Iron (III) oxide solid and gaseous carbon monoxide yield iron solid and carbon dioxide gas?

1 mole of gas occupies 22.4 L at S.T.P.
Molar mass of Fe₂O₃ = 55.8×2 + 16.0×3 = 159.6 g/mol
Molar mass of Fe = 55.8 g
1 mole of molecules = 6.02 × 10²³

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


A)
Refer to the equation above. Mole ratio Fe₂O₃ : CO₂ = 1 : 3
No. of moles of CO₂ produced = 45.5/22.4 mol
No. of moles of Fe₂O₃ needed = (45.5/22.4) × (1/3) mol
Mass of Fe₂O₃ needed = 159.6 × (45.5/22.4) × (1/3) = 108 g


B)
Refer to the equation above. Mole ratio CO : CO₂ = 1 : 1
No. of moles of CO₂ produced = 45.5/22.4 mol
No. of moles of CO needed = 45.5/22.4 mol
No. of CO molecules needed = (6.02 × 10²³) × (45.5/22.4) = 1.22 × 10²⁴


C)
Refer to the equation above. Mole ratio Fe₂O₃ : Fe = 1 : 2
No. of moles of Fe₂O₃ = (4.56 × 10²³)/(6.02 × 10²³)
No. of moles of Fe = [(4.56 × 10²³)/(6.02 × 10²³)] × 2
Mass of Fe = 55.8 × [(4.56 × 10²³)/(6.02 × 10²³)] × 2 = 84.5 g