Please check the examination details below before entering your candidate information

Candidate surname Other names

Centre Number Candidate Number

Pearson Edexcel International GCSE

Tuesday 12 November 2024
Paper
Morning (Time: 2 hours)
reference 4CH1/1C 4SD0/1C
Chemistry  

UNIT: 4CH1
Science (Double Award) 4SD0
PAPER: 1C
You must have: Total Marks
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.
• Show all the steps in any calculations and state the units.
Information
•• The total mark for this paper is 110.
The marks for each question are shown in brackets
– use this as a guide as to how much time to spend on each question.

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

P75946A
©2024 Pearson Education Ltd.
V:1/1/1/1/1/1/1/
*P75946A0132*
 2
2
The Periodic Table of the Elements
1 2 3 4 5 6 7 0
1 4
H He
hydrogen helium

Key 1 2

7 9 relative atomic mass 11 12 14 16 19 20

Li Be atomic symbol B C N O F Ne
lithium beryllium name boron carbon nitrogen oxygen fluorine neon
3 4 atomic (proton) number 5 6 7 8 9 10

23 24 27 28 31 32 35.5 40
Na Mg Al Si P S Cl Ar
sodium magnesium aluminium silicon phosphorus sulfur chlorine argon
11 12 13 14 15 16 17 18

39 40 45 48 51 52 55 56 59 59 63.5 65 70 73 75 79 80 84
K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
potassium calcium scandium titanium vanadium chromium manganese iron cobalt nickel copper zinc gallium germanium arsenic selenium bromine krypton
19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36

85 88 89 91 93 96 [98] 101 103 106 108 112 115 119 122 128 127 131
Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe
rubidium strontium yttrium zirconium niobium molybdenum technetium ruthenium rhodium palladium silver cadmium indium tin antimony tellurium iodine xenon
37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54

133 137 139 178 181 184 186 190 192 195 197 201 204 207 209 [209] [210] [222]
Cs Ba La* Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
caesium barium lanthanum hafnium tantalum tungsten rhenium osmium iridium platinum gold mercury thallium lead bismuth polonium astatine radon

*P75820A0224*
*P75946A0232*
55 56 57 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86

[223] [226] [227] [261] [262] [266] [264] [277] [268] [271] [272]
Fr Ra Ac* Rf Db Sg Bh Hs Mt Ds Rg Elements with atomic numbers 112–116 have been reported but not fully
francium radium actinium rutherfordium dubnium seaborgium bohrium hassium meitnerium darmstadtium roentgenium
authenticated
87 88 89 104 105 106 107 108 109 110 111

* The lanthanoids (atomic numbers 58–71) and the actinoids (atomic numbers 90–103) have been omitted.

The relative atomic masses of copper and chlorine have not been rounded to the nearest whole number.

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 Answer ALL questions.
Some questions must be answered with a cross in a box . If you change your mind about an

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answer, put a line through the box and then mark your new answer with a cross .
1 The three states of matter are solid, liquid and gas.
(a) Substances can change from one state to another.
The box gives some words about changes of state.

condensing cooling evaporation

freezing heating melting sublimation

Complete the table by giving the correct word from the box for each change
of state.
You may use each word once, more than once or not at all.
(3)

Change of state Name of change

from liquid to solid

from gas to liquid

from solid to gas

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*P75946A0432* 
 (b) The diagram shows two states of matter for a substance.
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solid liquid gas

Each circle represents an atom of the substance.

(i) Complete the diagram by drawing six circles to represent atoms in the
gas state.
(1)

(ii) Which statement is correct about this substance?

(1)
A the atoms move randomly in the gas state

B the atoms move randomly in the solid state

C the atoms are in fixed positions in the gas state

D the atoms are in fixed positions in the liquid state

(c) Complete the equation, by adding the state symbols, for the conversion of water
into ice.
(1)

H2O(. . . ............................ ) → H2O(............................... )

(Total for Question 1 = 6 marks)

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2 The table gives some information about five gases.

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Name Formula Boiling point in °C

chlorine Cl2 –35

hydrogen chloride HCl –114

oxygen O2 –183

nitrogen N2 –196

hydrogen H2 –253

(a) Use gases from the table to answer these questions.

