NATIONAL SENIOR CERTIFICATE EXAMINATION

NOVEMBER 2014

PHYSICAL SCIENCES: PAPER II

Time: 3 hours 200 marks

PLEASE READ THE FOLLOWING INSTRUCTIONS CAREFULLY

1. This question paper consists of 14 pages, a Data Sheet of 3 pages (i – iii) with data and
formulae and an Answer Sheet. Please remove the Data Sheet and Answer Sheet from the
middle of your paper.

2. Please check that your question paper is complete.

3. ALL the questions in this paper must be answered.

4. Question 1 consists of 10 multiple-choice questions. There is only one correct answer to

each question. These questions are answered on the inside front 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.

5. START EACH QUESTION ON A NEW PAGE.

6. Read the questions carefully.

7. Use the data and formulae whenever necessary.

8. Express ALL answers correct to TWO decimal places.

9. An approved calculator (non-programmable, non-graphical) may be used.

10. Show all the necessary steps in calculations.

11. It is in your own interest to write legibly and to set your work out neatly.

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QUESTION 1

Answer these questions on the inside front cover of your Answer Book. Make a cross (X) over the
letter of the response which you consider to be the most correct.

1.1 Sodium chloride (NaCℓ) is a solid which is soluble in water. Which one of the following
describes the intermolecular forces that exist between sodium chloride and water in
solution?

A Ion-dipole
B Dipole-dipole
C Ion-induced dipole
D Induced dipole-dipole

1.2 Consider the structure of hexane.

A molecule of hexane is considered to be non-polar. Which one of the following statements

best describes the reason why hexane is non-polar?

A Hexane contains only single bonds between atoms

B The electronegativity difference between C and H atoms is so small as to be
considered non-polar
C Hexane is a linear molecule hence is symmetrical
D The charge distribution of electrons within the hexane molecule is symmetrical

1.3 Hydrogen bonding is a type of intermolecular force that can exist between the molecules of
certain compounds. Which one of the statements below best describes the conditions under
which hydrogen bonding is most likely to occur?

It occurs between …

A small molecules which contain hydrogen atoms

B molecules in which hydrogen is bonded to small atoms with high electronegativity
C large molecules which contain both hydrogen and oxygen atoms
D molecules in which hydrogen is bonded to small atoms with low electronegativity

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To answer Questions 1.4 and 1.5, refer to the description below and the graphs A to D that are
provided.

In an experiment to determine the effect of concentration on reaction rate, a constant volume of

HCℓ(aq) of concentration 2 mol·dm–3 is added to a constant volume of Na2S2O3(aq) of varying
concentrations.

1.4 Which one of the graphs A, B, C or D represents the plot of concentration of sodium
thiosulphate (vertical axis) against time taken (horizontal axis) for the reaction?

1
1.5 Which one of the graphs A, B, C or D represents the plot of reciprocal of time   (vertical
t
axis) against concentration of sodium thiosulphate (horizontal axis) for this reaction?

1.6 Consider the following statements with respect to a chemical reaction in a state of dynamic
chemical equilibrium:

I The concentrations of the reactants and products are identical provided the reaction
occurs in a closed system.
II The rates of the forward and reverse reactions are identical provided the reaction
occurs in a closed system.
III The amounts of reactant and product remain unchanged provided the reaction occurs
in a closed system.

Which of the statement(s) above is/are true?

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

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1.7 Consider the following equilibrium established in a closed container at constant temperature.

2NO(g) + 2H2(g) N2(g) + 2H2O(g) ΔH < 0

Which one of the following sets of conditions listed below will produce the lowest yield of
N2(g)?

Pressure Temperature
A Increase by decreasing volume Decrease
B Increase by decreasing volume Increase
C Decrease by increasing volume Increase
D Decrease by increasing volume Decrease

1.8

The compounds X and Y may respectively be:

A CH3CH2CH3 and CH3CH2OOCCH2CH3

B CH3CHCH2 and CH3CH2CH2CH2OOCH
C CH3CHCH2 and CH3CH2CH2OOCCH3
D CH3CH2CH2 and CH3CH2CH2OOCCH3

1.9 Which one of the acids listed below is an example of a polyprotic acid?

A HNO3
B HCℓ
C H2SO4
D CH3COOH

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1.10 Consider beakers A and B as illustrated below.

