Cambridge IGCSE Physical Science 0652 — 2011 Oct/Nov Paper 3 · Variant 1

This document consists of 19 printed pages and 1 blank page. IB11 11_0652_31/3RP © UCLES 2011 [Turn over *0849225562* For Examiner's Use 1 2 3 4 5 6 7 8 9 Total UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education PHYSICAL SCIENCE 0652/31 Paper 3 (Extended) October/November 2011 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. You may use a soft pencil for any diagrams, graphs, tables 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 20. 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.

2 © UCLES 2011 0652/31/O/N/11 For Examiner's Use 1 Two cars are being tested on a straight level track. Fig. 1.1 shows the speed-time graphs for the two cars, each of mass 1500 kg. speed m / s car car A car car B 60 40 20 0 0 10 20 30 40 time / s car A car B Fig. 1.1 (a) Determine the maximum velocity of car A. velocity = m / s [1] (b) Describe the motion of car A after 26 s. [2]

3 © UCLES 2011 0652/31/O/N/11 [Turn over For Examiner's Use (c) (i) Use the graph to calculate the acceleration of car B during the first 10 s of the test. acceleration = [2] (ii) Calculate the resultant force on car B during this period. force = [2] (iii) Explain why the engine must provide a greater force than that given in your answer to (c)(ii). [2] (d) As the two cars approach the end of the track they brake and come to rest. Explain which car produces the greater braking force. [2]

4 © UCLES 2011 0652/31/O/N/11 For Examiner's Use 2 Fig. 2.1 shows a catalytic converter, which is part of a car exhaust system. catalytic converter gases from the engine gases to the air A B Fig. 2.1 Scientists analyse the gases at A and at B. Their results are shown in Table 2.1. Table 2.1 gas percentage at A percentage at B carbon dioxide 8.0 9.2 carbon monoxide 5.0 3.8 hydrogen 2.0 0.8 nitrogen 71.0 71.3 nitrogen monoxide 0.3 0.0 oxygen 4.0 2.8 water vapour 9.0 10.7 (a) The scientists conclude that in the catalytic converter nitrogen monoxide is converted to nitrogen by reaction with carbon monoxide. (i) Write a balanced equation for this reaction. Use the data in Table 2.1 to help you. [2] (ii) Use this reaction to explain the meaning of the terms reduced and oxidised. [2] (iii) Explain how the results in Table 2.1 support the conclusion that this reaction takes place in the catalytic converter. [2]

5 © UCLES 2011 0652/31/O/N/11 [Turn over For Examiner's Use (iv) Use data from Table 2.1 to suggest another reaction that takes place in the catalytic converter. [1] (b) Parts of the car exhaust system are made from galvanised steel. (i) Explain how galvanising prevents steel from rusting. [3] (ii) Suggest why galvanising is a better method of rust prevention than painting. [1]

6 © UCLES 2011 0652/31/O/N/11 For Examiner's Use 3 A student experiments with a rubber band. She stretches it between two retort stands and notices that it produces a sound when she plucks it. The apparatus is shown in Fig. 3.1. rubber band Fig. 3.1 (a) Explain why the sound is produced. [2]

7 © UCLES 2011 0652/31/O/N/11 [Turn over For Examiner's Use (b) The student sets up a cathode ray oscilloscope and a microphone, as shown in Fig. 3.2, to display the sound trace produced by the apparatus in Fig. 3.1. microphone cathode ray oscilloscope Fig. 3.2 The time base is set to 2.5 ms / division. Calculate the frequency of the sound wave. Show your working in the box. frequency = Hz [3]

8 © UCLES 2011 0652/31/O/N/11 For Examiner's Use 4 Silver salts are used in photography. (a) The action of light on silver bromide releases an electron. Ag+Br - Ag+ + Br + e- (i) How does light enable this reaction to take place? [1] (ii) The silver ion is converted into a silver atom. Why is this said to be a reduction reaction? [1] (iii) Write an ionic equation to show this reduction of a silver ion. [1] (b) Silver bromide can be made from the reaction between silver nitrate and potassium bromide. AgNO3(aq) + KBr(aq) AgBr(s) + KNO3(aq) (i) Describe how you would prepare a pure, dry sample of silver bromide from solutions of silver nitrate and potassium bromide. [4]

