What effect does a catalyst have on the activation energy of a reaction?

A catalyst plays a crucial role in facilitating chemical reactions by lowering the activation energy required for the reaction to proceed. Activation energy is the minimum energy that reactant molecules must possess in order to react and form products. When a catalyst is introduced, it provides an alternative pathway for the reaction that has a lower activation energy barrier. This means that a greater proportion of reactant molecules will have sufficient energy to overcome the barrier, thereby increasing the rate of the reaction.

By decreasing the activation energy, the catalyst accelerates the reaction without being consumed in the process, thus allowing it to be used repeatedly. This characteristic is fundamental in various chemical processes, including those in industrial applications and biological systems, where catalysts (such as enzymes) are essential for survival and efficiency.