## Fe2O3 (s hematite) + 3 CO (g) → 2 Fe (s alpha) + 3 CO2 (g)

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## Stoichiometry

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 Fe2O3          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

[2ΔHf(Fe (s alpha)) + 3ΔHf(CO2 (g))] - [1ΔHf(Fe2O3 (s hematite)) + 3ΔHf(CO (g))]
[2(0) + 3(-393.51)] - [1(-824.25) + 3(-110.54)] = -24.6600000000001 kJ
-24.66 kJ     (exothermic)

## Entropy Change

[2ΔSf(Fe (s alpha)) + 3ΔSf(CO2 (g))] - [1ΔSf(Fe2O3 (s hematite)) + 3ΔSf(CO (g))]
[2(27.28) + 3(213.68)] - [1(87.4) + 3(197.9)] = 14.4999999999999 J/K
14.50 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(Fe (s alpha)) + 3ΔGf(CO2 (g))] - [1ΔGf(Fe2O3 (s hematite)) + 3ΔGf(CO (g))]
[2(0) + 3(-394.38)] - [1(-742.24) + 3(-137.28)] = -29.0599999999999 kJ
-29.06 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-28.98 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

123417.00974
This process is favorable at 25°C.

## Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; pp 116, 224.
Kotz, John C., Treichel, Paul, and Weaver, Gabriela. Chemistry & Chemical Reactivity 6th ed.; Thomson Brooks/Cole: Belmont, CA, 2006; p 166.