Cambridge International Examinations Cambridge ...maxpapers.com/wp-content/uploads/2012/11/0620_m15_qp_all.pdfbromine liquid brown iodine ? ? astatine solid black Which information

The syllabus is approved for use in England, Wales and Northern Ireland as a Cambridge International Level1/Level 2 Certificate.

This document consists of 15 printed pages and 1 blank page.

IB15 03_0620_12/2RP © UCLES 2015 [Turn over

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Cambridge International Examinations Cambridge International General Certificate of Secondary Education

CHEMISTRY 0620/12

Paper 1 Multiple Choice February/March 2015

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, 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 16.

Electronic calculators may be used.

2

© UCLES 2015 0620/12/F/M/15

1 A crystal of purple potassium manganate(VII) was added to each of the beakers shown in the diagram.

hot water cold water

crystal of potassiummanganate(VII)

One beaker contained hot water and the other beaker contained cold water.

In both beakers the purple colour of the potassium manganate(VII) spreads out.

Which result and explanation are correct?

result explanation

A colour spreads faster in cold water particles move faster at a higher temperature

B colour spreads faster in cold water particles move slower at a higher temperature

C colour spreads faster in hot water particles move faster at a higher temperature

D colour spreads faster in hot water particles move slower at a higher temperature

2 During a reaction, the following changes take place.

1 The temperature rises.

2 A gas is given off.

Which apparatus is required to measure the rate of this reaction?

A balance and burette

B balance and gas syringe

C gas syringe and burette

D gas syringe and stopclock 3 Which statement about bonding is not correct?

A Carbon can form four single covalent bonds.

B Chlorine atoms react to gain a noble gas electronic structure.

C Covalent bonding involves losing and gaining electrons.

D Hydrogen molecules have the formula H2.

3

© UCLES 2015 0620/12/F/M/15 [Turn over

4 The table shows the numbers of particles present in the nuclei of four atoms or ions.

protons neutrons electronic structure

1 18 22 2,8,8

2 19 20 2,8,8

3 19 21 2,8,8,1

4 20 20 2,8,8,2

Which two particles belong to the same element?

A 1 and 2 B 1 and 4 C 2 and 3 D 2 and 4 5 Which substance is an ionic compound?

volatility electrical conductivity

when molten solubility in water

A high good soluble

B high poor insoluble

C low good soluble

D low poor insoluble

6 Covalent bonds are formed when electrons are ……1…… . Most covalent compounds have ……2…… electrical conductivity.

Which words correctly complete gaps 1 and 2?

1 2

A shared high

B shared low

C transferred high

D transferred low

7 Which equation for the reaction between sodium carbonate and dilute hydrochloric acid is

correct?

A Na2CO3(s) + HCl (aq) → NaCl (aq) + CO2(g) + H2O(I)

B Na2CO3(s) + HCl (aq) → Na2Cl (aq) + CO2(g) + H2O(I)

C Na2CO3(s) + 2HCl (aq) → NaCl (aq) + CO2(g) + H2O(I)

D Na2CO3(s) + 2HCl (aq) → 2NaCl (aq) + CO2(g) + H2O(I)

4

© UCLES 2015 0620/12/F/M/15

8 The diagram shows an electrolysis experiment.

electrode P

X

electrode Q

During the electrolysis, sodium was formed at electrode P and chlorine at electrode Q.

Which row correctly identifies P, Q and X?

P Q X

A

anode

cathode

concentrated solution of sodium chloride in water

B anode cathode molten sodium chloride

C

cathode

anode

concentrated solution of sodium chloride in water

D cathode anode molten sodium chloride

9 The diagram shows apparatus for plating a spoon with silver.

spoon metal electrode

electrolyte

Which statement is not correct?

A Silver would stick to the spoon because it is a very reactive metal.

B The electrolyte would be a silver salt dissolved in water.

C The metal electrode would be made from silver.

D The spoon would be connected to the negative terminal of the power supply.

5


10 Limestone can be changed into slaked lime in two chemical reactions.

1 When limestone, CaCO3, is heated it decomposes into lime, CaO.

2 Water is slowly dripped onto the cooled lime. The lime appears to expand and steam is produced. Slaked lime, Ca(OH)2, is formed.

Which row shows the correct description of each of the chemical reactions?

reaction 1 reaction 2

A endothermic endothermic

B endothermic exothermic

C exothermic endothermic

D exothermic exothermic

11 A student investigates the rate of reaction between marble chips and hydrochloric acid.

The mass of the reaction flask is measured.

The graph shows the results of two experiments, P and Q.

0

mass ofreaction flask

time

P

Q

Which change explains the difference between P and Q?

A A catalyst is added in P.

B A higher temperature is used in P.

C Bigger marble chips are used in Q.

D Hydrochloric acid is more concentrated in Q.

6

© UCLES 2015 0620/12/F/M/15

12 Hydrated cobalt(II) chloride decomposes on heating.

The equation for the reaction is

CoCl 2.6H2O CoCl 2 + 6H2O

The reaction is reversed by adding water.

Which row describes the colour change and the type of reaction for the reverse reaction?

colour change type of reaction

A blue to pink endothermic

B blue to pink exothermic

C pink to blue endothermic

D pink to blue exothermic

13 When copper is heated in air a black coating forms on the copper.

What happens to the copper in this reaction?

A The copper catches fire.

B The copper decomposes.

C The copper gains oxygen.

D The copper loses oxygen. 14 Three chemicals, P, Q and R, were each dissolved in water. The table shows some of the

reactions of these solutions.

solution reaction when solid sodium

carbonate is added reaction when heated with solid ammonium chloride

P gas evolved no reaction

Q no reaction gas evolved

R no reaction no reaction

The pH of the three solutions was also measured.

