Cambridge IGCSE Sciences - Co-ordinated (Double) 0654 — 2014 Oct/Nov Paper 3 · Variant 3

This document consists of 27 printed pages and 1 blank page. DC (LK/CGW) 89053/4 © UCLES 2014 [Turn over Cambridge International Examinations Cambridge International General Certificate of Secondary Education * 4 5 2 3 4 6 3 3 9 3 * CO-ORDINATED SCIENCES 0654/33 Paper 3 (Extended) October/November 2014 2 hours 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 soft 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. Electronic calculators may be used. You may lose marks if you do not show your working or if you do not use appropriate units. A copy of the Periodic Table is printed on page 28. 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 0654/33/O/N/14 © UCLES 2014 1 (a) Use the words in the list to complete the sentences, which are about evolution. You may use each word once, more than once or not at all. adaptation reproduction respond selection survive variation Organisms show … , which means that no two individuals are exactly alike. Some individuals show better … to their environment, and these individuals are more likely to … and reproduce. This may lead to evolution as a result of the process of natural … . [4] (b) Table 1.1 shows, for a species of bacterium, the percentage of bacteria that were resistant to the antibiotic penicillin. The data are for samples of bacteria taken in two different countries in the years 1980 and 2010. Table 1.1 country A country B percentage of antibiotic-resistant bacteria in 1980 3 4 percentage of antibiotic-resistant bacteria in 2010 54 12 (i) Compare the incidence of antibiotic-resistance in the two countries in 1980, … … in 2010. … … [2]

3 0654/33/O/N/14 © UCLES 2014 [Turn over (ii) In both countries, antibiotic-resistance increased between 1980 and 2010. Use the idea of evolution to explain how this may have happened. … … … … …[3] (iii) Suggest a reason why resistance to antibiotics increased faster in country A than in country B. … …[1]

4 0654/33/O/N/14 © UCLES 2014 2 (a) An electric heater is rated at 3 kW. The mains voltage is 250 V. (i) Show that the current used by the heater is 12 A. Show your working. [2] (ii) Calculate the resistance of the heater. State the formula that you use, show your working and state the unit of your answer. formula working resistance = ……………..unit ………… [3]

5 0654/33/O/N/14 © UCLES 2014 [Turn over (b) Fig. 2.1 shows the apparatus used in an experiment. N S Fig. 2.1 A current passes through a wire placed between the poles of a magnet. When the switch is closed, the wire moves upwards. Describe and explain what happens when (i) the three cells are replaced by six similar cells, … …[1] (ii) the three cells are reversed in the circuit. … …[1]

6 0654/33/O/N/14 © UCLES 2014 3 (a) The air is a mixture of gases. The two most abundant gases are nitrogen and oxygen. (i) State, to the nearest whole number, the percentage of the air that consists of gases other than nitrogen and oxygen. …[1] (ii) Name one gaseous element other than nitrogen or oxygen that is found in unpolluted air. …[1] (b) Fig. 3.1 shows containers filled with 1.0 mole of nitrogen and 1.0 mole of oxygen. 1.0 mole nitrogen 1.0 mole oxygen Fig. 3.1 The gases inside the containers are both at room temperature and pressure. (i) The volume of the nitrogen gas is 24 dm3. State the volume of the oxygen gas. …[1] (ii) Explain your answer to (i). … …[1] (iii) State one difference, other than being different elements, between 1.0 mole of nitrogen and 1.0 mole of oxygen. … …[1]

7 0654/33/O/N/14 © UCLES 2014 [Turn over (c) Nitrogen combines with hydrogen in the Haber process to form ammonia. The balanced equation for the formation of ammonia is N2 + 3H2 2NH3 (i) Nitrogen may be obtained from liquid air. Name the method used to separate nitrogen from liquid air. …[1] (ii) Name one raw material that is used to produce hydrogen for the Haber process. …[1] (iii) Work through the steps in the calculation below to find the mass of nitrogen gas that reacts to produce 1000 g of ammonia. Show your working. • Calculate the number of moles of ammonia in 1000 g. The relative formula mass of ammonia is 17. number of moles of ammonia = … • State the number of moles of nitrogen that react to produce 1000 g of ammonia. number of moles of nitrogen = … • Calculate the mass of the number of moles of nitrogen gas you found in the previous step. mass of nitrogen = … [4]

