Chemistry/Science Unit 1: Chemistry in Our World
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1 Write your name here Surname Other names Edexcel GCSE Centre Number Chemistry/Science Unit 1: Chemistry in Our World Candidate Number Thursday 1 March 2012 Morning Time: 1 hour You must have: Calculator, ruler Higher Tier Paper Reference 5CH1H/01 Total Marks Instructions Use black ink or ball-point pen. Fill in the boxes at the top of this page with your name, centre number and candidate number. Answer all questions. Answer the questions in the spaces provided there may be more space than you need. Information The total mark for this paper is 60. The marks for each question are shown in brackets use this as a guide as to how much time to spend on each question. Questions labelled with an asterisk (*) are ones where the quality of your written communication will be assessed you should take particular care with your spelling, punctuation and grammar, as well as the clarity of expression, on these questions. Advice Read each question carefully before you start to answer it. Keep an eye on the time. Try to answer every question. Check your answers if you have time at the end. Turn over P40198A 2012 Pearson Education Ltd. 1/1/1/1/ *P40198A0120*
2 The Periodic Table of the Elements Li lithium 3 23 Na sodium K potassium 19 9 Be beryllium 4 24 Mg magnesium Ca calcium Sc scandium 21 Key relative atomic mass atomic symbol name atomic (proton) number 48 Ti titanium V vanadium Cr chromium Mn manganese 25 1 H hydrogen 1 56 Fe iron Co cobalt Ni nickel Cu copper Zn zinc B boron 5 27 Al aluminium Ga gallium C carbon 6 28 Si silicon Ge germanium N nitrogen 7 31 P phosphorus As arsenic O oxygen 8 32 S sulfur Se selenium F fluorine Cl chlorine Br bromine 35 4 He helium 2 20 Ne neon Ar argon Kr krypton Rb rubidium Sr strontium Y yttrium Zr zirconium Nb niobium Mo molybdenum 42 [98] Tc technetium Ru ruthenium Rh rhodium Pd palladium Ag silver Cd cadmium In indium Sn tin Sb antimony Te tellurium I iodine Xe xenon Cs caesium Ba barium La* lanthanum Hf hafnium Ta tantalum W tungsten Re rhenium Os osmium Ir iridium Pt platinum Au gold Hg mercury Tl thallium Pb lead Bi bismuth 83 [209] Po polonium 84 [210] At astatine 85 [222] Rn radon 86 [223] Fr francium 87 [226] Ra radium 88 [227] Ac* actinium 89 [261] Rf rutherfordium 104 [262] Db dubnium 105 [266] Sg seaborgium 106 [264] Bh bohrium 107 [277] Hs hassium 108 [268] Mt meitnerium 109 [271] Ds darmstadtium 110 [272] Rg roentgenium 111 Elements with atomic numbers have been reported but not fully authenticated * The lanthanoids (atomic numbers 58-71) and the actinoids (atomic numbers ) have been omitted. The relative atomic masses of copper and chlorine have not been rounded to the nearest whole number. 2 *P40198A0220*
3 BLANK PAGE TURN OVER FOR QUESTION 1 *P40198A0320* 3 Turn over
4 Answer ALL questions. Some questions must be answered with a cross in a box. If you change your mind about an answer, put a line through the box and then mark your new answer with a cross. Useful products from crude oil 1 Fractional distillation is used to separate crude oil into fractions. A fractionating column is used for the process. The diagram shows a fractionating column and the fractions obtained when crude oil is fractionally distilled. (a) Which of the following statements is true? Put a cross ( ) in the box next to your answer. A fuel oil has a lower boiling point than petrol B kerosene is more viscous than bitumen C molecules in diesel oil are larger than molecules in petrol D diesel oil is easier to ignite than petrol (b) Some fractions obtained from crude oil are cracked to produce alkenes. (i) crude oil Explain what is meant by cracking. fraction gases petrol kerosene diesel oil fuel oil bitumen 4 *P40198A0420*
5 (ii) One alkene obtained is ethene. The diagram shows the structure of a molecule of ethene. H H C C H H Ethene is unsaturated. Ethene is a hydrocarbon. Explain why ethene is described as an unsaturated hydrocarbon. (3) (iii) Describe what you would see when a sample of ethene is shaken with bromine water. (Total for Question 1 = 8 marks) *P40198A0520* 5 Turn over
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7 Gases in the atmosphere 2 (a) The table shows possible percentages of some of the gases in the Earth s early atmosphere. (i) oxygen nitrogen gas percentage in early atmosphere (%) small amount small amount carbon dioxide 12 water vapour 77 Some time after the early atmosphere had been formed, oceans appeared on the Earth s surface. State how these oceans were formed. (ii) The amount of carbon dioxide in today s atmosphere is much lower than that in the early atmosphere. State how the formation of the oceans caused this reduction. (iii) The amount of oxygen in today s atmosphere is much higher than that in the early atmosphere. Describe the process that has caused this increase. *P40198A0720* 7 Turn over
