Consider the following plots of rate constant versus (1)/(T) for...

Consider the following plots of rate constant versus

\dfrac{1}{T}

for four different reactions. Which of the following orders is correct for the activation energies of these reactions?
Consider the following plots of rate constant versus (1)/(T) for four different reactions. Which of the following

Consider the following plots of rate constant versus (1)/(T) for four different reactions. Which of the following

Options

A ${E}_{b} > {E}_{a} > {E}_{d} > {E}_{c}$
B ${E}_{a} > {E}_{c} > {E}_{d} > {E}_{b}$
C ${E}_{c} > {E}_{a} > {E}_{d} > {E}_{b}$
D ${E}_{b} > {E}_{d} > {E}_{c} > {E}_{a}$

Correct answer

C. ${E}_{c} > {E}_{a} > {E}_{d} > {E}_{b}$

Step-by-step solution

$logk = logA - \dfrac{{E}_{a}}{2 .303 RT}$

Slope $= - \dfrac{{E}_{a}}{2 .303 RT} ⟹ {E}_{c} > {E}_{a} > {E}_{d} > {E}_{b}$

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