Chemstry June 2001 - Paper 1

UNIVERSITY OF CAMBRIDGE LOCAL EXAMINATIONS SYNDICATE General Certificate of Education Ordinary Level

CHEMISTRY

5070/1

PAPER 1 Multiple Choice MAY/JUNE SESSION 2001

1 hour

Additional materials: Mathematical tables and/or calculator Multiple choice answer sheet Soft clean eraser Soft pencil (type B or HB is recommended)

TIME

1 hour

INSTRUCTIONS TO CANDIDATES Do not open this booklet until you are told to do so. Write your name, Centre number and candidate number on the answer sheet in the spaces provided unless this has already been done for you. There are forty questions in 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 very carefully the instructions on the answer sheet. INFORMATION FOR CANDIDATES 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. Mathematical tables are available. You may use a calculator. A copy of the Periodic Table is printed on page 16.

This question paper consists of 16 printed pages. SB (CW/CG) QF10456/3 © UCLES 2001

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2 1

The coverplate was removed from the gas jars shown in the diagram. After several days, the colour of the gas was the same in both jars.

oxygen cover plate bromine

Which statement explains this change?

2

A

Oxygen and bromine gases have equal densities.

B

Oxygen and bromine molecules are in random motion.

C

Oxygen and bromine molecules diffuse at the same rate.

D

Equal volumes of oxygen and bromine contain equal numbers of molecules.

A 50 cm3 sample of alcohol is mixed with 50 cm3 of water. 50 cm3 of alcohol

50 cm3 of water

The volume of the mixed alcohol and water is found to be 97 cm3. Which of the following is the best explanation? A

Alcohol molecules fit into gaps between water molecules.

B

Some alcohol molecules evaporate.

C

Water and alcohol react to form a gas which escapes.

D

Water and alcohol react to produce a salt which then dissolves.

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3 3

The apparatus shown is used to distil a dilute solution of ethanol in water. [B.P. ethanol, 78 °C, water 100 °C]

thermometer

water out

fractionating column water in

boiling flask mixture of ethanol and water heat Which graph shows the change in concentration of the ethanol in the boiling flask as the distillation proceeds. concentration of ethanol

concentration of ethanol

A

B

0

time

concentration of ethanol

0

time

0

time

concentration of ethanol

C

D

0

time

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4 4

What is the formula of uranium(VI) oxide? A

5

6

U6O

B

U2O3

C

UO3

D

UO6

Which of the following describes the structure of diamond? A

a giant structure of atoms bonded covalently

B

a regular arrangement of oppositely charged ions

C

layers of rings of atoms

D

positively charged ions surrounded by a ‘sea of electrons’

Which of the following describes the electrical conductivity of sodium chloride? electrical conductivity

7

when solid

when molten

in aqueous solution

A

no

no

no

B

no

yes

yes

C

yes

no

no

D

yes

yes

yes

One mole of hydrated copper(II) sulphate, CuSO4.5H2O, is dissolved in water. How many moles of ions does the solution contain? A

8

1

B

2

C

6

D

7

Which quantity is the same for one mole of ethanol and one mole of ethane? A

mass

B

number of atoms

C

number of molecules

D

volume at r.t.p.

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5 9

A compound P is the only substance formed when two volumes of ammonia gas react with one volume of carbon dioxide (both volumes being measured at r.t.p.). What is the most likely formula of P? A

(NH4)2CO3

B

NH2CO2NH4

C

(NH2)2CO

D

NH4CO2NH4

10 What is the definition of nucleon (mass) number? A

the mass in grams of an atom

B

the number of electrons in an atom

C

the number of nuclei in a molecule

D

the total number of protons and neutrons in an atom

11 The diagram shows two electrolysis cells, X and Y.

inert cathode

inert anode

copper cathode

copper anode

aqueous copper(II) sulphate cell X

cell Y

What are the changes in mass, if any, of the anodes? cell X

cell Y

A

decrease

decrease

B

decrease

increase

C

increase

no change

D

no change

decrease

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6 12 Rubidium, Rb, is in the same group of the Periodic Table as sodium. Which products are obtained from the electrolysis of concentrated aqueous rubidium chloride? cathode product