8 0654/33/O/N/14 © UCLES 2014 4 (a) Fig. 4.1 shows a car travelling from left to right. Two horizontal forces affect its motion. These are the forward driving force and air resistance. air resistance forward driving force Fig. 4.1 (i) The car is accelerating. Tick one of the boxes to show which of the following statements is correct. The driving force is greater than the air resistance. The driving force is equal to the air resistance. The driving force is less than the air resistance. Explain your answer. … …[1] (ii) The car accelerates from 16 m / s to 30 m / s in 4 seconds. The mass of the car is 1200 kg. Calculate the force required to produce this acceleration. State the formula that you use and show your working. formula used working force = … N [3]

9 0654/33/O/N/14 © UCLES 2014 [Turn over (iii) Calculate the change in kinetic energy of the car during this acceleration. State the formula that you use and show your working. formula working change in kinetic energy = … J [3] (b) Car A approaches a road junction. Fig. 4.2 shows the road junction seen from above. STOP M high wall high wall car A car B Fig. 4.2 A mirror is placed at point M to allow the driver of car A to see car B. Draw the mirror at a suitable angle to show how it should be placed so that the driver of car A can see car B. Draw a ray of light from car B which travels to the driver of car A. [3] (c) The noise vibration from the car engine can be heard by the driver. Describe in terms of air particles how the sound from the engine is heard by its driver. … … …[2]

10 0654/33/O/N/14 © UCLES 2014 5 Fig. 5.1 shows apparatus that can be used to investigate the effect of varying light intensity on the rate of photosynthesis in an aquatic plant. The light intensity is varied by changing the brightness of the lamp. test-tube containing water gas collects here bubbles produced by plant aquatic plant capillary tube water level moves down as gas is produced scale lamp light Fig. 5.1 The rate of photosynthesis is determined by measuring the rate at which the water level moves down in the capillary tube. This happens because the gas produced in photosynthesis forces the water down the tube. (a) State why light is necessary for photosynthesis. … …[1] (b) Name the gas that collects at the top of the test-tube in Fig. 5.1. … [1] (c) Write a balanced chemical equation for photosynthesis. …[2]

11 0654/33/O/N/14 © UCLES 2014 [Turn over (d) (i) Using the axes in Fig. 5.2, sketch a graph to show how the rate of photosynthesis of the plant will change as the light intensity varies from very low to very high. rate of photosynthesis very low very high light intensity Fig. 5.2 [2] (ii) Suggest reasons for the shape of your graph at low light intensities, … … at very high light intensities. … …[2] (e) Name two environmental conditions other than light intensity that affect the rate of photosynthesis. 1 … 2 …[2] (f) Only the green parts of a plant can photosynthesise. (i) Name the green substance present in plants. … [1] (ii) State why this green substance is needed for photosynthesis. …[1]

12 0654/33/O/N/14 © UCLES 2014 6 The halogens are found in Group VII of the Periodic Table. (a) Complete the table which shows some of the properties of chlorine, bromine and iodine. element physical state at 20 °C colour formula of molecules chlorine pale green bromine liquid iodine I2 [3] (b) Iodine is found combined in aqueous solutions containing sodium iodide. Iodine may be extracted from sodium iodide by reaction with chlorine. Suggest the word chemical equation for the reaction of sodium iodide with chlorine. …[1] (c) In many countries, chlorine is added to water supplied to homes. Predict and explain what may happen to people drinking the water if chlorine is not added to the supply. … … …[2]

13 0654/33/O/N/14 © UCLES 2014 [Turn over (d) Fluorine gas reacts violently with water. Fig. 6.1 shows fluorine gas being blown onto a water surface, and the two products of the reaction. hydrogen fluoride HF dissolves oxygen gas O2 fluorine gas F2 water Fig. 6.1 Use the information shown in Fig. 6.1 to construct a balanced chemical equation for the reaction of fluorine gas with water to produce oxygen gas and hydrogen fluoride. …[2]

