[hallie3]

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!

[Rutherford]

I don't see why you shouldn't. But, what exactly do you mean by 'total'? I guess that you are familiar with Hess law.