NATIONAL SENIOR CERTIFICATE EXAMINATION

NOVEMBER 2017

PHYSICAL SCIENCES: PAPER II

Time: 3 hours 200 marks

PLEASE READ THE FOLLOWING INSTRUCTIONS CAREFULLY

1. This question paper consists of 19 pages, a yellow Answer Sheet of 2 pages (i–ii)
and a green Data Sheet of 3 pages (i–iii). Please make sure that your question
paper is complete.

2. Remove the Data Sheet and Answer Sheet from the middle of this question paper.
Write your examination number on the yellow Answer Sheet.

3. Read the questions carefully.

4. ALL of the questions in this paper must be answered.

5. Question 1 consists of 10 multiple-choice questions. There is only one correct

answer to each question. The questions are to be answered on the Answer Sheet
provided on the inside cover of your Answer Book. The letter that corresponds with
your choice of the correct answer must be marked with a cross as shown in the
example below:

A B C D Here the answer C has been marked.

6. START EACH QUESTION ON A NEW PAGE.

7. Please ensure that you number your answers as the questions are numbered.

8. Unless instructed otherwise it is NOT necessary to give state symbols (phase

indicators) when asked to write a balanced chemical equation.

9. Use the data and formulae whenever necessary.

10. Show all the necessary steps in calculations.

11. Where appropriate take your answers to 2 decimal places.

12. It is in your own interest to write legibly and to present your work neatly.

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QUESTION 1 MULTIPLE CHOICE

Answer these questions on the multiple-choice Answer Sheet on the inside front
cover of your Answer Book. Make a cross (X) in the box corresponding to the letter
representing the answer that you consider to be the most correct.

1.1 The chemical formula for aluminium hydrogen sulphate is:

A Aℓ(HSO4)3
B Aℓ3H2SO4
C Aℓ2(HSO4)3
D Aℓ2H2(SO4)3

1.2 Which one of the following gives the number of methane molecules in 12 g
of CH4(g)?

16 × 6,02 ×1023
A
12
12
B
16 × 6,02 ×1023
16
C
12 × 6,02 ×1023

12 × 6,02 ×1023
D
16

1.3 A violet coloured solution is prepared by dissolving cobalt chloride crystals

in a mixture of ethanol and water. This violet colour is due to two different
coloured cobalt (II) complex ions existing together in equilibrium in the
solution as shown in the balanced chemical equation:

CoCℓ42- + 6H2O Co(H2O)62+ + 4Cℓ- ∆H < 0

BLUE PINK

What colour change will be observed when a few drops of concentrated

HCℓ are added to 1 cm3 of the violet solution?

A The solution turns colourless

B The solution turns blue
C The solution turns pink
D No colour change

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1.4 Hydrogen gas and iodine gas are introduced into a flask, which is then
sealed and allowed to reach dynamic chemical equilibrium. The balanced
chemical equation for the reaction is:

H2(g) + I2(g) 2HI(g)

Which one of the following graphs shows how the rates of the forward and
reverse reactions change with time?

1.5 Which one of the following gives the approximate pH of an aqueous solution
of ammonium chloride and the relevant hydrolysis equation?

pH Hydrolysis equation
A Greater than 7 NH4+ + H2O NH3 + H3O+
B Less than 7 NH4+ + H2O NH3 + H3O+
C Greater than 7 Cℓ – + H2O HCℓ + OH–
D Less than 7 Cℓ – + H2O HCℓ + OH–

1.6 A table of acid-base indicators and the pH ranges over which they change
colour is shown below. Which one of these indicators is most suitable for
use in the titration of hydrochloric acid with sodium hydroxide?

Indicator pH range
A Bromophenol blue 3,0– 4,6
B Litmus 4,5–8,3
C Bromothymol blue 6,0–7,6
D Cresolphthalein 8,2–9,8

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1.7 Which one of the following redox reactions is NON-SPONTANEOUS under

standard conditions?

