Correct statements regarding Arrhenius equati | vedclass

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(D) Statement $(A)$ is incorrect because the factor $e^{-Ea/RT}$ represents the fraction of molecules having kinetic energy equal to or greater than t

Vedclass · Accepted Answer

$B$ and $C$ only

Vedclass · Answer

(D) Statement $(A)$ is incorrect because the factor $e^{-Ea/RT}$ represents the fraction of molecules having kinetic energy equal to or greater than the activation energy $(Ea)$.Statement $(B)$ is correct because a lower activation energy $(Ea)$ means a larger fraction of molecules can cross the energy barrier, leading to a faster reaction rate.Statement $(C)$ is correct as a general rule of thumb for many reactions, an increase in temperature by $10^{\circ}C$ approximately doubles the rate constant.Statement $(D)$ is incorrect because the plot of $\log k$ vs $\frac{1}{T}$ gives a straight line with a slope of $-\frac{Ea}{2.303R}$, not $-\frac{Ea}{R}$.Therefore, statements $(B)$ and $(C)$ are correct.

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