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GCE JAN 2011 : (A2 1) Periodic Trends and Further Organic Physical and Inorganic Chemistry - Revised

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Centre Number 71 Candidate Number ADVANCED General Certificate of Education January 2011 Chemistry assessing Periodic Trends and Further Organic, Physical and Inorganic Chemistry AC212 Assessment Unit A2 1 [AC212] WEDNESDAY 26 JANUARY, MORNING TIME 2 hours. INSTRUCTIONS TO CANDIDATES Write your Centre Number and Candidate Number in the spaces provided at the top of this page. Answer all sixteen questions. Answer all ten questions in Section A. Record your answers by marking the appropriate letter on the answer sheet provided. Use only the spaces numbered 1 to 10. Keep in sequence when answering. Answer all six questions in Section B. Write your answers in the spaces provided in this question paper. 111590 INFORMATION FOR CANDIDATES The total mark for this paper is 120. Quality of written communication will be assessed in Question 15(b)(iii). In Section A all questions carry equal marks, i.e. two marks for each question. In Section B the figures in brackets printed down the right-hand side of pages indicate the marks 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 Section A 1 10 Section B 11 12 13 14 15 16 Total Marks 6851.02R Section A For each of the following questions only one of the lettered responses (A D) is correct. Select the correct response in each case and mark its code letter by connecting the dots as illustrated on the answer sheet. 1 When the contents of a gas cylinder containing 19 kg of propane have been completely burned the increase in atmospheric carbon dioxide is A B C D 2 19 kg 38 kg 57 kg 76 kg For the reaction of hydrogen with nitrogen monoxide the rate equation is: Rate = k[H2][NO]2 What are the units of the rate constant? A B C D 3 mol 1 dm3 s 1 mol dm 3 s 1 mol 2 dm 6 s 1 mol 2 dm6 s 1 Which one of the following oxides has ionic bonding and reacts with water to form a strongly alkaline solution? A B C D 6851.02R Al2O3 Na2O P4O10 SO3 2 [Turn over 4 Which one of the following graphs shows a reaction that is first order with respect to reactant Z? Rate Rate [Z] [Z] A B [Z] Time [Z] Time C 5 D Which one of the following represents the units of Kc for the equilibrium shown below? N2(g) + A B C D 6 3H2(g) 2NH3(g) mol 2 dm 6 mol 2 dm6 mol2 dm 6 mol2 dm6 The partition coefficient of an organic acid between ether and water is 5. When 100 cm3 of a solution containing 10 g of the acid is shaken with two successive 20.0 cm3 portions of ether, what mass of the acid would be extracted? A B C D 6851.02R 2.5 g 5.0 g 6.0 g 7.5 g 3 [Turn over 7 Which one of the following organic compounds does not exist? A B C D 8 An aldehyde with formula C2H4O An alkene with formula C6H12 An ester with formula C3H6O2 A ketone with formula C2H4O Consider the equilibrium: 2SO2(g) + O2(g) 2SO3(g) Which one of the following is true when the total pressure of the system is increased at a constant temperature? Mole fraction of SO3 Increases Increases Decreases Increases A B C D 9 Value of Kp Decreases Increases Unchanged Unchanged An equilibrium mixture contains 56 g of nitrogen gas, 14 g of hydrogen gas and 34 g of ammonia gas. Which one of the following is the mole fraction of hydrogen gas? A B C D 0.135 0.250 0.636 0.700 10 Which one of the following salts will dissolve to produce a solution with the highest pH? A B C D 6851.02R ammonium chloride ammonium ethanoate sodium chloride sodium ethanoate 4 [Turn over Section B Examiner Only Marks Remark Answer all six questions in the spaces provided. 11 Data for the reduction of iron(III) oxide by carbon, are shown in the table below. 2Fe2O3(s) + 3C(s) 4Fe(s) + 3CO2(g) Substance Hf /kJ mol 1 S /J K 1 mol 1 Fe2O3 824.2 87.4 C 0.0 5.7 Fe 0.0 27.3 CO2 393.5 213.6 (a) (i) Calculate the values of H , S and G for the reaction at 298 K. H ______________________________________________________ _________________________________________________________ _______________________________________________________ [2] S ______________________________________________________ _________________________________________________________ _______________________________________________________ [2] G ______________________________________________________ _________________________________________________________ _______________________________________________________ [1] (ii) Using your results from part (i) explain why this reaction is not feasible at 298 K. _______________________________________________________ [1] (b) Calculate the temperature above which this reaction is feasible. _____________________________________________________________ _____________________________________________________________ ___________________________________________________________ [2] 6851.02R 5 [Turn over 12 The strength of the ionic bonding in compounds, such as magnesium fluoride and magnesium chloride, is related to the lattice enthalpy of the compound. Examiner Only Marks Remark (a) Define the term lattice enthalpy. _____________________________________________________________ _____________________________________________________________ ___________________________________________________________ [2] (b) (i) Complete the Born-Haber cycle for magnesium fluoride: Mg2+(g) + 2e + 2F(g) Mg2+(g) + 2e + F2(g) Mg(g) + F2(g) [4] 6851.02R 6 [Turn over (ii) Using the data given below, calculate the lattice enthalpy for magnesium fluoride. Examiner Only Marks Remark kJmol 1 Standard