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  • The reaction is an exothermic reaction. Activation energy of the re

The reaction \mathrm{X \rightarrow Y} is an exothermic reaction. Activation energy of the reaction for x into y is \mathrm{175 \mathrm{~kJ} mol^{-1}.} Enthalpy of reaction is \mathrm{144 \mathrm{~kJ} mol^{-1}} The activation energy for the reverse reaction, \mathrm{y \rightarrow x} will be

Option: 1

\mathrm{290 \mathrm{~kJ} / \mathrm{mol}}


Option: 2

\mathrm{319 \mathrm{~kJ} / \mathrm{mol}}


Option: 3

\mathrm{119 \mathrm{~kJ} / \mathrm{mol}}


Option: 4

\mathrm{150 \mathrm{~kJ} / \mathrm{mol}}


Answers (1)

best_answer

\mathrm{ \begin{gathered} x \rightarrow \text { y } \quad \Delta H=-144 \mathrm{~kJ} / \mathrm{mol} \\\\ E_a=175 \mathrm{~kJ} / \mathrm{mol} \end{gathered} }

For Exothermic Reaction

           \mathrm{ \begin{aligned} & E_a(F \cdot R)=\Delta H+E_a(B \cdot R) \\\\ & 175=-144+E a(B \cdot R) \\\\ & E_a(B \cdot R)=319 \mathrm{~kJ} / m o l \end{aligned} }

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