In the recovery of iron from iron ore, the reduction of the ore is actually accomplished by reactions involving carbon monoxide. Use the following thermochemical equations,

Question

Fe2O2(s) + 3CO(g) ---> 2Fe(s) +3CO2(g)
ΔH° = -28kJ

3Fe2O2(s) + CO(g) ---> 2Fe3O4(s)+ CO2(g)
ΔH° = -59kJ

Fe3O4(s) + CO(g) ---> 3FeO(s) + CO2(g)
ΔH° = +38kJ

What is ΔH° for the reaction
FeO(s) + CO(g) ---> Fe(s) +CO2(g)

Answer 1

Note that Fe2O2 isn't correct. Didn't you intend to type Fe2O3

Answer 2

Correction:
3Fe2O3(s) + CO(g) ---> 2Fe3O4(s)+ CO2(g)
ΔH° = -59kJ
Is this right?
FeO(s) + CO(g) ---> Fe(s) +CO2(g)
ΔH° = -28/2
ΔH° = -14

Answer 3

No, I don't get that answer. I only went through it once so I could have made an error. Here is what I did.
The reverse of twice equation 3 + the reverse of equation 2 + 3x equation 1 and that gave me
6FeO + 6CO ==> 6Fe + 6CO2 and -101 kJ/mol. That divided by 6 = about -17 kJ/mol.