What is the value of the equilibrium constant for transformation of carbon from graphite to diamond at 360.0 C?
Substance ΔfH0
kJ/mol S0
J/mol K
graphite 0.0 5.7
diamond 1.9 2.4
Substance ΔfH0
kJ/mol S0
J/mol K
graphite 0.0 5.7
diamond 1.9 2.4
-
So the reaction is C(graphite) --> C(diamond)
For this reaction ΔH = ΔHf(diamond) - ΔHf(graphite) = 1.9 kJ/mol
ΔS = So(diamond) - So(graphite) = 2.4 J/molK - 5.7 J/mol K = - 3.3 J/mol K
ΔG = ΔH - TΔS = 1900 J/mol - 633 K (-3.3 J/molK) = 3989 J/mol
Now ΔG = -RT ln K
3989 J/mol = - 8.314 J/molK (633K) ln K
ln K = -0.758
K = 0.47
For this reaction ΔH = ΔHf(diamond) - ΔHf(graphite) = 1.9 kJ/mol
ΔS = So(diamond) - So(graphite) = 2.4 J/molK - 5.7 J/mol K = - 3.3 J/mol K
ΔG = ΔH - TΔS = 1900 J/mol - 633 K (-3.3 J/molK) = 3989 J/mol
Now ΔG = -RT ln K
3989 J/mol = - 8.314 J/molK (633K) ln K
ln K = -0.758
K = 0.47