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GCE JUN 2006 : (AS 2) Organic, Physical and Inorganic Chemistry

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Centre Number 71 Candidate Number ADVANCED SUBSIDIARY (AS) General Certificate of Education 2006 Chemistry assessing Module 2: Organic, Physical and Inorganic Chemistry ASC21 Assessment Unit AS 2 [ASC21] FRIDAY 23 JUNE, AFTERNOON 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 seventeen 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 seven questions in Section B. Write your answers in the spaces provided in this question paper. INFORMATION FOR CANDIDATES The total mark for this paper is 100. Quality of written communication will be assessed in question 13(a)(ii). 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 Number Section A 1 10 Section B 11 12 13 14 15 16 17 Total Marks ASC2S6 2553 Marks BLANK PAGE ASC2S6 2553 2 [Turn over 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 by connecting the dots as illustrated on the answer sheet. 1 The mechanism for the reaction between methane and chlorine is A B C D 2 electrophilic addition. free radical addition. free radical substitution. nucleophilic substitution. Which one of the following graphs shows the variation in the first ionisation energy of the Group II elements in periods 3, 4, 5 and 6? A B first ionisation energy Period 3 first ionisation energy 4 5 6 Period 3 C 3 6 5 6 D first ionisation energy Period 3 5 4 first ionisation energy 4 5 6 Period 3 4 A chemist carried out a flame test on a white powder and observed a red colour. When dilute hydrochloric acid was added to the white powder a gas was evolved which gave a white precipitate with calcium hydroxide solution. The powder was A B C D ASC2S6 barium carbonate or calcium carbonate. barium hydroxide or strontium hydroxide. calcium carbonate or strontium carbonate. calcium hydroxide or strontium hydroxide. 2553 3 [Turn over 4 Which one of the following would not give a precipitate of iodoform when reacted with iodine and sodium hydroxide? A B C D 5 Which one of the following can exist as cis-trans isomers? A B C D 6 but-l-ene but-2-ene chloroethene 2-chlorobut-l-ene Calculate the mass of magnesium chloride produced on neutralising 50 cm3 of 2 mol dm 3 hydrochloric acid with excess magnesium oxide A B C D 7 butan-2-ol ethanol methanol propan-2-ol 4.75 g 9.50 g 20.00 g 95.00 g In the reaction between hydrogen bromide and ethene A B C D ASC2S6 the product is unsaturated. the transition state is neutral. the hydrogen bromide bond splits to form ions. the product can exist as two different structural isomers. 2553 4 [Turn over 8 Which one of the following statements regarding the chemical equilibrium is correct: 2SO2(g) + O2(g) = 2SO3(g) A B C D 9 H= 192 kJ An increase in the concentration of O2 will increase the equilibrium amount of SO2. A decrease in the pressure will increase the equilibrium concentration of SO3. An increase in temperature will increase the equilibrium concentration of SO2. Removal of SO3 from the reaction vessel will increase the equilibrium concentration of SO2. Which one of the following sets of apparatus should be selected to separate a mixture of three or more liquids whose boiling points are close together? B A D C ASC2S6 2553 5 [Turn over 10 On the reaction profile shown, which one of the letters, A D, represents the activation energy for the back reaction? Enthalpy C Reactants D B A Products ASC2S6 2553 6 [Turn over Section B Examiner Only Marks Remark Answer all seven questions in the spaces provided 11 Concentrated orange juice contains a low percentage of dissolved sulphur dioxide as an antioxidant; household bleach contains dissolved chlorine. Both gases can be driven off by gentle warming. (a) Describe a chemical test for sulphur dioxide and state the observation for a positive result. Test __________________________________________________ [1] Observation ___________________________________________ [1] (b) Describe a chemical test for chlorine and state the observation for a positive result. Test __________________________________________________ [1] Observation ___________________________________________ [1] ASC2S6 2553 7 [Turn over 12 (a) Name the processes X and Z in the following flow scheme: Examiner Only Marks CH3 2 CH3 CH3CH2CH3 CH3CH2CH2CH2CH CH3CH2CH2CH2CH3 3 X Remark CH3CH2CH2C1 CH3 2CH2Cl A CH COOH CH3CH OH CH22=CH22 CH3CH22OH CH33COOH CH =CH B Y C D Z CH3COOCH2CH CH3COOCH2CH3 3 E X _________________________ Z _________________________ [2] (b) Name the compounds A and E. A _____________________________________________________ [1] E _____________________________________________________ [1] (c) State the temperature and pressure used in the industrial process Y and name the catalyst. temperature _____________________________________________ [1] pressure _____________________________________________ [1] catalyst _____________________________________________ [1] (d) (i) Compounds C and D react to form compound E. Name another compound which will react with C to form E. ____________________________________________________ [1] (ii) Write an equation for the reaction between C and the compound you have named