14 0654/33/O/N/14 © UCLES 2014 7 Fig. 7.1 shows some of the stages in human reproduction. body cell in organ V body cell in the ovary sperm cell Z cell W zygote embryo Y X Fig. 7.1 (a) Name organ V and cell W. organ V … cell W … [2] (b) Name the process that is occurring at X. … [1] (c) State what type of nuclear division is occurring when the cells divide at Y and Z. at Y … at Z … [2] (d) The nucleus of the cell in the ovary contains 46 chromosomes. State the number of chromosomes present in the nuclei of cell W, … a cell from the embryo. … [2]

15 0654/33/O/N/14 © UCLES 2014 [Turn over Please turn over for Question 8.

16 0654/33/O/N/14 © UCLES 2014 8 (a) In Australia in 2010, it was decided that only energy efficient (low energy) light bulbs (lamps) should be used in houses. A scientist measures the electrical power consumption of two types of lamp. The lamps are shown in Fig. 8.1. type A energy efficient compact fluorescent lamp type B traditional incandescent light bulb Fig. 8.1 Type A is the energy efficient compact fluorescent lamp and type B is the traditional incandescent light bulb. The scientist takes three sets of measurements for each of the two types of lamp. His results are shown on the graph in Fig. 8.2.

17 0654/33/O/N/14 © UCLES 2014 [Turn over 0 1.0 2.0 3.0 4.0 5.0 6.0 useful light energy output / W 130 120 110 100 90 80 70 60 50 40 30 20 10 0 electrical power consumption / W type type A type B type A Fig. 8.2 (i) Use the data in Fig. 8.2 to calculate the difference in electrical power consumption of the two types of lamp when the light energy output is 3.0 W. … W [1] (ii) Use the data in Fig. 8.2 to calculate the efficiency of the two types of lamp. Show your working. efficiency of type A = … efficiency of type B = … [2]

18 0654/33/O/N/14 © UCLES 2014 (iii) In Australia only type A lamps can be sold in shops. Use your answer to (ii) to suggest why this decision could benefit the Australian environment. … … … …[2] (b) Power stations generate electricity. In some power stations a nuclear fuel is used. The thermal energy released in the nuclear reactor is used to turn water into steam. Complete Fig. 8.3 to show the energy transformations that take place in a nuclear power station. thermal energy in steam electrical energy output … energy … energy in turbine and generator Fig. 8.3 [2] (c) One waste product from a nuclear power station is the isotope iodine-129. This has a half-life of 15.7 million years and releases β-radiation and γ-radiation. (i) State the meaning of the term half-life. … …[1] (ii) State two differences between β-radiation and γ-radiation. 1 … 2 …[2]

19 0654/33/O/N/14 © UCLES 2014 [Turn over 9 (a) Ethane and ethene are gaseous hydrocarbons. Fig. 9.1 shows apparatus that can be used to find out whether gases react with bromine solution. bromine solution gas Fig. 9.1 In separate experiments, ethane and ethene are passed into the apparatus. Each gas is passed through the bromine solution for a few seconds at room temperature. (i) Predict how the observations in the two experiments will be different. observation with ethane … … observation with ethene … …[2] (ii) Butene, CxHy, is another gaseous hydrocarbon. State the values of x and y in the formula of butene and name the homologous series to which butene belongs. value of x … value of y … homologous series … [3]

20 0654/33/O/N/14 © UCLES 2014 (b) When ethene is compressed and heated, a white solid substance, G, is produced. Substance G is made of very large hydrocarbon molecules. Fig. 9.2 shows the structure of a small section of one of these molecules. C H H C H H C H H C H H C H H C H H Fig. 9.2 (i) Give the full name of the type of chemical reaction that occurs when ethene is converted into substance G. …[2] (ii) Name substance G. …[1] (iii) Substance G is used to make a wide range of products including plastic bags, most of which are thrown away as plastic waste. One way of getting rid of plastic waste is to burn it. State the two compounds that will be produced when substance G undergoes complete combustion. … and … [2]

