The question
Name: ______________________ Date: ____________ Getting iron from its ore (4 points)
Data table
Two reactions in a blast furnace
Iron is made from iron(III) oxide in a blast furnace. Data at 298 K. R = 8.314 J/(mol·K).
| Reaction | Equation | ΔG° (kJ/mol) |
|---|---|---|
| 1 | Fe₂O₃(s) → 2 Fe(s) + 3/2 O₂(g) | +742.2 |
| 2 | CO(g) + 1/2 O₂(g) → CO₂(g) | −257.2 |
(a) Calculate ΔG° for Fe₂O₃(s) + 3 CO(g) → 2 Fe(s) + 3 CO₂(g). [1 point]
(b) Explain how adding CO allows iron to be produced even though Reaction 1 is not thermodynamically favored. [1 point]
(c) Calculate the equilibrium constant for the overall reaction at 298 K. [1 point]
(d) Iron(III) oxide and CO can be stored together at 298 K for months with no detectable iron forming. Explain how this observation is consistent with your answer to part (a). [1 point]