Thursday, 12 August 2021 08:06

PHYSICAL SCIENCES: CHEMISTRY PAPER 2 GRADE 12 QUESTIONS - NSC PAST PAPERS AND MEMOS FEBRUARY/MARCH 2018

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PHYSICAL SCIENCES: CHEMISTRY
PAPER 2
GRADE 12 
NSC PAST PAPERS AND MEMOS
FEBRUARY/MARCH 2018

INSTRUCTIONS AND INFORMATION 

  1. Write your centre number and examination number in the appropriate spaces  on the ANSWER BOOK. 
  2. This question paper consists of TEN questions. Answer QUESTION 5.3 on  the attached GRAPH PAPER. Answer ALL the questions in the ANSWER  BOOK. 
  3. Start EACH question on a NEW page in the ANSWER BOOK. 
  4. Number the answers correctly according to the numbering system used in this  question paper. 
  5. Leave ONE line between two subquestions, for example between  QUESTION 2.1 and QUESTION 2.2. 
  6. You may use a non-programmable calculator. 
  7. You may use appropriate mathematical instruments. 
  8. You are advised to use the attached DATA SHEETS. 
  9. Show ALL formulae and substitutions in ALL calculations.
  10. Round off your FINAL numerical answers to a minimum of TWO decimal  places. 
  11. Give brief motivations, discussions, et cetera where required.  
  12. Write neatly and legibly.

QUESTIONS

QUESTION 1:  MULTIPLE-CHOICE QUESTIONS
Various options are provided as possible answers to the following questions. Choose the answer and write only the letter (A-D) next to the question number (1.1-1.10) in the ANSWER BOOK, for example 1.11 D.
1.1  Which ONE of the following is the general formula of alkynes?

  1.  CnH2n
  2. C2nH2n
  3.   CnH2n - 2
  4.  CnH2n + 2    (2)

1.2  The type of reaction that takes place when a carboxylic acid and an alcohol react in the presence of an acid:

  1. Addition
  2. Hydrolysis
  3. Substitution
  4. Esterification  (2)

1.3 Which ONE of the following isomers has the LOWEST boiling point?

  1.  CH3CH2CH2CH2CH2CH3
  2.  CH3CH2C(CH3)2CH3
  3.  CH3CH(CH3)CH2CH2CH3
  4.  CH3CH2CH(CH3)CH2CH3     (2) 

1.4  Which ONE of the reaction rate versus time graphs below best represents the reaction between magnesium and EXCESS dilute hydrochloric acid?
reaction rate(2)
1.5  Which  ONE  of the following  will  NOT  affect  the  equilibrium position  of reversible chemical reactions?

  1. Temperature
  2. Catalyst
  3. Pressure
  4. Concentration (2) 

1.6   The following equilibrium exists in pure water at 25 °C.

2H2O(ℓ)  ⇌  H3O+(aq) + OH(aq)           ∆H > 0

At this temperature, the pH = 7 and Kw = 1 x 10-14. The temperature of the water is now increased to 90 °C.  Which ONE of the following is TRUE at the new temperature?

  1. pH = 7
  2. [H3O+] = [OH    ]
  3. [H3O+][OH   ] = 10-14
  4. [H3O+] = 10-7 mol∙dm-3        (2)

1.7  A  hydrochloric  acid  solution  is  titrated  against  an  ammonia  solution. The balanced equation for the reaction is:

HCℓ(aq)  +  NH4OH(aq)  →  NH4Cℓ(aq)  +  H2O(ℓ)

Which ONE of the following gives the pH of the solution at the end point and the reason for this pH? (2)

   pH   REASON
 3  H3O+(aq) is formed during the ionisation of HCℓ(aq).
 5  H3O+(aq) is formed during hydrolysis of NH (aq).
C  7  Neutralisation takes place at the end point.
D  8  OH-(aq) is formed during hydrolysis of NH4 (aq). 

