78392A02732* Turn over
(f ) A field needs 160 kg of N per hectare to be applied using urea fertiliser.
The field size is 500 m × 640 m.

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[1 hectare (ha) = 10 000 m2 , molar mass of urea = 60 g mol–1 ]
Urea contains 46.7 % N by mass.
Calculate the mass of urea, in tonnes, that needs to be applied to the field.
Give your answer to an appropriate number of significant figures.
(4)

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(Total for Question 22 = 20 marks)

TOTAL FOR SECTION C = 20 MARKS

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TOTAL FOR PAPER = 80 MARKS

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*P78392A03232*
32
Please check the examination details below before entering your candidate information
Candidate surname Other names

Centre Number Candidate Number

Pearson Edexcel International Advanced Level

Time 1 hour 30 minutes
Paper
reference WCH12/01
Chemistry
 

International Advanced Subsidiary/Advanced Level

UNIT 2: Energetics, Group Chemistry,
Halogenoalkanes and Alcohols
You must have: Total Marks
Scientific calculator, Data Booklet, ruler May/June 2022

Turn over

Q:1/1/1/
*P70965A0128*
SECTION A
Answer ALL the questions in this section.
You should aim to spend no more than 20 minutes on this section.
For each question, select one answer from A to D and put a cross in the box . If you change
your mind, put a line through the box and then mark your new answer with a cross .
1 Which equation represents the standard enthalpy change of formation, ΔfH d , for
aluminium oxide?

A 2Al(s) + 1½O2(g) → Al2O3(s)

B 2Al(s) + 3O(g) → Al2O3(s)

C 4Al(s) + 3O2(g) → 2Al2O3(s)

D 4Al(s) + 6O(g) → 2Al2O3(s)

(Total for Question 1 = 1 mark)

2 How does an oxidising agent change during a redox reaction?

Electrons Oxidation number

A gains electrons decreases

B gains electrons increases

C loses electrons decreases

D loses electrons increases

(Total for Question 2 = 1 mark)

3 Which of these compounds would be expected to have the

highest boiling temperature?

A (CH3)3COH

B CH3CH2CH2CH2OH

C CH3CH2CH(CH3)2

D CH3CH2CH2CH2CH3

(Total for Question 3 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

2
*P70965A0228*
4 What is the name of the compound with the formula KClO2 ?

A potassium chlorate(II)

B potassium chlorate(III)

C potassium chlorate(IV)
D potassium chlorate(V)

(Total for Question 4 = 1 mark)

5 A small piece of calcium is added to a beaker of distilled water.

(a) Which is the equation for this reaction?
(1)
A Ca + H2O → CaO + H2

B Ca + 2H2O → CaO2 + 2H2

C Ca + H2O → CaOH + ½H2
D Ca + 2H2O → Ca(OH)2 + H2

(b) Which element is oxidised and which is reduced when calcium reacts with water?
(1)

Element oxidised Element reduced

A calcium hydrogen

B calcium oxygen

C hydrogen calcium

D hydrogen oxygen

(Total for Question 5 = 2 marks)

6 Which is the ionic equation for the reaction of solid barium carbonate with
dilute hydrochloric acid?

A BaCO3(s) + 2H+(aq) → Ba2+(aq) + CO2(g) + H2O(l)

B Ba2CO3(s) + 2H+(aq) → 2Ba+(aq) + CO2(g) + H2O(l)

C CO32−(s) + 2H+(aq) → CO2(g) + H2O(l)

D CO32−(s) + 2HCl(aq) → 2Cl−(aq) + CO2(g) + H2O(l)

(Total for Question 6 = 1 mark)

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*P70965A0328* Turn over
7 The presence of ammonium ions in a compound can be shown by adding a reagent,
warming the mixture and testing the gas evolved.
What is the reagent and the result of the test for the gas evolved?

Reagent Result of test for gas

A HCl(aq) damp blue litmus paper turns red

B HCl(aq) damp red litmus paper turns blue

C NaOH(aq) damp blue litmus paper turns red

D NaOH(aq) damp red litmus paper turns blue

(Total for Question 7 = 1 mark)

8 Aqueous chlorine is added to an aqueous solution of potassium iodide.

A non-polar organic solvent is then added and the mixture is shaken.
The layers are allowed to separate.
What colour is seen in the organic layer?

