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GCE MAY 2009 : (A2 1) Further Organic, Physical and Inorganic Chemistry

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Centre Number 71 Candidate Number ADVANCED General Certificate of Education 2009 Chemistry assessing Module 4: Further Organic, Physical and Inorganic Chemistry A2C11 Assessment Unit A2 1 [A2C11] THURSDAY 21 MAY, 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. Answer all sixteen questions. Answer all ten questions in Section A. Record your answers by marking the appropriate letter in 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 answer in the spaces provided in this question paper. For Examiner s use only Question Number Section A 1 10 Section B 11 INFORMATION FOR CANDIDATES The total mark for this paper is 90. Quality of written communication will be assessed in question 14(b). 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. 4589.03R Marks 12 13 14 15 16 Total Marks Section A For each of the 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 Which one of the following substances, when added to water in equimolar amounts, will form a solution with the lowest pH? A B C D 2 Which one of the following equations represents the lattice enthalpy of calcium bromide? A B C D 3 Na2O CH3COOH SO2 SO3 Ca(s) + Br2(l) CaBr2(s) CaBr2(s) Ca(s) + Br2(g) Ca2+(g) + 2Br (g) CaBr2(g) CaBr2(s) Ca2+(g) + 2Br (g) The rate constants for the forward and reverse reactions in the formation of nitrogen(IV) oxide are k1 and k2 respectively. 2NO + O2 2NO2 The equilibrium constant for the forward reaction is K. What is the effect of a catalyst on k1, k2 and K? A B C D 4589 k1 decreases increases increases increases k2 decreases increases increases decreases K decreases increases no effect no effect 2 [Turn over 4 Concentrated nitric acid is used as A B C D 5 a dehydrating agent. a hydrating agent. an oxidising agent. a reducing agent. The rate equation for the reaction of iodide ions with hydrogen peroxide in acidic solution is rate = k[H2O2] [H+] [I ] What are the units of k? A B C D 6 Heating sucrose with dilute hydrochloric acid produces A B C D 7 fructose only. glucose only. glucose and fructose. glucose and maltose. Which one of the following compounds produced a silver mirror when heated with Tollen s reagent? A B C D 4589 mol 2 dm6 s 1 mol 1 dm3 s 1 mol dm 3 s 1 mol2 dm 6 s 1 CH3COCH3 CH3CO2H CH3CHO CH3CO2CH3 3 [Turn over 8 Which one of the following molecules contains a chiral centre? A B C D 9 CH3CH = CHCl CH3CH2CH2CHO CH3CH(CH3)CO2H CH3CH(OH)CO2CH3 Which one of the following equations does not represent a redox reaction of nitric acid or the nitrate ion? A B C D 8Al + 3NO3 + 30H+ 8Al3+ + 3NH4+ + 9H2O 4H+ + 2NO3 + 2I 2H2O + 2NO2 + I2 2HNO3 + K2CO3 2KNO3 + H2O + CO2 Pb + 4HNO3 Pb(NO3)2 + 2H2O + 2NO2 10 Given the following standard electrode potentials Fe2+(aq) 2e + + 2e Sn2+(aq) + 2e Sn4+(aq) + 2e I2(s) + 2e Br2(l) + 2e Ni2+(aq) Fe(s) Ni(s) Sn(s) Sn2+(aq) 2I (aq) 2Br (aq) E /V 0.44 0.25 0.14 +0.15 +0.54 +1.09 which one of the following species is reduced by Sn2+(aq)? A B C D 4589 Br (l) Fe2+(aq) I2(s) Ni2+(aq) 4 [Turn over Section B Examiner Only Marks Remark Answer all six questions in the spaces provided. 11 Some Scotch whiskies have the fragrance of cut grass. This smell is attributed to cis hex-3-enal, an unsaturated aldehyde. (a) Suggest a structure for cis hex-3-enal. [2] (b) What would be observed if cis hex-3-enal is warmed with Fehling s solution? _________________________________________________________ _______________________________________________________ [2] (c) Write the equation for the reaction between cis hex-3-enal and 2,4 dinitrophenylhydrazine. Represent the structure of cis hex-3-enal as C = O. There is no requirement to draw the full structure. [3] 4589 5 [Turn over 12 The wing of a hang glider is made from sheets of polyethylene terephthalate (PET). The frame is an alloy of magnesium and aluminium. Examiner Only Marks Remark (a) (i) Draw the structures of the two monomers used to make PET. [2] (ii) Draw the structure for one repeating unit of PET [2] (b) Aluminium and