# Physical Sciences Grade 12 P2 North West November 2015 Memo

> Grade 12 Physical Sciences Paper 2 memorandum from the North West November 2015, 16 pages. Read online or download the free PDF.

- Page: https://www.hlayiso.com/library/nw-2015-sept-chemistry-p2-memo/1993652a-c5c2-434e-84e1-feb1f975d859
- Updated: 2026-09-27
- Subject: Physical Sciences
- Grade: Grade 12
- Document type: Memorandum
- Year: 2015
- Exam period: North West November
- Paper: 2
- Curriculum: CAPS
- Pages: 16

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## About this document

Physical Sciences · Grade 12 · North West November · 2015. Memorandum, 16 pages. Read online or download the PDF.

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## Document text

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Education and Sport Development

Department of Education and Sport Development
Departement van Onderwys en Sportontwikkeling
Lefapha la Thuto le Tihabololo ya Metshameko

NORTH WEST PROVINCE

NATIONAL

SENIOR CERTIFICATE

GRADE 12
PHYSICAL SCIENCES: CHEMISTRY (P2) *
" SEPTEMBER 2015 :
‘ MEMORANDUM :
Sees sees ee eee eee
MARKS: 150

This memorandum consists of 17 pages.

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Physical Sciences/P2 2 NW/September 2015

NSC — Memorandum

GENERAL GUIDELINES

1. CALCULATIONS

1

1.2

1.3

1.4

1.5

1.6

1.7

Award marks for: correct formula, correct substitution and correct answer
with unit.

Do not award any marks if an incorrect or inappropriate formula is
used, even though there may be relevant symbols and applicable
substitutions.

When an error is made during substitution into a correct formula,
award a mark for the correct formula and for the correct substitutions, but
do not give any further marks.

If no formula is given, but all substitutions are correct, the candidate
forfeits one mark.
Example:

No K, expression, correct substitution:

=O ve ov 2.
“oa” * ? G

Marks are only awarded for a formula if a calculation has been attempted,
i.e. substitutions have been made or a numerical answer is given.

Marks can only be allocated for substitutions when values are substituted
into formulae and not when listed before a calculation starts.

All calculations, when not specified in the question, must be done correctly
to TWO decimal places.

2. DEFINITIONS

Award TWO marks for a correct definition. Do not award any marks for an
incorrect or partially correct definition.

3. UNITS

3.1

3.2

Candidates must be penalised only once for the repeated use of an
incorrect unit within a question or subquestion.

Units are only required in the final answer of a calculation.

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Physical Sciences/P2 3 NW/September 2015
NSC — Memorandum

3.3. Award marks for an answer only and not for a unit per se. Candidates
forfeit the mark allocated for the answer in each of the following situations:

- Garrect answer + wrong unit

- Wrong answer + correct unit
- Correct answer + no unit

3.4 Separate compound units with a multiplication dot, not a full stop, for
example, mol:dm’. Accept mol.dm® (or mol/dm*) for marking purposes.

4, GENERAL

4.1 _ If one answer or calculation is required, but the candidate gives two, mark
only the first one, irrespective of which one is correct. If two answers are
required, mark only the first two, etc.

4.2 When achemical FORMULA is asked, and the NAME is given as answer,
the candidate forfeits the marks. The same rule applies when the NAME is
asked and the FORMULA is given.

4.3. When redox half-reactions are to be written, the correct arrow should be
used. If the equation

HS +S+2H*+20 (34)

is the correct answer, the marks must be given as follows:

HS =S+2H*+2e (4)

HS —S+2H*+2e (%)
S + 2H’ +2e —H,S (%)

S +2H* + 2e = HS (%)

4.4 When candidates are required to give an explanation involving the relative
strength of oxidising and reducing agents, do not accept the following:

Stating the position of a substance on table 4 only (e.g. Cu is above Mg).
Using relative reactivity only (e.g. Mg is more reactive than Cu).

The correct answer would be for instance: Mg is a stronger reducing agent
than Cu and therefore Mg will be able to reduce Cu** ions to Cu. The
answer can also be given in terms of the relative strength as electron
acceptors and donors.

