Correct statements regarding Arrhenius equati | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

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

In the given graph,$E_{a}$ for the reverse reaction will be (in $kJ$)

For a reaction,the threshold energy is $75 \ kJ/mol$. If the internal energy of the reactants is $20 \ kJ/mol$,the activation energy (in $kJ/mol$) is

For a chemical reaction,if the temperature is increased from $25\,^{\circ}C$ to $55\,^{\circ}C$,the rate of reaction will change by a factor of (Assume $\mu = 3$).

Collision theory is applicable to

Vedclass Test Series

Exam Paper Generator

Online Exam Module