magnesium have typical metal structures. (i) Draw a labelled diagram to show the bonding within a metal such as aluminium. [2] (ii) State two properties of aluminium which make it suitable for use in the frame of a hang glider. _____________________________________________________ ___________________________________________________ [2] (c) If the frame is burned, the aluminium and magnesium form a mixture of oxides. Write the equation for the reaction between aluminium and oxygen. _______________________________________________________ [1] 4589 6 [Turn over (d) Aluminium oxide is amphoteric, reacting with both acids and alkalis. Examiner Only Marks Remark (i) Write the equation for the reaction between aluminium oxide and sulphuric acid. ___________________________________________________ [2] (ii) Write the equation for the reaction between aluminium oxide and aqueous sodium hydroxide. ___________________________________________________ [2] 4589 7 [Turn over 13 Car air bags contain a mixture of sodium azide, NaN3, potassium nitrate, KNO3, and silicon dioxide, SiO2. In a collision, a series of chemical reactions produce nitrogen to fill the airbag. Examiner Only Marks Remark (a) Firstly, the sodium azide decomposes. (i) Write an equation for the decomposition of sodium azide to form sodium and nitrogen. ___________________________________________________ [1] (ii) The azide ion can be written as + N=N=N Using a dot and cross diagram, draw the electron structure of the azide ion, showing the outer electrons of each atom. [2] (b) Secondly, the potassium nitrate reacts with the sodium metal to form potassium oxide, sodium oxide and more nitrogen. (i) Write an equation for the reaction. ___________________________________________________ [1] (ii) Use dot and cross diagrams to show the formation of sodium oxide from sodium and oxygen atoms [2] 4589 8 [Turn over (c) Metal oxides react with silicon dioxide to form metal silicates. Write an equation for the reaction of sodium oxide with silicon dioxide. Examiner Only Marks Remark _______________________________________________________ [1] (d) The table below gives the percentage by mass of the ingredients in a typical air bag. Ingredient Percentage by mass sodium azide 65 silicon dioxide 25 potassium nitrate 10 Calculate the maximum volume of nitrogen which could be obtained from 100 g of this mixture at 20 C and a pressure of one atmosphere. _________________________________________________________ _________________________________________________________ _________________________________________________________ _______________________________________________________ [3] (e) Draw a diagram to explain the structure of silicon dioxide. [2] 4589 9 [Turn over 14 Rapeseed oil is a tri-ester of linoleic acid and has the structure shown below: Examiner Only Marks Remark O CH2 O C (CH2)7 CH = CH CH2 CH = CH (CH2)4 CH3 O CH O C (CH2)7 CH = CH CH2 CH = CH (CH2)4 CH3 O CH2 O C (CH2)7 CH = CH CH2 CH = CH (CH2)4 CH3 (a) Rapeseed oil can be converted into biodiesel. The tri-ester is hydrolysed to form glycerol and linoleic acid. Esterification of the linoleic acid with methanol produces biodiesel. (i) Draw the structure of glycerol. [1] (ii) Draw the structure of a biodiesel molecule. [2] 4589 10 [Turn over (b) Describe how Wij s solution is used to determine the iodine value of rapeseed oil. No reference need be made to calculating the iodine value and no equations are required. Examiner Only Marks Remark _________________________________________________________ _________________________________________________________ _________________________________________________________ _________________________________________________________ _________________________________________________________ _________________________________________________________ _________________________________________________________ _______________________________________________________ [5] Quality of written communication [2] (c) Linoleic acid reacts with thionyl chloride to produce an acyl chloride. Write an equation for the reaction. _______________________________________________________ [2] (d) Calculate the volume of hydrogen needed to saturate the double bonds in 100 g of linoleic acid (RMM = 280). _________________________________________________________ _________________________________________________________ _________________________________________________________ _______________________________________________________ [3] 4589 11 [Turn over 15 Phosphorus pentachloride when pure is an almost colourless solid. X-ray analysis shows that it is composed of [PCl4]+ and [PCl6] ions. Cl Cl + Cl Cl Cl Cl P Cl PCl5 P Cl Cl Cl Remark Cl Cl P Examiner Only Marks Cl Cl Cl PCl4+ PCl6 (a) (i) State the shapes of the [PCl4]+ and [PCl6] ions. [PCl4]+ _____________________________________________ [1] [PCl6] _____________________________________________ [1] (ii) Calculate the oxidation number of phosphorus in [PCl4]+ and [PCl6] . ___________________________________________________ [1] (b) Phosphorus pentachloride reacts with carboxylic acids. Write the equation for the reaction between phosphorus pentachloride and ethanoic acid. _______________________________________________________ [2] 4589 12 [Turn over (c) When heated, phosphorus pentachloride vapourises and decomposes to form an equilibrium mixture. PCl5(g) PCl3(g) + Cl2(g) Examiner Only Marks Remark H = +91 kJ (i) Explain the effect of increasing the pressure on the equilibrium system. _____________________________________________________ ___________________________________________________ [2] (ii) Explain the effect of increasing the temperature on the equilibrium system. _____________________________________________________ ___________________________________________________ [2] (iii) If the equilibrium mixture contains 0.11 mol of phosphorus trichloride, 0.11 mol of chlorine and 0.39 mol of phosphorus pentachloride in a 1 dm3 container at 300 C and 1.0 105 Pa, calculate the dissociation constant, Kp and state its units. _____________________________________________________ _____________________________________________________ _____________________________________________________ ___________________________________________________ [3] 4589 13 [Turn over 16 Bromothymol blue is an indicator which changes colour over a pH range of 6.0 7.8. At pH 6.0 it is yellow, above pH 7.8 it is blue. Examiner Only Marks Remark (a) Bromothymol blue can be regarded as a weak acid HIn which is in equilibrium with the In ion. HIn H+ + In (i) State the conjugate base and conjugate acid in the equilibrium. conjugate base _______________________________________ [1] conjugate acid _______________________________________ [1] (ii) Using the equilibrium equation, explain the colour changes that occur when acid and alkali are added separately to the indicator. _____________________________________________________ ___________________________________________________ [2] (b) The titration curve below shows the titration of 0.1M ethanoic acid with sodium hydroxide. 12 pH 7 0 0 25 volume of 0.1M NaOH/cm3 40 (i) Calculate the pH of the ethanoic acid solution at the start of the titration. (Ka for ethanoic acid = 1.7 10 5 mol dm 3) _____________________________________________________ _____________________________________________________ ___________________________________________________ [2] 4589 14 [Turn over (ii) Explain whether bromothymol blue would be a suitable indicator for the titration. Examiner Only Marks Remark _____________________________________________________ ___________________________________________________ [2] (iii) Write an equation for the reaction of ethanoic acid with sodium hydroxide. ___________________________________________________ [1] (iv) Explain why a solution of sodium ethanoate is alkaline. _____________________________________________________ ___________________________________________________ [2] THIS IS THE END OF THE QUESTION PAPER 4589 15 [Turn over 937-051-1

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Additional Info : Gce Chemistry May 2009 Assessment Unit A2 1 Module 4: Further Organic, Physical and Inorganic Chemistry
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