What is the mass of Fe₂O₃ required to produce 930 kg of iron (Fe) in the reaction: Fe₂O₃ + 3CO → 2Fe + 3CO₂?

• A. 1,860 kg
• B. 2,660 kg
• C. 1,330 kg
• D. 930 kg

Answer: (C)

Verified step by step guidance

1. Start by writing the balanced chemical equation for the reaction: ${\mathrm{Fe}}_2{O}_3+3\mathrm{CO}\to 2\mathrm{Fe}+3{\mathrm{CO}}_2$.
2. Calculate the molar mass of Fe₂O₃. The molar mass of iron (Fe) is approximately 55.85 g/mol and oxygen (O) is approximately 16.00 g/mol. Therefore, the molar mass of Fe₂O₃ is: $2\times 55.85+3\times 16.00$ g/mol.
3. Determine the molar mass of iron (Fe), which is approximately 55.85 g/mol.
4. Use stoichiometry to relate the moles of Fe produced to the moles of Fe₂O₃ required. From the balanced equation, 2 moles of Fe are produced from 1 mole of Fe₂O₃. Therefore, the moles of Fe₂O₃ required is half the moles of Fe produced.
5. Convert the mass of iron (930 kg) to grams (930,000 g) and calculate the moles of iron using its molar mass. Then, use the stoichiometric relationship to find the moles of Fe₂O₃ required. Finally, convert the moles of Fe₂O₃ to mass using its molar mass to find the mass of Fe₂O₃ needed.