A brown

B green
C orange

D violet

(Total for Question 8 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

4
*P70965A0428*
9 A titration is carried out by adding dilute sulfuric acid from a burette to
aqueous sodium hydroxide in a conical flask. The indicator is methyl orange.
(a) What is the colour change of the indicator at the end-point of this titration?
(1)
A red to orange
B red to yellow

C yellow to orange

D yellow to red

(b) A student carried out the first titration and did not notice that there was an
air bubble between the tap and the tip of the burette.
During the titration, the air bubble filled with acid.
The student then carried out two accurate titrations in which there was
no air bubble in the burette. There were no other errors in these titrations.
Which of these could be the three titres for this student?
(1)
First titre / cm3 Second titre / cm3 Third titre / cm3

A 22.65 22.65 22.65

B 22.65 22.35 23.25

C 22.80 22.35 22.40

D 22.80 23.25 23.30

2NaOH(aq) + H2SO4(aq) → Na2SO4(aq) + 2H2O(l)

What is the concentration, in mol dm−3 , of the sulfuric acid?

(1)
A 0.0374

B 0.0668

C 0.134

D 0.267

(Total for Question 9 = 3 marks)

5
*P70965A0528* Turn over
10 Hydrogen peroxide decomposes as shown.

2H2O2(aq) → 2H2O(l) + O2(g)

(a) A catalyst increases the rate of decomposition by

(1)

A increasing the average kinetic energy of the H2O2 molecules

B decreasing the average kinetic energy of the H2O2 molecules

C increasing the activation energy of the reaction

D decreasing the activation energy of the reaction

(b) A bottle of hydrogen peroxide is labelled as ‘10 volume’.

This means that 1 cm3 of hydrogen peroxide solution decomposes to produce
10 cm3 oxygen at room temperature and pressure (r.t.p.).
What is the concentration of 10 volume hydrogen peroxide, in mol dm−3 ?

2H2O2(aq) → 2H2O(l) + O2(g)

[Molar volume of gas at r.t.p. = 24 000 cm3 mol−1]

(1)
A 0.100

B 0.208
C 0.417
D 0.833

(Total for Question 10 = 2 marks)

Use this space for any rough working. Anything you write in this space will gain no credit.

6
*P70965A0628*
11 A mixture of hydrogen and iodine is left in a sealed container at 300 °C until
equilibrium is established.

H2(g) + I2(g)  2HI(g)

The equilibrium mixture is then cooled and the colour of the mixture darkens.
Which is correct?

Change in position of
Enthalpy change of
equilibrium when the
forward reaction
system is cooled
A left endothermic

B left exothermic

C right endothermic

D right exothermic

(Total for Question 11 = 1 mark)

12 The structure of ethylamine is shown.

H H
δ+ δ−
H C C NH2

H H

What type of reagent will attack the Cδ+ atom?

A electrophile
B free radical

C nucleophile
D oxidising agent

(Total for Question 12 = 1 mark)

Use this space for any rough working. Anything you write in this space will gain no credit.

7
*P70965A0728* Turn over
13 Which of these alcohols will produce a carboxylic acid when heated under reflux with
acidified potassium dichromate(VI)?

P Q

OH OH

R S
OH OH

A P only
B P and Q only
C P, Q and R only
D P, Q, R and S

(Total for Question 13 = 1 mark)

14 Two reactions of cyclohexanol are shown.

OH O
Reaction 1 Reaction 2

cyclohexene cyclohexanol cyclohexanone

(a) What is the reagent for Reaction 1?

(1)
A acidified potassium manganate(VII)

B aqueous bromine

C concentrated phosphoric(V) acid

D phosphorus(V) chloride

8
*P70965A0828*
(b) The reagent for Reaction 2 is acidified potassium dichromate(VI).
Which equation best represents this reaction?
(1)
A C6H11OH → C6H10O + H2
B C6H11OH → C6H10O + 2[H]

C C6H11OH + [O] → C6H10O + H2O

D C6H11OH + ½O2 → C6H10O + H2O

(c) Cyclohexanol and cyclohexene each has a peak in their infrared spectrum which
is not present for the other compound.
Which are these peaks?
(1)
Peak only in cyclohexanol Peak only in cyclohexene
/ cm−1 / cm−1
A 2962-2853 1669-1645

B 2962-2953 1720-1700

C 3750-3200 1669-1645

D 3750-3200 1720-1700

(Total for Question 14 = 3 marks)

TOTAL FOR SECTION A = 20 MARKS

9
*P70965A0928* Turn over
SECTION B
Answer ALL the questions. Write your answers in the spaces provided.
15 This question is about calcium carbonate, CaCO3 .
(a) Calcium carbonate decomposes on heating.

