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.
• larger k value.
• slower rate of reaction.
• smaller 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 frequency of successful collisions and thus speeding up the reaction rate. The equilibrium constant ($K$) is related to the thermodynamics of the reaction and not directly to the activation - energy in a way that a lower activation energy would directly imply a change in $K$ value.

Answer:

A. faster rate of reaction.