1.8  A decrease in the oxidation number of an atom during a chemical reaction is known as …

  1.  redox.
  2.   oxidation.
  3.   reduction.
  4.   electrolysis. (2)

1.9 The two half-reactions below are used to construct a galvanic cell.

X+(aq)  +  e-  ⇌  X(s)              Eθreduction = + 0,15 V
Y2+(aq)  +  2e-  ⇌  Y(s)          Eθreduction = - 0,15 V

Which ONE of the statements below is CORRECT when  the cell is  in operation?

  1.  X+(aq) is reduced.
  2.  Y(s) is reduced.
  3.  X(s) | X+(aq) is the negative electrode.
  4.  Electrons flow from X(s) to Y(s) in the external circuit.  (2)

1.10  Which ONE of the following is CORRECT for the industrial preparation of sulphuric acid?  (2)[20]

  PROCESS    CATALYST 
 A  Ostwald    Platinum
 B Haber  Iron
 C Contact        Iron
 D Contact  Vanadium pentoxide

QUESTION 2   (Start on a new page.)
The letters A to E in the table below represent six organic compounds.
ethene
2.1 Write down the LETTER that represents EACH of the following:
2.1.1 A tertiary alcohol                      (1)
2.1.2 An aldehyde                  (1)
2.1.3 A ketone                       (1)
2.1.4  A functional isomer of compound B                                (1)
2.2 Write down the IUPAC name of:
2.2.1 Compound B                                (1)
2.2.2 Compound E                                (4)
2.3 Define positional isomers. (2)
2.4 Write down the STRUCTURAL FORMULA of:
2.4.1A positional isomer of compound C                                (2)
2.4.2 Compound D                                (2)
2.4.3The  organic  acid  that  will  react  with  compound  C to form butyl propanoate  (2) [17]
QUESTION 3   (Start on a new page.)
Study   the   vapour   pressure   versus   temperature   graphs   for   three   organic compounds, X, Y and Z, below which belong to different homologous series.
Atmospheric pressure is 100 kPa.
3
3.1 Write down the vapour pressure of compound Y at 90 °C.           (1)
3.2 The  graphs  can  be  used  to  determine  the  boiling  points  of  the  three compounds.
3.2.1Define boiling point.         (2)
3.2.2 Determine the boiling point of compound X.               (1)
3.3 The homologous series to which the three compounds of similar molecular masses belong, were identified in random order as: 

alcohol;  carboxylic acid;  ketone

3.3.1 Which compound (X, Y or Z) is the carboxylic acid?                   (1)
3.3.2 Explain the answer to QUESTION 3.3.1 by referring to the type of intermolecular forces in compounds of each of the homologous series above.      (4)
3.3.3Compound X has three carbon atoms per molecule. Write down the IUPAC name of compound X.      (1)  [10]

QUESTION 4   (Start on a new page.)
Consider the incomplete equations for reactions I to IV below. P, Q, R and S are organic compounds.
4
4.1Define a cracking reaction. (2)
4.2 Write down the reaction number (I, II, III or IV) that represents EACH of the following:
4.2.1A cracking reaction   (1)
4.2.2An addition reaction  (1)
4.2.3 A substitution reaction   (1)
4.3Write down:
4.3.1ONE reaction condition for reaction I      (1)
4.3.2 The compound (P, Q, R or S) that represents an unsaturated hydrocarbon   (1)
4.3.3 The IUPAC name of compound P  (1)
4.3.4 The molecular formula of compound R  (2)
4.3.5The structural formula of compound Q (2)
4.3.6The structural formula of compound S    (2) [14]

QUESTION 5   (Start on a new page.)
ANSWER QUESTION 5.3 ON THE ATTACHED GRAPH PAPER.
Learners use the reaction between sodium thiosulphate and hydrochloric acid to investigate one of the factors that affects reaction rate. The balanced equation for the reaction is:

Na2S2O3(aq)  +  2HCℓ(aq)  →  2NaCℓ(aq)  +  H2O(ℓ)  +  SO2(g)  +  S(s)

The diagram below shows the experimental setup.
5
In  the  first  experiment,    50 cm3  of  the  sodium  thiosulphate  solution  is added  to 100 cm3 of a 2 mol∙dm-3 dilute hydrochloric acid solution in a flask that is placed over a cross drawn on a sheet of white paper. The hydrochloric acid is in EXCESS.
The time taken for the cross to become invisible, when viewed from the top, is recorded.
The experiment is then repeated four times with different volumes of the sodium thiosulphate solution. The results obtained are shown in the table below.

