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NVAMediumJEE Main 2026 · 21 January, Shift 1Gibbs Free Energy & Equilibrium Constant

Chemistry Question from JEE Main 2026 · 21 January, Shift 1

Use the following data at 500 K500\,\text{K}:

SubstanceΔfH∘\Delta_f H^\circ / kJ mol−1^{-1}S∘S^\circ / J K−1^{-1} mol−1^{-1}
AB(g)AB(g)3232222222
A2(g)A_2(g)66146146
B2(g)B_2(g)xx280280
Data table at 500 K: AB(g) has standard enthalpy of formation 32 kJ per mole and standard entropy 222 J per kelvin per mole; A2(g) has 6 kJ per mole and 146 J per kelvin per mole; B2(g) has an unknown enthalpy of formation x and standard entropy 280 J per kelvin per mole.

One mole each of A2(g)A_2(g) and B2(g)B_2(g) are taken in a 1 L1 \, \text{L} closed flask and allowed to establish the equilibrium at 500 K500 \, \text{K}: A2(g)+B2(g)⇌2AB(g)A_{2}(g)+B_{2}(g) \rightleftharpoons 2AB(g). The value of xx (in kJ mol−1\text{kJ mol}^{-1}) is _____ . (Nearest integer)

(Given: log⁡K=2.2\log K = 2.2, R=8.3 J K−1mol−1R = 8.3 \, \text{J K}^{-1}\text{mol}^{-1})

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