21 0654/33/O/N/14 © UCLES 2014 [Turn over 10 (a) Fig. 10.1 is a plan of the human circulatory system. lungs other body tissues X Y P Q Fig. 10.1 (i) Name the blood vessel labelled X, and the chamber of the heart labelled Y. X … Y …[2] (ii) On Fig. 10.1, draw arrows to show the direction of blood flow in the vessels labelled P and Q. [2] (iii) With reference to Fig. 10.1, explain why the human circulatory system is described as a double circulation. … … …[2] (iv) Explain why the blood travelling to the lungs is at a lower pressure than the blood travelling to the rest of the body. … …[1]

22 0654/33/O/N/14 © UCLES 2014 (b) Fig. 10.2 shows how a person’s pulse can be measured by feeling the pulse at the wrist. Fig. 10.2 (i) Name the type of blood vessel in which the pulse at the wrist occurs. …[1] (ii) The pulse can be used as a way of measuring the heart rate. Explain why the beating of the heart causes a pulse at the wrist. … …[1] (iii) When a person starts to run, their pulse rate increases. Explain how this helps the person to run fast. … … …[2]

23 0654/33/O/N/14 © UCLES 2014 [Turn over 11 Fig. 11.1 shows some water being heated in a saucepan. bright silver surface heat water wooden handle Fig. 11.1 (a) Explain why the materials have been used to make the saucepan shown in Fig. 11.1. Use ideas of thermal energy transfer (heat energy) in your answer. (i) wooden handle … …[1] . (ii) bright silver surface … …[1] (b) Describe, in terms of particles, how thermal energy is transferred through the base of the saucepan by conduction and heats up all of the water by convection. … … … … … …[4]

24 0654/33/O/N/14 © UCLES 2014 (c) The weight of the saucepan and water is 15 N. The area of the saucepan in contact with the cooker is 300 cm2. Calculate the pressure exerted by the saucepan on the surface of the cooker in N / cm2. State the formula that you use and show your working. formula working pressure = … N / cm2 [2] (d) 500 g of water is heated from 20 °C to 50 °C. The thermal energy required is 63 000 J. Calculate the specific heating capacity of water. State the formula that you use and show your working. formula working specific heating capacity = … J / (kg °C) [3]

25 0654/33/O/N/14 © UCLES 2014 [Turn over 12 Aluminium is a metallic element in Group III of the Periodic Table. Iron is one of the transition metals in Period 4 of the Periodic Table. (a) State three properties of transition metals that are different from non-transition metals such as those in Groups I, II and III. 1 … 2 … 3 …[3] (b) (i) Use the Periodic Table to help you to deduce the number of electrons in one atom of iron. Explain how you chose your answer. number of electrons … explanation …[1] (ii) State the number of electrons in the outer shell of an atom of aluminium. Explain your answer. number of outer electrons … explanation … …[2]

26 0654/33/O/N/14 © UCLES 2014 (c) Fig. 12.1 shows some equipment that is used to produce molten iron for use in repairing broken steel rail track. molten iron released here reaction mixture containing aluminium and iron oxide break in steel rail track Fig. 12.1 The molten iron is a product of an exothermic reaction between aluminium and iron oxide. The balanced equation for the reaction is 2Al + Fe2O3 2Fe + Al2O3 (i) Explain, in terms of loss or gain of electrons, which atom or ion is oxidised in the reaction. particle … explanation … … …[3] (ii) State whether the products of the reaction in Fig. 12.1 contain more, less or the same quantity of chemical potential energy as the reactants. Explain your answer. … … …[2]

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28 0654/33/O/N/14 © UCLES 2014 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.). 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. 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.

