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UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Ordinary Level

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5070/11

CHEMISTRY Paper 1 Multiple Choice Additional Materials: Multiple Choice Answer Sheet Soft clean eraser Soft pencil (type B or HB recommended)

October/November 2011 1 hour

*0909424295*

READ THESE INSTRUCTIONS FIRST Write in soft pencil. Do not use staples, paper clips, highlighters, glue or correction fluid. Write your name, Centre number and candidate number on the Answer Sheet in the spaces provided unless this has been done for you. 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 12.

This document consists of 12 printed pages.
IB11 11_5070_11/2RP © UCLES 2011

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2 1 In a titration between an acid (in the burette) and an alkali, you may need to re-use the same titration flask. Which is the best procedure for rinsing the flask? A B C D 2 Rinse with distilled water and then with the alkali. Rinse with tap water and then with distilled water. Rinse with tap water and then with the acid. Rinse with the alkali.

The labels fell off two bottles each containing a colourless solution, one of which was sodium carbonate solution and the other was sodium chloride solution. The addition of which solution to a sample from each bottle would most readily enable the bottles to be correctly relabelled? A B C D ammonia hydrochloric acid lead(II) nitrate sodium hydroxide

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3 3 Oxygen was prepared from hydrogen peroxide, with manganese(IV) oxide as catalyst. The oxygen was collected as shown in the diagram. 2H2O2 → 2H2O + O2

aqueous hydrogen peroxide

oxygen

water

manganese(IV) oxide
The first few tubes of gas were rejected because the gas was contaminated by A B C D 4 hydrogen. hydrogen peroxide. nitrogen. water vapour.

Radium (Ra) is in the same group of the Periodic Table as magnesium. What is the charge on a radium ion? A 2– B 1– C 1+ D 2+

5

How many of the molecules shown contain only one covalent bond? Cl 2 A 2 B 3 H2 HCl C 4 N2 D O2 5

6

In which pair is each substance a mixture? A B C D air and water limewater and water quicklime and limewater sea water and air

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4 7 A researcher notices that atoms of an element are releasing energy. Why are the atoms releasing energy? A B C D 8 The atoms are absorbing light. The atoms are evaporating. The atoms are radioactive. The atoms react with argon in the air.

What happens when sodium chloride melts? A B C D Covalent bonds in a giant lattice are broken. Electrons are released from atoms. Electrostatic forces of attraction between ions are overcome. Molecules are separated into ions.

9

Which compound contains three elements? A B C D aluminium chloride iron(III) oxide potassium oxide sodium carbonate

10 Below are two statements about metals. 1 2 Metals contain a lattice of negative ions in a ‘sea of electrons’. The electrical conductivity of metals is related to the mobility of the electrons in the structure.

Which is correct? A B C D Both statements are correct and statement 1 explains statement 2. Both statements are correct but statement 1 does not explain statement 2. Statement 1 is correct and statement 2 is incorrect. Statement 2 is correct and statement 1 is incorrect.

11 What is the ratio of the number of molecules in 71 g of gaseous chlorine to the number of molecules in 2 g of gaseous hydrogen? [Relative atomic masses Ar (atomic weights): H, 1: Cl, 35.5] A 1:1 B 1:2 C 2:1 D 71 : 2

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5 12 What is the relative molecular mass Mr of CuSO4.5H2O? A 160 B 178 C 186 D 250

13 How can sodium be manufactured? A B C D by electrolysing aqueous sodium chloride by electrolysing aqueous sodium hydroxide by electrolysing molten sodium chloride by heating sodium oxide with carbon

14 Which statement about the electrolysis of an aqueous solution of copper(II) sulfate with platinum electrodes is correct? A B C D Oxygen is given off at the positive electrode. The mass of the negative electrode remains constant. The mass of the positive electrode decreases. There is no change in the colour of the solution.