What are the correct pH values of these solutions?

P Q R

A 2 7 13

B 2 13 7

C 7 2 13

D 13 7 2

7


15 The oxide of element X forms a solution with pH 4.

The oxide of element Y forms a solution that turns Universal Indicator blue.

Which row correctly classifies elements X and Y?

element X element Y

A metal metal

B metal non-metal

C non-metal metal

D non-metal non-metal

16 Which two processes are involved in the preparation of magnesium sulfate from dilute sulfuric

acid and an excess of magnesium oxide?

A neutralisation and filtration

B neutralisation and oxidation

C thermal decomposition and filtration

D thermal decomposition and oxidation

17 Which statement about aqueous sodium hydroxide is correct?

A When it is added to a solution containing sulfate ions, a white precipitate is formed.

B When it is added to a solution of copper(II) ions, a blue precipitate is formed which dissolves in excess to give deep blue solution.

C When it is added to a solution of iron(II) ions, a green precipitate is formed which does not dissolve in excess.

D When it is added to ammonium chloride, a gas is produced which turns blue litmus red. 18 Which pair of elements will react together most violently?

A chlorine and lithium

B chlorine and potassium

C iodine and lithium

D iodine and potassium

8

© UCLES 2015 0620/12/F/M/15

19 The table shows some information about elements in Group VII of the Periodic Table.

name state at room temperature

colour

chlorine gas yellow-green

bromine liquid brown

iodine ? ?

astatine solid black

Which information about iodine completes the table?

state colour

A liquid black

B liquid green

C solid grey

D solid yellow

20 The diagram shows a section of the Periodic Table.

Which element is described below?

‘A colourless, unreactive gas that is denser than air.’

AB

CD

21 Which is not a characteristic property of transition metals?

A act as catalysts

B form coloured compounds

C high melting point

D low density

9


22 Which statement is correct for all metals?

A conduct electricity when molten

B gain electrons when they form ions

C have a low density

D have a low melting point 23 Metal X lies between zinc and iron in the reactivity series.

Which statements about metal X are correct?

1 It reacts with steam to produce hydrogen gas.

2 It does not react with steam but will produce hydrogen with dilute acid.

3 The metal can be obtained from its oxide by heating strongly with charcoal.

4 The metal oxide cannot be reduced using carbon.

A 1 and 3 B 1 and 4 C 2 and 3 D 2 and 4 24 Which of these gases is an atmospheric pollutant?

1 carbon monoxide

2 nitrogen dioxide

3 sulfur dioxide

A 1 only B 2 only C 3 only D 1, 2 and 3 25 Molten iron from the blast furnace contains impurities.

The process of turning the impure iron into steel involves blowing oxygen into the molten iron and adding calcium oxide.

What are the reasons for blowing in oxygen and adding calcium oxide?

blowing in oxygen adding calcium oxide

A carbon is removed by reacting with oxygen reacts with acidic impurities making slag

B carbon is removed by reacting with oxygen reacts with slag and so removes it

C iron reacts with the oxygen reacts with acidic impurities making slag

D iron reacts with the oxygen reacts with slag and so removes it

10

© UCLES 2015 0620/12/F/M/15

26 Some properties of aluminium are listed.

1 It has mechanical strength.

2 It is resistant to corrosion.

3 It has a low density.

4 It conducts heat.

Which three properties make aluminium useful for making the bodies of aircraft?

A 1, 2 and 3 B 1, 2 and 4 C 1, 3 and 4 D 2, 3 and 4 27 The table describes three types of water.

water type

source of water

appearance before treatment

treatment appearance after

treatment

P river muddy none muddy

Q river muddy filtration and chlorination clear

R well clear chlorination only clear

Which statement is correct?

A Only Q and R are suitable for drinking, while P could be used for irrigation.

B Only Q and R are suitable for drinking, while P is unsuitable for any purpose.

C Only Q is suitable for drinking. R could be used for washing cars and P for irrigation.

D P, Q and R are suitable for irrigation and washing cars, but are not suitable for drinking. 28 A sample of air from a town centre was analysed and found to contain mainly nitrogen and

oxygen, but also traces of the four gases below.

Which of these gases is a pollutant?

A argon

B carbon dioxide

C sulfur dioxide

D water vapour 29 Which elements does an NPK fertiliser contain?

A nickel, phosphorus, potassium

B nickel, potassium, calcium

C nitrogen, phosphorus, potassium

D nitrogen, potassium, calcium

11


30 The diagram shows experiments involving the rusting of iron.

water boiledto remove air

water anhydrous calciumchloride to dry the air

oiliron nails

tube Q tube Rtube P

The following results were suggested.

1 In tube P, the iron nails rust.

2 In tube Q, the iron nails do not rust.

3 In tube R, the iron nails do not rust.

Which results are correct?

A 1 and 2 only

B 1 and 3 only

C 2 and 3 only

D 1, 2 and 3 31 Gas X is a waste gas from digestion in animals.

Gas Y is formed when gas X is burnt with a small amount of oxygen.

Gas Z is formed when gas X is burnt with an excess of oxygen.

What are X, Y and Z?

X Y Z

A carbon dioxide methane carbon monoxide

B carbon monoxide methane carbon dioxide

C methane carbon dioxide carbon monoxide

D methane carbon monoxide carbon dioxide

12

© UCLES 2015 0620/12/F/M/15

32 The list gives four experiments carried out with calcium carbonate.

1 acid added

2 alkali added

3 heated strongly

4 water added

Which experiments produce carbon dioxide?

A 1 and 2 B 1 and 3 C 2 and 3 D 2 and 4 33 The diagram shows the soil pH range over which a vegetable grows well.

