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**Iron metal is produced in a blast furnace through a complex series of reactions the involve reduction of iron(III) oxide with carbon monoxide**

a. Write a balanced overall equation for the process, including the other product.

a. Write a balanced overall equation for the process, including the other product.

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

**b. Use the equations below the calculate ∆H of rxn for the overall equation:**

3Fe2O3(s) + CO(g) → Fe3O4(s) + CO2(g) ∆Ho = -48.5 kJ

Fe(s) + CO2(g) → FeO(s) + CO(g) ∆Ho = -11.0 kJ

Fe3O4(s) + CO(g) → 3FeO(s) + CO2(g) ∆Ho = 22.0 kJ

3Fe2O3(s) + CO(g) → Fe3O4(s) + CO2(g) ∆Ho = -48.5 kJ

Fe(s) + CO2(g) → FeO(s) + CO(g) ∆Ho = -11.0 kJ

Fe3O4(s) + CO(g) → 3FeO(s) + CO2(g) ∆Ho = 22.0 kJ

This what I come up with, i get 2/3 Fe3O4 on one side and 1/3 Fe3O4 on the other side giving me a 1/3 of Fe3O4 that dose not cancel each other out.

Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) ∆H= ?

Fe2O3(s) + 1/3CO(g) → 1/3Fe3O4(s) + 1/3CO2(g) ∆Ho = -16.17kJ

2FeO(s) + 2CO(g) → 2 Fe(s) + 2CO2(g) ∆Ho = +22.0 kJ

2/3Fe3O4(s) + 2/3CO(g) → 2FeO(s) + 2/3CO2(g) ∆Ho = +14.67 kJ