OCR A Jun 2010 Paper 2 Q6

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21 6 An important reaction in the manufacture of nitric acid is the catalytic oxidation of ammonia. 4NH3(g) + 5O2(g) 4NO(g) + 6H2O(g) H =909 kJ mol1 (a) Low pressures and low temperatures would give the maximum equilibrium yield of NO. Explain why.[2] (b) The actual conditions used in the catalytic oxidation of ammonia include 900 C and an increase in pressure. Suggest why these conditions are a compromise.[3] (c) A factory makes 2.50105 mol of NO a day. (i) How much energy is released every day? energy released = . kJ [1] (ii) Suggest how this energy can be used to reduce the cost of making NO.[1]OCR 2010 [Total: 7] Turn over<br />

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