9 © UCLES 2011 0652/31/O/N/11 [Turn over For Examiner's Use (ii) What mass of silver bromide could be made from 5.0 g of silver nitrate? [relative atomic masses, Ar : Ag, 108; Br, 80; N, 14; O, 16] Show your working in the box. mass of silver bromide = g [3]

10 © UCLES 2011 0652/31/O/N/11 For Examiner's Use 5 Fig. 5.1 shows an electric circuit. The e.m.f. of the battery is 6.0 V. The total resistance of the variable resistor 48 Ω. V A B D C variable resistor sliding contact 6.0 V A Fig. 5.1 (a) (i) Calculate the current measured by the ammeter. current = [2] (ii) When the sliding contact is at point B the voltmeter reading is 4.5 V. Calculate the value of the resistance of the section of the variable resistor BC. resistance = [2] (b) The sliding contact is moved to point D. The reading on the voltmeter is now 3.0 V. Show that the resistance of the section CD of the variable resistor is 24 Ω. You may assume that the current through the circuit remains the same. [1]

11 © UCLES 2011 0652/31/O/N/11 [Turn over For Examiner's Use (c) The student realises that he could use this circuit as a variable voltage supply. He leaves the sliding contact at point D and connects a 3.0 V bulb of resistance 8 Ω in place of the voltmeter. (i) Show that the resistance of the parallel combination of the bulb and the section CD of the variable resistor is 6 Ω. [2] (ii) Calculate the total resistance in the circuit. resistance = [1] (iii) Calculate the potential drop across the section CD of the variable resistor. p.d. = [2] (iv) Comment on the brightness of the bulb. [1]

12 © UCLES 2011 0652/31/O/N/11 For Examiner's Use 6 When calcium carbonate is heated strongly it decomposes to form calcium oxide and carbon dioxide. CaCO3 CaO + CO2 (a) Calculate the volume of carbon dioxide, measured at room temperature and pressure, produced when 2.5 g of calcium carbonate is decomposed. [The volume of one mole of any gas is 24 dm3 at room temperature and pressure.] Show your working in the box. volume of carbon dioxide = dm3 [3] (b) Calcium oxide reacts with hydrochloric acid to form a salt. CaO + 2HCl CaCl2 + H2O In this reaction calcium oxide is acting as a base. (i) Use this reaction to define the terms acid and base in terms of proton transfer. acid base [2]

13 © UCLES 2011 0652/31/O/N/11 [Turn over For Examiner's Use (ii) Calcium oxide reacts with acids but not with alkalis. It is classified as a basic oxide. Complete Table 6.1 to classify three other oxides. Table 6.1 name formula property type of oxide calcium oxide CaO reacts with acids but not alkalis basic aluminium oxide Al2O3 reacts with both acids and alkalis carbon dioxide CO2 reacts with alkalis but not acids nitrogen monoxide NO reacts with neither acids nor alkalis [3]

14 © UCLES 2011 0652/31/O/N/11 For Examiner's Use 7 Fig. 7.1 shows a magnet and a coil which is connected to a sensitive voltmeter. S N coil cardboard tube sensitive voltmeter Fig. 7.1 (a) (i) Describe what you would observe as the magnet is moved away from the coil. [2] (ii) Explain this observation using the theory of electromagnetic induction. [2] (b) The magnet is now moved towards the coil. Describe what you would observe. [1]

15 © UCLES 2011 0652/31/O/N/11 [Turn over For Examiner's Use (c) The magnet is now replaced with a similar coil connected to an alternating supply. The original coil is connected to a cathode ray oscilloscope. This is shown in Fig. 7.2. S alternating supply cathode ray oscillosocope Fig. 7.2 State and explain what is observed when the switch S is closed. [2]

16 © UCLES 2011 0652/31/O/N/11 For Examiner's Use 8 Table 8.1 contains data about elements in Group 0 of the Periodic Table. Table 8.1 element symbol proton number boiling point / °C density of gas in kg / m3 helium He 2 −269 0.17 neon Ne 10 −246 0.84 argon Ar 18 −186 1.67 krypton Kr 36 −152 3.50 (a) (i) What name is given to the elements in Group 0? [1] (ii) Use information from Table 8.1 to describe a trend in one physical property shown by this group of elements. [2] (iii) Describe a chemical property common to all elements in this group. [1] (iv) Xenon is the next member of Group 0 after krypton. Predict the density of xenon. density = kg / m3 [1]

