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(A) The rate of a reaction increases with a rise in temperature primarily because a larger fraction of molecules possess kinetic energy equal to or gr

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An increased number of molecular collisions

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(A) The rate of a reaction increases with a rise in temperature primarily because a larger fraction of molecules possess kinetic energy equal to or greater than the activation energy $(E_a)$.According to the Arrhenius equation,$k = A e^{-E_a/RT}$,the rate constant $k$ increases exponentially with temperature $T$.While the number of collisions increases slightly,the most significant factor is the increase in the number of molecules having energy $\ge E_a$,which effectively lowers the energy barrier requirement for the reaction to proceed at a higher rate.

$A$ rise in temperature increases the velocity of a reaction. It is because it results in

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