What is the effect of a catalyst on the rate of reaction?

A catalyst increases the rate of reaction by providing an alternative pathway for the reaction that has a lower activation energy. This means that more reactant particles have the necessary energy to collide effectively and form products, leading to more frequent successful collisions. The presence of a catalyst does not change the overall enthalpy of the reaction; it simply speeds up the process by lowering the energy barrier that must be overcome for the reaction to proceed.

It's important to note that a catalyst is not consumed during the reaction; instead, it remains chemically unchanged and can participate in the reaction multiple times. This property makes catalysts particularly valuable in both industrial and laboratory settings, as they can enhance the efficiency of reactions without being depleted.