17 © UCLES 2011 0652/31/O/N/11 [Turn over For Examiner's Use (b) (i) Draw a diagram to show the electron arrangement in an atom of argon. [2] (ii) A calcium ion has the same electron arrangement as an argon atom. Give the name of, and the charge on, another ion apart from calcium that has the same electron arrangement as an argon atom. name charge [2] (iii) State how a calcium ion is formed from a calcium atom. [2]

18 © UCLES 2011 0652/31/O/N/11 For Examiner's Use 9 A student is investigating the cooling of a cup of tea. She makes the tea using water first boiled in a kettle. As the tea cools she notices that some of it evaporates. (a) (i) State one similarity between evaporation and boiling. [1] (ii) Explain the difference between evaporation and boiling. [2] (b) The graph in Fig. 9.1 shows how the temperature of the tea changes with time. 100 50 0 0 2 4 6 time / minutes temperature / °C Fig. 9.1 Use the graph to estimate room temperature. room temperature = °C [1] (c) Explain, in terms of the molecular kinetic theory, what happens to the tea as it cools. [2]

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20 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. © UCLES 2011 0652/31/O/N/11 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 Sulfur 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 October/November 2011 question paper for the guidance of teachers 0652 PHYSICAL SCIENCE 0652/31 Paper 3 (Extended Theory), maximum raw mark 80 This mark scheme is published as an aid to teachers and candidates, to indicate the requirements of the examination. It shows the basis on which Examiners were instructed to award marks. It does not indicate the details of the discussions that took place at an Examiners’ meeting before marking began, which would have considered the acceptability of alternative answers. Mark schemes must be read in conjunction with the question papers and the report on the examination. • Cambridge will not enter into discussions or correspondence in connection with these mark schemes. Cambridge is publishing the mark schemes for the October/November 2011 question papers for most IGCSE, GCE Advanced Level and Advanced Subsidiary Level syllabuses and some Ordinary Level syllabuses.

Page 2 Mark Scheme: Teachers’ version Syllabus Paper IGCSE – October/November 2011 0652 31 © University of Cambridge International Examinations 2011 1 (a) 50 m / s ; [1] (b) acceleration / deceleration / slowing down ; constant / steady referring to acceleration / deceleration (not at constant speed) / calculated value of acceleration / comes to rest ; [2] (c) (i) use of gradient, (a = (30 – 0) / (10 – 0)) ; 3.0 m / s2 ; [2] (ii) use of F = ma = 1500 × 3.0 (e.c.f.) ; = 4500 N ; [2] (iii) mention of frictional force / air resistance ; force from engine = accelerating force + frictional force / work done against friction ; [2] (d) (car B) ; larger gradient / same mass (not accept shorter period of time) ; greater acceleration / deceleration ; [2] (both marks can be scored for a correct calculation of both accelerations and comment) [Total: 11] 2 (a) (i) 2NO + 2CO → N2 + 2CO2 all formulae correct ; balanced ; [2] (NO + CO → N + CO2 max 1) (ii) nitrogen (monoxide) is reduced because it has lost oxygen ; carbon (monoxide) is oxidised because it has gained oxygen ; [2] (marks can be gained for correct reference to electron loss and gain / oxidation states) (1 max if general explanation without reference to NO and CO is given) (iii) any two: (percentage) of nitrogen monoxide has decreased ; (percentage) of nitrogen has increased ; (percentage) of carbon monoxide has decreased ; (percentage) of carbon dioxide has increased ; [max 2] (iv) carbon monoxide reacts with oxygen to form carbon dioxide / hydrogen reacts with oxygen to form water ; [1] (if the carbon monoxide to carbon dioxide process is not scored in (iii) it can score here) (b) (i) galvanising means coating with zinc ; zinc more reactive than steel / iron ; zinc reacts not iron / sacrificial reaction ; [3]