The pH of the soil to be used is 5.5.

5.0 6.0 7.0 8.0 9.0pH

vegetablegrows well

Why is lime added to the soil before planting the vegetable?

A The lime acts as a catalyst.

B The lime changes the soil acidity.

C The lime is an indicator.

D The lime supplies nitrogen. 34 The diagram shows the structure of a compound.

H

C

H

C

H

H

C

H

O H

H

C

H

Which functional groups does this molecule contain?

carboxylic

acid alkene alcohol

A no no no

B no yes yes

C yes no yes

D yes yes yes

13


35 Petroleum is separated into useful fractions by fractional distillation.

Separation occurs in a fractionating column.

Some properties of three of these fractions are shown.

fraction boiling point

range / °C

number of carbon atoms in the molecules

1 5–10

2 320–350 16–24

3 120–210

Which statement is correct?

A Fraction 1 has a higher boiling point range than fraction 2.

B Fraction 2 is removed from a higher point in the fractioning tower than fraction 1.

C Molecules in fraction 3 have shorter chains than those in fraction 2.

D None of the fractions is liquid at room temperature. 36 The structures of four molecules are shown.

C

H

H

C

H

H

4

C

H

H

CH OH

H

H

2

C

H

H

CH H

H

H

3

C

H

H

CH C

H

H

H

OH

H

1

Which molecules belong to the same homologous series?

A 1 and 2 B 1 and 3 C 2 and 4 D 3 and 4 37 Which statement about alkanes is correct?

A Ethane has one more carbon atom and one more hydrogen atom than methane.

B They are converted to alcohols by reaction with steam.

C They contain carbon-carbon double bonds.

D They form carbon dioxide and water on combustion.

14

© UCLES 2015 0620/12/F/M/15

38 Which statement about alkenes is not correct?

A They are hydrocarbons.

B They are saturated.

C They contain a C=C bond.

D They form polymers. 39 Ethene reacts with Y to produce ethanol.

ethene + Y → ethanol

What is Y?

A hydrogen

B oxygen

C steam

D yeast 40 Which description of ethanoic acid is correct?

A a clear, colourless and odourless liquid

B a colourless liquid with a distinctive odour

C a soft white solid with a distinctive odour

D a transparent solid with a low melting point

15

© UCLES 2015 0620/12/F/M/15

BLANK PAGE

16

To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge International Examinations Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download at www.cie.org.uk after the live examination series.

© UCLES 2015 0620/12/F/M/15

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

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91

238 U

Ura

nium

92

Np

Nep

tuni

um93

PuP

luto

nium

94

Am

Am

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ium

95

Cm

Cur

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96

Bk

Ber

keliu

m97

Cf

Cal

iforn

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98

EsE

inst

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Fm Ferm

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100

Md

Men

dele

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101

No

Nob

eliu

m10

2

LrLa

wre

nciu

m10

3

1 HH

ydro

gen

1

7 LiLi

thiu

m3

23 Na

Sod

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11

24 Mg

Mag

nesi

um12

40 Ca

Cal

cium

20

45 ScS

cand

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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

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29

65 Zn Zinc

30

70 Ga

Gal

lium

31

27 Al

Alu

min

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13

11 B Bor

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12 CC

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14 NN

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19 FFl

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28 Si Sili

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31 PP

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32 S Sul

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35.5 Cl

Chl

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40 Ar

Arg

on18

20 Ne

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4 He

Hel

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73 Ge

Ger

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75 As

Ars

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33

79 SeS

elen

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80 Br

Bro

min

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84 Kr

Kry

pton

36

39 KP

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19

88 SrS

tront

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89 YY

ttriu

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91 ZrZi

rcon

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93 Nb

Nio

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41

96 Mo

Mol

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TcTe

chne

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43

101

Ru

Rut

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103

Rh

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106

PdP

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46

108

Ag

Silv

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112

Cd

Cad

miu

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115

In Indi

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119

Sn Tin

50

122

SbA

ntim

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51

128

TeTe

lluriu

m52

127 I

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131

Xe Xen

on54

137

Ba

Bar

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139

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ntha

num

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181

TaTa

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184 W

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186

Re

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190

Os

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192

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Pla

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197

Au

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Hg

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204 Tl

Thal

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81

207

Pb Lead

82

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At

Ast

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Rn

Rad

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FrFr

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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 use an HB pencil for any diagrams or graphs.Do not use staples, paper clips, 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 0620/22

Paper 2 February/March 2015

1 hour 15 minutes

Candidates answer on the Question Paper.

No Additional Materials are required.

Cambridge International ExaminationsCambridge International General Certifi cate of Secondary Education

This document consists of 14 printed pages and 2 blank pages.

[Turn overIB15 03_0620_22/3RP© UCLES 2015

*6533820761*

The syllabus is approved for use in England, Wales and Northern Ireland as a Cambridge International Level 1/Level 2 Certifi cate.

2

0620/22/F/M/15© UCLES 2015

1 The diagram shows the structures of some substances containing carbon.

A B C

D E F

O C O H C

H

H

H

H

C H

Ca2+CO32–

CO32– CO3

2–

CO32– CO3

2–

CO32–

CO32– CO3

2–

Ca2+

Ca2+ Ca2+

Ca2+ Ca2+

Ca2+ Ca2+

C

Cl

ClClCl

C C

H

H

H

C

H

H

H

Answer the following questions about these substances. Each substance may be used once, more than once or not at all.

(a) Which substance, A, B, C, D, E or F

(i) is a saturated hydrocarbon, ................................................................................................

(ii) has an ionic structure, ........................................................................................................

(iii) is a product of respiration, ..................................................................................................

(iv) is in the same homologous series as methane, .................................................................