® 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 2014 series 0654 CO-ORDINATED SCIENCES 0654/33 Paper 3 (Extended Theory), maximum raw mark 120 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 2014 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 2014 0654 33 © Cambridge International Examinations 2014 1 (a) variation ; adaptation ; survive ; selection ; [4] (b) (i) (in 1980) no (significant) difference ; (in 2010) higher in country A / ORA ; [2] (ii) mutation produces resistant variety ; some bacteria more resistant than others / some bacteria are resistant ; antibiotics in (frequent) use ; resistant bacteria more likely to survive / natural selection / ORA ; and reproduce to pass on this resistance ; [max 3] (iii) more / incorrect antibiotic use in country A / ORA ; [1] [Total: 10] 2 (a) (i) 3000 (W) shown ; = 250 3000 (= 12 A) ; [2] (ii) (resistance =) current voltage ; 12 250 = 20.8 or 21 ; Ω ; [3] (b) (i) (larger current so) wire moves (upwards) higher / quicker / with more force ; [1] (ii) (current reversed so) wire moves downwards / direction reverses / force acts downwards ; [1] [Total: 7] 3 (a) (i) 1(%) ; [1] (ii) any noble gas ; [1] (b) (i) 24 dm3 ; [1] (ii) reference to the idea that 1 mole of any gas at room temperature and pressure has a volume of 24 dm3 / 1 mole of any gas under same conditions occupies the same volume ; [1] (iii) nitrogen has lower / different mass / lower density ; [1]

Page 3 Mark Scheme Syllabus Paper Cambridge IGCSE – October/November 2014 0654 33 © Cambridge International Examinations 2014 (c) (i) fractional distillation ; [1] (ii) hydrocarbon / named alkane / petroleum / water ; [1] (iii) 1000 ÷ 17 = 58.8(24) or 59 ; 58.8 ÷ 2 = 29.4(12) ; Mr N2 = 28 ; 29.4 × 28 = 823.2 g (unit required) ; [4] [Total: 11] 4 (a) (i) (positive acceleration: driving force is greater than air resistance OR negative acceleration: driving force is less than air resistance) there is a resultant / net force / sum of forces is not zero ; [1] (ii) (force =) mass × acceleration ; acceleration = 3.5 (m / s2) ; = 1200 × (3.5) = 4200 (N) ; [3] (iii) (KE =) ½ mv2 ; initial KE = 153 600 and final KE = 540 000 (J) ; difference = 540 000 – 153 600 = 386 400 (J) ; [max 3] (b) mirror drawn at suitable angle ; ray of light drawn from car B reflects off mirror to car A indicated by arrow ; angles between rays and mirror approximately correct ; [3] (c) engine vibration causes air particles to vibrate ; energy / vibrations passed from particle to particle ; compressions and rarefactions ; [max 2] [Total: 12]

Page 4 Mark Scheme Syllabus Paper Cambridge IGCSE – October/November 2014 0654 33 © Cambridge International Examinations 2014 5 (a) as an energy source ; [1] (b) oxygen ; [1] (c) 6CO2 + 6H2O → C6H12O6 + 6O2 formulae ; balancing ; [2] (d) (i) straight line for first part of graph ; levelling off at higher intensity ; [2] (ii) (at low) more light means more energy available / more light energy speeds up rate ; (at very high) not enough CO2 / plant photosynthesising as fast as it can / another limiting factor / limiting factor ; [2] (e) temperature ; CO2 concentration ; wavelength / frequency / colour of light ; rainfall / water / humidity ; lack of magnesium ; [max 2] (f) (i) chlorophyll ; [1] (ii) to absorb the light / energy ; [1] [Total: 12] rate of photosynthesis very low very high light intensity

Page 5 Mark Scheme Syllabus Paper Cambridge IGCSE – October/November 2014 0654 33 © Cambridge International Examinations 2014 6 (a) element physical state at 20 °C colour formula of molecules chlorine gas (pale green) Cl2 bromine (liquid) orange / brown Br2 iodine solid / crystals dark grey / black (I2) ;;; (1 mark for each correct column) [3] (b) chlorine + sodium iodide → iodine + sodium chloride ; [1] (c) become ill / be poisoned / might die ; because harmful microorganisms would not be killed ; [2] (d) 2F2 + 2H2O → O2 + 4HF formulae ; balanced ; [2] [Total: 8] 7 (a) V = testis ; W = ovum / egg ; [2] (b) fertilisation ; [1] (c) at Y = mitosis ; at Z = meiosis ; [2] (d) W = 23 ; embryo = 46 ; [2] [Total: 7]

