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 cataly

Step-by-step solution

As per the question 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 ) Ae - 300 × 10 3 600 × R = Ae - Ea 300 × R ⇒ 10 3 2 = Ea 300 ⇒ E a = 150 × 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 =