20 cm3 of the NaOH(aq) solution in beaker A is added to the NaCℓ(aq) solution in

beaker B. Which one of the following represents the correct calculation for the new
concentration of Na+(aq) ions in beaker B?

0 , 015  0 , 005
A
0 ,17
0 , 015  0 , 05
B
0 ,17
0 , 015  0 , 05
C
0 ,15
0 , 015  0 , 005
D
0 ,15
[20]

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QUESTION 2

Calcium chloride is prepared according to the following balanced chemical equation:

Ca(s) + 2HCℓ(aq) CaCℓ2(aq) + H2(g)

Hydrochloric acid is produced for this preparation by the ionisation of hydrogen chloride
gas in water.

2.1 Define the term 'ionisation'. (2)

2.2 Write down a balanced chemical equation for the ionisation of hydrogen chloride
gas in water. (2)

2.3 Name the type of bonding that is present in a molecule of hydrogen chloride. (1)

2.4 Define the term 'electronegativity'. (2)

2.5 Make use of the Pauling scale of electronegativities, as provided in the Periodic
Table, to explain the type of bonding found in hydrogen chloride and crystalline
calcium chloride. (4)

2.6 HCℓ molecules are described as 'dipoles'. Explain what is meant by this term. (2)

2.7 Calcium chloride is soluble in water. The structure of its crystal lattice is broken
down by the water molecules to form aqueous ions in solution.

2.7.1 Name the type of crystal lattice of which calcium chloride is an example. (1)

2.7.2 Using diagrams to illustrate your answer, explain how the crystal lattice of
calcium chloride is broken down during the dissolving process. (4)
[18]

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QUESTION 3

In order to investigate the rate of the reaction between a carbonate and an acid, calcium
carbonate and excess of 2 mol·dm-3 hydrochloric acid react in a reaction vessel. The
balanced chemical equation for this reaction is

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

Consider the potential energy profile for this reaction as illustrated below:

3.1 The graph has been labelled I – V to represent the various energies that are
illustrated by this energy profile. Identify each of these energies on the profile. (5)

3.2 Using the molecular collision theory, explain why the chemical reaction must gain
potential energy between position A and position B according to the energy profile. (2)

3.3 Provide a name for the position on the graph labelled B and what significant
process takes place at this point. (2)

3.4 Name the type of reaction this graph represents. Explain how you came to this
conclusion. (3)

3.5 The same reaction takes place in the presence of a catalyst. On the potential energy
profile provided, show how the graph would change in the presence of a catalyst. (2)

3.6 How would the presence of a catalyst affect the value of the energy labelled V?
Explain you answer. (3)
[17]

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QUESTION 4

Organic chemistry can be described as the study of the structure, properties and reactions
of carbon based compounds. The carbon atom is unique in that it has certain features that
enable it to be the building block of all organic compounds.

4.1 State THREE features of the carbon atom responsible for giving carbon this
uniqueness. (3)

4.2 Draw a Lewis Diagram to represent a molecule of methane. (2)

4.3 Consider the organic compounds represented by the letters A to F listed below:

A CH3CH2CH2Cℓ B CH3COOCH3 C CH3CH2CH3

D CH3CH2CH2OH E CH3CHCH2 F HCOOH

4.3.1 Give the IUPAC name for compound A. (2)

4.3.2 Which formula represents an unsaturated hydrocarbon? Write down only the
correct letter. (1)

4.3.3 Give the names of the homologous series to which

(a) compound A
(b) compound B
belong. (2)

4.3.4 Give the names of the functional groups represented in compounds D and F. (2)

4.3.5 Name the chemical test that is carried out to distinguish between compounds
C and E and list the observations that are made. (3)

4.3.6 Explain, with reference to the relevant intermolecular forces, why

compound D is a liquid at room temperature whereas compound C is a gas. (4)

4.3.7 Write down a balanced chemical equation for the complete combustion of
compound D in oxygen using molecular formulae. (3)

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4.4 Consider the following sequence of organic reactions and then answer the questions
that follow. Reactions are labelled A to E.