15 Which pair of statements about the combustion of a carbohydrate and its formation by photosynthesis is not correct? combustion A B C D chemical energy converted to heat energy no catalyst needed oxygen used up reaction exothermic photosynthesis chemical energy converted to light energy catalyst needed oxygen released reaction endothermic

16 The following reversible reaction takes place in a closed vessel at constant temperature. P(g) + Q(g) + R(g) S(g) + T(g)

When the system has reached equilibrium, more T is added. Which increases in concentration occur? A B C D P, Q, R and S P and Q only P, Q and R only S only

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6 17 Sulfur dioxide reacts with aqueous bromine according to the following equation. SO2(g) + Br2(aq) + 2H2O(l) → H2SO4(aq) + 2HBr(aq) Which element has been oxidised? A B C D bromine hydrogen oxygen sulfur

18 An excess of calcium hydroxide is added to an acidic soil. What happens to the pH of the soil? change in pH A B C D decrease decrease increase increase final pH 5 7 7 10

19 Which substance would not be used for preparing a pure sample of crystalline magnesium sulfate by reaction with dilute sulfuric acid? A B C D magnesium carbonate magnesium hydroxide magnesium nitrate magnesium oxide

20 Ammonium sulfate and potassium sulfate are salts which can be found in fertilisers. A sample of a fertiliser is warmed with aqueous sodium hydroxide and a gas with pH10 is given off. Which salt must be in the fertiliser and which gas is given off? salt in fertiliser A B C D ammonium sulfate ammonium sulfate potassium sulfate potassium sulfate name of gas ammonia sulfur dioxide ammonia sulfur dioxide

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7 21 The table gives the formulae of the catalysts used in some industrial processes. process Haber process Contact process cracking of alkanes polymerisation of ethene manufacture of silicones catalyst Fe + Mo V2O5 Al 2O3 + SiO2 Al (C2H5)3 + TiCl 4 CuCl

How many different transition metals are included, as elements or as compounds, in the list of catalysts? A 3 B 4 C 5 D 6

22 A lump of element X can be cut by a knife. During its reaction with water, X floats and melts. What is X? A B C D calcium copper magnesium potassium

23 Which statement about the elements chlorine, bromine and iodine is correct? A B C D They are all gases at room temperature and pressure. They are in the same period of the Periodic Table. They become darker in colour from chlorine to bromine to iodine. They possess one electron in the outermost shell.

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8 24 The diagram shows steel wool inside a test-tube. The test-tube is inverted in water, trapping air inside. What will be the water level inside the tube after several days?

steel wool air A

B C D

water level at beginning of experiment

25 Which carbonate decomposes on heating to give a black solid and a colourless gas? A B C D calcium carbonate copper(II) carbonate sodium carbonate zinc carbonate

26 Iron is manufactured in the blast furnace. Which statement about iron and its manufacture is not true? A B C D Iron ore is readily abundant. It is a continuous process. Pure iron is produced. The reducing agent is cheap.

27 Which row shows the three metals in the correct order of decreasing reactivity? most active A B C D copper iron iron zinc zinc copper zinc iron least active iron zinc copper copper

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9 28 Which gas cannot be removed from the exhaust gases of a petrol-powered car by its catalytic converter? A B C D carbon dioxide carbon monoxide hydrocarbons nitrogen dioxide

29 Which equation shows a reaction that would actually take place? A B C D 2MgO + C → CO2 + Mg MgO + Cu → CuO + Mg PbO + Zn → ZnO + Pb ZnO + H2 → H2O + Zn

30 Which statement shows that diamond and graphite are different forms of the element carbon? A B C D Both have giant molecular structures. Complete combustion of equal masses of each produces equal masses of carbon dioxide as the only product. Graphite conducts electricity, whereas diamond does not. Under suitable conditions, graphite can be converted into diamond.

31 What is the purpose of vanadium(V) oxide in the Contact Process? A B C D It oxidises sulfur to sulfur dioxide. It oxidises sulfur to sulfur trioxide. It speeds up the conversion of sulfur dioxide into sulfur trioxide. It speeds up the conversion of sulfur trioxide into sulfuric acid.

32 A sample of tap water gave a white precipitate with acidified silver nitrate. What does this show about the tap water? A B C D It contained chloride. It contained harmful microbes. It contained nitrates. It had not been filtered.

