Chemistry - Chemical Kinetics Question with Solution | TestHub

The Arrhenius equation, $k=A{e}^{-E_a/RT}$, describes the temperature dependence of the rate constant. Taking the natural logarithm gives $\ln k=\ln A-\frac{E_a}{RT}$. This is a linear equation ($y=mx+c$) when $\ln k$ is plotted against $1/T$, with slope $-\frac{E_a}{R}$. Thus, both statements are true, and the reason explains how activation energy is determined from the Arrhenius equation.