You may use each gas once, more than once or not at all.
(i) Name the gas needed for combustion.
(1)

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(ii) Name the gas that is most abundant in air.

(1)

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(iii) Name the gas that can bleach damp litmus paper.
(1)

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(b) Explain why hydrogen chloride is classified as a compound.

(2)

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*P75946A0632* 
 (c) Why does chlorine have the highest boiling point of the gases in the table?
(1)
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A chlorine has the strongest covalent bonds between its atoms

B chlorine has the strongest covalent bonds between its molecules

C chlorine has the strongest ionic bonds between its atoms

D chlorine has the strongest forces of attraction between its molecules

(Total for Question 2 = 6 marks)

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3 This question is about the rusting of iron.
(a) (i) Name the two substances needed for iron to rust.

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(2)

1 ............................ . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . ............................................................................................................................................ . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

2 ............................ . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . ............................................................................................................................................ . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

(ii) Give the chemical name for rust.

(1)

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(b) The diagram shows two methods used to prevent iron from rusting.

iron iron
paint zinc

Method A Method B

Method A will work only if the paint coating is not scratched.

Method B will work even if the zinc coating is scratched.
(i) Explain how method A prevents iron from rusting.
(2)

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(ii) Give the name of method B.

(1)

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*P75946A0832* 
 (iii) Explain how method B prevents iron from rusting even when the zinc coating
is scratched.
(2)
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(Total for Question 3 = 8 marks)

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*P75946A01032*
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10
 4 A student does an experiment to identify the dyes in inks A, B, C, D and E.
The student uses this apparatus.
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• a piece of chromatography paper

• a beaker
• a solvent
• inks A, B, C, D and E
(a) Describe how the student should set up the apparatus and do the experiment.
You may use a diagram to help your answer.
(5)

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 (b) The chromatogram shows the results for inks A, B, C, D and E.

solvent front

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A B C D E

(i) Explain which ink contains a dye that is insoluble in the solvent.
(2)

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

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

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

(ii) Explain which inks contain the same dye.

(2)

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*P75946A01232* 
 (iii) Describe how the student can use the chromatogram to determine the
Rf value for the dye in ink C.
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You do not need to calculate the Rf value.

(2)

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

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

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

(Total for Question 4 = 11 marks)

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
*P75946A01432*
BLANK PAGE

14
 5 Hydrogen peroxide decomposes to form water and oxygen.
This decomposition is shown in the equation.
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2H2O2 → 2H2O + O2

(a) Give the test for oxygen gas.

(1)

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

(b) The rate of reaction is increased by adding a suitable catalyst.

Describe how a catalyst increases the rate of a reaction.
(2)

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(c) A student uses this apparatus to investigate the rate of decomposition of

hydrogen peroxide solution.

hydrogen peroxide
solution
0 20 40 60 80 100 cm3

oxygen
B

catalyst

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 The student adds 100 cm3 of hydrogen peroxide solution at 20 °C to the apparatus
labelled A.

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The student records the volume of oxygen gas collected every minute for
16 minutes.
The graph shows the student’s results.

100

80

60
Volume of oxygen
in cm3
40

20

0
0 4 8 12 16
Time in minutes

(i) Name the pieces of apparatus labelled A and B.

(2)

A ............................ . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . ............................................................................................................................................ . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

B ............................ . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . ........................................................................................................................................... . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

(ii) Determine the volume of oxygen gas produced in the first 4 minutes.
Show on the graph how you obtain your answer.
(2)

volume of oxygen = ..................................... . . . . . . . . . . . . . . . . . . . . . . . . . cm3

16
*P75946A01632* 
 (iii) Determine the rate of reaction at 8 minutes by drawing a suitable tangent to
the curve.
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Include the units for the rate of reaction.

(4)

rate of reaction = .............................................................. units . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

(Total for Question 5 = 11 marks)

17
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6 This question is about ionic and covalent compounds.
(a) The table gives the formulae of some positive ions, some negative ions and some

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compounds containing these ions.

NH+4 Zn2+ Al3+

Cl– NH4Cl ZnCl2

SO42– (NH4)2SO4 Al2(SO4)3

N3– Zn3N2 AlN

(i) Complete the table by giving the three missing formulae.