4.4.1 Which one of the reactions A to E is …?

(Only write down the question number (a) to (d) and the letter you choose
next to it).

(a) a hydrolysis reaction

(b) a hydrohalogenation reaction
(c) a hydrogenation reaction
(d) a dehydration reaction (4)

4.4.2 Provide the chemical formula of a reagent that needs to be added for the
following to occur:

(a) Reaction B
(b) Reaction A (2)

4.4.3 Consider the product formed in reaction E. It is able to exist in two distinct
isomeric forms, one as a positional isomer and the other as a functional
isomer.

(a) Define the term 'isomers'. (2)

(b) State the difference between positional and functional isomerism. (4)
(c) (i) Draw the structural formula of a positional and a functional
isomer of the product formed in reaction E. (2)
(ii) Write down the IUPAC name of each isomer in
Question 4.4.3 (c)(i). (4)
[40]

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QUESTION 5

Nitrogen monoxide, released from the combustion engines of motor vehicles, reacts with
oxygen in the atmosphere to produce nitrogen dioxide. This reaction can be simulated in a
closed reaction container of volume 500 cm3 at a temperature of 100 oC. The reaction
reaches equilibrium according to the following chemical equation:

2NO(g) + O2(g) 2NO2(g)

Initially 4 mol of NO and 2,5 mol of O2 were placed in the reaction container with an
unknown amount of NO2. When equilibrium was established, it was found that the
concentration of NO present in the reaction container was 6,5 mol·dm-3. The equilibrium
constant, Kc, for the reaction at 100 ºC is 0,25.

5.1 State Le Chatelier's Principle. (3)

5.2 A chemical equilibrium occurs in a 'closed system'. State what is meant by the term
'closed system'. (2)

5.3 Calculate the number of moles of NO present at equilibrium. (3)

5.4 Calculate the number of moles of NO that were used up in reaching equilibrium. (2)

5.5 Calculate the concentration of O2 at equilibrium. (4)

5.6 Write down the expression for the equilibrium constant (Kc) for this reaction. (1)

5.7 Using the expression in Question 5.6 to assist in your calculation, determine the
number of moles of NO2 present in the system at equilibrium. (4)

5.8 Calculate the number of moles of NO2 initially present in the reaction container. (4)

5.9 When the temperature of the reaction mixture was increased from 100 oC to 175 oC,
the value of Kc decreased to 0,15. Is the forward reaction exothermic or
endothermic? Explain your answer by using Le Chatelier's principle. (5)
[28]

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QUESTION 6

6.1 Indicators (generally represented as HIn) are organic compounds which display
characteristic colours when placed in either an acidic or basic solution. They are
generally weak acids which will ionise in water to reach the following dynamic
equilibrium.

HIn(aq) + H2O(ℓ) H3O+(aq) + In–(aq)

(yellow) (blue)

Bromothymol blue is an indicator which is yellow in an acidic medium and blue in

an alkali.

6.1.1 Define an acid and a base in terms of the Brønsted-Lowry model. (2)

6.1.2 Indicators are said to be weak acids. State what is meant by the term 'weak
acid'. (2)

6.1.3 By referring to Le Chatelier's principle, explain why bromothymol blue

displays a blue colour when placed in a solution of sodium hydroxide. (4)

6.2 Potassium hydroxide is a strong base that dissociates when placed in water. A
standard solution of potassium hydroxide of concentration 0,45 mol·dm-3 is
prepared in a 250 cm3 volumetric flask at a temperature of 298 K.

