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The presence of a catalyst in a chemical reaction functions primarily by lowering the activation energy required for the reaction to proceed. Activation energy is the minimum energy that reactants must possess in order to transform into products. By providing an alternative pathway for the reaction with a lower activation energy, a catalyst makes it easier for the reactants to overcome the energy barrier, leading to an increased reaction rate without being consumed in the process.

This reduction in activation energy does not alter the energy of the reactants or products; rather, it simply facilitates the transition states involved in the reaction mechanism. Therefore, the catalyst allows the reaction to proceed more efficiently at a given temperature, resulting in a faster formation of products.