enthalpy of formation for magnesium fluoride 1123 First electron affinity of fluorine 348 Atomisation enthalpy of fluorine 79 First ionisation enthalpy of magnesium 736 Second ionisation enthalpy of magnesium 1450 Atomisation enthalpy of magnesium 150 _________________________________________________________ _________________________________________________________ _________________________________________________________ _______________________________________________________ [2] (c) Magnesium fluoride and magnesium chloride are both soluble in water. Magnesium chloride has an enthalpy of solution of 155 kJ mol 1. (i) Using diagrams, show how magnesium and fluoride ions interact with water molecules in an aqueous solution of magnesium fluoride. [2] (ii) Given that the enthalpies of hydration of magnesium ions and chloride ions are 1920 kJ mol 1 and 364 kJ mol 1 respectively, calculate the lattice enthalpy of magnesium chloride. _________________________________________________________ _________________________________________________________ _______________________________________________________ [2] 6851.02R 7 [Turn over 13 Butanone reacts with hydrogen cyanide to form a product that contains an asymmetric centre. Examiner Only Marks Remark OH CH3CH2 C CN CH3 The reaction mechanism is similar to that for the reaction between hydrogen cyanide and propanone. (a) (i) Give the systematic name of the product. _______________________________________________________ [2] (ii) What type of stereoisomerism is shown by the product? _______________________________________________________ [1] (iii) Draw the 3D representations of the stereoisomers. [2] (iv) Name the mechanism for the reaction. _______________________________________________________ [1] (v) Draw the mechanism for this reaction. [3] 6851.02R 8 [Turn over (b) Butanone can be reduced using lithal. The product is optically inactive and dehydrates to give a mixture of but-1-ene and but-2-ene. Examiner Only Marks Remark (i) Using [H] to represent lithal, write the balanced equation for the reduction. _______________________________________________________ [2] (ii) Name the product. _______________________________________________________ [1] (iii) Give the meaning of the term optically inactive. _________________________________________________________ _______________________________________________________ [1] (iv) Suggest why the product is optically inactive. _________________________________________________________ _______________________________________________________ [2] (v) Draw and label the E and Z isomers of but-2-ene. [2] 6851.02R 9 [Turn over (c) Butanal is a structural isomer of butanone. Describe, giving practical details, how you would carry out a chemical test to distinguish between samples of butanal and butanone. Examiner Only Marks Remark _____________________________________________________________ _____________________________________________________________ _____________________________________________________________ _____________________________________________________________ _____________________________________________________________ ___________________________________________________________ [3] (d) 2,4-dinitrophenylhydrazine reacts with both butanone and butanal to form 2,4-dinitrophenylhydrazones. (i) Write the equation for the reaction of butanone with 2,4-dinitrophenylhydrazine. [3] (ii) What would be observed in the reaction? _________________________________________________________ _______________________________________________________ [2] 6851.02R 10 [Turn over (iii) Explain, experimentally, how the 2,4-dinitrophenylhydrazones can be used to confirm the identity of the reactants. Examiner Only Marks Remark _________________________________________________________ _________________________________________________________ _________________________________________________________ _________________________________________________________ _______________________________________________________ [4] 6851.02R 11 [Turn over 14 At 25 C, the acid dissociation constant, Ka, for propanoic acid is 1.35 10 5 mol dm 3. A buffer solution can be prepared by mixing a solution of propanoic acid with a solution of sodium propanoate. Examiner Only Marks Remark (a) (i) Write the expression for the acid dissociation constant of propanoic acid. [1] (ii) Calculate the pH of a 0.25 mol dm 3 solution of propanoic acid. _________________________________________________________ _________________________________________________________ _________________________________________________________ _______________________________________________________ [3] (iii) What is meant by the term buffer solution? _________________________________________________________ _________________________________________________________ _______________________________________________________ [2] 6851.02R 12 [Turn over (iv) Calculate the pH of the buffer solution formed when 300 cm3 of a 0.25 mol dm 3 solution of propanoic acid is mixed with 200 cm3 of a 0.15 mol dm 3 solution of sodium propanoate. Examiner Only Marks Remark _________________________________________________________ _________________________________________________________ _________________________________________________________ _________________________________________________________ _________________________________________________________ _______________________________________________________ [4] (b) The titration curve below shows the change in pH when a 0.20 mol dm 3 solution of sodium