UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS...

This document consists of 18 printed pages and 2 blank pages.

IB13 11_0620_11/2RP © UCLES 2013 [Turn over

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UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education

CHEMISTRY 0620/11

Paper 1 Multiple Choice October/November 2013

45 Minutes Additional Materials: Multiple Choice Answer Sheet Soft clean eraser Soft pencil (type B or HB is recommended)

READ THESE INSTRUCTIONS FIRST

Write in soft pencil.

Do not use staples, paper clips, highlighters, glue or correction fluid.

Write your name, Centre number and candidate number on the Answer Sheet in the spaces provided unless this has been done for you.

DO NOT WRITE IN ANY BARCODES.

There are forty questions on this paper. Answer all questions. For each question there are four possible answers A, B, C and D.

Choose the one you consider correct and record your choice in soft pencil on the separate Answer Sheet.

Read the instructions on the Answer Sheet very carefully.

Each correct answer will score one mark. A mark will not be deducted for a wrong answer.

Any rough working should be done in this booklet.

A copy of the Periodic Table is printed on page 20.

Electronic calculators may be used.

2

© UCLES 2013 0620/11/O/N/13

1 An attempt was made to compress a gas and a solid using the apparatus shown.

piston

gas solid

Which substance would be compressed and what is the reason for this?

substance reason

A gas the gas particles are close together

B gas the gas particles are far apart

C solid the solid particles are close together

D solid the solid particles are far apart

2 A student measures the rate of two reactions.

In one reaction, there is a change in mass of the reactants during the reaction.

In the second reaction, there is a change in temperature during the reaction.

Which piece of apparatus would be essential in both experiments?

A balance

B clock

C pipette

D thermometer

3

© UCLES 2013 0620/11/O/N/13 [Turn over

3 Diagram 1 shows the paper chromatogram of substance X.

R

Y

X

diagram 1

Diagram 2 shows the cooling curve for substance Y.

0

147

0

temperature / °C

time

diagram 2

Which statement about X and Y is correct?

A X is a mixture and Y is a pure substance.

B X is a pure substance and Y is a mixture.

C X and Y are mixtures.

D X and Y are pure substances.

4

© UCLES 2013 0620/11/O/N/13

4 Element X has 7 protons.

Element Y has 8 more protons than X.

Which statement about element Y is correct?

A Y has more electron shells than X.

B Y has more electrons in its outer shell than X.

C Y is in a different group of the Periodic Table from X.

D Y is in the same period of the Periodic Table as X

5 Which statements about a sodium atom, Na,23

11 are correct?

1 The number of protons and neutrons is the same.

2 The number of protons and electrons is the same.

3 The number of outer electrons is one.

A 1, 2 and 3 B 1 and 2 only C 1 and 3 only D 2 and 3 only 6 Rubidium is in Group I of the Periodic Table and bromine is in Group VII.

Rubidium reacts with bromine to form an ionic compound.

Which row shows the electron change taking place for rubidium and the correct formula of the rubidium ion?

electron change formula of ion formed

A electron gained Rb+

B electron gained Rb–

C electron lost Rb+

D electron lost Rb–

7 The diagrams show the electron arrangements in the atoms of four elements.

Which element does not form a covalent bond?

e e

e e e

e e

e e

e e e e

e e e e

e e key

electron

nucleus

A B C D

e e

e e e e

e e

5


8 A solid mixture contains an ionic salt, X, and a covalent organic compound, Y.

Two students suggest methods of separating the mixture as shown.

method 1

method 2

shake withwater

X + Y

shake withethanol

X + Y

Which methods of separation are likely to work?

1 2

A � �

B � �

C � �

D � �

9 The formulae of compounds W, X and Y are shown.

W CuSO4.5H2O

X MgSO4.7H2O

Y Cu(NO3)2.6H2O

Which statement is correct?

A W contains twice as many hydrogen atoms as oxygen atoms.

B X contains the most oxygen atoms.

C Y contains the most hydrogen atoms.

D Y contains the same number of hydrogen and oxygen atoms.

6

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10 Which relative molecular mass, Mr, is not correct for the molecule given?

molecule Mr

A ammonia, NH3 17

B carbon dioxide, CO2 44

C methane, CH4 16

D oxygen, O2 16

11 The diagram shows the circuit for electrolysing lead(II) bromide and sodium chloride to liberate

the metal.

A

container forlead(II) bromide

container forsodium chloride

In what form are these salts electrolysed for liberating the metal?

lead(II) bromide sodium chloride

A concentrated solution concentrated solution

B concentrated solution molten

C molten concentrated solution

D molten molten

7


12 The diagram shows the electrolysis of concentrated aqueous sodium chloride.

+ –anode cathode

concentratedaqueous sodiumchloride and litmus

carbonrods

What is the colour of the litmus at each electrode after five minutes?

colour at anode colour at cathode

A blue red

B red blue

C red colourless

D colourless blue

13 When anhydrous copper(II) sulfate is added to water a solution is formed and heat is given out.

water

anhydrouscopper(II) sulfate

thermometer

Which row correctly shows the temperature change and the type of reaction taking place?

temperature change type of reaction

A decreases endothermic

B decreases exothermic

C increases endothermic

D increases exothermic

8

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14 Which fuel does not produce carbon dioxide when it burns?

A coal

B hydrogen

C methane

D petrol 15 A student investigates the rate of reaction between zinc and an excess of sulfuric acid.

The graph shows the results of two experiments, X and Y.

0

X

Y

time0

volume ofhydrogen

Which change explains the difference between X and Y?

A A catalyst is added in Y.

B A lower temperature is used in Y.

C Larger pieces of zinc are used in Y.

D Less concentrated acid is used in Y.

16 Anhydrous copper(II) sulfate can be made by heating hydrated copper(II) sulfate.

CuSO4.5H2O → CuSO4 + 5H2O

What can be added to anhydrous copper(II) sulfate to turn it into hydrated copper(II) sulfate?

A concentrated sulfuric acid

B sodium hydroxide powder

C sulfur dioxide

D water

9


17 The reactions shown may occur in the air during a thunder storm.

N2 + O2 → 2NO

2NO + O2 → 2NO2

NO + O3 → NO2 + O2

Which row shows what happens to the reactant molecules in each of these reactions?

N2 NO O3

A oxidised oxidised oxidised

B oxidised oxidised reduced

C reduced reduced oxidised

D reduced reduced reduced

18 Which are properties of an acid?

1 reacts with ammonium sulfate to form ammonia

2 turns red litmus blue

1 2

A � �

B � �

C � �

D � �

19 Which of the following are properties of the oxides of non-metals?

property 1 property 2

A acidic covalent

B acidic ionic

C basic covalent

D basic ionic

10

© UCLES 2013 0620/11/O/N/13

20 Compound X is tested and the results are shown in the table.

test result

aqueous sodium hydroxide is

added, then heated gently

gas given off which turns damp

red litmus paper blue

dilute hydrochloric acid is added effervescence, gas given off

which turns limewater milky

Which ions are present in compound X?

A ammonium ions and carbonate ions

B ammonium ions and chloride ions

C calcium ions and carbonate ions

D calcium ions and chloride ions 21 Calcium, on the left of Period 4 of the Periodic Table, is more metallic than bromine on the right of

this period.

Why is this?

Calcium has

A fewer electrons.

B fewer protons.

C fewer full shells of electrons.

D fewer outer shell electrons. 22 The diagrams show the labels of four bottles.

Which label is not correct?

A B C D

Bromine Br2

Harmful liquid.

Do not spill.

Iodine

I2

Danger Avoid breathing vapour

from the solid.

Potassium

K

Danger Store under water.

Sodium

Na

Danger Store under oil.

11


23 An element has a melting point of 1084 °C and a density of 8.93 g / cm3. It’s oxide can be used as a catalyst.

In which position in the Periodic Table is the element found?

A B C

D

24 The diagram shows a light bulb.

filament

argon

Why is argon used instead of air in the light bulb?

A Argon is a good conductor of electricity.

B Argon is more reactive than air.

C The filament glows more brightly.

D The filament does not react with the argon. 25 Some properties of four elements W, X, Y and Z are listed.

1 W melts at 1410 °C and forms an acidic oxide.

2 X has a high density and is easily drawn into wires.

3 Y acts as a catalyst and its oxide reacts with acids.

4 Z is a red-brown solid used to make alloys.

Which of the elements are metals?

A 1 and 3 B 2, 3 and 4 C 2 and 3 only D 2 and 4 only

12

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26 M is a shiny silver metal. It has a melting point of 1455 °C. Many of its compounds are green.

What is metal M?

A aluminium

B copper

C mercury

D nickel 27 Reactions of three metals and their oxides are listed in the table.

metal reacts with cold water

metal oxide reacts with carbon

W no no

X no yes

Y yes no

What is the order of reactivity of the metals?

least reactive most reactive

A W X Y

B X W Y

C X Y W

D Y W X

28 Equations P and Q represent two reactions which occur inside a blast furnace.

P Fe2O3 + 3CO → 2Fe + 3CO2

Q CaCO3 → CaO + CO2

Which type of reactions are P and Q?

P Q

A redox redox

B redox thermal decomposition

C thermal decomposition redox

D thermal decomposition thermal decomposition

13


29 Which row describes the uses of mild steel and stainless steel?

mild steel stainless steel

A car bodies, cutlery chemical plant, machinery

B car bodies, machinery chemical plant, cutlery

C chemical plant, cutlery car bodies, machinery

D chemical plant, machinery car bodies, cutlery

30 In which process is carbon dioxide not formed?

A burning of natural gas

B fermentation

C heating lime

D respiration 31 Farmers add calcium oxide (lime) and ammonium salts to their fields.

The compounds are not added at the same time because they react with each other.

Which gas is produced in this reaction?

A ammonia

B carbon dioxide

C hydrogen

D nitrogen 32 The diagrams show four uses of iron.

In which of these uses is the iron most likely to rust?

iron bucketelectroplated

with zinc

A

iron coredaluminium

electricity cables

B

iron hingeson a gate

C

paintediron fence

D

14

© UCLES 2013 0620/11/O/N/13

33 Which air pollutant is not made when coal burns in a power station?

A carbon monoxide

B lead compounds

C nitrogen oxides

D sulfur dioxide 34 In many countries river water is used for the washing of clothes.

The same water is not considered to be safe for drinking.

Why is it not safe for drinking?

A because river water contains dissolved salts

B because river water may contain harmful bacteria

C because river water may contain small particles of sand

D because river water may contain soap from washing clothes 35 The diagram shows a kiln used to heat limestone.

gas burners

productair

waste gases

limestone

What is the product and what waste gas is formed?

product waste gas

A lime, CaO carbon monoxide

B lime, CaO carbon dioxide

C slaked lime, Ca(OH)2 carbon monoxide

D slaked lime, Ca(OH)2 carbon dioxide

15


36 Three types of organic compound are alkanes, alkenes and alcohols.

Which structure does not belong to any of these three types of compound?

H C

H

H

C

H

H

C

O

O H H C

H

H

C

H

H

C

H

H

OH

H C

H

H

HC C

H

H

H

HC

H

H

A B

C D

C

H

H

C

H

H

37 The diagram shows some properties of two organic compounds X and Y.

reactswith

bromine

polymerises

X

usedas afuel

usedas a

solvent

Ysteamand a

catalyst

What are X and Y?

X Y

A ethane ethanoic acid

B ethane ethanol

C ethene ethanoic acid

D ethene ethanol

16

© UCLES 2013 0620/11/O/N/13

38 Petroleum is a mixture of hydrocarbons which can be separated into fractions using fractional distillation.

Which fraction is used as fuel in jet engines?

A bitumen

B gasoline

C kerosene

D naphtha 39 The diagram represents ethene.

C C

H

H

H

H

Which compound has chemical properties similar to those of ethene?

C CH H

H

H

H

A

H

C CH H

H

H

H

B

H

C

H

H

C CH

H

H

H

D

C

H

H

C CH H

H

H

C

O

H

H

17

© UCLES 2013 0620/11/O/N/13

40 A chemist carried out a cracking reaction on a hydrocarbon, X, and obtained two products, Y and Z.

H C

H

H

C

H

H

C

H

H

C

H

H

H H C

H

H

C

H

C

H

H

+X

Y Z

The chemist then wrote the following statements in his notebook.

1 A molecule of X has 7 carbon atoms.

2 Y is unsaturated.

3 Z will decolourise bromine water.

Which statements are correct?

A 3 only B 1 and 2 C 1 and 3 D 1, 2 and 3

18

© UCLES 2013 0620/11/O/N/13

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19

© UCLES 2013 0620/11/O/N/13

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20

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.

Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.

© UCLES 2013 0620/11/O/N/13

Gro

up

140

Ce

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PrP

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Nd

Neo

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PmP

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150

SmS

amar

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152

EuE

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Gd

Gad

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159

Tb Terb

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65

162

Dy

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165

Ho

Hol

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Er Erb

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Tm Thul

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YbY

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Cm

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Cf

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Man

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56 Fe Iron

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59 Co

Cob

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Nic

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64 Cu

Cop

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70 Ga

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Cd

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In Indi

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Sn Tin

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Gol

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IB13 11_0620_12/FP © UCLES 2013 [Turn over

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CHEMISTRY 0620/12















2

© UCLES 2013 0620/12/O/N/13

1 An attempt was made to compress a gas and a solid using the apparatus shown.

piston

gas solid

Which substance would be compressed and what is the reason for this?

substance reason

A gas the gas particles are close together

B gas the gas particles are far apart

C solid the solid particles are close together

D solid the solid particles are far apart

2 A student measures the rate of two reactions.

In one reaction, there is a change in mass of the reactants during the reaction.

In the second reaction, there is a change in temperature during the reaction.

Which piece of apparatus would be essential in both experiments?

A balance

B clock

C pipette

D thermometer

3



R

Y

X

diagram 1


0

147

0

temperature / °C

time

diagram 2






4 Which statements about a sodium atom, Na,23

11 are correct?

1 The number of protons and neutrons is the same.

2 The number of protons and electrons is the same.

3 The number of outer electrons is one.

A 1, 2 and 3 B 1 and 2 only C 1 and 3 only D 2 and 3 only

4

© UCLES 2013 0620/12/O/N/13

5 The diagrams show the electron arrangements in the atoms of four elements.

Which element does not form a covalent bond?

e e

e e e

e e

e e

e e e e

e e e e

e e key

electron

nucleus

A B C D

e e

e e e e

e e

6 Rubidium is in Group I of the Periodic Table and bromine is in Group VII.

Rubidium reacts with bromine to form an ionic compound.

Which row shows the electron change taking place for rubidium and the correct formula of the rubidium ion?

electron change formula of ion formed

A electron gained Rb+

B electron gained Rb–

C electron lost Rb+

D electron lost Rb–

7 Element X has 7 protons.

Element Y has 8 more protons than X.

Which statement about element Y is correct?

A Y has more electron shells than X.

B Y has more electrons in its outer shell than X.

C Y is in a different group of the Periodic Table from X.

D Y is in the same period of the Periodic Table as X

5


8 The formulae of compounds W, X and Y are shown.

W CuSO4.5H2O

X MgSO4.7H2O

Y Cu(NO3)2.6H2O

Which statement is correct?

A W contains twice as many hydrogen atoms as oxygen atoms.

B X contains the most oxygen atoms.

C Y contains the most hydrogen atoms.

D Y contains the same number of hydrogen and oxygen atoms. 9 A solid mixture contains an ionic salt, X, and a covalent organic compound, Y.


method 1

method 2

shake withwater

X + Y

shake withethanol

X + Y


1 2

A � �

B � �

C � �

D � �

6

© UCLES 2013 0620/12/O/N/13

10 The diagram shows the circuit for electrolysing lead(II) bromide and sodium chloride to liberate the metal.

A

container forlead(II) bromide

container forsodium chloride

In what form are these salts electrolysed for liberating the metal?

lead(II) bromide sodium chloride

A concentrated solution concentrated solution

B concentrated solution molten

C molten concentrated solution

D molten molten


molecule Mr

A ammonia, NH3 17


C methane, CH4 16

D oxygen, O2 16

7


12 When anhydrous copper(II) sulfate is added to water a solution is formed and heat is given out.

water

anhydrouscopper(II) sulfate

thermometer

Which row correctly shows the temperature change and the type of reaction taking place?

temperature change type of reaction

A decreases endothermic

B decreases exothermic

C increases endothermic

D increases exothermic

13 The diagram shows the electrolysis of concentrated aqueous sodium chloride.

+ –anode cathode

concentratedaqueous sodiumchloride and litmus

carbonrods

What is the colour of the litmus at each electrode after five minutes?

colour at anode colour at cathode

A blue red

B red blue

C red colourless

D colourless blue

8

© UCLES 2013 0620/12/O/N/13

14 Anhydrous copper(II) sulfate can be made by heating hydrated copper(II) sulfate.

CuSO4.5H2O → CuSO4 + 5H2O

What can be added to anhydrous copper(II) sulfate to turn it into hydrated copper(II) sulfate?

A concentrated sulfuric acid

B sodium hydroxide powder

C sulfur dioxide

D water 15 Which fuel does not produce carbon dioxide when it burns?

A coal

B hydrogen

C methane

D petrol 16 A student investigates the rate of reaction between zinc and an excess of sulfuric acid.


0

X

Y

time0

volume ofhydrogen






9





1 2

A � �

B � �

C � �

D � �



A acidic covalent

B acidic ionic

C basic covalent

D basic ionic


N2 + O2 → 2NO

2NO + O2 → 2NO2

NO + O3 → NO2 + O2


N2 NO O3





10

© UCLES 2013 0620/12/O/N/13

20 Calcium, on the left of Period 4 of the Periodic Table, is more metallic than bromine on the right of this period.

Why is this?

Calcium has

A fewer electrons.

B fewer protons.


D fewer outer shell electrons. 21 Compound X is tested and the results are shown in the table.

test result

aqueous sodium hydroxide is

added, then heated gently

gas given off which turns damp

red litmus paper blue

dilute hydrochloric acid is added effervescence, gas given off

which turns limewater milky

Which ions are present in compound X?

A ammonium ions and carbonate ions

B ammonium ions and chloride ions

C calcium ions and carbonate ions

D calcium ions and chloride ions 22 Some properties of four elements W, X, Y and Z are listed.

1 W melts at 1410 °C and forms an acidic oxide.

2 X has a high density and is easily drawn into wires.

3 Y acts as a catalyst and its oxide reacts with acids.

4 Z is a red-brown solid used to make alloys.

Which of the elements are metals?

A 1 and 3 B 2, 3 and 4 C 2 and 3 only D 2 and 4 only

11



filament

argon





D The filament does not react with the argon.



A B C

D

25 The diagrams show the labels of four bottles.


A B C D

Bromine Br2

Harmful liquid.

Do not spill.

Iodine

I2


from the solid.

Potassium

K


Sodium

Na


12

© UCLES 2013 0620/12/O/N/13

26 Equations P and Q represent two reactions which occur inside a blast furnace.

P Fe2O3 + 3CO → 2Fe + 3CO2

Q CaCO3 → CaO + CO2

Which type of reactions are P and Q?

P Q

A redox redox

B redox thermal decomposition

C thermal decomposition redox

D thermal decomposition thermal decomposition

27 Farmers add calcium oxide (lime) and ammonium salts to their fields.

The compounds are not added at the same time because they react with each other.

Which gas is produced in this reaction?

