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:
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.
