What is the difference between activation energy and reaction energy?

Activation energy is the minimum energy required for a reaction to occur, while reaction energy is the overall energy change during a reaction.

Activation energy is the energy required to break the bonds of the reactants and initiate a chemical reaction. It is the energy barrier that must be overcome for the reaction to proceed. The activation energy is specific to each reaction and can be affected by factors such as temperature, concentration, and catalysts.

On the other hand, reaction energy is the overall energy change that occurs during a chemical reaction. It is the difference between the energy of the reactants and the energy of the products. If the reaction releases energy, it is exothermic, and if it absorbs energy, it is endothermic.

The activation energy and reaction energy are related, but they are not the same thing. The activation energy determines the rate of the reaction, while the reaction energy determines the overall energy change. A reaction with a high activation energy may have a low reaction energy if the products have lower energy than the reactants.

Understanding the difference between activation energy and reaction energy is important in understanding the factors that affect the rate and outcome of chemical reactions. It also helps in the design of catalysts and other strategies to control and optimize chemical reactions.