A ammonia

B carbon dioxide

C hydrogen

D nitrogen 28 Which row describes the uses of mild steel and stainless steel?

mild steel stainless steel

A car bodies, cutlery chemical plant, machinery

B car bodies, machinery chemical plant, cutlery

C chemical plant, cutlery car bodies, machinery

D chemical plant, machinery car bodies, cutlery

13


29 Reactions of three metals and their oxides are listed in the table.

metal reacts with cold water

metal oxide reacts with carbon

W no no

X no yes

Y yes no

What is the order of reactivity of the metals?


A W X Y

B X W Y

C X Y W

D Y W X

30 The diagrams show four uses of iron.

In which of these uses is the iron most likely to rust?

iron bucketelectroplated

with zinc

A

iron coredaluminium

electricity cables

B

iron hingeson a gate

C

paintediron fence

D

31 In which process is carbon dioxide not formed?


B fermentation

C heating lime

D respiration

14

© UCLES 2013 0620/12/O/N/13

32 M is a shiny silver metal. It has a melting point of 1455 °C. Many of its compounds are green.

What is metal M?

A aluminium

B copper

C mercury

D nickel 33 In many countries river water is used for the washing of clothes.

The same water is not considered to be safe for drinking.

Why is it not safe for drinking?

A because river water contains dissolved salts

B because river water may contain harmful bacteria

C because river water may contain small particles of sand

D because river water may contain soap from washing clothes

15


34 The diagram shows a kiln used to heat limestone.

gas burners

productair

waste gases

limestone


product waste gas





35 Which air pollutant is not made when coal burns in a power station?

A carbon monoxide

B lead compounds

C nitrogen oxides

D sulfur dioxide

16

© UCLES 2013 0620/12/O/N/13

36 The diagram shows some properties of two organic compounds X and Y.

reactswith

bromine

polymerises

X

usedas afuel

usedas a

solvent

Ysteamand a

catalyst

What are X and Y?

X Y

A ethane ethanoic acid

B ethane ethanol

C ethene ethanoic acid

D ethene ethanol

37 Three types of organic compound are alkanes, alkenes and alcohols.

Which structure does not belong to any of these three types of compound?

H C

H

H

C

H

H

C

O

O H H C

H

H

C

H

H

C

H

H

OH

H C

H

H

HC C

H

H

H

HC

H

H

A B

C D

C

H

H

C

H

H

17

© UCLES 2013 0620/12/O/N/13

38 The diagram represents ethene.

C C

H

H

H

H

Which compound has chemical properties similar to those of ethene?

C CH H

H

H

H

A

H

C CH H

H

H

H

B

H

C

H

H

C CH

H

H

H

D

C

H

H

C CH H

H

H

C

O

H

H 39 Petroleum is a mixture of hydrocarbons which can be separated into fractions using fractional

distillation.

Which fraction is used as fuel in jet engines?

A bitumen

B gasoline

C kerosene

D naphtha 40 A chemist carried out a cracking reaction on a hydrocarbon, X, and obtained two products, Y

and Z.

H C

H

H

C

H

H

C

H

H

C

H

H

H H C

H

H

C

H

C

H

H

+X

Y Z

The chemist then wrote the following statements in his notebook.

1 A molecule of X has 7 carbon atoms.

2 Y is unsaturated.

3 Z will decolourise bromine water.

Which statements are correct?

A 3 only B 1 and 2 C 1 and 3 D 1, 2 and 3

18

© UCLES 2013 0620/12/O/N/13

BLANK PAGE

19

© UCLES 2013 0620/12/O/N/13

BLANK PAGE

20



© UCLES 2013 0620/12/O/N/13

Gro

up

140

Ce

Cer

ium

58

141

PrP

rase

odym

ium

59

144

Nd

Neo

dym

ium

60

PmP

rom

ethi

um61

150

SmS

amar

ium

62

152

EuE

urop

ium

63

157

Gd

Gad

olin

ium

64

159

Tb Terb

ium

65

162

Dy

Dys

pros

ium

66

165

Ho

Hol

miu

m67

167

Er Erb

ium

68

169

Tm Thul

ium

69

173

YbY

tterb

ium

70

175

LuLu

tetiu

m71

232

Th Thor

ium

90

PaP

rota

ctin

ium

91

238 U

Ura

nium

92

Np

Nep

tuni

um93

PuP

luto

nium

94

Am

Am

eric

ium

95

Cm

Cur

ium

96

Bk

Ber

keliu

m97

Cf

Cal

iforn

ium

98

EsE

inst

eini

um99

Fm Ferm

ium

100

Md

Men

dele

vium

101

No

Nob

eliu

m10

2

LrLa

wre

nciu

m10

3

1 HH

ydro

gen

1

7 LiLi

thiu

m3

23 Na

Sod

ium

11

24 Mg

Mag

nesi

um12

40 Ca

Cal

cium

20

45 ScS

cand

ium

21

48 TiTi

tani

um22

51 VVa

nadi

um23

52 Cr

Chr

omiu

m24

55 Mn

Man

gane

se25

56 Fe Iron

26

59 Co

Cob

alt

27

59 Ni

Nic

kel

28

64 Cu

Cop

per

29

65 Zn Zinc

30

70 Ga

Gal

lium

31

27 Al

Alu

min

ium

13

11 B Bor

on5

12 CC

arbo

n6

14 NN

itrog

en7

16 OO

xyge

n8

19 FFl

uorin

e9

28 Si Sili

con

14

31 PP

hosp

horu

s15

32 S Sul

fur

16

35.5 Cl

Chl

orin

e17

40 Ar

Arg

on18

20 Ne

Neo

n10

4 He

Hel

ium

2

73 Ge

Ger

man

ium

32

75 As

Ars

enic

33

79 SeS

elen

ium

34

80 Br

Bro

min

e35

84 Kr

Kry

pton

36

39 KP

otas

sium

19

88 SrS

tront

ium

38

89 YY

ttriu

m39

91 ZrZi

rcon

ium

40

93 Nb

Nio

bium

41

96 Mo

Mol

ybde

num

42

TcTe

chne

tium

43

101

Ru

Rut

heni

um44

103

Rh

Rho

dium

45

106

PdP

alla

dium

46

108

Ag

Silv

er47

112

Cd

Cad

miu

m48

115

In Indi

um49

119

Sn Tin

50

122

SbA

ntim

ony

51

128

TeTe

lluriu

m52

127 I

Iodi

ne53

131

Xe Xen

on54

137

Ba

Bar

ium

56

139

LaLa

ntha

num

57

*

178

Hf

Haf

nium

72

181

TaTa

ntal

um73

184 W

Tung

sten

74

186

Re

Rhe

nium

75

190

Os

Osm

ium

76

192

Ir Iridi

um77

195 Pt

Pla

tinum

78

197

Au

Gol

d79

201

Hg

Mer

cury

80

204 Tl

Thal

lium

81

207

Pb Lead

82

209 Bi

Bis

mut

h83

PoP

olon

ium

84

At

Ast

atin

e85

Rn

Rad

on86

FrFr

anci

um87

227

Ac

Act

iniu

m89

9 Be

Ber

ylliu

m4

III

IIIIV

VV

IV

II0

85 Rb

Rub

idiu

m37

133

Cs

Cae

sium

55

226

Ra

Rad

ium

88

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3

at ro

om te

mpe

ratu

re a

nd p

ress

ure

(r.t.p

.).

a Xb

a =

rela

tive

atom

ic m

ass

X =

atom

ic s

ymbo

l

b =

prot

on (a

tom

ic) n

umbe

r

Key

* 58-

71 L

anth

anoi

d se

ries

90-1

03 A

ctin

oid

serie

s

DAT

A SH

EET

The

Perio

dic

Tabl

e of

the

Elem

ents

This document consists of 19 printed pages and 1 blank page.

IB13 11_0620_13/RP © UCLES 2013 [Turn over

*5450428188*


CHEMISTRY 0620/13















2

© UCLES 2013 0620/13/O/N/13

1 A gas jar of bromine vapour and a gas jar of air are set up as shown in diagram 1.

The glass slide is removed. Diagram 2 shows the appearance of the gas jars after one hour.

diagram 1 diagram 2

brominevapour

mixture of airand bromine

air

glass slide

Which statement explains why the bromine and air mix together?

A Bromine is denser than air.

B Bromine is lighter than air.

C Bromine molecules moved upwards and molecules in air moved downwards.

D Molecules in bromine and air moved randomly. 2 The diagram shows a method for separating a substance that contains X and Y.

filter paper

X

Y

Which types of substance can be separated as shown?

A compounds

B elements

C mixtures

D molecules

3



R

Y

X

diagram 1


0

147

0

temperature / °C

time

diagram 2






4

© UCLES 2013 0620/13/O/N/13

4 The atomic structures of four atoms are shown.

atom number of neutrons

number of protons

number of electrons

W 6 6 6

X 7 7 7

Y 8 6 6

Z 8 8 8

Which pair of atoms are isotopes?

A W and X B W and Y C X and Y D Y and Z 5 The diagram shows the structure of three particles, R, S and T.

3 p3 n

key

= electron

= neutron

= proton

= nucleus

e ee

e

n

p

R

3 p3 n

e e

S

3 p4 n

e ee

T

Which row describes these particles?

ions isotopes

A R S and T

B R and S T

C S R and T

D T R and S

6 Which statement about the bonding in a molecule of water is not correct?

A Both hydrogen and oxygen have a noble gas configuration of electrons.

B Each hydrogen shares its one electron with oxygen.

C Oxygen shares one of its own electrons with each hydrogen.

D Oxygen shares two of its own electrons with each hydrogen.

5


7 The electronic structures of atoms P and Q are shown.

P Q

P and Q react to form an ionic compound.

What is the formula of the compound?

A Q7P B QP C QP3 D QP7 8 A solid mixture contains an ionic salt, X, and a covalent organic compound, Y.


method 1

method 2

shake withwater

X + Y

shake withethanol

X + Y


1 2

A � �

B � �

C � �

D � �

6

© UCLES 2013 0620/13/O/N/13


molecule Mr

A ammonia, NH3 17


C methane, CH4 16

D oxygen, O2 16

10 Two electrolysis experiments were carried out as shown in the diagram below.

The graphite electrodes are labelled 1-4.

molten sodium chloride

1 2 3 4

concentrated aqueoussodium chloride

+ +– –

Which row describes the products at the electrodes in these experiments?

electrode 1 electrode 2 electrode 3 electrode 4

A chlorine hydrogen chlorine hydrogen

B chlorine sodium chlorine hydrogen

C chlorine sodium hydrogen chlorine

D sodium chlorine sodium chlorine

7


11 One molten compound and two aqueous solutions were electrolysed.

The table gives the compounds electrolysed and the electrodes used.

substance electrolysed electrodes

1 concentrated hydrochloric acid carbon

2 concentrated sodium chloride platinum

3 molten lead bromide platinum

In which experiments is a gas evolved at the cathode?

A 1, 2 and 3 B 1 and 2 only C 1 only D 3 only 12 When ammonium nitrate is added to water the temperature of the water decreases.

The ammonium nitrate can be recovered by evaporating the water added.

Which explains these observations?

A The ammonium nitrate dissolves in the water and the process is endothermic.

B The ammonium nitrate reacts with the water and the process is endothermic.

C The ammonium nitrate dissolves in the water and the process is exothermic.

D The ammonium nitrate reacts with the water and the process is exothermic. 13 Which substance could not be used as a fuel to heat water in a boiler?

A ethanol

B hydrogen

C methane

D oxygen 14 Which substance is not a fossil fuel?

A coal B kerosene C gasoline D wood

8

© UCLES 2013 0620/13/O/N/13

15 A student investigates the rate of reaction between zinc and an excess of sulfuric acid.


0

X

Y

time0

volume ofhydrogen






16 When green iron(II) sulfate is heated, it turns white and a colourless liquid is produced. When the liquid is put back into the white solid it changes back to green.

What type of reaction takes place and what is the name of the liquid?

type of reaction name of liquid

A redox sulfuric acid

B redox water

C reversible sulfuric acid

D reversible water

9



N2 + O2 → 2NO

2NO + O2 → 2NO2

NO + O3 → NO2 + O2


N2 NO O3








1 2

A � �

B � �

C � �

D � �



A acidic covalent

B acidic ionic

C basic covalent

D basic ionic

10

© UCLES 2013 0620/13/O/N/13

20 The cations shown are identified by the colour of the precipitates formed when an excess of an aqueous solution of X is added.

cations present effect of adding an excess of

aqueous X

iron(II) (Fe2+) green precipitate

copper(II) (Cu2+) light blue precipitate

iron(III) (Fe3+) red-brown precipitate

What is X?

A ammonia

B limewater

C silver nitrate

D sodium hydroxide 21 Calcium, on the left of Period 4 of the Periodic Table, is more metallic than bromine on the right of

this period.

Why is this?

Calcium has

A fewer electrons.

B fewer protons.


D fewer outer shell electrons. 22 The diagrams show the labels of four bottles.


A B C D

Bromine Br2

Harmful liquid.

Do not spill.

Iodine

I2


from the solid.

Potassium

K


Sodium

Na


11




A B C

D


filament

argon





D The filament does not react with the argon. 25 Duralumin is an alloy. It contains aluminium, copper and magnesium.

It has many uses including the manufacture of cooking utensils and ships.

Which statement about duralumin and its properties is correct?

A It is a good conductor of electricity.

B It is brittle.

C It is soluble in water.

D The aluminium, copper and magnesium are chemically combined.

12

© UCLES 2013 0620/13/O/N/13

26 The list gives the order of some metals (and hydrogen) in the reactivity series.

Metal X is also included:

Most reactive K

Mg

Zn

(H)

X

Least reactive Cu

Which row correctly shows the properties of metal X?

reacts with dilute acids

oxide reduced by carbon

A no no

B no yes

C yes no

D yes yes

27 A new bicycle is being developed. Two different materials are used in its construction, both of which must be corrosion resistant.

Which two metals could be used?

A aluminium and mild steel

B aluminium and stainless steel

C mild steel and pure iron

D pure iron and stainless steel

13


28 Iron is extracted from hematite in the Blast Furnace.

waste gases

raw materials

firebrick lining

air

slag

molten iron

The hematite contains silica as an impurity. What reacts with this impurity to remove it?

A calcium oxide

B carbon

C carbon dioxide

D oxygen 29 In which process is carbon dioxide not formed?


B fermentation

C heating lime

D respiration

14

© UCLES 2013 0620/13/O/N/13

30 Carbon dioxide is produced when

X reacts with ethanol.

Y reacts with sodium carbonate.

What are X and Y?

X Y

A H2 HCl

B H2 NaOH

C O2 HCl

D O2 NaOH

31 A sample of fertiliser is tested by warming it with aqueous sodium hydroxide.

A colourless gas is produced which turns red litmus paper blue.

Which element, essential for plant growth, must be present?

A nitrogen

B phosphorus

C potassium

D sulfur 32 Iron rusts. This process involves the ……1…… of iron. Rusting can be prevented by covering the

iron with grease or paint which stops ……2…… from reaching the surface of the iron.

Which words correctly complete gaps 1 and 2?

1 2

A oxidation nitrogen

B oxidation oxygen

C reduction nitrogen

D reduction oxygen

15


33 Oxides of nitrogen are given out from car exhausts.

Which row best shows why oxides of nitrogen are unwanted?

acidic toxic

A no no

B no yes

C yes no

D yes yes

34 Water is treated at a water works to make it fit to drink.

What is present in the water when it leaves the waterworks?

A bacteria only

B bacteria and insoluble substances

C chlorine only

D chlorine and soluble substances

16

© UCLES 2013 0620/13/O/N/13

35 The diagram shows a kiln used to heat limestone.

gas burners

productair

waste gases

limestone


product waste gas





36 Molecule X is both an alkene and a carboxylic acid.

Which row describes X?

saturated –COOH present

A no no

B no yes

C yes no

D yes yes

37 Which hydrocarbon reacts with steam to produce ethanol?

A C2H4 B C2H6 C C3H6 D C3H8

17


38 Petroleum is a mixture of different hydrocarbons.

Which process is used to separate the petroleum into groups of similar hydrocarbons?

A combustion

B cracking

C fractional distillation

D reduction 39 Which row represents compounds in the same homologous series?

H C

H

H

C

H

H

C

H

H

H

H C

H

H

C

H

H

C

H

H

C

H

H

H

H C

H

H

C

H

H

C

H

H

H

H C

H

H

C

H

H

O H

H C

H

H

C

OH

H

C

H

H

H

C C

H

H

H

C

H

H

C

H

H

H

H C

H

H

C

H

H

H

H C

H

H

O

H

H

C H

H C

H

H

C

Br

H

C

H

H

H

H C

H

C

H

H

C

H

C

H

H

H

H C

H

H

C

O

O H

A

B

C

D

C C

H

H

H

C

H

H

C

H

H

H

H

H

18

© UCLES 2013 0620/13/O/N/13

40 The diagram shows a flow diagram.

petroleum

substance X

● burns with a yellow flame

● does not decolourise bromine water

substance Y

● decolourises bromine water

● undergoes addition polymerisation

Which type of organic compounds are X and Y?

substance X substance Y

A alcohol alkane

B alkane alkene

C alkene alkane

D alkane alcohol

19

© UCLES 2013 0620/13/O/N/13

BLANK PAGE

20



© UCLES 2013 0620/13/O/N/13

Gro

up

140

Ce

Cer

ium

58

141

PrP

rase

odym

ium

59

144

Nd

Neo

dym

ium

60

PmP

rom

ethi

um61

150

SmS

amar

ium

62

152

EuE

urop

ium

63

157

Gd

Gad

olin

ium

64

159

Tb Terb

ium

65

162

Dy

Dys

pros

ium

66

165

Ho

Hol

miu

m67

167

Er Erb

ium

68

169

Tm Thul

ium

69

173

YbY

tterb

ium

70

175

LuLu

tetiu

m71

232

Th Thor

ium

90

PaP

rota

ctin

ium

91

238 U

Ura

nium

92

Np

Nep

tuni

um93

PuP

luto

nium

94

Am

Am

eric

ium

95

Cm

Cur

ium

96

Bk

Ber

keliu

m97

Cf

Cal

iforn

ium

98

EsE

inst

eini

um99

Fm Ferm

ium

100

Md

Men

dele

vium

101

No

Nob

eliu

m10

2

LrLa

wre

nciu

m10

3

1 HH

ydro

gen

1

7 LiLi

thiu

m3

23 Na

Sod

ium

11

24 Mg

Mag

nesi

um12

40 Ca

Cal

cium

20

45 ScS

cand

ium

21

48 TiTi

tani

um22

51 VVa

nadi

um23

52 Cr

Chr

omiu

m24

55 Mn

Man

gane

se25

56 Fe Iron

26

59 Co

Cob

alt

27

59 Ni

Nic

kel

28

64 Cu

Cop

per

29

65 Zn Zinc

30

70 Ga

Gal

lium

31

27 Al

Alu

min

ium

13

11 B Bor

on5

12 CC

arbo

n6

14 NN

itrog

en7

16 OO

xyge

n8

19 FFl

uorin

e9

28 Si Sili

con

14

31 PP

hosp

horu

s15

32 S Sul

fur

16

35.5 Cl

Chl

orin

e17

40 Ar

Arg

on18

20 Ne

Neo

n10

4 He

Hel

ium

2

73 Ge

Ger

man

ium

32

75 As

Ars

enic

33

79 SeS

elen

ium

34

80 Br

Bro

min

e35

84 Kr

Kry

pton

36

39 KP

otas

sium

19

88 SrS

tront

ium

38

89 YY

ttriu

m39

91 ZrZi

rcon

ium

40

93 Nb

Nio

bium

41

96 Mo

Mol

ybde

num

42

TcTe

chne

tium

43

101

Ru

Rut

heni

um44

103

Rh

Rho

dium

45

106

PdP

alla

dium

46

108

Ag

Silv

er47

112

Cd

Cad

miu

m48

115

In Indi

um49

119

Sn Tin

50

122

SbA

ntim

ony

51

128

TeTe

lluriu

m52

127 I

Iodi

ne53

131

Xe Xen

on54

137

Ba

Bar

ium

56

139

LaLa

ntha

num

57

*

178

Hf

Haf

nium

72

181

TaTa

ntal

um73

184 W

Tung

sten

74

186

Re

Rhe

nium

75

190

Os

Osm

ium

76

192

Ir Iridi

um77

195 Pt

Pla

tinum

78

197

Au

Gol

d79

201

Hg

Mer

cury

80

204 Tl

Thal

lium

81

207

Pb Lead

82

209 Bi

Bis

mut

h83

PoP

olon

ium

84

At

Ast

atin

e85

Rn

Rad

on86

FrFr

anci

um87

227

Ac

Act

iniu

m89

9 Be

Ber

ylliu

m4

III

IIIIV

VV

IV

II0

85 Rb

Rub

idiu

m37

133

Cs

Cae

sium

55

226

Ra

Rad

ium

88

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3

at ro

om te

mpe

ratu

re a

nd p

ress

ure

(r.t.p

.).

a Xb

a =

rela

tive

atom

ic m

ass

X =

atom

ic s

ymbo

l

b =

prot

on (a

tom

ic) n

umbe

r

Key

* 58-

71 L

anth

anoi

d se

ries

90-1

03 A

ctin

oid

serie

s

DAT

A SH

EET

The

Perio

dic

Tabl

e of

the

Elem

ents


Write your Centre number, candidate number and name in the spaces at the top of this page.Write in dark blue or black pen.You may need to use a pencil for any diagrams, graphs or rough working.Do not use staples, paper clips, highlighters, glue or correction fl uid.DO NOT WRITE IN ANY BARCODES.

