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UK GCSE 2007 : Higher Tier, Chemistry Paper 1

24 pages, 61 questions, 1 questions with responses, 1 total responses,

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Centre Number 71 Candidate Number General Certificate of Secondary Education 2007 Paper 1 Higher Tier G1403 Science: Chemistry [G1403] WEDNESDAY 13 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(a)(iv). 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 G141H7 2556 Marks BLANK PAGE G141H7 2556 2 [Turn over 1 (a) The element chlorine exists as diatomic molecules. The diagram below represents the bonding in a chlorine molecule. Examiner Only Marks Remark C1 C1 (i) Explain why chlorine exists as diatomic molecules rather than as chlorine atoms. ______________________________________________________ ___________________________________________________ [1] (ii) Name the type of bonding found in a chlorine molecule. ___________________________________________________ [1] (iii) Explain as fully as possible how the two chlorine atoms bond together. ______________________________________________________ ___________________________________________________ [2] (b) The element chlorine reacts with metals like sodium and calcium to form metal chlorides. (i) Write the formula of sodium chloride. ___________________________________________________ [1] G141H7 2556 3 [Turn over (ii) Explain in detail how atoms of calcium combine with atoms of chlorine to form calcium chloride. You must use a diagram in your answer. Examiner Only Marks Remark ______________________________________________________ ______________________________________________________ ______________________________________________________ ___________________________________________________ [6] (iii) What type of bonding is found in calcium chloride? ___________________________________________________ [1] (c) The physical properties of a substance depend on its bonding and structure. For each of the following substances, describe the structure and state two physical properties of the substance. (i) Methane, CH4 Structure: __________________________________________ [1] Physical Properties: 1. ___________________________________________________ 2. ________________________________________________ [2] G141H7 2556 4 [Turn over (ii) Diamond Examiner Only Marks Remark Structure: __________________________________________ [1] Physical Properties: 1. ___________________________________________________ 2. ________________________________________________ [2] (iii) Sodium oxide, Na2O Structure: __________________________________________ [1] Physical Properties: 1. ___________________________________________________ 2. ________________________________________________ [2] (d) Describe the bonding and structure in a typical metal like sodium. You may use a labelled diagram to help answer this question. _________________________________________________________ _________________________________________________________ _________________________________________________________ ______________________________________________________ [3] G141H7 2556 5 [Turn over 2 (a) Most of our fuels come from animals and plants that lived millions of years ago. Fuels formed in this way are called fossil fuels and they are non-renewable fuels. Propane is a non-renewable fuel. Examiner Only Marks Remark (i) Name the homologous series of organic compounds to which propane belongs. ___________________________________________________ [1] (ii) Write a balanced symbol equation to show the complete combustion of propane. ___________________________________________________ [3] (iii) Explain what you understand by the term non-renewable. ______________________________________________________ ___________________________________________________ [2] (b) Ethanoic acid is a weak acid and is the main constituent of vinegar. (i) Write the molecular formula of ethanoic acid. ___________________________________________________ [1] (ii) Draw the full structural formula of ethanoic acid, showing all bonds. [2] G141H7 2556 6 [Turn over (c) Ethanoic acid behaves as a typical dilute acid. A student decided to investigate some of the reactions of ethanoic acid. Examiner Only Marks Remark (i) Some copper carbonate was added to a solution of ethanoic acid with stirring. Describe the observations the student would make during this reaction. ______________________________________________________ ______________________________________________________ ______________________________________________________ ___________________________________________________ [3] (ii) A strip of magnesium metal was added to a solution of ethanoic acid. State the name of the gas given off during this reaction and describe a test which could be carried out to confirm the presence of this gas. Gas ______________________________________________ [1] Test __________________________________________________ ______________________________________________________ ___________________________________________________ [2] (iii) Finally