CaCO3(s) → CaO(s) + CO2(g)

Explain why calcium carbonate decomposes at a higher temperature than

magnesium carbonate, in terms of the charge and size of the cations.
(3)

10
*P70965A01028*
(b) Calcium carbonate reacts with dilute hydrochloric acid.

CaCO3(s) + 2HCl(aq) → CaCl2(aq) + CO2(g) + H2O(l)

A student determines the initial rate of this reaction by collecting the

carbon dioxide in a gas syringe and measuring the volume at regular
time intervals.
(i) The gas syringe can measure a maximum of 100 cm3 of gas.
Calculate the maximum volume of 0.500 mol dm−3 hydrochloric acid that
can be added to excess calcium carbonate at room temperature and
pressure (r.t.p.) without exceeding the measurable volume of the gas syringe.
[Molar volume of gas at r.t.p. = 24 000 cm3 mol−1]
(3)

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(ii) The results of the student’s experiment are shown on the graph.

100

60
Volume of CO2
/ cm3
40

0
0 120 240 360 480 600

Time / s

Calculate the initial rate of this reaction.

You must show your working on the graph.
Include units in your answer.
(3)

(iii) The student repeats the experiment but uses hydrochloric acid with a
concentration of 0.250 mol dm−3 . All other variables are kept the same.
State what would happen to the initial rate of reaction and the final volume of
carbon dioxide collected.
(1)
Initial rate of reaction

Final volume of carbon dioxide collected

(Total for Question 15 = 10 marks)

12
*P70965A01228*
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13
*P70965A01328* Turn over
16 This question is about the halogens and some of their compounds.
(a) Descending the group from fluorine to iodine, the electronegativity of the atoms
decreases even though their nuclear charge increases.
Explain the trend in electronegativity.
(2)

(b) Iodate(V) ions, IO3− , react with iodide ions in acid solution.

IO3− + 5I− + 6H+ → 3I2 + 3H2O

Explain, in terms of the oxidation numbers of iodine in the three species, why this
is not a disproportionation reaction.
(2)

(c) Hydrogen bromide and hydrogen iodide reduce sulfuric acid.

Identify, by name or formula, the compound produced containing sulfur with its
lowest oxidation number in that reaction.
(1)

Compound produced with the lowest

Hydrogen halide
oxidation number of sulfur

HBr

14
*P70965A01428*
(d) The graph shows the boiling temperatures of the hydrogen halides.

350

300

250

200
Boiling temperature
/K 150

100

0
HF HCl HBr HI

Explain the trend in the boiling temperatures of the hydrogen halides.

(4)

15
*P70965A01528* Turn over
(e) A sample of seawater was evaporated to dryness.
The solid residue was weighed, then dissolved completely in deionised water.
Excess aqueous silver nitrate was added to the solution.
All the chloride ions in the seawater formed a precipitate of silver chloride.

Ag+(aq) + Cl−(aq) → AgCl(s)

The precipitate was filtered, washed, dried and weighed.

Results:
Mass of solid residue from seawater = 0.098 g
Mass of silver chloride precipitate = 0.226 g
Calculate the percentage, by mass, of chloride ions in the solid residue.
[Assume silver chloride is the only precipitate.]
(3)

(Total for Question 16 = 12 marks)

16
*P70965A01628*
17 This question is about some halogenoalkanes.
(a) Give the classification of each halogenoalkane shown in the table as primary,
secondary or tertiary.
(1)

Halogenoalkane Classification

(b) Samples of 1-iodobutane and 2-chloro-2-methylpropane were hydrolysed using

aqueous silver nitrate in ethanol.
Explain whether or not it is possible to predict the relative rate of hydrolysis of
these two compounds.
(3)

17
 *P70965A01728* Turn over
(c) Butylamine is formed when 1-bromobutane reacts with
excess concentrated alcoholic ammonia.

CH3CH2CH2CH2Br + 2NH3 → CH3CH2CH2CH2NH2 + NH4Br

(i) Give a reason why this reaction should be carried out by heating the reactants
in a sealed tube rather than heating under reflux.
(1)

(ii) Complete the mechanism for this reaction by adding curly arrows, and any
relevant lone pairs and dipoles.
(4)

C3H7 H C3H7

H C Br H N+ C H + Br−

H H H
H3N H3N

H C3H7

N C H + NH4+

H H

18
*P70965A01828* 
(d) Bromoethane is prepared by reacting ethanol with potassium bromide and
concentrated sulfuric acid.