Answer all questions.Electronic calculators may be used.A copy of the Periodic Table is printed on page 16.You may lose marks if you do not show your working or if you do not use appropriate units.

At the end of the examination, fasten all your work securely together.The number of marks is given in brackets [ ] at the end of each question or part question.

CHEMISTRY 0620/21

Paper 2 October/November 2013

1 hour 15 minutes

Candidates answer on the Question Paper.

No Additional Materials are required.

UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONSInternational General Certifi cate of Secondary Education


[Turn overIB13 11_0620_21/3RP© UCLES 2013

*7249373810*

2

0620/21/O/N/13© UCLES 2013

ForExaminer’s

Use

1 (a) Choose from the list of elements below to answer the following questions.

calciumheliumiodinenickel

nitrogensodiumsulfur

Each element can be used once, more than once or not at all.

Which element:

(i) is an element present in most fertilisers, .................................................... [1]

(ii) is in Group VI of the Periodic Table, ........................................................... [1]

(iii) is in Period 5 of the Periodic Table, ............................................................ [1]

(iv) has a single electron shell containing two electrons, .................................. [1]

(v) is a transition element, ................................................................................ [1]

(vi) forms ions with a single negative charge? .................................................. [1]

(b) What is the meaning of the term element ?

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

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

(c) Many of the elements in the Periodic Table have metallic properties. Describe three physical properties which are typical of most metals.

1. .......................................................................................................................................

2. .......................................................................................................................................

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

[Total: 10]

3

0620/21/O/N/13© UCLES 2013 [Turn over

ForExaminer’s

Use

2 Hydrogen chloride is an acidic gas.

(a) (i) Complete the dot and cross diagram to show the electronic structure of hydrogen chloride.

HCl

[2]

(ii) Is hydrogen chloride a covalent or an ionic compound? Give a reason for your answer.

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

(b) Hydrogen chloride reacts with water to form hydrochloric acid. Which one of the following is the most likely pH of hydrochloric acid? Put a ring around the correct answer.

pH 2 pH 7 pH 9 pH 14[1]

(c) Hydrochloric acid reacts with both metal oxides and carbonates.

(i) Complete the word equation for the reaction of hydrochloric acid with calcium carbonate.

hydrochloric + calcium → ...................... + ...................... + ...................... acid carbonate ...................... ...................... [3]

(ii) Complete the symbol equation for the reaction of magnesium oxide with hydrochloric acid. Name the salt which is formed.

MgO + ......HCl → MgCl 2 + H2O

name of salt ......................................................................................................... [2]

4

0620/21/O/N/13© UCLES 2013

ForExaminer’s

Use

(d) A student reacted magnesium with hydrochloric acid to fi nd out how concentration affects the rate of reaction. The magnesium was in excess. He measured the volume of hydrogen produced at various time intervals.

The graph shows his results.

0 50 100 150 200 250 300 350

50

40

30

20

10

0

volu

me

of h

ydro

gen

/ cm

3

time / seconds

(i) At what time had the reaction just fi nished?

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

(ii) What volume of hydrogen gas is given off during the fi rst 50 seconds of the reaction?

volume of hydrogen ........................... cm3 [1]

(iii) The student repeated the experiment. State two factors, apart from the concentration of hydrochloric acid, that should be

kept constant when repeating the experiment.

1. ................................................................................................................................

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

[Total: 13]

5


ForExaminer’s

Use

3 Organic compounds can be put into groups called homologous series.

(a) Complete the following sentences about organic compounds and homologous series. Use words from the list below.

carbon chlorine different elements functional

hydrocarbon hydrogen oxide similar sulfur

Organic compounds usually contain atoms of ........................... and ........................... .

Each homologous series contains compounds with ................................. chemical

properties due to the presence of the same ................................. group. [4]

(b) Ethanol belongs to the alcohol homologous series.

(i) Draw the structure of ethanol, showing all atoms and bonds.

[2]

(ii) State the name of the two compounds formed when ethanol burns in excess air.

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

6

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ForExaminer’s

Use

(c) Salicylic acid is used to make aspirin. The structure of salicylic acid is shown below.

C

C

C C

C C

O H

H H

H

O OC

H

H

(i) On this structure, put a ring around the carboxylic acid functional group. [1]

(ii) How many carbon atoms are there in one molecule of salicylic acid?

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

(iii) When making drugs and medicines, it is important that the chemicals used are pure. State one other area of everyday life where purity is important.

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

[Total: 11]

7


ForExaminer’s

Use

4 The structures of diamond and graphite are shown below.

diamond graphite

= carbon atom

(a) Describe the similarities and differences between these structures.

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

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

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

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

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

..................................................................................................................................... [4]

(b) Graphite burns in excess air to form carbon dioxide. Describe a test for carbon dioxide.

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

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

(c) When graphite is burnt in a limited supply of air, carbon monoxide is formed. State one adverse effect of carbon monoxide on health.

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

(d) In the blast furnace for the production of iron, carbon monoxide reduces iron(III) oxide.

Fe2O3 + 3CO → 2Fe + 3CO2

How does this equation show that carbon monoxide is acting as a reducing agent?

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

(e) Iron(III) oxide and coke (carbon) are raw materials used in the production of iron. State the names of two other raw materials used in the blast furnace for the production

of iron.

1. .......................................................................................................................................

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

[Total: 10]

8

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ForExaminer’s

Use

5 Many plants contain coloured pigments. A student crushes some plant leaves in alcohol to extract the pigments. She then separates the pigments using the apparatus shown below.

(a) Write the correct labels in the boxes in the diagram above. [2]

(b) Draw an X on the diagram above to show where a drop of the pigment solution is placed at the start of the experiment. [1]

(c) After leaving the apparatus for half an hour, the pigments separated from each other. State the name given to this method of separating pigments.

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

(d) Some plants can absorb nickel from the ground. The nickel can then be extracted from the plants and purifi ed by electrolysis.

+ – rod ofpure nickel

electrolyte

rod ofimpure nickel

power supply

(i) Which one of the following is the most suitable electrolyte for this electrolysis. Tick one box.

aqueous copper(II) sulfate

aqueous nickel(II) sulfate

solid nickel(II) sulfate

water [1]

9


ForExaminer’s

Use

(ii) Which one of the following elements is most likely to be formed at the negative electrode during this electrolysis?

Put a ring around the correct answer.

chlorine nickel sulfur oxygen[1]

(iii) The positive electrode is called the anode. State the name of the negative electrode.

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

(e) Electroplating is used to put a thin layer of one metal on top of another by electrolysis. Give two reasons for electroplating metals.

1. .......................................................................................................................................

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

(f) (i) Hydrated nickel(II) chloride is green in colour. When hydrated nickel(II) chloride is heated gently, it changes colour from green to

white. Complete the symbol equation for this reaction.

NiCl 2.6H2O(s) NiCl 2(s) + .................... hydrated nickel(II) chloride [1]

(ii) What does the sign mean?

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

(iii) How can you obtain a sample of green nickel(II) chloride starting with white nickel(II) chloride?

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

[Total: 12]

10

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Use

6 The diagram shows a kettle of boiling water.

kettlewater vapour

water droplets

As the water vapour cools it turns back to water droplets.

(a) Describe this change of state in terms of the kinetic particle theory. In your answer, include

● the difference in the closeness of the water molecules as the water vapour changes to water,

● the difference in the motion of the water molecules as the water vapour changes to water.

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

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

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

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

..................................................................................................................................... [4]

(b) Water is a common solvent in the laboratory.

(i) What is meant by the term solvent ?

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

(ii) State the name of the solvent whose formula is C2H5OH.

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

(c) When ammonium chloride dissolves in water the temperature of the solution falls. State the name of the energy change which results in the temperature falling.

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

11


ForExaminer’s

Use

(d) Which one of the following conducts electricity. Tick one box.

aqueous ammonium chloride

solid ammonium chloride

ammonia gas

chlorine gas

[1]

(e) (i) Complete the symbol equation for the reaction of lithium with water to form lithium hydroxide and hydrogen.

2Li + .....H2O → 2.......... + H2[2]

(ii) When 14 g of lithium react with water, 4 g of hydrogen are formed. Calculate the mass of hydrogen formed when 70 g of lithium react with water.

[1]

[Total: 11]

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Use

7 The table shows some properties of seven different substances.

substance density/ g per cm3

relative strength

relative electrical conductivity

relative thermal

conductivity

aluminium 2.7 15 42 200.0

ceramic 2.5 15 does not conduct 1.6

copper 8.9 20 63 385.0

iron 7.9 25 11 80.0

lead 11.4 15 5 38.0

poly(ethene) 0.9 1 does not conduct 0.3

steel 7.8 90 2 25.0

(a) Use the information in this table to answer the following questions.

(i) Which substance is the best conductor of heat?

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

(ii) Suggest why copper is preferred to iron for electrical wiring in houses.

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

(iii) What property of ceramic makes it a good electrical insulator?

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

(iv) Which pure metal in the table conducts electricity least well?

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

(v) Suggest why steel rather than iron is used in making machinery.

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

(vi) Which metal in the table is the most dense?

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

(b) A solution of a metal salt reacts with aqueous sodium hydroxide to form a white precipitate. The white precipitate is soluble in excess aqueous sodium hydroxide.

(i) Which one of the following ions is most likely to be present in the salt? Put a ring around the correct answer.

calcium copper(II) iron(II) zinc[1]

(ii) State the name of the white precipitate.

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

13


ForExaminer’s

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(c) Copper(II) chloride can be made by the action of hydrochloric acid on copper(II) oxide. Put the statements, A, B, C and D, about this preparation in the correct order.

A Leave the saturated solution to crystallise. B Filter the solution to remove excess copper(II) oxide. C Add excess copper(II) oxide to hydrochloric acid and warm. D Evaporate the fi ltrate to the crystallisation point.

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

(d) The structure of copper(II) chloride is shown below.

Cu2+

Cu2+

Cu2+Cu2+

Cl – Cl –

Cl – Cl –

Cl – Cl –

Cu2+

Cu2+

Cl – Cl –

Cl – Cl –

Cl – Cl –

Write the simplest formula for copper(II) chloride.

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

(e) Suggest the product formed at each electrode when molten copper(II) chloride is electrolysed.

at the positive electrode ....................................................................................................

at the negative electrode ............................................................................................ [2]

(f) When copper(II) chloride is heated strongly, a gas is given off. The gas is green in colour and bleaches litmus paper. State the name of this gas.

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

[Total: 13]

14

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© UCLES 2013

15

0620/21/O/N/13

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© UCLES 2013

16

Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Everyreasonable 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.

University of Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.

0620/21/O/N/13© UCLES 2013

Gro

up

140

Ce

Cer

ium

58

141

PrP

rase

odym

ium

59

144

Nd

Neo

dym

ium

60

PmP

rom

ethi

um61

150

SmS

amar

ium

62

152

EuE

urop

ium

63

157

Gd

Gad

olin

ium

64

159

Tb Terb

ium

65

162

Dy

Dys

pros

ium

66

165

Ho

Hol

miu

m67

167

Er Erb

ium

68

169

Tm Thul

ium

69

173

YbY

tterb

ium

70

175

LuLu

tetiu

m71

232

Th Thor

ium

90

PaP

rota

ctin

ium

91

238 U

Ura

nium

92

Np

Nep

tuni

um93

PuP

luto

nium

94

Am

Am

eric

ium

95

Cm

Cur

ium

96

Bk

Ber

keliu

m97

Cf

Cal

iforn

ium

98

EsE

inst

eini

um99

Fm Ferm

ium

100

Md

Men

dele

vium

101

No

Nob

eliu

m10

2

LrLa

wre

nciu

m10

3

1 HH

ydro

gen

1

7 LiLi

thiu

m3

23 Na

Sod

ium

11

24 Mg

Mag

nesi

um12

40 Ca

Cal

cium

20

45 ScS

cand

ium

21

48 TiTi

tani

um22

51 VVa

nadi

um23

52 Cr

Chr

omiu

m24

55 Mn

Man

gane

se25

56 Fe Iron

26

59 Co

Cob

alt

27

59 Ni

Nic

kel

28

64 Cu

Cop

per

29

65 Zn Zinc

30

70 Ga

Gal

lium

31

27 Al

Alu

min

ium

13

11 B Bor

on5

12 CC

arbo

n6

14 NN

itrog

en7

16 OO

xyge

n8

19 FFl

uorin

e9

28 Si Sili

con

14

31 PP

hosp

horu

s15

32 S Sul

fur

16

35.5 Cl

Chl

orin

e17

40 Ar

Arg

on18

20 Ne

Neo

n10

4 He

Hel

ium

2

73 Ge

Ger

man

ium

32

75 As

Ars

enic

33

79 SeS

elen

ium

34

80 Br

Bro

min

e35

84 Kr

Kry

pton

36

39 KP

otas

sium

19

88 SrS

tront

ium

38

89 YY

ttriu

m39

91 ZrZi

rcon

ium

40

93 Nb

Nio

bium

41

96 Mo

Mol

ybde

num

42

TcTe

chne

tium

43

101

Ru

Rut

heni

um44

103

Rh

Rho

dium

45

106

PdP

alla

dium

46

108

Ag

Silv

er47

112

Cd

Cad

miu

m48

115

In Indi

um49

119

Sn Tin

50

122

SbA

ntim

ony

51

128

TeTe

lluriu

m52

127 I

Iodi

ne53

131

Xe Xen

on54

137

Ba

Bar

ium

56

139

LaLa

ntha

num

57

*

178

Hf

Haf

nium

72

181

TaTa

ntal

um73

184 W

Tung

sten

74

186

Re

Rhe

nium

75

190

Os

Osm

ium

76

192

Ir Iridi

um77

195 Pt

Pla

tinum

78

197

Au

Gol

d79

201

Hg

Mer

cury

80

204 Tl

Thal

lium

81

207

Pb Lead

82

209 Bi

Bis

mut

h83

PoP

olon

ium

84

At

Ast

atin

e85

Rn

Rad

on86

FrFr

anci

um87

227

Ac

Act

iniu

m89

9 Be

Ber

ylliu

m4

III

IIIIV

VV

IV

II0

85 Rb

Rub

idiu

m37

133

Cs

Cae

sium

55

226

Ra

Rad

ium

88

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3

at ro

om te

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(r.t.p

.).

a Xb

a =

rela

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atom

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X =

atom

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l

b =

prot

on (a

tom

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Key

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Elem

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CHEMISTRY 0620/22


1 hour 15 minutes






*5048513202*

2

0620/22/O/N/13

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© UCLES 2013

3


ForExaminer’s

Use

1 (a) Choose from the list of compounds below to answer the following questions.

ammoniaammonium chloridecalcium carbonate

calcium oxidecopper(II) sulfate

ethaneiron(II) chloride

methanewater

Each compound can be used once, more than once or not at all.

Which compound:

(i) is an alkaline gas, ................................................................................... [1]

(ii) is a gas contributing to climate change, ................................................. [1]

(iii) is a salt containing only non-metals, ....................................................... [1]

(iv) turns blue cobalt chloride paper pink, ..................................................... [1]

(v) reacts with an acid to release carbon dioxide, ........................................ [1]

(vi) gives a light blue precipitate when aqueous sodium hydroxide is added to a solution of its aqueous ions? ................................................................................ [1]

(b) What is the meaning of the term compound ?

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

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

(c) Complete the following symbol equation for the complete combustion of methane in oxygen.

CH4 + .......O2 → .................. + 2H2O[2]

[Total: 9]

4

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Use

2 (a) The table describes the reactivity of some metals with hydrochloric acid.

metal observations

calcium Many bubbles produced. Reaction mixture may boil.

magnesium Steady stream of bubbles produced. Reaction mixture gets hot.

sodium Many bubbles produced. May explode.

zinc Slow stream of bubbles produced. Reaction mixture rises slightly in temperature.

Put these metals in order of their reactivity.


[2]

(b) Complete the word equation for the reaction of magnesium with hydrochloric acid.

magnesium + hydrochloric acid → ............................ + ............................

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

(c) When magnesium reacts with hydrochloric acid, magnesium atoms lose electrons. What type of magnesium particle is formed? Put a ring around the correct answer.

covalent ion molecule proton[1]

(d) Complete the diagram to show the electronic structure of a sodium atom.

Na

[2]

5


ForExaminer’s

Use

(e) A student added large lumps of zinc to 20 cm3 of 2 mol / dm3 hydrochloric acid. She carried out the reaction at 15 °C. She measured the volume of gas given off at various time intervals.

(i) Draw a labelled diagram of the apparatus she could use for this experiment.

[3]

(ii) Describe three different things she could do to increase the rate of this reaction.

1. ................................................................................................................................

2. ................................................................................................................................

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

[Total: 13]

6

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Use

3 The diagram below shows the apparatus which can be used to obtain pure water fromsea-water.

heat

sea-water

pure water

(a) State the name of this process.

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

(b) Label the boxes on the diagram above with the correct names of the pieces of apparatus shown. [3]

(c) Complete the following sentences using words from the list below.

boils condenses cools freezes

higher lower melts

Water has a ............................. boiling point than salt. When a solution of salt is heated

strongly, the water ............................. and escapes as steam. When the steam cools, it

............................. back to liquid water. [3]

7


ForExaminer’s

Use

(d) The table shows the concentration of the seven most abundant compounds in sea-water.

compound ions present concentrationin g / m3

calcium carbonate Ca2+ and CO32– 100

calcium sulfate Ca2+ and SO42– 1 800

magnesium chloride Mg2+ and Cl – 6 800

magnesium sulfate 5 700

potassium bromide K+ and Br – 100

potassium chloride K+ and Cl – 800

sodium chloride Na+ and Cl – 28 000

(i) Which negative ion is present in the greatest concentration in sea-water?