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Physical Sciences/P2 4 NW/September 2015

45

46

4.7

4.8

4.9

4.10

NSC — Memorandum
One mark is forfeited when the charge of an ion is omitted per equation.

The error carrying principle does not apply to chemical equations or half
reactions. For example, if a learner writes the wrong oxidation/reaction haif-
reaction in the subquestion and carries the answer to another sub-question

(balancing of equations or calculation of E:.,) then the learner must not be
credited for this substitution.

In the structural formula of an organic molecule all hydrogen atoms must be
shown. Marks must be deducted if hydrogen atoms are omitted.

When a structural formula is asked, marks must be deducted if the learner
writes the condensed formula.

When an IUPAC name is asked and the candidate omits the hyphen (e.g.
instead of pent-1-ene or 1-pentene the candidate writes pent 1 ene or 1
pentene), marks must be forfeited.

When a chemical reaction is asked, marks are awarded for correct
reactants, correct products and correct balancing.

If only a reactant(s) followed by an arrow, or only a product(s) preceded by
an arrow is/are written, marks may be awarded for the reactant(s) or
product(s). If only a reactant(s) or only a product(s) is written without an
arrow, no marks are awarded for the reactant(s) or product(s).

Example: No + 3H2v —» 2NHs” bal. W

No + 3H, —»¥ 1/3

—> NH3Y 1/3
No + 3He 0/3
NH3 0/3

5. POSITIVE MARKING

Positive marking regarding calculations is followed in the following cases:

5.1

Subquestion to subquestion: When a certain variable is calculated in one
subquestion (e.g. 3.1) and needs to be substituted in another (3.2 or 3.3),
e.g. if the answer for 3.1 is incorrect and is substituted correctly in 3.2 or
3.3, full marks must be awarded for the subsequent subquestions.

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 The correct option is B

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Physical Sciences/P2 6 NW/September 2015
NSC — Memorandum
2.4
H oH H
“Ty —H —> 1 ain + /\
H H 4H H H H H H
vv mn ())
2.5
2.5.1. Dehydration ¥ (1)
2.5.2 Propenev (1)
2.6
2.6.1 Propan-2-one vv (2)
2.6.2 Aldehydes ¥ (1)
[15]
QUESTION 3
3.1
3.1.1. Functional group v (1)
3.1.2 Melting point. v (1)
3.1.3 Number of C-atoms (All have single bonds). v (1)
3.2 Carboxylic acid vv (2)
3.3 CnHan+2 Vv (2)
3.4 Melting points increases from A-C. vv (2)
3.5 Compound A has weak Van der Waal’s forces (London forces) whilst B and C

have strong hydrogen bonds between their molecules.v Hence, less energy

is needed to break the weak intermolecular forces in A than in B and C.v

Compound B has one site of hydrogen-bonding whilst compound

C has two sites of H-bonding.v Thus, C has stronger intermolecular forces

between its molecules than B,“ hence more energy is needed

to overcome the intermolecular forces in C than in B. “ (5)
[14]

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Physical Sciences/P2 7 NW/September 2015
NSC ~ Memorandum
QUESTION 4
4.144
H
i
H—C——-c— Br
H——C—H
I
H
vv (2)
4.1.2
| i
n—bow H-——C——H
a 4 v v
v H:0 |
Hi ——-C——Br + KOH Hi i c fo] H + KBr
H H
H—C——H H—C——H
| |
H H
(3)
4.1.3 Ethanol as solvent” / NaOH(aq) Yor KOH(aq) / Mild heat (2)

4.1.4 Hydrolysis / Substitution reactionv “

(2)

4.2.1. Condensation polymer is a polymer formed by two monomers with
different functional groups that are linked together in a condensation
reaction in which a small molecule (usually water) is lost. (2)

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Physical Sciences/P2 8 NW/September 2015
NSC — Memorandum

H cl
\ —o”
4 oN

4.2.3. Chloroethylene /Chloroethene/Vinyl chloride. vv

4.3.1. Condensation polymer “
4.3.2 Addition polymer “

4.4 ANY of the following:

- Blood transfusion sets”; - Transparent food packaging trays;
~ Plumbing pipes; - Synthetic leather, etc.

