Cambridge IGCSE Physical Science 0652 — 2005 Oct/Nov Paper 3 · Variant 1

Centre Number Candidate Number Name UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education PHYSICAL SCIENCE 0652/03 Paper 3 October/November 2005 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 pencil for any diagrams, graphs, tables or rough working. Do not use staples, paper clips, highlighters, glue or correction fluid. Answer all questions. 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. For Examiner’s Use 1 2 3 4 5 6 7 8 9 10 Total This document consists of 14 printed pages and 2 blank pages. IB05 11_0652_03/3RP  UCLES 2005 [Turn over 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. www.XtremePapers.com

2 © UCLES 2005 0652/03/O/N/05 For Examiner's Use 1 Fig. 1.1 shows the arrangement of electrons in a lithium atom. e e e e = electron Fig. 1.1 (a) Lithium and potassium are both Group I metals. Complete the diagram in Fig. 1.2 to show the arrangement of electrons in a potassium atom. e e e = electron Fig. 1.2 [2] (b) When a small piece of lithium is dropped into a trough half filled with water a reaction takes place. Bubbles of the gas hydrogen are given off slowly and lithium hydroxide is formed. (i) Write a balanced equation for this reaction. [2] (ii) Describe how you could prove that the gas given off is hydrogen. test result [2]

3 © UCLES 2005 0652/03/O/N/05 [Turn over For Examiner's Use (c) A small piece of potassium is dropped into a trough half filled with water. Describe two differences that you would see between the reaction of lithium with water and that of potassium with water. 1. 2. [2] 2 A ray of light enters a rectangular glass block at an angle of incidence of 66o. The glass has a refractive index of 1.45. (a) Calculate the angle of refraction for this ray of light. Write down the equation that you use and show all your working. [3] (b) Draw a fully labelled diagram to show the refraction of the light as it enters and leaves the glass block. [3]

4 © UCLES 2005 0652/03/O/N/05 For Examiner's Use 3 Copper(II) oxide reacts with dilute sulphuric acid. CuO + H2SO4 CuSO4 + H2O In the preparation of copper(II) sulphate, copper(II) oxide is added to 20 cm3 of sulphuric acid of 1.0 mol / dm3 concentration until no more reacts. (a) (i) Calculate the number of moles in the 20 cm3 of sulphuric acid. moles of sulphuric acid = [1] (ii) How many moles of copper(II) sulphate are produced in the reaction? moles of copper(II) sulphate = [1] (iii) Calculate the relative formula mass, Mr, of copper(II) sulphate, CuSO4. Show your working. Mr = [2] (iv) Calculate the mass of copper(II) sulphate, CuSO4, formed. Show your working. mass = g [2] (b) Describe how crystals of copper(II) sulphate can be prepared from the mixture of excess copper(II) oxide and copper(II) sulphate solution obtained when the reaction stops. [3]

5 © UCLES 2005 0652/03/O/N/05 [Turn over For Examiner's Use 4 A player throws a ball, of mass 0.15 kg, horizontally. The ball has a constant acceleration for a time of 0.10s and then moves at a constant speed of 20.0 m / s for 0.80 s before being caught and brought to rest in a further time of 0.30 s. As the ball is caught it decelerates non-uniformly. (a) On Fig. 4.1 draw a graph showing the speed of the ball from when it was thrown until the time it came to rest. 20 15 10 5 0 0 0.20 0.40 0.60 0.80 1.00 1.20 speed in m / s time in s Fig. 4.1 [4] (b) Calculate the maximum kinetic energy of the ball. Show all your working. maximum kinetic energy = [3] (c) Calculate the acceleration of the ball during the first 0.10 s. Write down the equation that you use and show all your working. acceleration = [3]

6 © UCLES 2005 0652/03/O/N/05 For Examiner's Use 5 Fig. 5.1 shows the gas hydrogen being burned in air. hydrogen glass tube flame Fig. 5.1 (a) When hydrogen burns the only product is water. Write a balanced equation for the burning of hydrogen. [2] (b) When petrol is burned in a car engine a number of products are formed. Some of these products cause pollution. These include carbon monoxide and oxides of nitrogen. (i) How are the oxides of nitrogen removed from the exhaust gases of modern cars. [1] (ii) Why may the presence of carbon monoxide in car exhaust systems cause a health problem? [1] (c) It has been suggested that hydrogen may replace petrol as a fuel for cars. Suggest one advantage and one disadvantage of using hydrogen instead of petrol. advantage disadvantage [2]

7 © UCLES 2005 0652/03/O/N/05 [Turn over For Examiner's Use 6 (a) Explain what is meant by an object being in equilibrium. [2] (b) Fig. 6.1 shows a method of measuring the mass of a uniform loaded ruler. The ruler is pivoted at the 18 cm mark. 18 cm 0 cm 50 g Fig. 6.1 (i) The ruler is uniform. What does this tell you about the position of its centre of mass? [1] (ii) The total length of the ruler is 80 cm. The 50 g mass is hung from the 8 cm mark on the ruler. Calculate the mass of the ruler. Show all your working. mass of ruler = g [4]

