Question

In a separate experiment, the student is given a sample of powdered Fe(s) that contains an inert impurity. The student uses a procedure to oxidize the Fe(s) in the sample to Fe₂O₃(s). The student collects the following data during the experiment.

Mass of Fe(s) with inert impurity: 6.724 g
Mass of Fe₂O₃(s) produced: 7.531 g

Calculate the number of moles of Fe in the Fe₂O₃(s) produced.

Answer 1

To calculate the number of moles of Fe in Fe₂O₃(s), divide the mass of Fe₂O₃ by its molar mass. The stoichiometric mole ratio between Fe and Fe₂O₃ is 1:1, so the number of moles of Fe in the Fe₂O₃(s) is also 0.0472 mol.

Step-by-step explanation:

To calculate the number of moles of Fe in Fe₂O₃(s), we need to use the given data:

Mass of Fe(s) with inert impurity = 6.724 g

Mass of Fe₂O₃(s) produced = 7.531 g

We can calculate the number of moles of Fe₂O₃ using its molar mass:

Molar mass of Fe₂O₃ = 2(55.85 g/mol) + 3(16.00 g/mol) = 159.70 g/mol

Number of moles of Fe₂O₃ = Mass of Fe₂O₃ / Molar mass of Fe₂O₃ = 7.531 g / 159.70 g/mol = 0.0472 mol

Since the stoichiometric mole ratio between Fe and Fe₂O₃ is 1:1, the number of moles of Fe in Fe₂O₃ is also 0.0472 mol. Therefore, the number of moles of Fe in the Fe₂O₃(s) produced is 0.0472 mol.