some sodium hydroxide solution was mixed with a solution of ethanoic acid. State the name and write the formula of the salt produced. Name _____________________________________________ [1] Formula ___________________________________________ [1] G141H7 2556 7 [Turn over (d) Esters are organic compounds which occur naturally in fruits. One such ester, ethyl ethanoate, can be produced by reacting ethanol with ethanoic acid. Examiner Only Marks Remark (i) Write a balanced symbol equation for the formation of ethyl ethanoate. ___________________________________________________ [2] (ii) What conditions are required for the preparation of ethyl ethanoate in the laboratory? ______________________________________________________ ______________________________________________________ ___________________________________________________ [3] (iii) Draw the structural formula of ethyl ethanoate, showing all bonds. [2] (iv) State one use of ethyl ethanoate. ___________________________________________________ [1] G141H7 2556 8 [Turn over 3 Many calcium containing compounds such as limestone (calcium carbonate) and gypsum (hydrated calcium sulphate) occur naturally. Examiner Only Marks Remark (a) Plaster of Paris is formed by heating gypsum to just above 100 C: 1 1 CaSO4.2H2O CaSO4. H2O + 1 H2O 2 2 gypsum plaster of Paris (i) Calculate the percentage of water present in gypsum. [3] (ii) State one other use of calcium sulphate. ___________________________________________________ [1] (iii) What is meant by the term hydrated? ___________________________________________________ [1] G141H7 2556 9 [Turn over (b) In industry, limestone undergoes thermal decomposition to make quicklime (calcium oxide). The diagram below represents a limekiln which is used for this process. Excess air and gas A Examiner Only Marks Remark Limestone and coke Blast of air Quicklime (i) What is meant by the term thermal decomposition? ______________________________________________________ ___________________________________________________ [2] (ii) Write a balanced symbol equation for the thermal decomposition of limestone. ___________________________________________________ [2] (iii) The decomposition of limestone is endothermic. What is the meaning of the term endothermic? ______________________________________________________ ___________________________________________________ [2] (iv) Name the main element present in coke. ___________________________________________________ [1] (v) Explain why air is blown into the kiln. ______________________________________________________ ___________________________________________________ [1] G141H7 2556 10 [Turn over (vi) Name gas A which escapes from the top of the kiln. Examiner Only Marks Remark ___________________________________________________ [1] (vii) State one other use of calcium carbonate. ___________________________________________________ [1] (c) In the laboratory, calcium carbonate reacts with hydrochloric acid to produce calcium chloride solution. (i) Write a balanced symbol equation for this reaction. ___________________________________________________ [3] (ii) State two observations you would make during this reaction. ______________________________________________________ ______________________________________________________ ___________________________________________________ [2] (iii) Sodium hydroxide solution is added slowly to the solution of calcium chloride. What would you observe? ______________________________________________________ ___________________________________________________ [2] (iv) A flame test is carried out using the solution of calcium chloride. State the flame colour observed. ___________________________________________________ [1] G141H7 2556 11 [Turn over 4 Lignite is a young coal which is brown in colour and has a high moisture and carbon content. Examiner Only Marks Remark (a) A sample of lignite was heated in a boiling tube. Drops of water were formed at the top of the boiling tube and the lignite changed colour from brown to grey. clamp drops of water lignite HEAT stand (i) What piece of equipment is used to heat the sample of lignite? ___________________________________________________ [1] (ii) State one safety precaution you would take when carrying out this experiment. ___________________________________________________ [1] (iii) Explain how the drops of water at the top of the boiling tube have formed. ______________________________________________________ ______________________________________________________ ___________________________________________________ [2] G141H7 2556 12 [Turn over (iv) Describe a chemical test for water and state the result for a positive test. Examiner Only Marks Remark ______________________________________________________ ______________________________________________________ ___________________________________________________ [3] Quality of written communication [2] (b) Major deposits of lignite have been found at three different sites in Northern Ireland. Lignite develops underground through bacterial action on peat. Peat