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0620 w08 qp_2
1.
This document consists
of 16 printed pages. IB08 11_0620_02/6RP © UCLES 2008 [Turn over *0269167397* For Examiner's Use 1 2 3 4 5 6 7 Total UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education CHEMISTRY 0620/02 Paper 2 October/November 2008 1 hour 15 minutes Candidates answer on the Question Paper. No Additional Materials are required. READ THESE INSTRUCTIONS FIRST Write your Centre number, candidate number and name in the spaces at the top of this page. Write in dark blue or black pen. You may need to use a pencil for any diagrams, graphs or rough working. Do not use staples, paper clips, highlighters, glue or correction fluid. DO NOT WRITE IN ANY BARCODES. Answer all questions. A copy of the periodic table is printed on page 16. 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. w w w .Xtrem ePapers.com
2.
2 © UCLES 2008
0620/02/O/N/08 For Examiner's Use 1 (a) The table gives some information about five elements, A, B, C, D and E. Complete the table by writing either metal or non-metal in the last column. element properties metal or non-metal A shiny solid which conducts electricity B reddish brown liquid with a low boiling point C a form of carbon which is black in colour and conducts electricity D white solid which is an insulator and has a high melting point E dull yellow solid which does not conduct heat [5] (b) Describe how metallic character changes across a Period. [1] (c) Sodium is in Group I of the Periodic Table. (i) Draw a diagram to show the full electronic structure of sodium. [1] (ii) Complete the equation to show what happens when a sodium atom forms a sodium ion. Na Na+ + [1]
3.
3 © UCLES 2008
0620/02/O/N/08 [Turn over For Examiner's Use (d) Complete these sentences about the properties of the Group I elements using words from the list. acidic basic decrease hard increase lithium potassium soft The Group I elements are relatively metals which in reactivity going down the Group. Sodium reacts more violently with water than . The Group I metals all form oxides. [4] [Total: 12]
4.
4 © UCLES 2008
0620/02/O/N/08 For Examiner's Use 2 (a) Match up the atmospheric pollutants on the left with their main source on the right. The first one has been done for you. chlorofluorocarbons car exhausts sulphur dioxide aerosol sprays carbon monoxide combustion of fossil fuels containing sulphur nitrogen oxides incomplete combustion of fossil fuels [3] (b) One stage in the manufacture of sulphuric acid involves the oxidation of sulphur dioxide by oxygen in the air to form sulphur trioxide. 2SO2 + O2 2SO3 (i) Explain how this reaction shows that sulphur dioxide is oxidized. [1] (ii) What is the percentage of oxygen in clean air? [1] (iii) Sulphuric acid is used to make the fertiliser ammonium sulphate. ammonia + sulphuric acid ammonium sulphate What type of reaction is this? [1]
5.
5 © UCLES 2008
0620/02/O/N/08 [Turn over For Examiner's Use (iv) Why do farmers need to use fertilisers? [2] (v) Another fertiliser can be made by the reaction of ammonia with nitric acid. State the chemical name of this fertiliser. [1] [Total: 9]
6.
6 © UCLES 2008
0620/02/O/N/08 For Examiner's Use 3 Calcium carbonate, CaCO3, is the raw material used in the manufacture of lime, CaO. (a) (i) Describe how lime is manufactured from calcium carbonate. [1] (ii) Write a symbol equation for this reaction. [1] (iii) State one large scale use of lime. [1] (b) A student investigated the speed of reaction of calcium carbonate with hydrochloric acid using the apparatus shown below. (i) Complete the labelling of the apparatus by filling in the three boxes. [3] reaction mixture water bath at 40°C (ii) The equation for the reaction is CaCO3 + 2HCl CaCl2 + CO2 + H2O Write the word equation for this reaction. [2]
7.
7 © UCLES 2008
0620/02/O/N/08 [Turn over For Examiner's Use (iii) The student carried out the reaction at 40°C using large pieces of calcium carbonate. The results of the experiment are shown below. 80 60 40 20 0 0 20 40 60 80 100 120 140 160 time/seconds cm3 gasreleased 100 At what time did the reaction stop? [1] (iv) The student repeated the experiment using the same mass of powdered calcium carbonate. All other conditions were kept the same. On the grid above, sketch the graph for the reaction with calcium carbonate powder. [2] (v) How does the speed of reaction change when the concentration of hydrochloric acid is decreased, the temperature is increased? [2] [Total: 13]
8.
