Đề thi Cambridge IGCSE™ chính thức môn Hoá tháng 062023 (Đề tự luận_Số 43_ Nâng cao_Có đáp án)

Cambridge IGCSE™

*9534637521*

CHEMISTRY0620/43
May/June 2023

Paper 4 Theory (Extended)

1 hour 15 minutes


You must answer on the question paper.
No additional materials are needed.

INSTRUCTIONS
● Answer all questions.
● Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
● Write your name, centre number and candidate number in the boxes at the top of the page.
● Write your answer to each question in the space provided.
● Do not use an erasable pen or correction fluid.
● Do not write on any bar codes.
● You may use a calculator.
● You should show all your working and use appropriate units.

INFORMATION
● The total mark for this paper is 80.
● The number of marks for each question or part question is shown in brackets [ ].
● The Periodic Table is printed in the question paper.

This document has 16 pages.

IB23 06_0620_43/2RP
© UCLES 2023

[Turn over


2
1Some symbol equations and word equations, A to J, are shown.


AH+ + OH– → H2O



BCr3+ + 3OH– → Cr(OH)3



C methane + chlorine → chloromethane + hydrogen chloride



D propene + bromine → 1,2-dibromopropane



EC10H22 → C8H18 + C2H4

F



G methane + oxygen → carbon monoxide + water



HC2H5COOH + CH3OH → C2H5COOCH3 + H2O



I



J6CO2 + 6H2O → C6H12O6 + 6O2

chlorine + aqueous potassium bromide → bromine + aqueous potassium chloride

hydrogen + oxygen → water

Use the equations to answer the questions that follow.
Each equation may be used once, more than once, or not at all.
Give the letter, A to J, for the equation which represents:


(a)photosynthesis ��������������������������������������������������������������������������������������������������������������������� [1]

(b)an addition reaction ������������������������������������������������������������������������������������������������������������� [1]



(c)a precipitation reaction �������������������������������������������������������������������������������������������������������� [1]



(d)incomplete combustion �������������������������������������������������������������������������������������������������������� [1]



(e)a displacement reaction ������������������������������������������������������������������������������������������������������� [1]



(f)a substitution reaction. ��������������������������������������������������������������������������������������������������������� [1]



[Total: 6]

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3

Question 2 starts on the next page.

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4
2

(a)The symbols of the elements in Period 3 of the Periodic Table are shown.
Na

Mg

Al

Si

P

S

Cl

Ar

Use the symbols of the elements in Period 3 to answer the questions that follow.

Each symbol may be used once, more than once, or not at all.
Give the symbol of the element that:


(i) is present in purified bauxite ����������������������������������������������������������������������������������������� [1]



(ii)contains atoms with a full outer shell of electrons �������������������������������������������������������� [1]



(iii)is used to kill microbes in water treatment �������������������������������������������������������������������� [1]



(iv)forms an amphoteric oxide ������������������������������������������������������������������������������������������� [1]



(v)forms an oxide which causes acid rain ������������������������������������������������������������������������� [1]



(vi)has an oxidation number of –1 when it forms a compound with hydrogen.



........................................................................................................................................ [1]

(b)The relative atomic masses of elements can be calculated from the relative masses of isotopes
and their percentage abundances.



(i)Identify the isotope to which all relative masses are compared.



........................................................................................................................................ [1]



(ii)Table 2.1 shows the relative masses and the percentage abundances of the two isotopes
in a sample of magnesium.
Table 2.1
relative mass of isotope

percentage abundance of isotope

24

85

26

15

Calculate the relative atomic mass of magnesium to one decimal place.



© UCLES 2023

relative atomic mass = .............................. [2]

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5



(c)An ion contains 10 electrons, 13 protons and 14 neutrons.
(i)State the nucleon number of the ion.




........................................................................................................................................ [1]
(ii)Identify the element that forms this ion.



........................................................................................................................................ [1]



[Total: 11]

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6
3Magnesium forms ionic compounds.



(a) M
 agnesium reacts with fluorine to form the ionic compound magnesium fluoride.
The electronic configurations of an atom of magnesium and an atom of fluorine are shown in
Fig. 3.1.
magnesium atom

fluorine atom

Mg

F

Fig. 3.1


(i) Ions are formed by the transfer of electrons from magnesium atoms to fluorine atoms.

