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GCE MAY 2009 : (AS 3) Practical Examination 2 - Revised

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Sp ec Ne i w ca tio n Centre Number 71 Candidate Number ADVANCED SUBSIDIARY (AS) General Certificate of Education 2009 Chemistry assessing Module 3: Practical Examination 2 AC132 Assessment Unit AS 3 [AC132] FRIDAY 15 MAY, MORNING TIME 2 hours 30 minutes. INSTRUCTIONS TO CANDIDATES Write your Centre Number and Candidate Number in the spaces provided at the top of this page. Answer all seven questions. Write your answers in the spaces provided. INFORMATION FOR CANDIDATES The total mark for this paper is 90. Section A Question 1 is a practical exercise worth 25 marks. Question 2 is a practical exercise worth 29 marks. Section B Question 3 is a planning exercise worth 20 marks. Questions 4 7 are written questions worth a total of 16 marks, testing aspects of experimental chemistry. Figures in brackets printed down the right-hand side of pages indicate the mark awarded to each question or part question. A Periodic Table of Elements (including some data) is provided. For Examiner s use only Question Marks Number 1 2 3 4 5 6 7 Total Marks 4959 Section A Examiner Only Marks 1 Remark Titration exercise You are provided with: Sodium hydroxide solution of concentration 0.05 mol dm 3. Vinegar (ethanoic acid) of unknown concentration. Phenolphthalein indicator. You are required to carry out a titration and use your results to calculate the concentration of ethanoic acid in the vinegar. (a) Give details of the procedure you intend to use: _____________________________________________________________ _____________________________________________________________ _____________________________________________________________ _____________________________________________________________ _____________________________________________________________ _____________________________________________________________ ___________________________________________________________ [4] 4959 2 [Turn over (b) Carry out your procedure. Present your results in a suitable table and calculate the average titre. Examiner Only Marks Remark [12] (c) State the colour change at the end point of your titration ___________________________ to ___________________________ [1] 4959 3 [Turn over (d) Write the equation, including state symbols, for the reaction of sodium hydroxide with the ethanoic acid present in vinegar. Examiner Only Marks Remark ___________________________________________________________ [2] (e) (i) Calculate the number of moles of sodium hydroxide used in the titration. _________________________________________________________ _______________________________________________________ [2] (ii) Calculate the number of moles of ethanoic acid neutralised in the titration. _________________________________________________________ _______________________________________________________ [1] (iii) Calculate the concentration (in mol dm 3) of ethanoic acid in the vinegar. _________________________________________________________ _______________________________________________________ [2] (iv) Calculate the concentration (in g dm 3) of ethanoic acid in the vinegar. _________________________________________________________ _______________________________________________________ [1] 4959 4 [Turn over BLANK PAGE (Questions continue overleaf) 4959 5 [Turn over 2 Observation/deduction Examiner Only Marks Remark Safety goggles must be worn at all times and care should be exercised during this practical examination. (a) You are provided with a mixture of two salts, labelled B, which have a common cation. Carry out the following experiments on the mixture. Record your observations and deductions in the spaces below and identify the two salts. Experiment Observations Deductions 1 Describe the appearance of B. 2 Dip a wire loop in concentrated hydrochloric acid; touch sample B with the wire, then hold it in a blue Bunsen ame. 3 In a fume cupboard, add about 1 cm3 of concentrated sulphuric acid to a half spatula-measure of B in a test tube. Heat the test tube gently. 4 Make a solution of B by dissolving a half spatula-measure of B in a test tube half-full of water. Put 1 cm3 of the solution into each of two separate test tubes. (a) (i) Add a few drops of silver nitrate solution into the rst test tube. (ii) Then, in a fume cupboard, add about 2 cm3 of concentrated ammonia into the same test tube. (b) Add a few drops of barium chloride solution to the second test tube and then add 2 cm3 of dilute nitric acid. Name the two salts present in B: _____________________________________________________________ _____________________________________________________________ 4959 6 [Turn over (b) You are provided with an aqueous solution containing an organic substance Y. Carry out the following experiments. Record your observations and deductions in the spaces below. Experiment Observations Examiner Only Marks Remark Deductions 1 Describe the solution and test it with Universal Indicator paper. 2 In a fume cupboard, shake a small volume of the solution with bromine water. 