to form E. ____________________________________________________ [2] ASC2S6 2553 8 [Turn over (e) Compound B can be converted into HD polythene. Examiner Only Marks Remark (i) State the conditions for the production of HD polythene. ______________________________________________________ ______________________________________________________ ____________________________________________________ [2] (ii) Explain the relationship between the flexibility and softening temperature of HD polythene and its structure. ______________________________________________________ ____________________________________________________ [2] ASC2S6 2553 9 [Turn over 13 Samples of 1-iodobutane, 1-bromobutane and 1-chlorobutane are placed in three test tubes labelled A, B and C respectively. Silver nitrate solution is added to each test tube and the mixtures warmed gently. Examiner Only Marks Remark (a) (i) State what you should observe in the test tube A when the reaction is complete. ____________________________________________________ [1] (ii) Explain the relative rates of hydrolysis in terms of the bond enthalpies and bond polarities of the three carbon halogen bonds. ____________________________________________________ [3] Quality of written communication [2] (iii) Write equations for the two reactions which occur in test tube B. 1. __________________________________________________ [1] 2. __________________________________________________ [1] ASC2S6 2553 10 [Turn over (b) 2-bromo-2-methylpropane is an isomer of 1-bromobutane which also undergoes reaction with water or sodium hydroxide. Examiner Only Marks Remark (i) Explain why 2-bromo-2-methylpropane is an isomer of 1-bromobutane. ______________________________________________________ ____________________________________________________ [2] (ii) Write a flow scheme for the mechanism of the reaction between 2-bromo-2-methylpropane and hydroxide ions. [3] (iii) When three drops of phenolphthalein are added to 5 cm3 of a 0.1 mol dm 3 solution of sodium hydroxide solution, a pink colour is observed. When 1 cm3 of 2-bromo-2-methylpropane is then added, the solution eventually turns colourless. Suggest an explanation for this observation. ______________________________________________________ ____________________________________________________ [1] ASC2S6 2553 11 [Turn over 14 5.49 g of a metal oxide of formula MO were completely dissolved in 100 cm3 of a 2.0 mol dm 3 solution of hydrochloric acid (an excess). The remaining acid required 27.5 cm3 of a 0.20 mol dm 3 sodium hydroxide solution to be neutralised. This method is called a back titration and is used to determine the amount of the unreacted acid. Examiner Only Marks Remark (a) Write an equation for the reaction between the oxide, MO, and hydrochloric acid. _______________________________________________________ [1] (b) Calculate the number of moles of hydrochloric acid added to the metal oxide. _______________________________________________________ [1] (c) Calculate the number of moles of unreacted hydrochloric acid. HCl + NaOH NaCl + H2O _______________________________________________________ [1] (d) Calculate the number of moles of hydrochloric acid reacting with the metal oxide. _______________________________________________________ [1] (e) Calculate the number of moles of the metal oxide that reacted with the hydochloric acid. _______________________________________________________ [1] (f) Calculate the relative formula mass of the metal oxide. _______________________________________________________ [1] (g) Calculate the relative atomic mass of M. _______________________________________________________ [1] ASC2S6 2553 12 [Turn over BLANK PAGE (Questions continue overleaf) ASC2S6 2553 13 [Turn over 15 Ammonia takes its name from the worshippers of the Egyptian god Amun, the Ammonians, because they heated ammonium chloride with alkali to produce ammonia for use in their religious ceremonies. Today ammonia is made by the Haber Bosch process. Examiner Only Marks Remark (a) (i) Write an equation for the reaction between nitrogen and hydrogen in the Haber process. ____________________________________________________ [2] (ii) The graph below shows the percentage of ammonia produced at a series of pressures and temperatures in the Haber Bosch process. % yield of ammonia 70 350 C 60 400 C 50 450 C 40 500 C 30 550 C 20 10 0 0 0 100 200 300 pressure (atmospheres) 400 Explain why a temperature of 450 C, and not 350 C, is chosen for the industrial process. ______________________________________________________ ____________________________________________________ [1] (iii) Explain why a pressure of 200 atm, and not 400 atm, is chosen. ______________________________________________________ ____________________________________________________ [1] ASC2S6 2553 14 [Turn over (iv) State the catalyst used in the Haber Bosch process. Examiner Only Marks Remark ____________________________________________________ [1] (v) Suggest why the catalyst in the reaction chamber is in the form of pellets rather than as a powder. ____________________________________________________ [1] (vi) The diagram below shows the reaction profile for the uncatalysed reaction between nitrogen