A 2I–(aq) + 2Ag+(aq) I2(s) + 2Ag(s)

B Pb2+(aq) + Cu(aq) Cu2+(aq) + Pb(s)
C Pb2+(aq) + Ni(s) Pb(s ) + Ni2+(aq)
D 2Ag(s) + Cℓ2(g) 2Cℓ –(aq) + 2Ag+(aq)

1.8 The diagram below represents a cell used in the electroplating of a wedding
ring with silver metal.

How does the mass of the pure silver electrode and the concentration of the
AgNO3 electrolyte change during electrolysis?

Mass of silver electrode Concentration of AgNO3 electrolyte

A Decreases Increases
B Increases No change
C Decreases No change
D Increases Decreases

1.9 Which of the following statements would apply to organic compounds that
belong to the same homologous series?

I They have the same boiling points.

II They have the same functional group.
III They have the same molecular formula.

A II only
B I and II only
C II and III only
D I, II and III

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1.10 The organic compounds shown in the table below all have the same molar
mass (60 gmol–1).

Structural formula of compound Boiling point (oC)

X 97

Y ?

Z 32

Which one of the following is most likely to be the boiling point (in °C) of
compound Y?

A 24
B 40
C 90
D 118
[20]

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QUESTION 2 CHEMICAL BONDING

2.1 Define a covalent bond. (2)

2.2 State the difference between a non-polar covalent bond and a polar
covalent bond. (2)

2.3 The following table contains eight substances.

graphite hydrogen fluoride aluminium oxide argon

chlorine hydrogen chloride magnesium hydrogen

Select substances from this table when answering each of the following
questions.

Identify:

2.3.1 a molecular substance with non-polar covalent bonds. (1)

2.3.2 a molecular substance with polar covalent bonds. (1)

2.3.3 a substance with ionic bonding. (1)

2.3.4 a substance which has hydrogen bonding intermolecular forces. (1)

2.3.5 a different substance to that given in Question 2.3.4 which has

dipole-dipole intermolecular forces. (1)

2.3.6 a substance which has London forces between its atoms. (1)

2.3.7 a substance which consists of positive atomic kernels surrounded by

a sea of delocalised electrons. (1)

2.3.8 a substance which has a giant network structure in which the atoms
are held together by covalent bonds. (1)
[12]

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QUESTION 3 ENERGY CHANGE

Ammonia is prepared in industry by means of the Haber process. The balanced

chemical equation for the reaction is given below.

N2(g) + 3H2(g) 2NH3(g) ΔH = – 92,4 kJmol–1

The activation energy for this reaction is 242,6 kJmol–1.

3.1 Define the following terms:

3.1.1 Activation energy. (2)

3.1.2 Catalyst. (2)

3.2 Calculate the activation energy for the REVERSE reaction. (2)

3.3 A learner incorrectly states:

"A catalyst lowers the activation energy which results in more collisions
taking place per second."

Explain why this statement is incorrect. (2)

3.4 The following table shows two catalysts that can be used for this reaction
and their corresponding activation energies.

Catalyst Activation energy (kJmol–1)

Platinum catalyst 70,6
Osmium catalyst 104,6

Which catalyst, platinum or osmium, will be most effective for this reaction?
Explain. (4)
[12]

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QUESTION 4 RATES OF REACTION

Two experiments were conducted to investigate the rate of reaction between

EXCESS calcium carbonate and dilute hydrochloric acid. The balanced chemical
equation for the reaction is given below.

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

The diagrams show the reaction conditions used in each experiment.

