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Enthalpy of Reaction
[2ΔHf(CO2 (g))] - [2ΔHf(CO (g)) + 1ΔHf(O2 (g))]
[2(-393.51)] - [2(-110.54) + 1(0)] = -565.94 kJ
-565.94 kJ (exothermic)
[2ΔSf(CO2 (g))] - [2ΔSf(CO (g)) + 1ΔSf(O2 (g))]
[2(213.68)] - [2(197.9) + 1(205.03)] = -173.47 J/K
-173.47 J/K (decrease in entropy)
Free Energy of Reaction (at 298.15 K)
From ΔGf° values:
[2ΔGf(CO2 (g))] - [2ΔGf(CO (g)) + 1ΔGf(O2 (g))]
[2(-394.38)] - [2(-137.28) + 1(0)] = -514.2 kJ
-514.20 kJ (spontaneous)
From ΔG = ΔH - TΔS:
-514.22 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; p 184.
Kotz, John C., Treichel, Paul, and Weaver, Gabriela. Chemistry & Chemical Reactivity 6th ed.; Thomson Brooks/Cole: Belmont, CA, 2006; p 152.