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- faster rate of reaction.\n- larger k value.\n- slower rate of reaction.\n- smaller 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 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.