Question

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

• A. $\log kvs\frac{1}{\log T}$
• B. $\log kvs\frac{1}{T}$
• C. $kvsT$
  
• D. $kvs\frac{1}{\log T}$

Answer 1

Answer: (B)

$\log kvs\frac{1}{T}$

According to Arrhenius equation,
$k=A{e}^{-E_a/RT}$
$lnk=lnA-\frac{E_a}{RT}$
or
$logk=logA-\frac{E_a}{2.303RT}$
Hence, $E_a$ is calculated with the help of slope $m=-\frac{E_a}{2.303\times R}$.