# Physical Sciences Grade 12 P2 KwaZulu Natal Mock 2018 QP

> Grade 12 Physical Sciences Paper 2 question paper from the KwaZulu Natal Mock Exam 2018, 23 pages. Read online or download the free PDF.

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- Updated: 2026-09-27
- Subject: Physical Sciences
- Grade: Grade 12
- Document type: Question paper
- Year: 2018
- Exam period: KwaZulu Natal Mock Exam
- Paper: 2
- Curriculum: CAPS
- Pages: 23

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### Page 1

Education

NATIONAL
SENIOR CERTIFICATE

--GRADE 12 —

TIME : 3Hours

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KwaZulu-Natal Department of Education

. PHYSICAL SCIENCES P2 (CHEMISTRY)
: PREPARATORY EXAMINATION
a SEPTEMBER 2018

MARKS : 150

This question paper consists of 22 pages including data sheets.

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Physical Sciences P2

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nse

INSTRUCTIONS AND INFORMATION TO CANDIDATES

t.

10.

11.
12), °

Write your name and other information in the appropriate spaces on the
ANSWER BOOK.

The question paper consists of TEN questions. Answer ALL the questions

in the ANSWER BOOK.
Start EACH question on a NEW page in the ANSWER BOOK.

Number the answers correctly according to the numbering system used
in this question paper.

Leave one line between two sub-questions, for example between
QUESTION 2.1 and QUESTION 2.2.

You may use a non-programmable pocket calculator.
You may use appropriate mathematical instruments.

You are advised to use the attached DATA SHEETS.
Show ALL formulae and substitutions in ALL calculations.

Round off your final numerical answers to a minimum of TWO decimal
places where applicable. ,

Give brief motivations, discussions, et cetera where required.

Write neatly and legibly.

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September 2018 Preparatory Examination

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Physical Sciences P2 3

September 2018 Preparatory Examination
NSC

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 equations represents the incomplete combustion
of pentane?

A 2 CH3sCH2CH2CH2CHs + 11 O02 + 10CO2 + 12H:0

B 2 CHsCH2CH2CH2CHs + 1102 > 10CO + 12H20

Cc CH3CH2CH2CH2CHs + 8O2 + 5CO2 + 6H2O

D CH3sCH2CH2CH2CH3 + 8O2 > 5CO + 6H20 (2)

1.2 A polymer formed as a result of addition polymerisation is most likely to be
derived from a monomer that is ...

A An ester.

B An alcohol.

Cc A hydrocarbon.

D A carboxylic acid. (2)

1.3. The IUPAC name of an organic compound with the molecular formula CsH100 can be:
A pentan-1-ol

B pentanoic acid
Cc 3-methylbutanal
D _—_3-methylbutan-1-one (2)

1.4 The following reaction reaches equilibrium in a sealed container.
2SO2(g) + O2(g) = 2S0s(g)

Which ONE of the following graphs correctly illustrates the relationship between

percentage yield of SOs(g) and pressure for the above reaction, at constant
temperature.

A B

Percentage Yield
Percentage Yield

Co

Pressure Pressure

Percentage Yield

Percentage Yield

—— __ (2)

Pressure Pressure
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Physical Sciences P2 * 4 September 2018 Preparatory Examination
SC

1.5 The graph below represents the change in potential energy against time for the
following reaction:

Az(g) + 2B2(g) = — 2AB2(g)

Reaction co-ordinate

Which ONE of the following statements is correct?

A The forward reaction is exothermic.

B_ The heat of reaction for the forward reaction is Q —P. |
C The activation energy for the forward reaction is R—Q.

D_ The activation energy for the reverse reaction is R—P. (2)

1.6 A mixture of sulphur dioxide and oxygen gases, together with a suitable catalyst,
are placed in an evacuated, sealed container.
The following reaction takes place in the container at constant temperature:

4 .NH3(g) + 5 O2(g) 24NO(g) + 6 H20(g)

The mass of the catalyst is measured over time.
Which ONE of the following graphs correctly illustrates the relationship between the
mass of the catalyst and time?