Complete the dot-and-cross diagrams in Fig. 3.2 to show the electronic configurations of
one magnesium ion and one fluoride ion. Show the charges on the ions.
magnesium ion

fluoride ion
.....

Mg

.....
F

Fig. 3.2
[3]


(ii) Deduce the formula of magnesium fluoride.



........................................................................................................................................ [1]



(iii) W
 hen solid magnesium  fluoride is dissolved in water it forms a solution that conducts
electricity.

State one other change that can be made to solid magnesium fluoride to allow it to conduct
electricity.



........................................................................................................................................ [1]

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7



(b)Silicon tetrachloride, SiCl 4, and silicon(IV) oxide, SiO2, are covalent compounds.
Complete the dot-and-cross diagram in Fig.  3.3 to show the electronic configuration in a
molecule of silicon tetrachloride. Show outer shell electrons only.

Cl

Cl

Si

Cl

Cl

Fig. 3.3
[2]


(c)The melting points of silicon tetrachloride and silicon(IV) oxide are shown in Table 3.1.
Table 3.1
melting point / °C



silicon tetrachloride

–69

silicon(IV) oxide

1710

(i)Silicon tetrachloride has a low melting point because it has weak forces of attraction
between particles.

Name the type of particles that are held together by these weak forces of attraction.


........................................................................................................................................ [1]

(ii)Explain, in terms of structure and bonding, why silicon(IV) oxide has a high melting point.



..............................................................................................................................................



..............................................................................................................................................



..............................................................................................................................................



........................................................................................................................................ [2]



[Total: 10]

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8
4Hydrogen is produced by the reaction between zinc and dilute sulfuric acid, H2SO4.
Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g)


(a)A student carries out an experiment using excess zinc and dilute sulfuric acid.

The student measures the volume of hydrogen produced at regular time intervals using the
apparatus shown in Fig. 4.1.
Lumps of zinc are used.

gas syringe
lumps of zinc

dilute sulfuric acid

Fig. 4.1
The rate of reaction decreases as the reaction progresses. The rate eventually becomes zero.


(i)Explain why the rate of reaction decreases as the reaction progresses.



..............................................................................................................................................



........................................................................................................................................ [1]

(ii)Explain why the rate of reaction eventually becomes zero.



..............................................................................................................................................



........................................................................................................................................ [1]


(b)The experiment is repeated using powdered zinc instead of lumps of zinc.
All other conditions remain the same.
Explain, in terms of collision theory, why the rate of reaction increases if powdered zinc is used.


.....................................................................................................................................................



.....................................................................................................................................................



............................................................................................................................................... [2]

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9


(c)The equation for the reaction is shown.
Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g)

25.0  cm3 of 2.00 mol / dm3 H2SO4(aq) is added to excess zinc.
Calculate the volume of H2 formed at room temperature and pressure (r.t.p.). The volume of
one mole of any gas is 24 dm3 at r.t.p.
Use the following steps.
●

Calculate the number of moles of H2SO4 used.



.............................. mol
●

Deduce the number of moles of H2 produced.



.............................. mol
●

Calculate the volume of H2 formed at r.t.p.


.............................. dm3
[3]



(d)Hydrogen can also be produced by the reaction of zinc with dilute hydrochloric acid.
(i)Write a symbol equation for this reaction.




........................................................................................................................................ [2]
(ii)State the test for hydrogen gas.

test .......................................................................................................................................

positive result .......................................................................................................................
[1]


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[Total: 10]

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10
5This question is about electricity and chemical reactions.

(a)Aqueous copper(II) sulfate is an electrolyte.
The electrolysis of aqueous copper(II) sulfate using inert electrodes forms:
● copper at the cathode
● oxygen at the anode.


(i)State what is meant by the term electrolyte.



..............................................................................................................................................



........................................................................................................................................ [2]



(ii)State the term given to the Roman numeral, (II), in the name copper(II) sulfate.



........................................................................................................................................ [1]

(iii)State what happens to the colour of the aqueous copper(II) sulfate as this electrolysis
progresses.



........................................................................................................................................ [1]



(iv)Write an ionic half-equation for the formation of copper at the cathode.




........................................................................................................................................ [2]
(v)Give the formula of the ion that forms oxygen at the anode.




........................................................................................................................................ [1]
(b)The electrolysis of aqueous copper(II) sulfate is repeated using copper electrodes.

