Cambridge IGCSE Physical Science 0652 — 2015 Oct/Nov Paper 3 · Variant 2

This document consists of 20 printed pages and 4 blank pages. DC (ST/FD) 117452 © UCLES 2015 [Turn over Cambridge International Examinations Cambridge International General Certificate of Secondary Education * 8 5 3 8 7 0 2 7 3 2 * PHYSICAL SCIENCE 0652/32 Paper 3 (Extended) October/November 2015 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 an HB pencil for any diagrams, graphs, tables or rough working. Do not use staples, paper clips, glue or correction fluid. DO NOT WRITE IN ANY BARCODES. Answer all questions. A copy of the Periodic Table is printed on page 24. Electronic calculators may be used. 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 0652/32/O/N/15 © UCLES 2015 1 Fig. 1.1 shows an Atlas space rocket as it takes off from its launch pad. Fig. 1.1 (a) The initial mass of the rocket and fuel is 160 000 kg. Calculate the weight of the rocket and fuel. Use g = 10 m / s2. weight = … N [1] (b) The initial thrust from the rocket motors is 2 000 000 N. (i) Calculate the resultant upward force on the rocket. force = … N [1] (ii) Calculate the initial acceleration of the rocket and state the unit. acceleration = … unit … [3]

3 0652/32/O/N/15 © UCLES 2015 [Turn over (c) The thrust from the motors is constant. However, the acceleration of the rocket increases. Suggest a reason for this increase. … … … [1]

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5 0652/32/O/N/15 © UCLES 2015 [Turn over 2 Acids react with bases to form salts. Table 2.1 shows some reactions of acids and bases and the salts formed. Table 2.1 acid base salt formed sulfuric acid sodium hydroxide sodium sulfate hydrochloric acid sodium carbonate zinc oxide zinc nitrate sulfuric acid magnesium sulfate (a) Complete Table 2.1 by filling in the empty boxes. [3] (b) Write a balanced equation for the reaction between hydrochloric acid and sodium carbonate. … [2] (c) Zinc oxide will react with alkalis as well as acids. State the name given to this sort of oxide. … [1] (d) (i) When an acid is added to an alkali, a salt and water only are formed. This is a neutralisation reaction. Write an equation, using ions, to represent the neutralisation in such a reaction. … [1] (ii) Dilute sulfuric acid is added to an aqueous solution of sodium hydroxide. Use ideas of proton transfer to explain why sodium hydroxide is the base in this reaction. … … [1]

6 0652/32/O/N/15 © UCLES 2015 3 (a) Fig. 3.1 shows a piece of apparatus, viewed from above. Four different metal strips are fixed to a wooden ring. ZRRGHQULQJ DOXPLQLXP LURQ FRSSHU EUDVV Fig. 3.1 Fig. 3.2 shows an experiment using the apparatus. A match head is placed on the end of each metal strip. The strips are then heated at the centre. match heads heat Fig. 3.2 Each of the match heads ignites after a different length of time. This is shown in Table 3.1. Table 3.1 metal strip time for match head to ignite / minutes aluminium 4 brass 3 copper 1 iron 8 List the metals in order of their thermal conductivity. most conductive … … … least conductive … [2]

7 0652/32/O/N/15 © UCLES 2015 [Turn over (b) Fig. 3.3 shows an experiment to investigate the energy absorbed by different surfaces. thermometer $ heater thermometer % foil painted black shiny silver foil Fig. 3.3 The two thermometers are equal distances from the heater. Both of their bulbs are wrapped in aluminium foil. The foil on thermometer A is painted black and the foil on thermometer B is left shiny silver. At the beginning of the experiment the two thermometers both show a temperature of 18 °C. The heater is switched on. (i) State the main method of thermal energy transfer that takes energy from the heater to the thermometers. … [1] The heater is left on for ten minutes. Thermometer A now shows a reading of 32 °C. (ii) Predict the temperature reading shown by thermometer B. temperature = … °C [1] (iii) Explain why there is a difference in the two thermometer readings. … … [1]

8 0652/32/O/N/15 © UCLES 2015 4 Fig. 4.1 shows the structural formulae of ethene and two compounds, A and B, that can be made from ethene. HWKHQH FRPSRXQG$ FRPSRXQG% & + + + + & & & + + + + + + Q + %U %U + & & Fig. 4.1 (a) Ethene can be made from the large chain alkanes found in crude oil. Name this process and state the conditions necessary for it to occur. … … [2] (b) Compound A is formed in a test to distinguish between ethane and ethene. Describe this test and the results you would expect for each. test … … … result with ethane … … result with ethene … … [2] (c) State the type of reaction used to make compound B from ethene. … [2]

