Thermodynamics

Consider the following reaction :

$$ \begin{aligned} & 2 \mathrm{~A}(\mathrm{~g})+\mathrm{B}(\mathrm{~g}) \rightarrow 2 \mathrm{D}(\mathrm{~g}) \\ & \Delta \mathrm{U}^{\ominus}=-10 \mathrm{~kJ} \mathrm{~mol}^{-1} \text { and } \Delta \mathrm{S}^{\ominus}=-44 \mathrm{JK}^{-1} \text { at } 298 \mathrm{~K} . \end{aligned} $$

Identify the correct option with $\Delta \mathrm{G}^{\ominus}$ for the reaction and spontaneity of the reaction at 298 K .

(Given : $\mathrm{R}=8.31 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$ )