(v) is used for cutting? .............................................................................................................[5]

(b) Substance D is an element.

Explain why substance D is an element.

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

[Total: 6]

3

0620/22/F/M/15© UCLES 2015 [Turn over

2 Some properties of the halogens are shown in the table.

halogen boiling point/ °C

state at room temperatureand pressure

fl uorine –188

chlorine –35 gas

bromine +59 liquid

iodine +184 solid

astatine solid

(a) Use the information in the table to deduce

(i) the boiling point of astatine,

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

(ii) the state of fl uorine at room temperature and pressure.

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

(b) When chlorine reacts with aqueous potassium iodide, the solution turns brown.

(i) Write a word equation for this reaction.

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

(ii) Explain why iodine does not react with aqueous potassium chloride.

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

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

(c) When sodium reacts with iodine, energy is released.

(i) What is the name given to a reaction which releases energy?

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

(ii) Explain what happens in terms of electron transfer when a sodium atom reacts with an iodine atom.

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

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

[Total: 8]

4

0620/22/F/M/15© UCLES 2015

3 The diagram shows a limestone column in an industrial town. Limestone is largely calcium carbonate.

column when first built the same columnafter 40 years

iron pins

(a) Describe and explain the changes to the column over 40 years. In your answer refer to

• the change to the limestone, • the name of a pollutant causing this change, • the chemistry involved in this change.

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

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

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

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

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

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

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

(b) The sections of the column are joined with iron pins which rust when exposed to the atmosphere.

Describe two methods of rust prevention and explain how they prevent rusting.

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

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

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

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

5


(c) Iron is a transition element.

Give two properties of transition elements that make them different from non-transition metals such as magnesium.

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

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

(d) An isotope of iron has 58 nucleons.

Complete the table to show

• the number of electrons and neutrons in this isotope of iron, • the relative charges on each particle.

particle number of eachparticle present

relative chargeon the particle

electron

neutron no charge

proton 26

[4]

(e) Iron reacts with hydrochloric acid to form iron(II) chloride and a gas which ‘pops’ with a lighted splint.

Complete the symbol equation for this reaction.

Fe + ....... HCl → FeCl 2 + ............[2]

[Total: 15]

6

0620/22/F/M/15© UCLES 2015

4 Ammonium phosphate, (NH4)3PO4, is a fertiliser.

(a) Which two elements in ammonium phosphate are important for plant growth?

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

(b) Aqueous ammonium phosphate can be made in the laboratory by reacting aqueous ammonia with aqueous phosphoric acid.

aqueousphosphoric acid

flask

A

aqueousammonia

(i) State the name of the piece of apparatus labelled A.

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

(ii) Suggest the pH value of aqueous phosphoric acid.

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

(iii) Describe how the pH of the mixture in the fl ask changes as the acid is added.

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

(iv) Which one of the following best describes the reaction of aqueous ammonia with aqueous phosphoric acid?

Put a ring around the correct answer.

combustion decomposition neutralisation reduction[1]

(c) When sodium hydroxide is added to ammonium phosphate, ammonia is released.

Complete the symbol equation for this reaction.

(NH4)3PO4 + 3NaOH → Na3PO4 + .......NH3 + 3 ...............[2]

[Total: 7]

7


5 The table shows the concentration of some ions present in a sample of seawater.

name of ion formula of ion concentrationin g / dm3

bromide Br – 0.06

calcium Ca2+ 0.30

chloride Cl – 20.00

I– 0.04

magnesium Mg2+ 1.00

potassium K+ 0.50

sodium Na+ 11.00

sulfate SO42– 0.80

(a) (i) Which positive ion in the table has the lowest concentration?

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

(ii) Give the name of the ion with the formula I–.

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

(iii) Which two ions in the table are formed from elements in Group II of the Periodic Table?

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

(iv) Give the names of two ions in the table which move towards the anode (positive electrode) when a sample of this seawater is electrolysed.

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

8

0620/22/F/M/15© UCLES 2015

(b) Sodium chloride can be extracted from seawater. Concentrated aqueous sodium chloride is electrolysed using the apparatus shown.

+ –

graphiteanode

concentrated aqueoussodium chloride

graphitecathode

battery

(i) Suggest why the anode and cathode are made of graphite.

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

(ii) Give the name of the product formed at the cathode (negative electrode).

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

(iii) Chlorine is formed at the anode.

Complete the electronic structure of a chlorine molecule. Show only the outer shell electrons.

Cl Cl

[2]

(c) Molten magnesium bromide is electrolysed.

Predict the products at the anode (positive electrode) and cathode (negative electrode).

anode .........................................................................................................................................

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

[Total: 11]

9


6 Zinc oxide is used for making baby soap and cream for treating sunburn.

(a) Suggest why the zinc oxide used for these purposes needs to be pure.

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

(b) Zinc oxide can be reduced by carbon. Carbon monoxide is one of the products.

(i) What is the meaning of the term reduction?

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

(ii) Write a word equation for the reaction of zinc oxide with carbon.

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

(iii) Explain why, in the laboratory, the reaction should be carried out in a fume cupboard.

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

(c) The table shows how easy it is to reduce various metal oxides by heating with carbon.

metal oxide ease of reduction with carbon

lead oxide easily reduced at 300 °C

magnesium oxide not reduced at 900 °C

nickel oxide easily reduced at 500 °C

zinc oxide fairly easily reduced at 900 °C

Use the information in the table to put the metals in order of their reactivity.

least reactive most reactive

[2]

(d) Zinc oxide reacts with sulfuric acid.

Complete the word equation for this reaction.

zinc oxide + sulfuric acid → zinc sulfate + ............................[1]

10

0620/22/F/M/15© UCLES 2015

(e) Pure dry crystals of zinc sulfate can be made by the reaction of dilute sulfuric acid with excess zinc.