Page 6 Mark Scheme Syllabus Paper Cambridge IGCSE – October/November 2014 0654 33 © Cambridge International Examinations 2014 8 (a) (i) 68 (W) ; [1] (ii) working for A OR B ; A = 25% and B = 3.75% ; [2] (iii) A is more efficient than B / less energy consumed ; valid environmental statement e.g. less fossil fuels burned / non-renewable resources used / less CO2 released ; [2] (b) nuclear ; kinetic ; [2] (c) (i) time taken for half the atoms / nuclei to decay / time for radioactivity to fall to half ; [1] (ii) β particles and γ wave ; β more ionising ; β less penetrating ; β has charge and γ has no charge ; β has mass and γ has no mass ; [max 2] [Total: 10] 9 (a) (i) with ethane no colour change / stays orange ; with ethene orange solution becomes colourless ; [2] (ii) x is 4 ; y is 8 ; alkenes ; [3] (b) (i) polymerisation ; addition (polymerisation) ; [2] (ii) poly(ethene) ; [1] (iii) carbon dioxide ; water ; [2] [Total: 10]

Page 7 Mark Scheme Syllabus Paper Cambridge IGCSE – October/November 2014 0654 33 © Cambridge International Examinations 2014 other body tissues lungs P Q 10 (a) (i) X = pulmonary vein ; Y = right atrium ; [2] (ii) correct arrow on P ; correct arrow on Q ; [2] (iii) blood flows twice through the heart (for each complete circuit) ; through lungs, then through body tissues / v.v. ; idea of separate oxygenated and deoxygenated blood ; [max 2] (iv) blood has less far to travel / flows through fewer capillaries / organs ; right (ventricle of) heart has less muscle ; [max 1] (b) (i) artery ; [1] (ii) surge of blood / pressure into the vessel ; vessel wall stretches (and recoils) with each beat ; [max 1] (iii) more blood to muscles ; so more oxygen / glucose ; removes more CO2 ; increased respiration ; increased energy released ; [max 2] [Total: 11]

Page 8 Mark Scheme Syllabus Paper Cambridge IGCSE – October/November 2014 0654 33 © Cambridge International Examinations 2014 11 (a) (i) poor (heat) conductor / idea of heat not passing through handle ; [1] (ii) shiny / silver surface poor heat emitter ; [1] (b) (in base of saucepan) increased particle movement / vibration / kinetic energy ; energy transferred by collision, vibration / energy, passed from particle to particle ; (in water) water particles move further apart ; less dense water rises ; [4] (c) (pressure =) area force ; = 300 15 = 0.05 (N / cm2) ; [2] (d) (c =) θ m H or T m H ∆ ; ( ) 30 0.5 000 63 × ; = 4200 (J / kg °C) ; [3] [Total: 11] 12 (a) transition metals have high density ; transition metals (and compounds) can act as catalysts ; transition metals (often) form coloured compounds ; transition metals have high melting / boiling points ; reference to variable oxidation states / valency ; [max 3] (b) (i) (26) same as proton number ; [1] (ii) 3 ; same as Group number ; electrons arranged in 2,8,3 ; [max 2] (c) (i) aluminium atom / Al ; becomes a positive ion ; (aluminium atoms) lose electrons (when they ionise) / electron loss is oxidation / electrons transferred to iron (ions) / oilrig explained ; [max 3]

Page 9 Mark Scheme Syllabus Paper Cambridge IGCSE – October/November 2014 0654 33 © Cambridge International Examinations 2014 (ii) less ; reaction is exothermic ; chemical energy in reactants has been transferred to surroundings / changed to thermal energy (and so less in products) ; [max 2] [Total: 11]