GR 11 SEP 2023..
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Subject
Chemistry
Date
Nov 24, 2024
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NATIONAL
SENIOR CERTIFICATE
GRADE 11
SEPTEMER
202
3
PHYSICAL SCIENCES
MARKS:
100
TIME:
2
hours
INSTRUCTIONS AND INFORMATION
1.
Write your full NAME and SURNAME in the appropriate spaces in your
ANSWER BOOK.
2.
The question paper consists of EIGHT questions.
Answer ALL the questions.
3.
Start EACH question on a new page in the ANSWER BOOK.
4.
Number your answers correctly according to the numbering system used in this question
paper.
5.
Leave ONE line open between sub-questions, for example QUESTION 2.1 and
QUESTION 2.2.
6.
A non-programmable calculator may be used.
7.
Appropriate mathematical instruments may be used.
8.
You are advised to use the attached DATA SHEETS and the PERIODIC
TABLE.
9.
Shows ALL formulae and institutions in ALL your calculations.
10.
Round off your final numerical answers to a minimum of TWO decimal places.
11.
Wherever motivations, discussions, etc. are required, be brief.
Write neatly and legibly.
QUESTION 1: MULTIPLE-CHOICE QUESTIONS
Four options are provided as possible answers to the following questions.
Each
question has only ONE correct answer.
Write only the correct answer (A−D) next to the question
number (1.1
–
1.5) in the ANSWER BOOK.
1.1
The CORRECT formula for nitric acid:
A
H
2
SO
4
B
CH
3
COOH
C
NH
3
D
HNO
3
(2)
1.2
Which ONE of the reactions below will produce the salt sodium ethanoate
(sodium acetate)?
A
HCℓ(s) + CH
3
COOH(aq)
→
B
CH
3
COOH(aq) + H
2
O(ℓ)
→
C
CH
3
COOH(aq) + NaOH(aq)
→
D
H
2
CO
3
(aq) + NaOH(aq)
→
(2)
1.3
Consider the reaction represented by the equation below:
2Fe(s) + 3CO
2
(g) → Fe
2
O
3
(s) + 2CO(g)
ΔH = + 53,2 kJ
Which ONE of the following statements is TRUE?
For each mole of Fe that reacts, …
A
26,6 kJ of energy are released.
B
26,6 kJ of energy are absorbed.
C 53,2 kJ of energy are released.
D
53,2 kJ of energy are absorbed. (2)
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1.4
10 moles of hydrogen gas (H
2
) and 2,5 moles of nitrogen gas (N
2
) are mixed
and
allowed to react to form ammonia (NH
3
) according to the following balanced
equation:
3H
2
(g) + N
2
(g) → 2NH
3
(g)
If 4 moles of NH
3
(g) is formed during the reaction, the number of moles of H
2
(g) and
N
2
(g) that remain in the container are respectively:
(2)
1.5
Consider the following acid-base reactions:
NH
3
(g)
+
H
2
O(l)
NH
4
+
(aq)
+
OH
-
(aq)
SO
4
2-
(aq)
+
HNO
3
(aq)
HSO
4
-
(aq)
+
NO
3
-
(aq)
The substances acting as proton acceptors in the above reactions are:
A
H
2
O and SO
4
2-
B
NH
3
and SO
4
2-
C
NH
3
and HNO
3
D
H
2
O and HNO
3
(2)
[10]
Moles of H
2
(g)
Moles of N
2
(g)
A
0
0
B
7
1,5
C
4
0,5
D
4
2
QUESTION 2
2.1
Define the term
molar mass
of a substance.
(1)
2.2
Calculate the number of moles of water in 100 g of water.
(3)
2.3 Methyl benzoate is a compound used in the manufacture of perfumes. It is
found that
a 5,325 g sample of methyl benzoate contains 3,758 g of carbon, 0,316 g of
hydrogen and 1,251 g of oxygen.
2.3.1
Define the term
empirical formula
.
(2)
2.3.2
Determine the empirical formula of methyl benzoate.
(7)
2.3.3
If the molar mass of methyl benzoate is 136 gmol
-1
, what is its
molecular formula?
(2)
[15]
QUESTION 3
3.1
Define the term
limiting reactant
.
(2)
3.2 Iron (Fe) reacts with sulphur (S) to form iron sulphide (FeS) according to the
following balanced
equation:
Fe(s) + S(s) → FeS
3.2.1
Calculate which of the two substances will be used up completely if
20 g of Fe and 10 g of S are mixed and heated.
(5)
3.2.2
How many grams of the other substance are in excess?
(2)
3.3 Magnesium burns in air to form magnesium oxide according to the following balanced equation:
2Mg(s) + O
2
(g) → 2MgO(s)
If the
percentage yield
of this reaction is only 80%, calculate the mass of
Magnesium (Mg) that needs to be burned to produce 30 g of magnesium oxide.
(6)
[15]
QUESTION 4
4.1 Limestone, or sometimes ash, is used in pit latrines (long drops) to neutralise acidic waste.
Limestone reacts with hydrochloric acid according to the following UNBALANCED equation:
CaCO
3
(s) + HCℓ(aq) → CaCℓ
2
(aq) + H
2
O(ℓ) + CO
2
(g)
4.1.1
Define an
acid
in terms of the Arrhenius theory.
