Why do catalysts not alter the amounts of reactants and products present at equilibrium?

Chemical equilibrium occurs when the rates of the forward and reverse reactions in a chemical process are equal, resulting in constant concentrations of reactants and products. At this state, the system is dynamic, meaning that reactions continue to occur, but there is no net change in the amounts of substances involved.

Catalysts are substances that increase the rate of a chemical reaction without being consumed in the process. They work by lowering the activation energy required for the reaction to occur, allowing reactants to convert to products more efficiently. However, they do not affect the position of equilibrium or the final concentrations of reactants and products.

Le Chatelier's Principle states that if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust to counteract that change and restore a new equilibrium. Since catalysts do not change the energy levels of reactants or products, they do not shift the equilibrium position, thus leaving the amounts of reactants and products unchanged.