State what happens to the anode.


............................................................................................................................................... [1]

(c)Spoons can be electroplated with silver.



(i)Name the substances used as:



the anode (positive electrode) .............................................................................................



the cathode (negative electrode) .........................................................................................


the electrolyte. .....................................................................................................................
[3]


(ii)State two reasons why spoons are electroplated.

1 ...........................................................................................................................................
2 ...........................................................................................................................................
[2]
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11

(d)Hydrogen–oxygen fuel cells can be used to produce electricity to power cars.
Petrol produces carbon dioxide and carbon monoxide when it powers cars.


(i)State one adverse effect of carbon dioxide and carbon monoxide.



carbon dioxide .....................................................................................................................


carbon monoxide .................................................................................................................
[2]


(ii)State one disadvantage, other than cost, of using hydrogen–oxygen fuel cells to power
cars compared to using petrol.



........................................................................................................................................ [1]



[Total: 16]

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12
6This question is about nitrogen and compounds of nitrogen.
(a)
Ammonia is manufactured by the reaction between nitrogen and hydrogen in the Haber
process.
The equation is shown.



N2(g) + 3H2(g)


(i)State the source of nitrogen for the Haber process.




........................................................................................................................................ [1]
(ii)State the source of hydrogen for the Haber process.




2NH3(g)

........................................................................................................................................ [1]

(iii)State the typical conditions used in the Haber process.

temperature .......................................... °C
pressure ................................................ atm
[2]


(iv)Name the catalyst used in the Haber process.




........................................................................................................................................ [1]
(v)State what is meant by the term catalyst.



..............................................................................................................................................



........................................................................................................................................ [2]





(b)Ammonia is converted into nitric acid.
(i) T
 he first stage is the conversion of ammonia into nitrogen monoxide, NO.

The equation is shown.
4NH3(g) + 5O2(g)

4NO(g) + 6H2O(g)

The reaction is carried out at a temperature of 900 °C and a pressure of 7 atm.
The forward reaction is exothermic.
Using explanations that do not involve cost:
●


explain why a temperature less than 900 °C is not used

..............................................................................................................................................
●

explain why a pressure greater than 7 atm is not used.


..............................................................................................................................................
[2]

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13

(ii)In the second stage, nitrogen monoxide reacts with water and oxygen to produce nitric acid.

Balance the symbol equation for the reaction.


.....NO + .....O2 + .....H2O → .....HNO3[1]



(c)A student makes aqueous copper(II) nitrate by adding an excess of solid copper(II) carbonate
to dilute nitric acid.



(i)Write the symbol equation for this reaction.




........................................................................................................................................ [2]
(ii)State two observations that indicate the copper(II) carbonate is in excess.

1 ...........................................................................................................................................
2 ...........................................................................................................................................
[2]


(iii)Name one compound, other than copper(II) carbonate, that can be added to dilute
nitric acid to produce aqueous copper(II) nitrate.

........................................................................................................................................ [1]



[Total: 15]

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14
7This question is about organic compounds.


(a)Propane and chlorine react at room temperature. An equation for the reaction is shown.
C3H8 + Cl 2 → C3H7Cl + HCl



(i)State the condition required for this reaction.




........................................................................................................................................ [1]

(ii)Draw the displayed formulae of two structural isomers with the formula C3H7Cl.

[2]



(b)Alkenes are a homologous series of hydrocarbons.
(i)State two characteristics that all members of the same homologous series have in
common.

1 ...........................................................................................................................................
2 ...........................................................................................................................................
[2]


(ii)Addition polymers are made from alkenes.

Complete Fig. 7.1 to show one repeat unit of the addition polymer formed from but-2-ene.

C

C

Fig. 7.1
[2]

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15

(c)A repeat unit of a condensation polymer is shown in Fig. 7.2.
The polymer is made from two monomers.
O
C

O
CH2

C

O

CH2CH2

O

Fig. 7.2


(i)Draw the structures of the monomers used to produce the polymer in Fig. 7.2.

[2]


(ii)Name the type of condensation polymer in Fig. 7.2.

........................................................................................................................................ [1]
(iii)Name the two homologous series to which the monomers in (i) belong.

1 ...........................................................................................................................................
2 ...........................................................................................................................................
[2]


[Total: 12]

Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of Cambridge Assessment. Cambridge Assessment is the brand name of the University of Cambridge
Local Examinations Syndicate (UCLES), which is a department of the University of Cambridge.