hydroxide is added, from a burette, to 25.0 cm3 of a solution of propanoic acid of unknown concentration. pH 18.5 Volume of NaOH added (cm3) (i) Write the equation for the neutralisation reaction which occurs. _______________________________________________________ [1] 6851.02R 13 [Turn over (ii) Suggest a suitable indicator for this titration. Give the colour change and explain why the indicator is suitable. Examiner Only Marks Remark _________________________________________________________ _________________________________________________________ _________________________________________________________ _______________________________________________________ [4] (iii) Calculate the concentration of the propanoic acid. _________________________________________________________ _________________________________________________________ _________________________________________________________ _______________________________________________________ [3] (iv) At 25 C, Kw has the value 1.00 10 14 mol2 dm 6. Calculate the pH of the 0.20 mol dm 3 solution of sodium hydroxide. _________________________________________________________ _________________________________________________________ _______________________________________________________ [2] 6851.02R 14 [Turn over 15 Fats and vegetable oils are triesters of long-chain carboxylic acids. Base catalysed hydrolysis of an oil produces glycerol and the sodium salt of octadeca-9,12-dienoic acid as the only products. CH3(CH2)4CH CHCH2CH Examiner Only Marks Remark CH(CH2)7COOH octadeca-9,12-dienoic acid (a) (i) Draw the structure of glycerol. [1] (ii) State the systematic name for glycerol. _______________________________________________________ [2] (iii) Draw the structure of the oil. [1] (iv) Define the term iodine value as applied to an oil. _________________________________________________________ _________________________________________________________ _______________________________________________________ [2] 6851.02R 15 [Turn over (v) Use the definition given in part (iv) and the structure given in part (iii) to calculate the iodine value of the oil. Examiner Only Marks Remark _________________________________________________________ _________________________________________________________ _________________________________________________________ _________________________________________________________ _________________________________________________________ _______________________________________________________ [4] (b) Simple monoesters, such as the one shown below, can be prepared by reacting carboxylic acids with alcohols: CH3 H C CH3 H O C C O CH3 H (i) Give the systematic names of the carboxylic acid and alcohol required to prepare this ester. Acid ___________________________________________________ [1] Alcohol ________________________________________________ [1] (ii) Write the equation for the formation of the ester. _______________________________________________________ [2] 6851.02R 16 [Turn over (iii) Describe, giving experimental details, the preparation of a pure, dry sample of the ester. Examiner Only Marks Remark _________________________________________________________ _________________________________________________________ _________________________________________________________ _________________________________________________________ _________________________________________________________ _________________________________________________________ _________________________________________________________ _________________________________________________________ _________________________________________________________ _________________________________________________________ _______________________________________________________ [6] Quality of written communication 6851.02R [2] 17 [Turn over 16 The concentration of CO2 in the atmosphere depends on natural and man-made processes. Examiner Only Marks Remark (a) State two natural processes by which CO2 concentration in the atmosphere is decreased. ___________________________________________________________ [2] (b) Carbon dioxide can be produced during the production of electricity. (i) Explain why the carbon dioxide forms. _________________________________________________________ _________________________________________________________ _______________________________________________________ [2] (ii) Industry attempts to reduce the emission of CO2 by reacting emitted gases with alkaline slurries containing hydroxide ions. Write an equation for the reaction of aqueous carbon dioxide with OH ions. _______________________________________________________ [2] (c) Carbon dioxide molecules in the atmosphere absorb IR radiation which leads to carbon dioxide being called a Greenhouse gas. (i) Explain how CO2 absorbs IR radiation. _________________________________________________________ _______________________________________________________ [1] (ii) Explain what a Greenhouse gas does in terms of Global Warming. _________________________________________________________ _________________________________________________________ _______________________________________________________ [2] 6851.02R 18 [Turn over THIS IS THE END OF THE QUESTION PAPER 6851.02R 1 9 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. 111590R

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Additional Info : Gce Chemistry January 2011 Assessment Unit A2 1 Periodic Trends and Further Organic Physical and Inorganic Chemistry - Revised
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