3 Heat about 2 cm3 of the solution with 2 cm3 of potassium dichromate solution and 2 cm3 of dilute sulphuric acid. Based on the above tests, suggest A functional group which may be present in Y: _____________________________________________________________ A functional group which the tests above show is absent from Y: __________________________________________________________ [29] 4959 7 [Turn over Section B Examiner Only Marks 3 Remark Planning You are required to plan an experiment to determine the degree of hydration in a sample of zinc sulphate. If the sample of hydrated zinc sulphate is heated in a crucible to constant mass and appropriate masses measured, the value of x in the formula ZnSO4.xH2O can be found. (a) (i) Explain the meaning of the term hydrated zinc sulphate . [1] (ii) Draw a labelled diagram to show the apparatus which could be used to heat the hydrated zinc sulphate. [3] 4959 8 [Turn over (b) (i) What masses should be recorded before heating the hydrated zinc sulphate? Examiner Only Marks Remark _________________________________________________________ _______________________________________________________ [2] (ii) The hydrated zinc sulphate is heated to remove all the water. What steps would you take to ensure that it had all been removed? _________________________________________________________ _________________________________________________________ _______________________________________________________ [3] (iii) After heating, state one safety precaution which should be followed before weighing. _________________________________________________________ _______________________________________________________ [1] (c) When 8.63 g of hydrated zinc sulphate was heated, 4.85 g of anhydrous zinc sulphate was formed. (i) What is the mass of water lost? _______________________________________________________ [1] (ii) What is the number of moles of water lost? _______________________________________________________ [1] (iii) What is the number of moles of anhydrous zinc sulphate formed? _______________________________________________________ [1] (iv) Calculate the value of x in ZnSO4.xH2O. _________________________________________________________ _______________________________________________________ [2] 4959 9 [Turn over (d) A solution of zinc sulphate is formed when zinc powder is added to a solution of copper sulphate. When 6.00 g of zinc powder (an excess) was added to 50.0 cm3 of a 0.5 mol dm 3 solution of copper sulphate in a polystyrene cup, a temperature increase of 25.3 K was recorded. Examiner Only Marks Remark Zn + CuSO4 ZnSO4 + Cu (i) Calculate the number of moles of copper sulphate. _________________________________________________________ _______________________________________________________ [1] (ii) Assuming that the solution has a heat capacity of 4.2 J K 1 g 1 and that the density of the solution is 1.0 g cm 3, calculate the heat energy (in J) released in this reaction. _________________________________________________________ _______________________________________________________ [2] (iii) Given that zinc is present in excess, calculate the enthalpy change for the reaction (in kJ per mole of copper sulphate). _________________________________________________________ _______________________________________________________ [2] 4959 10 [Turn over 4 A student reacted 11.4 cm3 of ethanoic acid (density = 1.05 g cm 3 and RFM = 60) with excess ethanol to produce 5.28 g of ethyl ethanoate (RFM = 88). Examiner Only Marks Remark (a) Calculate the mass of ethanoic acid used. _____________________________________________________________ ___________________________________________________________ [1] (b) Calculate the number of moles of ethanoic acid used. _____________________________________________________________ ___________________________________________________________ [1] (c) What is the theoretical yield of ethyl ethanoate in moles? _____________________________________________________________ ___________________________________________________________ [1] (d) Calculate the actual yield of ethyl ethanoate in moles. _____________________________________________________________ ___________________________________________________________ [1] (e) State the equation which is used to calculate the percentage yield of a product. ___________________________________________________________ [1] (f) Calculate the percentage yield of product. _____________________________________________________________ ___________________________________________________________ [1] 4959 11 [Turn over 5 Separating a product from a mixture by distillation is an important practical technique in organic chemistry. Examiner Only Marks Remark (a) Draw a labelled diagram of the apparatus used to carry out a distillation. [3] (b) Why are anti-bumping granules added to the mixture? ___________________________________________________________ [1] 6 It is possible, using a suitable reagent, to confirm the presence of Cu2+ ions in solution. (a) Name the reagent which can be used to confirm the presence of Cu2+ ions in solution. ___________________________________________________________ [1] (b) What would be observed when the reagent is added slowly, until present in excess, to a solution containing Cu2+? _____________________________________________________________ ___________________________________________________________ [2] 4959 12 [Turn over 7 Separating funnels can be used to remove impurities from crude organic liquids. They are shaken with an aqueous solution and then separated from the aqueous layer. Examiner Only Marks Remark (a) How would you decide which layer was the organic layer? _____________________________________________________________ _____________________________________________________________ ___________________________________________________________ [2] (b) Why would anhydrous calcium chloride be added to the organic liquid after separation? _____________________________________________________________ ___________________________________________________________ [1] THIS IS THE END OF THE QUESTION PAPER 4959 13 [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. 936-020-1

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Additional Info : Gce Chemistry May 2009 Assessment Unit AS 3 Module 3: Practical Examination 2 - Revised
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