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

(ii) Which positive ion is present in the lowest concentration in sea-water? .............................................................................................................................. [1]

(iii) Write the formulae of the two ions present in magnesium sulfate.

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

[Total: 11]

8

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Use

4 (a) Match the compounds on the left with the statements on the right. The fi rst one has been done for you.

butane

poly(ethene)

ethene

methane

ethanoic acid

a hydrocarbon containingfour carbon atoms

it decolourisesbromine water

it is the main constituentof natural gas

it contains a –COOHfunctional group

it has a very long chainof carbon atoms

[4]

(b) Methane and ethene are hydrocarbons.

(i) What is meant by the term hydrocarbon ?

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

(ii) The structure of ethene is shown below.

C C

H

H

H

H

Use this structure to explain why ethene is an unsaturated hydrocarbon.

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

(c) Molecules of ethene react together at high temperature and pressure to form poly(ethene).

Which one of the following words best describes the molecules of ethene in this reaction? Put a ring around the correct answer.

acids alkanes monomers polymers[1]

9


ForExaminer’s

Use

(d) Ethanoic acid can be made by the oxidation of ethanol.

(i) What is meant by the term oxidation ?

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

(ii) Ethanol can be made by fermentation. Complete the word equation for fermentation.

yeast.......................... → .......................... + ethanol

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

[Total: 10]

10

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ForExaminer’s

Use

5 (a) Explain why metals are often used in the form of alloys. In your answer, write about

● the structure of an alloy, ● why alloys are often more useful than pure metals.

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

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

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

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

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

(b) Iron is a transition element.

(i) Which two of the following statements about iron are correct? Tick two boxes.

A freshly-cut surface of iron is green in colour.

Iron exists in only one oxidation state in its compounds.

Iron has a high density.

Iron has a giant covalent structure.

Iron has a high melting point. [2]

(ii) Describe one method of rust prevention and explain how it works.

method .......................................................................................................................

how this works ...........................................................................................................

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

(c) Iron is used as a catalyst in the Haber process for making ammonia.

(i) What does the term catalyst mean?

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

(ii) Describe a test for ammonia.

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

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

11


ForExaminer’s

Use

(iii) Ammonia is used to make fertilisers. Explain why farmers need to add fertilisers to the soil.

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

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

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

[Total: 12]

12

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ForExaminer’s

Use

6 (a) Garlic is a vegetable that is often used in cooking. It has a strong smell. A student is cutting up garlic in the kitchen.

After a time, the smell of the garlic travels all over the house even though there are no currents of air.

Use the kinetic particle theory to explain why the smell of garlic travels all over the house.

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

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

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

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

(b) The smell of garlic is due to a compound containing sulfur. The structure of this compound (compound A) is shown below.

CH2 CH — CH2 — S — S — CH2 — CH CH2

compound A

(i) Write the molecular formula for this compound.

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

(ii) Another organic sulfur compound (compound B) is shown below.

CH2H2C

C2H5

S

CHC

compound B

By comparing the formulae of compound A and compound B, how can you tell that compound A has the higher relative molecular mass?

You are not required to do any mathematical calculations.

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

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

13


ForExaminer’s

Use

(c) An isotope of sulfur has a nucleon number of 34 and an atomic number of 16.

(i) How many neutrons are there in one atom of this isotope of sulfur?

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

(ii) What is meant by the terms

isotope, ......................................................................................................................

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

nucleon number ? ................................................................................................ [1]

(iii) Some fuels contain sulfur as a contaminating substance. Complete the following sentences using words from the list below.

coal dioxide hydrogen monoxide

nitrogen oxidised reduced water

Fuels such as ........................... contain sulfur.

When these fuels burn, the sulfur is ........................... to sulfur ........................... .

This reacts with ........................... in the atmosphere to form an acidic solution. [4]

(iv) Describe and explain the effect of acid rain on buildings made of limestone.

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

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

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

[Total: 15]

14

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Use

7 The diagram shows a kiln for making lime (calcium oxide) from limestone (calcium carbonate).

A

B

D

C

brick lime kiln

(a) (i) Which letter on the diagram above shows

where the limestone is added, ...................................................................................

where the waste gases exit from the kiln? ........................................................... [2]

(ii) Complete the symbol equation for the decomposition of limestone.

CaCO3 → CaO + .............[1]

(iii) When 50 g of calcium carbonate is decomposed, 28 g of calcium oxide is formed. Calculate the minimum mass of calcium carbonate needed to produce 8.4 g of

calcium oxide.

[1]

(b) The table below shows the temperatures at which some Group II carbonates decompose.

Group II carbonate temperature at which Group IIcarbonates decompose / °C

beryllium carbonate 100

magnesium carbonate 350

calcium carbonate 900

(i) Describe the pattern in the ease of decomposition of Group II carbonates.

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

15


ForExaminer’s

Use

(ii) Predict the decomposition temperature of barium carbonate.

......................... °C [1]

(c) Lime is calcium oxide.

(i) State one use of lime.

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

(ii) What type of oxide is calcium oxide?

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

(iii) Calculate the relative formula mass of calcium oxide. Use your Periodic Table to help you.

[1]

(d) Calcium is extracted from its compounds by electrolysis. Suggest why calcium is extracted by electrolysis rather than by reduction with carbon.

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

[Total: 10]

16



0620/22/O/N/13© UCLES 2013

Gro

up

140

Ce

Cer

ium

58

141

PrP

rase

odym

ium

59

144

Nd

Neo

dym

ium

60

PmP

rom

ethi

um61

150

SmS

amar

ium

62

152

EuE

urop

ium

63

157

Gd

Gad

olin

ium

64

159

Tb Terb

ium

65

162

Dy

Dys

pros

ium

66

165

Ho

Hol

miu

m67

167

Er Erb

ium

68

169

Tm Thul

ium

69

173

YbY

tterb

ium

70

175

LuLu

tetiu

m71

232

Th Thor

ium

90

PaP

rota

ctin

ium

91

238 U

Ura

nium

92

Np

Nep

tuni

um93

PuP

luto

nium

94

Am

Am

eric

ium

95

Cm

Cur

ium

96

Bk

Ber

keliu

m97

Cf

Cal

iforn

ium

98

EsE

inst

eini

um99

Fm Ferm

ium

100

Md

Men

dele

vium

101

No

Nob

eliu

m10

2

LrLa

wre

nciu

m10

3

1 HH

ydro

gen

1

7 LiLi

thiu

m3

23 Na

Sod

ium

11

24 Mg

Mag

nesi

um12

40 Ca

Cal

cium

20

45 ScS

cand

ium

21

48 TiTi

tani

um22

51 VVa

nadi

um23

52 Cr

Chr

omiu

m24

55 Mn

Man

gane

se25

56 Fe Iron

26

59 Co

Cob

alt

27

59 Ni

Nic

kel

28

64 Cu

Cop

per

29

65 Zn Zinc

30

70 Ga

Gal

lium

31

27 Al

Alu

min

ium

13

11 B Bor

on5

12 CC

arbo

n6

14 NN

itrog

en7

16 OO

xyge

n8

19 FFl

uorin

e9

28 Si Sili

con

14

31 PP

hosp

horu

s15

32 S Sul

fur

16

35.5 Cl

Chl

orin

e17

40 Ar

Arg

on18

20 Ne

Neo

n10

4 He

Hel

ium

2

73 Ge

Ger

man

ium

32

75 As

Ars

enic

33

79 SeS

elen

ium

34

80 Br

Bro

min

e35

84 Kr

Kry

pton

36

39 KP

otas

sium

19

88 SrS

tront

ium

38

89 YY

ttriu

m39

91 ZrZi

rcon

ium

40

93 Nb

Nio

bium

41

96 Mo

Mol

ybde

num

42

TcTe

chne

tium

43

101

Ru

Rut

heni

um44

103

Rh

Rho

dium

45

106

PdP

alla

dium

46

108

Ag

Silv

er47

112

Cd

Cad

miu

m48

115

In Indi

um49

119

Sn Tin

50

122

SbA

ntim

ony

51

128

TeTe

lluriu

m52

127 I

Iodi

ne53

131

Xe Xen

on54

137

Ba

Bar

ium

56

139

LaLa

ntha

num

57

*

178

Hf

Haf

nium

72

181

TaTa

ntal

um73

184 W

Tung

sten

74

186

Re

Rhe

nium

75

190

Os

Osm

ium

76

192

Ir Iridi

um77

195 Pt

Pla

tinum

78

197

Au

Gol

d79

201

Hg

Mer

cury

80

204 Tl

Thal

lium

81

207

Pb Lead

82

209 Bi

Bis

mut

h83

PoP

olon

ium

84

At

Ast

atin

e85

Rn

Rad

on86

FrFr

anci

um87

227

Ac

Act

iniu

m89

9 Be

Ber

ylliu

m4

III

IIIIV

VV

IV

II0

85 Rb

Rub

idiu

m37

133

Cs

Cae

sium

55

226

Ra

Rad

ium

88

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3

at ro

om te

mpe

ratu

re a

nd p

ress

ure

(r.t.p

.).

a Xb

a =

rela

tive

atom

ic m

ass

X =

atom

ic s

ymbo

l

b =

prot

on (a

tom

ic) n

umbe

r

Key

* 58-

71 L

anth

anoi

d se

ries

90-1

03 A

ctin

oid

serie

s

DAT

A SH

EET

The

Perio

dic

Tabl

e of

the

Elem

ents





CHEMISTRY 0620/23


1 hour 15 minutes






*3407475716*

2

0620/23/O/N/13© UCLES 2013

ForExaminer’s

Use

1 (a) Choose from the list of metals below to answer the following questions.

aluminiumbariumcalciumironlithiumsilver

Each metal can be used once, more than once or not at all.

(i) Which metal has an atom with three electrons in its outer electron shell?

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

(ii) Which two metals are in the same Period of the Periodic Table?

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

(iii) Which metal has an atom with three protons in its nucleus?

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

(iv) Which metal has a nitrate which is used to test for halide ions?

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

(v) Which metal is used in food containers because of its resistance to corrosion?

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

(b) Describe two chemical properties of iron.

1. .......................................................................................................................................

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

(c) Describe briefl y how iron from the blast furnace is made into steel.

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

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

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

[Total: 9]

3


ForExaminer’s

Use

2 Helium is in Group 0 of the Periodic Table.

(a) Describe the structure of a helium atom. Use your Periodic Table to help you. In your answer, include

● the type and number of subatomic particles present, ● the position of these particles in the atom, ● the relative charges on the particles.

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

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

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

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

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

..................................................................................................................................... [5]

(b) Give one use of helium.

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

(c) Some elements in Group 0 can form compounds with fl uorine and oxygen. The structure of one of these compounds is shown below.

XeFF

FO

F

Calculate the relative molecular mass of this compound. Use your Periodic Table to help you. You must show all your working.

[2]

(d) Fluorine is a diatomic molecule. It melts at –220 °C and boils at –188 °C.

(i) What is the physical state of fl uorine

at room temperature, .................................................................................................

at –200 °C? .......................................................................................................... [2]

(ii) What is meant by the term diatomic ?

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

[Total: 11]

4

0620/23/O/N/13© UCLES 2013

ForExaminer’s

Use

3 This question is about calcium and some calcium compounds.

(a) Calcium is in Group II of the Periodic Table. Complete the diagram below to show the electronic structure of calcium.

Ca

[2]

(b) Calcium reacts with hydrochloric acid to form a salt with the formula CaCl 2. State the name of this salt.

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

(c) Calcium carbonate reacts with hydrochloric acid. The course of this reaction can be followed by measuring the volume of carbon dioxide

given off at various time intervals. The graph below shows the results obtained from an experiment using 0.15 g of calcium

carbonate in small pieces.

0 50 100 150 200

time / seconds

250 300 350 400

volu

me

of c

arbo

n di

oxid

e / c

m3

50

40

30

20

10

0

5


ForExaminer’s

Use

(i) What volume of gas is given off in the fi rst 75 seconds of the reaction?

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

(ii) On the grid opposite, sketch the line you would expect for the same reaction using large pieces of calcium carbonate. Assume that the mass of the calcium carbonate and all other conditions remain the same. [2]

(iii) What would happen to the rate of this reaction if:

the temperature is increased,

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

the concentration of hydrochloric acid is decreased?

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

(d) When calcium carbonate is heated at high temperatures, calcium oxide and carbon dioxide are formed.

(i) Which one of the following words best describes this reaction? Put a ring around the correct answer.

combustion decomposition exothermic reduction[1]

(ii) Describe a test for carbon dioxide.

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

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

(e) Calcium oxide can be used to neutralise acidic industrial waste.

(i) Complete the word equation for the reaction of calcium oxide with nitric acid.

calcium oxide + nitric acid → ........................ + ........................

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

(ii) State one other use of calcium oxide.

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

(iii) When calcium oxide reacts with water, heat is given off. State the name given to a chemical reaction which gives off heat.

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

[Total: 15]

6

0620/23/O/N/13© UCLES 2013

ForExaminer’s

Use

4 The diagram shows how a liquid alkane can be cracked in a school laboratory to form a mixture of gaseous and liquid hydrocarbons.

water

catalyst(aluminium oxide granules)

liquid alkane(absorbed in mineral wool)

(a) What piece of apparatus is missing from the diagram?

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

(b) On the diagram above, put an X to show where the gas is collected. [1]

(c) What is the purpose of the catalyst?

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

(d) Complete the equation to show the cracking of dodecane, C12H26, to form octane and one other substance.

C12H26 → C8H18 + .................[1]

(e) Cracking produces a mixture of shorter-chain alkanes and alkenes.

(i) Describe what you would observe when a few drops of bromine water are added to an alkene.

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

7


ForExaminer’s

Use

(ii) Which one of the following compounds, A, B, C or D, is formed when bromine water reacts with ethene?

C

H H

C

A

Br Br

CH

H H

C H

B

Br Br

CH C H

OH OH

OH OH

C

C C

D

Br Br

BrBr

Br Br

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

(iii) Poly(ethene) is made by combining ethene monomers. Which one of the following describes this reaction? Tick one box.

decomposition

neutralisation

oxidation

polymerisation [1]

(f) Many alkanes found in petrol are branched hydrocarbons. One example is shown below.

C C

C

H

H

H H

C

H

H

C C

H

H

H

H

H

H

HH

H

H

C

(i) Write the molecular formula for this hydrocarbon.

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

(ii) What is meant by the term hydrocarbon ?

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

(g) State the name of the two products formed when a hydrocarbon burns in excess air.

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

[Total: 11]

8

0620/23/O/N/13© UCLES 2013

ForExaminer’s

Use

5 Ethanol can be made by fermentation.

fermentationmixture

U-shaped tubecontaining water

(a) Apart from yeast, what other substances are present in the reaction mixture? Tick two boxes.

copper sulfate

ethene

sugar

methane

water [2]

(b) What method is used to separate ethanol from the rest of the reaction mixture?

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

(c) Complete the structure of ethanol.

CC

H

H

H

H

H

[1]

(d) Ethanol belongs to the alcohol homologous series. Which one of the following compounds also belongs to the alcohol homologous series? Put a ring around the correct answer.

butene hexane ethanoic acid octanol[1]

(e) Describe one other way, apart from fermentation, by which ethanol can be made on an industrial scale. Include the necessary reaction conditions in your answer.

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

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

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

[Total: 8]

9


ForExaminer’s

Use

6 (a) When hydrated copper(II) sulfate is heated, the following reaction occurs:

CuSO4.5H2O(s) CuSO4(s) + 5H2O(l) hydrated copper(II) sulfate anhydrous copper(II) sulfate

(i) What does the sign mean?

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

(ii) Explain how this reaction is used as a chemical test for water.

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

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

(iii) Copper(II) sulfate is a salt. Sodium chloride is also a salt. Solid sodium chloride does not conduct electricity. Suggest two things you could do to make solid sodium chloride conduct electricity.

1. ................................................................................................................................

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

(b) Copper ore contains copper, iron and sulfur. Copper is extracted by heating copper ore with sand and oxygen.

(i) In the fi rst stage of this process, the copper ore is heated in a furnace. A liquid mixture containing copper sulfi de and iron sulfi de is formed. The sand reacts

with the impurities to form a slag.

waste gases

oxygen

slag out

mixture out

slag

mixture ofcopper sulfide+ iron sulfide

What information in the diagram above suggests that the slag is less dense than the mixture of copper and iron sulfi des.

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

10

0620/23/O/N/13© UCLES 2013

ForExaminer’s

Use

(ii) In a later stage, copper sulfi de is reacted with more oxygen.

Cu2S + O2 → 2Cu + SO2

How does this equation show that the sulfur in copper sulfi de gets oxidised?

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

(iii) Copper is purifi ed by electrolysis using copper electrodes.

+ –

A

C

D

B

Which letter, A, B, C or D, in the diagram above represents

the cathode, ...............................................................................................................

the electrolyte? .................................................................................................... [2]

[Total: 9]

11


ForExaminer’s

Use

7 The graph below shows how the temperature rises with time when a solid, P, is heated steadily and changes to a liquid and then to a gas.

0 20 40 60

200

180

160

140

120

100

80

60

40

20

0

tem

pera

ture

/ °C

time / seconds

(a) Use the information on the graph to deduce

the melting point of P, .......................................................................................................

the state of P at 160 °C. .............................................................................................. [2]

(b) Explain what happens to the arrangement and motion of the particles when a solid changes to a liquid.

arrangement .....................................................................................................................

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

12

0620/23/O/N/13© UCLES 2013

ForExaminer’s

Use

(c) A student placed a purple crystal in a fl ask of organic solvent. After 10 minutes, the crystal had completely disappeared and a dense purple colour was

observed at the bottom of the fl ask. After 2 hours, the purple colour had spread throughout the solvent.

organicsolvent

crystal at start

after 10 minutes after 2 hours

Use the kinetic particle theory to explain these observations.

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

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

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

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

[Total: 7]

13


ForExaminer’s

Use

8 (a) State two differences between a mixture and a compound.

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

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

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

(b) Plant ash is a mixture of large insoluble particles and salts which are soluble in water.

In parts of Africa, salts are traditionally obtained from plant ash. Water is added to the plant ash. The apparatus shown below is then used to remove the insoluble particles.

clay pot

clay bowl

holes inclay bowl

plant ashand water strips of banana leaf

with holes in them

Explain how this apparatus separates the salts from the insoluble particles.

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

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

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

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

14

0620/23/O/N/13© UCLES 2013

ForExaminer’s

Use

(c) The composition and solubility of some salts found in the ash from the papyrus plant are shown in the table below.

salt ion presentin the salt

mass of salt per100 g of ash / g

solubility of saltin g / dm3

magnesium sulfate Mg2+ and SO42– 5 220

potassium carbonate K+ and CO32– 10 1120

potassium chloride K+ and Cl – 18 359

potassium sulfate 4 122

sodium carbonate Na+ and CO32– 12 70

sodium chloride Na+ and Cl – 40 359

(i) Which salt in the table has the lowest solubility in g / dm3?

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

(ii) Which negatively-charged ion is present in the highest amount in the ash?

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

(iii) Write the symbols for the two ions present in potassium sulfate.

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

(d) Sodium chloride reacts with lead(II) nitrate to form sodium nitrate and lead(II) chloride. Complete the symbol equation for this reaction.

.......NaCl + Pb(NO3)2 → 2NaNO3 + PbCl 2[1]

(e) Complete the following sentence about the formation of chloride ions.

