Question

Define activation energy. What role does activation energy play in chemical kinetics?

Short answer

Activation energy is the minimum energy required for a reaction to happen. It plays a vital role in chemical kinetics by influencing the rate of reactions. Higher activation energy results in slower reaction rates, and vice versa. Temperature also plays a role by affecting how many molecules can overcome the activation energy barrier.

Step-by-step solution

Define Activation Energy

Activation energy, often represented as \(E_a\), is the minimum amount of energy that reactants must possess for a chemical reaction to occur. It serves as a barrier to the progress of a reaction. No reaction can occur unless the reactant molecules possess this required amount of energy.

Explain Activation Energy’s Role in Chemical Kinetics

Activation energy plays a key role in chemical kinetics, which deal with the rate of reactions. Higher activation energy implies that fewer molecules will have sufficient energy to react, thus the reaction rate will be slower. Conversely, a lower activation energy means that more molecules can undergo the reaction, leading to a faster reaction rate. Temperature also affects this process. As temperature increases, more molecules possess the necessary energy to exceed the activation energy barrier, hence the reaction rate increases.