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In conversion of lime-stone to lime, ${CaCO}_{3} (s) ⟶ CaO (s) + {CO}_{2} (g)$ the value of $Δ H^{\circ}$ and $Δ S^{\circ}$ are $+ 179.1 kJ {mol}^{- 1}$ and $160.2 J / K$ respectively at 298 K and 1 bar. Assuming that $Δ H^{\circ}$ and $Δ S^{\circ}$
do not change with temperature, temperature above which conversion of lime-stone to lime will be just spontaneous is :

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detailed solution

Correct option is B

Here, Gibbs free energy is less than zero.

$\begin{array}{l} Δ G^{\circ} < 0 \\ \Rightarrow Δ H^{\circ} - T Δ S^{\circ} < 0 \\ \Rightarrow T > \frac{Δ H^{\circ}}{Δ S^{\circ}} = \frac{179.1 \times 10^{3}}{160.2} = 1118 K \end{array}$

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