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 , 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 -9028

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1. The effect of a catalyst and using a temperature of 220°C:

   When we use a catalyst, it makes the reaction go faster by lowering the activation energy. It helps both the forward and backward reactions happen more quickly. This means that equilibrium is reached faster. The catalyst gives the particles an easier way to react by providing an alternative reaction pathway. However, it does not affect the position of equilibrium, so the yield stays the same.

   Using a temperature of 220°C instead of a lower one also affects the reaction. At higher temperature, the particles move faster because they have more kinetic energy. This leads to more frequent and energetic collisions, so equilibrium is reached in a shorter time.

   Also, if the forward reaction is endothermic (takes in heat), then increasing the temperature makes the equilibrium shift to the right-hand side, so the yield of hydrogen increases.

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