What distinguishes a catalyst from an intermediate?

A catalyst is a substance that increases the rate of a chemical reaction without being consumed in the process. It works by providing an alternative reaction pathway with a lower activation energy, allowing reactants to convert to products more efficiently. Catalysts can be reused multiple times, making them essential in both industrial processes and biological systems.

Intermediates are transient species formed during the conversion of reactants to products in a chemical reaction. They exist only for a short duration and are not present in the final products. Unlike catalysts, intermediates are consumed in subsequent steps of the reaction mechanism, playing a crucial role in the overall reaction pathway.

A reaction mechanism is a detailed description of the step-by-step process by which reactants are transformed into products. It outlines the sequence of elementary steps, including the formation and consumption of intermediates and the role of catalysts. Understanding the mechanism is vital for distinguishing between catalysts and intermediates, as it clarifies their functions and lifetimes in the reaction.