Chloride ions are formed when chlorine atoms gain .................................... . [1]

[Total: 10]

15

0620/23/O/N/13

BLANK PAGE

© UCLES 2013

16



0620/23/O/N/13© UCLES 2013

Gro

up

140

Ce

Cer

ium

58

141

PrP

rase

odym

ium

59

144

Nd

Neo

dym

ium

60

PmP

rom

ethi

um61

150

SmS

amar

ium

62

152

EuE

urop

ium

63

157

Gd

Gad

olin

ium

64

159

Tb Terb

ium

65

162

Dy

Dys

pros

ium

66

165

Ho

Hol

miu

m67

167

Er Erb

ium

68

169

Tm Thul

ium

69

173

YbY

tterb

ium

70

175

LuLu

tetiu

m71

232

Th Thor

ium

90

PaP

rota

ctin

ium

91

238 U

Ura

nium

92

Np

Nep

tuni

um93

PuP

luto

nium

94

Am

Am

eric

ium

95

Cm

Cur

ium

96

Bk

Ber

keliu

m97

Cf

Cal

iforn

ium

98

EsE

inst

eini

um99

Fm Ferm

ium

100

Md

Men

dele

vium

101

No

Nob

eliu

m10

2

LrLa

wre

nciu

m10

3

1 HH

ydro

gen

1

7 LiLi

thiu

m3

23 Na

Sod

ium

11

24 Mg

Mag

nesi

um12

40 Ca

Cal

cium

20

45 ScS

cand

ium

21

48 TiTi

tani

um22

51 VVa

nadi

um23

52 Cr

Chr

omiu

m24

55 Mn

Man

gane

se25

56 Fe Iron

26

59 Co

Cob

alt

27

59 Ni

Nic

kel

28

64 Cu

Cop

per

29

65 Zn Zinc

30

70 Ga

Gal

lium

31

27 Al

Alu

min

ium

13

11 B Bor

on5

12 CC

arbo

n6

14 NN

itrog

en7

16 OO

xyge

n8

19 FFl

uorin

e9

28 Si Sili

con

14

31 PP

hosp

horu

s15

32 S Sul

fur

16

35.5 Cl

Chl

orin

e17

40 Ar

Arg

on18

20 Ne

Neo

n10

4 He

Hel

ium

2

73 Ge

Ger

man

ium

32

75 As

Ars

enic

33

79 SeS

elen

ium

34

80 Br

Bro

min

e35

84 Kr

Kry

pton

36

39 KP

otas

sium

19

88 SrS

tront

ium

38

89 YY

ttriu

m39

91 ZrZi

rcon

ium

40

93 Nb

Nio

bium

41

96 Mo

Mol

ybde

num

42

TcTe

chne

tium

43

101

Ru

Rut

heni

um44

103

Rh

Rho

dium

45

106

PdP

alla

dium

46

108

Ag

Silv

er47

112

Cd

Cad

miu

m48

115

In Indi

um49

119

Sn Tin

50

122

SbA

ntim

ony

51

128

TeTe

lluriu

m52

127 I

Iodi

ne53

131

Xe Xen

on54

137

Ba

Bar

ium

56

139

LaLa

ntha

num

57

*

178

Hf

Haf

nium

72

181

TaTa

ntal

um73

184 W

Tung

sten

74

186

Re

Rhe

nium

75

190

Os

Osm

ium

76

192

Ir Iridi

um77

195 Pt

Pla

tinum

78

197

Au

Gol

d79

201

Hg

Mer

cury

80

204 Tl

Thal

lium

81

207

Pb Lead

82

209 Bi

Bis

mut

h83

PoP

olon

ium

84

At

Ast

atin

e85

Rn

Rad

on86

FrFr

anci

um87

227

Ac

Act

iniu

m89

9 Be

Ber

ylliu

m4

III

IIIIV

VV

IV

II0

85 Rb

Rub

idiu

m37

133

Cs

Cae

sium

55

226

Ra

Rad

ium

88

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3

at ro

om te

mpe

ratu

re a

nd p

ress

ure

(r.t.p

.).

a Xb

a =

rela

tive

atom

ic m

ass

X =

atom

ic s

ymbo

l

b =

prot

on (a

tom

ic) n

umbe

r

Key

* 58-

71 L

anth

anoi

d se

ries

90-1

03 A

ctin

oid

serie

s

DAT

A SH

EET

The

Perio

dic

Tabl

e of

the

Elem

ents


Write your Centre number, candidate number and name on all the work you hand in.Write in dark blue or black pen.You may use a pencil for any diagrams, graphs or rough working.Do not use staples, paper clips, highlighters, glue or correction fl uid.DO NOT WRITE IN ANY BARCODES.



CHEMISTRY 0620/31

Paper 3 (Extended) October/November 2013

1 hour 15 minutes





[Turn overIB13 11_0620_31/3RP R© UCLES 2013

2

0620/31/O/N/13© UCLES 2013

ForExaminer’s

Use

1 For each of the following, name an element which matches the description.

(a) It is used as a fuel in nuclear reactors.

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

(b) It is the only non-metal which is a good conductor of electricity.

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

(c) Inert electrodes are made from this metal.

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

(d) This gaseous element is used to fi ll balloons in preference to hydrogen.

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

(e) An element which can form an ion of the type X3–.

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

(f) It has the same electron distribution as the calcium ion, Ca2+.

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

(g) The element is in Period 5 and Group VI.

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

[Total: 7]

3


ForExaminer’s

Use

2 (a) Give three differences in physical properties between the Group I metal, potassium, and the transition element, iron.

1. .......................................................................................................................................

2. .......................................................................................................................................

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

(b) The following metals are in order of reactivity.

potassium zinc copper

For those metals which react with water or steam, name the products of the reaction, otherwise write ‘no reaction’.

potassium .........................................................................................................................

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

zinc ...................................................................................................................................

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

copper ...............................................................................................................................

..................................................................................................................................... [5]

[Total: 8]

4

0620/31/O/N/13© UCLES 2013

ForExaminer’s

Use

3 Ammonia is manufactured by the Haber process.

N2(g) + 3H2(g) 2NH3(g)

The forward reaction is exothermic.

(a) Describe how the reactants are obtained.

(i) Nitrogen

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

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

(ii) Hydrogen

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

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

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

(b) The percentage of ammonia in the equilibrium mixture varies with temperature and pressure.

(i) Which pair of graphs, A, B or C, shows correctly how the percentage of ammonia at equilibrium varies with temperature and pressure?

percentageNH3 atequilibrium

temperature


pressure

pair A


temperature


pressure

pair B


temperature


pressure

pair C

The pair with both graphs correct is ................................................................. [1]

5


ForExaminer’s

Use

(ii) Give a full explanation of why the pair of graphs you have chosen in (i) is correct.

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

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

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

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

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

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

.............................................................................................................................. [6]

(iii) Catalysts do not alter the position of equilibrium. Explain why a catalyst is used in this process.

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

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

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

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

[Total: 14]

6

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ForExaminer’s

Use

4 20.0 g of small lumps of calcium carbonate and 40 cm3 of hydrochloric acid, concentration 2.0 mol / dm3, were placed in a fl ask on a top pan balance. The mass of the fl ask and contents was recorded every minute.

cotton wool to preventdrops of acid spray escaping

flask

40 cm3 of hydrochloric acid, 2.0 mol / dm3

20.0 g of small lumps ofcalcium carbonate

balance

The mass of carbon dioxide given off was plotted against time.

00 time

mass ofcarbon dioxide

CaCO3(s) + 2HCl (aq) CaCl 2(aq) + H2O(l) + CO2(g)

In all the experiments mentioned in this question, the calcium carbonate was in excess.

(a) (i) Explain how you could determine the mass of carbon dioxide given off in the fi rst fi ve minutes.

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

(ii) Label the graph F where the reaction rate is the fastest, S where it is slowing down and 0 where the rate is zero. [2]

(iii) Explain how the shape of the graph shows where the rate is fastest, where it is slowing down and where the rate is zero.

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

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

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

(b) Sketch on the same graph, the line which would have been obtained if 20.0 g of small lumps of calcium carbonate and 80 cm3 of hydrochloric acid, concentration 1.0 mol / dm3, had been used. [2]

7


ForExaminer’s

Use

(c) Explain in terms of collisions between reacting particles each of the following.

(i) The reaction rate would be slower if 20.0 g of larger lumps of calcium carbonate and 40 cm3 of hydrochloric acid, concentration 2.0 mol / dm3, were used.

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

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

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

(ii) The reaction rate would be faster if the experiment was carried out at a higher temperature.

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

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

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

(d) Calculate the maximum mass of carbon dioxide given off when 20.0 g of small lumps of calcium carbonate react with 40 cm3 of hydrochloric acid, concentration 2.0 mol / dm3.

CaCO3(s) + 2HCl (aq) CaCl 2(aq) + H2O(l) + CO2(g)

number of moles of HCl used =

mass of carbon dioxide = ................. g [4]

[Total: 15]

8

0620/31/O/N/13© UCLES 2013

ForExaminer’s

Use

5 The alkenes are unsaturated hydrocarbons. They form a homologous series, the members of which have the same chemical properties.

They undergo addition reactions and are easily oxidised.

(a) The following hydrocarbons are isomers.

CH3

CH3

CH2CH CH CH3 CH2CH2CH2 CH

(i) Explain why these two hydrocarbons are isomers.

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

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

(ii) Give the structural formula of another hydrocarbon which is isomeric with the above.

[1]

(b) Give the structural formula and name of each of the products of the following addition reactions.

(i) ethene and bromine

structural formula of product

name of product ................................................................................................... [2]

(ii) propene and hydrogen


name of product ................................................................................................... [2]

(iii) but-1-ene and water


name of product ................................................................................................... [2]

9


ForExaminer’s

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(c) Alkenes can be oxidised to carboxylic acids.

(i) For example, propene, CH3 – CH = CH2, would produce ethanoic acid, CH3 – COOH, and methanoic acid, H – COOH. Deduce the formulae of the alkenes which would form the following carboxylic acids when oxidised.

ethanoic acid and propanoic acid

only ethanoic acid

[2]

(ii) Describe the colour change you would observe when an alkene is oxidised with acidifi ed potassium manganate(VII).

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

(d) Alkenes polymerise to form addition polymers. Draw the structural formula of poly(cyanoethene), include at least two monomer units.

The structural formula of the monomer, cyanoethene, is given below.

C C

H

CN

H

H

[3]

[Total: 16]

10

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ForExaminer’s

Use

6 Lead is an excellent roofi ng material. It is malleable and resistant to corrosion. Lead rapidly becomes coated with basic lead carbonate which protects it from further corrosion.

(a) Lead has a typical metallic structure which is a lattice of lead ions surrounded by a ‘sea’ of mobile electrons. This structure is held together by attractive forces called a metallic bond.

(i) Explain why there are attractive forces in a metallic structure.

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

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

(ii) Explain why a metal, such as lead, is malleable.

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

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

(b) Basic lead(II) carbonate is heated in the apparatus shown below. Water and carbon dioxide are produced.

soda lime,carbon dioxidereacts here

basic leadcarbonate

heat

U-tube filledwith silica gel

to absorb water

(i) Silica gel absorbs water. Silica gel often contains anhydrous cobalt(II) chloride. When this absorbs water it changes from blue to pink.

Suggest a reason.

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

(ii) Soda lime is a mixture of sodium hydroxide and calcium oxide. Why do these two substances react with carbon dioxide?

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

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

(iii) Name two substances formed when soda lime reacts with carbon dioxide.

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

11


ForExaminer’s

Use

(c) Basic lead(II) carbonate has a formula of the type xPbCO3.yPb(OH)2 where x and y are whole numbers.

Determine x and y from the following information.

PbCO3 PbO + CO2

Pb(OH)2 PbO + H2O

When heated, the basic lead(II) carbonate gave 2.112 g of carbon dioxide and 0.432 g of water.

Mass of one mole of CO2 = 44 g Mass of one mole of H2O = 18 g

Number of moles of CO2 formed = ..................... [1]

Number of moles of H2O formed = ..................... [1]

x = ..................... and y = .....................

Formula of basic lead(II) carbonate is ........................................................................ [1]

[Total: 12]

12

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Use

7 (a) The following are two examples of substitution reactions. Only the reaction involving chlorine is a photochemical reaction.

CH4 + Cl 2 CH3Cl + HCl

CH4 + Br2 CH3Br + HBr

(i) Explain the phrase substitution reaction.

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

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

(ii) How do photochemical reactions differ from other reactions?

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

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

(b) Bond forming is exothermic, bond breaking is endothermic. Explain the difference between an exothermic reaction and an endothermic reaction.

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

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

13


ForExaminer’s

Use

(c) Use the bond energies to show that the following reaction is exothermic. Bond energy is the amount of energy (kJ / mol) which must be supplied to break one mole

of the bond.

H C

H

H

H H C

H

H

Cl Cl Cl H Cl+ +→

Bond energies in kJ / mol

Cl –Cl +242 C–Cl +338 C–H +412 H–Cl +431

bonds broken energy in kJ / mol

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

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

total energy = .............................

bonds formed energy in kJ / mol

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

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

total energy = .............................

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

..................................................................................................................................... [4]

[Total: 8]

14

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0620/31/O/N/13

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© UCLES 2013

16



0620/31/O/N/13© UCLES 2013

Gro

up

140

Ce

Cer

ium

58

141

PrP

rase

odym

ium

59

144

Nd

Neo

dym

ium

60

PmP

rom

ethi

um61

150

SmS

amar

ium

62

152

EuE

urop

ium

63

157

Gd

Gad

olin

ium

64

159

Tb Terb

ium

65

162

Dy

Dys

pros

ium

66

165

Ho

Hol

miu

m67

167

Er Erb

ium

68

169

Tm Thul

ium

69

173

YbY

tterb

ium

70

175

LuLu

tetiu

m71

232

Th Thor

ium

90

PaP

rota

ctin

ium

91

238 U

Ura

nium

92

Np

Nep

tuni

um93

PuP

luto

nium

94

Am

Am

eric

ium

95

Cm

Cur

ium

96

Bk

Ber

keliu

m97

Cf

Cal

iforn

ium

98

EsE

inst

eini

um99

Fm Ferm

ium

100

Md

Men

dele

vium

101

No

Nob

eliu

m10

2

LrLa

wre

nciu

m10

3

1 HH

ydro

gen

1

7 LiLi

thiu

m3

23 Na

Sod

ium

11

24 Mg

Mag

nesi

um12

40 Ca

Cal

cium

20

45 ScS

cand

ium

21

48 TiTi

tani

um22

51 VVa

nadi

um23

52 Cr

Chr

omiu

m24

55 Mn

Man

gane

se25

56 Fe Iron

26

59 Co

Cob

alt

27

59 Ni

Nic

kel

28

64 Cu

Cop

per

29

65 Zn Zinc

30

70 Ga

Gal

lium

31

27 Al

Alu

min

ium

13

11 B Bor

on5

12 CC

arbo

n6

14 NN

itrog

en7

16 OO

xyge

n8

19 FFl

uorin

e9

28 Si Sili

con

14

31 PP

hosp

horu

s15

32 S Sul

fur

16

35.5 Cl

Chl

orin

e17

40 Ar

Arg

on18

20 Ne

Neo

n10

4 He

Hel

ium

2

73 Ge

Ger

man

ium

32

75 As

Ars

enic

33

79 SeS

elen

ium

34

80 Br

Bro

min

e35

84 Kr

Kry

pton

36

39 KP

otas

sium

19

88 SrS

tront

ium

38

89 YY

ttriu

m39

91 ZrZi

rcon

ium

40

93 Nb

Nio

bium

41

96 Mo

Mol

ybde

num

42

TcTe

chne

tium

43

101

Ru

Rut

heni

um44

103

Rh

Rho

dium

45

106

PdP

alla

dium

46

108

Ag

Silv

er47

112

Cd

Cad

miu

m48

115

In Indi

um49

119

Sn Tin

50

122

SbA

ntim

ony

51

128

TeTe

lluriu

m52

127 I

Iodi

ne53

131

Xe Xen

on54

137

Ba

Bar

ium

56

139

LaLa

ntha

num

57

*

178

Hf

Haf

nium

72

181

TaTa

ntal

um73

184 W

Tung

sten

74

186

Re

Rhe

nium

75

190

Os

Osm

ium

76

192

Ir Iridi

um77

195 Pt

Pla

tinum

78

197

Au

Gol

d79

201

Hg

Mer

cury

80

204 Tl

Thal

lium

81

207

Pb Lead

82

209 Bi

Bis

mut

h83

PoP

olon

ium

84

At

Ast

atin

e85

Rn

Rad

on86

FrFr

anci

um87

227

Ac

Act

iniu

m89

9 Be

Ber

ylliu

m4

III

IIIIV

VV

IV

II0

85 Rb

Rub

idiu

m37

133

Cs

Cae

sium

55

226

Ra

Rad

ium

88

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3

at ro

om te

mpe

ratu

re a

nd p

ress

ure

(r.t.p

.).

a Xb

a =

rela

tive

atom

ic m

ass

X =

atom

ic s

ymbo

l

b =

prot

on (a

tom

ic) n

umbe

r

Key

* 58-

71 L

anth

anoi

d se

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90-1

03 A

ctin

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DAT

A SH

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The

Perio

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Tabl

e of

the

Elem

ents





CHEMISTRY 0620/32


1 hour 15 minutes






*3900490383*

2

0620/32/O/N/13© UCLES 2013

ForExaminer’s

Use

1 The table gives the melting points, the boiling points and the electrical properties of six substances A to F.

substance melting point/ °C

boiling point/ °C

electrical conductivityas a solid

electrical conductivityas a liquid

A –210 –196 does not conduct does not conduct

B 777 1627 does not conduct good conductor

C 962 2212 good conductor good conductor

D –94 63 does not conduct does not conduct

E 1410 2355 does not conduct does not conduct

F 1064 2807 good conductor good conductor

(a) Which two substances could be metals? ................................................................... [1]

(b) Which substance could be nitrogen? .......................................................................... [1]

(c) Which substance is an ionic solid? ............................................................................. [1]

(d) Which substance is a liquid at room temperature? ..................................................... [1]

(e) Which substance has a giant covalent structure similar to that of diamond? .............. [1]

(f) Which two substances could exist as simple covalent molecules? ........................... [1]

[Total: 6]

3


ForExaminer’s

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2 The halogens are a collection of diatomic non-metals in Group VII.

(a) (i) Defi ne the term diatomic.

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

(ii) What do the electron distributions of the halogens have in common?

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

(iii) How do their electron distributions differ?

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

(iv) Complete the table.

halogen solid, liquid or gasat room temperature colour

chlorine ......................................... .........................................

bromine ......................................... .........................................

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

(b) The halogens react with other non-metals to form covalent compounds. Draw a diagram which shows the arrangement of the valency electrons in one molecule

of the covalent compound arsenic trifl uoride. The electron distribution of an arsenic atom is 2 + 8 + 18 + 5.

Use x to represent an electron from an arsenic atom. Use o to represent an electron from a fl uorine atom.

[3]

4

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(c) Photochromic glass is used in sunglasses. In bright light, the glass darkens reducing the amount of light reaching the eye. When the light is less bright, the glass becomes colourless increasing the amount of light reaching the eye.

Photochromic glass contains very small amounts of the halides silver(I) chloride and copper(I) chloride.

The reaction between these two chlorides is photochemical.

AgCl + CuCl Ag + CuCl 2 colourless colourless black colourless

How does photochromic glass work?

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

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

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

[Total: 11]

5


ForExaminer’s

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3 (a) Nitric acid is now made by the oxidation of ammonia. It used to be made from air and water. This process used very large amounts of electricity.

