When the activation energy is lower, it becomes easier for a chemical reaction to occur. Activation energy is the minimum energy required for a reaction to take place, specifically the energy needed to break the existing bonds in the reactant molecules and initiate the formation of new bonds to produce the products.
When the activation energy is reduced, several consequences can occur:
Increased reaction rate: Lowering the activation energy increases the number of reacting molecules that have sufficient energy to overcome the energy barrier and participate in the reaction. As a result, the reaction rate generally increases. More reactant molecules possess the necessary energy, leading to a greater frequency of successful collisions and a faster overall reaction.
Greater proportion of successful collisions: By reducing the activation energy, a larger fraction of the colliding particles will have the required energy and orientation to overcome the activation energy barrier and lead to a successful reaction. Consequently, a higher proportion of collisions will result in product formation.
Lower temperature dependence: Activation energy influences the temperature dependence of a reaction. Lowering the activation energy decreases the sensitivity of the reaction rate to changes in temperature. This means that even at lower temperatures, a significant number of molecules will have enough energy to surpass the lower activation energy barrier, enabling the reaction to occur more readily.
Enhanced reaction feasibility: Some reactions may have very high activation energies, making them slow or even seemingly impossible under normal conditions. By reducing the activation energy, these reactions can become feasible and occur more readily, allowing for the transformation of reactants into products.
It is worth noting that the activation energy can be lowered through various means, such as the presence of catalysts. Catalysts provide an alternative reaction pathway with a lower activation energy, allowing the reaction to proceed more efficiently.