OCR A Jun 2015 Paper 2 Q3

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3 Methanol, CH3OH, is an important feedstock for the chemical industry. In the manufacture of methanol, carbon dioxide and hydrogen are reacted together in the reversible reaction shown below. CO2(g) + 3H2(g) CH3OH(g) + H2O(g) H = 49 kJ mol1 (a) Describe and explain the effect of increasing the pressure on the reaction rate.[2] (b) State le Chateliers principle.[1] (c) High pressures and low temperatures would give a maximum equilibrium yield of methanol. (i) Explain this statement in terms of le Chateliers principle.[3] (ii) Explain why the actual conditions used by the chemical industry might be different.[2]OCR 2015<br />
 (d) The manufacture of methanol uses a catalyst. Sketch a labelled diagram of the Boltzmann distribution on the grid provided. Label your axes.Using your Boltzmann distribution, explain how the catalyst increases the rate of reaction.[4] (e) Explain why the use of a catalyst can reduce the demand for energy.[1] [Total: 13]OCR 2015 Turn over<br />

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