EXPERIMENT

VOLUME OF 
Na2S2O3
(cm3)

VOLUME OF  
H2O (cm3)

TIME

(s)

AVERAGE RATE
   1     )
tim e
(x 10-2 s-1)

1

50

0

22,7

4,4

2

40

10

28,6

3,5

3

30

20

38,5

2,6

4

20

30

58,8

1,7

5

10

40

111,1

0,9

5.1  Define reaction rate.        (2)
5.2 How  does  the  concentration  of  the  sodium  thiosulphate  solution  used in experiment 2 compare to that used in experiment 5? Choose from MORE THAN, LESS THAN or EQUAL TO.  (1)
5.3 Draw a graph of average reaction rate versus volume of sodium thiosulphate used on the attached GRAPH SHEET. 
(ATTACH THIS GRAPH SHEET TO YOUR ANSWER BOOK.)      (3)
5.4 Use the information in the graph to answer the following questions.
5.4.1Determine  the  volume  of  dilute  sodium  thiosulphate  solution that needs to react in order for the cross to become invisible in 40 seconds. 
USE DOTTED LINES ON THE GRAPH TO SHOW HOW YOU ARRIVED AT THE ANSWER.     (3)
5.4.2Write down a conclusion for this investigation.           (2)
5.5 Use the collision theory to explain the effect of an increase in concentration on reaction rate.  (3)
5.6   The mass of sulphur produced in experiment 1 is 1,62 g. Calculate the mass of the sodium thiosulphate used in experiment 1.    (4) [18]

QUESTION 6   (Start on a new page.)
6.1  A reversible gaseous reaction is allowed to reach equilibrium in a closed container at different temperatures and pressures.
The graph below shows the percentage yield for this reaction at 30 kPa as the temperature is increased.
6
Use the information in the graph above to answer the following questions.
6.1.1 State Le Chatelier's principle.     (2)
6.1.2 The heat of reaction (∆H) for the forward reaction is POSITIVE. Use Le Chatelier's principle to explain this statement.  (3)
The graph below show the percentage yield for this reaction as pressure changes at constant temperature.
6.1
6.1.3  Explain the effect of an increase in pressure on the equilibrium position of a reaction.  (2)
6.1.4 Which ONE of the following equations (I, II or III) represents the equilibrium above?

  1. 2A(g)  +  3B(g)  ⇌  3C(g)
  2. A(g)  +  B(g)  ⇌  3C(g)
  3. A(g)  +  B(g)  ⇌  2C(g)   (2)

6.2  A  mixture  of     0,2  moles  of  hydrogen  chloride      (HCℓ)  and    0,11  moles of oxygen gas (O2) is sealed in a 200 cm3 flask at a certain temperature.
The reaction reaches equilibrium according to the balanced equation below:

4HCℓ(g)  +  O2(g)  ⇌  2Cℓ2(g)  +  2H2O(g)

It is found that 1,825 g of hydrogen chloride is present at equilibrium.
Calculate the equilibrium constant, Kc, for this reaction at this temperature.   (9)  [18]

QUESTION 7   (Start on a new page.)
7.1  The balanced equation below represents the first step in the ionisation of sulphuric acid (H2SO4) in water:

H2SO4(ℓ) + H2O(ℓ)  ⇌  H3O+(aq) + HSO-4 (aq)

7.1.1 Write down the FORMULAE of the TWO bases in the equation above. (2)
7.1.2 Is sulphuric acid a STRONG or a WEAK acid? Give a reason for  the answer.  (2)
7.2  Learners use the reaction of a 0,15 mol∙dm-3 sulphuric acid solution with a sodium  hydroxide  solution  in  two  different  experiments.  The  balanced equation for the reaction is:

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

7.2.1 They  use    24  cm3  of  H2SO4(aq)  in  a  titration  to  neutralise 26 cm3 of NaOH(aq).
Calculate the concentration of the NaOH(aq).   (5)
7.2.2 In  another  experiment,     30  cm3  of  the  H2SO4(aq)  is  added to 20 cm3 of a 0,28 mol∙dm-3 NaOH solution in a beaker.
Calculate the pH of the final solution.   (8)  [17]

QUESTION 8   (Start on a new page.)
8.1           A  group  of  learners  use  the  redox  reaction  below  to  construct  an electrochemical cell.

Sn2+(aq)  +  2Ag+(aq)  →  2Ag(s)  +  Sn4+(aq)

8.1.1 Define a reducing agent in terms of electron transfer.     (2)
8.1.2  Name a substance that should be used as electrode in the anode half-cell.  (1)
8.1.3 Write down the NAME or FORMULA of the reducing agent.        (1)
8.1.4 Write down the cell notation of the cell.            (3)
8.1.5 Calculate the initial emf of this cell under standard conditions.                                                                                                                       (4)
8.2  In a separate experiment, the learners place magnesium ribbon in a beaker containing a blue solution of copper(II) sulphate. After a while the solution becomes colourless.
8
8.2.1 State ONE observable change in the beaker, besides a colour change of the solution, that the learners can make. (1)
8.2.2 Refer to the relative strengths of oxidising agents or reducing agents to explain why the solution becomes colourless. (3)  [15]

QUESTION 9   (Start on a new page.)
The  graph  below  represents  the  changes  in  mass  that  occur  at  electrode  A and electrode B in an electrolytic cell during the purification of copper.
9
9.1 Define electrolysis.   (2)
9.2 Which graph, A or B, represents the change in mass of the anode during electrolysis?  (1)
9.3 Write down the equation of the half-reaction which takes place at the cathode of this cell.(2)
9.4 Use the information in the graph and calculate the percentage purity of the impure copper.   (4)  [9]

QUESTION 10   (Start on a new page.)
10.1  The   diagram   below   shows   processes   involved   in   the   production   of fertiliser X and fertiliser Z.
10
Write down the:
10.1.1  Balanced equation for the formation of product Q   (3)
10.1.2 FORMULA of fertiliser X   (1)
10.1.3 NAME of process A     (1)
10.1.4  NAME of fertiliser Z    (1)
10.2  A 10 kg bag of NPK fertiliser is labelled 6 : 1 : 5 (22).
10.2.1 What is the meaning of NPK?      (1)
10.2.2 What is the meaning of (22) on the label?   (1)
10.2.3  Calculate the mass of potassium in the bag.  (4)  [12] 

TOTAL: 150

DATA FOR PHYSICAL SCIENCES GRADE 12 PAPER 2 (CHEMISTRY)

TABLE 1: PHYSICAL CONSTANTS

NAME  SYMBOL   VALUE 
Standard pressure   pθ 1,013 x 105 Pa 
Molar gas volume at STP   Vm 22,4 dm3∙mol-1 
Standard temperature   Tθ  Tθ 273 K 
Charge on electron   e e -1,6 x 10-19
Avogadro’s constant   NA NA 6,02 x 1023 mol-1


TABLE 2: FORMULAE

n = m
      M

n = N
      NA
c = n
      V
or c = m
          MV
n = V
      Vm
caVana
cbVb    nb
pH= -log[H3O+]
Kw = [H3O+][OH-] = 1x10-14 at 298K   

 

Eθ cell = Eθ cathode – Eθ anode 
Eθ cell = Eθ reduction – Eθ oxidation 
Eθ cell = Eθ oxidising agent – Eθ reducing agent 

 

periodic
A
B
C

Last modified on Friday, 13 August 2021 07:05