Air was blown through an electric arc and heated to 3000 °C.

N2(g) + O2(g) 2NO(g) equilibrium 1 nitric oxide

The equilibrium mixture leaving the arc contained 5 % of nitric oxide. This mixture was cooled rapidly. At lower temperatures, nitric oxide will react with oxygen to form nitrogen dioxide.

2NO(g) + O2(g) 2NO2 equilibrium 2

Nitrogen dioxide reacts with oxygen and water to form nitric acid.

(i) Suggest a reason why the yield of nitric oxide in equilibrium 1 increases with temperature.

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

(ii) What effect, if any, would increasing the pressure have on the percentage of nitric oxide in equilibrium 1? Explain your answer.

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

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

(iii) Deduce why equilibrium 2 is only carried out at lower temperatures.

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

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

(iv) Complete the equation for the reaction between nitrogen dioxide, water and oxygen to form nitric acid.

........NO2 + O2 + ............ → ............HNO3 [2]

(v) Ammonia is more expensive than water and air. Suggest a reason why theammonia-based process is preferred to the electric arc process.

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

6

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Use

(b) (i) Nitric acid is used to make the fertiliser ammonium nitrate, NH4NO3. What advantage has this fertiliser over another common fertiliser, ammonium sulfate,

(NH4)2SO4?

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

(ii) Plants need nitrogen to make chlorophyll. Explain why chlorophyll is essential for plant growth.

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

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

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

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

.............................................................................................................................. [4]

[Total: 13]

7


ForExaminer’s

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4 For centuries, iron has been extracted from its ore in the blast furnace. The world production of pig iron is measured in hundreds of million tonnes annually.

(a) The following raw materials are supplied to a modern blast furnace.

iron ore which is hematite, Fe2O3

limestone which is calcium carbonate carbon in the form of coke air

Describe the essential reactions in the blast furnace. Each of the four raw materials must be mentioned at least once. Give the equation for the reduction of hematite.

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

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

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

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

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

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

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

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

..................................................................................................................................... [6]

(b) Each year, blast furnaces discharge millions of tonnes of carbon dioxide into the atmosphere. This will increase the percentage of atmospheric carbon dioxide.

(i) Explain why this increased percentage of carbon dioxide may cause problems in the future.

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

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

(ii) Until the early eighteenth century, charcoal, not coke, was used in the blast furnace. Charcoal is made from wood but coke is made from coal. Explain why the use of charcoal would have a smaller effect on the level of atmospheric carbon dioxide.

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

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

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

8

0620/32/O/N/13© UCLES 2013

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Use

(iii) A method being developed to produce iron with lower emissions of carbon dioxide is by electrolysis. Hematite, Fe2O3, is dissolved in molten lithium carbonate and electrolysed. The ore is spilt into its constituent elements.

Write an equation for the reaction at the negative electrode (cathode).

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

Complete the equation for the reaction at the positive electrode (anode).

........O2– → ............... + ............... [3]

[Total: 13]

9


ForExaminer’s

Use

5 Silver(I) chromate(VI) is an insoluble salt. It is prepared by precipitation. 20 cm3 of aqueous silver(I) nitrate, concentration 0.2 mol / dm3, was mixed with 20 cm3 of

aqueous potassium chromate(VI), concentration 0.1 mol / dm3. After stirring, the mixture was fi ltered. The precipitate was washed several times with distilled water. The precipitate was then left in a warm oven for several hours.

2AgNO3(aq) + K2CrO4(aq) → Ag2CrO4(s) + 2KNO3(aq)

(a) What diffi culty arises if the name of a compound of a transition element does not include its oxidation state, for example iron oxide?

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

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

(b) These questions refer to the preparation of the salt.

(i) Why is it necessary to fi lter the mixture after mixing and stirring?

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

(ii) What is the purpose of washing the precipitate?

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

(iii) Why leave the precipitate in a warm oven?

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

(c) (i) Explain why the concentrations of silver(I) nitrate and potassium chromate(VI) are different.

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

(ii) What mass of silver(I) nitrate is needed to prepare 100 cm3 of silver(I) nitrate solution, concentration 0.2 mol / dm3?

The mass of one mole of AgNO3 is 170 g.

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

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

(iii) What is the maximum mass of silver(I) chromate(VI) which could be obtained from 20 cm3 of aqueous silver(I) nitrate, concentration 0.2 mol / dm3?

number of moles of AgNO3 used = ..................... [1]

number of moles of Ag2CrO4 formed = ..................... [1]

mass of one mole of Ag2CrO4 = 332 g

mass of Ag2CrO4 formed = ..................... g [1]

[Total: 11]

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Use

6 The following reactivity series shows both familiar and unfamiliar elements in order of decreasing reactivity. Each element is represented by a redox equation.

Rb Rb+ + e–

Mg Mg2+ + 2e–

Mn Mn2+ + 2e–

Zn Zn2+ + 2e–

H2 2H+ + 2e–

Cu Cu2+ + 2e–

Hg Hg2+ + 2e–

Two of the uses of the series are to predict the thermal stability of compounds of the metals and to explain their redox reactions.

(a) Most metal hydroxides decompose when heated.

(i) Complete the equation for the thermal decomposition of copper(II) hydroxide.

Cu(OH)2 → ............... + ............... [1]

(ii) Choose a metal from the above series whose hydroxide does not decompose when heated.

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

(b) (i) Defi ne in terms of electron transfer the term oxidation.

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

(ii) Explain why the positive ions in the above equations are oxidising agents.

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

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

(c) (i) Which metals in the series above do not react with dilute acids to form hydrogen?

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

(ii) Describe an experiment which would confi rm the prediction made in (c)(i).

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

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

(d) (i) Which metal in the series above can form a negative ion which gives a pink / purple solution in water?

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

(ii) Describe what you would observe when zinc, a reducing agent, is added to this pink / purple solution.

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

[Total: 8]

11


ForExaminer’s

Use

7 Plants can make complex molecules from simple starting materials, such as water, carbon dioxide and nitrates. Substances produced by plants include sugars, more complex carbohydrates, esters, proteins, vegetable oils and fats.

(a) (i) Describe how you could decide from its molecular formula whether a compound is a carbohydrate.

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

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

(ii) Plants can change the sugar, glucose, into starch which is a more complex carbohydrate. What type of reaction is this?

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

(b) The fermentation of glucose can be carried out in the apparatus shown below. After a few days the reaction stops. A 12% aqueous solution of ethanol has been produced.

water allows carbondioxide to escape butprevents air from entering

aqueous glucoseand yeast

(i) The enzyme, zymase, catalyses the anaerobic respiration of the yeast. Explain the term respiration.

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

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

(ii) Complete the equation.

C6H12O6 → ......................... + ................................... [2] glucose ethanol carbon dioxide

(iii) Why must air be kept out of the fl ask?

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

12

0620/32/O/N/13© UCLES 2013

ForExaminer’s

Use

(c) The ester methyl butanoate is found in apples. It can be made from butanoic acid and methanol. Their structural formulae are given below.

C

H

H

C

O

O H

C

H

H

C

H

H

H HOC

H

H

H

butanoic acid methanol

Use the information given above to deduce the structural formula of methyl butanoate showing all the bonds.

[2]

(d) The equation represents the hydrolysis of a naturally occurring ester.

C17H35 CO2 CH2

C17H35 CO2 3C17H35COONa CHOHCH 3NaOH+ +→

C17H35 CO2 CH2

CH2OH

CH2OH

(i) Which substance in the equation is an alcohol? Put a ring around this substance in the equation above. [1]

(ii) Is the alkyl group, C17H35, in this ester saturated or unsaturated? Give a reason for your choice.

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

(iii) What type of compound is represented by the formula C17H35COONa? What is the major use for compounds of this type?

type of compound ......................................................................................................

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

13


ForExaminer’s

Use

(e) Proteins are natural macromolecules. Draw the structural formula of a typical protein. Include three monomer units. You may represent amino acids by formulae of the type drawn below.

H2N COOH H2N COOH

[3]

[Total: 18]

14

0620/32/O/N/13

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© UCLES 2013

15

0620/32/O/N/13

BLANK PAGE

© UCLES 2013

16



0620/32/O/N/13© UCLES 2013

Gro

up

140

Ce

Cer

ium

58

141

PrP

rase

odym

ium

59

144

Nd

Neo

dym

ium

60

PmP

rom

ethi

um61

150

SmS

amar

ium

62

152

EuE

urop

ium

63

157

Gd

Gad

olin

ium

64

159

Tb Terb

ium

65

162

Dy

Dys

pros

ium

66

165

Ho

Hol

miu

m67

167

Er Erb

ium

68

169

Tm Thul

ium

69

173

YbY

tterb

ium

70

175

LuLu

tetiu

m71

232

Th Thor

ium

90

PaP

rota

ctin

ium

91

238 U

Ura

nium

92

Np

Nep

tuni

um93

PuP

luto

nium

94

Am

Am

eric

ium

95

Cm

Cur

ium

96

Bk

Ber

keliu

m97

Cf

Cal

iforn

ium

98

EsE

inst

eini

um99

Fm Ferm

ium

100

Md

Men

dele

vium

101

No

Nob

eliu

m10

2

LrLa

wre

nciu

m10

3

1 HH

ydro

gen

1

7 LiLi

thiu

m3

23 Na

Sod

ium

11

24 Mg

Mag

nesi

um12

40 Ca

Cal

cium

20

45 ScS

cand

ium

21

48 TiTi

tani

um22

51 VVa

nadi

um23

52 Cr

Chr

omiu

m24

55 Mn

Man

gane

se25

56 Fe Iron

26

59 Co

Cob

alt

27

59 Ni

Nic

kel

28

64 Cu

Cop

per

29

65 Zn Zinc

30

70 Ga

Gal

lium

31

27 Al

Alu

min

ium

13

11 B Bor

on5

12 CC

arbo

n6

14 NN

itrog

en7

16 OO

xyge

n8

19 FFl

uorin

e9

28 Si Sili

con

14

31 PP

hosp

horu

s15

32 S Sul

fur

16

35.5 Cl

Chl

orin

e17

40 Ar

Arg

on18

20 Ne

Neo

n10

4 He

Hel

ium

2

73 Ge

Ger

man

ium

32

75 As

Ars

enic

33

79 SeS

elen

ium

34

80 Br

Bro

min

e35

84 Kr

Kry

pton

36

39 KP

otas

sium

19

88 SrS

tront

ium

38

89 YY

ttriu

m39

91 ZrZi

rcon

ium

40

93 Nb

Nio

bium

41

96 Mo

Mol

ybde

num

42

TcTe

chne

tium

43

101

Ru

Rut

heni

um44

103

Rh

Rho

dium

45

106

PdP

alla

dium

46

108

Ag

Silv

er47

112

Cd

Cad

miu

m48

115

In Indi

um49

119

Sn Tin

50

122

SbA

ntim

ony

51

128

TeTe

lluriu

m52

127 I

Iodi

ne53

131

Xe Xen

on54

137

Ba

Bar

ium

56

139

LaLa

ntha

num

57

*

178

Hf

Haf

nium

72

181

TaTa

ntal

um73

184 W

Tung

sten

74

186

Re

Rhe

nium

75

190

Os

Osm

ium

76

192

Ir Iridi

um77

195 Pt

Pla

tinum

78

197

Au

Gol

d79

201

Hg

Mer

cury

80

204 Tl

Thal

lium

81

207

Pb Lead

82

209 Bi

Bis

mut

h83

PoP

olon

ium

84

At

Ast

atin

e85

Rn

Rad

on86

FrFr

anci

um87

227

Ac

Act

iniu

m89

9 Be

Ber

ylliu

m4

III

IIIIV

VV

IV

II0

85 Rb

Rub

idiu

m37

133

Cs

Cae

sium

55

226

Ra

Rad

ium

88

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3

at ro

om te

mpe

ratu

re a

nd p

ress

ure

(r.t.p

.).

a Xb

a =

rela

tive

atom

ic m

ass

X =

atom

ic s

ymbo

l

b =

prot

on (a

tom

ic) n

umbe

r

Key

* 58-

71 L

anth

anoi

d se

ries

90-1

03 A

ctin

oid

serie

s

DAT

A SH

EET

The

Perio

dic

Tabl

e of

the

Elem

ents





CHEMISTRY 0620/33


1 hour 15 minutes




This document consists of 12 printed pages.


*1277729958*

2

0620/33/O/N/13© UCLES 2013

ForExaminer’s

Use

1 Zirconium (Zr) is a metal in Period 5. Its main oxidation state is +4.

(a) The following are all zirconium atoms: 90Zr40 , 91Zr40 and 92Zr40 .

In terms of numbers of electrons, neutrons and protons, how are these three atoms the same and how are they different?

They are the same because .............................................................................................

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

They are different because ...............................................................................................

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

(b) Containers for fuel rods in nuclear reactors are made of zirconium. Nuclear reactors are used to produce energy and to make radioactive isotopes.

(i) Which isotope of a different element is used as a fuel in nuclear reactors?

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

(ii) State one medical and one industrial use of radioactive isotopes.

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

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

(iii) Above 900 °C, zirconium reacts with water to form zirconium(IV) oxide, ZrO2, and hydrogen. Write an equation for this reaction.

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

(iv) In a nuclear accident, water may come in contact with very hot zirconium. Explain why the presence of hydrogen inside the reactor greatly increases the

danger of the accident.

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

(c) It is possible to determine whether zirconium(IV) oxide is acidic, neutral, basic or amphoteric using an acid and an alkali. Complete the table of possible results. If the oxide is predicted to react write ‘R’, if it is predicted not to react write ‘NR’.

if the oxide is predicted result withhydrochloric acid

predicted result with aqueoussodium hydroxide

acidic

neutral

basic

amphoteric

[4]

[Total: 13]

3


ForExaminer’s

Use

2 (a) The diagram shows the lattice of a typical ionic compound.

–

+

–

+

–

–

+

– +

+

–

+

– + – +

+

–

–

– +

+

+

–

(i) Explain the term ionic lattice.

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

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

(ii) In this lattice, the ratio of positive ions to negative ions is 1:1. In the lattice of a different ionic compound, the ratio of positive ions to negative ions

is 1:2. Suggest why this ratio varies in different ionic compounds.

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

(iii) Give three physical properties of ionic compounds.

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

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

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

(b) Strontium oxide is an ionic compound. Draw a diagram which shows its formula, the charges on the ions and the arrangement of the valency electrons around the negative ion.

The electron distribution of a strontium atom is 2 + 8 + 18 + 8 + 2.

Use o to represent an electron from a strontium atom. Use x to represent an electron from an oxygen atom.

[3]

[Total: 9]

4

0620/33/O/N/13© UCLES 2013

ForExaminer’s

Use

3 The main uses of zinc are preventing steel from rusting and making alloys.

(a) The main ore of zinc is zinc blende. Zinc blende consists mainly of zinc sulfi de, ZnS. There are two major methods of extracting zinc from its ore. They are the direct reduction of zinc oxide to zinc and by electrolysis. In both methods, zinc oxide is made from the zinc sulfi de in the ore.

(i) How is zinc oxide made from zinc sulfi de?

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

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

(ii) Write an equation for the reaction used to reduce zinc oxide to zinc.

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

(b) In the electrolytic method, zinc oxide reacts with sulfuric acid to form impure aqueous zinc sulfate. This solution contains Ni2+, Co2+ and Cu2+ ions as impurities.

(i) Write the equation for the reaction between zinc oxide and sulfuric acid.

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

(ii) Nickel, cobalt and copper are all less reactive than zinc. Explain why the addition of zinc powder removes these ions from the solution.

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

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

(c) The solution of zinc sulfate is electrolysed using inert electrodes. This electrolysis is similar to that of copper(II) sulfate with inert electrodes.

(i) Write the equation for the reaction at the negative electrode (cathode).

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

(ii) Complete the equation for the reaction at the positive electrode (anode).

.........OH– → 2H2O + ......... + .........e– [2]

(iii) The electrolyte changes from zinc sulfate to

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

5


ForExaminer’s

Use

(d) (i) Brass is an alloy of copper and zinc. Suggest two reasons why brass is often used in preference to copper.

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

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

(ii) Sacrifi cial protection is a method of rust prevention. Explain in terms of electron transfer why steel, which is in electrical contact with zinc, does not rust.

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

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

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

.............................................................................................................................. [4]

[Total: 15]

6

0620/33/O/N/13© UCLES 2013

ForExaminer’s

Use

4 Sulfuric acid is a strong acid. Hexanesulfonic acid is also a strong acid. It has similar properties to sulfuric acid.

(a) Sulfonic acids are made from alkanes and oleum, H2S2O7.

C6H14 + H2S2O7 → C6H13SO3H + H2SO4

(i) Describe how oleum is made from sulfur by the Contact process. Give equations and reaction conditions.

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

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

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

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

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

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

.............................................................................................................................. [6]

(ii) How is concentrated sulfuric acid made from oleum?

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

(b) The formula of the hexanesulfonate ion is C6H13SO3–.

The formula of the barium ion is Ba2+. What is the formula of barium hexanesulfonate?

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

(c) Complete the following equations.

(i) magnesium + hexanesulfonic → ............................. + ......................... acid ............................. [1]

(ii) calcium + hexanesulfonic → ............................. + ......................... oxide acid ............................. [1]

(iii) .....C6H13SO3H + Na2CO3 → ............................. + ............ + ............ [2]

7


ForExaminer’s

Use

(d) (i) Sulfuric acid is a strong acid. You are given aqueous sulfuric acid, concentration 0.1 mol / dm3, and aqueous

hexanesulfonic acid, concentration 0.2 mol / dm3. Describe how you could show that hexanesulfonic acid is also a strong acid.

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

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

(ii) Deduce why, for a fair comparison, the two acid solutions must have different concentrations.

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

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

(iii) Explain the terms strong acid and weak acid.

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

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

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

[Total: 17]

8

0620/33/O/N/13© UCLES 2013

ForExaminer’s

Use

5 Domestic rubbish is disposed of in landfi ll sites. Rubbish could include the following items.

item of rubbish approximate time foritem to break down

newspaper one month

cotton rag six months

woollen glove one year

aluminium container up to 500 years

styrofoam cup 1000 years

(a) Explain why aluminium, a reactive metal, takes so long to corrode.

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

(b) Both paper and cotton are complex carbohydrates. They can be hydrolysed to simple sugars such as glucose.

The formula of glucose can be represented as:

HO OH

Draw the structural formula of a complex carbohydrate, such as cotton. Include at least two glucose units.

[2]

9


ForExaminer’s

Use

(c) Wool is a protein. It can be hydrolysed to a mixture of monomers by enzymes.

(i) What are enzymes?

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

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

(ii) Name another substance which can hydrolyse proteins.

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

(iii) What type of compound are the monomers formed by the hydrolysis of proteins?

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

(iv) Which technique could be used to identify the individual monomers in the mixture?

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

(v) Proteins contain the amide linkage. Name a synthetic macromolecule which contains the same linkage.

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

(d) (i) What is the scientifi c term used to describe polymers which do not break down in landfi ll sites?

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

(ii) Styrofoam is poly(phenylethene). It is an addition polymer. Its structural formula is given below. Deduce the structural formula of the monomer, phenylethene.

n

CH2 CH

C6H5

[1]

[Total: 11]

10

0620/33/O/N/13© UCLES 2013

ForExaminer’s

Use

6 The alcohols form a homologous series. The fi rst fi ve members are given in the table below.

(a)

alcohol formula heat of combustionin kJ / mol

methanol CH3OH 730

ethanol CH3–CH2–OH 1380

propan-1-ol

butan-1-ol CH3–CH2–CH2–CH2–OH 2680

pentan-1-ol CH3–CH2–CH2–CH2–CH2–OH 3350

(i) Complete the table. [2]

(ii) Complete the equation for the combustion of pentan-1-ol in excess oxygen.

