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:
<em>Fe₂O₃ + 3CO → 2Fe + 3CO₂,</em>
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.
<em>a) If 4.00 kg Fe₂O₃ are available to react, how many moles of CO are needed?</em>
- 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.
<u><em>Using cross multiplication:</em></u>
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.
<em>b) How many moles of each product are formed?</em>
- To find the no. of moles of Fe formed:
<em><u>Using cross multiplication:</u></em>
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:
<u><em>Using cross multiplication:</em></u>
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.
