[leve]

 :delta:H = -285.4 kJ and  :delta:S = 137.4 J/K for the reaction
2 O3(g)  3 O2(g)
Calculate the equilibrium constant K for this reaction at 100 deg C.

The answer is 1.3E47

This is my work getting to the answer

 :delta:G =  :delta:H - T :delta:S
 :delta:G = -285400 - 373(137.4)
 :delta:G = -336650J

 :delta:G⁰ = -RTlnK
-336650 = -8.3145(373)lnK
K = 1.3E47

My question is is it correct that I replaced  :delta:G with  :delta:G⁰? Or is there another way to do the problem? I do not quite understand why :delta:G is replaced with  :delta:G⁰.


Thank you