What happens to the activation energy when a catalyst is present?

When a catalyst is present in a chemical reaction, it serves to lower the activation energy barrier that reactants must overcome to form products. Activation energy is the minimum energy required for a reaction to occur, and by providing an alternative reaction pathway, catalysts make it easier for reactants to convert to products. This is achieved without altering the overall energy change of the reaction.

The decrease in activation energy allows reactions to proceed at a faster rate at a given temperature, thereby improving the efficiency of the reaction. Catalysts do not get consumed in the reaction, meaning they can be used repeatedly to lower the activation energy for multiple reaction cycles.

Understanding this concept is critical in various applications, including industrial processes, where catalysts are employed to increase the rate of reactions without the need for excessive heat or pressure, leading to safer and more economical processes.