## FeO (s) + 1 CO (g) → Fe (s alpha) + CO2 (g)

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## Stoichiometry

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 FeO            Mass: g CO             Mass: g or Gas Volume: L Fe             Mass: g CO2            Mass: g or Gas Volume: L Heat Released: kJ

## Enthalpy of Reaction

[1ΔHf(Fe (s alpha)) + 1ΔHf(CO2 (g))] - [1ΔHf(FeO (s)) + 1ΔHf(CO (g))]
[1(0) + 1(-393.51)] - [1(-271.96) + 1(-110.54)] = -11.01 kJ
-11.01 kJ     (exothermic)

## Entropy Change

[1ΔSf(Fe (s alpha)) + 1ΔSf(CO2 (g))] - [1ΔSf(FeO (s)) + 1ΔSf(CO (g))]
[1(27.28) + 1(213.68)] - [1(60.75) + 1(197.9)] = -17.69 J/K
-17.69 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Fe (s alpha)) + 1ΔGf(CO2 (g))] - [1ΔGf(FeO (s)) + 1ΔGf(CO (g))]
[1(0) + 1(-394.38)] - [1(-251.46) + 1(-137.28)] = -5.63999999999999 kJ
-5.64 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-5.74 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

9.7306136842
This process is close to or at equilibrium at 25°C.

## Reference(s):

Swaddle, T.W. Inorganic Chemistry; Academic Press: San Diego, 1997; p 378.