What is the main function of catalysts in chemical reactions?

The primary function of catalysts in chemical reactions is to speed up the reaction without being consumed in the process. Catalysts work by providing an alternative pathway for the reaction to occur, which often involves a lower activation energy compared to the uncatalyzed reaction. As a result, more reactant molecules attain the necessary energy to undergo the reaction in a given time frame, leading to an increased reaction rate.

Importantly, catalysts do not alter the fundamental nature of the reactants or the products. They facilitate the reaction but do not become part of the final product nor do they change the chemical identity of the reactants. After the reaction has completed, the catalyst can be recovered in its original form, which is a defining characteristic that distinguishes catalysts from reactants.

This property also means that catalysts are often used in small amounts relative to the reactants, making them efficient in industrial applications where maximizing output while minimizing costs is essential. By increasing the speed of reactions, catalysts can enhance the productivity of chemical processes, making them indispensable in various chemical and manufacturing industries.