(i) How is excess zinc removed from the reaction mixture?

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

(ii) Describe how you would obtain pure dry crystals of zinc sulfate from an aqueous solution of zinc sulfate.

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

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

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

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

(iii) Zinc sulfate can be made from the reaction of sulfuric acid with zinc oxide or zinc.

Give the name of another compound that reacts with sulfuric acid to produce zinc sulfate.

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

(f) A student reacts zinc with excess sulfuric acid. She obtains 16.1 g of zinc sulfate from 6.5 g of zinc.

(i) Calculate the mass of zinc sulfate she would obtain from 26.0 g of zinc.

[1]

(ii) Calculate the relative formula mass of zinc sulfate, ZnSO4.

[2]

[Total: 15]

11


7 Petroleum is separated into useful fractions by fractional distillation.

kerosene fraction

T

gasoline fraction

refinery gas

fractions

fuel oil

lubricating fractionpetroleum

bitumen

diesel oil

(a) (i) Put an X on the diagram to show where the temperature in the column is the highest. [1]

(ii) Give the name of the fraction labelled T.

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

(iii) The lubricating fraction is used to make lubricants.

Give one other use of this fraction.

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

(b) Each fraction contains alkanes.

Which two of the following statements are correct? Tick two boxes.

Alkanes burn to form carbon dioxide and hydrogen.

Ethene is an alkane with two carbon atoms.

Alkanes polymerise to form poly(alkanes).

Alkanes are generally unreactive apart from burning.

Methane is an alkane present in natural gas.[2]

12

0620/22/F/M/15© UCLES 2015

(c) Hydrogen can be made by cracking.

(i) What is meant by the term cracking?

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

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

(ii) Complete the equation for the cracking of propane.

C3H8 → ................ + H2[1]

(d) Ethanol is formed by the catalytic addition of steam to ethene.

(i) Complete the structures of ethene and ethanol in the equation below, showing all atoms and bonds.

+

ethene

H

H

C

ethanol

H

H

CHO

H H

[2]

(ii) What does the symbol mean?

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

[Total: 11]

13


8 A student placed a crystal of purple potassium manganate(VII) on a fi lter paper which had been soaked in water.

After 5 minutes, a purple colour had spread out from the crystal. After 30 minutes, the purple colour had spread further out.

crystal ofpotassiummanganate(VII)

at the start after 5 minutes after 30 minutes

wet filter paper

(a) Use the kinetic particle theory to explain these observations.

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

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

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

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

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

(b) Describe the closeness and motion of the particles in a crystal of potassium manganate(VII).

closeness ...................................................................................................................................

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

(c) Mixtures of dyes can be separated by paper chromatography using the apparatus shown below.

base line

On the diagram above

• draw a line to show the solvent level at the beginning of the experiment, • put a cross to show where the spot of dye mixture is placed at the beginning of the

experiment.[2]

[Total: 7]

14

0620/22/F/M/15© UCLES 2015

BLANK PAGE

15

0620/22/F/M/15© UCLES 2015

BLANK PAGE

16

0620/22/F/M/15© UCLES 2015


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 an HB pencil for any diagrams or graphs.Do not use staples, paper clips, 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 12.You may lose marks if you do not show your working or if you do not use appropriate units.


CHEMISTRY 0620/32

Paper 3 (Extended) February/March 2015

1 hour 15 minutes






*3584316295*


2

0620/32/F/M/15© UCLES 2015

1 For each of the following, give the name of an element from Period 3 (sodium to argon), which matches the description.

(a) an element which is gaseous at room temperature and pressure

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

(b) an element that is added to water to kill bacteria

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

(c) an element that forms a basic oxide of the type XO

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

(d) an element used as an inert atmosphere in lamps

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

(e) an element that forms an amphoteric oxide

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

(f) an element that reacts vigorously with cold water to produce hydrogen

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

[Total: 6]

2 (a) Defi ne the term isotope.

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

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

(b) The table gives information about four particles, A, B, C and D.

Complete the table. The fi rst line has been done for you.

particle numberof protons

numberof electrons

numberof neutrons

nucleonnumber

symbolor formula

A 6 6 6 12 C

B 11 10 12

C 8 8 O2–

D 10 28 Al 3+

[7]

[Total: 9]

3


3 Ammonia is manufactured by the Haber process. Nitrogen and hydrogen are passed over a catalyst at a temperature of 450 °C and a pressure of 200 atmospheres.

The equation for the reaction is as follows.

N2 + 3H2 2NH3

The forward reaction is exothermic.

(a) State one use of ammonia.

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

(b) What is the meaning of the symbol ?

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

(c) What are the sources of nitrogen and hydrogen used in the Haber process?

nitrogen ......................................................................................................................................

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

(d) Name the catalyst in the Haber process.

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

(e) (i) If a temperature higher than 450 °C was used in the Haber process, what would happen to the rate of the reaction? Give a reason for your answer.

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

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

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

(ii) If a temperature higher than 450 °C was used in the Haber process, what would happen to the yield of ammonia? Give a reason for your answer.

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

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

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

4

0620/32/F/M/15© UCLES 2015

(f) (i) If a pressure higher than 200 atmospheres was used in the Haber process, what would happen to the yield of ammonia? Give a reason for your answer.

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

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

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

(ii) Explain why the rate of reaction would be faster if the pressure was greater than 200 atmospheres.

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

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

(iii) Suggest one reason why a pressure higher than 200 atmospheres is not used in the Haber process.

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

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

(g) Draw a dot-and-cross diagram to show the arrangement of the outer (valency) electrons in one molecule of ammonia.

