IJC 2011_H2_CHEM_P3_QN_P

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2 PRELIM 2 © INNOVA 9647/03/2011 [Turn over Answer 4 out of 5 questions. 1 (a) (i) Manganese(IV) oxide, MnO 2 is the most common starting material for the production of compounds of manganese of other oxidation states. With reference to the Data Booklet , state which of the following ions would convert manganese(IV) oxide to manganese(II) sulfate in an acidic solution. P b 4+(aq) / Pb2+(aq) E = +1.69V C o 3+(aq) / Co2+(aq) E = +1.82V F e 3+(aq) / Fe2+(aq) E = +0.77V (ii) Calculate the E cell value to prove that the reaction between MnO 2 and the ion that you have chosen in a(i) is feasible and write a balanced equation for the reaction. (iii) What would be the colour of the final solution observed? [5] (b) (i) Write the full electronic configuration of Zn2+ and Mn2+. (ii) Explain why manganese forms compounds that are often coloured whereas compounds of zinc are usually white. [5] (c) MnO 2 undergoes the following reaction as shown in the schematic diagram below: Step I: Oxidation of MnO 2 in molten KOH with oxygen from the air produces a green compound, A. Step II: Reaction of A with dilute acid produced 0.174 g of MnO 2 and a purple solution of compound B was observed. A solution of compound B is just decolourised by 40.0 cm3 of 0.500 mol dm-3 iron(II) sulphate. (