For a reversible reaction A B, the H forward reaction = 20 kJ mol -1 . The activation energy of the uncatalyzed forward reaction is 300 kJ mol -1 . When the reaction is catalysed keeping the reactant concentration same, the rate of the catalysed forward reaction at 27°C is found to be same as that of the uncatalyzed reaction at 327°C. The activation energy of the catalysed backward reaction is kJ mol -1 .
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To determine the activation energy of the catalyzed backward reaction, we need to use the Arrhenius equation and the given information.
The Arrhenius equation is given by:
k = Ae (-Ea/RT)
E a = 150 x 10 3 J mol -1
E a = 150 kJ mol -1
Activation energy of catalysed backward reaction
Energy of activation for backward reaction E b = E a - 
H
= 150 - 20 = 130 kJ mol -1
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