Explain the rate of reaction with energy of activation and temperature with the help of the Arrhenius equation and state its importance.

(N/A) The Arrhenius equation describes the relationship between the rate constant of a chemical reaction and temperature:
$k = A e^{-\frac{E_{a}}{RT}}$
Where:
$k = \text{Rate constant of reaction (proportional to rate)}$
$E_{a} = \text{Activation energy (J mol}^{-1})$
$T = \text{Absolute temperature (K)}$
$R = \text{Gas constant (8.314 J K}^{-1} \text{ mol}^{-1})$
$A = \text{Arrhenius frequency factor (or pre-exponential factor)}$
Taking the natural logarithm of both sides:
$\ln k = -\frac{E_{a}}{RT} + \ln A$
This equation follows the linear form $y = mx + c$,where $\ln k$ is $y$,$-\frac{E_{a}}{R}$ is the slope $m$,$\frac{1}{T}$ is $x$,and $\ln A$ is the intercept $c$.
$A$ plot of $\ln k$ versus $\frac{1}{T}$ yields a straight line with a negative slope equal to $-\frac{E_{a}}{R}$ and a y-intercept equal to $\ln A$.
Importance:
$1$. It allows for the calculation of activation energy $(E_{a})$ and the frequency factor $(A)$ experimentally.
$2$. It explains why reaction rates increase with temperature,as the fraction of molecules with energy greater than $E_{a}$ increases exponentially with $T$.