What does a catalyst do to a chemical reaction?

A catalyst plays a crucial role in chemical reactions by lowering the activation energy required for the reaction to occur. Activation energy is the minimum energy that reactants must possess for a reaction to take place. By providing an alternative reaction pathway that requires less energy, a catalyst makes it easier for the reactants to convert into products. This means that the reaction can proceed more quickly or at a lower temperature than it would without the catalyst.

The catalyst itself does not participate in the overall reaction; it is not consumed in the process and can be used repeatedly. This characteristic is essential for various industrial processes, as it can enhance reaction rates without the need for increasing temperature or pressure significantly, which could lead to other complications or increased costs.

In contrast, increasing the temperature generally increases the energy of the molecules but does not specifically define the function of a catalyst. Changing the products of the reaction is not a role of a catalyst; it simply facilitates the formation of the reaction products that would naturally occur. Lastly, a catalyst does not remove reactants from the system; it allows for the existing reactants to react more efficiently.