Consider the following reaction :
$2A (g) + B (g) \rightarrow 2D(g)$
$\Delta U^{\circ} = -10 \text{ kJ mol}^{-1}$ and $\Delta S^{\circ} = -44 \text{ J K}^{-1} \text{ mol}^{-1}$ at $298 \text{ K}$.
Identify the correct option with $\Delta G^{\circ}$ for the reaction and spontaneity of the reaction at $298 \text{ K}$.
(Given : $R = 8.31 \text{ J mol}^{-1} \text{ K}^{-1}$)

• A
  $+ 0.636 \text{ kJ mol}^{-1}$, non-spontaneous
• B
  $- 0.636 \text{ kJ mol}^{-1}$, spontaneous
• C
  $- 1.635 \text{ kJ mol}^{-1}$, spontaneous
• D
  $+ 1.635 \text{ kJ mol}^{-1}$, non-spontaneous