QUESTION 5
5.1 An acid is a proton donor. v “
5.2

5.2.1  H2O0 v

5.2.2 H,0* v

5.3
5.3.1 lonises / dissociates completely (in water) Vv v

§.3.2 pH =-log [H30*]
Ratio: 1:2
0,025 mol H3SO4 —»0,05 mol H30* “
PH = -log [Hs07] ¥
= -log [0,05] “
=1,3¥

5.4
5.41 OH Vv
5.4.2 DECREASE v

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(2)

(2)

(1)
(1)

(1)
[18]

(2)

(1)

(2)

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Physical Sciences/P2 9 NW/September 2015
NSC — Memorandum

5.5 — n(H2SO4) = cV Y = (0,4)(15x10°) v

= 6x10 mol ¥

n(NaQH) = cV— = (0,2)(25x10°) v

= 5x10° mol
From the balanced equation:
4 mol of HoSO, =2 mol of NaOH
Hence, n(NaOQH) needed to neutralise the acid = 2(6x10°°) =12x10° mol ¥
Therefore insufficient NaOH was added to the acid since 5x10° mol

is less than the required 12x10 mol ¥ (6)
[18]

QUESTION 6

6.1. What is the relationship between the reaction surface or state of division of a
solid and the rate of a reaction? / How does reaction surface (or state of
division) influence the rate of a chemical reaction? v v

OR
What is the relationship between the reaction surface (of a reactant) and the
time that reaction takes to progress completely? (2)
6.2 CaCOa,(s) + 2HCl(aq) v —» CaClo(aq) + H20(I) + CO2(g) “ bal ¥ (3)

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Physical Sciences/P2

6.3

10 NW/September 2015

NSC — Memorandum

GRAPH OF DECREASE IN MASS VERSUS TIME

2,0¢

im

TOS TTY

1,5

1,0 y

Decrease in mass (g)

0,5

6 8
Time (min)

CHECKLIST

MARK ALLOCATION

Heading

v

Correct scale on both axes

Correct labelling of both axes

Plotting of points

Vv

Correct shape of curves

6.4 Reaction A is faster than Reaction BY

6.5 The same (2g) v

6.6 The greater the reaction surface, the higher the rate of reaction will be.v “

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(6)
(1)
(1)
(2)

[15]

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Physical Sciences/P2 11 NW/September 2015
NSC — Memorandum

QUESTION 7

7.1 Le Chatelier’s principle: When the equilibrium in a closed system is
disturbed, the system will re-instate a new equilibrium by favouring
the reaction that will oppose the disturbance.
OR
Le Chatelier’s principle: When conditions (concentration, temperature
and pressure) are changed in equilibrium in a closed system, equilibrium
is shifted to the side which opposes the change. (2)

7.2.
OPTION 1: CALCULATION USING CONCENTRATION

1 He 1cO 1H20 1cO
Initial x/10 0,03 0 0
concentration
Reacted/produced | 0,02 0,02 0,02 v 0,02 v
Equilibrium X/10 - 0,02 | 0,01 0,02 0,02
v
Ke [CO]LH,O} v No Ke expression, correct

[H,][CO,] substitution Max. 7/8
(0,02)(0,02) y Wrong Kc expression

4v = Max. 4/8
X/10 ~0,02)(0,01) ax
X = 0,3
n(H2) = 0,3 mol v
OPTION 2: CALCULATION USING NUMBER OF MOLES
1H 1CO. | 1H,0 1co0
Initial quantity (mol) X 0,3 0 ie)
Change (mol) -0,2 -0,2 0,2 0,2 | Mole
tatio ~
Quantity at equilibrium (mol) X-0,2 O41 027% (02 |v
Equilibruim concentration X-0,2 0,01 0,02 0,02 | Divide
(mol.dm’?) 10 by 10 v
[COMH,O]
[H, CO, ]
av = —(0,02)(0.02)
X/10 -0,02)(0,01)
X = 03 Thus n(H2)= 0,3 mol ¥ (8)

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Physical Sciences/P2 12 NW/September 2015
NSC — Memorandum

7.3.

