For the following reaction:
16H2S(g) + 8SO2(g) → 3S8(g) + 16H2O(l)
Compound ΔH°f (kJ mol-1) S° (J mol-1 K-1)
H2S (g) -20.60 205.81
SO2 (g) -296.84 248.20
S8 (g) 0.00 430.23
H2O (l) -285.83 69.91
Calculate ΔG°rx (in kJ) at 506.3 K for this reaction. Assume ΔH°f and S° do not vary as a function of temperature.
In order to correctly calculate the answer for this question, should I: convert the S° values to kJ, and then multiply each ΔH°f and S° by their given coefficient in my balanced equation. Then use the formula ΔG = ΔH - ΔS(T) after I total all of my ΔH and and total all of my ΔS values?
I'm a little unsure how to go about solving this type of question...
Thank you very much in advance!