4Fe + 3O2 = 2Fe2O3
158g of Fe will react with how many litres of O2 to produce the maximum amount of Fe2O3
mols Fe ==> grams/molar mass = ?
Convert to mols O2. That's ?mols Fe x (3 mols O2/4 mols Fe) = ?
Then mols O2 x 22.4 L/mol = L O2
To solve this problem, we need to determine the number of moles of Fe and O2 and then use the balanced chemical equation to calculate the stoichiometry of the reaction. Finally, we can convert the moles of O2 to liters using the ideal gas law.
1. Calculate the number of moles of Fe:
First, we need to determine the molar mass of Fe (iron) from the periodic table. The molar mass of Fe is approximately 55.85 g/mol.
Number of moles of Fe = mass of Fe (g) / molar mass of Fe
Number of moles of Fe = 158 g / 55.85 g/mol
Number of moles of Fe ≈ 2.827 mol
2. Use the balanced chemical equation to determine the stoichiometry:
The balanced chemical equation shows that 4 moles of Fe react with 3 moles of O2 to produce 2 moles of Fe2O3. Therefore, the stoichiometric ratio of Fe to O2 is 4:3.
3. Calculate the number of moles of O2:
Using the stoichiometric ratio, we can determine the number of moles of O2 that will react with 2.827 moles of Fe.
Number of moles of O2 = (Number of moles of Fe / ratio of Fe to O2) * ratio of O2 to Fe
Number of moles of O2 = (2.827 mol / 4) * 3
Number of moles of O2 ≈ 2.12025 mol
4. Convert moles of O2 to liters:
To convert moles of O2 to liters, we can use the ideal gas law, which states that the volume of a gas is directly proportional to the number of moles at a constant temperature and pressure. At standard temperature and pressure (STP), 1 mole of any ideal gas occupies approximately 22.4 liters.
Number of liters of O2 = Number of moles of O2 * 22.4 L/mol
Number of liters of O2 ≈ 2.12025 mol * 22.4 L/mol
Number of liters of O2 ≈ 47.48 L (rounded to two decimal places)
Therefore, approximately 47.48 liters of O2 will react with 158g of Fe to produce the maximum amount of Fe2O3.