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Enthalpy of Reaction
[1ΔHf(CO2 (g))] - [1ΔHf(C (s graphite)) + 1ΔHf(O2 (g))]
[1(-393.51)] - [1(0) + 1(0)] = -393.51 kJ
-393.51 kJ (exothermic)
[1ΔSf(CO2 (g))] - [1ΔSf(C (s graphite)) + 1ΔSf(O2 (g))]
[1(213.68)] - [1(5.69) + 1(205.03)] = 2.96000000000001 J/K
2.96 J/K (increase in entropy)
Free Energy of Reaction (at 298.15 K)
From ΔGf° values:
[1ΔGf(CO2 (g))] - [1ΔGf(C (s graphite)) + 1ΔGf(O2 (g))]
[1(-394.38)] - [1(0) + 1(0)] = -394.38 kJ
-394.38 kJ (spontaneous)
From ΔG = ΔH - TΔS:
-394.39 kJ (spontaneous)
Equilibrium Constant, K (at 298.15 K)
This process is favorable at 25°C.
Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; pp 202, 204, 224.