For the reversible reaction.
\(\mathrm{A}(\mathrm{s})+\mathrm{B}(\mathrm{g}) \rightleftharpoons \mathrm{C}(\mathrm{g})+\mathrm{D}(\mathrm{g});\)
\(\Delta \mathrm{G}^{\circ}=-350 \mathrm{~kJ}\)
Which one of the following statements is true?

In the reversible reaction,
\[
\begin{aligned}
\mathrm{A}(\mathrm{s})+\mathrm{B}(\mathrm{g}) \rightleftharpoons \mathrm{C}(\mathrm{g})+\mathrm{D}(\mathrm{g}) \\
\Delta \mathrm{G}^{\circ}=-350 \mathrm{~kJ}
\end{aligned}
\]
Since, the randomness increases (because solid is changing into gas), entropy will increase and thus, \(\Delta \mathrm{S}\) is positive. Reversible reaction never undergo to completion (ie, never be instantaneous).
\(\because\) For the given reaction, \(\Delta \mathrm{G}^{\circ}=-350 \mathrm{~kJ}\) and we know that
\[
\begin{aligned}
\Delta G^{\circ} &=-R T \log K \\
-350 &=-R T \log K
\end{aligned}
\]
ie, \(\mathrm{K}\) (equilibrium constant) is greater than one. Moreover, the reaction is thermodynamically feasible.