Cambridge O Level: Chemistry 5070/11
Cambridge O Level: Chemistry 5070/11
Cambridge O Level: Chemistry 5070/11
CHEMISTRY 5070/11
Paper 1 Multiple Choice May/June 2021
1 hour
INSTRUCTIONS
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 multiple choice answer sheet.
Follow the instructions on the multiple choice answer sheet.
Write in soft pencil.
Write your name, centre number and candidate number on the multiple choice answer sheet in the
spaces provided unless this has been done for you.
Do not use correction fluid.
Do not write on any bar codes.
You may use a calculator.
INFORMATION
The total mark for this paper is 40.
Each correct answer will score one mark.
Any rough working should be done on this question paper.
The Periodic Table is printed in the question paper.
IB21 06_5070_11/4RP
© UCLES 2021 [Turn over
2
A B C D
2 Which property of a liquid ester can be used to check its purity before use as a food flavouring?
A boiling point
B colour
C smell
D solubility in water
4 J is an aqueous solution.
Aluminium foil is added to the warmed mixture. A gas is formed that turns damp red litmus paper
blue.
1 colourless
2 no effect on either damp red or blue litmus papers
3 no effect on limewater
4 flammable
What is gas X?
A ammonia
B chlorine
C hydrogen
D oxygen
P Q
A P only P only
B P only Q only
C both P and Q P only
D both P and Q Q only
9 The empirical formula of compound X is CH2 and the relative molecular mass, Mr, of X is 70.
10 A chemist wants to make calcium nitrate. They start with 8.00 g of pure calcium oxide and an
excess of dilute nitric acid. They produce 12.65 g of pure, dry anhydrous calcium nitrate crystals.
relative
compound
formula mass
A Al 2O3 102
B CuO 80
C H2SO4 98
D HNO3 63
A 2 B 4 C 10 D 15
13 An aqueous mixture of copper(II) nitrate and silver nitrate is electrolysed with pure copper
electrodes.
A Cu Cu2+ + 2e–
B Cu2+ + 2e– Cu
C Ag Ag+ + e–
D Ag+ + e– Ag
14 The diagram shows the electrolysis of concentrated and dilute aqueous sodium chloride using
inert electrodes. Gases are produced and collected in each of the test-tubes W, X, Y and Z.
W X Y Z
concentrated dilute
aqueous aqueous
sodium chloride sodium chloride
17 Ethanol is produced by the fermentation of glucose from sugar cane. In some countries ethanol is
used as a fuel.
A 1 only
B 2 only
C both 1 and 2
D neither 1 nor 2
experiment 1 24.0 g of powdered magnesium is reacted with 100 cm3 of 1.0 mol / dm3
sulfuric acid.
experiment 2 24.0 g of powdered magnesium is reacted with 50 cm3 of 2.0 mol / dm3
sulfuric acid.
During each experiment the volume of hydrogen produced is measured. The results are plotted
on a graph.
A B
0 0
0 time 0 time
C D
volume of volume of
hydrogen hydrogen
produced produced
0 0
0 time 0 time
oxidation
1 CH4 + 2O2 o CO2 + 2H2O
reduction
2 2H2S + SO2 o 3S + 2H2O
reduction
3 BrO3– + 5Br – + 6H+ o 3Br2 + 3H2O
22 Which row shows the pH values for 0.1 mol / dm3 solutions of ammonia, hydrochloric acid,
sodium chloride and sodium hydroxide?
pH values
NH3 HCl NaCl NaOH
A 1 7 13 11
B 7 1 11 13
C 11 1 7 13
D 13 11 7 1
23 The water in a lake is acidic and the fish are dying. The water in the lake needs to be neutralised.
Which compound can be added in excess to neutralise the water in the lake?
A calcium carbonate
B phosphoric acid
C potassium hydroxide
D sodium nitrate
24 Two incomplete statements about the preparation of an insoluble salt are given.
1 2 3 4
25 The Haber process is used to make ammonia at a temperature of 400 C and a pressure of
20 000 kPa. The temperature is changed to 500 C but the pressure is kept the same.
