How Do Proximity and Orientation Influence Reaction Kinetics?
Reaction kinetics are heavily influenced by how reactants are positioned and aligned relative to the catalyst. Proximity reduces the diffusion distance, thereby decreasing the time it takes for reactants to reach the active site. Orientation ensures that the transition state is easily accessible, lowering the activation energy required for the reaction. Together, these factors can significantly accelerate the reaction rate, as described by the Arrhenius equation.