8 © UCLES 2008
0620/02/O/N/08 For Examiner's Use 4 Iron is extracted from its ore in a blast furnace. (a) State the name of the ore from which iron is extracted. [1] (b) The diagram shows a blast furnace. A B C D coke + limestone + iron ore firebrick lining air in (i) Which one of the raw materials is added to the blast furnace to help remove the impurities from the iron ore? [1] (ii) The impurities are removed as a slag. Which letter on the diagram shows the slag? [1] (c) Carbon monoxide is formed in the blast furnace by reaction of coke with oxygen. (i) Complete the equation for this reaction. C + CO [2] (ii) State the adverse affect of carbon monoxide on human health. [1]
9.
9 © UCLES 2008
0620/02/O/N/08 [Turn over For Examiner's Use (d) In the hottest regions of the blast furnace the following reaction takes place. Fe2O3 + 3C 2Fe + 3CO Which two of these sentences correctly describe this reaction? Tick two boxes. The iron oxide gets reduced. The reaction is a thermal decomposition. The carbon gets oxidised. The carbon gets reduced. Carbon neutralises the iron oxide. [1] (e) Aluminium cannot be extracted from aluminium oxide in a blast furnace. Explain why aluminium cannot be extracted in this way. [2] (f) (i) State the name of the method used to extract aluminium from its oxide ore. [1] (ii) State one use of aluminium. [1] [Total: 11]
10.
10 © UCLES 2008
0620/02/O/N/08 For Examiner's Use 5 The apparatus shown below can be used to measure the energy released when a liquid fuel is burnt. The amount of energy released is calculated from the increase in temperature of a known amount of water. iron can water ethanol (a) (i) Explain how this experiment shows that the burning of ethanol is an exothermic reaction. [1] (ii) Complete the word equation for the complete combustion of ethanol. ethanol + oxygen + [2] (b) Ethanol is a fuel containing carbon. State the names of two other commonly used fuels containing carbon. and [2] (c) Give the formula of the functional group present in ethanol. [1] (d) The can contains water. Describe a chemical test for water. test result [2]
11.
11 © UCLES 2008
0620/02/O/N/08 [Turn over For Examiner's Use (e) The iron can used in this experiment rusts easily. (i) Describe a method which can be used to prevent iron from rusting. [1] (ii) Rust contains hydrated iron(III) oxide. What do you understand by the term hydrated? [1] (iii) Iron is a transition metal. State two properties which are typical of transition metals. [2] [Total: 12]
12.
12 © UCLES 2008
0620/02/O/N/08 For Examiner's Use 6 The compound shown below is the first member of the alkane homologous series. H H C HH (a) State two characteristics of a homologous series. [2] (b) Name and draw the structure of the next member of the alkane homologous series. name structure [2] (c) Complete the table to show the structure and uses of some organic compounds. name of compound molecular formula structure (showing all atoms and bonds) use ethene C2H4 ethanoic acid C2H4O2 making esters dibromoethane Br H C CH Br H H CH4 H H C HH [6]
13.
