Correct statements regarding Arrhenius equation among the following are :
A. Factor $$e^{-Ea / RT}$$ corresponds to fraction of molecules having kinetic energy less than Ea.
B. At a given temperature, lower the Ea, faster is the reaction.
C. Increase in temperature by about $$10^{\circ}C$$ doubles the rate of reaction.
D. Plot of log k vs $$\frac{1}{T}$$ gives a straight line with slope = $$- \frac{Ea}{R}$$.
Choose the correct answer from the options given below :

Arrhenius equation: $$k = Ae^{-E_a/RT}$$, or $$\ln k = \ln A - \frac{E_a}{RT}$$.

A. Factor $$e^{-E_a/RT}$$ corresponds to fraction of molecules having kinetic energy less than $$E_a$$.

The Boltzmann factor $$e^{-E_a/RT}$$ represents the fraction of molecules with energy GREATER than or equal to $$E_a$$, not less than. FALSE.

B. At a given temperature, lower the $$E_a$$, faster is the reaction.

Lower $$E_a$$ means $$e^{-E_a/RT}$$ is larger, giving larger $$k$$. TRUE.

C. Increase in temperature by about 10°C doubles the rate of reaction.

This is the general empirical observation (van't Hoff rule). TRUE (approximately).

D. Plot of $$\log k$$ vs $$1/T$$ gives straight line with slope = $$-E_a/R$$.

$$\log k = \log A - \frac{E_a}{2.303RT}$$. The slope is $$-\frac{E_a}{2.303R}$$, not $$-E_a/R$$. FALSE.

Correct statements: B and C.

The correct answer is Option D: B and C Only.