[chanelo]

The question says that at standard conditions of 298 K and 1 atm pressure, N₂(g) + 3H₂(g) 2NH₃(g) has a ΔG° of -72.6 kJ/mol. What is the ΔG at 298K when the partial pressures are 0.450 atm for N₂, 0.450 atm for H₂, and 0.800 atm for NH₃?
My work:
ΔG = ΔG° + RTln(Q)
Q = (0.800)² / (0.450)(0.450)³
Q = 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!

[CrazyAssasin]

You made a mistake in calculations. Reaction quotient is 15,6 for me.

[chanelo]

Oops, I think I must have entered the partial pressure for H₂ as ² instead of ³. Thanks!