Given (i) 2Fe₂O₃(s) → 4Fe(s) + 3O₂(g); ΔrG° = +1487.0 kJ/mol (ii) 2CO(g) + O₂(g) → 2CO₂(g); ΔrG° = -514.4 kJ/mol Free energy change, ΔrG° for the reaction, 2Fe₂O₃(s) + 6CO(g) → 4Fe(s) + 6CO₂(g) will be?

(i) 2Fe₂O₃(s) → 4Fe(s) + 3O₂(g); ΔrG° = +1487.0 kJ/mol
(ii) 2CO(g) + O₂(g) → 2CO₂(g); ΔrG° = -514.4 kJ/mol
We need to find the ΔrG° for the reaction:
2Fe₂O₃(s) + 6CO(g) → 4Fe(s) + 6CO₂(g)
We can obtain this by manipulating equations (i) and (ii).
Multiply equation (ii) by 3:
3[2CO(g) + O₂(g) → 2CO₂(g)]
6CO(g) + 3O₂(g) → 6CO₂(g); ΔrG° = 3 * (-514.4 kJ/mol) = -1543.2 kJ/mol
Now add this to equation (i):
2Fe₂O₃(s) → 4Fe(s) + 3O₂(g); ΔrG° = +1487.0 kJ/mol

• 6CO(g) + 3O₂(g) → 6CO₂(g); ΔrG° = -1543.2 kJ/mol

2Fe₂O₃(s) + 6CO(g) → 4Fe(s) + 6CO₂(g); ΔrG° = +1487.0 kJ/mol - 1543.2 kJ/mol = -56.2 kJ/mol
Therefore, the free energy change for the reaction is approximately -56.2 kJ/mol. None of the given options exactly match this value. There may be a slight discrepancy due to rounding in the provided data.