Question

The temperature dependence of rate constant $\left(k\right)$ of a chemical reaction is written in terms of Arrhenius equation, $k=A{e}^{-E_a/RT}$. Activation energy $\left(E_a\right)$ of the reaction can be calculated by plotting:

• A. $\log k$ vs $T$
• B. $\log k$ vs $\frac{1}{T}$
• C. $k$ vs $T$
• D. $k$ vs $\frac{1}{\log T}$

Answer 1

The correct option is B $\log k$ vs $\frac{1}{T}$

$\log \left(k\right)=\log \left(A\right)-\frac{E_a}{2.303R}.\frac{1}{T}$

so a $\log \left(k\right)$ us $\frac{1}{T}$ plot gives us all of the information.