4.1 Suggest a suitable method of measuring the rates of the reactions in these
experiments. Additional apparatus besides that shown in the diagrams may
be used. State what apparatus is required and what reading(s) would need
to be taken. (3)

4.2 Identify the independent variable in Experiment 1. (1)

4.3 In Experiment 1, in which flask, W or X, will the reaction rate be faster?

Explain fully. (4)

4.4 Calculate the volume of CO2(g) produced at STP in flask W. (5)

4.5 Consider the reaction conditions given for Experiment 2.

4.5.1 How will the rate of reaction in flask Z compare to that in flask Y?
Choose from GREATER THAN Y, LESS THAN Y or EQUAL TO Y. (1)

4.5.2 It is observed that the total volume of gas produced in flask Z is

greater than that produced in flask Y. Account for this observation. (2)
[16]

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QUESTION 5 CHEMICAL EQUILIBRIUM

The hydrogen gas used in the Haber process is prepared by the reaction of
methane and steam as shown in the following balanced chemical equation.

CH4(g) + H2O(g) CO(g) + 3H2(g) ΔH = +206 kJ

Initially 1,2 moles of methane and 1,4 moles of steam are placed in a closed
container. They react and then dynamic chemical equilibrium is reached at a fixed
temperature. The following graph shows the changes in the number of moles of
methane, steam and carbon monoxide as the reaction proceeds.

5.1 State why there is no change in the number of moles of each of the gases
between times t1 and t2. (2)

5.2 The above graph has been reproduced on your ANSWER SHEET.
On the graph on your ANSWER SHEET:

5.2.1 Draw a line to show the change in the number of moles of hydrogen
gas between t0 and t2. Label this line H2(g). (3)

5.2.2 Draw a dashed line (- - - ) to show how the number of moles of

methane gas would change with time if a catalyst had been added to
the container at time t0. (2)

5.3 Calculate the value of the equilibrium constant, K c , at the fixed temperature
used in this reaction. The volume of the container is 2 dm3. (6)

5.4 What does the K c value indicate about the yield of products? (1)

5.5 State Le Chatelier's principle. (2)

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5.6 How will an increase in pressure affect the yield of hydrogen? Explain. (3)

5.7 How will an increase in pressure affect the equilibrium constant, Kc , for this
reaction?

Choose from INCREASES, DECREASES or NO CHANGE. (1)

5.8 This reaction is carried out in industry at a temperature of 1 000 °C. State
TWO reasons why high temperatures are an advantage. No explanations
are required. (2)
[22]

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QUESTION 6 EXPERIMENTAL SKILLS AND THE AUTO-IONISATION OF

WATER
The balanced chemical equation for the auto-ionisation (autoprotolysis) of water is
given below.
H2O(ℓ) + H2O(ℓ) H3O+(aq) + OH–(aq)

The table below gives the variation of the equilibrium constant of water, Kw, and
the concentration of hydronium ions, [H3O+], with temperature (T).

T (oC) Kw (× 10–14) [H3O +] (× 10–7) (moldm–3)

0 0,114 0,34
10 0,293 0,54
20 0,681 0,83
30 1,47 1,21
40 1,71
50 5,48 2,34

6.1 Calculate the value of Kw at 40 oC. (2)

6.2 Is the auto-ionisation (autoprotolysis) of water EXOTHERMIC or
ENDOTHERMIC? Explain. (3)
6.3 Use the GRAPH PAPER PROVIDED ON YOUR ANSWER SHEET to plot a
graph of concentration of hydronium ions versus temperature. Draw the line
of best fit. (6)
6.4 Use your graph to determine the concentration of hydronium ions, [H3O+] at
a temperature of 45 oC. (Indicate clearly on your graph how you achieved
your answer.) (2)
6.5 A learner draws the following conclusion from the graph:
"The concentration of hydronium ions, [H3O+] is directly proportional to the
temperature of the water."
Give TWO features of the graph which do NOT support this relationship. (2)
6.6 A small amount of NaOH is now added to the water at 25 °C.
How will this affect the:
6.6.1 Kw? (1)
6.6.2 [H3O+]? (1)
Choose from INCREASES, DECREASES or REMAINS THE SAME.
6.7 How will the pH of pure water be affected by increasing the temperature of
the water?
Choose from INCREASES, DECREASES or NO CHANGE. (1)
[18]

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QUESTION 7 ACIDS & BASES

7.1 Define an acid. (1)

7.2 State the difference between a concentrated acid and a strong acid. (2)

7.3 0,1 moldm-3 aqueous solutions of the following compounds are prepared.

