Question

Consider the following plots of rate Consider the following plots of rate $\frac{1}{T}$ for four different reactions. Which of the following orders is correct for the activation energies of these reactions ?

• A. $E_{b} > E_{a} > E_{d} > E_{c}$
• B. $E_{a} > E_{c} > E_{d} > E_{b}$
• C. $E_{b} > E_{d} > E_{c} > E_{a}$
• D. $E_{c} > E_{a} > E_{d} > E_{b}$

Answer 1

Answer: (D)

$log \,K=\frac{-Ea}{2.3030RT}+log\,A$
Acrroding to Arrhenius equation plot of $'log\, K'$
$Vs. \frac{1}{T}$ is linear with.
Slope $=\frac{-Ea}{2.3030R}$
From plot we conclude :
$\underset{\text{(magnitude)}}{\text{|Slope|}}: C>a>d>b$
$\therefore E_{c}>E_{a}>E_{d}>E_{b}$