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UK GCSE 2009 : Higher Tier, Chemistry Paper 1

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Centre Number 71 Candidate Number General Certificate of Secondary Education 2009 Paper 1 Higher Tier G1403 Science: Chemistry [G1403] THURSDAY 4 JUNE, MORNING TIME 1 hour 30 minutes. INSTRUCTIONS TO CANDIDATES Write your Centre Number and Candidate Number in the spaces provided at the top of this page. Write your answers in the spaces provided in this question paper. Answer all five questions. INFORMATION FOR CANDIDATES The total mark for this paper is 120. Quality of written communication will be assessed in question 4(d)(iii). Figures in brackets printed down the right-hand side of pages indicate the marks awarded to each question or part question. A Data Leaflet which includes a Periodic Table of the Elements is provided. For Examiner s use only Question Number 1 2 3 4 5 Total Marks 4536 Marks 1 (a) All playstations and games consoles contain a microchip made from the element silicon which has the symbol Si and atomic number 14. Examiner Only Marks Remark AP/Press Association Images (i) What is meant by the term element? ______________________________________________________ ___________________________________________________ [2] (ii) What is meant by the term atomic number? ___________________________________________________ [1] (b) An atom of silicon contains protons, electrons and neutrons. Complete the table below to show the relative mass and relative charge of each particle. Particle Relative mass Relative charge proton electron neutron [3] 4536 2 [Turn over (c) Silicon has 3 stable isotopes, 28Si, 29Si and 30Si. Examiner Only Marks Remark (i) Complete the table below to give the number of protons, electrons and neutrons present in one atom of each of the isotopes of silicon. Isotope Number of protons Number of electrons Number of neutrons 28Si 29Si 30Si [3] (ii) Explain what you understand by the term isotope. ______________________________________________________ ___________________________________________________ [2] (d) Silicon is rarely found in nature in its uncombined form, but is found as silicon dioxide (quartz) or in minerals called silicates, many of which contain the silicate(IV) ion. (i) Complete the table to give information about silicon dioxide, SiO2 (quartz). Type of bonding present in silicon dioxide Type of structure of silicon dioxide [2] 4536 3 [Turn over (ii) Given that the formula of the silicate(IV) ion is SiO4 , write the 4 formula of sodium silicate. Examiner Only Marks Remark ___________________________________________________ [1] (iii) The structure of sodium silicate is a giant ionic lattice. State two physical properties of sodium silicate. 1. ____________________________________________________ 2. _________________________________________________ [2] (e) Very pure silicon is needed to make microchips. One method originally used to produce pure silicon involved reacting silicon tetrachloride, SiCl4, with metallic zinc at 950 C. The word equation for this reaction is: silicon tetrachloride + zinc silicon + zinc chloride (i) Write a balanced symbol equation for this reaction. ___________________________________________________ [3] (ii) Describe the structure and bonding in zinc metal. You may use a labelled diagram to help answer this question. ______________________________________________________ ______________________________________________________ ___________________________________________________ [3] 4536 4 [Turn over (f) Another method of producing silicon in industry is by the reaction of silicon dioxide with charcoal in an electric arc furnace. Examiner Only Marks Remark SiO2 + C Si + CO2 The carbon reduces the silicon dioxide. The reaction is exothermic. (i) Explain in terms of bond breaking and bond making why this reaction is exothermic. ______________________________________________________ ______________________________________________________ ______________________________________________________ ______________________________________________________ ______________________________________________________ ______________________________________________________ ______________________________________________________ ______________________________________________________ ___________________________________________________ [5] (ii) Explain why SiO2 is described as being reduced in this reaction. ______________________________________________________ ______________________________________________________ ___________________________________________________ [2] 4536 5 [Turn over 2 (a) Two iron nails were placed in separate test tubes containing water. The nail in test tube A was galvanised, but the nail in test tube B was not. After a few days, the nail in test tube B had rusted. Examiner Only Marks Remark test tube rack A B (i) State one observation which would indicate that rusting is a chemical reaction. ______________________________________________________ ___________________________________________________ [1] (ii) What material is used to galvanise iron? ___________________________________________________ [1] (iii) State two other methods which could be used to prevent iron from rusting. 