How does a catalyst affect the rate of reaction in collision theory?

In collision theory, a catalyst facilitates a chemical reaction by providing an alternative reaction pathway with a lower activation energy. It does not change the thermodynamics of the reaction but increases the likelihood of successful collisions between reactant molecules. Catalysts achieve this by forming temporary bonds with reactant molecules, stabilizing transition states, and lowering the energy barrier for the reaction. This allows a greater proportion of collisions to result in a successful reaction, effectively accelerating the reaction rate. By providing an alternative, more accessible route for the reaction, catalysts enhance reaction efficiency without being consumed in the process.