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A catalyst lowers the activation energy of a reaction but is not consumed. If you look at the elementary steps of a reaction, you will see that a catalyst is present as a reactant at the very beginning of a reaction, but is also produced as a product at the end. This means that is was not "consumed" in the reaction since it was not changed by the reaction.
There are two types of catalysts that are both not necessarily consumed within the reaction. The first is a homogeneous catalyst, which is a same phase catalyst. This form of catalyst is made up of the same starting materials, and the reaction typically occurs within solution. The second is a heterogeneous catalyst, which is a different phase catalyst and catalysis typically occurs on a surface. In both examples, the catalyst isn't consumed by the reaction, but lowers the activation energy for the reaction to occur
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