Correct statements regarding Arrhenius equation among the following...

The Arrhenius equation is given by $k = A e^{-E_a/RT}$.
Statement A: The factor $e^{-E_a/RT}$ represents the fraction of molecules having kinetic energy equal to or greater than the activation energy $E_a$. Thus, statement A is incorrect.
Statement B: From the equation, as $E_a$ decreases, the value of $k$ increases, leading to a faster reaction rate. Thus, statement B is correct.
Statement C: For many reactions, the temperature coefficient is approximately 2, meaning the rate of reaction doubles for every $10^{\circ}C$ rise in temperature. Thus, statement C is correct.
Statement D: Taking the natural logarithm of the Arrhenius equation, $\ln k = \ln A - \frac{E_a}{RT}$. Converting to base 10, $\log k = \log A - \frac{E_a}{2.303RT}$. A plot of $\log k$ vs $\frac{1}{T}$ gives a straight line with slope $= -\frac{E_a}{2.303R}$. The statement says slope $= -\frac{E_a}{R}$, which is only true for a $\ln k$ vs $\frac{1}{T}$ plot. Thus, statement D is incorrect.
Therefore, statements B and C are correct.