[2]

(h) Ammonia acts as a base when it reacts with sulfuric acid.

(i) What is a base?

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

(ii) Write a balanced equation for the reaction between ammonia and sulfuric acid.

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

[Total: 18]

5


4 (a) A compound X contains 82.76% of carbon by mass and 17.24% of hydrogen by mass.

(i) Calculate the empirical formula of compound X.

[2]

(ii) Compound X has a relative molecular mass of 58.

Deduce the molecular formula of compound X.

[2]

(b) Alkenes are unsaturated hydrocarbons.

(i) State the general formula of alkenes.

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

(ii) State the empirical formula of alkenes.

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

(c) What is meant by the term unsaturated hydrocarbon?

unsaturated ................................................................................................................................

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

hydrocarbon ...............................................................................................................................

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

6

0620/32/F/M/15© UCLES 2015

(d) Describe a test that would distinguish between saturated and unsaturated hydrocarbons.

reagent ......................................................................................................................................

observation (saturated hydrocarbon) .........................................................................................

observation (unsaturated hydrocarbon) .....................................................................................[3]

(e) Addition polymers can be made from alkenes. The diagram shows part of an addition polymer.

C

H

C2H5 H C2H5 H

H H H

C C C

(i) Draw a circle on the diagram to show one repeat unit in this polymer. [1]

(ii) Give the structure and the name of the monomer used to make this polymer.

structure

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

(iii) Give the structure of an isomer of the alkene in (e)(ii).

[1]

[Total: 15]

7


5 Aluminium and iron are extracted from their ores by different methods.

Aluminium is extracted from its purifi ed oxide ore by electrolysis.

cathode(negative electrode)

oxygen given offat anode (positive electrode)

aluminium oxide dissolvedin molten cryolite

aluminium

waste gases

(a) What is the name of the ore of aluminium which consists mainly of aluminium oxide?

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

(b) The electrodes are both made of the same substance.

Name this substance.

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

(c) Aluminium oxide is dissolved in molten cryolite before it is electrolysed.

Give two reasons why aluminium oxide dissolved in molten cryolite is electrolysed rather than molten aluminium oxide alone.

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

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

(d) Write the ionic equations for the reactions at the electrodes in this electrolysis.

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

cathode (negative electrode) .....................................................................................................[2]

8

0620/32/F/M/15© UCLES 2015

(e) Iron is extracted from its oxide ore by reduction using carbon in a blast furnace.

slag

molten iron

air air

waste gases

raw materials:coke,iron ore,limestone.

(i) Place the elements aluminium, carbon and iron in order of reactivity with the least reactive element fi rst.

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

(ii) Use your answer to (e)(i) to explain why iron is extracted by reduction using carbon but aluminium is not.

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

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

(f) What is the name of the ore of iron which consists mainly of iron(III) oxide?

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

(g) Write balanced equations for the reactions occurring in the blast furnace which involve

(i) the complete combustion of coke (carbon),

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

(ii) the production of carbon monoxide from carbon dioxide,

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

(iii) the reduction of iron(III) oxide,

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

(iv) the formation of slag.

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

[Total: 13]

9


6 A student is told to produce the maximum amount of copper from a mixture of copper and copper(II) carbonate.

The student adds the mixture to an excess of dilute sulfuric acid in a beaker and stirs the mixture with a glass rod. The copper(II) carbonate reacts with the sulfuric acid, forming a solution of copper(II) sulfate but the copper does not react with the sulfuric acid.

The student then

• removes the unreacted copper from the mixture, • converts the solution of copper(II) sulfate into copper by a series of reactions.

(a) Describe two things that the student would observe when the mixture is added to the dilute sulfuric acid.

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

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

(b) Describe how the student can produce pure dry copper from the mixture of copper and copper(II) sulfate solution.

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

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

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

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

(c) The student then adds sodium hydroxide solution to the copper(II) sulfate solution to produce copper(II) hydroxide.

(i) Describe what the student would observe.

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

(ii) Write an ionic equation for this reaction.

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

(d) After separating the copper(II) hydroxide from the mixture, the copper(II) hydroxide is heated strongly. The copper(II) hydroxide decomposes into copper(II) oxide and steam.

(i) Write an equation for the decomposition of copper(II) hydroxide. Include state symbols.

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

(ii) Name a non-metallic element that can be used to convert copper(II) oxide into copper.

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

[Total: 10]

10

0620/32/F/M/15© UCLES 2015

7 Ethanol is manufactured from glucose, C6H12O6, by fermentation according to the following equation.

C6H12O6 → 2C2H5OH + 2CO2

(a) State the conditions required for this reaction.

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

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

(b) In an experiment, 30.0 g of glucose was fermented.

(i) Calculate the number of moles of glucose in 30.0 g.

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

(ii) Calculate the maximum mass of ethanol that could be obtained from 30.0 g of glucose.

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

(iii) Calculate the volume of carbon dioxide at room temperature and pressure that can be obtained from 30.0 g of glucose.

......................... dm3 [1]

(c) Ethanol can also be manufactured from ethene.

(i) Name the raw material which is the source of ethene.

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

(ii) Write a balanced equation for the manufacture of ethanol from ethene.

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

[Total: 9]

11

0620/32/F/M/15© UCLES 2015

BLANK PAGE

12

0620/32/F/M/15© UCLES 2015


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.You may lose marks if you do not show your working or if you do not use appropriate units.Practical notes are provided on page 8.


CHEMISTRY 0620/52

Paper 5 Practical Test February/March 2015

1 hour 15 minutes


Additional Materials: As listed in the Confi dential Instructions




*7312444178*

For Examiner’s Use

Total


2

0620/52/F/M/15© UCLES 2015

BLANK PAGE

3


1 You are going to investigate the solubility of salt D in water at various temperatures.

Read all the instructions below carefully before starting the experiments.

