N₂(g) + 3H₂(g) = 2NH₃(g)
K = 5.6 x 10⁵ at 298 K
∆Hºᵣₓₙ = -91.8 kJ/molᵣₓₙ
The synthesis of NH₃ is represented by the equation above. Based on the equilibrium constant, K, and ∆H⁰ᵣₓₙ given above, which of the following can best be used to justify that the reaction is thermodynamically favorable at 298 K and constant pressure?
a. ∆G⁰ = -RT in K > 0 because K>>1
b. ∆G⁰ = -RT in K < 0 because K>>1
c. ∆G⁰ = ∆H⁰ - T∆S⁰ < 0 because ∆H⁰ < 0 and ∆S⁰ > 0
d. ∆G⁰ = ∆H⁰ - T∆S⁰ > 0 because ∆H⁰ <0 and ∆S⁰ < 0