What role do catalysts play in chemical reactions?

Catalysts are essential in chemical reactions because they increase the reaction rate without being consumed in the process. This means that they can facilitate the conversion of reactants to products more efficiently, allowing the reaction to occur faster than it would without the catalyst. The unique aspect of catalysts is that they remain unchanged after the reaction, so they can be used repeatedly.

Catalysts work by providing an alternative pathway for the reaction that has a lower activation energy than the uncatalyzed reaction. This reduced activation energy means that more reactant molecules have the necessary energy to overcome this barrier, leading to a higher rate of reaction.

While some catalysts can influence the temperature at which a reaction occurs, their primary function is not to lower temperatures but to enhance the speed of the reaction. Additionally, catalysts do not alter the overall energy change of the reaction; they do not change the position of equilibrium or the energy of the products and reactants. Lastly, catalysts are not reactants; they participate in the reaction but do not get consumed or become part of the final product.