C5H11OH + .......O2 → ..................... + ..................... [1]

(b) State three characteristics of a homologous series other than the variation of physical properties down the series.

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

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

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

(c) The following alcohols are isomers.

CH3–CH2–CH2–CH2–OH and (CH3)2CH–CH2–OH

(i) Explain why they are isomers.

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

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

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

(ii) Draw the structural formula of another isomer of the above alcohols.

[1]

11


ForExaminer’s

Use

(d) Alcohols can be made by fermentation and from petroleum.

(i) Ethanol is made from sugars by fermentation.

C6H12O6 → 2C2H5OH + 2CO2

The mass of one mole of glucose, C6H12O6, is 180 g. Calculate the maximum mass of ethanol which could be obtained from 72 g of

glucose.

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

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

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

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

(ii) Describe how ethanol is made from petroleum.

petroleum (alkanes) → ethene → ethanol

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

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

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

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

[Total: 15]

12



0620/33/O/N/13© UCLES 2013

Gro

up

140

Ce

Cer

ium

58

141

PrP

rase

odym

ium

59

144

Nd

Neo

dym

ium

60

PmP

rom

ethi

um61

150

SmS

amar

ium

62

152

EuE

urop

ium

63

157

Gd

Gad

olin

ium

64

159

Tb Terb

ium

65

162

Dy

Dys

pros

ium

66

165

Ho

Hol

miu

m67

167

Er Erb

ium

68

169

Tm Thul

ium

69

173

YbY

tterb

ium

70

175

LuLu

tetiu

m71

232

Th Thor

ium

90

PaP

rota

ctin

ium

91

238 U

Ura

nium

92

Np

Nep

tuni

um93

PuP

luto

nium

94

Am

Am

eric

ium

95

Cm

Cur

ium

96

Bk

Ber

keliu

m97

Cf

Cal

iforn

ium

98

EsE

inst

eini

um99

Fm Ferm

ium

100

Md

Men

dele

vium

101

No

Nob

eliu

m10

2

LrLa

wre

nciu

m10

3

1 HH

ydro

gen

1

7 LiLi

thiu

m3

23 Na

Sod

ium

11

24 Mg

Mag

nesi

um12

40 Ca

Cal

cium

20

45 ScS

cand

ium

21

48 TiTi

tani

um22

51 VVa

nadi

um23

52 Cr

Chr

omiu

m24

55 Mn

Man

gane

se25

56 Fe Iron

26

59 Co

Cob

alt

27

59 Ni

Nic

kel

28

64 Cu

Cop

per

29

65 Zn Zinc

30

70 Ga

Gal

lium

31

27 Al

Alu

min

ium

13

11 B Bor

on5

12 CC

arbo

n6

14 NN

itrog

en7

16 OO

xyge

n8

19 FFl

uorin

e9

28 Si Sili

con

14

31 PP

hosp

horu

s15

32 S Sul

fur

16

35.5 Cl

Chl

orin

e17

40 Ar

Arg

on18

20 Ne

Neo

n10

4 He

Hel

ium

2

73 Ge

Ger

man

ium

32

75 As

Ars

enic

33

79 SeS

elen

ium

34

80 Br

Bro

min

e35

84 Kr

Kry

pton

36

39 KP

otas

sium

19

88 SrS

tront

ium

38

89 YY

ttriu

m39

91 ZrZi

rcon

ium

40

93 Nb

Nio

bium

41

96 Mo

Mol

ybde

num

42

TcTe

chne

tium

43

101

Ru

Rut

heni

um44

103

Rh

Rho

dium

45

106

PdP

alla

dium

46

108

Ag

Silv

er47

112

Cd

Cad

miu

m48

115

In Indi

um49

119

Sn Tin

50

122

SbA

ntim

ony

51

128

TeTe

lluriu

m52

127 I

Iodi

ne53

131

Xe Xen

on54

137

Ba

Bar

ium

56

139

LaLa

ntha

num

57

*

178

Hf

Haf

nium

72

181

TaTa

ntal

um73

184 W

Tung

sten

74

186

Re

Rhe

nium

75

190

Os

Osm

ium

76

192

Ir Iridi

um77

195 Pt

Pla

tinum

78

197

Au

Gol

d79

201

Hg

Mer

cury

80

204 Tl

Thal

lium

81

207

Pb Lead

82

209 Bi

Bis

mut

h83

PoP

olon

ium

84

At

Ast

atin

e85

Rn

Rad

on86

FrFr

anci

um87

227

Ac

Act

iniu

m89

9 Be

Ber

ylliu

m4

III

IIIIV

VV

IV

II0

85 Rb

Rub

idiu

m37

133

Cs

Cae

sium

55

226

Ra

Rad

ium

88

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3

at ro

om te

mpe

ratu

re a

nd p

ress

ure

(r.t.p

.).

a Xb

a =

rela

tive

atom

ic m

ass

X =

atom

ic s

ymbo

l

b =

prot

on (a

tom

ic) n

umbe

r

Key

* 58-

71 L

anth

anoi

d se

ries

90-1

03 A

ctin

oid

serie

s

DAT

A SH

EET

The

Perio

dic

Tabl

e of

the

Elem

ents



Answer all questions.Electronic calculators may be used.Practical notes are provided on page 8.You may lose marks if you do not show your working or if you do not use appropriate units.


CHEMISTRY 0620/51

Paper 5 Practical Test October/November 2013

1 hour 15 minutes


Additional Materials: As listed in the Confi dential Instructions




*1146292889*

For Examiner’s Use

Total

2

0620/51/O/N/13© UCLES 2013

ForExaminer’s

Use

1 You are going to investigate what happens when aqueous sodium hydroxide reacts with acid K.

Read all the instructions below carefully before starting the experiments.

Instructions You are going to carry out two experiments.

(a) Experiment 1

Use a measuring cylinder to pour 25 cm3 of acid K into a conical fl ask. Add fi ve drops of phenolphthalein to the fl ask.

Fill the burette with the aqueous sodium hydroxide to the 0.0 cm3 mark. Slowly add the aqueous sodium hydroxide to acid K in the fl ask and shake the mixture. Continue to add aqueous sodium hydroxide to the fl ask until the solution shows a

permanent colour change. Measure and record the volume in the table. Complete the table. Pour the solution away and rinse the conical fl ask.

burette reading

fi nal volume / cm3

initial volume / cm3

difference / cm3

[3]

(b) Experiment 2

Use a measuring cylinder to pour 50 cm3 of acid K into a conical fl ask. Add the 0.3 g of powdered calcium carbonate to the fl ask and shake the fl ask until no further reaction is observed.

Add fi ve drops of phenolphthalein to the mixture in the fl ask.

Fill the burette with aqueous sodium hydroxide and record the burette reading. Slowly add aqueous sodium hydroxide from the burette to the fl ask and shake the mixture. Continue to add aqueous sodium hydroxide to the fl ask until the solution shows a permanent colour change.

Measure and record the volume in the table. Complete the table.

burette reading

fi nal volume / cm3


difference / cm3

[3]

3


ForExaminer’s

Use

(c) What colour change was observed after the sodium hydroxide solution was added to the fl ask?

from ............................................................ to ............................................................ [2]

(d) What type of chemical reaction occurs when acid K reacts with sodium hydroxide?

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

(e) If Experiment 1 was repeated using 50 cm3 of acid K, what volume of sodium hydroxide would be required to change the colour of the indicator?

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

(f) (i) What is the effect of adding 0.3 g of powdered calcium carbonate to acid K?

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

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

(ii) Use your answers from (b) and (e) to work out the difference in the volume of sodium hydroxide added when 0.3 g of calcium carbonate is mixed with 50 cm3 of acid K in Experiment 2.

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

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

(iii) Estimate the mass of calcium carbonate that would need to be added to 50 cm3 of acid K to require 0.0 cm3 of sodium hydroxide.

[1]

(g) What would be the effect on the results if the solutions of acid K were warmed before adding the sodium hydroxide? Give a reason for your answer.

effect on results ................................................................................................................

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

4

0620/51/O/N/13© UCLES 2013

ForExaminer’s

Use

(h) Suggest the advantage, if any, of

(i) using a pipette to measure the volume of acid K.

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

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

(ii) using a polystyrene cup instead of a fl ask.

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

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

[Total: 22]

5


ForExaminer’s

Use

2 You are provided with two liquids, L and M. Carry out the following tests on L and M, recording all of your observations in the table. Conclusions must not be written in the table.

tests observationstests on liquid L

(a) Describe the appearance of liquid L. ................................................................ [1]

Divide liquid L into fi ve equal portions in separate test-tubes.

(b) (i) Add the fi rst portion of liquid L to the test-tube containing the iodine crystal. Stopper the test-tube and shake the contents.

Now add an equal volume of liquid M to the test-tube, stopper and shake the contents. Leave to stand for fi ve minutes and continue to part (c).

(ii) After fi ve minutes, remove most of the top layer using a teat pipette and add ethanol to the liquid which you have removed. Stopper the test-tube and shake the contents. Leave to stand for fi ve minutes.

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

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

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

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

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

(c) To the second portion of liquid L, add a few drops of dilute nitric acid and about 1 cm3 of barium nitrate solution. ................................................................ [1]

(d) To the third portion of liquid L, add a few drops of dilute nitric acid and about 1 cm3 of silver nitrate solution. ................................................................ [2]

(e) To the fourth portion of liquid L, add about 1 cm3 of aqueous copper sulfate, shake and leave to stand for fi ve minutes.

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

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

(f) To the fi fth portion of liquid L, add about 2 cm3 of aqueous hydrogen peroxide.

Now add about 1 cm3 of starch solution.

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

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

6

0620/51/O/N/13© UCLES 2013

ForExaminer’s

Use

(g) Why does the colour of liquid L change in test (b)(i)?

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

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

(h) What conclusions can you draw about liquid M from test (b)(i)?

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

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

(i) What conclusions can you draw about liquid L?

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

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

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

[Total: 18]

8



0620/51/O/N/13

NOTES FOR USE IN QUALITATIVE ANALYSIS

Test for anions

anion test test result

carbonate (CO32–) add dilute acid effervescence, carbon dioxide

produced

chloride (Cl –)[in solution]

acidify with dilute nitric acid, thenadd aqueous silver nitrate

white ppt.

iodide (I–)[in solution]


yellow ppt.

nitrate (NO3–)

[in solution]add aqueous sodium hydroxidethen aluminium foil; warm carefully

ammonia produced

sulfate (SO42–)

[in solution]acidify with dilute nitric acid, thenaqueous barium nitrate

white ppt.

Test for aqueous cations

cation effect of aqueous sodium hydroxide effect of aqueous ammonia

aluminium (Al 3+) white ppt., soluble in excess givinga colourless solution

white ppt., insoluble in excess

ammonium (NH4+) ammonia produced on warming –

calcium (Ca2+) white ppt., insoluble in excess no ppt., or very slight white ppt.

copper (Cu2+) light blue ppt., insoluble in excess light blue ppt., soluble in excessgiving a dark blue solution

iron(II) (Fe2+) green ppt., insoluble in excess green ppt., insoluble in excess

iron(III) (Fe3+) red-brown ppt., insoluble in excess red-brown ppt., insoluble in excess

zinc (Zn2+) white ppt., soluble in excess givinga colourless solution

white ppt., soluble in excess givinga colourless solution

Test for gases

gas test and test results

ammonia (NH3) turns damp red litmus paper blue

carbon dioxide (CO2) turns limewater milky

chlorine (Cl 2) bleaches damp litmus paper

hydrogen (H2) ‘pops’ with a lighted splint

oxygen (O2) relights a glowing splint

© UCLES 2013

2

0620/52/O/N/13© UCLES 2013

ForExaminer’s

Use

1 You are going to investigate what happens when aqueous sodium hydroxide reacts with acid K.


Instructions You are going to carry out two experiments.

(a) Experiment 1

Use a measuring cylinder to pour 25 cm3 of acid K into a conical fl ask. Add fi ve drops of phenolphthalein to the fl ask.

Fill the burette with the aqueous sodium hydroxide to the 0.0 cm3 mark. Slowly add the aqueous sodium hydroxide to acid K in the fl ask and shake the mixture. Continue to add aqueous sodium hydroxide to the fl ask until the solution shows a

permanent colour change. Measure and record the volume in the table. Complete the table. Pour the solution away and rinse the conical fl ask.

burette reading

fi nal volume / cm3


difference / cm3

[3]

(b) Experiment 2

Use a measuring cylinder to pour 50 cm3 of acid K into a conical fl ask. Add the 0.3 g of powdered calcium carbonate to the fl ask and shake the fl ask until no further reaction is observed.

Add fi ve drops of phenolphthalein to the mixture in the fl ask.

Fill the burette with aqueous sodium hydroxide and record the burette reading. Slowly add aqueous sodium hydroxide from the burette to the fl ask and shake the mixture. Continue to add aqueous sodium hydroxide to the fl ask until the solution shows a permanent colour change.

Measure and record the volume in the table. Complete the table.

burette reading

fi nal volume / cm3


difference / cm3

[3]

3


ForExaminer’s

Use


from ............................................................ to ............................................................ [2]

(d) What type of chemical reaction occurs when acid K reacts with sodium hydroxide?

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

(e) If Experiment 1 was repeated using 50 cm3 of acid K, what volume of sodium hydroxide would be required to change the colour of the indicator?

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

(f) (i) What is the effect of adding 0.3 g of powdered calcium carbonate to acid K?

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

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

(ii) Use your answers from (b) and (e) to work out the difference in the volume of sodium hydroxide added when 0.3 g of calcium carbonate is mixed with 50 cm3 of acid K in Experiment 2.

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

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

(iii) Estimate the mass of calcium carbonate that would need to be added to 50 cm3 of acid K to require 0.0 cm3 of sodium hydroxide.

[1]



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

4

0620/52/O/N/13© UCLES 2013

ForExaminer’s

Use



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

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


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

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

[Total: 22]

5


ForExaminer’s

Use

2 You are provided with two liquids, L and M. Carry out the following tests on L and M, recording all of your observations in the table. Conclusions must not be written in the table.

tests observationstests on liquid L

(a) Describe the appearance of liquid L. ................................................................ [1]

Divide liquid L into fi ve equal portions in separate test-tubes.

(b) (i) Add the fi rst portion of liquid L to the test-tube containing the iodine crystal. Stopper the test-tube and shake the contents.

Now add an equal volume of liquid M to the test-tube, stopper and shake the contents. Leave to stand for fi ve minutes and continue to part (c).

(ii) After fi ve minutes, remove most of the top layer using a teat pipette and add ethanol to the liquid which you have removed. Stopper the test-tube and shake the contents. Leave to stand for fi ve minutes.

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

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

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

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

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

(c) To the second portion of liquid L, add a few drops of dilute nitric acid and about 1 cm3 of barium nitrate solution. ................................................................ [1]

(d) To the third portion of liquid L, add a few drops of dilute nitric acid and about 1 cm3 of silver nitrate solution. ................................................................ [2]

(e) To the fourth portion of liquid L, add about 1 cm3 of aqueous copper sulfate, shake and leave to stand for fi ve minutes.

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

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

(f) To the fi fth portion of liquid L, add about 2 cm3 of aqueous hydrogen peroxide.

Now add about 1 cm3 of starch solution.

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

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

6

0620/52/O/N/13© UCLES 2013

ForExaminer’s

Use

(g) Why does the colour of liquid L change in test (b)(i)?

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

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

(h) What conclusions can you draw about liquid M from test (b)(i)?

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

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

(i) What conclusions can you draw about liquid L?

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

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

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

[Total: 18]

8



0620/52/O/N/13


Test for anions



produced



white ppt.



yellow ppt.

nitrate (NO3–)


ammonia produced

sulfate (SO42–)


white ppt.












Test for gases







© UCLES 2013





CHEMISTRY 0620/53


1 hour 15 minutes






*7606081731*


Total

2

0620/53/O/N/13© UCLES 2013

ForExaminer’s

Use

1 You are going to investigate the reaction between aqueous potassium manganate(VII), solution C, and two different acidic solutions, D and E.


Instructions You are going to carry out three experiments.

(a) Experiment 1

Fill the burette with the solution C of potassium manganate(VII) to the 0.0 cm3 mark. Using a measuring cylinder, pour 25 cm3 of solution D into the conical fl ask.

Add 1.0 cm3 of the solution C to the fl ask, with shaking. Continue to add solution C to the fl ask until the mixture just turns permanently pink. Record the burette reading in the table and complete the table.

Pour away the contents of the conical fl ask and rinse the fl ask with distilled water.

burette reading

fi nal burette reading / cm3

initial burette reading / cm3

difference / cm3

[3]

(b) Experiment 2

Repeat Experiment 1 using 25 cm3 of solution E instead of solution D. Record the burette readings in the table and complete the table.

burette reading



difference / cm3

[3]

(c) Experiment 3

To about 2 cm3 of solution E in a test-tube, add an equal volume of aqueous ammonia. Shake the test-tube and note any observations. Leave the mixture to stand for 5 minutes and note any changes.

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

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

3


ForExaminer’s

Use

(d) (i) What colour change was observed as potassium manganate(VII) solution was added to the fl ask in Experiment 1?

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

(ii) Why is an indicator not added to the fl ask?

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

(e) (i) In which experiment was the greatest volume of potassium manganate(VII) solution used?

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

(ii) Compare the volumes of potassium manganate(VII) used in Experiments 1 and 2.

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

(iii) Suggest an explanation for the difference in volumes.

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

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

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

(f) If Experiment 2 was repeated using 12.5 cm3 of solution E, what volume of potassium manganate(VII) solution would be used? Explain your answer.

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

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

(g) Give one advantage and one disadvantage of using a measuring cylinder for solutions D and E.

advantage .........................................................................................................................

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

(h) Explain your observations in Experiment 3.

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

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

[Total: 21]

4

0620/53/O/N/13© UCLES 2013

ForExaminer’s

Use

2 You are provided with liquid F. Carry out the following tests on the liquid, recording all of your observations in the table. Conclusions must not be written in the table.

tests observations

Divide liquid F into fi ve equal portions in separate test-tubes.

(a) Describe the appearance of liquid F.

Test the pH of the liquid.

To the fi rst portion of liquid F, add an equal volume of dilute sulfuric acid.

Now add excess aqueous sodium hydroxide and shake the mixture.

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

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

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

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

(b) To the second portion of liquid F, add an equal volume of dilute sulfuric acid followed by about 2 cm3 of hydrogen peroxide.

Shake the mixture and test the gas given off with a splint.

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

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

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

(c) To the third portion of liquid F, add aqueous silver nitrate followed by excess dilute nitric acid. Shake the mixture.

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

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

(d) To the fourth portion of liquid F, add aqueous barium nitrate followed by excess dilute nitric acid. Shake the mixture.

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

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

(e) To the fi fth portion of liquid F, add an equal volume of sulfuric acid and one spatula measure of iron fi lings.

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

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

5


ForExaminer’s

Use

(f) What type of reaction happened in test (a)? Explain your answer.

type of reaction .................................................................................................................

explanation .......................................................................................................................

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

(g) Identify the gas given off in test (b).

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

(h) Draw one conclusion about liquid F.

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

[Total: 19]

8



0620/53/O/N/13


Test for anions



produced



white ppt.



yellow ppt.

nitrate (NO3–)


ammonia produced

sulfate (SO42–)


white ppt.












