If the energy of activation of a chemical reaction is very low, the rate of that chemical reaction is observed to be very high because?

Explanation

Option A is incorrect because the concentration of reactants, still, is a factor regardless of other factors such as low activation energy. (Same goes for all other factors that affect the rate of reaction) Option B is incorrect, as the transition state is always present regardless of activation energy. Option C is correct, as low activation energy means that many more reactant particles have the minimum energy required to produce products so, with a greater number of particles possessing energy equal to or greater than the activation energy collide, they produce products. Hence, more fruitful collisions occur. Option D is incorrect, as reactant particles move slowly if there is less heat energy applied, which was not mentioned in the question.