(2)
4.1.2
Is ash acidic or basic?
(1)
4.1.3
Rewrite the above equation into your ANSWER BOOK and then
balance the equation.
(1)
4.2
Sulphuric acid reacts with water in two steps as represented by the equations below.
Equation
I
:
H
2
SO
4
(aq) + H
2
O(ℓ)
⇌
H
3
O
+
(aq) + HSO
−
4
(aq)
Equation
II
: HSO
−
4
(aq) + H
2
O(ℓ)
⇌
H
3
O
+
(aq) + SO
2
4
−
(aq)
4.2.1 Define the Base in terms of Lowry Bronsted.
(2)
4.2.2
Write down the NAME of the conjugate base of the hydrogen
sulphate ion.
(2)
4.3
A standard sodium carbonate solution is prepared in a 250 cm
3
volumetric flask.
During a titration, 20 cm
3
of a 0,1 mol·dm
-3
nitric acid solution neutralises 25 cm
3
of the
above standard solution according to the following balanced equation:
2HNO
3
(aq) + Na
2
CO
3
(aq) → 2NaNO
3
(aq) + H
2
O(ℓ) + CO
2
(g)
4.3.1
Write down the NAME of the salt formed in the above reaction.
(1)
4.3.2
Calculate the mass of sodium carbonate used to prepare the
standard solution in the volumetric flask.
(5)
[14]
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QUESTION 5
Consider the two acid-base reactions below and answer the questions which follow:
(i)
HCℓ (aq)
+
H
2
O (ℓ)
→
Cℓ
−
(aq)
+ H
3
O
+
(aq)
(ii)
H
2
O (ℓ)
+
NH
3
(aq)
→
NH
4
+
(aq)
+
OH
−
(aq)
5.1
Define the term
ampholyte
and identify the substance which acts as an
ampholyte in the above reactions.
(3)
5.2
Identify the conjugate acid-base pairs in equation (i).
(2)
5.3
In a laboratory, one beaker contains a solution involving reaction (i) and another beaker
contains a solution involving reaction (ii).
A learner wants to test the solutions to determine whether
they are acidic or alkaline.
5.3.1
Define the term STANDARD SOLUTION.
(2)
5.3.2
Which ONE of the two solutions will have a pH below 7?
Give a
reason for your answer.
(3)
5
.4 If HCℓ (g) should react with NH
3
(g) in a sealed container, a salt will be
formed. Give the NAME and FORMULA of the salt that is formed.
(2)
[12]
QUESTION 6
6.1 The decomposition of hydrogen peroxide in the presence of a catalyst at standard
pressure and room temperature is given by the unbalanced chemical equation
below.
H
2
O
2
(aq)
→
H
2
O(ℓ) + O
2
(g)
The oxygen gas is collected and the volume is recorded over a period of time. The
reaction is completed at time
t
.
The results are plotted on a
graph of volume O
2
versus time
, as shown
below.
600
t
Time (s)
Take the
molar gas volume (V
m
) as 24,45 dm
3
at room temperature and
standard
pressure.
6.1.1
Balance the equation.
(2)
6.1.2
How would a catalyst affect the reaction?
(2)
6.1.3
Use the information on the graph to calculate the mass of hydrogen peroxide
that decomposed.
(6)
[10]
QUESTION 7
Plants manufacture their own food through the process of photosynthesis by making use of water,
carbon dioxide and sunlight (energy). The balanced equation for this reaction is:
6CO
2
(g) + 6H
2
O (ℓ)
→
C
6
H
12
O
6
(s) + 6O
2
(g)
∆
H > 0
The food gives the plants (and animals which eat it) energy to perform their daily life functions.
The food is broken down during cellular respiration in the presence of oxygen to release the
energy according to the following equation:
C
6
H
12
O
6
(s) + 6O
2
(g)
→
6CO
2
(g) + 6H
2
O (ℓ)
∆
H < 0
The graph which follows represents the change in potential energy for one of the two reactions
listed above.
A
B
Progress of reaction
7.1
Is the process of photosynthesis an example of an ENDOTHERMIC or EXOTHERMIC
reaction?
Give a reason for your answer.
(2)
7.2
Does the above graph represent the change in potential energy for
PHOTOSYNTHESIS or CELLULAR RESPIRATION?
Briefly explain how you
got to the answer you chose.
(3)
7.3
Supply labels for
A
and
B
which appear on the graph.
(2)
7.4
The reaction for cellular respiration is
catalysed by enzymes
.
Explain how the
Enzymes or catalyst will influence the rate of the reaction.
(2)
[9]
8.1.1
Give an investigative question for this investigation.
(2)
8.1.2
Give a hypothesis for this investigation.
(2)
8.1.3
Name TWO variables which must be constant during this
investigation.
(2)
8.1.4
Calculate the value of
x
on the graph.
(6)
8.1.5
Name and state in words the law that is being investigated here.
(2)
8.1.6
Use the graph above to express this law mathematically.
(1)
(15)
GRAND TOTAL = 100
QUESTION 8
8.1
A group of learners investigated the relationship between the pressure and
volume of an enclosed gas.
The graph of
the
pressure against
the
reciprocal
of volume, which follows, was obtained from the results:
P
)
kPa
(
120
100
x
5
,
3
1
V
(
dm
-
3
)
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