Calculate the change in Gibbs energy at 298K for the following reaction:
4NH3(g) + 3O2(g) -> 2N2(g) + 6H2O(l)
Given:
Gof(NH3(g)) = -16.45 KJ/mol
Gof(O2(g)) = 0.0 KJ/mol
Gof(N2(g)) = 0.0 KJ/mol
Gof(H2O(l)) = -237.129 KJ/mol
Balanced chemical equation is:
4 NH3(g) + 25 O2(g) ---> 2 N2(g) + 6 H2O(l)
ΔGo rxn = 2*Gof(N2(g)) + 6*Gof(H2O(l)) - 4*Gof( NH3(g)) - 25*Gof(O2(g))
ΔGo rxn = 2*(0.0) + 6*(-237.129) - 4*(-16.45) - 25*(0.0)
ΔGo rxn = -1356.974 KJ
Answer: 1357.0 KJ
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