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An exothermic reaction $\mathrm{x \rightarrow 4}$ has an activation energy $\mathrm{45 \, \, \mathrm{kJmol}^{-1}}$ . If energy change $\mathrm{\Delta E}$ during the reaction is $\mathrm{- 35 \, \mathrm{k} \mathrm{Jmol}^{-1}}$ . Calculate the activation energy for the reverse reaction in kJ.
Option: 1
$\mathrm{80 \mathrm{~kJ} \mathrm{~mol}^{-1}}$

Option: 2
$\mathrm{95 \mathrm{~kJ} \mathrm{~mol}^{-1}}$

Option: 3
$\mathrm{34 \mathrm{~kJ} \mathrm{~mol}^{-1}}$

Option: 4
$\mathrm{50 \mathrm{~kJ} \mathrm{~mol}^{-1}}$

Answers (1)

best_answer

$\mathrm{x \rightarrow y, }$ exothermic reaction $\mathrm{\Delta E}$ or $\mathrm{\Delta H=-20 k J}$ $\mathrm{mol ^{-1}}$

Given activation energy of the forward rxn

$\mathrm{ \begin{aligned} & (X \rightarrow Y) \\\\ & E_a^f=45 \mathrm{~kJ} \mathrm{~mol}^{-1} \end{aligned} }$
Activation energy of the backward rxn $\mathrm{(Y \rightarrow E)}$ , that is $\mathrm{E a^b}$

$\mathrm{\begin{aligned} & \Delta H=E_a^{+}-E_a^b \\\\ & E_a^b=E_a^f-\Delta H \\\\ & E_a^b=45-(-35) \\\\ & E_a^b=80 \, \mathrm{kJmOl}^{-1} \end{aligned}}$

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