The hydrogen used in a hydrogen-oxygen fuel cell can be produced from methanol, CH3OH. In this reaction the forward reaction is endothermic and heat energy is taken in from the surroundings. The conditions used for this reaction are a nickel catalyst and a temperature of 220 °C . Explain, in terms of their effects on the rate of attainment of equilibrium and the equilibrium yield of hydrogen, why the reaction is carried out using a catalyst at 220 °C rather than without a catalyst at a lower temperature – 9035

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1. Using a catalyst increases the rate at which equilibrium is reached because it speeds up both the forward and backward reactions. It does this by lowering the activation energy and giving the reaction an alternative pathway. However, a catalyst does not change the equilibrium yield.

   Using a temperature of 220°C instead of a lower temperature also helps equilibrium happen faster because the particles have more kinetic energy and collide more often and with more energy. Since the forward reaction is endothermic, increasing the temperature shifts the equilibrium to the right-hand side, which increases the yield of hydrogen.

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