Question

Does changing the concentration of reactants in a chemical reaction affect the activation energy of the reaction? If it does, why?

Answer 1

Step-by-step explanation:

For a chemical reaction to occur, there must be a certain number of molecules with energies equal to or greater than the activation energy. With an increase in concentration, the number of molecules with the minimum required energy will increase, and therefore the rate of the reaction will increase.

Answer 2

The activation energy is the minimum amount of energy required for a reaction to occur. It is determined by the nature of the reactants and the reaction mechanism, and it remains constant regardless of the concentration of the reactants. Therefore, changing the concentration of reactants in a chemical reaction does not affect the activation energy of the reaction. However, changing the concentration of reactants can affect the rate of the reaction. According to the collision theory, the rate of a reaction is proportional to the number of collisions between reactant molecules per unit time. If the concentration of reactants is increased, the number of collisions will increase, and the rate of the reaction will increase. Conversely, if the concentration of reactants is decreased, the rate of the reaction will decrease.