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  •  For a reversible reaction A  B, the <img alt="\Delta" src="https://entrancecorn

 For a reversible reaction A \rightleftharpoons B, the \Delta H forward reaction =25 \mathrm{kJmol}^{-1}. The activation energy of the uncatalyzed forward reaction is 350\mathrm{KJ} \mathrm{mol}^{-1}. When the reaction is catalysed keeping the reactant concentration same, the rate of the catalysed forward reaction at 37^{\circ} \mathrm{C} is found to be same as that of the untatalyzed reaction at 427^{\circ} \mathrm{C}. Calculate the activation energy of the catalyzed reaction \mathrm{ \left \{ backward \right \}} in \mathrm{KJ \mathrm{mol}^{-1}.}

Option: 1

85.7


Option: 2

94.5


Option: 3

33.7


Option: 4

84.2


Answers (1)

best_answer

By Arrhenius eq :-
\mathrm{\begin{aligned} & K=A e^{(-E a / R T)} \\ & A e^{-\frac{250 \times 10^3}{+700 \times R}}=A e^{\frac{-E a}{310 \times R}} \\ & \frac{250 \times 10^3}{700}=\frac{E a}{310} \\ & E a=\frac{250 \times 310 \times 10^3}{700} \\ & E a=110.7 \mathrm{kJmol}^{-1} \end{aligned}}

\therefore Activation energy of catalysed backward Reaction
Energy of activation for backward reaction
\mathrm{\begin{aligned} & E_b=E_a-\Delta H \\ & E_b=110.7-25 \\ & E_b=85.7 \end{aligned} }

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shivangi.shekhar

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