The question says that at standard conditions of 298 K and 1 atm pressure, N
2(g) + 3H
2(g)
2NH
3(g) has a ΔG° of -72.6 kJ/mol. What is the ΔG at 298K when the partial pressures are 0.450 atm for N
2, 0.450 atm for H
2, and 0.800 atm for NH
3?
My work:
ΔG = ΔG° + RTln(Q)
Q = (0.800)
2 / (0.450)(0.450)
3Q = 7.02
ΔG = -72.6 kJ/mol + 0.008314 kJ/mol·K x 298 K x ln7.02
ΔG = -67.8 kJ/mol
But this answer is wrong. Can someone tell me where I messed up? Thanks!