Chemistry
posted by Matt .
Calculate ∆G (in kJ) at 541 K for the following reaction under the given conditions. Use data obtained from the table below and assume that ∆Hfo and So do not vary with temperature. Report your answer to three significant figures in scientific notation (i.e. 1.23E4).
2 H2S (g) + 3 O2 (g) ⇌ 2 SO2 (g) + 2 H2O (l)
Compound ÄHfo So P (atm)
H2S (g) 20.6 205.81 2.3
O2 (g) 0 205.7 9.9
SO2 (g) 296.81 248.2 6.3
H2O (l) 285.83 69.91 
I know how to do the question, I was just confused about the Q value, it turns out to be a negative and so I can't take the ln of it. What do I do?

Can you turn the reaction around (which will change the sign of K?) and work it that way. Then after finding delta G for the reverse direction, that can be reversed again for delta G in the original direction.

I didn't post three of the same answers on purpose.