Cambridge IGCSE Science - Combined 0653 — 2003 Oct/Nov Paper 3 · Variant 1

This document consists of 15 printed pages and 1 blank page. SP (KN/KN) S42683/2 © CIE 2003 [Turn over CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education COMBINED SCIENCE 0653/03 Paper 3 October/November 2003 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 on all the work you hand in. Write in dark blue or black pen in the spaces provided on the Question Paper. You may use a soft pencil for any diagrams, graphs or rough working. Do not use staples, paper clips, highlighters, glue or correction fluid. Answer all questions. 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. A copy of the Periodic Table is printed on page 16. Centre Number Candidate Number Name If you have been given a label, look at the details. If any details are incorrect or missing, please fill in your correct details in the space given at the top of this page. Stick your personal label here, if provided. For Examiner’s Use 3 2 1 4 8 7 9 10 TOTAL 6 5 www.XtremePapers.com

2 0653/03/O/N/03 1 (a) Fig. 1.1 shows some information about three enzymes which act in the human digestive system. Fig. 1.1 Complete the table by writing the appropriate word or words in each of the four spaces. [4] (b) Seeds and fruits are important sources of nutrients for many animals, including humans. Many seeds and fruits contain sugar, starch and protein. (i) Explain how the presence of these nutrients can help the seeds or fruits to be dispersed to new areas. … … …[2] (ii) Describe how you would test a seed for the presence of protein, and state what you would see if the test was positive. … … … …[3] For Examiner’s Use enzyme substance which substance which place where the enzyme digests is produced the enzyme works starch sugar (maltose) mouth and small intestine lipase fatty acids and small intestine glycerol protease proteins

3 0653/03/O/N/03 [Turn over 2 (a) Fig. 2.1 shows an observer’s eye looking at a lamp in a mirrror. (i) On Fig. 2.1, draw a ray of light to show how the observer is able to see the lamp in the mirror. [3] Fig. 2.1 (ii) On Fig. 2.1 show the position of the image. [2] (b) Light waves and radio waves are both parts of the electromagnetic spectrum. (i) State one property that is the same for both of these waves. …[1] (ii) State one property that is different for each of these waves. …[1] lamp observer's eye Mirror For Examiner’s Use

4 0653/03/O/N/03 3 Fig. 3.1 shows a blast furnace which is used to extract iron from iron ore. Iron ore is a rock containing iron(III) oxide. Fig. 3.1 (a) (i) Iron ore and coke are added to the furnace at A. Name the other raw material that is added at A. …[1] (ii) Iron(III) oxide is reduced to iron at B. Write a word equation for the reaction at B. …[2] (iii) Explain why iron(III) oxide is said to be reduced in this reaction. …[1] (b) (i) The chemical formula of iron(III) oxide is Fe2O3. The formula of the oxide ion is O2–. Deduce the formula of the iron ion. Show how you obtained your answer. …[2] A B For Examiner’s Use

5 0653/03/O/N/03 [Turn over (ii) Calculate the relative formula mass of iron(III) oxide. Show your working. …[2] For Examiner’s Use

6 0653/03/O/N/03 4 A student investigated the effect of temperature on the transpiration rate of potted plants. She took three similar plants growing in pots, and added the same volume of water to the soil in each pot. Then she fastened a transparent polythene bag around each one. For plants A and B, the bag covered the pot only. For plant C, the bag covered the pot and also the plant, as shown in Fig. 4.1. Plants A and C were left in a room kept at 20°C. Plant B was left in a room kept at 10°C. Fig. 4.1 Each plant was placed on a balance and its mass was recorded at the same time each day for one week. The loss of mass was then calculated. The results are shown in Fig. 4.2. Fig. 4.2 1 2 3 4 5 6 7 0 10 20 30 40 50 total loss of mass/g time/days C A B A 20°C B 10°C C 20°C transparent bag For Examiner’s Use

7 0653/03/O/N/03 [Turn over (a) (i) Suggest one factor which should have been the same in the two rooms, to make sure that the student’s results were valid. …[1] (ii) Explain why the polythene bags needed to be transparent. … … …[2] (b) (i) Explain why plants A and B lost mass, but plant C did not. … … … …[3] (ii) Explain why plant A lost more mass than plant B. … … … …[3] (iii) The conditions in the two rooms were kept constant throughout the experiment. Suggest why plant A lost mass more slowly towards the end of the week. … … …[2] For Examiner’s Use

