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

If the definition of the temperature coefficient of the reaction holds good for a reaction between $27^{\circ} C$ and $37^{\circ} C$,the activation energy for the reaction in $kJ \cdot mol^{-1}$ is

The rate of a reaction:

In the Arrhenius plot of $\log_{10} k$ versus $1 / T$,find the value of the intercept on the $y$-axis.

Which one of the following does not represent the Arrhenius equation?

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