Correct statements regarding Arrhenius equati | vedclass

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Question

(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.

Similar Questions

Among the following,the $INCORRECT$ statement regarding the collision theory of chemical reaction is:

The rate constants $k_1$ and $k_2$ for two different reactions are $10^{16} \cdot e^{-2000/T}$ and $10^{15} \cdot e^{-1000/T},$ respectively. The temperature at which $k_1 = k_2$ is

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Which of the following statements is correct for the activation energy of a reaction?

Which of the following graphs of $\log \, K \rightarrow 1/T$ can be used to calculate the activation energy?

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