A A B A
n
3 3
E =
Pa i
Time (s) Time (s)
Cc a D h
g
g :
. z
ees
Time (s) Time (s)

(2)

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1.7. The balanced equation below represents the first step in the ionization of
sulphuric acid in water:

H2SOa(t) + H2O0(2) = HsO*(aq) + HSO; (aq)
The TWO Bronsted bases in the equation above are:

A H2SO4 and H20

B H30* and HSO;

Cc H2SO4 and H30*

D H2O0 and HSO; (2)

1.8 | Apiece of magnesium ribbon is placed in a beaker containing a blue solution
of copper(Il)sulphate.

CuSOa(aq)

Mg

After a while, it is observed that the solution becomes colourless. The reason
that the solution becomes colourless is:

The Cu** is a stronger oxidising agent than Mg2* and is reduced to Cu.

The Mg?* is a stronger oxidising agent than Cu2* and is reduced to Mg.

Mg is a weaker reducing agent than Cu and will reduce Cu2* to Cu.

Cu is a stronger reducing agent than Mg and will oxidise Mg to Mg?*. (2)

0DQOWD>

1.9 Which ONE of the following statements about the extraction of aluminium is TRUE?
A Aluminium oxide is dissolved in molten cryolite.

B The ore of aluminium oxide is called cryolite.
Cc When the cell is in operation, aluminium forms at the anode.
D When the cell is in operation, carbon dioxide gas forms at the cathode. (2)

1.10 Which ONE of the following is a primary nutrient for plants?

A Carbon

B Oxygen

Cc Potassium

D Magnesium (2)

[20]

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QUESTION 2 (Start on a new page.)

September 2018 Preparatory Examination

The letters A to G in the table below represent six organic compounds.

. i : i |
jonas eae: es OS
aE aie eee eae e |

i —H H
i — CHs

H — ; — H
H

c t D | CHsCH2CH(CHs)CH2CH(CHs)CHs

—- ¢C—C—c —

| |
E fe} F
I fe)
CHs — C — O — CHo — Chs ||
— C —H

G | Ethene
2.1 Write down the LETTER that represents EACH of the following:

2.434

2.1.2

A functional isomer of butanoic acid.
The compound that has a carboxyl group.

A saturated hydrocarbon.

The structural formula of the functional group of an aldehyde.

The smallest organic molecule that can be covalently bonded to each other

in a repeating pattern.

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(1)
(1) \
(1)
(1)

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Physical Sciences P2 7 September 2018 Preparatory Examination
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2.2 For compound A, write down the:
2.2.1 IUPAC name. (2)
2.2.2 General formula of the homologous series to which it belongs. (1)
2.3. Consider compound E:
2.3.1 Write down the IUPAC name of the alcohol required to prepare compound E. (1)

2.3.2 The name of the catalyst that is used in the reaction that produces
Compound E. (1)

[10]

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QUESTION 3 (Start on a new page.)

The boiling points of organic compounds from 3 different homologous series are given
in the table below: '

[ COMPOUND BOILING POINT
A 78,40 °C
B -89,00 °C
Cc 118,50 °C
3.1 Define each of the following terms:
3.1.1 homologous series. (2)
3.1.2 boiling point. (2)
3.2 Which compound A, B or C will have the lowest vapour pressure?
Explain the answer. . (3)
3.3. Which compound A, B or Cis a gas at room temperature? (1)

3.4 The homologous series to which the three compounds A, B and C belong, were
identified in random order as : ETHANOIC ACID, ETHANOL AND ETHANE.

3.4.1 What is the boiling point of ethanoic acid? (1)

3.4.2 Explain the answer to question 3.4.1 by referring to the type of intermolecular
forces and the energy involved in the compound from each homologous
series. (4)

[13]

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QUESTION 4 (Start on a new page.)

In the flow diagram below, W, X, Y and Z represent organic reactions. Q, S and R represents
organic compounds. Q is the major product.

ate tb bab ye teadioni Feaeouere

REACTANT P
H H H H

| | HBr
H H

reaction X

reaction Y

reaction Z PRODUCT S

PRODUCT R
CH3sCHCH2CHs

+ Fel © |

41

4.2
4.3
44
4.5
4.6

Name the type of reaction that is represented by...

4.1.1. W. (1)
41.2 Y. he (1)
Write down the structural formula and IUPAC name for the product Q. (3)

Is product R a primary, secondary or tertiary alcohol? Give a reason for the answer. (3)
Name the type of elimination reaction represented by Z. (1)
State TWO reaction conditions that must be satisfied for reaction Y to take place. (2)

Product S is a positional isomer of reactant P.