© UCLES 2023

0620/43/M/J/23


© UCLES 2023

12

V

Cr

Mn

Co

27

Ni

28

Cu

29

Zn

30

Fe

57–71

56

55

0620/43/M/J/23

–

90

89

232

thorium

actinium

–

Th

Ac

140

cerium

139

lanthanum

59

231

protactinium

Pa

91

141

praseodymium

Pr

–

58

Ce

–

Db

dubnium

Rf

rutherfordium

La

57

actinoids

105

181

Ta

tantalum

73

93

niobium

Nb

41

51

vanadium

238

uranium

U

92

144

neodymium

60

Nd

–

Sg
seaborgium

106

184

W
tungsten

74

96

molybdenum

Mo

42

52

chromium

–

neptunium

Np

93

–

promethium

61

Pm

–

Bh
bohrium

107

186

Re
rhenium

75

–

technetium

Tc

43

55

manganese

–

plutonium

Pu

94

150

samarium

62

Sm

–

Hs
hassium

108

190

Os
osmium

76

101

ruthenium

Ru

44

56

iron

–

americium

Am

95

152

europium

63

Eu

–

Mt
meitnerium

109

192

Ir

iridium

77

103

rhodium

Rh

45

59

cobalt

–

curium

Cm

96

157

gadolinium

64

Gd

–

Ds
darmstadtium

110

195

Pt
platinum

78

106

palladium

Pd

46

59

nickel

The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).

actinoids

lanthanoids

–

Ra

radium

Fr

francium

89–103

178

104

137

88

133

87

Hf

hafnium

Ba

barium

lanthanoids

Cs

72

91

zirconium

Zr

40

48

titanium

caesium

89

yttrium

88

strontium

85

rubidium

Y

39

45

Sr

38

40

Ca

Rb

37

39

K

scandium

–

berkelium

Bk

97

159

terbium

65

Tb

–

Rg
roentgenium

111

197

gold

Au

79

108

silver

Ag

47

64

copper

–

californium

Cf

98

163

dysprosium

66

Dy

–

Cn
copernicium

112

201

Hg
mercury

80

112

cadmium

Cd

48

65

zinc

calcium

Ti

26

potassium

Sc

25

31

24

–

einsteinium

Es

99

165

holmium

67

Ho

–

Nh
nihonium

113

204

Tl
thallium

81

115

indium

In

49

70

gallium

Ga

27

20

24

19

23

aluminium

Al

13

11

boron

magnesium

23

1

sodium

22

B

C

N

7

O

8

VI

F

9

VII

2

VIII

–

fermium

Fm

100

167

erbium

68

Er

–

Fl

flerovium

114

207

lead

Pb

82

tin

119

Sn

50

73

germanium

Ge

32

28

silicon

Si

14

12

carbon

–

mendelevium

Md

101

169

thulium

69

Tm

–

Mc
moscovium

115

209

Bi
bismuth

83

122

antimony

Sb

51

75

arsenic

As

33

31

phosphorus

P

15

14

nitrogen

–

nobelium

No

102

173

ytterbium

70

Yb

–

Lv
livermorium

116

–

Po
polonium

84

128

tellurium

Te

52

79

selenium

Se

34

32

sulfur

S

16

16

oxygen

–

Lr

lawrencium

103

175

lutetium

71

Lu

–

Ts
tennessine

117

–

At
astatine

85

127

iodine

I

53

80

bromine

Br

35

35.5

chlorine

Cl

17

19

fluorine

–

Og
oganesson

118

–

Rn
radon

86

131

xenon

54

Xe

84

krypton

36

Kr

40

argon

18

Ar

20

neon

Ne

10

4

helium

6

V

hydrogen

5

IV

He

Mg

21

relative atomic mass

name

atomic symbol

atomic number

Key

III

H

1

Group

Na

9

11

7

Be

beryllium

Li

4

3

lithium

II

I

The Periodic Table of Elements

16


Cambridge IGCSE™
CHEMISTRY

0620/43

Paper 4 Theory (Extended)

May/June 2023

MARK SCHEME
Maximum Mark: 80

Published

This mark scheme is published as an aid to teachers and candidates, to indicate the requirements of the
examination. It shows the basis on which Examiners were instructed to award marks. It does not indicate the
details of the discussions that took place at an Examiners’ meeting before marking began, which would have
considered the acceptability of alternative answers.
Mark schemes should be read in conjunction with the question paper and the Principal Examiner Report for
Teachers.
Cambridge International will not enter into discussions about these mark schemes.
Cambridge International is publishing the mark schemes for the May/June 2023 series for most

Cambridge IGCSE, Cambridge International A and AS Level and Cambridge Pre-U components, and some
Cambridge O Level components.

This document consists of 11 printed pages.
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Cambridge IGCSE – Mark Scheme
PUBLISHED
Generic Marking Principles

May/June 2023

These general marking principles must be applied by all examiners when marking candidate answers. They should be applied alongside the
specific content of the mark scheme or generic level descriptors for a question. Each question paper and mark scheme will also comply with these
marking principles.
GENERIC MARKING PRINCIPLE 1:
Marks must be awarded in line with:




the specific content of the mark scheme or the generic level descriptors for the question
the specific skills defined in the mark scheme or in the generic level descriptors for the question
the standard of response required by a candidate as exemplified by the standardisation scripts.

GENERIC MARKING PRINCIPLE 2:
Marks awarded are always whole marks (not half marks, or other fractions).
GENERIC MARKING PRINCIPLE 3:
Marks must be awarded positively:






marks are awarded for correct/valid answers, as defined in the mark scheme. However, credit is given for valid answers which go beyond
the scope of the syllabus and mark scheme, referring to your Team Leader as appropriate
marks are awarded when candidates clearly demonstrate what they know and can do
marks are not deducted for errors
marks are not deducted for omissions
answers should only be judged on the quality of spelling, punctuation and grammar when these features are specifically assessed by the
question as indicated by the mark scheme. The meaning, however, should be unambiguous.

GENERIC MARKING PRINCIPLE 4:
Rules must be applied consistently, e.g. in situations where candidates have not followed instructions or in the application of generic level
descriptors.

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Cambridge IGCSE – Mark Scheme

PUBLISHED

May/June 2023

GENERIC MARKING PRINCIPLE 5:
Marks should be awarded using the full range of marks defined in the mark scheme for the question (however; the use of the full mark range may
be limited according to the quality of the candidate responses seen).
GENERIC MARKING PRINCIPLE 6:
Marks awarded are based solely on the requirements as defined in the mark scheme. Marks should not be awarded with grade thresholds or
grade descriptors in mind.

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Cambridge IGCSE – Mark Scheme
PUBLISHED

May/June 2023

Science-Specific Marking Principles
1

Examiners should consider the context and scientific use of any keywords when awarding marks. Although keywords may be present, marks
should not be awarded if the keywords are used incorrectly.

2

The examiner should not choose between contradictory statements given in the same question part, and credit should not be awarded for
any correct statement that is contradicted within the same question part. Wrong science that is irrelevant to the question should be ignored.

3

Although spellings do not have to be correct, spellings of syllabus terms must allow for clear and unambiguous separation from other
syllabus terms with which they may be confused (e.g. ethane / ethene, glucagon / glycogen, refraction / reflection).

4

The error carried forward (ecf) principle should be applied, where appropriate. If an incorrect answer is subsequently used in a scientifically
correct way, the candidate should be awarded these subsequent marking points. Further guidance will be included in the mark scheme
where necessary and any exceptions to this general principle will be noted.

5

‘List rule’ guidance
For questions that require n responses (e.g. State two reasons …):






The response should be read as continuous prose, even when numbered answer spaces are provided.
Any response marked ignore in the mark scheme should not count towards n.
Incorrect responses should not be awarded credit but will still count towards n.
Read the entire response to check for any responses that contradict those that would otherwise be credited. Credit should not be
awarded for any responses that are contradicted within the rest of the response. Where two responses contradict one another, this

should be treated as a single incorrect response.
Non-contradictory responses after the first n responses may be ignored even if they include incorrect science.