9 0652/32/O/N/15 © UCLES 2015 [Turn over (d) Ethanol can be made by the reaction of ethene with steam. C2H4 + H2O C2H5OH Calculate the mass of ethanol that can be made from 1.0 kg of ethene. [Relative atomic masses: Ar: C, 12; H, 1; O, 16.] Show your working in the box. mass of ethanol = … kg [3]

10 0652/32/O/N/15 © UCLES 2015 5 Fig. 5.1 shows a ray of light entering a lens. The insert shows an enlarged view. UD\RIOLJKW OHQV LQVHUW Fig. 5.1 (a) On the enlarged insert, identify and label, with the letter r, the angle of refraction the ray of light makes with the lens. [1] (b) The ray of light has an angle of incidence of 16.0° at the lens and the angle of refraction is 11.0°. Calculate the refractive index of the lens. Give your answer to 3 significant figures. refractive index = … [2] (c) Fig. 5.2 shows the lens being used as a magnifying glass to study a beetle. EHHWOH OHQV H\H Fig. 5.2 (i) Mark, with an X, on Fig. 5.2 a possible position of the principal focus of the lens. [1]

11 0652/32/O/N/15 © UCLES 2015 [Turn over (ii) State three words that describe the image seen when a lens is used as a magnifying glass. 1. … 2. … 3. … [3]

12 0652/32/O/N/15 © UCLES 2015 6 Table 6.1 shows properties of some metals. Table 6.1 metal density g / cm3 melting point / °C relative measurements strength hardness electrical conductivity aluminium 2.7 660 21 48 62 copper 8.9 1085 78 52 100 iron 7.9 1538 50 65 17 titanium 4.5 1668 100 100 3 (a) Use information from Table 6.1 to explain why (i) copper is used in electrical wiring in houses, … [1] (ii) aluminium is the main metal in the alloy used to make aeroplane bodies. … [1] (b) An alloy of aluminium, containing small quantities of copper, manganese and magnesium, is used to make aeroplane bodies. (i) Suggest how the properties of this alloy make it more suitable for use in aeroplane bodies than pure aluminium. … … [1]

13 0652/32/O/N/15 © UCLES 2015 [Turn over (ii) Use ideas about metallic bonding to explain this difference in properties. You may draw a diagram to help your answer. … … … … … [4] (c) (i) When exposed to humid air, iron rusts until none of the metal remains. Aluminium does not react in a similar way. Explain this difference. … … [1] (ii) Iron can be galvanised to prevent rusting. The iron is covered with a layer of zinc. This stops the iron rusting even if the layer of zinc is scratched to expose iron. Explain why this layer of zinc prevents the exposed iron from rusting. … [1]

14 0652/32/O/N/15 © UCLES 2015 7 A student constructs the circuit shown in Fig. 7.1 using a cell of e.m.f. 6.0 V, a resistor of resistance 20 Ω and a resistance wire of length 25 cm. A 6.0 V 201 resistance wire Fig. 7.1 (a) Explain what is meant by the term e.m.f. (electromotive force). … … … [2] (b) The ammeter reading is 0.24 A and the potential difference across the resistor is 4.8 V. (i) Calculate the charge passing through the resistor in 5 minutes. Give the unit. charge = … unit … [3] (ii) Calculate the energy dissipated in the resistor in this time. energy = … J [2] (iii) Calculate the potential difference across the resistance wire. potential difference = … V [1] (iv) Use your result from (iii) to calculate the resistance of this wire. resistance = … Ω [2]

15 0652/32/O/N/15 © UCLES 2015 [Turn over (c) The student replaces the resistance wire with one made from the same material but of length 50 cm and half the diameter. (i) Calculate the resistance of the replacement wire. resistance = … Ω [2] (ii) State how the potential difference across the resistor changes and explain your answer. … … … [2]

16 0652/32/O/N/15 © UCLES 2015 8 Table 8.1 shows how the concentration of nitrogen oxides and carbon dioxide in the air increased during the twentieth century. Table 8.1 year concentration in parts per million nitrogen oxides carbon dioxide 1900 18 300 1920 18 305 1940 20 310 1960 25 320 1980 30 340 2000 35 370 (a) Describe and compare the trends shown in Table 8.1. … … … … [2] (b) It is suggested that these trends may have been due to an increased use of cars. Since 2000, the number of cars fitted with catalytic converters has increased. This equation shows the reaction taking place in a catalytic converter. 2NO + 2CO N2 + 2CO2 Suggest and explain what effect the increased use of catalytic converters may have on the concentration of nitrogen oxides in the air. … … … … [2]