HNO3 H2SO4 KCℓ NaHCO3

H3PO4 LiOH HCOOH

Choose from this list a:

7.3.1 Strong base. (1)

7.3.2 Weak polyprotic acid. (1)

7.3.3 Strong monoprotic acid. (1)

7.3.4 Weak monoprotic acid. (1)

7.3.5 Solution with a pH of approximately 8,5. (1)

7.4 Write a balanced chemical equation to show the ionisation of sulphuric acid
in water. (3)

7.5 Katie is given the task of determining the percentage of magnesium oxide in
a health tablet. She dissolves the tablet in 0,05 dm3 of 0,8 moldm-3
hydrochloric acid.

7.5.1 Calculate the number of moles of acid present in 0,05 dm 3 of

0,8 moldm-3 hydrochloric acid solution. (3)

All of the magnesium oxide in the tablet reacts with the hydrochloric acid as
shown in the balanced chemical equation below.

MgO(s) + 2HCℓ(aq)  MgCℓ2(aq) + H2O(ℓ)

Not all of the hydrochloric acid reacts. Katie titrates the excess hydrochloric
acid with a solution of sodium hydroxide. It takes 0,02 dm3 of 0,5 moldm-3
sodium hydroxide to neutralise the excess hydrochloric acid. The
hydrochloric acid and sodium hydroxide react as shown in the balanced
chemical equation below.

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

7.5.2 The original mass of the tablet is 0,96 g. Calculate the percentage of
magnesium oxide in the tablet. (7)
[21]

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QUESTION 8 GALVANIC CELLS

Ayanda and Zoe are given three unknown half-cells I, II and III. The half-reaction
taking place in each half-cell is given below.

Half-cell I X2+(aq) + 2e– X (s)

Half-cell II Y3+(aq) + 3e– Y (s)
Half-cell III Z+(aq) + e– Z (s)

Ayanda and Zoe connect half-cell I to half-cell II under standard conditions and
record the cell potential (Eocell) as well as the metal electrode that acted as the
anode. They then connect half-cell I to half-cell III under standard conditions and
again record the cell potential (Eocell) as well as the metal electrode that acted as
the anode.

The results for the two half-cell combinations are given in the table below.

Cell Combination Eocell (V) Anode

A Half-cell I + Half-cell II 0,84 X
B Half-cell I + Half-cell III 0,68 Z

8.1 Define the following terms:

8.1.1 Anode. (2)

8.1.2 Reducing agent. (1)

8.2 State the energy conversion that takes place in these cells. (1)

8.3 State the standard conditions under which these cells operate. (2)

8.4 Write down the balanced chemical equation for the reaction taking place in
Cell A. (3)

8.5 Write down the symbol of the oxidising agent in Cell A. (1)

8.6 Write down the cell notation for Cell B. Standard conditions and state
symbols do not need to be shown. (3)

8.7 Give the symbol of the chemical species that is reduced in Cell B. (1)

8.8 8.8.1 Which metal, X, Y or Z is the strongest reducing agent? (1)

8.8.2 Which metal, X, Y or Z is the weakest reducing agent? (1)

8.9 Ayanda and Zoe now connect half-cell II to half-cell III, under standard
conditions, to make Cell C. Calculate the cell potential (Eocell) of Cell C.
Show all workings. (3)
[19]

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QUESTION 9 ELECTROLYTIC CELL

Kamo sets up TWO different cells for the electrolysis of sodium chloride as shown
in the diagrams below.