Instructions You are going to carry out four experiments.

(a) Experiment 1

You are provided with a clean boiling tube containing 4 g of salt D. Fill the burette provided with distilled water and add 10.0 cm3 of water to the boiling tube. Heat

the mixture of salt D and water carefully until all of the solid has dissolved.

Remove the boiling tube from the heat and allow the solution to cool. Stir the solution gently with the thermometer.

Note the temperature at which crystals fi rst appear and record the temperature in the table at the top of page 4.

Keep the boiling tube and its contents for the remaining three experiments in this question.

(b) Experiment 2

From the burette, add a further 2.0 cm3 of water to the boiling tube and contents from Experiment 1.

Heat the mixture to dissolve the crystals as before. Find the temperature at which crystals fi rst appear.

It will help if the boiling tube is dipped for short periods of time in a beaker of cold water to speed up the rate of cooling.

Record, in the table, the total volume of water in the boiling tube and the temperature at which crystals fi rst appear.

(c) Experiment 3

From the burette, add a further 2.0 cm3 of water to the boiling tube and contents from Experiment 2. Repeat the experiment exactly as before.

Record, in the table, the total volume of water in the boiling tube and the temperature at which crystals fi rst appear.

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0620/52/F/M/15© UCLES 2015

(d) Experiment 4

From the burette, add a further 4.0 cm3 of water to the boiling tube and contents from Experiment 3. Repeat the experiment exactly as before.

Note all the results in the table.

At the end of Experiment 4, the total volume of water in the boiling tube will be 18.0 cm3.

Experimentnumber

total volume ofwater / cm3

temperature at whichcrystals fi rst appear / °C

1 10.0

2

3

4[5]

(e) Plot the results on the grid below and draw a smooth line graph.

8 10 12 14 16

total volume of water / cm3

18 20 22

temperatureat which crystalsfirst appear / °C

[5]

5


(f) From your graph, fi nd the temperature at which crystals of D would fi rst appear if the total volume of water in the solution was 20.0 cm3.

Show clearly on the grid how you worked out your answer.

..............................°C [2]

(g) How did you know when salt D was completely dissolved in the water?

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

(h) The solubility of salt D at 100 °C is 57 g in 100 cm3 of water.

Suggest, with a reason, the effect of using 8 g of salt D instead of 4 g in these experiments.

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

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

(i) Salt C is less soluble in water than salt D.

Sketch on the grid the graph you would expect for salt C. Label this graph. [2]

(j) Describe and explain one improvement that could be made to the experimental method to obtain more reliable results in this investigation.

improvement ..............................................................................................................................

explanation ................................................................................................................................

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

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

[Total: 19]

Before moving on to Question 2, carefully place your solution of salt D, boiling tube, stopper and thermometer into the container labelled waste for Question 1.

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2 You are provided with two metal salt solutions, E and F. Carry out the following tests on E and F, recording all of your observations in the table. Conclusions must not be written in the table.

tests observations

tests on solution E

(a) Describe the appearance of solution E. ................................................................ [1]

Divide the solution into three equal portions in separate test-tubes.

(b) To the fi rst portion of the solution, add a few drops of dilute nitric acid and about 1 cm3 of aqueous barium nitrate. ................................................................ [2]

(c) To the second portion of the solution, add excess aqueous sodium hydroxide and shake the mixture.

Filter the mixture. Gently warm the fi ltrate and test the gas given off.

Note how the residue on the fi lter paper changes after fi ve minutes.

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

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

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

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

(d) To the third portion of the solution, add about 1 cm3 of aqueous potassium manganate(VII).

Now add aqueous sodium hydroxide to the mixture.

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

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

tests on solution F

(e) (i) Describe the appearance of solution F.

(ii) Test the pH of solution F.

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

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

(f) Add a few zinc granules to the solution F provided in the boiling tube. Shake the tube every minute.

Note how the colour of the solution changes over the next fi ve minutes.

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

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

7


(g) What conclusions can you draw about solution E?

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

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

(h) What conclusions can you draw about solution F?

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

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

[Total: 21]

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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.

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]

acidify with dilute nitric acid, thenadd aqueous silver nitrate

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

This document consists of 12 printed pages.


*7492298954*



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 0620/62

Paper 6 Alternative to Practical February/March 2015

1 hour





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1 A teacher separated a mixture of two liquids using the apparatus shown. The liquids were:

• ethanoic acid, boiling point 118 °C,

• chloroethanoic acid, boiling point 190 °C.

heat

cold water out

cold water in

smallglass beads

fractionating column

mixture of liquids

(a) Complete the boxes to label the pieces of apparatus used. [2]

(b) (i) Which liquid would be collected fi rst? Explain why.

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

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

(ii) How would the teacher know when all of this liquid had been collected?

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

(c) Suggest why small glass beads are used in the fractionating column instead of large glass beads.

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

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

(d) Give a test to show that the liquids are acidic.

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

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

[Total: 8]

3


2 The rate of reaction between excess calcium carbonate and dilute hydrochloric acid was investigated using the apparatus shown below. The temperature of the hydrochloric acid was 25 °C.

hydrochloric acid

excess calcium carbonate

gas syringe

The volume of carbon dioxide evolved was measured every minute for six minutes.

(a) Use the gas syringe diagrams to complete the table of results.

0 10 20 30 50 6040

0 10 20 30 50 6040

0 10 20 30 50 6040

30 40 50 60 80 9070

30 40 50 60 80 9070

30 40 50 60 80 9070

30 40 50 60 80 9070

time/ minutes

0

1

2

3

4

5

6

gas syringe diagram total volume ofcarbon dioxide evolved / cm3

[3]

4

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(b) Plot the results on the grid below and draw a smooth line graph.

