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Question

(C) According to the collision theory,for a reaction to occur,colliding molecules must possess kinetic energy at least equal to the activation energy

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$A$ larger fraction of molecules possess energy greater than the activation energy.

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(C) According to the collision theory,for a reaction to occur,colliding molecules must possess kinetic energy at least equal to the activation energy $(E_a)$.At higher temperatures,the distribution of kinetic energy shifts such that a larger fraction of molecules have energy $\ge E_a$.This leads to an increase in the number of effective collisions,thereby increasing the rate of reaction.Additionally,as per the Arrhenius equation,$k = Ae^{-E_a/RT}$,the rate constant $k$ increases exponentially with temperature.

Why does the rate of a reaction increase with a rise in temperature?

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