9.1 Explain why Kamo had to either melt or dissolve the solid sodium chloride in
order to electrolyse it in each of the respective cells. (2)

9.2 Give TWO reasons why graphite electrodes are suitable in Cell A. (2)

9.3 Write down the equation for the half-reaction taking place at the:

9.3.1 Anode in Cell A. (2)

9.3.2 Cathode in Cell A. (2)

9.3.3 Cathode in Cell B. (2)

9.4 Give the symbol of the ions which pass through the membrane in Cell B. (1)

9.5 Identify product X in Cell B. (1)

Kamo carries out an investigation to determine how the concentration of the NaCℓ
solution used in Cell B affects the purity of the chlorine gas produced at the anode.
She records her observations in the table below.

Concentration of NaCℓ(aq) Purity of chlorine gas

HIGH (saturated solution) Fairly pure, low contamination with oxygen gas.
LOW (dilute solution) Impure, high contamination with oxygen gas.

9.6 Explain why the chlorine gas produced from a dilute solution of NaCℓ was
highly contaminated with oxygen gas compared to that from the saturated
NaCℓ solution. Write down an equation for a suitable half-reaction which
supports your answer. (4)
[16]

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QUESTION 10 ORGANIC CHEMISTRY (1)

10.1 The structural formula of an organic compound found in pears, raspberries

and pineapples is given below.

10.1.1 Name the homologous series to which this compound belongs. (1)

10.1.2 Give the IUPAC name of this compound. (2)

10.1.3 Give the IUPAC name of the organic acid used to make this
compound. (2)

10.1.4 Write a balanced chemical equation, using molecular formulae, for the
complete combustion of this compound. (3)

10.1.5 Define the term isomers. (2)

10.1.6 Give the IUPAC name of a:

(a) positional isomer of this compound. (2)

(b) functional isomer of this compound. (2)

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10.2 2-chloropropane is heated under reflux with an aqueous solution of sodium

hydroxide as shown in the diagram.

10.2.1 Name the type of reaction taking place between 2-chloropropane

and aqueous sodium hydroxide. (1)

10.2.2 Using condensed structural formulae, write a balanced chemical

equation for this reaction. (5)

10.2.3 A second reaction using 2-chloropropane and sodium hydroxide was

done. This time the NaOH was dissolved in ethanol and the mixture
was heated strongly. Give the structural formula of the organic
product of this reaction. (2)
[22]

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QUESTION 11 ORGANIC CHEMISTRY (2)

Kerosene is a mixture of a number of long chain saturated hydrocarbons. When

kerosene is strongly heated in the presence of a hot catalyst, it decomposes to
produce a gaseous mixture of butane, ethene and other short chain hydrocarbons.
The gas mixture produced can be collected in the laboratory as shown in the
diagram below.

[Source: <http://www.entertainmentbazar.com>]

11.1 What name is given to the type of elimination reaction described above? (1)

11.2 Define saturated hydrocarbon. (3)

11.3 Name the homologous series to which the saturated hydrocarbons belong. (1)

11.4 The gases produced in this process are collected by the downward
displacement of water. With reference to the relevant intermolecular forces,
explain why these gases are insoluble in water. (3)

11.5 The test tube containing the gas mixture collected in this reaction is shaken
with a solution of bromine. The bromine solution rapidly loses its colour.

11.5.1 Which compound (butane or ethene) reacted most to cause the

rapid decolourisation of bromine? (1)

11.5.2 Name the type of reaction that has taken place. (1)

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11.6 One of the branched chain hydrocarbon products of this reaction is shown
below.

CH2CH3
|
CH3 – CH – CH3
|
CH3

Write down the IUPAC name of this compound. (4)

11.7 One of the components of kerosene has the molecular formula C 12H26. The
equation below shows the hydrocarbon products formed when C12H26
breaks down.
Heat
C12H26(ℓ) C4H10(g) + C2H4 (g) + 2 X(g)
Catalyst
11.7.1 Determine the molecular formula of compound X. Show all
workings. (3)

11.7.2 With reference to the intermolecular forces and the factors

influencing their strength, explain why C12H26 is a liquid but the
hydrocarbon products of this reaction are all gases at room
temperature. (5)
[22]

Total: 200 marks

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