Page 3 Mark Scheme: Teachers’ version Syllabus Paper IGCSE – October/November 2011 0652 31 © University of Cambridge International Examinations 2011 (ii) painted steel will rust if scratched or chipped but galvanised will not (rust) ; [1] (both required, but allow the comment re zinc not reacting if included in (i)) [Total: 11] 3 (a) the band vibrates ; causing air (molecules) to vibrate / forming a longitudinal / compression wave in the air ; [2] (b) 4.5 or 5 waves number of waves or specified number of divisions ; 4.5 in 4 divs (accept 5 waves in 5 divs) ; f = 450 (Hz) ; [3] (allow rounding errors for answer) (use of only one wave – 2 max, raw answer 400 Hz – 2 max) [Total: 5] 4 (a) (i) light provides energy ; [1] (ii) reduction is gain of an electron / oxidation state goes down ; [1] (iii) Ag+ + e– → Ag ; [1] (b) (i) add potassium bromide solution to silver nitrate solution until no further reaction ; filter (to obtain ppt) ; wash ppt with distilled water ; leave ppt to dry ; keep in dark ; [max 4] (ii) AgNO3 = 170 and AgBr = 188 ; number of moles = 170 5 (accept 188 5 ) ; = 5.5 g ; [3] [Total: 10] 5 (a) (i) use of I = V / R (= 6 / 48) ; = 0.125 A (0.13 A) ; [2] (ii) (e.c.f.) use of R = V / I (= 4.5 / 0.125) ; = 36 Ω ; [2] (b) R = V/I = 3.0 / 0.125 = 24 Ω / discussion re ½ potential difference leads to ½ R ; [1] (c) (i) use of 1 / R = 1 / R1 + 1 / R2 = 1 / 24 + 1 / 8 = 4 / 24 (accept sum / product) ; R = 24 / 4 = 6 Ω ; [2] (must show R = 6 Ω)

Page 4 Mark Scheme: Teachers’ version Syllabus Paper IGCSE – October/November 2011 0652 31 © University of Cambridge International Examinations 2011 (ii) (6 + 24 =) 30 Ω ; [1] (iii) (e.c.f.) current = 6 / 30 = 0.2 A ; potential difference = 0.2 × 6 = 1.2 V ; [2] (iv) dim / not properly lit if potential difference < 3, bright if potential difference > 3, normal if potential difference = 3 ; [1] [Total: 11] 6 (a) CaCO3 = 100 ; number of moles = 100 5 . 2 or 0.025 ; = 0.6 dm3 ; [3] (b) (i) calcium oxide is a base because it gains a proton / the oxide ion gains a proton ; hydrochloric acid is an acid because it donates a proton ; [2] (max 1 if neither refers to specific reaction) (ii) amphoteric ; acidic ; neutral ; [3] [Total: 8] 7 (a) (i) the needle of the voltmeter moves ; then goes back to zero ; (do not allow if there is a residual current. e.g. needle falls to zero) [2] (ii) when the magnet moves the coil cuts / there is a change in magnetic flux ; which induces an e.m.f./current ; [2] (b) the needle of the voltmeter moves in the opposite direction ; [1] (c) wave trace seen on the cathode ray oscilloscope ; changing current produces changing field ; [2] [Total: 7] 8 (a) (i) noble gases (do not accept inert, rare) ; [1] (ii) boiling point increases / density increases / mass increases ; with increasing atomic number / down group ; [2] (iii) unreactive (accept inert) ; [1] (iv) any value between 4.5 and 9.9 kg / m3 ; [1]

Page 5 Mark Scheme: Teachers’ version Syllabus Paper IGCSE – October/November 2011 0652 31 © University of Cambridge International Examinations 2011 (b) (i) diagram showing 8 electrons in outer shell ; 3 shells with 2 electrons in first shell and 8 in second shell ; [2] (ii) potassium, 1+ OR chloride, 1− ;; [2] (iii) loses electrons ; two electrons are lost ; [2] [Total: 11] 9 (a) (i) liquid turns to vapour / gas (not molecules) ; [1] (ii) boiling: bubbles of vapour form in the liquid ; evaporation: molecules leave the surface of the liquid ; OR boiling occurs at fixed temperature ; evaporation at a range of temperatures 1 ; [max 2] OR boiling is a violent process (1 max) ; (b) 15 – 25 °C ; [1] (c) molecules lose energy / slow down etc. ; (not accept molecules lose thermal energy) clear energy loss is loss in kinetic energy / energy is transferred to the surroundings / hence temperature falls ; [2] [Total: 6]