Which of the following statements is incorrect about activation energy?

Step-by-step solution

Activation energy ( E_a ) is the minimum extra amount of energy absorbed by a reactant molecule to get converted into product. According to the Arrhenius equation, k = A e^ -E_a / RT , where k is the rate constant. Higher E_a leads to a smaller value of k , meaning a slower reaction rate. Thus, the statement that higher activation energy results in a slower rate is correct. A catalyst provides an alternative reaction pathway with a lower activation energy, which is a correct statement. The SI unit of energy is Joul