N₂(g)+3H₂(g)⇄2NH₃(g) K=5.6×10⁵ at 298K ΔH°rxn=−91.8kJ/molrxn

The synthesis of NH3 is represented by the equation above. Based on the equilibrium constant, K, and ΔH°rxn given above, which of the following can best be used to justify that the reaction is thermodynamically favorable at 298K and constant pressure?


a) ΔG°=−RTlnK<0 because K>>1
b) ΔG°=−RTlnK>0 because K>>1
c) ΔG°=ΔH°−TΔS°<0 because ΔH°<0 and ΔS°>0
d) ΔG°=ΔH°−TΔS°>0 because ΔH°<0 and ΔS°<0