6.2.1 State what is meant by the term 'standard solution'. (2)

6.2.2 Write down a chemical equation to show the dissociation of potassium

hydroxide in water. (2)

6.2.3 Calculate the mass of potassium hydroxide used in the preparation of the
standard solution. (5)

6.2.4 The ionisation constant for water (Kw) is 1 × 10-14 at 298 K. Calculate the
concentration of hydronium ions in the potassium hydroxide solution at
298 K. (4)

The standard potassium hydroxide solution prepared in Question 6.2 is used to

determine the unknown concentration of a solution of the weak acid, oxalic acid
(COOH)2. 25 cm3 of oxalic acid is placed in a conical flask with a few drops of
indicator. Exactly 15 cm3 of potassium hydroxide is required to reach the
equivalence point in the titration according to the following balanced chemical
equation:

(COOH)2(aq) + 2KOH(aq) (COOK)2(aq) + 2H2O(ℓ)

6.2.5 State what is meant by the term 'equivalence point' in a titration. (2)

6.2.6 Calculate the number of moles of potassium hydroxide used in the titration. (2)

6.2.7 Calculate the number of moles of oxalic acid that were neutralised by the
potassium hydroxide. (2)

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6.2.8 Calculate the unknown concentration of the oxalic acid. (3)

The table below lists the indicators that are most commonly used in a school
laboratory.

Indicator pH range or sensitivity range

Bromothymol blue 6,0 to 7,6
Methyl orange 3,1 to 4,4
Phenolphthalein 8,3 to 10

6.2.9 Explain what is meant by the term 'hydrolysis'. (2)

6.2.10 Which indicator would best be suited for the titration of the potassium
hydroxide solution against the oxalic acid solution? Use your knowledge of
hydrolysis to explain your answer. (4)
[36]

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QUESTION 7

Consider the silver-cobalt galvanic cell that is shown in the diagram below which is
operated under standard conditions. The two half cells are connected by a salt bridge which
contains an aqueous saturated solution of potassium nitrate.

7.1 State what is meant by the following terms:

7.1.1 electrolyte (2)

7.1.2 half cell (2)

7.2 State the energy conversion that takes place in a galvanic cell. (2)

7.3 Name a suitable electrolyte that could be used in the silver half cell. (1)

7.4 State what is meant by the term 'standard conditions' with particular reference to the
silver half cell. (2)

7.5 Identify the half cell that is the anode in this galvanic cell. (1)

7.6 Will the electrode in the cathode half cell increase or decrease in mass as the
galvanic cell delivers current? Explain your answer. (3)

7.7 The cell delivers 0,75 A of current for 10 minutes. Calculate the increase or
decrease in mass that the cathode will experience during this time period (assume
concentrations of electrolytes remain constant). (5)

7.8 Write down the net cell reaction for the silver-cobalt galvanic cell. (3)

7.9 With reference to the changing ionic conditions in each half cell, explain how the
salt bridge functions to maintain half cell neutrality within each half cell. (4)

7.10 Aqueous potassium nitrate is a very popular electrolyte used in the salt bridge of a
galvanic cell. Explain the significance of using an electrolyte such as potassium
nitrate. (2)

7.11 With reference to the standard cell conditions, write the full cell notation for this
galvanic cell. (3)
[30]
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QUESTION 8

Copper is a metal that can be purified from its ore through an electrolytic technique. The
impure copper ore, known as blister copper, is the anode of the cell while a pure copper
plate is used as the cathode. These electrodes are placed in an electrolyte of aqueous
copper sulphate as shown in the diagram below

Blister copper contains several metal impurities, most commonly silver (Ag), gold (Au),
iron (Fe) and zinc (Zn).

8.1 Name the electrolytic technique described in this question. (1)

8.2 Write down the half reaction that occurs at the cathode. (1)

8.3 Use the table of Standard Electrode Potentials to explain each of the following:

8.3.1 Why copper metal and not water is oxidised at the anode. (2)

8.3.2 With reference to the potential difference applied in the purification, explain
why iron and zinc will be oxidised at the anode, but gold and silver are not. (3)

8.3.3 Why Fe2+(aq) and Zn2+(aq) are not reduced at the cathode. (2)

8.4 Write down the net cell reaction for the purification of impure copper metal. (2)
[11]

Total: 200 marks

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