4.6.1 Define the term positional isomer. (2)

4.6.2 Classify reaction X as, substitution, addition or elimination. (1)
4.6.3 Use structural formulae to write a balanced equation for the formation of

product S from product Q. (3)

F [17]

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QUESTION 5 (Start on a new page)

5.1 The graph drawn below shows how the mass of powdered calcium carbonate
changes with time when the powdered calcium carbonate reacts with a specific
volume of hydrochloric acid of known concentration at conditions of standard
temperature and pressure.

The balanced equation for the reaction that takes place is given below:

CaCOs(s) + 2HCt(aq) > CaCh(aq) + CO2(g) + H20(£)

100
80 |
i)
© 60
fe}
()
3 =
(6)
Ko) coos a
& 40
G
=
20
0 :
0 10 20 30 40 50 60 70
Time (s)
5.1.1 Define reaction rate in words. (2)
5.1.2 After how many seconds does the reaction between calcium carbonate and
hydrochloric acid stop? (1)

5.1.3 Calculate the volume of hydrochloric acid that was required at conditions of
standard temperature and pressure for the above reaction to reach
completion. (5)

The above reaction is repeated under the same conditions but the powdered calcium
carbonate is replaced by the same initial mass of lumps of calcium carbonate.

5.1.4 Write down the mass in grams of calcium carbonate at the end of the reaction. (1)

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Physical Sciences P2 11 September 2018 Preparatory Examination
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5.1.5 How will the time for the reaction to reach completion be affected?
(Write down only, INCREASES, DECREASES or REMAINS THE SAME) (1)

5.1.6 Use the attached copy of the above graph and on the same set of axes
sketch a graph to show how the rate of the reverse reaction changes with
time for the same reaction. Label this graph lumps. (3)

5.2 The figure below shows the Maxwell-Boltzmann distribution curves for the above

reaction at two different temperatures. The activation energy for this reaction is
indicated on the graph by the vertical line and labelled as EA.

300 K

Number of particles

Kinetic energy En

5.2.1 Write down the name of the theory used to explain how reactions occur at the
molecular level. (1)

5.2.2 Referring to the shaded areas in the distribution curves provided, use the
theory named in QUESTION 5.2.1 to explain why an increase in temperature

causes an increase in reaction rate. (3)
[17]

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Physical Sciences P2 12 September 2018 Preparatory Examination
NSC

QUESTION 6 (Start on a new Page)

A mixture of 2 moles of hydrogen and 2 moles of iodine is sealed ina 4 dm? flask
at 180 °C. The reaction reaches equilibrium according to the balanced equation below:

Ha(g) + I2(g) = 2HIg)
The information in the table below also applies to the reaction above.

T°C Ke
180 49
450 48
6.1 State Le Chatelier’s Principle. (2)

6.2 What effect will the following changes have on the concentration of HI(g) at
equilibrium? ;

Choose from INCREASES,DECREASES or REMAINS THE SAME

6.2.1 The pressure on the system is increased without changing the volume. (1)

6.2.2 More Ha(g) is added to the system, without a change in pressure, (1)

6.2.3 A catalyst is added, : (1)

6.2.4 The temperature is decreased. (1)

6.3 Explain the answer to question 6.2.4, by referring to Le Chatlier’s Principle. (3)
6.4 Calculate the mass of HI present in the container when equilibrium is reached

at 180 °C. (10)

[19]

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Physical Sciences P2 13 September 2018 Preparatory Examination
NSC

QUESTION 7 (Start on a new page.)
A learner prepares a standard solution of barium hydroxide at 25 °C. She completely
dissolves an unknown mass of pure barium hydroxide in enough distilled water to make

a solution of volume 250 cm®. The prepared solution of barium hydroxide has a
pH of 13,45.

7.1 Give a reason why barium hydroxide is regarded as a STRONG base. (1)

The barium hydroxide solution prepared by the learner is dilute.

7.2 Explain what is meant by the above statement. (2)

Barium hydroxide dissociates as follows:
Ba(Oh)2 (aq) = Ba?* (aq) + 2 OH-(aq)

7.3 Calculate the mass of the barium hydroxide that was completely dissolved to make
the above solution. (7)

7.4 Calculate the volume of a 0,5 mol.dm*? hydrochloric acid solution, needed to

completely neutralize 60 cm® of the barium hydroxide solution prepared by the
learner. The balanced equation below represents the reaction that takes place.

