Question

The temperature dependence of rate constant $(k)$ of a chemical reaction is written in terms of Arrhenius equation $k=A e^{-E_{\alpha} / R T}$. Activation energy $\left(E_{a}\right)$ of the reaction can be calculated by ploting

• 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

Answer: (B)

$k=A e^{-E_{a} / R T}$
$\log k=\log A-\frac{E_{a}}{2.303 R T}$
Comparing this equation with straight line
$y=m x+ c$
$y=\log k$ and $x-\frac{1}{T}$
$\therefore E_{a}$ is calculated with the help of slope by plotting the curve between $\log k$ and $\frac{1}{T}$.