17 0652/32/O/N/15 © UCLES 2015 [Turn over (c) Cars release pollutants other than those shown in Table 8.1 into the air. Name two of these other pollutants. 1. … 2. … [2] (d) One of the hydrocarbons in petrol is octane, C8H18. This equation shows the complete combustion of octane. 2C8H18 + 25O2 16CO2 + 18H2O Calculate the volume of carbon dioxide, measured at room temperature and pressure, produced when 1.0 kg of octane burns completely. [Relative atomic masses: Ar: C, 12; H, 1; O, 16] 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 [4]

18 0652/32/O/N/15 © UCLES 2015 9 Fi g. 9.1 shows an experiment where a magnet is placed near a coil of wire. The voltmeter is shown at the beginning of the experiment. SRVLWLRQ ; 1 6 1 6 SRVLWLRQ < PDJQHW FRLO YROWPHWHU Fig. 9.1 (a) State what is observed when (i) the magnet is moved from position Y to position X, … … (ii) the magnet is moved from position X to position Y, … … (iii) the magnet is moved from position X to position Y at a greater speed, … … (iv) the coil is moved towards the magnet. … … [5]

19 0652/32/O/N/15 © UCLES 2015 [Turn over (b) The magnet is replaced by a current carrying coil of wire as shown in Fig. 9.2. 6 Fig. 9.2 Switch S is initially closed and there is a current in the coil of wire. Switch S is then opened and the current falls to zero. State and explain, by referring to magnetic fields, what is observed. … … … … [3]

20 0652/32/O/N/15 © UCLES 2015 10 Table 10.1 gives information about some of the elements in Group VII. Table 10.1 element atomic number melting point / °C colour chlorine 17 −101 light green bromine 35 −7 red iodine 53 114 dark grey (a) Describe two trends shown in Table 10.1 that occur with increasing atomic number of the element. 1. … … 2. … … [2] (b) The halogens decrease in reactivity with increasing atomic number. Bromine is added to a solution of potassium iodide. Iodine is displaced, forming a brown coloured solution. The equation for this reaction is shown below. Br2 + 2KI 2KBr + I2 Predict and explain what you would see if chlorine is added to a solution of potassium iodide. prediction … explanation … … … [2]

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24 0652/32/O/N/15 © UCLES 2015 Group 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 91 238 231 147 237 244 243 247 247 251 252 257 258 259 260 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 82 209 209 210 222 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 55 226 223 Ra Radium 88 a X b a = relative atomic mass X = atomic symbol b = atomic (proton) number Key DATA SHEET * 58–71 Lanthanoid series † 90–103 Actinoid series The volume of one mole of any gas is 24dm3 at room temperature and pressure (r.t.p.). To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge International Examinations Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download at www.cie.org.uk after the live examination series.

® IGCSE is the registered trademark of Cambridge International Examinations. CAMBRIDGE INTERNATIONAL EXAMINATIONS Cambridge International General Certificate of Secondary Education MARK SCHEME for the October/November 2015 series 0652 PHYSICAL SCIENCE 0652/32 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 should be read in conjunction with the question paper and the Principal Examiner Report for Teachers. Cambridge will not enter into discussions about these mark schemes. Cambridge is publishing the mark schemes for the October/November 2015 series for most Cambridge IGCSE®, Cambridge International A and AS Level components and some Cambridge O Level components.

Page 2 Mark Scheme Syllabus Paper Cambridge IGCSE – October/November 2015 0652 32 © Cambridge International Examinations 2015 1 (a) 1 600 000 (N) ; [1] (b) (i) (2 000 000 – 1 600 000 =) 400 000 (N) ; [1] (ii) Use of (a = F / m =) 400 000 / 160 000 ; 1 2.5 ; 1 m s–2 ; 1 [3] (c) (Fuel burnt so) mass / weight decreases / gravity gets less / air resistance decreases (as rocket rises) ; [1] [Total: 6] 2 (a) sodium chloride ; nitric acid ; magnesium hydroxide / magnesium oxide / magnesium carbonate / magnesium bicarbonate / magnesium hydrogencarbonate ; [3] (b) 2HCl + Na2CO3 → 2NaCl + H2O + CO2 M1 correct formulae ; M2 correct balancing of a correct equation ; [2] (c) amphoteric ; [1] (d) (i) H+ + OH– → H2O ; Ignore: spectator ions but must be correct ions and must balance [1] (ii) (hydroxide ion of sodium hydroxide) accepts proton / hydrogen ion / H+ ; (and so it is a base) [1] [Total: 8] 3 (a) copper best, iron worst ; 1 brass better conductor than aluminium ; 1 [2] (b) (i) IR / infra-red / radiation ; [1] (ii) 19–31 (inclusive) ; [1] (iii) black is a (better) absorber (of radiation than silver) / silver is a (better) reflector ; [1] [Total: 5]