solution produced

A

hydrogen

acidic

B

hydrogen

alkaline

C

rubidium

acidic

D

rubidium

alkaline

13 The diagram shows a simple cell in which metals X and Y are the electrodes. voltmeter

electrolyte X

Y

Which pair of metals would be expected to produce the highest voltage? X

Y

A

Cu

Ag

B

Mg

Ag

C

Mg

Zn

D

Zn

Fe

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7 14 The rate of the reaction between a given mass of calcium carbonate and an excess of hydrochloric acid was studied by collecting the carbon dioxide in a graduated syringe. The results are shown in the graph. 100

80

total volume of carbon dioxide/cm3

60

40

20

0

0

1

3

2

4

5

6

time/min How much time was required for half the calcium carbonate to react? A

0.95 min

B

1.5 min

C

2.0 min

D

3.0 min

15 At 400 °C the reaction between hydrogen and iodine reaches an equilibrium. H2(g) + I2(g)

2HI(g)

∆H = –13 kJ/mol

Which change in conditions would increase the percentage of hydrogen iodide in the equilibrium mixture? A

a decrease in pressure

B

a decrease in temperature

C

an increase in pressure

D

an increase in temperature

16 Which reaction is an example of a redox reaction? A

CuO + H2SO4 → CuSO4 + H2O

B

H+ + OH– → H2O

C

Ag+ + Cl – → AgCl

D

2SO2 + O2 → 2SO3

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8 17 Which of the following is a characteristic property of alkalis in aqueous solution? A

They liberate ammonia from ammonium salts.

B

They liberate carbon dioxide from carbonates.

C

They give hydrogen with any metal.

D

They turn Universal Indicator paper red.

18 The formulae of some oxides are shown below. Na2O MgO A l2 O 3 SO2 CO2 Which entry in the table gives the correct number of each type of oxide? number of each type of oxide acidic

amphoteric

basic

A

1

2

2

B

2

0

3

C

1

1

3

D

2

1

2

19 The table shows the solubilities of some lead salts. salt

solubility in water

PbCl2

slightly soluble in cold water, soluble in hot water

PbCO3, PbSO4

insoluble

Pb(NO3)2

soluble

What will be the best method for making a sample of lead(II) chloride? A

Add dilute hydrochloric acid to aqueous lead(II) nitrate, filter.

B

Heat lead(II) sulphate with dilute hydrochloric acid, cool, filter.

C

Heat powdered lead with aqueous sodium chloride, cool, filter.

D

Shake lead(II) carbonate with cold dilute hydrochloric acid, filter.

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9 20 Which element is in Group IV, Period 5 of the Periodic Table? A

antimony

B

arsenic

C

lead

D

tin

21 A metal X forms oxides with the formulae XO and X2O3. Where is X in the Periodic Table? A

in Group II

B

in Group III

C

the second Period

D

in the transition elements

22 Fluorine is the first element in Group VII of the Periodic Table. Which statement about fluorine is not correct? A

It is a gas at room temperature and pressure.

B

Its molecules are monatomic at room temperature.

C

It is a more powerful oxidising agent than chlorine.

D

It forms ionic compounds with metals.

23 Which element is always present with iron in mild steel? A

aluminium

B

carbon

C

chromium

D

nickel

24 Hydrogen gas will reduce A

calcium oxide,

B

silver oxide,

C

magnesium oxide,

D

potassium oxide.

