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)

$\log \,k\,vs\,\frac{1}{T}$

Answer 2

$k=A e^{-E_{a} / R T}$ $\log k=\log A-\frac{E_{a}}{2.303 R T}$ 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 $\frac{1}{T}$.