In a blast furnace, iron(iii) oxide is used to produce iron by the following (unbalanced) reaction: fe2o3 + > 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?

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:

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?

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?

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.

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.

you gotta add the following molecules so we can give u an answer

explanation: