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

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 should be used to measure exactly 21.4 cm3 of water? A 25 cm3 beaker B 25 cm3 pipette C 50 cm3 burette D 50 cm3 measuring cylinder

Accepted Answer

C

Question 3

3 The chromatogram for an unknown dye is shown. solvent front 12 cm 15 cm 9 cm 2 cm What is the Rf value of the dye? A 0.60 B 0.64 C 0.75 D 0.82

Accepted Answer

C

Question 4

4 The atomic number and nucleon number of a potassium atom are shown. potassium atom atomic number 19 nucleon number 39 How many protons, neutrons and electrons are in a potassium ion, K+? protons neutrons electrons A 19 20 18 B 19 20 20 C 20 19 18 D 20 19 19

Accepted Answer

A

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 row contains a description of metallic bonding and a property that is explained by reference to metallic bonding? description of property explained by metallic bonding metallic bonding A a lattice of negative ions a metal will react with an in a sea of electrons acid, producing hydrogen B a lattice of negative ions a piece of a metal can be in a sea of electrons moulded into different shapes C a lattice of positive ions a metal will react with an in a sea of electrons acid, producing hydrogen D a lattice of positive ions a piece of a metal can be in a sea of electrons moulded into different shapes

Accepted Answer

D

Question 7

7 Which statement explains why methane has a lower boiling point than water? A Methane has weaker covalent bonds than water. B Methane has weaker attractive forces than water. C Methane molecules are heavier than water molecules. D Methane molecules have more bonds than water molecules.

Accepted Answer

B

Question 8

8 A solution of iron(III) sulfate reacts with aqueous sodium hydroxide to form a red–brown precipitate. What is the balanced equation, including state symbols, for the reaction? A FeSO4(aq)  +  2NaOH(aq)  →  Fe(OH)2(s)  +  Na2SO4(aq) B FeSO4(l)  +  2NaOH(l)  →  Fe(OH)2(s)  +  Na2SO4(l) C Fe2(SO4)3(aq)  +  6NaOH(aq)  →  2Fe(OH)3(s)  +  3Na2SO4(aq) D Fe2(SO4)3(l)  +  6NaOH(aq)  →  2Fe(OH)3(s)  +  3Na2SO4(l)

Accepted Answer

C

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 Dilute aqueous sodium chloride is electrolysed using platinum electrodes. What is the half-equation for the reaction at the cathode? A 2H+  +  2e–  →  H2 B Na+  +  e–  →  Na C 2Cl –  →  Cl 2  +  2e– D 4OH–  →  2H2O  +  O2  +  4e–

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 The equation for the complete combustion of methane gas is shown. CH4(g)  +  2O2(g)  →  CO2(g)  +  2H2O(g) Bond energies are shown. bond energy bond in kJ / mol C–H 412 H–O 463 C=O 743 O=O 498 What is the overall energy change, in kJ / mol, for the above reaction? A –1192 B –694 C +694 D +1192

Accepted Answer

B

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 diagram represents a chemical change? A B C D

Accepted Answer

D

Question 15

15 The rate of reaction between calcium carbonate chips and hydrochloric acid is studied by collecting the volume of gas released in one minute at different temperatures. A graph of rate of reaction against temperature is shown. 80 70 60 50 rate of reaction 40 cm3 / min 30 20 10 0 0 10 20 30 40 50 60 temperature / °C Which statement fully explains why increasing the temperature has this effect on the rate? A The kinetic energy of the particles increases so the collisions are harder. B The number of collisions between particles increases. C The activation energy needed for the particles to react is reduced. D There are more frequent collisions between particles with enough energy to react.

Accepted Answer

D

Question 16

16 The equation shows the equilibrium between dinitrogen tetroxide, N2O4, and nitrogen dioxide, NO2. The colours of the reactant and product are also shown. N2O4(g) 2NO2(g) colourless brown The forward reaction is endothermic. Which statement is not correct? A At equilibrium the concentrations of the reactant and the product are constant. B At equilibrium the rate of the forward reaction is equal to the rate of the reverse reaction. C When the pressure is increased a darker brown colour is seen. D When the temperature is increased a darker brown colour is seen.

Accepted Answer

C

Question 17

17 The equations for two reactions of iodide ions are shown. reaction 1 2I–(aq)  +  H2O2(aq)  →  I2(aq)  +  2OH–(aq) reaction 2 I–(aq)  +  Ag+(aq)  →  AgI(s) Which statement is correct? A Both reactions are redox reactions. B Neither reaction is a redox reaction. C Only reaction 1 is a redox reaction. D Only reaction 2 is a redox reaction.

Accepted Answer

C

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 Lead(II) sulfate is an insoluble salt. Which method is suitable for obtaining solid lead(II) sulfate? A Mix aqueous lead(II) nitrate and aqueous potassium sulfate, heat to evaporate all of the water, collect the solid and then wash and dry it. B Mix aqueous lead(II) nitrate and aqueous potassium sulfate, filter, collect the filtrate, crystallise, then wash and dry the crystals. C Mix aqueous lead(II) nitrate and dilute sulfuric acid, filter, then wash and dry the residue. D Titrate aqueous lead(II) hydroxide with dilute sulfuric acid, crystallise, then wash and dry the crystals.

Accepted Answer

C

Question 22

22 A Group I metal (lithium, sodium or potassium) is reacted with a Group VII element (chlorine, bromine or iodine). Which compound is formed when the Group I metal of highest density reacts with the Group VII element of lowest density? A lithium chloride B potassium chloride C potassium iodide D lithium iodide

Accepted Answer

B

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 A balloon is filled with helium. Helium is a noble gas and makes the balloon rise up in the air. The density of air is 1.23 g / dm3. Which gas is helium? density in g / dm3 reaction with oxygen A 0.0899 burns rapidly B 0.179 does not react with oxygen C 1.78 does not react with oxygen D 3.75 does not react with oxygen

Accepted Answer

B

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 Sodium nitrate is a white crystalline solid that decomposes on heating. sodium nitrate heat Which row describes the decomposition products formed when sodium nitrate is heated strongly? solid products gaseous products A sodium nitrite NO2 and O2 B sodium nitrite O2 only C sodium oxide NO2 and O2 D sodium oxide O2 only

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 Element Y reacts with copper(II) oxide to form copper. Element Y will not react with zinc oxide. Copper has no reaction with zinc oxide. What is the order of reactivity of these three elements, most reactive first? A Cu → Y → Zn B Cu → Zn → Y C Zn → Cu → Y D Zn → Y → Cu

Accepted Answer

D

Question 29

29 Which statement shows that a liquid is pure water? A It boils at 100 °C. B It has a pH value of 7. C It turns blue cobalt(II) chloride pink. D It turns white copper(II) sulfate blue.

Accepted Answer

A

Question 30

30 Which process removes carbon dioxide from the atmosphere? A combustion B decomposition C photosynthesis D respiration

Accepted Answer

C

Question 31

31 Ammonia is manufactured by the Haber process. N2(g)  +  3H2(g) 2NH3(g) What are the conditions used in the Haber process? temperature pressure / °C / atm A 400 100 B 400 300 C 20 300 D 20 100

Accepted Answer

B

Question 32

32 Coating iron helps to prevent rusting. Which coating will continue to protect the iron even when the coating is damaged? A copper B paint C plastic D zinc

Accepted Answer

D

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 The Contact process is used to manufacture concentrated sulfuric acid and consists of four steps. Which step involves a catalyst? A production of sulfur dioxide gas B production of sulfur trioxide gas C production of oleum D production of concentrated sulfuric acid

Accepted Answer

B

Question 35

35 Which row about the production of ethanol by fermentation is correct? raw materials energy requirement rate of reaction A non-renewable high slow B renewable low slow C non-renewable low fast D renewable high fast

Accepted Answer

B

Question 36

36 Which statement about homologous series is correct? A Members of a homologous series have the same structural formula. B Members of a homologous series all have similar chemical properties. C Members of a homologous series all have similar physical properties. D Members of all homologous series are hydrocarbons.

Accepted Answer

B

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 Some properties of an organic compound J are listed. ● It is a liquid at room temperature. ● It is soluble in water. ● A solution of J reacts with calcium carbonate to form carbon dioxide. ● A solution of J has a pH of 3. In which homologous series does J belong? A alkane B alkene C alcohol D carboxylic acid

Accepted Answer

D

Question 39

39 Ethane, C2H6, reacts with chlorine in a substitution reaction. What are the products of this reaction? A chloroethane and hydrogen B chloroethane and hydrogen chloride C chloroethene and hydrogen D chloroethene and hydrogen chloride

Accepted Answer

B

Question 40

40 Which polymers or types of polymer are synthetic? 1 carbohydrates 2 nylon 3 proteins 4 Terylene A 1 and 3 B 1 and 4 C 2 and 3 D 2 and 4

Accepted Answer

D

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 should be used to measure exactly 21.4 cm3 of water?

Q3 · The chromatogram for an unknown dye is shown

Q4 · The atomic number and nucleon number of a potassium atom are shown

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

Q6 · Which row contains a description of metallic bonding and a property that is explained by…

Q7 · Which statement explains why methane has a lower boiling point than water?

Q8 · A solution of iron(III) sulfate reacts with aqueous sodium hydroxide to form a red–brown…

Q9 · The Haber process is a reversible reaction

Q10 · Dilute aqueous sodium chloride is electrolysed using platinum electrodes

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

Q12 · The equation for the complete combustion of methane gas is shown

Q13 · Which statements about hydrogen fuel cells are correct?

Q14 · Which diagram represents a chemical change?

Q15 · The rate of reaction between calcium carbonate chips and hydrochloric acid is studied by…

Q16 · The equation shows the equilibrium between dinitrogen tetroxide, N2O4, and nitrogen…

Q17 · The equations for two reactions of iodide ions are shown

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 · Lead(II) sulfate is an insoluble salt

Q22 · A Group I metal (lithium, sodium or potassium) is reacted with a Group VII element…

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

Q24 · A balloon is filled with helium

Q25 · Which property is shown by all metals?

Q26 · Sodium nitrate is a white crystalline solid that decomposes on heating

Q27 · Molten iron from the blast furnace contains impurities

Q28 · Element Y reacts with copper(II) oxide to form copper

Q29 · Which statement shows that a liquid is pure water?

Q30 · Which process removes carbon dioxide from the atmosphere?

Q31 · Ammonia is manufactured by the Haber process

Q32 · Coating iron helps to prevent rusting

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

Q34 · The Contact process is used to manufacture concentrated sulfuric acid and consists of…

Q35 · Which row about the production of ethanol by fermentation is correct?

Q36 · Which statement about homologous series is correct?

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

Q38 · Some properties of an organic compound J are listed

Q39 · Ethane, C2H6, reacts with chlorine in a substitution reaction

Q40 · Which polymers or types of polymer are synthetic?

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