2HCE£ (aq) + Ba(OH)2 (aq) = BaCtfe (aq) + 2H20(aq) (4)
[14]

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NSC

QUESTION 8 (Start on a new page.)

The electrochemical cell shown below consists of a chlorine half cell and an aluminium
half cell at standard conditions.

BO,

Clo(g}—= At

Pt |

Ct(aq) At*(aq)

8.1 Does the above electrochemical cell represent and ELECTROLYTIC or

GALVANIC cell? Give a reason for the answer. (2)
8.2 Write down three standard conditions needed for the above cell fo function. (3)
8.3 Write down the name of the oxidising agent in the above cell, (2)
8.4 — Calculate the initial emf of the above Cell under standard conditions, (4)

8.5 Write down the balanced NET (overall) cell reaction that takes place in this
cell. No spectator ions are required. (3)

8.6 How will the initial voltmeter reading change if the:
(Write down only INCREASES, DECREASES or REMAINS THE SAME)

8.6.1 Size of the platinum electrode is increased. (1)
8.6.2 Initial concentration of the electrolyte in the CATHODE HALF-CELL
is increased. (1)
[16]

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Physical Sciences P2 15 September 2018 Preparatory Examination
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QUESTION 9 (Start on a new page.)

The simplified diagram below shows an electrochemical cell used in refining copper.

Electrode P

Electrolyte X Electrode Q

9.1 Define an electrolyte. (1)

9.2 Write down the formula of the cation in the elecirolyte X in the above
electrochemical cell. (1)

9.3. When an electric current passes through the electrolyte the masses of the
electrodes change.

9.3.1 Does the mass of electrode P increase or decrease? (1)
| 9.3.2 Write down the relevant half reaction to support the answer to question 9.3.1 (2)
9.4 During the process illustrated by the above cell, a total of 2,259 x 104 cations are

reduced.
| Calculate the mass by which the cathode should change. (4)

[9]

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Physical Sciences P2 16 September 2018 Preparatory Examination
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QUESTION 10 (Start on a new Page.)

The different processes used in the preparation of fertilisers P and Q are represented
in the flow diagram below:

N2 He
Process X .
Product G j
Process Y i
v
NO
O2(g)
Acid R Acid S
N
Gas J if
Fertiliser P Fertiliser Q
Ammonium sulphate
10.1 Write down the name of:
10.1.1 Process X. (1)
10.1.2 Process Y. (1)
10.1.3 Gas J. (1)
10.1.4 Fertiliser P. (1)
10.2 Product G reacts with acid S to form fertiliser Q. Write down:
10.2.4 The name or formula of acid S. (1)
10.2.2 A balanced equation for the preparation of ammonium sulphate
as shown the flow diagram above. (3)
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Physical Sciences P2

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NSC

September 2018 Preparatory Examination

10.3 A bag of a certain brand of fertiliser, is labelled as shown in the diagram below:

FERTILISER

14: 1:5 (36)

The total mass of nitrogen in the bag of fertiliser shown above is 12,60 kg.
Calculate the value m, in kilograms indicated on the bag.

(4)

10.4 A farm wants to improve the quality of fruit produced on his farm. He has available
TWO bags of fertiliser as shown below:

| ||| FERTILISER

4:5: 5 (36)

FERTILISER A

FERTILISER

13: 5:9 (36)

FERTILISER B

Explain with reasons whether the farmer should apply fertiliser A or fertiliser B to

improve the quality of fruit produced on his farm.

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(3)
[15]

TOTAL MARKS: 150

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NSC

DATA FOR PHYSICAL SCIENCES GRADE 12

PAPER 2 (CHEMISTRY)

GEGEWENS VIR FISIESE WETENSKAPPE GRAAD 12

VRAESTEL 2 (CHEMIE)

