For ${\mathrm{A}}_{2}+{\mathrm{B}}_{2}⇌2\mathrm{AB}$ ${\mathrm{E}}_{\mathrm{a}}$ for forward and backward reaction are $180$ and $200\mathrm{kJ}{\mathrm{mol}}^{-1}$ respectively. If catalyst lowers ${\mathrm{E}}_{\mathrm{a}}$ for both reaction by $100\mathrm{kJ}{\mathrm{mol}}^{-1}$. Which of the following statement is correct? [JEE Main 2025, 4 Apr (Shift 1)]

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YESPYQ · Accepted Answer

Correct answer: a) Catalyst does not alter the Gibbs energy change of a reaction.. A 2 + B 2 ⇌ 2AB E f = 180 kJ mol −1 E b = 200 kJ mol −1 ΔH = E f − E b = −20 kJ mol −1 In presence of catalyst: E f = 180 − 100 = 80 kJ mol −1 E b = 200 − 100 = 100 kJ mol −1 Catalyst does not change ΔH or ΔG of a reaction.

For \({\mathrm{A}}_{2}+{\mathrm{B}}_{2}⇌2\mathrm{AB}\) \({\mathrm{E}}_{\mathrm{a}}\) for forward and backward reaction a…

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