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10 33 Which noble gas is present in the largest percentage by volume in air? A B C D argon helium krypton neon

34 A hydride is a compound containing only two elements, one of which is hydrogen. Which element forms the most hydrides? A B C D carbon chlorine nitrogen oxygen

35 The structural formulae of some organic compounds are shown below.
H H H C H H C H 1 H H C H H 2 O H H O H C C C H H H

H H O C H

H C H 3

H C H O H H

H C H

H C H 4

O C O H

Which compounds are alcohols? A 1, 2, 3 and 4 B 1 and 2 only C 1, 2 and 3 only D 4 only

36 Which compound is manufactured by reacting ethene with steam in the presence of a heated catalyst? A C2H6 B C2H5OH C C4H8 D C4H9OH

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11 37 A hydrocarbon, C3Hy, burns in air to form carbon dioxide and water. C3Hy(g) + 5O2(g) → 3CO2(g) + What is the value of y? A 4 B 6 C 7 D 8

y H2O(g) 2

38 Which pair of macromolecules both contain the linkage shown?

O C N H
A B C D fats and proteins nylon and proteins starch and sugars Terylene and sugars

39 Under certain conditions 1 mole of ethane reacts with 2 moles of chlorine in a substitution reaction. What is the formula of the organic product in this reaction? A C2H5Cl B C2H4Cl 2 C C2H2Cl 4 D CH2Cl 2

40 Shown below are some properties of compound X. ● ● ● What is X? A B C D ethanol ethanoic acid ethyl ethanoate ethyl methanoate reacts with potassium carbonate to produce carbon dioxide reacts with ethanol to produce a sweet-smelling liquid reacts with sodium hydroxide to produce a salt

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© UCLES 2011

DATA SHEET The Periodic Table of the Elements
Group III
1

I H
Hydrogen

II

IV

V

VI

VII

0
4

He
Helium

1 11 12 14 16 19

2 20

7

9

Li
Boron Carbon

Be
5 27 28 6 7

B

C

N
Nitrogen

O
Oxygen

F
Fluorine

Ne
Neon

Lithium

Beryllium

3

4

8 31 32

9 35.5

10 40

23

24

Na
Aluminium

Mg
13 51 52 55 56 59 59 64 65 70

Al
14

Si
Silicon

P
Phosphorus

S
Sulfur

Cl
Chlorine

Ar
Argon

Sodium

Magnesium

11

12

15 73 75

16 79

17 80

18 84

39

40

45

48

K
Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc

Ca
23 93 96 101 103 106 108 112 24 25 26 27 28 29 30

Sc

Ti

V

Cr

Mn

Fe

Co

Ni

Cu

Zn
31

Ga
Gallium

Ge
Germanium

As
Arsenic

Se
Selenium

Br
Bromine

Kr
Krypton

Potassium

Calcium

Scandium

Titanium

19

20

21

22

32 115 119

33 122

34 128

35 127

36 131

12

85

88

89

91

Rb
Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver

Sr
41 181 195 184 186 190 192 197 42 43 44 45 46 47

Y

Zr

Nb

Mo

Tc

Ru

Rh

Pd

Ag
48

Cd
Cadmium

In
Indium

Sn
Tin

Sb
Antimony

Te
Tellurium

I
Iodine

Xe
Xenon

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.

University of Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.
49 201 204 50 207 51 209 52 53 54

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Rubidium

Strontium

Yttrium

Zirconium

37

38

39

40

133

137

139

178

Cs
Tantalum Iridium Tungsten Rhenium Osmium Platinum

Ba
73 77 74 75 76 78

La Ta W Re Os Pt

Hf

Ir
79

Au
Gold

Hg
Mercury

Tl
Thallium

Pb
Lead

Bi
Bismuth

Po
Polonium

At
Astatine

Rn
Radon

Caesium

Barium

Lanthanum

Hafnium

55

56

57

*

72

80

81

82

83

84

85

86

226

227

Fr
140 141 144 150

Ra

Ac
152 157 159 162 165 167 169 173 175

Francium

Radium

Actinium

87

88

89

*58-71 Lanthanoid series 90-103 Actinoid series Ce
Cerium Praseodymium Neodymium Promethium

Pr
59 60 238 61

Nd

Pm
62

Sm
Samarium

Eu
Europium

Gd
Gadolinium

Tb
Terbium

Dy
Dysprosium

Ho
Holmium

Er
Erbium

Tm
Thulium

Yb
Ytterbium

Lu
Lutetium

58 232

63

64

65

66

67

68

69

70

71

a

a = relative atomic mass

Key Th
Thorium Protactinium Uranium

X Pa
91 92

X = atomic symbol
90

U
93

Np
Neptunium

Pu
Plutonium

Am
Americium

Cm
Curium

Bk
Berkelium

Cf
Californium

Es
Einsteinium

Fm
Fermium

Md
Mendelevium

No
Nobelium

Lr
Lawrencium

b

b = proton (atomic) number

94

95

96

97

98

99

100

101

102

103

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