## H2O (g) + 1 CO (g) → H2 (g) + CO2 (g)

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## Stoichiometry

Enter a mass or volume in one of the boxes below. Upon hitting submit, the stoichiometric equivalents will be calculated for the remaining reactants and products. All gases are assumed to be at STP.

 H2O            Mass: g or Gas Volume: L CO             Mass: g or Gas Volume: L H2             Mass: g or Gas Volume: L CO2            Mass: g or Gas Volume: L Heat Released: kJ

## Enthalpy of Reaction

[1ΔHf(H2 (g)) + 1ΔHf(CO2 (g))] - [1ΔHf(H2O (g)) + 1ΔHf(CO (g))]
[1(0) + 1(-393.51)] - [1(-241.82) + 1(-110.54)] = -41.15 kJ
-41.15 kJ     (exothermic)

## Entropy Change

[1ΔSf(H2 (g)) + 1ΔSf(CO2 (g))] - [1ΔSf(H2O (g)) + 1ΔSf(CO (g))]
[1(130.59) + 1(213.68)] - [1(188.72) + 1(197.9)] = -42.35 J/K
-42.35 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(H2 (g)) + 1ΔGf(CO2 (g))] - [1ΔGf(H2O (g)) + 1ΔGf(CO (g))]
[1(0) + 1(-394.38)] - [1(-228.59) + 1(-137.28)] = -28.51 kJ
-28.51 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-28.52 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

98858.456849
This process is favorable at 25°C.

## Reference(s):

Jolly, William L. The Chemistry of the Non-Metals; Prentice-Hall: Englewood Cliffs, New Jersey, 1966; p 3.
Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 264.