Question

activation energy describes the amount of energy required for a successful collision. given the same conditions, a reaction with a lower activation energy will have a...

faster rate of reaction.

smaller k value.

slower rate of reaction.

larger k value.

Explanation:

Activation energy is the energy barrier for a reaction. A lower activation energy means more reactant molecules have enough energy to react, increasing the reaction - rate. The Arrhenius equation $k = A e^{-\frac{E_a}{RT}}$ shows that a lower activation energy ($E_a$) leads to a larger rate - constant ($K$). So, a reaction with lower activation energy has a faster rate of reaction.

Answer:

A. faster rate of reaction.