Answer:
To determine the number of moles of O2 needed to produce 24.7 g of Fe2O3, we first need to calculate the molar mass of Fe2O3.
The molar mass of Fe2O3 can be calculated by adding the atomic masses of iron (Fe) and oxygen (O) in the compound.
Molar mass of Fe = 55.845 g/mol
Molar mass of O = 15.999 g/mol
Molar mass of Fe2O3 = (2 * Molar mass of Fe) + (3 * Molar mass of O)
= (2 * 55.845 g/mol) + (3 * 15.999 g/mol)
= 111.69 g/mol + 47.997 g/mol
= 159.687 g/mol
Now, we can use the molar mass of Fe2O3 to calculate the number of moles.
Number of moles = Mass / Molar mass
= 24.7 g / 159.687 g/mol
≈ 0.1546 mol
According to the balanced chemical equation, the stoichiometric ratio between Fe2O3 and O2 is 3:3. This means that for every 3 moles of O2, we produce 2 moles of Fe2O3.
So, the number of moles of O2 needed can be calculated using the ratio:
Number of moles of O2 = (2 moles Fe2O3 / 3 moles O2) * 0.1546 mol
≈ 0.1029 mol
Therefore, approximately 0.1029 moles of O2 are needed to produce 24.7 g of Fe2O3.