and hydrogen. Draw the reaction profile for the catalysed reaction on the diagram. enthalpy nitrogen and hydrogen ammonia [1] (vii)Describe the test for ammonia and state the observation for a positive result. test ________________________________________________ [1] observation __________________________________________ [1] ASC2S6 2553 15 [Turn over (b) Excess ammonia reacts with 1,5-dichloropentane to produce cadaverine, a putrid product formed from the decay of flesh: Examiner Only Marks Remark H2N(CH2)5NH2 cadaverine (i) Suggest an equation for this reaction. ____________________________________________________ [2] (ii) The smell of cadaverine may be eliminated by adding hydrochloric acid. What does this suggest about the chemical nature of cadaverine? ____________________________________________________ [1] (c) (i) l,5-dichloropentane reacts with sodium hydroxide in ethanol to produce pent-l,4-diene. 2NaOH + Cl(CH2)5Cl CH2 CHCH2CH CH2 + 2NaCl + 2H2O What is the name given to this type of reaction? ____________________________________________________ [1] (ii) State the reagent and catalyst needed to convert pent-1,4-diene to pentane. ______________________________________________________ ____________________________________________________ [2] (iii) Write an equation for the conversion of pent-1,4-diene to pentane. ____________________________________________________ [2] ASC2S6 2553 16 [Turn over 16 Magnesium is being increasingly used in the frames of some modern bicycles. This is due to the discovery of an electrolytic process which puts Keronite , a thin layer of magnesium oxide, on a surface to prevent oxidation. Examiner Only Marks Remark (a) (i) Write an equation for the reaction between magnesium and oxygen. ____________________________________________________ [1] (ii) State one property of magnesium which makes it suitable for use in bicycle frames. ____________________________________________________ [1] (b) Group II carbonates show changes in properties as the metal ion changes. (i) How does the size of the positive ion change from magnesium to barium? ____________________________________________________ [1] (ii) State the effect on the thermal stability of the carbonate ion as the size of the positive ion changes from magnesium to barium. ____________________________________________________ [1] (iii) Apart from the changing size of the positive ion, what other factor affects the thermal stability of the carbonate, going from magnesium to barium? ____________________________________________________ [1] (iv) Write an equation for the thermal decomposition of magnesium carbonate. ____________________________________________________ [1] (c) Explain, using an equation, how magnesium ions can be used to distinguish between carbonate ions and hydrogencarbonate ions in solution. __________________________________________________________ __________________________________________________________ _______________________________________________________ [3] ASC2S6 2553 17 [Turn over 17 Ethanol is produced commercially by the fermentation of sucrose which is initially converted to glucose, C6H12O6. Examiner Only Marks Remark (a) (i) Explain the term fermentation. ____________________________________________________ [1] (ii) Write an equation for the production of ethanol from glucose. ____________________________________________________ [2] (b) In the UK it is illegal to drive if the alcohol level in blood is above 80 mg per 100 cm3. In the original breathalysers, a motorist blew through a tube containing a mixture of sulphuric acid and potassium dichromate on silica gel. (i) Write an equation for the oxidation of ethanol, using [O] to represent the oxidising agent. ____________________________________________________ [2] (ii) State the colour change observed in the breathalyser when ethanol is detected. ____________________________________________________ [2] (iii) If a suspect s breath contains 90 mg of ethanol per 100 cm3, calculate the concentration of ethanol in mol dm 3. ______________________________________________________ ______________________________________________________ ____________________________________________________ [3] (iv) Which organ of the body may be permanently affected by alcohol? ____________________________________________________ [1] ASC2S6 2553 18 [Turn over (c) Ethanol is also oxidised when it is burnt in air. In some countries ethanol is used as an alternative to petrol. (i) Write an equation for the complete combustion of ethanol. ____________________________________________________ [1] (ii) Write one equation for the incomplete combustion of ethanol. ____________________________________________________ [1] (iii) Explain the environmental advantage of using ethanol rather than petrol in cars. ______________________________________________________ ____________________________________________________ [2] ASC2S6 2553 19 Examiner Only Marks Remark S 2/06 0000 302507(163) [Turn over

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Additional Info : Gce Chemistry June 2006 Assessment Unit AS 2Module 2: Organic, Physical and Inorganic Chemistr
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