Test for gases







© UCLES 2013



Answer all questions.Electronic calculators may be used.You may lose marks if you do not show your working or if you do not use appropriate units.


CHEMISTRY 0620/61

Paper 6 Alternative to Practical October/November 2013

1 hour






*8106479956*

2

0620/61/O/N/13© UCLES 2013

ForExaminer’s

Use

1 A student investigated the products formed when ethanol was burned using the apparatus shown.

suctionpump

liquid F

(a) Complete the box to identify the piece of apparatus. [1]

(b) Why is a suction pump used?

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

(c) (i) Suggest the purpose and identity of liquid F.

identity .......................................................................................................................

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

(ii) Why is the end of the delivery tube below the surface of liquid F?

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

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

(d) Give one expected observation in the horizontal part of the delivery tube. Explain your answer.

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

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

[Total: 7]

3


ForExaminer’s

Use

2 Eight steel rods of the same size were placed in solutions of different pH for one week. The percentage corrosion of the rods was measured and the results plotted on the grid below.

30

20

10

0

perc

enta

ge c

orro

sion

of s

teel

rod

0 1 2 3 4pH of solution

5 6 7 8

(a) Draw a best fi t straight line through the points. [1]

(b) Why were the steel rods the same size?

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

(c) State one other variable which should have been kept constant.

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

(d) State one conclusion that could be drawn from the results.

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

(e) Determine the percentage corrosion of a steel rod in a solution of pH 6.5.

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

[Total: 5]

4

0620/61/O/N/13© UCLES 2013

ForExaminer’s

Use

3 A student investigated the reaction between aqueous sodium hydroxide and acid K. Two experiments were carried out.

(a) Experiment 1

Using a measuring cylinder, 25 cm3 of acid K was poured into a conical fl ask. Phenolphthalein indicator was added to the fl ask. A burette was fi lled with aqueous sodium hydroxide to the 0.0 cm3 mark. Aqueous sodium hydroxide was added from the burette to the fl ask and the mixture shaken until the solution showed a permanent colour change.

The fi nal volume was measured. Use the burette diagram to record the fi nal volume in the table and complete the table.

37

38

39

final volume

burette reading

final volume / cm3


difference / cm3

[2]

(b) Experiment 2

The solution was poured away and the conical fl ask rinsed. Using a measuring cylinder, 50 cm3 of acid K was poured into the conical fl ask. 0.3 g of

powdered calcium carbonate was added to the fl ask and the fl ask shaken until no further reaction was observed.

Phenolphthalein was added to the mixture in the fl ask. A burette was fi lled with the same aqueous sodium hydroxide and the initial volume

measured. Aqueous sodium hydroxide was added from the burette to the fl ask and the mixture shaken until the solution showed a permanent colour change.

Use the burette diagrams to record the initial and fi nal volumes in the table and complete the table.

initial volume final volume

28

29

30

9

10

11

burette reading

final volume / cm3


difference / cm3

[2]

5


ForExaminer’s

Use


from ............................................................ to ............................................................ [2]

(d) What type of chemical reaction occurred when acid K reacted with sodium hydroxide?

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

(e) If Experiment 1 were repeated using 50 cm3 of acid K, what volume of sodium hydroxide would be required to change the colour of the indicator?

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

(f) (i) What were the effects of adding 0.3 g of powdered calcium carbonate to acid K?

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

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

(ii) Use your answer in (e) to work out the difference between the volume of sodium hydroxide needed to completely react with 50 cm3 of acid K and the volume of sodium hydroxide used in Experiment 2.

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

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

(iii) Estimate the mass of calcium carbonate that would be needed to be added to 50 cm3 of acid K to require 0.0 cm3 of sodium hydroxide.

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



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

6

0620/61/O/N/13© UCLES 2013

ForExaminer’s

Use



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

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


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

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

[Total: 20]

7


ForExaminer’s

Use

4 Two liquids, L and M, were analysed. L was aqueous potassium iodide. M was a colourless liquid.

The tests on the liquids and some of the observations are in the following table. Complete the observations in the table.

tests observations

tests on liquid L

(a) Appearance of liquid L. ............................................................ [1]

Liquid L was divided into three equal portions in separate test-tubes.

(b) (i) An iodine crystal was added to the fi rst portion of liquid L. The test-tube was stoppered and the contents shaken.

(ii) An equal volume of liquid M was added to the test-tube, the contents shaken and left to stand for fi ve minutes.

liquid turned orange

two layers were formed,pink top layer and orange lower layer

(c) To the second portion of liquid L, dilute nitric acid and barium nitrate solution were added. ............................................................ [1]

(d) To the third portion of liquid L, dilute nitric acid and silver nitrate solution were added. ............................................................ [2]

(e) Why does the colour of liquid L change in test (b)(i)?

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

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

(f) What conclusions can you draw about liquid M from test (b)(ii)?

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

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

[Total: 7]

8

0620/61/O/N/13© UCLES 2013

ForExaminer’s

Use

5 Two experiments using catalysts were carried out. Catalysts R and S were used to break down 50 cm3 of aqueous hydrogen peroxide at a temperature of 20 °C. The volume of oxygen given off was measured using the apparatus shown.

aqueoushydrogen peroxide

catalyst

gas syringe

The gas syringe diagrams show the volume of oxygen formed every 30 seconds in each experiment.

(a) Use the syringe diagrams to complete the volumes in the table.

time / s syringe diagram

using catalyst R using catalyst S

volume / cm3 syringe diagram volume / cm3

0 100

20 30 40

30 40 50

50 60 70

60 70 80

60 70 80

60 70 80

0 10

10 20 30

30 40 50

50 60 70

60 70 80

60 70 80

60 70 80

30

60

90

120

150

180

[4]

9


ForExaminer’s

Use

(b) Plot a graph to show each set of results. Clearly label the graphs R and S.

80

70

60

50

40

30

20

10

0

volume ofoxygen / cm3

0 30 60 90 120time / s

150 180

[6]

(c) Which result using catalyst R was inaccurate?

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

(d) Which is the better catalyst in this reaction? Explain your answer.

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

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

(e) Sketch a line on the grid to show the graph you would expect if the reaction with catalyst R was repeated at 50 °C. [2]

[Total: 15]

10

0620/61/O/N/13© UCLES 2013

ForExaminer’s

Use

6Old documents

Some documents are stored in containers with packets of silica gel crystals. These crystals absorb water from air that enters the container. Water could damage the documents.

Anhydrous cobalt(II) chloride is added to the silica gel. As the crystals absorb water they change colour from blue to pink. Heating the silica gel in an oven removes the water from the crystals so that the crystals can be reused.

Plan an experiment to fi nd the mass of water absorbed by a packet of silica gel crystals.

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

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

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

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

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

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

............................................................................................................................................ [6]

[Total: 6]





CHEMISTRY 0620/62


1 hour




This document consists of 12 printed pages.


*4045280680*

2

0620/62/O/N/13© UCLES 2013

ForExaminer’s

Use

1 Alkenes can be made by cracking long chain alkanes. A student used the apparatus below to demonstrate cracking.

broken tileliquid alkane

on mineral wool

very strongheat

water

(a) Complete the box to show the apparatus used. [1]

(b) Indicate with an arrow where the alkenes are collected. [1]

(c) Suggest the purpose of the mineral wool.

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

(d) Why are small pieces of broken tile used?

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

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

(e) Describe a test to show that alkenes have been made.

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

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

[Total: 6]

3


ForExaminer’s

Use

2 Substance M is a mixture of four dyes. Three of the dyes have different solubilities in propanone. The fourth dye is insoluble in propanone.

(a) Name the process that could be used to separate these dyes.

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

(b) Sketch on the right hand diagram the results you would expect if M was analysed as shown.

base-line

propanoneat the beginning at the end

M

[2]

(c) Why is the base-line not drawn in ink?

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

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

(d) Why must the level of the propanone be below the base-line?

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

[Total: 5]

4

0620/62/O/N/13© UCLES 2013

ForExaminer’s

Use

3 A student investigated the formation of calcium oxide by heating calcium in air, using the apparatus shown.

heat

crucible

She weighed an empty crucible and its lid. She then added some calcium to the crucible and reweighed it.

(a) Use the balance diagrams to record the masses in the table.

balance diagram mass / g

mass of crucible and lid

32

31

mass of crucible, lid and calcium

32

31

[1]

The student then heated the calcium in the crucible for ten minutes. The lid was raised occasionally using a pair of tongs. After ten minutes, the crucible was allowed to cool and reweighed. This procedure was repeated twice.

(b) Use the balance diagrams to complete the table of results.

time / min 10 20 30

balance diagram

32

31

33

32

33

32

mass of crucible, lid and calcium oxide / g

[2]

5


ForExaminer’s

Use

(c) Why was the lid of the crucible raised occasionally?

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

(d) Explain why the crucible was heated three times.

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

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

The table shows the results of experiments using different masses of calcium.

experiment mass ofcalcium / g

mass ofcalcium oxide / g

mass ofoxygen reacted / g

1 0.12 0.20 0.08

2 0.20 0.32 0.12

3 0.30 0.49 0.19

4 0.40 0.61

5 0.44 0.72

6 0.48 0.79

7 0.56 0.92

(e) Complete the table of results. [1]

(f) Plot the results on the grid and draw a straight line graph.

0.5

0.4

0.3

0.2

0.1

0.00.0 0.1 0.2 0.3 0.4

mass of calcium / g0.5 0.6 0.7

mas

s of

oxy

gen

reac

ted

/ g

[5]

6

0620/62/O/N/13© UCLES 2013

ForExaminer’s

Use

(g) Which result is inaccurate?

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

(h) Use your graph to work out the mass of calcium oxide formed when 0.7 g of calcium is heated in air. Show clearly on the grid how you used your graph.

[3]

[Total: 16]

7


ForExaminer’s

Use

4 A student investigated what happened when dilute hydrochloric acid and aqueous copper(II) sulfate solution reacted with different metals.

Five experiments were carried out.

(a) Experiment 1

Using a measuring cylinder 10 cm3 of dilute hydrochloric acid was poured into a boiling tube. The temperature of the solution was measured.

1 g of zinc powder was added to the boiling tube and the mixture stirred with the thermometer. The maximum temperature of the mixture was measured.

(b) Experiment 2

Experiment 1 was repeated using 1 g of iron powder instead of zinc. The initial and maximum temperatures were measured.

(c) Experiment 3

Experiment 1 was repeated using 1 g of magnesium powder instead of zinc. The initial and maximum temperatures were measured.

Use the thermometer diagrams to record the temperatures in the table. Complete the table.

experiment thermometer diagram

initialtemperature / °C

thermometer diagram

maximumtemperature / °C

temperaturerise / °C

1

30

25

20

30

25

20

2

30

25

20

30

25

20

3

30

25

20

80

75

70

[3] (d) Experiment 4

Using a measuring cylinder, 10 cm3 of aqueous copper sulfate was poured into a boiling tube. The temperature of the solution was measured.

1 g of magnesium powder was added to the boiling tube and the mixture stirred with the thermometer.

The gas was tested with a lighted splint and a loud pop was observed. The maximum temperature of the mixture was measured.

8

0620/62/O/N/13© UCLES 2013

ForExaminer’s

Use

(e) Experiment 5

Experiment 4 was repeated using 1 g of iron powder instead of magnesium. A red-brown solid was formed.

Use the thermometer diagrams to record the temperatures in the table. Complete the table.

experiment thermometer diagram

initialtemperature / °C

thermometer diagram

maximumtemperature / °C


4

5

[3]

(f) Draw a labelled bar chart for the results of Experiments 1, 2, 3, 4 and 5 on the grid below.


[5]

9


ForExaminer’s

Use

Use the results and observations to answer the following questions.

(g) (i) Which Experiment produced the largest temperature rise?

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

(ii) Suggest why this Experiment produced the largest temperature rise.

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

(h) Name the gas given off in Experiment 4.

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

(i) (i) Identify the red-brown solid formed in Experiment 5.

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

(ii) What type of chemical reaction occurs when iron reacts with aqueous copper(II) sulfate in Experiment 5?

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

(j) Predict the effect on the temperature change if 1 g of magnesium ribbon was used in Experiment 3. Explain your answer.

effect .................................................................................................................................

explanation .......................................................................................................................

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

(k) Suggest why potassium was not used as one of the metals in these experiments.

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

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

[Total: 19]

10

0620/62/O/N/13© UCLES 2013

ForExaminer’s

Use

5 Two different liquids, A and B, were analysed. A was an aqueous solution of ethanoic acid and B was a pure liquid. The tests on the liquids and some of the observations are in the following table. Complete the observations in the table.

tests observations

tests on liquid A

Liquid A was divided into three equal portions in separate test-tubes.

(a) Colour and smell of liquid A.

The liquid was added to Universal Indicator.

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

colour changed from green to ......................

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

(b) A piece of magnesium ribbon was added to the second portion of liquid A.

The gas given off was tested with a splint.

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

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

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

(c) Calcium carbonate was added to the third portion of liquid A. ................................................................ [1]

11


ForExaminer’s

Usetests observations

tests on liquid B

(d) Dilute sulfuric acid was added to liquid B followed by aqueous potassium manganate(VII). The mixture was heated.

changed colour from purple to colourless

(e) Liquid B was poured onto a dry watch glass. The surface of the liquid was touched with a lighted splint.

liquid burned with a yellow / blue fl ame

(f) What conclusions can you draw about liquid B?

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

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

[Total: 9]

12



0620/62/O/N/13© UCLES 2013

ForExaminer’s

Use

6Hair bleach

A solution of hydrogen peroxide can be used to bleach hair. Hairdressers buy ‘20 volume’ hydrogen peroxide. One volume of this solution breaks down to form 20 volumes of oxygen. For example 10 cm3 of 20 volume hydrogen peroxide will break down to produce 200 cm3 of oxygen.

Old solutions of hydrogen peroxide will produce less oxygen than expected.

Plan an experiment to fi nd out which of two solutions of hydrogen peroxide, H and J, is new and which is old. You are provided with common laboratory apparatus and the catalyst manganese(IV) oxide which speeds up the break down of hydrogen peroxide.

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

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

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

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

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

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

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

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

............................................................................................................................................ [5]

[Total: 5]

2

0620/63/O/N/13© UCLES 2013

ForExaminer’s

Use

1 A student tried to separate a mixture of salt and sand. Salt, sodium chloride, is soluble in water. Sand, silicon(IV) oxide, is insoluble in water. He added the mixture to water. Three sets of apparatus are shown.

A B C

(a) Complete the boxes to identify the pieces of apparatus. [2]

(b) Fill in the blanks in the following sentences.

Liquids that dissolve substances are called ........................ .

The clear liquid formed is a ................................. . [2]

(c) Which set of apparatus should be used to obtain

the sand, ...................................

salt crystals? ............................. [2]

(d) What happened to the water used in the experiment?

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

[Total: 7]

3


ForExaminer’s

Use

2 Sulfur dioxide is a poisonous gas which is denser than air and soluble in water. Sulfur dioxide can be prepared by adding dilute hydrochloric acid to sodium sulfi te and

warming the mixture. Study the diagram of the apparatus used.

hydrochloricacid

sodium sulfite water

heat

(a) Identify and explain three mistakes in the diagram.

1 mistake ........................................................................................................................

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

2 mistake ........................................................................................................................

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

3 mistake ........................................................................................................................

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

(b) State one precaution that should be taken when carrying out this experiment.

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

[Total: 7]

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3 A scientist measured the boiling point of water at different pressures.

(a) Use the thermometer diagrams in the table to complete the boiling point temperatures.

pressure/ atmospheres

thermometerdiagram

boiling point/ °C

1

105

100

95

2

125

120

115

3

140

135

130

4

140

135

130

5

155

150

145

6

160

155

150

7

170

165

160

[3]

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(b) Plot the points on the grid and draw a smooth line graph.

170

160

150

140

130

120

110

1000 1 2 3 4

pressure / atmospheres

5 6 7 8

boili

ng p

oint

/ °C

[4]

(c) State which point is inaccurate. Why have you chosen this point?

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

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

(d) Use your graph to fi nd the boiling point of water at a pressure of 7.5 atmospheres. Show clearly on the grid how you obtained your answer.

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

(e) State a chemical test for water.

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

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

[Total: 14]

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4 A student investigated the reaction between aqueous potassium manganate(VII), which is purple, and two different colourless acidic solutions, D and E.

Three experiments were carried out.

(a) Experiment 1

A burette was fi lled with the solution of potassium manganate(VII) to the 0.0 cm3 mark. Using a measuring cylinder, 25 cm3 of solution D was poured into a conical fl ask.

Potassium manganate(VII) solution was added to the fl ask until the mixture just turned permanently pink.

Use the burette diagram to record the fi nal volume in the table and complete the table.

14

15

16

final reading

burette reading



difference / cm3

[2]

(b) Experiment 2

Experiment 1 was repeated using 25 cm3 of solution E instead of solution D.

Use the burette diagrams to record the readings in the table and complete the table.

15

16

27

initial reading

46

47

48

final reading

burette reading



difference / cm3

[2]

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(c) Experiment 3

Aqueous ammonia was added to solution E in a test-tube. A green precipitate was observed.

The mixture was left to stand for 5 minutes. The surface of the precipitate turned brown.

What conclusions can you draw from these observations?

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

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

(d) (i) What colour change was observed as potassium manganate(VII) solution was added to the fl ask in Experiment 1?

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

(ii) Why was an indicator not added to the fl ask?

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

(e) (i) In which experiment was the greatest volume of potassium manganate(VII) solution used?

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

(ii) Compare the volumes of potassium manganate(VII) used in Experiments 1 and 2.

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

(iii) Suggest an explanation for the difference in volumes.

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

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

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

(f) If Experiment 2 was repeated using 12.5 cm3 of solution E, what volume of potassium manganate(VII) solution would be used? Explain your answer.

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

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

(g) Give one advantage and one disadvantage of using a measuring cylinder for solutions D and E.

advantage .........................................................................................................................

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

[Total: 17]

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5 Two liquids, F and G, were analysed. G was an aqueous solution of potassium chloride. The tests on the liquids and some of the observations are in the following table. Complete the observations in the table.

tests observations

tests on liquid F

(a) (i) Appearance of liquid F.

The pH of the liquid was tested.

(ii) An equal volume of dilute sulfuric acid was added to liquid F.

Excess aqueous sodium hydroxide was then added to the mixture.

yellow solution

pH = 7

solution turned orange

solution turned from orange to yellow

(b) Dilute sulfuric acid was added to liquid F followed by hydrogen peroxide.

The mixture was shaken and the gas given off tested with a splint.

rapid effervescence

glowing splint relit

tests on liquid G

(c) Dilute nitric acid was added to liquid G followed by aqueous barium nitrate. ................................................................ [1]

(d) Dilute nitric acid was added to liquid G followed by aqueous silver nitrate. ................................................................ [2]

(e) What does test (a)(i) tell you about liquid F?

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

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

(f) What type of reaction happened in test (a)(ii)? Explain your answer.

type of reaction .................................................................................................................

explanation .......................................................................................................................

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

(g) Identify the gas given off in test (b).

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

[Total: 8]

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6Indigestion tablets

Indigestion pain is caused by too much acid in your stomach. The acid is hydrochloric acid. Indigestion tablets contain a base which neutralises the acid.

You are provided with two different brands of indigestion tablets, Painremuve and Indcure.

Plan an investigation to compare which of these brands of tablet is the most effective. You are provided with dilute hydrochloric acid and common laboratory apparatus.

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

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

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

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

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

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

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

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

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

............................................................................................................................................ [7]

[Total: 7]

UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS...

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