For the hypothetical reaction $A_{2} (g) + B_{2} (g) ⟶ 2 A B (g)$
If $Δ G_{r}^{\circ}$ and $Δ S_{r}^{\circ}$ are $20 kJ / mol$ and $- 20 {JK}^{- 1} {mol}^{- 1}$ respectively at $200 K$ .

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$28 kJ / mol$

$20 kJ / mol$

$7.98 kJ / mol$

None of these

answer is A.

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Detailed Solution

$\begin{array}{l} Δ H^{\circ} = Δ G^{\circ} + T Δ S^{\circ} = 20 - \frac{20 \times 200}{1000} = 16 \\ Δ H_{T_{2}}^{\circ} - Δ H_{T_{1}}^{\circ} = Δ C_{P} (T_{2} - T_{1}) \\ Δ H_{T_{2}}^{\circ} = 16 + 20 \times \frac{200}{1000} \end{array}$

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