B indicates the higher reaction rate because of a lower activation energy. Option B.
Activation energy represents the minimum energy that reactants of a reaction need to surmount in order to make it to products. The higher this energy, the lower the reaction rate of reactions
B having lower activation energy means it requires less energy for reactant molecules to reach the transition state, facilitating faster reactions.
With a lower energy barrier, a greater proportion of molecules in B can overcome this barrier, resulting in a higher reaction rate compared to A.
Lower activation energy increases the likelihood of successful collisions between reacting particles, enhancing the rate of the chemical reaction.
Thus, B's lower activation energy is a key factor contributing to its higher reaction rate compared to A.