Question

If 4000 g of Fe2O3 reacts, how many moles of CO are needed? (add work)

Answer 1

Answer:

75.15 mol.

Explanation:

• Firstly, we need to write the balanced equation of the reaction:

Fe₂O₃ + 3CO → 2Fe + 3CO₂.

It is clear that 1.0 mole of Fe₂O₃ reacts with 3.0 moles of CO to produce 2.0 moles of Fe and 3.0 moles of CO₂.

∴ Fe₂O₃ reacts with CO with (1: 3) molar ratio.

• we need to calculate the no. of moles of (4000 g) of Fe₂O₃:

no. of moles of Fe₂O₃ = mass/molar mass = (4000 g)/(159.69 g/mol) = 25.05 mol.

Using cross multiplication:

1.0 mole of Fe₂O₃ needs → 3.0 moles of CO,

∴ 25.05 mole of Fe₂O₃ needs → ??? moles of CO.

∴ The no. of moles of CO needed = (3.0 mol)(25.05 mol)/(1.0 mol) = 75.15 mol.