8 © UCLES 2005 0652/03/O/N/05 For Examiner's Use 7 Powdered calcium carbonate is added to excess hydrochloric acid of three different concentrations, A, B and C. CaCO3 + 2HCl CaCl2 + CO2 + H2O In each experiment the same mass of powder is used and the acid is at the same temperature. The volume of carbon dioxide gas given off is measured at time intervals. The results of these experiments are shown in Fig. 7.1. 100 50 0 0 60 time / s 120 volume of gas / cm3 A B C Fig. 7.1 (a) (i) Which of the three solutions of hydrochloric acid, A, B or C, is the most concentrated? [1] (ii) Explain how Fig. 7.1 shows your answer to (i) is correct. [2] (iii) Why do each of the three experiments give the same total volume of gas? [1] (b) A fourth experiment is carried out using hydrochloric acid solution A and the same mass of powdered calcium carbonate. This time the experiment is carried out at a higher temperature. Sketch on Fig. 7.1 the result you would expect for this fourth experiment. [2]

9 © UCLES 2005 0652/03/O/N/05 [Turn over For Examiner's Use (c) (i) Calculate the number of moles in the 100 cm3 of carbon dioxide gas produced. (Assume the volume of carbon dioxide is measured at r.t.p. The volume of one mole of any gas is 24 dm3 at r.t.p.). moles of carbon dioxide = [1] (ii) Calculate the number of moles of calcium carbonate used to produce 100 cm3 of carbon dioxide gas. moles of calcium carbonate = [1] (iii) Calculate the mass of calcium carbonate used to produce 100 cm3 of carbon dioxide gas. Show your working. (The relative formula mass, Mr, of calcium carbonate = 100.) mass of calcium carbonate = g [2]

10 © UCLES 2005 0652/03/O/N/05 For Examiner's Use 8 (a) (i) Name the process by which the Sun produces energy. [1] (ii) Explain what happens in this process. [3] (b) Calculate the energy released in the Sun when its mass decreases by 1200 kg as a result of this process. Write down the equation you use and show all your working. The speed of light = 3.0 x 108 m / s. energy released = J [4] 9 Fig. 9.1 shows the graphical formulae of five organic compounds. C H H C H H H H H C H H C H H O H H C H H C O O H A B C C C H H C H H H H C H H D H H H H E C Fig. 9.1

11 © UCLES 2005 0652/03/O/N/05 [Turn over For Examiner's Use (a) (i) Which two compounds are alkanes? [1] (ii) Which compound dissolves in water to give an acidic solution? [1] (b) (i) Describe a test to distinguish between compounds C and D. test result [2] (ii) In industry compound D is made from compound C. Name the type of reaction that is used. [1] (c) Compound D can be used to make a polymer. Draw the structure for this polymer. [2]

12 © UCLES 2005 0652/03/O/N/05 For Examiner's Use 10 Fig. 10.1 shows a circuit with a high resistance voltmeter being used to measure the e.m.f. of a cell. V Fig. 10.1 (a) Explain why the voltmeter must have a high resistance if it is to measure an accurate value of the e.m.f. [2] (b) Fig. 10.2 shows a cell with an internal resistance of 5 Ω. A voltmeter which has a resistance of 995 Ω is connected across the cell. The e.m.f. of the cell is 1.50 V. V 995 Ω 5 Ω internal resistance Fig. 10.2 (i) Calculate the current in the circuit. current = A [3]

13 © UCLES 2005 0652/03/O/N/05 For Examiner's Use (ii) Calculate the potential difference across the voltmeter. potential difference = V [2] (iii) Explain why this voltmeter gives a good approximation to the e.m.f. of the cell. [2]

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16 0652/03/O/N/05 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 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 DATA SHEET The Periodic Table of the Elements

UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education MARK SCHEME for the November 2005 question paper 0652 PHYSICAL SCIENCE 0652/03 Paper 3 (Extended) maximum raw mark 80 This mark scheme is published as an aid to teachers and students, to indicate the requirements of the examination. It shows the basis on which Examiners were initially instructed to award marks. It does not indicate the details of the discussions that took place at an Examiners’ meeting before marking began. Any substantial changes to the mark scheme that arose from these discussions will be recorded in the published Report on the Examination. All Examiners are instructed that alternative correct answers and unexpected approaches in candidates’ scripts must be given marks that fairly reflect the relevant knowledge and skills demonstrated. Mark schemes must be read in conjunction with the question papers and the Report on the Examination. The minimum marks in these components needed for various grades were previously published with these mark schemes, but are now instead included in the Report on the Examination for this session. • CIE will not enter into discussion or correspondence in connection with these mark schemes. CIE is publishing the mark schemes for the November 2005 question papers for most IGCSE and GCE Advanced Level and Advanced Subsidiary Level syllabuses and some Ordinary Level syllabuses. www.XtremePapers.com

