The activation energy is needed amount for the reaction to occur. High activation energy act as a barrier resulting in low reaction rates. Thus, option B is correct.
Activation energy is the least amount of the energy possessed by a reactant to initiate the reaction to yield a product. It is the minimum energy required to activate the reaction to convert the reactants.
The activation energy affects the reaction rate as low energy increases the rate of reaction but high activation energy slows the rate of reaction.
The activation energy determines the velocity rate, collision, and kinetic energy of the atoms and molecules of the reactant undergoing chemical changes to produce products.
Therefore, high activation energy lowers the reaction rate.
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