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10 25 Copper(II) oxide is reduced to copper as shown. The burner is then turned off but the hydrogen is kept flowing until the tube is cold. excess hydrogen burning dry hydrogen copper(II) oxide

burner What is the main reason why the hydrogen is kept flowing? A

to lessen the risk of explosion in the hot tube

B

to make certain that the reaction is complete

C

to prevent the copper from reacting with the air

D

to remove any traces of water left in the tube

26 The diagram shows how hydrogen can be manufactured and used. substance X

carbon monoxide heated catalyst

steam

unsaturated vegetable oil

hydrogen

catalyst substance Y

Which substances could be X and Y? X

Y

A

methane

margarine

B

methane

soap

C

ethene

soap

D

ethene

margarine

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11 27 Iron filings are wrapped in a damp cloth and left to rust in the apparatus as shown. Which letter indicates the water level when rusting has finished? iron filings in the damp cloth

cm3

graduated tube 10 20 30 40 50

water level at start

rusty iron filings in damp cloth

cm3

graduated tube 10 20 30 40 50

A B C D

water

28 Farmers use potassium chloride on agricultural land. Why is it used? A

It removes excess acidity in the soil.

B

It kills harmful bacteria in the soil.

C

It provides potassium which is essential for healthy plant growth.

D

It reacts with salts in the soil releasing ammonia.

29 In which pair do both pollutants cause damage to buildings? A

carbon monoxide and lead compounds

B

carbon monoxide and sulphur dioxide

C

lead compounds and nitrogen dioxide

D

nitrogen dioxide and sulphur dioxide

30 Which substances can be obtained from calcium carbonate using only heat and water? A

Ca,

CaO,

Ca(OH)2

B

Ca,

Ca(OH)2

CO2

C

CaO,

Ca(OH)2,

CO2

D

CaO,

CO2,

O2

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12 31 The properties of two varieties of an element are shown in the table. variety 1

variety 2

colourless solid

black solid

hard

soft

cannot conduct electricity

conducts electricity

What do these descriptions of the two varieties indicate? A

They are allotropes of the same element.

B

They are isotopes of the same element.

C

They are isomers of the same substances.

D

They are members of the same homologous series.

32 Graphite is used to make A

glass,

B

cutting tools,

C

electrical wiring,

D

electrodes.

33 A mineral X dissolves in dilute hydrochloric acid, giving off a gas which turns limewater milky. When aqueous ammonia is added to the colourless solution, a white precipitate is formed. The precipitate dissolves in an excess of aqueous ammonia to give a colourless solution. What is X? A

calcium carbonate

B

copper(II) carbonate

C

zinc carbonate

D

zinc sulphide

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13 34 A mixture containing 1 mole of ethene and 4 moles of oxygen is ignited, in a sealed container at 100 °C. The reaction occurring is shown by the equation. C2H4(g) + 3O2(g) → 2CO2(g) + 2H2O(g) What was the total number of moles of gas at the end of the reaction? A

2

B

3

C

4

D

5

35 All the members of a homologous series have the same A

empirical formula,

B

general formula,

C

molecular formula,

D

physical properties.

36 The structural formula of butenedioic acid is shown. O C H

H

H

C

C

O C O

O

H

Which statement about butenedioic acid is not correct? A

It decolourises aqueous bromine.

B

Its aqueous solution reacts with sodium carbonate.

C

Its empirical formula is the same as its molecular formula.

D

Its relative molecular mass is 116.

37 Vinegar is a solution of ethanoic acid made by the reaction of ethanol with air. Which gas in air takes part in this reaction? A

carbon dioxide

B

nitrogen

C

oxygen

D

water vapour

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14 38 ‘The polymer …1… has the same linkages as …2… . It is therefore likely to be …3… by heating with aqueous acids and alkalis.’ Which set of words correctly completes the sentences above? 1

2

3

A

nylon

proteins

unaffected

B

poly(ethene)

carbohydrates

unaffected

C

starch

esters

unaffected

D

Terylene

fats

hydrolysed

39 Poly(carbonates) are synthetic polymers. Their structure can be as shown. O O

C

O O

O

C

O

Which of the following has a type of linkage similar to that of a poly(carbonate)? A

a polyamide

B

a polyester

C

poly(propene)

D

starch

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15 40 A hydrocarbon X reacts in darkness with bromine to form the compound with the formula shown.