13 © UCLES 2008
0620/02/O/N/08 [Turn over For Examiner's Use (d) Calculate the relative molecular mass of dibromoethane. [1] [Total: 11]
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0620/02/O/N/08 For Examiner's Use 7 The diagram shows the structures of calcium chloride, calcium and chlorine. Ca Ca Ca Ca Ca Ca Ca Ca Ca Ca Ca Ca2+ Cl– Cl– Ca2+ Cl– Cl– Ca2+ Cl– Cl– Ca2+ Cl– Cl– Cl Cl Cl Cl Cl Cl Cl Cl calcium chloride calcium chlorine (a) Use ideas about structure and bonding to explain the following: (i) Calcium chloride conducts electricity when molten but not when solid. [2] (ii) At room temperature, calcium is a solid but chlorine is a gas. [2]
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0620/02/O/N/08 For Examiner's Use (b) Calcium is manufactured by the electrolysis of molten calcium chloride. calcium – + molten calcium chloride water-cooled steel cathode (i) State the products formed at the anode, at the cathode. [2] (ii) Suggest a non-metal that can be used as an anode in this electrolysis. [1] (iii) A stream of inert gas is blown over the calcium as it is removed from the molten calcium chloride. Suggest why a stream of inert gas is blown over the hot calcium. [1] (iv) State the name of a gas which is inert. [1] (c) Aqueous sodium hydroxide or aqueous ammonia can be used to test for calcium ions in solution. Describe the results of these tests with aqueous sodium hydroxide, [2] with aqueous ammonia. [1] [Total: 12]
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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. © UCLES 2008 0620/02/O/N/08 Group 140 Ce Cerium 58 141 Pr Praseodymium 59 144 Nd Neodymium 60 Pm Promethium 61 150 Sm Samarium 62 152 Eu Europium 63 157 Gd Gadolinium 64 159 Tb Terbium 65 162 Dy Dysprosium 66 165 Ho Holmium 67 167 Er Erbium 68 169 Tm Thulium 69 173 Yb Ytterbium 70 175 Lu Lutetium 71 232 Th Thorium 90 Pa Protactinium 91 238 U Uranium 92 Np Neptunium 93 Pu Plutonium 94 Am Americium 95 Cm Curium 96 Bk Berkelium 97 Cf Californium 98 Es Einsteinium 99 Fm Fermium 100 Md Mendelevium 101 No Nobelium 102 Lr Lawrencium 103 1 H Hydrogen 1 7 Li Lithium 3 23 Na Sodium 11 24 Mg Magnesium 12 40 Ca Calcium 20 45 Sc Scandium 21 48 Ti Titanium 22 51 V Vanadium 23 52 Cr Chromium 24 55 Mn Manganese 25 56 Fe Iron 26 59 Co Cobalt 27 59 Ni Nickel 28 64 Cu Copper 29 65 Zn Zinc 30 70 Ga Gallium 31 27 Al Aluminium 13 11 B Boron 5 12 C Carbon 6 14 N Nitrogen 7 16 O Oxygen 8 19 F Fluorine 9 28 Si Silicon 14 31 P Phosphorus 15 32 S Sulphur 16 35.5 Cl Chlorine 17 40 Ar Argon 18 20 Ne Neon 10 4 He Helium 2 73 Ge Germanium 32 75 As Arsenic 33 79 Se Selenium 34 80 Br Bromine 35 84 Kr Krypton 36 39 K Potassium 19 88 Sr Strontium 38 89 Y Yttrium 39 91 Zr Zirconium 40 93 Nb Niobium 41 96 Mo Molybdenum 42 Tc Technetium 43 101 Ru Ruthenium 44 103 Rh Rhodium 45 106 Pd Palladium 46 108 Ag Silver 47 112 Cd Cadmium 48 115 In Indium 49 119 Sn Tin 50 122 Sb Antimony 51 128 Te Tellurium 52 127 I Iodine 53 131 Xe Xenon 54 137 Ba Barium 56 139 La Lanthanum 57* 178 Hf Hafnium 72 181 Ta Tantalum 73 184 W Tungsten 74 186 Re Rhenium 75 190 Os Osmium 76 192 Ir Iridium 77 195 Pt Platinum 78 197 Au Gold 79 201 Hg Mercury 80 204 Tl Thallium 81 207 Pb Lead 82 209 Bi Bismuth 83 Po Polonium 84 At Astatine 85 Rn Radon 86 Fr Francium 87 227 Ac Actinium 89 9 Be Beryllium 4 IIIIIIIVVVIVII0 85 Rb Rubidium 37 133 Cs Caesium 55 226 Ra Radium 88 Thevolumeofonemoleofanygasis24dm3atroomtemperatureandpressure(r.t.p.). a X b a=relativeatomicmass X=atomicsymbol b=proton(atomic)number Key *58-71Lanthanoidseries 90-103Actinoidseries DATASHEET ThePeriodicTableoftheElements
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