For the Reaction H₂(g) + S(s) $\rarr$ H₂S(g) $\Delta$ H ^$\circ$ = -20

For the reaction H₂(g) + S(s) $\rarr$ H₂S(g) , $\Delta$ H ^$\circ$ = -20.2 kJ/mol and $\Delta$ S ^$\circ$ = +43.1 J/K·mol. Which of these statements is true

A) The reaction is only spontaneous at low temperatures.
B) The reaction is spontaneous at all temperatures.
C) ( $\Delta$ G ^$\circ$ ) becomes less favorable as temperature increases.
D) The reaction is spontaneous only at high temperatures.
E) The reaction is at equilibrium at 25 ^$\circ$ C under standard conditions.