H

Br

Br

Br

Br

C

C

C

C

H

H

H

H

H

What is the formula of the hydrocarbon X? A

H

H

H

H

H

C

C

C

C

H

H

H

H

H

B H C

H

H

H

C

C

C

H

H

H

C H

H

H

H

H

C

C

C

C

H

D

H

H

H C H

H

H

H

C

C

H C H

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Magnesium

Sodium

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Strontium

Rubidium

89

Key

b

X

a

†

72

b = proton (atomic) number

X = atomic symbol

a = relative atomic mass

*58-71 Lanthanoid series †90-103 Actinoid series

88

Ac

Actinium

Ra

Radium

Fr

Francium

87

*

Hafnium

Lanthanum

57

178

Hf

40

Zirconium

Zr

91

Titanium

139

Yttrium

22

48

Ti

La

39

Y

89

Scandium

21

227

56

Barium

Caesium

45

Sc

226

55

137

Ba

133

Cs

38

Sr

Rb

37

88

Calcium

85

19

20

40

Ca

39

K

12

24

Mg

23

Na

Beryllium

4

Lithium

Potassium

11

3

9

Be

7

II

Li

I

Ta

181

Niobium

Nb

93

90

58

73

52

Mo

96

W

184

Protactinium

Thorium

55

Tc 186

Re

144

Nd

92

60

Uranium

U

238

Neodymium

75

Rhenium

43

Technetium

25

Manganese

Mn 27

59

28

59

29

64

30

65

5

6

Ru

101

Iron

190

Pm

Osmium

Os

Np 93

Neptunium

61

Promethium

76

44

Ruthenium

26

56

Fe

Sm

150

Iridium

Pu 94

Plutonium

62

152

Eu

Am 95

Americium

63

Europium

78

Platinum

195

Pt

Ir

46

Palladium

Pd

106

Nickel

Ni

192

Samarium

77

45

Rhodium

Rh

103

Cobalt

Co

Gd

157

Gold

Au

197

Silver

96

64

Curium

Cm

Gadolinium

79

47

Ag

108

Copper

Cu

201

Bk

Terbium

Tb

159

Mercury

Hg

97

Berkelium

65

80

48

Cadmium

Cd

112

Zinc

Zn

Dy

162

Thallium

Tl

204

Cf 98

Californium

66

Es

Holmium

Ho

165

Lead

Pb

207

Tin

99

Einsteinium

67

82

50

Sn

In Indium

119

32

Germanium

Ge

73

Silicon

115

Gallium

Dysprosium

81

49

31

70

Ga

14

28

Si

Carbon

27

Aluminium

13

12

C

Al

Boron

B

11

7

75

Sb

122

Arsenic

As

Bi

209

Fermium

Fm

Erbium

Er

167

Bismuth

100

68

83

51

Antimony

33

15

Phosphorus

P

31

Nitrogen

N

14

8

Se

79

Sulphur

Po

169

Md

Thulium

Tm

101

Mendelevium

69

84

Polonium

52

Tellurium

Te

128

Selenium

34

16

S

32

Oxygen

O

16

9

Yb

173

Astatine

At

Iodine

I

127

Bromine

Br

80

Chlorine

No 102

Nobelium

70

Ytterbium

85

53

35

17

Cl

35.5

Fluorine

F

19

2

0

Lr

Lutetium

Lu

175

Radon

Rn

Xenon

Xe

131

Krypton

Kr

84

Argon

Ar

40

Neon

103

Lawrencium

71

86

54

36

18

10

Ne

20

Helium

VII

Hydrogen

VI

4

V

He

IV

H

III 1

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

91

Pa

Th

232

Praseodymium

Cerium

59

141

Pr

140

74

Tungsten

42

Molybdenum

24

Chromium

Cr

Ce

Tantalum

41

23

Vanadium

V

51

1

Group

DATA SHEET The Periodic Table of the Elements

16

17

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