8 0653/03/O/N/03 5 Liquid water may freeze into solid ice on a cold night but may evaporate into water vapour on a hot day. Explain in terms of particles how water can be found as ice, liquid water or water vapour under these different conditions. You may wish to use diagrams in your answer. Your answer must refer to • the motion of the particles, • the separation of the particles, • the forces between the particles. … … … … … … … …[5] For Examiner’s Use

9 0653/03/O/N/03 [Turn over 6 Most of the compounds in petroleum (crude oil) are hydrocarbons but some sulphur compounds are also present. (a) (i) Write a word equation for the complete combustion of the hydrocarbon, methane. [2] (ii) Explain how sulphur compounds may cause damage to the environment if they are not removed from petroleum. … … … …[3] (b) Some hydrocarbons are cracked to form smaller molecules such as ethene which contains a double bond. Describe how a hydrocarbon is tested to find out whether it contains a double bond. … … …[2] (c) Fig. 6.1 shows the displayed formula of a small part of a molecule of poly(ethene). Fig. 6.1 (i) State the number of ethene monomers which have joined to form this section of the poly(ethene) molecule. …[1] (ii) Explain your answer to (i). … …[1] C H H H H H H H H H H H H H H H H H H H H C C C C C C C C C For Examiner’s Use

10 0653/03/O/N/03 7 Fig. 7.1 shows two beakers A and B, both full of water. Fig. 7.1 (a) (i) When both beakers are full of water, beaker A has twice the weight of beaker B. What can be said about the masses of the two beakers when they are full of water? Explain your answer. … … …[2] (ii) Fig. 7.2 shows the two beakers balanced on a thin beam. Fig. 7.2 What is the value of X? Explain your answer. … … …[2] A B 30cm Xcm A B For Examiner’s Use

11 0653/03/O/N/03 [Turn over (b) Fig. 7.3 shows a conical flask and a drinking glass, both full of water. Fig. 7.3 (i) Label each container with a C to show the approximate centre of mass in each one. [2] (ii) Explain why it is more difficult to tip over the conical flask than the drinking glass. You may draw diagrams if it helps your answer. … … …[2] For Examiner’s Use

12 0653/03/O/N/03 8 If an onion bulb is cut open, it can be seen to be made of several different layers. Each layer has a very thin ‘skin’ covering its inner surface. This skin is called an epidermal tissue. (a) What is the term that is used to describe a structure such as an onion bulb, which is made of several tissues grouped together? …[1] (b) The outline shows the shape of a plant cell in the epidermal tissue of an onion bulb. (i) In the space below, draw a diagram to show how at least six of these cells are grouped together to form the epidermal tissue. [3] (ii) State one way in which a cell in onion epidermal tissue differs from a cell in the palisade mesophyll of a leaf. Explain the reason for this difference. difference … … reason for this difference … … …[3] For Examiner’s Use

13 0653/03/O/N/03 [Turn over 9 The pH values of three acidic solutions are shown below. vinegar 4 lemon juice 3 battery acid 1 (a) The formula of the ion present in all acids is H+. (i) Which of the solutions shown above contains the highest concentration of this ion? …[1] (ii) Write an ionic equation which describes the neutralisation of any acid by any alkali. …[2] (b) When sodium carbonate is added to dilute hydrochloric acid, there is a vigorous reaction in which the acid is neutralised and a gas is given off. Complete the word equation for this reaction. [3] (c) Copper(II) oxide is an insoluble base. Describe how crystals of copper(II) sulphate could be made from copper(II) oxide and dilute sulphuric acid. … … … … … …[4] For Examiner’s Use hydrochloric acid sodium carbonate + + +

14 0653/03/O/N/03 10 Radon is a gas that emits alpha radiation. (a) Explain why alpha radiation is dangerous to human beings. … … …[2] (b) Explain why alpha radiation is affected by an electric field. … … …[2] (c) Describe the differences in the structure of the nucleus of a radon-220 atom before and after the emission of an alpha particle. … … …[2] For Examiner’s Use

16 0653/03/O/N/03 Group DATA SHEET The Periodic Table of the Elements 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 I II III IV V VI VII 0 85 Rb Rubidium 37 133 Cs Caesium 55 226 Ra Radium 88 The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.). a X b a = relative atomic mass X = atomic symbol b = proton (atomic) number Key *58-71 Lanthanoid series †90-103 Actinoid series