Fe₂O₃ reacts with carbon to produce carbon dioxide.
The equation for the reaction is:
2Fe₂O₃(s) + 3C(s) → 4Fe(s) + 3CO₂(g)
Calculate the volume of carbon dioxide gas at room temperature and pressure that is produced from 40.0 kg of Fe₂O₃ using excess carbon.
Relative formula mass (Mᵣ): Fe₂O₃ = 160
The volume of 1 mole of any gas at room temperature and pressure is 24 dm³.

This is a reacting mass calculation that involves finding the volume of a gaseous product. **Step 1: Convert the mass of Fe₂O₃ to grams.** The Mᵣ is given in g/mol, so we must work in grams. 40.0 kg × 1000 g/kg = 40000 g **Step 2: Calculate the moles of Fe₂O₃.** Moles = Mass / Mᵣ Moles(Fe₂O₃) = 40000 g / 160 g/mol = 250 mol **Step 3: Use the molar ratio from the balanced equation to find the moles of CO₂.** The equation is 2Fe₂O₃ + 3C → 4Fe + 3CO₂. The ratio of Fe₂O₃ to CO₂ is 2 : 3. This means for every 2 moles of Fe₂O₃ that react, 3 moles of CO₂ are produced. Moles(CO₂) = Moles(Fe₂O₃) × (3/2) Moles(CO₂) = 250 mol × 1.5 = 375 mol **Step 4: Calculate the volume of CO₂ gas.** The volume of 1 mole of any gas at room temperature and pressure (RTP) is 24 dm³. Volume = Moles × Molar Volume Volume(CO₂) = 375 mol × 24 dm³/mol Volume(CO₂) = 9000 dm³