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Enthalpy of Reaction
[2ΔHf(CO (g))] - [2ΔHf(C (s graphite)) + 1ΔHf(O2 (g))]
[2(-110.54)] - [2(0) + 1(0)] = -221.08 kJ
-221.08 kJ (exothermic)
[2ΔSf(CO (g))] - [2ΔSf(C (s graphite)) + 1ΔSf(O2 (g))]
[2(197.9)] - [2(5.69) + 1(205.03)] = 179.39 J/K
179.39 J/K (increase in entropy)
Free Energy of Reaction (at 298.15 K)
From ΔGf° values:
[2ΔGf(CO (g))] - [2ΔGf(C (s graphite)) + 1ΔGf(O2 (g))]
[2(-137.28)] - [2(0) + 1(0)] = -274.56 kJ
-274.56 kJ (spontaneous)
From ΔG = ΔH - TΔS:
-274.57 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 138, 204.
Swaddle, T.W. Inorganic Chemistry; Academic Press: San Diego, 1997; p 372.
Kotz, John C. and Treichel, Paul. Chemistry & Chemical Reactivity 4th ed.; Thomson Brooks/Cole: Belmont, CA, 1999; p 157.