A It is made at an increased rate and the position of the equilibrium moves to the left.
B It is made at an increased rate and the position of the equilibrium moves to the right.
C It is made at a decreased rate and the position of the equilibrium moves to the left.
D It is made at a decreased rate and the position of the equilibrium moves to the right.
1 metallic character
2 number of electron shells in an atom
3 number of protons in an atom
4 total number of electrons in an atom
28 The elements in Group I of the Periodic Table show trends in both their reactivities and their
melting points. Rubidium is in Group I.
Student X suggests that the Group I elements are above hydrogen in the metal reactivity series
but that not all transition elements are.
Student Y suggests that the densities of Group I elements are lower than those of the transition
elements.
A both X and Y
B X only
C Y only
D neither X nor Y
31 Tin is more reactive than lead but less reactive than iron.
Which method would be most suitable for extracting tin from its ore?
A electrolysis
B heating alone
C heating with carbon
D reacting with hydrogen
32 Attaching pieces of magnesium to underground iron pipes can protect the iron from corrosion.
33 Which reactions take place during the extraction of aluminium from aluminium oxide using carbon
electrodes?
1 2O2– O2 + 4e–
2 C + O2 CO2
3 Al 2+ + 2e– Al
35 How many moles of hydrogen chloride are formed when one mole of methane reacts with a large
excess of chlorine in sunlight?
A 1 B 2 C 3 D 4
H H
C C C H
H H H
A It is a saturated hydrocarbon.
B It is an isomer of butene.
C It will decolourise bromine water.
D Its name is propane.
X Y
H H H H H H H H
H C C C C H H C C C C H
H O H H H H H O
H H
40 X is a polymer.
NH2
CH3 C COOH
H
Y
A a complex carbohydrate
B a fat
C a protein
D an addition polymer
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© UCLES 2021
I II III IV V VI VII VIII
1 2
H He
hydrogen helium
Key 1 4
3 4 atomic number 5 6 7 8 9 10
Li Be atomic symbol B C N O F Ne
lithium beryllium name boron carbon nitrogen oxygen fluorine neon
7 9 relative atomic mass 11 12 14 16 19 20
11 12 13 14 15 16 17 18
Na Mg Al Si P S Cl Ar
sodium magnesium aluminium silicon phosphorus sulfur chlorine argon
23 24 27 28 31 32 35.5 40
19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36
K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
potassium calcium scandium titanium vanadium chromium manganese iron cobalt nickel copper zinc gallium germanium arsenic selenium bromine krypton
39 40 45 48 51 52 55 56 59 59 64 65 70 73 75 79 80 84
37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54
Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe
rubidium strontium yttrium zirconium niobium molybdenum technetium ruthenium rhodium palladium silver cadmium indium tin antimony tellurium iodine xenon
16
85 88 89 91 93 96 – 101 103 106 108 112 115 119 122 128 127 131
55 56 57–71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86
5070/11/M/J/21
lanthanoids
Cs Ba Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
caesium barium hafnium tantalum tungsten rhenium osmium iridium platinum gold mercury thallium lead bismuth polonium astatine radon
133 137 178 181 184 186 190 192 195 197 201 204 207 209 – – –
87 88 89–103 104 105 106 107 108 109 110 111 112 114 116
actinoids
Fr Ra Rf Db Sg Bh Hs Mt Ds Rg Cn Fl Lv
francium radium rutherfordium dubnium seaborgium bohrium hassium meitnerium darmstadtium roentgenium copernicium flerovium livermorium
– – – – – – – – – – – – –
57 58 59 60 61 62 63 64 65 66 67 68 69 70 71
lanthanoids La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
lanthanum cerium praseodymium neodymium promethium samarium europium gadolinium terbium dysprosium holmium erbium thulium ytterbium lutetium
139 140 141 144 – 150 152 157 159 163 165 167 169 173 175
89 90 91 92 93 94 95 96 97 98 99 100 101 102 103
actinoids Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
actinium thorium protactinium uranium neptunium plutonium americium curium berkelium californium einsteinium fermium mendelevium nobelium lawrencium
– 232 231 238 – – – – – – – – – – –
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).