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0620/43
6

Cambridge IGCSE – Mark Scheme
PUBLISHED

May/June 2023

Calculation specific guidance
Correct answers to calculations should be given full credit even if there is no working or incorrect working, unless the question states ‘show
your working’.
For questions in which the number of significant figures required is not stated, credit should be awarded for correct answers when rounded
by the examiner to the number of significant figures given in the mark scheme. This may not apply to measured values.
For answers given in standard form (e.g. a  10n) in which the convention of restricting the value of the coefficient (a) to a value between 1
and 10 is not followed, credit may still be awarded if the answer can be converted to the answer given in the mark scheme.
Unless a separate mark is given for a unit, a missing or incorrect unit will normally mean that the final calculation mark is not awarded.
Exceptions to this general principle will be noted in the mark scheme.

7

Guidance for chemical equations
Multiples / fractions of coefficients used in chemical equations are acceptable unless stated otherwise in the mark scheme.

State symbols given in an equation should be ignored unless asked for in the question or stated otherwise in the mark scheme.

© UCLES 2023

Page 5 of 11


0620/43

Cambridge IGCSE – Mark Scheme
PUBLISHED

Question

Answer

May/June 2023
Marks

1(a)

J

1

1(b)

D

1

1(c)

B

1

1(d)

G

1

1(e)

F

1

1(f)

C

1

Question

Answer

Marks

2(a)(i)

Al

1

2(a)(ii)

Ar

1

2(a)(iii)

Cl

1

2(a)(iv)

Al

1

2(a)(v)

S

1

2(a)(vi)

Cl

1

2(b)(i)

12C

1

2(b)(ii)

M1 24  85(%) + 26  15(%)

2

M2 2430 / 100 = 24.3
2(c)(i)

27

1

2(c)(ii)

Aluminium / Al

1

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Page 6 of 11


0620/43

Cambridge IGCSE – Mark Scheme
PUBLISHED

Question
3(a)(i)

Answer
M1 eight crosses in second shell of Mg

May/June 2023
Marks
3

M2 7 dots and 1 cross in second shell of F
M3 ‘2+’ charge on Mg ion on correct answer line
and ‘–‘ charge on F ion on correct answer line
3(a)(ii)

MgF2

1

3(a)(iii)

melting

1

M1 4 dot and cross single bonds

2

3(b)

M2 3 pairs of non-bonding e on each Cl and no non-bonding e on Si
3(c)(i)

molecule(s)

1

3(c)(ii)

M1 covalent bonds

2

M2 strong bonds
and
giant (covalent) structure

Question
4(a)(i)

Answer

Marks
1

concentration (of sulfuric acid particles) decreases
OR
frequency of collisions between particles decreases

4(a)(ii)

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all the (sulfuric) acid has reacted

1

Page 7 of 11


0620/43

Cambridge IGCSE – Mark Scheme
PUBLISHED

Question
4(b)

Answer
M1 greater surface area (of zinc)

May/June 2023
Marks
2

M2 frequency of collisions between (zinc and acid) particles increases
4(c)

3

M1 mol H2SO4 = 2.00 x 25.0/1000 = 0.05(00)
M2 mol H2 = M1 = 0.05(00)
M3 vol H2 = M2  24 = 1.2(0)

4(d)(i)

Zn + 2HCl → ZnCl2 + H2
M1 ZnCl2
M2 equation correct

2

4(d)(ii)

lighted splint and (squeaky) pop

1

Question
5(a)(i)

Answer
M1 ionic compound

Marks
2

M2 molten and / or aqueous
5(a)(ii)

oxidation number (of copper)

1

5(a)(iii)

fades / (becomes) colourless

1

5(a)(iv)

Cu2+ + 2e → Cu

2

M1 Cu2+ and (any number of) e on left hand side

M2 equation correct
5(a)(v)
5(b)
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OH–

1

anode dissolves

1
Page 8 of 11


0620/43

Cambridge IGCSE – Mark Scheme
PUBLISHED

Question
5(c)(i)

Answer
M1 silver

May/June 2023
Marks
3

M2 spoon
M3 (aqueous or solution) of silver nitrate
5(c)(ii)

M1 prevent corrosion

2

M2 improve appearance
5(d)(i)

M1 carbon dioxide: (increased) global warming

2

M2 carbon monoxide: toxic
5(d)(ii)

needs high pressure to store hydrogen

1

Question

Answer

Marks

6(a)(i)

air

1

6(a)(ii)

methane

1

6(a)(iii)

M1 450 (°C)
M2 200 (atm)

2

6(a)(iv)

iron

1

6(a)(v)

M1 (a substance which) increases the rate of a reaction

2

M2 remains unchanged at the end of the reaction

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