activation energy describes the amount of energy required for a successful collision. given the same…
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...\n\nfaster rate of reaction.\n\nsmaller k value.\n\nslower rate of reaction.\n\nlarger k value.
Answer
Brief Explanations:
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.