Page 3 Mark Scheme Syllabus Paper Cambridge IGCSE – October/November 2015 0652 32 © Cambridge International Examinations 2015 4 (a) cracking ; 1 using a catalyst and reference to temperature ; OR high temperatures and reference to pressure ; 1 [2] (b) add bromine (water) ; 1 ethane: no change / red or orange colour remains AND ethene: decolourises (the bromine water) ; 1 [2] (c) addition ; 1 polymerisation ; 1 [2] (d) RFM ethene 28 or RFM ethanol 46 or 1:1 mole ratio identified ; 1 (mass ethanol =) 46 / 28 ; 1 1.6 (kg) ; 1 [3] [Total: 9] 5 (a) angle of refraction correctly marked ; [1] (b) (n =) sin i / sin r OR sin 16 / sin 11 ; 1 1.44(457 ...) ; 1 [2] (c) (i) Point marked, on line between centre of eye and beetle and further from lens than beetle ; [1] (ii) upright ; 1 enlarged ; 1 virtual ; 1 [3] [Total: 7]

Page 4 Mark Scheme Syllabus Paper Cambridge IGCSE – October/November 2015 0652 32 © Cambridge International Examinations 2015 6 (a) (i) (copper is) best / good (electrical) conductor ; [1] (ii) (aluminium is) lowest / low density ; [1] (b) (i) makes it strong ; [1] (ii) Any 4 from: For pure metal: diagram and/or description of positive ions ; in sea of electrons ; For alloy: ions of added metals different size to (aluminium ions) ; layers cannot slide / less easy to deform (lattice) ; In a pure metal: layers can slide in a pure metal / or layers cannot slide as easily in an alloy ; [4] (c) (i) (aluminium has protective / waterproof) oxide layer ; [1] (ii) zinc is more reactive (than iron) / zinc reacts before iron ; [1] [Total: 9]

Page 5 Mark Scheme Syllabus Paper Cambridge IGCSE – October/November 2015 0652 32 © Cambridge International Examinations 2015 7 (a) energy given or supplied (by the battery) OR (total) work done in (complete) circuit ; 1 per unit charge ; 1 [2] (b) (i) Use of (q = I t) = 0.24 × 5 × 60 ; 1 72 ; 1 C or coulomb ; 1 [3] (ii) Use of (E = V q or V I t) = 4.8 × 72 ; 1 346 (J) ; 1 [2] (iii) (battery emf – potential drop across resistor = 6.0 – 4.8 =) 1.2 (V) ; 1 [1] (iv) Use of R = V / I (=1.2 / 0.24) ; 1 5.0 (Ω) ; 1 [2] (c) (i) either recognition that 2 × length leads to 2 × resistance OR ½ × diameter leads to 4 × resistance ; 1 (r = 5.0 × 2 × 4 =) 40.0 (Ω) ; 1 [2] (ii) less ; 1 good reason, example: current less thus IR less, larger share of voltage across (resistance) wire ; 1 [2] [Total: 14] 8 (a) (concentration of) nitrogen oxides and carbon dioxide increased (with time) ; 1 Quantitative interpretation comment: e.g. percentage increase greater for NOx than CO2 ; 1 [2] (b) reduce /stop increase (in nitrogen oxides) ; 1 catalytic converters change nitrogen oxide to nitrogen ; 1 [2] (c) Any two from: carbon monoxide ; lead compounds ; carbon particulates / soot ; unburned hydrocarbons ; sulfur oxide(s) or dioxide or trioxide / SOx / SO2 / SO3 (volatile) organic compounds / VOC ; [2]

Page 6 Mark Scheme Syllabus Paper Cambridge IGCSE – October/November 2015 0652 32 © Cambridge International Examinations 2015 (d) Evidence of 114 e.g. 12 × 8 + 18 (allow: 228) ; 1 1000 / 114 or 8.77 (moles of octane) ; 1 2:16 or 1:8 mole ratio ; 1 (8.77 × 8 = 70.2 moles 1 mole = 24 dm3 24 × 70.) = 1684 / 1680 ; 1 [4] [Total: 10] 9 (a) (i) deflection of the voltmeter needle / there is a reading on voltmeter / emf induced ; 1 *(needle) goes back again ; 1 [2] (ii) deflection in the opposite direction ; [1] (iii) larger deflection ; [1] (iv) deflection (as in (ii)) ; [1] (b) current ( in primary coil) has magnetic field OR magnetic field changes (when switch opened) ; 1 field from primary coil links with secondary coil ; 1 (changed magnetic field) produces a deflection (when switch initially opens) ; 1 [3] [Total: 8] 10 (a) melting point increases ; 1 colour becomes darker ; 1 [2] (b) Any two from: brown colour / the same (as for bromine) ; chlorine displaces iodine / iodine displaced ; chlorine more reactive ; [2] [Total: 4]