C2H5OH + KBr + H2SO4 → C2H5Br + KHSO4 + H2O

Calculate the maximum mass of bromoethane that could be prepared from

4.65 g of ethanol, 14.90 g of potassium bromide and a solution containing
16.35 g of H2SO4 .

[Ar values: H = 1.0 C = 12.0 O = 16.0 S = 32.1 K = 39.1 Br = 79.9]

(3)

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*(e) The reaction between 2-bromopropane and potassium hydroxide takes place
under two different conditions:
• in aqueous solution
• in ethanolic solution.
Compare and contrast these two reactions.
Include equations for the reactions.
Detailed mechanisms of these reactions are not required.
(6)

20
*P70965A02028* 
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(Total for Question 17 = 18 marks)

TOTAL FOR SECTION B = 40 MARKS

21
 *P70965A02128* Turn over
SECTION C
Answer ALL the questions. Write your answers in the spaces provided.
18
Fuels
Fuels burn in oxygen to release a lot of energy.
Many hydrocarbons and alcohols are used as fuels. During complete combustion,
they produce carbon dioxide and water.
Petrol contains 2,2,4-trimethylpentane, an isomer of octane, that promotes
smooth combustion.

2,2,4-trimethylpentane

Alcohols, such as methanol and ethanol, can be used as fuels either on their own or
as additives in petrol.

(a) The standard enthalpy change of combustion, ΔcH d , of 2,2,4-trimethylpentane

is −5461 kJ mol−1 .
(i) State the two standard conditions for this enthalpy change.
(1)

(ii) Write the equation for the complete combustion of 2,2,4-trimethylpentane,

using molecular formulae.
State symbols are not required.
(2)

22
*P70965A02228* 
(iii) Draw a labelled enthalpy level diagram for the complete combustion of
2,2,4-trimethylpentane.
(2)

(iv) Calculate the heat energy released during the complete combustion of
1 dm3 of 2,2,4-trimethylpentane.
[Density of 2,2,4-trimethylpentane = 0.692 g cm−3 ]
(3)

23
 *P70965A02328* Turn over
(b) In an experiment to determine the enthalpy change of combustion of
ethanol, C2H5OH, a student used the apparatus shown.

thermometer

beaker
clamp

water

wick burner

ethanol

Results:
Mass of water = 100.0 g
Mass of ethanol used = 0.305 g
Temperature rise of water = 13.2 °C
(i) Calculate the enthalpy change of combustion of ethanol.
Give your answer to an appropriate number of significant figures, and include
a sign and units.
[Specific heat capacity of water = 4.18 J g−1 °C−1 ]
(4)

24
*P70965A02428* 
(ii) The uncertainty in each thermometer reading is ±0.05 °C.
Calculate the percentage uncertainty in the temperature rise in
this experiment.
(1)

(iii) The student looked in a data book and found the actual value for the
standard enthalpy change of combustion of ethanol was more exothermic
than the experimental value obtained.
Give two reasons for the difference between the data book value and the
experimental value, other than referring to standard conditions.
(2)

25
 *P70965A02528* Turn over
(c) The enthalpy changes for the conversion of four compounds in the gas phase into
their constituent atoms are shown.
H2O(g) → 2H(g) + O(g) ΔrH = +928 kJ mol−1
CH4(g) → C(g) + 4H(g) ΔrH = +1740 kJ mol−1
CH3OH(g) → C(g) + 4H(g) + O(g) ΔrH = +2105 kJ mol−1
C2H5OH(g) → 2C(g) + 6H(g) + O(g) ΔrH = +3322 kJ mol−1
Calculate the bond enthalpy of the C C bond, in kJ mol−1 .
You must show your working.
(3)

26
*P70965A02628* 
(d) Ethanol can be manufactured by reacting ethene with steam.

C2H4(g) + H2O(g)  C2H5OH(g) ΔrH = −45 kJ mol−1

This reaction is usually carried out in industry at 300 °C and 70 atm pressure using
a catalyst.
Explain the effect on the equilibrium position and the equilibrium yield of ethanol
if the reaction is carried out at 300 °C and 200 atm pressure.
(2)

(Total for Question 18 = 20 marks)

TOTAL FOR SECTION C = 20 MARKS

TOTAL FOR PAPER = 80 MARKS

27
 *P70965A02728*
28
*P70965A02828* 

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