TABLE 1: PHYSICAL CONSTANTS/TABEL 1: FISIESE KONSTANTES

NAME/NAAM SYMBOL/SIMBOOL VALUE/WAARDE
teal oe p® 1,013 x 10° Pa
Moe cenardinensce Vn 22,4 dm®.-mot"
Santeade een uy 273 K

por age eres e 1,6x10%c
peat Ratan Na 6,02 x 10 mort

TABLE 2: FORMULAE/TABEL 2: FORMULES

September 2018 Preparatory Examination

ain Aa:
M Na
n m Vv
c=— or/of c=—— n=—
Vv MV Vin
CaV, _ Ny = +
av, PH = -log[H30*]
Kw = [H30°][OH] = 1 x 10° at/by 298 k
a = =e on Lees / =i = =a = Fe hede
or/of
hay = redo ~ Fe estdeiny Later = Ercaiste = E ocaidasie
or/of
Bea a FES adeng agent 3 Eacdasgeat / ES = Ee ssatapojatigel z Eechisbatinidal

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NSC

Physical Sciences P2

TABEL 3: DIE PERIODIEKE TABEL VAN ELEMENTE

| 2 3 4 5 6 7 8 9 10 1 12 13 14 15 16 17 18
() (Ul) ; qm) (vy) st) vty
Atomic number
1 KEY/SLEUTEL Atoomgetal .
a H He
4 29 4
3 4 Electronegativity | g Symbol 5 6 7 8 9 10
< Li |? Be Elektronegatiwiteit °| = “ ~simboo! S Bs bs BS = Ne
7 9 is 11 12 14 16 19 20
1 12 t ‘| 43 | 14] #15; 16] 17 {| 18
3 Na/& Mg Approximate relative atomic mass 2 A2|2 SEIS a =Ce| Ar
23 24 Benaderde relatiewe atoommassa 27 28 31 32 35,5| 40
19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36
& K |2 Cal2 Sc |2 Ti |2 ©@ Cr |2Mn/[Z Fe |2 Co/® Ni |2 Cu|® Zn |2 Ga|2 Ge|& As |& Se | Br| Kr
39 40 45 48 51 52 55 56 59 59 63,5 65 70 73 75 79 80 84
37 38 39 40 41 42 43 44 45 46 47 43 49 50 51 52 53 54
e Rb{= Sr = Zr| Nb/2Mo/Z Tc /& Ru|s Rh|a& Pd |Z Ag /= Cd|= In |2 Sn|2 SbjG Te |& 1 | Xe
86 88 89 91 92 96 101 103 106 108 112 115 119 122 128 127 131
55 | . 56 57 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86
5 Cs|2 Ba| La|2 Hf| Ta} W] Re] Os| Ir| Pt] Au] Hg|2 T@/2Pb/2 Bi|% Pols At} Rn
133 137 139 179 181 184| 186 190 192 195 197 201 204 207 209
87 88 89
rd fe
S Fr js Re Ac 58 59 60 61 62 63 64 65 66 67 68 69 70 71
Ce | Pr | Nd | Pm|Sm| Eu | Gd | Tbh | Dy | Ho} Er | Tm | Yb} Lu
140 141 144 150 152 157 159 163 165 167 | 169 173 175
90 91 92 93 94 95 96 97 98 99 100 101 102 103
Th | Pa | U | Np} Pu | Am|Cm| Bk | Cf | Es | Fm| Md | No | Lr
232 238

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Physical Sciences P2

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Increasing oxidising ability/Toenemende oksiderende vermoé

TABLE 4A: STANDARD REDUCTION POTENTIALS
TABEL 4A: STANDAARD- REDUKSIEPOTENSIALE

20
NSC

September 2018 Preparatory Examination

_Half-reactions/Halfreaksies E7(v)
F2(g)+2e = 2F + 2,87
Co* +e a Co* +1,81
H202+2H"+2e" = 2H20 44,77
MnO] + 8H" + Se Mn**+4H,0 | +1,54
Cf2(g) + 2e7 2cr + 1,36
CrOF +44H"+6e = 2C*+7H,0 | 41,93
O2(g)+4H*+4e"  ° 2H20 + 1,23
MnOz2+4H*+2e" = Mn**+2H,0 + 1,23
PPt+2e pt + 1,20
Bro(t)+2e° = = 2Br + 1,07
NO3 +4H"+3e" =. NO(g)+2H20 | +0,96
Hg** + 26° Ha(2) + 0,85
Ag’+e a Ag + 0,80
NO3 +2H’+e" = NO2(g)+H20 | +0,80
Fe* +e  Fe* +077
O2(g) + 2H*+2e7 2 H2O2 + 0,68
k+2e = ar + 0,54
Cute ee Cu” + 0,52
SO2+4H"+4e7 =. S+2H20 +045
2H20+02+4e = 40H +0,40
Cu*+2e = Cu +0,34
SOF +4H*+2e" <2 $02(9)+2H20| +0,17
Cu* +e 2 Cur +0,16
Sn +2e Sn* +0,15
S+2H"+2e" = H2S(g) +014

