Question

Which of the following explains the importance of the activation energy acting as a barrier for reactants? A:It prevents most reactions from occurring spontaneously. B:It ensures the activated complexes remain stable. C:It allows energy to be released slowly from products. D: It stops the activated complexes from ever forming.

Answer 1

A: It prevents most reactions from occurring spontaneously.

The answer above is correct.

Answer 2

Answer: Option (A) is the correct answer.

Step-by-step explanation:

Activation energy is the minimum amount of energy required to carry out a chemical reaction.

So, when reactant molecules does not have the minimum amount of energy then they are not able to participate in a chemical reaction. Hence, the reaction does not take place.

Therefore, a catalyst acts as an initiator in this situation to carry out the reaction.

Thus, we can conclude that the importance of the activation energy acting as a barrier for reactants as it prevents most reactions from occurring spontaneously.