A catalyst increases the rate of a reaction by providing an alternative pathway with a lower activation energy. In a reversible reaction the same catalyst lowers the activation energy of both the forward and the reverse reactions.
The rates of the forward and reverse reactions are increased equally. This means a catalyst has no effect on the position of equilibrium, so it does not change the yield or the equilibrium concentrations.What a catalyst does change is how quickly equilibrium is reached. The same equilibrium mixture is produced, but in a shorter time.This is very useful in industry. A catalyst gives a reasonable rate at a lower temperature than would otherwise be needed, which saves energy. Examples are iron in the Haber process for making ammonia and vanadium(V) oxide in the Contact process for making sulfuric acid.Catalysts are not used up, so a small amount can be used over and over again.
The rates of the forward and reverse reactions are increased equally. This means a catalyst has no effect on the position of equilibrium, so it does not change the yield or the equilibrium concentrations.What a catalyst does change is how quickly equilibrium is reached. The same equilibrium mixture is produced, but in a shorter time.This is very useful in industry. A catalyst gives a reasonable rate at a lower temperature than would otherwise be needed, which saves energy. Examples are iron in the Haber process for making ammonia and vanadium(V) oxide in the Contact process for making sulfuric acid.Catalysts are not used up, so a small amount can be used over and over again.