(3)
(ii) Give the name of the compound with the formula Al2(SO4)3
(1)

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

(b) The diagram shows the arrangement of electrons in an atom of magnesium and
an atom of chlorine.

Magnesium Chlorine

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*P75946A01832* 
 Describe, in terms of electrons, what happens when magnesium atoms and
chlorine atoms form magnesium chloride.
(3)
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................................ . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . ............................................................................................................................................ . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

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

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

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

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

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

(c) (i) Complete the dot-and-cross diagram to show the outer shell electrons in a
molecule of ammonia.
(2)

N H
H

(ii) Describe the forces of attraction in a covalent bond.

(2)

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

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

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

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

(Total for Question 6 = 11 marks)

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7 Magnesium sulfate crystals have the formula MgSO4.xH2O
A student uses this apparatus to heat tube A and collect water of crystallisation in

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tube B.

magnesium sulfate
crystals tube A

tube B

heat

ice
water

The student records the mass of tube B at the start and every minute for 6 minutes.
The table gives the student’s results.

Time in minutes Mass of tube B in g

0 15.8

1 16.5

2 17.6

3 19.2

4 20.4

5 22.1

6 22.1

(a) (i) Give a reason why the student surrounds tube B with ice.
(1)

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(ii) State how the student knows when all the water of crystallisation has been
given off.
(1)

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*P75946A02032* 
 (b) Describe a chemical test the student can use to show that the liquid in tube B
contains water.
(2)
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................................ . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . ............................................................................................................................................ . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

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

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

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

(c) The decomposition of hydrated magnesium sulfate is shown in the equation.

MgSO4.xH2O → MgSO4 + xH2O

At the end of the reaction, the mass of MgSO4 remaining in the tube is 6.0 g.

Use this mass and the results in the table to calculate x in MgSO4.xH2O
[for MgSO4 , Mr = 120 for H2O, Mr = 18]
(4)

x = ......................... . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .
(Total for Question 7 = 8 marks)

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8 A student uses this apparatus to investigate the rate of reaction between marble chips
and dilute hydrochloric acid.

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cotton wool

dilute hydrochloric acid

marble chips

balance
g

This is the equation for the reaction.

CaCO3(s) + 2HCl(aq) → CaCl2(aq) + H2O(l) + CO2(g)

(a) Give a reason why the reading on the balance decreases during the reaction.
(1)

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

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(b) Explain why the rate of reaction is greatest at the start.

(2)

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(c) After 10 minutes, the reaction stops even though there are marble chips remaining.
Give a reason why the reaction stops.
(1)

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22
*P75946A02232* 
 (d) The student repeats the experiment with hydrochloric acid at a higher
temperature to investigate the effect on the rate of reaction.
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(i) Give two variables that should be controlled to make sure the results are valid.
(2)

1 ............................ . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . ............................................................................................................................................ . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

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

2 ............................ . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . ............................................................................................................................................ . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

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

(ii) Explain the effect of increasing the temperature of hydrochloric acid on the
rate of reaction.
(3)

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

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

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

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

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

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

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

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

(Total for Question 8 = 9 marks)

23
 *P75946A02332* Turn over
9 A student uses this apparatus to investigate the heat energy released when a liquid
fuel burns.

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thermometer

aluminium can

water

spirit burner
liquid fuel

This is the student’s method.

• measure the mass of the spirit burner and fuel
• add 100 g of water to the aluminium can
• measure the temperature of the water
• use the spirit burner to heat the water until the temperature rises by 50 °C
• measure the new mass of the spirit burner and fuel
(a) Give a reason why the student uses an aluminium can rather than a glass beaker.
(1)

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

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

(b) When the fuel burns, a black solid forms on the aluminium can.
(i) Identify the black solid.
(1)

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(ii) Give a reason why the black solid forms.

(1)

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

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

24
*P75946A02432* 
 (c) (i) Show that the heat energy needed to raise the temperature of 100 g of water
by 50 °C is approximately 20 000 J.
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[for water, c = 4.2 J/g/°C]

(2)

(ii) The student burns 1.84 g of ethanol.

