What is the purpose of a catalyst in a chemical reaction?

The purpose of a catalyst in a chemical reaction is to lower the activation energy required for the reaction to proceed. Activation energy is the minimum amount of energy needed for reactants to overcome the energy barrier and transform into products. By providing an alternative pathway for the reaction, catalysts enable the reaction to occur more easily and at lower energy levels, which can significantly increase the reaction rate without being consumed in the process.

Catalysts do not alter the overall energy balance or change the products of the reaction; they merely speed up the rate at which equilibrium is reached. This is essential in many chemical manufacturing processes where efficiency and reaction times are critical.

In contrast, increasing the temperature generally raises the kinetic energy of reactants but does not specifically address the role of a catalyst. Changing the reaction product is not in the scope of what a catalyst does, as it facilitates the reaction without altering the end result. Increasing the concentration of reactants can shift the reaction equilibrium but is not a function of a catalyst. Thus, lowering the activation energy is the defining characteristic of how catalysts operate within chemical reactions.