Question

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

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

Answer 1

Answer: (A)

As we know that Arrhenius equation is given as
$K=\text{A}\text{e}^{- \frac{E_{a}}{\text{RT}}}$
$log K=log ⁡ A-\frac{E_{a}}{2.303 \, R T}$
$\text{Slope}=-\frac{E_{a}}{2.303 \text{ R}}$
Slope $c>a>d>b.$
$E_{c}>E_{a}>E_{d}>E_{b}$