1. _________________________________________________ [1] 2. _________________________________________________ [1] (iv) The chemical name for rust is hydrated iron(III) oxide. What is meant by the term hydrated? ______________________________________________________ ___________________________________________________ [1] 4536 6 [Turn over (b) Many chemical rust removers contain acids such as sulphuric acid. The rust is removed in a chemical reaction. Examiner Only Marks Remark A rusty iron nail is placed in a solution of sulphuric acid for a few days. The rust disappears and the solution changes colour. (i) Write a balanced symbol equation for the reaction of iron(III) oxide with sulphuric acid. ___________________________________________________ [3] (ii) The nail was removed from the solution and a few drops of aqueous ammonia solution were added to the remaining solution. What would you observe? ___________________________________________________ [2] (c) Copper metal is used for roofing. Copper reacts over time forming copper(II) oxide which reacts further with carbon dioxide in the air to form copper(II) carbonate. Acids will react with copper(II) carbonate. (i) Write a balanced symbol equation for the reaction of copper with oxygen in the air forming copper(II) oxide. ___________________________________________________ [3] (ii) Write a balanced symbol equation for the reaction of copper(II) oxide with carbon dioxide forming copper(II) carbonate. ___________________________________________________ [2] (iii) State the colours of: copper _________________________________ copper(II) oxide _________________________________ copper(II) carbonate _________________________________ [3] (iv) Name the acid which reacts with copper(II) carbonate to form a solution of copper(II) sulphate. ___________________________________________________ [1] 4536 7 [Turn over (d) Magnesium reacts with copper(II) sulphate solution according to the equation Examiner Only Marks Remark Mg + CuSO4 MgSO4 + Cu The reaction may be described as a redox reaction. Explain in terms of electrons why this reaction may be described as a redox reaction. You may use ionic equations to help answer this question. _________________________________________________________ _________________________________________________________ _________________________________________________________ _________________________________________________________ _________________________________________________________ _________________________________________________________ ______________________________________________________ [7] 4536 8 [Turn over BLANK PAGE (Questions continue overleaf) 4536 9 [Turn over 3 (a) The diagram below shows the apparatus used to carry out the electrolysis of copper(II) sulphate solution. Graphite electrodes are used. Examiner Only Marks Remark + anode cathode copper(II) sulphate solution (i) What is meant by the term electrolysis? ______________________________________________________ ______________________________________________________ ___________________________________________________ [2] (ii) During the electrolysis of copper(II) sulphate solution, the ions present in the solution are attracted to the electrodes where they may be discharged. The table below gives some of the details of the ions and the electrode to which they are attracted. Complete the table. You may find your Data Leaflet useful in answering this question. Name of ion Attracted to positive electrode Copper(II) Attracted to negative electrode Formula of ion (including charge) SO2 4 H+ Hydroxide [6] 4536 10 [Turn over (b) The apparatus shown below is used to carry out the electrolysis of dilute sulphuric acid using platinum electrodes. gas A Remark gas B anode Examiner Only Marks cathode dilute sulphuric acid + (i) Name gases A and B. Gas A ________________________________________________ Gas B _____________________________________________ [2] (ii) Write half equations for the reactions occurring at the anode and the cathode during the electrolysis of dilute sulphuric acid. Anode ____________________________________________ [3] Cathode ____________________________________________ [3] 4536 11 [Turn over 4 In the laboratory, gases are made from the reaction between a solid and a solution. Two such gases are chlorine and hydrogen chloride. (a) The diagram below shows apparatus used to prepare chlorine gas in the laboratory. solution B cover chlorine gas silica gel solid A Examiner Only Marks Remark (i) Name solid A and solution B. Solid A _____________________________________________ [1] Solution B __________________________________________ [2] (ii) Suggest the purpose of the silica gel. ___________________________________________________ [1] 4536 12 [Turn over (b) Chlorine gas reacts with hydrogen gas to form hydrogen chloride. Examiner Only Marks Remark (i) Write a balanced symbol equation for the reaction between chlorine gas and hydrogen gas. ___________________________________________________ [3] (ii) Suggest two safety measures which should be taken when carrying out the reaction. 