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

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## Stoichiometry

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 Heat Added: kJ FeO            Mass: g C              Mass: g Fe             Mass: g CO             Mass: g or Gas Volume: L

## Enthalpy of Reaction

[1ΔHf(Fe (s alpha)) + 1ΔHf(CO (g))] - [1ΔHf(FeO (s)) + 1ΔHf(C (s graphite))]
[1(0) + 1(-110.54)] - [1(-271.96) + 1(0)] = 161.42 kJ
161.42 kJ     (endothermic)

## Entropy Change

[1ΔSf(Fe (s alpha)) + 1ΔSf(CO (g))] - [1ΔSf(FeO (s)) + 1ΔSf(C (s graphite))]
[1(27.28) + 1(197.9)] - [1(60.75) + 1(5.69)] = 158.74 J/K
158.74 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Fe (s alpha)) + 1ΔGf(CO (g))] - [1ΔGf(FeO (s)) + 1ΔGf(C (s graphite))]
[1(0) + 1(-137.28)] - [1(-251.46) + 1(0)] = 114.18 kJ
114.18 kJ     (nonspontaneous)

From ΔG = ΔH - TΔS:
114.09 kJ     (nonspontaneous)

## Equilibrium Constant, K (at 298.15 K)

9.8950134418e-021
This process is not favorable at 25°C.

## Reference(s):

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