-ve marking

Exothermic “

A decrease in K, value at a higher temperature implies the reverse reaction
(endothermic)/ the reaction that uses energy is favoured. V Results in lower
product concentration (less products) OR higher reactant concentration

(more reactants). v Equilibrium position shifts to the right/ lies to the right. “ (4)
[14]
QUESTION 8
8.1 - Temperature of 25°C v
- Concentration of 1mol'dm® v (2)
8.2 Ag*(aq)+ @& — Ag(s) vv (2)
8.3 Ni v (1)
8.4 The emf decreases. v (1)
8.5  Ni(s) + 2Ag*(aq) “ — Ni**(aq) + 2Ag(s). Vv (3)
8.6 Ni-Ni**+2e
mol ratios: from the balanced equation is
02: 02 : 0,4
m=n(Ni).M %
=0,2x59v
= 11,8g of Ni is lost from the anode. “ (3)
8.7 A
-ve marking
Second (2") or B. Y
Magnesium (Mg) is a better reducing agent than Nickel (Ni) and its potential
difference is -2,36 V whilst that of Ni is -0,27 V. v
Silver (Ag) has the same oxidising ability in both galvanic cells. “ (3)
[15]

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Physical Sciences/P2 13 NW/September 2015
NSC ~ Memorandum

QUESTION 9

9.1. The process in which electricity is used to bring about a chemical
change in an electrolytic cell/ decompose /break compounds into components. “”

OR
A process in which electrical energy is converted to chemical energy. (2)
9.2 Pv’, itis the positive electrode/ anode. “
Oxidation takes place at the positive electrode /anode. “ (3)
9.3  Cu(aq)+2e — Cus) vv (2)

9.4 The rate at which copper is oxidised (at the anode) is equal to the rate
at which copper ions are reduced (at the cathode). v “

Rate of oxidation equals ihe rate of reduction. (2)
9.5 -Ornaments v; Electrical conductors v/Jewellery in
QUESTION 10
10.1 4NHa(q) +5 O2(aq) ~—» 4NO(g) + 6H2O(g) v ¥ (3)
10.2 Ptor Platinum ¥ (1)
10.3. Catalytic oxidation of NH3 VW” (2)
10.4 HNO ¥ (1)
10.5 Ostwald (process). v (1)
10.6 - Brown or yellow scorching around the edges of the leaves. “”
- Flowers become dull and sparse. “
- Fruit yield low and of poor quality. (2)
[10]
TOTAL: 150

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Physical Sciences/P2 14 NW/September 2014
NSC — Memorandum
PHYSICAL SCIENCES GRADE 12 PAPER 2 ANALYSIS 2015
Knowledge
Taxonom area
. ay
4 7) 2:3 n
a 5 zo a 7)
é = Zo 3a} O38 az} o/2
z Og og ac Fea ze]/ zZzj/H] ww] 2
© we as zs Spo wu] 1/5) ¥] &
8 “¢ 2% <6 3827]s/ &] Si=] Sl e&
3 wi § ug pH) st Siz] 3/9/28] =
ry og 6 Ze a aja §
= a fo} wos 10 & tig J 2
6 uz a2 ES a Fla! Zio}] E] g
S41 =8 ge RSG wl eiz] eo} 3
fe) on Py wt 2 EE] #/@]) Fl so
z ° Zz Ess 3/515
g o Bes =
a >2°o
oF 5
Content E|M/D M;D|E;]MjiD Mj}D Marks
71 | MOLECULAR
: STRUCTURES 2 2
PHYSICAL
1.2 | properties 2 2 2
RATE OF
1.3 | REACTION 2 2 2
TYPES OF
1.4 | Reactions 2 2 2
ACID-BASED
1.5 | REACTION 2 2 2
TYPES OF
1.6 | REACTIONS 2 2 2
REDOX
1.7 | REACTION 2 2 2
RATE OF
1.8 | REACTION 2 2 2
CHEMICAL
1.9 | Equivisrium 2 2 2
ACIDS AND
1.10 | Bases 2 2 | 20
2.1 ISOMERS 2 2 2
2.2 | isomers 2 2
STRUCTURAL
2.3.1 | FORMULAE 2 2 2
ORGANIC
2.3.2 | Propuct 1 1 ul
TYPE OF
2.4 | REACTION 3 3 3
STAUCTURAL
2.5.1 | FORMULAE 1 1 1
STRUCTURAL
2.5.2 | FORMULAE 1 1 1
2.6.1 | IUPAC NAMING 2 2 2
HOMOLOGOUS
2.6.2 | sens 1 1 1 | 1
PHYSICAL
3.1.1 | properties _| 1 1 1
PHYSICAL
3.1.2 | properties | 1 1 1
PHYSICAL
3.1.3 | PROPERTIES 1 1 1
HOMOLOGOUS
3.2 __| series 2 2
GENERAL
3.3 | FORMULAE 2 2 2
PHYSICAL
3.4 _| PROPERTIES 2 2 2
INTERMOLECU
3.5 _| LAR FORCES 5 5 5 | 14