Page 1 Mark Scheme Syllabus Paper IGCSE Examinations – November 2005 0652 3 © University of Cambridge International Examinations 2005 1 (a) one electron in outer shell ; eight electrons in each of second and third shells ; [2] (b) (i) 2Li + 2H2O → 2LiOH + H2 ;; one mark for formulae, one mark for balance [2] (ii) apply a lighted splint ; gas burns with a pop / squeak ; [2] (c) hydrogen catches fire / flame ; reaction quicker / moves more quickly around surface ; any two metal melts ; [2] Total [8] 2 (a) use of sini / sinr = n ; correct rearrangement or 0.63 seen ; 39.0(5)º ; [1] [1] [1] (b) block with incident, refracted and emergent rays ; incident and emergent rays parallel by eye ; incident and refracted angles consistent with part (a) ; [1] [1] [1] Total [6] 3 (a) (i) 1.0 x 20/1000 = 0.02 ; [1] (ii) 0.02 (allow error carried forward from (i)) ; [1] (iii) 64 + 32 + (4 x 16) ; = 160 ; [2] (iv) 160 x 0.02 ; (allow error carried forward from (ii) and (iii)) = 3.2 ; [2] (b) filter off the excess copper(II) oxide ; evaporate off some of the water ; leave solution to cool / collect crystals and dry ; [3] Total [9]

Page 2 Mark Scheme Syllabus Paper IGCSE Examinations – November 2005 0652 3 © University of Cambridge International Examinations 2005 4 (a) all timings accurate ; constant positive gradient from origin to (0.1,20) ; horizontal line from end of acceleration to (0.9,20) ; variable gradient line from end of constant speed to (1.2,0) ; [1] [1] [1] [1] (b) use of ½mv2 or ½ x 0.15 x 202 30 J [1] [1] [1] (c) acceleration equation or use of gradient 200 m/s2 [1] [1] [1] Total [10] 5 (a) 2H2 + O2 → 2H2O one mark for formulae ; one mark for balance ; [2] (b) (i) catalytic converter / using a catalyst ; [1] (ii) carbon monoxide is poisonous / uses blood’s O2 ; owtte [1] (c) advantage: no pollution / limitless supply / renewable ; disadvantage: needs to be pressurised / cooled ; [2] Total [6]

Page 3 Mark Scheme Syllabus Paper IGCSE Examinations – November 2005 0652 3 © University of Cambridge International Examinations 2005 6 (a) idea of balanced forces ; moments balanced ; [1] [1] (b) (i) centre of mass at its centre ; [1] (ii) attempted use of moments ; use of 10 cm and 22 cm ; 50 x 10 = m x 22 ; mass = 22.7(3) ; accept 23 [1] [1] [1] [1] Total [7] 7 (a) (i) A ; [1] (ii) reaction rate increases with concentration ; A has the steepest curve / has reaction completed in shortest time ; [2] (iii) same mass of calcium carbonate and excess acid used each time / same mass of acid and all calcium carbonate reacts each time ; [1] (b) sketch on graph with steeper slope than A ; starts at origin and reaches 100 cm3 before 20 s ; [2] (c) (i) 100/24000 = 0.0042 (accept 0.00417) ; [1] (ii) 0.0042 ; (allow error carried forward from (i)) [1] (iii) 100 x 0.0042 ; (allow error carried forward from (ii)) = 0.42 ; [2] Total [10]

Page 4 Mark Scheme Syllabus Paper IGCSE Examinations – November 2005 0652 3 © University of Cambridge International Examinations 2005 8 (a) (i) (nuclear) fusion ; [1] (ii) light nuclei fuse / join together ; forming heavier nuclei ; idea of increased mass defect and kinetic energy of fusion products / highly exothermic ; [1] [1] [1] (b) E = mc2 seen ; c squared (9 x 1016 seen or implied) ; 1.08 ; x 1020 J ; [1] [1] [1] [1] Total [8] 9 (a) (i) C and E (both required) [1] (ii) B [1] (b) (i) bubble through / shake with / add bromine (water) ; only D changes (red/orange of bromine) to colourless ; [2] (ii) (catalytic) cracking ; [1] (c) one mark for two carbon atoms and four hydrogen atoms with seven bonds shown, including a ‘spare’ bond on each side ; second mark for brackets and n or any number above 2 ; (marks can be scored for a diagram that shows three monomers joined ; with a ‘spare’ bond at each end ;) [2] Total [7] H H C C H H n

Page 5 Mark Scheme Syllabus Paper IGCSE Examinations – November 2005 0652 3 © University of Cambridge International Examinations 2005 10 (a) so that it draws negligible current ; almost no voltage is dropped across internal resistance ; [1] [1] (b) (i) R = 1000 (Ω) ; V = IR ; I = 1.5 mA ; in any form [1] [1] [1] (ii) 1.5 mA x 995 (Ω) ; 1.49(25) V ; [1] [1] (iii) its resistance is much higher than the internal resistance of the cell ; little voltage dropped across internal resistance ; [1] [1] Total [9]