Cambridge IGCSE Chemistry (9-1) 0971 — 2020 May/June Paper 2 · Variant 2

Question 1

1 A mixture of ice and water is left to stand and the ice melts. Which row describes what happens as the ice is melting? temperature of mixture energy changes A increases average kinetic energy of particles increases B increases energy is used to overcome attractive forces C stays the same average kinetic energy of particles increases D stays the same energy is used to overcome attractive forces

Accepted Answer

D

Question 2

2 Which piece of apparatus is used to measure 25.0 cm3 of aqueous sodium hydroxide? A B C D

Accepted Answer

D

Question 3

3 Paper chromatography is used to determine the Rf values for four different food colourings. Which food colouring has an Rf value of 0.6? solvent front 25 20 15 distance / cm 10 5 baseline 0 A B C D

Accepted Answer

C

Question 4

4 The diagram shows the electronic structure of a particle with a nucleon number (mass number) of 40. e e e e e e e e e e e 40 e e e e e e e The table shows the suggestions that three students, 1, 2 and 3, made to identify the particle. student 1 2 3 particle Ar Cl Ca2+ Which students are correct? A 1 and 2 only B 1 and 3 only C 2 and 3 only D 1, 2 and 3

Accepted Answer

B

Question 5

5 The electronic structures of two atoms, P and Q, are shown. P Q P and Q combine together to form a compound. What is the type of bonding in the compound and what is the formula of the compound? type of bonding formula A ionic PQ B ionic PQ2 C covalent PQ2 D covalent PQ

Accepted Answer

A

Question 6

6 Which statement about the structure of a metal explains why metals are malleable? A The electrons can move freely throughout the lattice. B The layers of metal ions can slide over each other. C The metal ions are positively charged. D There is a strong force of attraction between the metal ions and the electrons.

Accepted Answer

B

Question 7

7 The bonding, structure and melting point of sodium chloride and sulfur dichloride are shown. compound bonding structure melting point / °C sodium chloride ionic giant lattice 801 sulfur dichloride covalent simple molecular –121 Why does sulfur dichloride have a lower melting point than sodium chloride? A The covalent bonds in sulfur dichloride are weaker than the attractive forces between molecules in sodium chloride. B The covalent bonds in sulfur dichloride are weaker than the ionic bonds in sodium chloride. C The attractive forces between molecules in sulfur dichloride are weaker than the attractive forces between molecules in sodium chloride. D The attractive forces between molecules in sulfur dichloride are weaker than the ionic bonds in sodium chloride.

Accepted Answer

D

Question 8

8 Lead(II) nitrate, Pb(NO3)2, reacts with potassium iodide, KI, to form a yellow precipitate, PbI2, and a soluble salt, KNO3. What is the equation for the reaction? A Pb(NO3)2  +  KI  →  PbI2  +  KNO3 B Pb(NO3)2  +  2KI  →  PbI2  +  KNO3 C 2Pb(NO3)2  +  2KI  →  PbI2  +  2KNO3 D Pb(NO3)2  +  2KI  →  PbI2  +  2KNO3

Accepted Answer

D

Question 9

9 The Haber process is a reversible reaction. N2(g)  +  3H2(g) 2NH3(g) The reaction has a 30% yield of ammonia. Which volume of ammonia gas, NH3, measured at room temperature and pressure, is obtained by reacting 0.75 moles of hydrogen with excess nitrogen? A 3600 cm3 B 5400 cm3 C 12 000 cm3 D 18 000 cm3

Accepted Answer

A

Question 10

10 Electrolytes can be broken down by electrolysis. Which rows are correct for each electrolyte? reaction product electrolyte at cathode at anode 1 dilute aqueous sodium chloride 2H+  +  2e–  →  H2 oxygen 2 concentrated hydrochloric acid 2H+  +  2e–  →  H2 chlorine 3 molten aluminium oxide 2O2–  →  O2  +  4e– aluminium 4 concentrated aqueous sodium bromide Na+  +  e–  →  Na bromine A 1 and 2 B 1 and 4 C 2 and 3 D 3 and 4

Accepted Answer

A

Question 11

11 The electrolysis of aqueous copper(II) sulfate, using inert electrodes, is shown. + – aqueous copper(II) sulfate Which statement about a reaction at an electrode is correct? A Copper ions gain electrons at the negative electrode. B Copper ions gain electrons at the positive electrode. C Hydrogen ions gain electrons at the negative electrode. D Hydrogen ions gain electrons at the positive electrode.

Accepted Answer

A

Question 12

12 Methane burns in excess oxygen. The equation is shown. CH4(g)  +  2O2(g)  →  CO2(g)  +  2H2O(g) Bond energies are shown. bond energy bond / kJ mol–1 C=O 805 C–H 410 O=O 496 O–H 460 What is the energy change for the reaction? A (4 × 410 + 2 × 496) – (2 × 805 + 4 × 460) B (2 × 805 + 2 × 460) – (410 + 2 × 496) C (410 + 2 × 496) – (805 + 2 × 460) D (410 + 496) – (805 + 460)

Accepted Answer

A

Question 13

13 Which statements about hydrogen fuel cells are correct? 1 Water is formed as the only waste product. 2 Both water and carbon dioxide are formed as waste products. 3 The overall reaction is  2H2  +  O2  →  2H2O. 4 The overall reaction is endothermic. A 1 and 3 B 1 and 4 C 2 and 3 D 2 and 4

Accepted Answer

A

Question 14

14 Which list contains only chemical changes? A melting, evaporating, dissolving B rusting, freezing, subliming C neutralisation, polymerisation, combustion D boiling, condensing, distillation

Accepted Answer

C

Question 15

15 The results of adding excess marble chips (calcium carbonate) to hydrochloric acid at 50 °C and at 30 °C are shown. Only the temperature is changed. 50 °C volume of 30 °C carbon dioxide given off / cm3 0 0 time / s Which row describes the reacting particles at 30 °C compared to those at 50 °C? collision rate collision energy A higher higher B higher lower C lower higher D lower lower

Accepted Answer

D

Question 16

16 Methane reacts with steam and an equilibrium is reached. CH4(g)  +  H2O(g) CO(g)  +  3H2(g) The forward reaction is endothermic. Which row shows how the amount of hydrogen at equilibrium changes when the pressure or temperature is changed as indicated? change in change in amount of temperature pressure hydrogen A decrease no change increase B increase no change decrease C no change increase decrease D no change decrease decrease

Accepted Answer

C

Question 17

17 When aqueous iron(III) chloride is added to aqueous potassium iodide a chemical reaction occurs and iodine is formed. Which statement is correct? A Iodide ions are oxidised, they gain electrons in this reaction. B Iodide ions are oxidised, they lose electrons in this reaction. C Iron(III) chloride is oxidised in this reaction. D Neither iodide ions nor iron(III) chloride is oxidised in this reaction.

Accepted Answer

B

Question 18

18 The graph shows how the pH of a solution changes as an acid is added to an alkali. acid  +  alkali  →  salt  +  water Which letter represents the area of the graph where both acid and salt are present? A 14 B C pH 7 D 0 volume of acid added

Accepted Answer

D

Question 19

19 Which statement describes a weak acid? A It is a proton acceptor and is fully ionised in aqueous solution. B It is a proton acceptor and is partially ionised in aqueous solution. C It is a proton donor and is fully ionised in aqueous solution. D It is a proton donor and is partially ionised in aqueous solution.

Accepted Answer

D

Question 20

20 The apparatus shown is used to prepare aqueous copper(II) sulfate. filter paper stirrer excess of solid X solid X Y aqueous copper(II) sulfate heat What are X and Y? X Y A copper aqueous iron(II) sulfate B copper(II) chloride dilute sulfuric acid C copper(II) oxide dilute sulfuric acid D sulfur aqueous copper(II) chloride

Accepted Answer

C

Question 21

21 Which process is not used in the preparation of an insoluble salt? A filtration B washing C crystallisation D drying

Accepted Answer

C

Question 22

22 Which statement about Group I and Group VII elements is correct? A Group VII elements are monoatomic non-metals. B Lithium is more reactive with water than caesium. C The melting points of Group I metals increase down the group. D Potassium bromide reacts with chlorine to produce an orange solution.

Accepted Answer

D

Question 23

23 The properties of the element titanium, Ti, can be predicted from its position in the Periodic Table.

Which row identifies the properties of titanium?

forms coloured
compounds

can be used conducts electricity
as a catalyst when solid

has low density

v v x

v v v
v x v
x v v

Accepted Answer

B

Question 24

24 Which diagram shows a mixture of noble gases? A B C D

Accepted Answer

A

Question 25

25 Which property is shown by all metals? A They are extracted from their ores by heating with carbon. B They conduct electricity. C They form acidic oxides. D They react with hydrochloric acid to form hydrogen.

Accepted Answer

B

Question 26

26 Many metal carbonates decompose when they are heated. Which row describes what happens when potassium carbonate, calcium carbonate and copper(II) carbonate are heated using a Bunsen burner? decomposes does not decompose at decomposes easily with difficulty Bunsen temperatures A calcium carbonate copper(II) carbonate potassium carbonate B copper(II) carbonate calcium carbonate potassium carbonate C copper(II) carbonate potassium carbonate calcium carbonate D potassium carbonate calcium carbonate copper(II) carbonate

Accepted Answer

B

Question 27

27 Molten iron from the blast furnace contains impurities. The process of turning the impure iron into steel involves blowing oxygen into the molten iron and adding calcium oxide. What are the reasons for blowing in oxygen and adding calcium oxide? blowing in oxygen adding calcium oxide A carbon is removed by reacting with oxygen reacts with acidic impurities making slag B carbon is removed by reacting with oxygen reacts with slag and so removes it C iron reacts with the oxygen reacts with acidic impurities making slag D iron reacts with the oxygen reacts with slag and so removes it

Accepted Answer

A

Question 28

28 Four iron nails are added to four different metal sulfate solutions. In which solution does a displacement reaction occur? A copper(II) sulfate B magnesium sulfate C sodium sulfate D zinc sulfate

Accepted Answer

A

Question 29

29 Which statement about pure water is not correct? A It condenses at 100 °C. B It freezes at 0 °C. C It turns cobalt(II) chloride paper blue. D It turns anhydrous copper(II) sulfate blue.

Accepted Answer

C

Question 30

30 Three processes in the carbon cycle are shown. 1 Methane reacts with oxygen producing carbon dioxide and water. 2 Carbon dioxide and water are absorbed and used by plants to make oxygen. 3 Oxygen is used by living things to release energy. Which processes have taken place? 1 2 3 A combustion photosynthesis respiration B combustion respiration photosynthesis C photosynthesis combustion respiration D respiration photosynthesis combustion

Accepted Answer

A

Question 31

31 In the Haber process, nitrogen and hydrogen are reacted to make ammonia. N2(g)  +  3H2(g) 2NH3(g) The forward reaction is exothermic. Which conditions produce the maximum yield of ammonia? pressure temperature A high high B high low C low high D low low

Accepted Answer

B

Question 32

32 Which process, used to prevent iron from rusting, involves sacrificial protection? A alloying B electroplating C galvanising D painting

Accepted Answer

C

Question 33

33 A student suggests three uses of calcium carbonate (limestone). 1 manufacture of cement 2 manufacture of iron 3 treating alkaline soils Which suggestions are correct? A 1 and 2 only B 1 and 3 only C 2 and 3 only D 1, 2 and 3

Accepted Answer

A

Question 34

34 One of the reactions used in the manufacture of sulfuric acid is shown. 2SO2  +  O2 2SO3 Which catalyst is used to increase the rate of this reaction? A iron B manganese(IV) oxide C vanadium(V) oxide D nickel

Accepted Answer

C

Question 35

35 Ethanol is made on an industrial scale by the fermentation of sugars or by the reaction of ethene with steam in the presence of a suitable catalyst. What is a disadvantage of making ethanol from ethene rather than by fermentation? A A continuous production process is used. B A non-renewable raw material is used. C The product is very pure. D The rate of reaction is very high.

Accepted Answer

B

Question 36

36 Which statement about compounds in the same homologous series is correct? A They have the same chemical properties because they have the same number of carbon atoms. B They have the same physical properties because they have the same number of carbon atoms. C They have different chemical properties because they have different numbers of carbon atoms. D They have different physical properties because they have different numbers of carbon atoms.

Accepted Answer

D

Question 37

37 Increasing the number of atoms in one molecule of a hydrocarbon increases the amount of energy released when it burns. What is the correct order? less energy more energy released released A ethene ethane methane B ethene methane ethane C methane ethane ethene D methane ethene ethane

Accepted Answer

D

Question 38

38 An organic compound, P, reacts with zinc to produce a gas, Q. What are P and Q? P Q A ethanoic acid carbon dioxide B ethanoic acid hydrogen C ethanol carbon dioxide D ethanol hydrogen

Accepted Answer

B

Question 39

39 Alkanes undergo substitution reactions in the presence of UV light. Which equation represents a substitution reaction of ethane? A C2H6  +  Cl 2  →  C2H4  +  2HCl B C2H6  +  Cl 2  →  C2H5Cl  +  HCl C C2H6  +  Cl 2  →  C2H4Cl 2  +  H2 D C2H6  +  HCl  →  C2H5Cl  +  H2

Accepted Answer

B

Question 40

40 Which substances are natural polymers? 1 proteins 2 carbohydrates 3 nylon 4 poly(ethene) A 1 and 2 B 1 and 3 C 2 and 3 D 3 and 4

Accepted Answer

A

Question paper16 pages

Mark scheme3 pages

Questions as text

Q1 · A mixture of ice and water is left to stand and the ice melts

Q2 · Which piece of apparatus is used to measure 25.0 cm3 of aqueous sodium hydroxide?

Q3 · Paper chromatography is used to determine the Rf values for four different food colourings

Q4 · The diagram shows the electronic structure of a particle with a nucleon number (mass…

Q5 · The electronic structures of two atoms, P and Q, are shown

Q6 · Which statement about the structure of a metal explains why metals are malleable?

Q7 · The bonding, structure and melting point of sodium chloride and sulfur dichloride are…

Q8 · Lead(II) nitrate, Pb(NO3)2, reacts with potassium iodide, KI, to form a yellow…

Q9 · The Haber process is a reversible reaction

Q10 · Electrolytes can be broken down by electrolysis

Q11 · The electrolysis of aqueous copper(II) sulfate, using inert electrodes, is shown

Q12 · Methane burns in excess oxygen

Q13 · Which statements about hydrogen fuel cells are correct?

Q14 · Which list contains only chemical changes?

Q15 · The results of adding excess marble chips (calcium carbonate) to hydrochloric acid at 50…

Q16 · Methane reacts with steam and an equilibrium is reached

Q17 · When aqueous iron(III) chloride is added to aqueous potassium iodide a chemical reaction…

Q18 · The graph shows how the pH of a solution changes as an acid is added to an alkali

Q19 · Which statement describes a weak acid?

Q20 · The apparatus shown is used to prepare aqueous copper(II) sulfate

Q21 · Which process is not used in the preparation of an insoluble salt?

Q22 · Which statement about Group I and Group VII elements is correct?

Q23 · The properties of the element titanium, Ti, can be predicted from its position in the…

Q24 · Which diagram shows a mixture of noble gases?

Q25 · Which property is shown by all metals?

Q26 · Many metal carbonates decompose when they are heated

Q27 · Molten iron from the blast furnace contains impurities

Q28 · Four iron nails are added to four different metal sulfate solutions

Q29 · Which statement about pure water is not correct?

Q30 · Three processes in the carbon cycle are shown

Q31 · In the Haber process, nitrogen and hydrogen are reacted to make ammonia

Q32 · Which process, used to prevent iron from rusting, involves sacrificial protection?

Q33 · A student suggests three uses of calcium carbonate (limestone)

Q34 · One of the reactions used in the manufacture of sulfuric acid is shown

Q35 · Ethanol is made on an industrial scale by the fermentation of sugars or by the reaction…

Q36 · Which statement about compounds in the same homologous series is correct?

Q37 · Increasing the number of atoms in one molecule of a hydrocarbon increases the amount of…

Q38 · An organic compound, P, reacts with zinc to produce a gas, Q

Q39 · Alkanes undergo substitution reactions in the presence of UV light

Q40 · Which substances are natural polymers?

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