0 1 2 3 4

time / minutes

5 6

volume ofcarbon dioxideevolved / cm3

100

80

60

40

20

0

[4]

(c) (i) Which point appears to be inaccurate? Explain why.

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

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

(ii) Use your graph to work out the volume of gas expected at that time. Show clearly on the grid how you worked out your answer.

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

(d) Sketch, on the grid, the graph you would expect if the experiment was repeated using hydrochloric acid at a temperature of 50 °C. [2]

[Total: 13]

5


3 Electricity was passed through concentrated hydrochloric acid using the apparatus shown.

concentratedhydrochloric acid andUniversal Indicator

+ –

battery

negativeelectrode

positiveelectrode

Effervescence was observed at both electrodes.

(a) Name this process used to break down concentrated hydrochloric acid.

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

(b) Suggest why the electrodes are made of platinum and not aluminium.

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

(c) (i) Name the gas given off at the positive electrode.

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

(ii) What would be the colour of the Universal Indicator around the positive electrode at the end of the experiment?

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

[Total: 4]

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4 A student investigated the solubility of salt D in water at various temperatures.

Four experiments were carried out.

(a) Experiment 1

4 g of salt D was added to a boiling tube. A burette was fi lled with distilled water and 10.0 cm3 of water added to the boiling tube. The mixture of salt D and water was heated carefully until all of the solid had dissolved. The boiling tube was removed from the heat and the solution allowed to cool. The solution was stirred gently with a thermometer.

The temperature at which crystals fi rst appeared was noted.

The boiling tube and its contents were kept for the remaining three experiments.

(b) Experiment 2

From the burette another 2.0 cm3 of water was added to the boiling tube and contents from Experiment 1.

The mixture was heated to dissolve the crystals and allowed to cool as in Experiment 1. The temperature at which crystals fi rst appeared was noted.

Record, in the table, the total volume of water in the boiling tube.

(c) Experiment 3

From the burette another 2.0 cm3 of water was added to the boiling tube and contents from Experiment 2. The experiment was repeated exactly as before.

Record, in the table, the total volume of water in the boiling tube.

7


(d) Experiment 4

From the burette another 4.0 cm3 of water was added to the boiling tube and contents from Experiment 3. The experiment was repeated exactly as before.

Record in the table the total volume of water in the boiling tube.

Use the thermometer diagrams in the table to record the temperatures at which crystals fi rst appeared in the four experiments.

Experimentnumber

total volumeof water / cm3 thermometer diagram temperature at which

crystals fi rst appeared / °C

1 10.0

95

90

85

2

80

75

70

3

70

65

60

4

60

55

50

[3]

8

0620/62/F/M/15© UCLES 2015

(e) Plot the results on the grid below and draw a smooth line graph.

8.0 10.0 12.0 14.0 16.0

total volume of water / cm3

18.0 20.0

temperatureat which crystalsfirst appeared / °C

[5]

(f) From your graph, fi nd the temperature at which crystals of D would fi rst appear if the total volume of water in the solution was 20.0 cm3.

Show clearly on the grid how you worked out your answer.

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

(g) How would the student know when salt D was completely dissolved in the water?

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

9


(h) The solubility of salt D at 100 °C is 57 g in 100 cm3 of water. Suggest, with a reason, the effect of using 8 g of salt D instead of 4 g in these experiments.

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

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

(i) Salt C is less soluble in water than salt D.

Sketch on the grid the graph you would expect for salt C. Label this graph. [2]

(j) Describe and explain one improvement that could be made to the experimental method to obtain more reliable results in this investigation.

improvement ..............................................................................................................................

explanation ................................................................................................................................

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

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

[Total: 18]

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5 Two metal salt solutions, E and F, were analysed. E was a mixture of iron(II) sulfate and ammonium sulfate. The tests on the solutions and some of the observations are in the following table. Complete the observations in the table.

tests observations

tests on solution E

(a) Appearance of solution E. ................................................................ [1]

The solution was divided into three equal portions in separate test-tubes.

(b) Dilute nitric acid and aqueous barium nitrate were added to the fi rst portion of the solution. ................................................................ [1]

(c) (i) Excess aqueous sodium hydroxide was added to the second portion of the solution.

(ii) The mixture was fi ltered and the fi ltrate heated.

The gas given off was tested with damp litmus paper.

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

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

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

(d) Dilute sulfuric acid and aqueous potassium manganate(VII), an oxidising agent, were added to the third portion of the solution.

Aqueous sodium hydroxide was then added to the mixture. ................................................................ [1]

tests on solution F

(e) Appearance of solution F. yellow liquid

(f) Zinc powder was added to solution F.

The solution was observed for fi ve minutes.

The gas given off was tested with a splint.

rapid effervescence

turned blue, then green and fi nally light purple

lighted splint popped

11


(g) Identify the gas given off in test (f).

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

(h) What conclusions can you draw about solution F?

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

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

[Total: 10]

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0620/62/F/M/15© UCLES 2015

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.

6 Rhubarb Leaves

Ethanedioic acid dihydrate, H2C2O4.2H2O, is a white crystalline solid. This acid is water-soluble and is found in rhubarb leaves.

Plan an investigation to obtain crystals of ethanedioic acid dihydrate from some rhubarb leaves. You are provided with common laboratory apparatus, water and sand.

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

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

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

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

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

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

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

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

..................................................................................................................................................... [7]

[Total: 7]

Cambridge International Examinations Cambridge ...maxpapers.com/wp-content/uploads/2012/11/0620_m15_qp_all.pdfbromine liquid brown iodine ? ? astatine solid black Which information

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