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Physical Sciences/P2

Content E|M

NSC - Memorandum

15

D

NW/September 2015

Marks

414

STRUCTURAL 2
FORMULAE

4.1.2

STRUCTURAL
FORMULAE

4.1.3.

REACTION
CONDITIONS

nN

4.1.4

TYPE OF 2
REACTION

4.2.1

POLYMERS 2

4.2.2

POLYMERS

4.2.3

POLYMERS

MyMPNy

MIM {|My [MY jw [hy

4.3.1

POLYMERS

—

4.3.2

POLYMERS

4.4

POLYMERS

a

18

5.1

ACIDS &
BASES

5.2.1

ACIDS &
BASES

= jp

§.2.2

ACIDS AND
BASES

—

5.3.1

ACIDS &
BASES

5.3.2

ACIDS AND
BASES

5.4.1

ACIDS &
BASES

5.4.2

ACIDS &
BASES

5.5

ACIDS &
BASES

18

6.1

RATE OF
REACTION

6.2.

BALANCING
REACTIONS

6.3

GRAPHS
INTERPRETATI
ONS

6.4

RATE OF
REACTION

6.5

REDOX
REACTIONS

6.6

RATE OF
REACTION

15

7A

APPLICATION
OF
EQUILIBRIUIM

7.2,

APPLICATION
OF
EQUILIBRIUM

7.3.

APPLICATION
OF
EQUILIBRIUM

14

8.1

ELECTROCHE-
MICAL
REACTIONS

8.2

ELECTROCHE-
MICAL.
REACTIONS

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Physical Sciences/P2

16

NSC ~ Memorandum

NW/September 2014

8.3

ELECTROCHE-
MICAL 1
REACTIONS

8.4

ELECTROCHE-
MICAL
REACTIONS

8.5

ELECTROCHE-
MICAL
REACTIONS

8.6

ELECTROCHEMI
STRY
(APPLICATION )

8.7

ELECTROCHEMI
STRY
{APPLICATION )

wo

15

9.1

ELECTROLYSIS

9.2

ELECTROLYTIC
CELLS

9.3

ELECTROLYTIC
CELLS

9.4

ELECTROLYTIC
CELLS

9.5

ELECTROLYTIC
CELLS

NO] mlm] o] wy

11

10.1

ELECTROCHEMI
CAL CELL

w IN IS |S [wo [hw

10.2

ELECTROCHEMI
CAL CELL

ae

10.3

ELECTROCHEMI 2
CAL CELL

10.4

ELECTROCHEMI 1
CAL CELL

—~{ Mls o

10.5

ELECTROCHEMI
CAL CELL

10.6

FERTILISERS 2

10

ACTUAL
MARKS

18%

% ACHIEVED

EXPECTED

MARKS ae

36%

ee

9%

Overall Easy

Medium

Difficult

ACTUAL
MARKS 34

68

48

23%
% ACHIEVED

45%

32%

EXPECTED 30
MARKS ca

40

30

Copyright reserved

60%

7%

100%

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