What is the purpose of a catalyst in chemical reactions at equilibrium?

The purpose of a catalyst in chemical reactions at equilibrium primarily revolves around its role in lowering the activation energy for both the forward and reverse reactions. By providing an alternative pathway with a lower energy barrier, a catalyst speeds up the rate at which equilibrium is reached without being consumed in the reaction itself.

This means that while the catalyst accelerates the process, it does not change the position of the equilibrium or affect the yield of products in the final state. Instead, it enables the system to attain equilibrium faster. Since the catalyst facilitates both the formation of products and the reformation of reactants equally, it ensures that the relative amounts of reactants and products at equilibrium remain unchanged.

In contrast, increasing the yield of the products, stabilizing temperature, or shifting the equilibrium position are not functions of a catalyst. These outcomes can be influenced by changes in concentration, pressure, or temperature but not by the addition of a catalyst.