8 (b) John was doing an experiment to find the percentage of oxygen in air at room temperature. He used this apparatus. copper powder heat gas syringe The copper powder in the test tube was heated strongly so that it could react with oxygen in the air in the apparatus. John stopped heating the copper when there was no further change in the reading on the gas syringe. (i) Complete the sentence by putting a cross ( ) in the box next to your answer. At the end of the experiment the apparatus was allowed to cool before the final reading on the syringe was recorded. This is because A reading the volume while the apparatus is hot is dangerous B the apparatus must be left to allow the reaction to finish C the gas must be at room temperature when its volume is measured D the copper expands when it is hot (ii) At the end of the experiment not all of the copper had reacted. Suggest a reason for this. 8 *P40198A0820*
9 (iii) John s results were initial volume of gas in syringe = 32 cm 3 final volume of gas in syringe = 24 cm 3 Calculate the percentage decrease in the volume of gas originally in the syringe. percentage decrease =... (iv) The percentage of oxygen in air at room temperature is 21%. John thought the answer to part (iii) was the percentage of oxygen in air and was surprised that the value was too high. John confirmed that he had not made an error when doing his experiment. Suggest why the answer calculated in part (iii) is higher than John expected. (Total for Question 2 = 9 marks) *P40198A0920* 9 Turn over
10 Metals 3 Metals have many uses. (a) Complete the sentence by putting a cross ( ) in the box next to your answer. Aluminium and magnesium are melted together to form magnalium. Magnalium is A an element B an ore C an alloy D a type of steel (b) Describe how iron is extracted from its ore. (c) Copper oxide reacts with hydrogen to form copper and water. The equation for the reaction is CuO + H 2 Cu + H 2 O Explain how this reaction involves both oxidation and reduction. (3) 10 *P40198A01020*
11 (d) Some modern spectacle frames are made of shape memory alloys. Explain why shape memory alloys are better than other alloys for making spectacle frames. (e) Complete the sentence by putting a cross ( ) in the box next to your answer. Alloys are usually stronger than the pure metals from which they are made because they A have stronger bonds between the molecules they contain B combine the properties of the metals from which they are made C have atoms of different sizes in their structures D are made using electrolysis (Total for Question 3 = 9 marks) *P40198A01120* 11 Turn over
12 Rocks 4 A student produced this sketch of a quarry face. Y soil limestone granite marble (a) The limestone shown was originally formed in layers. State what type of rock limestone is. (b) Granite is an igneous rock formed from magma. (i) X Explain how the marble has formed above the granite. (ii) Explain why the rock at X contained larger crystals than the rock at Y. 12 *P40198A01220*
13 (c) Limestone is a natural form of calcium carbonate. When calcium carbonate, CaCO 3, is heated it decomposes. (i) Complete the equation for this reaction. CaCO 3 CaO +... (ii) Calcium oxide reacts with water to form calcium hydroxide. Write the balanced equation for this reaction. (iii) Explain why calcium hydroxide (slaked lime) is spread on fields. (Total for Question 4 = 10 marks) *P40198A01320* 13 Turn over
14 Chemical reactions 5 (a) Complete the sentence by putting a cross ( ) in the box next to your answer. When dilute hydrochloric acid reacts with copper oxide one of the products is A copper B copper hydroxide C copper chlorate D copper chloride (b) Chlorine is manufactured by electrolysis. Explain what is meant by electrolysis. (c) Chlorine gas reacts with sodium hydroxide solution to form sodium chlorate(i), NaOCl, sodium chloride and water. Write the balanced equation for this reaction. (3) 14 *P40198A01420*
15 *(d) Sulfur is an impurity in some fossil fuels. Explain how the presence of sulfur in fossil fuels can lead to damage to the environment and how the amount of damage can be reduced. (6) (Total for Question 5 = 12 marks) *P40198A01520* 15 Turn over
16 Burning fuels 6 The picture shows a gas water heater. The fuel used in this heater is natural gas which is mainly methane. (a) Complete the sentence by putting a cross ( ) in the box next to your answer. Natural gas is a good fuel because A supplies of it will never run out B it always burns with a yellow flame that is easily seen C it produces no waste gases on complete combustion D it produces no solid waste on complete combustion (b) The complete combustion of fossil fuels releases gases into the atmosphere. Explain how these gases could cause an increase in the temperature of the Earth. (c) Biofuels, made from plants, can be used as alternatives to fossil fuels. (i) State an advantage of replacing fossil fuels with biofuels made from plants. 16 *P40198A01620*
17 (ii) Explain a disadvantage of replacing fossil fuels with biofuels made from plants. *(d) Incomplete combustion of methane can occur in gas heaters such as the one shown in the photograph. Explain how incomplete combustion occurs and the problems it can cause. (6) (Total for Question 6 = 12 marks) total for paper = 60 marks *P40198A01720* 17
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