How does a catalyst affect a chemical reaction?

A catalyst plays a crucial role in a chemical reaction by lowering the activation energy required for the reaction to proceed. Activation energy is the minimum energy that must be overcome for reactants to be transformed into products. By providing an alternative pathway with a lower activation energy, a catalyst increases the rate at which the reaction occurs without being consumed in the process. This means that the reaction can reach equilibrium faster compared to a reaction that occurs without a catalyst.

While catalysts do not change the overall energy balance of the reaction or affect the position of equilibrium, they significantly enhance reaction rates by making it easier for reactants to collide in a way that leads to product formation. This is particularly important in both industrial processes and biological systems where efficiency and speed are often critical factors.