The reason for almost doubling the rate of re | vedclass

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(C) The correct answer is $(C)$.According to the Arrhenius theory,the rate of reaction is proportional to the fraction of molecules having energy grea

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The fraction of the molecule having energy equal to threshold energy or more increases

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(C) The correct answer is $(C)$.According to the Arrhenius theory,the rate of reaction is proportional to the fraction of molecules having energy greater than or equal to the activation energy $(E_a)$.When the temperature is increased by $10 \, ^\circ C$,the Maxwell-Boltzmann distribution curve shifts to the right.This shift significantly increases the number of molecules possessing kinetic energy equal to or greater than the threshold energy.Although collision frequency increases slightly,the exponential increase in the fraction of effective collisions is the primary reason for the doubling of the reaction rate.

The reason for almost doubling the rate of reaction on increasing the temperature of the reaction system by $10 \, ^\circ C$ is

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$A$ reaction having equal energies of activation for forward and reverse reactions has

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