Calculate the molar enthalpy change, ΔH, in kJ/mol, for the combustion
of ethanol.
Include a sign in your answer.
[for ethanol, Mr = 46]
(4)

ΔH = ............................................. . . . . . . . . . . . . . . . . . kJ/mol

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 *P75946A02532* Turn over
 (d) In a different experiment, the student burns 3.7 g of butanol.
This is an equation for the incomplete combustion of butanol.

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C4H9OH(l) + . . . . . . . . . . . . . . . . ............... O2(g) → 2CO2(g) + 2CO(g) + 5H2O(g)

(i) Complete the equation for the incomplete combustion of butanol.

(1)
(ii) Calculate the total amount, in moles, of gas produced by the incomplete
combustion of 3.7 g of butanol.
(3)

amount of gas = ..................................... . . . . . . . . . . . . . . . . . . . . . . . . . mol

(Total for Question 9 = 13 marks)

26
*P75946A02632* 
 10 This question is about alkanes and alkenes.
(a) Ethane and ethene each react with bromine, but under different conditions.
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(i) Give a reason why ethane does not undergo an addition reaction
with bromine.
(1)

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

(ii) Complete the equation for the substitution reaction between ethane and
bromine, including an essential condition for the reaction.
(2)

C2H6 + Br2 → ............................... + ...............................

condition

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

(iii) Give the colour change that occurs when ethene reacts with bromine water.
(1)

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

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 *P75946A02732* Turn over
 (b) The diagram shows the displayed formulae of two compounds in the
homologous series of alkenes.

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H H H H H H H H

C C C C H H C C C C H

H H H H H

(i) Compounds in the same homologous series have the same general formula.
Give two other characteristics of compounds in the same homologous series.
(2)

1 ............................ . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . ............................................................................................................................................ . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

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

2 ............................ . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . ............................................................................................................................................ . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

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

(ii) Explain why the alkenes in the diagram are isomers.

(2)

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

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

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

(iii) Draw the displayed formula of another alkene that is an isomer of these
two alkenes.
(1)

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*P75946A02832* 
 (c) The reaction used to make poly(ethene) can be represented by this equation.

( (
H H
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H H
n C C C C
H H H H n

Describe the differences between the reactant and the product in this reaction.
Refer to carbon chain length, type of bond and state of matter in your answer.
(3)

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

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

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

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

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

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

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

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

(Total for Question 10 = 12 marks)

29
 *P75946A02932* Turn over
11 This question is about the reactions of some compounds of lead.
(a) Lead can be extracted from lead(II) sulfide, PbS, in two stages.

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Stage 1 lead(II) sulfide is heated in air and reacts with oxygen to produce
lead(II) oxide, PbO, and sulfur dioxide
Stage 2 lead(II) oxide is heated with carbon in a furnace

(i) Write a chemical equation for the reaction in stage 1.

(2)

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(ii) Give a reason why sulfur dioxide should not be released into the atmosphere.
(1)

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

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

(iii) This is the equation for stage 2.

2PbO + C → 2Pb + CO2

A mass of 892 tonnes of lead(II) oxide is heated in a furnace with an excess

of carbon.
Calculate the maximum mass, in tonnes, of carbon dioxide that could be
released into the atmosphere.
[1 tonne = 1 × 106 g]
[for PbO, Mr = 223 for CO2 , Mr = 44]
(3)

mass = ............................................. . . . . . . . . . . . . . . . . . tonnes

30
*P75946A03032* 
 (iv) The diagram shows the structures of lead(II) sulfide and sulfur dioxide.
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Lead(II) sulfide Sulfur dioxide

Explain, in terms of bonding and structure, why lead(II) sulfide is a solid with a
very high melting point at room temperature and why sulfur dioxide is a gas
at room temperature.
(5)
lead(II) sulfide

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

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

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

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

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

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

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

sulfur dioxide

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

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

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

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

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

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

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

QUESTION 11 CONTINUES ON NEXT / BACK PAGE.

31
 *P75946A03132* Turn over
 (b) A different oxide of lead contains 90.7% by mass of lead and 9.3% by mass
of oxygen.

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Determine the empirical formula of this oxide of lead.
(4)

empirical formula = ......................... . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

(Total for Question 11 = 15 marks)

TOTAL FOR PAPER = 110 MARKS

32
*P75946A03232* 