2H*+2e =  Ha(g) 0,00

Fe"+3e «= Fe — 0,06
Pb*+2e = Pb = 0,13
Sn*+2e° 2. Sn - 0,14
Ni*+2e Ni ~0,27
Co*+2e- = Co — 0,28
Cd*+2e 4 Cd — 0,40
Ch+e = ct - 0,44
Fe*+2e Fe —0,44
Cr*+3e = Cr -0,74
Zn*+2e = Zn 0,76
2H20+2e° = Ha(g) + 20H™ ~ 0,83
CH +20 a Cr - 0,94
Mn*+2e° a Mn -1,18
AG + 36° At -1,66
Mg" +2e = Mg ~ 2,36
Na*+e oo Na -2,71
Ca*+2e = Ca — 2,87
SP+2e = Sr 2,89
Ba" +2e = Ba - 2,90
Cs*+e 4 Cs - 2,92
K+e a K 2,93
lite 2 — 3,05

Increasing reducing ability/Toenemende reduserende vermoé

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Physical Sciences P2 21 September 2018 Preparatory Examination

TABLE 4B: STANDARD REDUCTION POTENTIALS
TABEL 4B: STANDAARD- REDUKSIEPOTENSIALE

Half-reactions/Halfreaksies E“(v)
lite se Li - 3,05
Kiem kK 2,93
Cst+e = Cs — 2,92
Ba*+2e = Ba ~ 2,90
SP+2e = Sr - 2,89
Ca*+2e = Ca - 2,87
Na*+e7 = Na -2,71
Mg"*+2e = Mg ~ 2,36
AGt+3e = AL 1,66 4
Mn*+2e7 = Mn -1,18
10 Ce +2e = Cr -0,91
& 2H20 +26" = Ha(g)+20H” | ~0,83
o Zn*+2e = Zn -0,76 ©
3 Cr*+3e" = Cr 0,74 £
3 Fe** + 267 Fe -0,44 o
2 Crt +e cr* -0,41 =
\ $s Ca*+2e = Cd - 0,40 zg
G Co*+2e7 = Co - 0,28 2
S NP*4+ 26" = Ni -0,27 g
3 Sn*+2e" a Sn ~0,14 3
5 Pb*+2e = Pb - 0,13 NS
iS Fe"+3e = Fe - 0,08 3
& 2H #26" = Hala) 0,00 5
| 3 S+2H'+2e" = H2S(g) +014 iS
| & sni+2e° = Sn** +015 2
| £ Cu*+e" = Cu +0,16 e
2 SO% +4H'+2e = SO2(g)+2H20 | +0,17 S
3 Cu*+2e° = Cu + 0,34 =
‘Oo 2H20+02+4e = 40H" +0,40 o
3 S02+4H*+4e a S+2H20 +045 >
3 Cu’+e” = Cu + 0,52 3
| > +20 = 2r +0,54 3
{ DB O2(g) + 2H*+2e = H202 + 0,68 =
BY Fe*+e = Fe* + 0,77 =
8 NOZ+2H*+e" = NOa(g)+H20 | +0,80 @
i Ag’te = Ag +0,80 5
Hg**+2e" = Hg(t) + 0,85 £
O05 +4H*+3e == NO(g)+2H20 | +0,96
Bro(t)+2e° = 2Br + 1,07
PH+2e = Pt +1,20
MnO2+4H*+2e" = Mn* +2H20 + 1,23
O2x(g)+4H*+4e° =) 2H20 +1,23
C07 +14H*+6e° = 2CP+7H20 | +14,33
Chig)+2e = 2cr + 1,36
MnO3 +8H'+5e" = Mn +4H20 +1,51
H202+2H"+2e° = 2H20 +177
Co*+e" = Co* + 1,81
F2(g)+2e7 a * 2F7 + 2,87

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Physical Sciences P2 September 2018 Preparatory Examination

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September 2018 Preparatory Examination

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QUESTION 5.1.6

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Time (s)

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