Explain the concept of activation energy and it... - SS2 Chemistry Chemical Kinetics Question

Activation energy is the minimum energy required for a chemical reaction to occur. It is the energy needed to break the bonds in the reactant molecules, enabling the formation of new bonds and the conversion of reactants into products.

In a chemical reaction, reactant molecules need to overcome the energy barrier represented by the activation energy. Only when the reactants have sufficient energy to surpass this barrier can they proceed to form products. The activation energy determines the rate of reaction because it influences the frequency of successful collisions and the formation of activated complexes.

A higher activation energy generally results in a slower reaction rate since fewer reactant molecules possess the necessary energy to surpass the barrier. Conversely, a lower activation energy allows a larger fraction of reactant molecules to overcome the barrier and proceed to form products, leading to a faster reaction rate.

Catalysts play a crucial role in modifying the activation energy of a reaction. They lower the activation energy by providing an alternative reaction pathway with a lower energy barrier. This reduction in activation energy allows more reactant molecules to reach the activation energy threshold, resulting in an increased reaction rate.