is cut from peat bogs and dried, whereas lignite, like coal, must be mined. Both lignite and peat are used as fuels. Coal mine Peat bog (i) Explain why peat is dried after being cut from the bog. ______________________________________________________ ___________________________________________________ [2] (ii) Describe one negative effect of peat extraction on the local environment. ______________________________________________________ ___________________________________________________ [1] (iii) Suggest two reasons why local residents would be opposed to lignite mining in their area. 1. ____________________________________________________ ______________________________________________________ 2. ____________________________________________________ ___________________________________________________ [2] G141H7 2556 13 [Turn over (iv) Suggest one positive effect of a lignite mine for the local community. Examiner Only Marks Remark ______________________________________________________ ___________________________________________________ [1] (c) Waste materials in Northern Ireland are either recycled or they are disposed of by one of two methods, landfill or incineration. Materials like paper, aluminium, polythene and glass are recycled. (i) Only one of the recycled materials is an element. Which one? ___________________________________________________ [1] (ii) State one disadvantage of each method of disposal. Landfill: ______________________________________________ ______________________________________________________ ______________________________________________________ Incineration: ___________________________________________ ______________________________________________________ ___________________________________________________ [2] G141H7 2556 14 [Turn over (d) The table below shows some of the raw materials from which useful materials are made. Place the following four useful materials in their correct place in the table. oxygen sodium chloride Raw material Air iron Remark plastics Useful materials nitrogen Rocks Crude oil Examiner Only Marks aluminium petrol Sea water [4] G141H7 2556 15 [Turn over 5 Borax is a salt which is hydrated and is used in cleaning agents. The formula may be represented by Na2B4O7.xH2O. Borax dissolves in water to give a solution which acts as a weak alkali. Examiner Only Marks Remark (a) 4.775 g of Borax were weighed out and made up to a volume of 250 cm3 with deionised water. 25.0 cm3 portions of this solution were titrated against nitric acid of concentration 0.094 mol/dm3 (moles per litre). The results were recorded in the table below. Initial burette reading (cm3) Final burette reading (cm3) Volume of nitric acid used (titre) (cm3) Rough titration 0.0 26.9 26.9 1st Accurate titration 0.0 26.7 26.7 2nd Accurate titration 0.0 26.5 26.5 (i) Calculate the average titre. [2] G141H7 2556 16 [Turn over (ii) The indicator used was methyl orange. State the colour change of the indicator in this titration. From _____________________ to _____________________ Examiner Only Marks Remark [2] (iii) Calculate the number of moles of nitric acid used in this titration. [2] The equation for the reaction is Na2B4O7 + 2HNO3 + 5H2O 2NaNO3 + 4H3BO3 (iv) Use the equation to deduce the number of moles of Borax which reacted with the nitric acid. [2] (v) Calculate the concentration of the Borax in mol/dm3 (moles per litre). [2] G141H7 2556 17 [Turn over (vi) From the mass of Borax used, calculate the concentration of Borax in g/dm3. Examiner Only Marks Remark [1] (vii)Using your answers to parts (v) and (vi) find the formula mass of the Borax, Na2B4O7.xH2O, and hence find the value of x. (Relative atomic masses: H = 1; B = 11; O = 16; Na = 23) [3] (b) When Borax crystals are left in air they lose some of their water of crystallisation. To find the value of x in a sample of hydrated Borax Na2B4O7.xH2O, which had been left in air for a month, the sample was heated to constant mass. 7.28 g of hydrated Borax produced 4.04 g of anhydrous Borax. (Relative atomic masses: H = 1; B = 11; O = 16; Na = 23) (i) What is meant by heated to constant mass ? ______________________________________________________ ___________________________________________________ [2] G141H7 2556 18 [Turn over (ii) Calculate the mass of water lost. Examiner Only Marks Remark [1] (iii) Calculate the number of moles of water lost. [2] (iv) Calculate the number of moles of anhydrous Borax. [1] (v) Using your answers to (iii) and (iv) determine the value of x in Na2B4O7.xH2O. [2] G141H7 2556 19 [Turn over (c) When anhydrous Borax is heated it decomposes according to the equation: anhydrous Borax Na2B4O7 sodium metaborate 2NaBO2 + + Examiner Only Marks Remark Boric oxide B2O3 Calculate the mass of sodium metaborate which is produced when 5.05 g of anhydrous Borax is heated. (Relative atomic masses: B = 11; O = 16; Na = 23) [4] G141H7 2556 20 [Turn over THIS IS THE END OF THE QUESTION PAPER G141H7 2556 21 [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. S 6/06 7-082-1

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