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Consider the following plots of rate constant(k) versus $(\frac{1}{T})$ for four different reactions(a,b,c & d). Which of the following orders is correct for the activation energies of these reactions?

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Ea > Ec > Ed > Eb

Ec > Ea > Ed > Eb

Eb > Ea > Ed > Ec

Eb > Ed > Ec > Ea

answer is B.

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Detailed Solution

$k = {Ae}^{- Ea / RT}$ Arrheneous equation

$logk = logA - \frac{E_{a}}{RT}$

Roughly, K depends on activation energy ( $E_{a}$ )

$A E = E_{c} > E_{a} > E_{d} > E_{b}$

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