1. ____________________________________________________ 2. _________________________________________________ [2] (c) The diagram below shows the apparatus commonly used to produce hydrogen chloride gas in the laboratory. solution D cover hydrogen chloride gas solid C (i) Name solid C and solution D. Solid C _____________________________________________ [1] Solution D _________________________________________ [2] (ii) Describe what would be observed during the reaction. ______________________________________________________ ___________________________________________________ [2] 4536 13 [Turn over (d) In industry, ammonia gas is made from the reaction between nitrogen gas and hydrogen gas in the Haber Process. Examiner Only Marks Remark (i) Write a balanced symbol equation for the production of ammonia gas in the Haber Process. ___________________________________________________ [3] (ii) Complete the table below, giving the operating conditions used in the Haber Process. Name of catalyst Temperature ( C) Pressure (atm) [3] (iii) Describe a chemical test for ammonia gas and state the result for a positive test. ______________________________________________________ ______________________________________________________ ______________________________________________________ ______________________________________________________ ___________________________________________________ [4] Quality of written communication 4536 [2] 14 [Turn over BLANK PAGE (Questions continue overleaf) 4536 15 [Turn over 5 Oxides and hydroxides of metals are solids at room temperature and pressure. Many oxides of non-metals are gases. Examiner Only Marks Remark (a) 2.74 g of a sample of solid oxide of lead, Pb3O4, decomposes when heated according to the equation below. 2Pb3O4(s) 6PbO(s) + O2(g) The decomposition is carried out in a fume cupboard using the apparatus shown below. glowing splint Pb3O4 clamp HEAT Adapted from: http://www.practicalchemistry.org/data/images/originals/heatingsolidstesttubes-76.jpg (i) What would happen to the glowing splint? ___________________________________________________ [1] (ii) Calculate the mass of PbO which would be formed on heating 2.74 g of Pb3O4 to constant mass. (Relative atomic masses: O = 16; Pb = 207) [5] 4536 16 [Turn over (iii) Calculate the volume of oxygen gas which would be produced by heating this sample to constant mass. (1 mole of any gas occupies a volume of 24 000 cm3) Examiner Only Marks Remark Volume of oxygen gas = _____________ cm3 [2] (b) Sulphur dioxide is an oxide of the non-metal sulphur. It can be produced in the reaction of sodium thiosulphate, Na2S2O3, with hydrochloric acid, HCl. Na2S2O3 + 2HCl 2NaCl + S + SO2 + H2O A solution of sodium thiosulphate is prepared by dissolving 5.53 g of Na2S2O3 in deionised water. The hydrochloric acid has a concentration of 2 mol/dm3 (moles per litre). (i) Calculate the number of moles of sodium thiosulphate used. (Relative atomic masses: Na = 23, S = 32, O = 16) [2] (ii) Calculate the number of moles of hydrochloric acid required to react with this number of moles of sodium thiosulphate in (b)(i). [2] 4536 17 [Turn over (iii) Calculate the volume of hydrochloric acid required to react completely with the sodium thiosulphate solution. Examiner Only Marks Remark [2] (c) An insoluble unknown metal hydroxide can be written M(OH)2 where M represents the metal M. 3.0 g of solid M(OH)2 is added to 50.0 cm3 of 1 mol/dm3 (moles per litre) hydrochloric acid with stirring. Some solid M(OH)2 is observed lying at the bottom. The solution is filtered and the residue washed with some water and dried. The mass of unreacted M(OH)2 is 0.55 g. (i) What mass of M(OH)2 reacted with the hydrochloric acid? ___________________________________________________ [1] (ii) Calculate the number of moles of hydrochloric acid used. [2] 4536 18 [Turn over (iii) Using the balanced symbol equation Examiner Only Marks Remark M(OH)2 + 2HCl MCl2 + 2H2O Calculate the number of moles of M(OH)2 required to react with the hydrochloric acid. [2] (iv) Using the answers to (c)(i) and (c)(iii) above, calculate the Relative Formula Mass (RFM) of M(OH)2. [2] (v) Determine the Relative Atomic Mass (RAM) of M and identify it using your Periodic Table. RAM of M ____________________________________________ ______________________________________________________ Identity of M _______________________________________ [2] THIS IS THE END OF THE QUESTION PAPER 4536 19 [Turn over Permission to reproduce all copyright material has been applied for. In some cases, efforts to contact copyright holders may have been unsuccessful and CCEA will be happy to rectify any omissions of acknowledgement in future if notified. 938-022-1 [Turn over

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