Question

In a blast furnace, iron(III) oxide is used to produce iron by the following (unbalanced) reaction: Fe2O3 + CO---------->Fe + CO2 a) If 4.00 kg FeO3 are available to react, how many moles of CO are needed? b) How many moles of each product are formed?

Answer 1

Answer:

a) The no. of moles of CO are needed = 75.15 mol.

b) The no. of moles of Fe are produced = 50.1 mol.

The no. of moles of CO₂ are needed = 75.15 mol.

Explanation:

• Firstly, we need to write the balanced reaction:

Fe₂O₃ + 3CO → 2Fe + 3CO₂,

It is clear that 1 mol of Fe₂O₃ reacts with 3 mol of CO to produce 2 mol of Fe and 3 mol of CO₂.

a) If 4.00 kg Fe₂O₃ are available to react, how many moles of CO are needed?

• We need to calculate the no. of moles of 4.00 kg Fe₂O₃:

n = mass/molar mass = (4000 g)/(159.69 g/mol) = 25.05 mol.

Using cross multiplication:

1 mol of Fe₂O₃ need  → 3 mol of CO to react completely, from stichiometry.

25.05 mol of Fe₂O₃ need  → ??? mol of CO to react completely.

∴ The no. of moles of CO are needed = (3 mol)(25.05 mol)/(1 mol) = 75.15 mol.

b) How many moles of each product are formed?

• To find the no. of moles of Fe formed:

Using cross multiplication:

1 mol of Fe₂O₃ produce  → 2 mol of Fe, from stichiometry.

25.05 mol of Fe₂O₃ produce  → ??? mol of Fe.

∴ The no. of moles of Fe are produced = (2 mol)(25.05 mol)/(1 mol) = 50.1 mol.

• To find the no. of moles of CO₂ formed:

Using cross multiplication:

1 mol of Fe₂O₃ produce  → 3 mol of CO₂, from stichiometry.

25.05 mol of Fe₂O₃ produce  → ??? mol of CO₂.

∴ The no. of moles of CO₂ are needed = (3 mol)(25.05 mol)/(1 mol) = 75.15 mol.