Using the equation 4Fe + 3O2 -> 2Fe2O3, calculae the total mass of oxgen needed to react wih all of 0.55 g of iron.
mols Fe = grams/molar mass = ?
mols O2 = ? mols Fe x (3 mol O2/4 mol Fe) = ?
?mols O2 x molar mass O2 = grams O2.
320
To calculate the total mass of oxygen needed to react with all of the iron (Fe), we need to use the balanced equation provided:
4Fe + 3O2 -> 2Fe2O3
From the equation, we can determine that for every 4 moles of iron, we need 3 moles of oxygen to form 2 moles of iron(III) oxide (Fe2O3).
First, we need to calculate the molar mass of iron (Fe) and oxygen (O2):
- The molar mass of Fe is 55.85 g/mol since its atomic mass is approximately 55.85 g/mol.
- The molar mass of O2 is 32.00 g/mol (16.00 g/mol x 2).
Now, let's calculate the number of moles of iron (Fe) present in 0.55 g of iron:
Number of moles = Mass (g) / Molar mass (g/mol)
Number of moles of Fe = 0.55 g / 55.85 g/mol
Number of moles of Fe ≈ 0.00985 mol
Using the stoichiometry of the balanced equation, we can determine the moles of oxygen (O2) needed:
Moles of O2 = (Number of moles of Fe / 4) x 3
Moles of O2 = (0.00985 mol / 4) x 3
Moles of O2 ≈ 0.00739 mol
Finally, we can calculate the mass of oxygen (O2) needed by multiplying the moles of O2 by its molar mass:
Mass of O2 = Moles of O2 x Molar mass of O2
Mass of O2 = 0.00739 mol x 32.00 g/mol
Mass of O2 ≈ 0.236 g
Therefore, the total mass of oxygen needed to react with all of 0.55 g of iron is approximately 0.236 g.