Consider the combustion of ethane (C2H6):

C2H6(g) + O2(g) -- CO2(g) + H2O(l)

If ΔG°f (in kJ/mol) for: C2H6(g) = -32.9, O2(g) = 0, CO2(g) = -394.4, and H2O(l) = -237.2; calculate ΔG° for the reaction.

Question

Consider the combustion of ethane (C2H6):

C2H6(g) + O2(g) --> CO2(g) + H2O(l)

If ΔG°f (in kJ/mol) for: C2H6(g) = -32.9, O2(g) = 0, CO2(g) = -394.4, and H2O(l) = -237.2; calculate ΔG° for the reaction.

anonymous · Answer

This is what I did

deltaG CO2+ deltaG H2O - [deltaG C2H6+ deltaG O2]
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-393.4-237.2+32.9= -598.7 

So is deltaG= -598.7 kJ ?