To determine the molar mass of FeSO4·6H2O (iron(II) sulfate hexahydrate), we need to consider the individual atomic masses of the elements present and account for the number of atoms of each element in the compound.
The formula FeSO4·6H2O indicates that there is one iron atom (Fe), one sulfur atom (S), four oxygen atoms (O), and six water molecules (H2O).
The atomic masses of the elements are as follows:
- Iron (Fe): 55.845 g/mol
- Sulfur (S): 32.06 g/mol
- Oxygen (O): 16.00 g/mol
- Hydrogen (H): 1.008 g/mol
To calculate the molar mass, we sum up the masses of the individual atoms:
Molar mass = (mass of Fe) + (mass of S) + (mass of O) + (mass of H) + (mass of O from H2O)
Molar mass = (1 × 55.845 g/mol) + (1 × 32.06 g/mol) + (4 × 16.00 g/mol) + (12 × 1.008 g/mol) + (6 × [(2 × 1.008 g/mol) + 16.00 g/mol])
Molar mass ≈ 55.845 g/mol + 32.06 g/mol + 64.00 g/mol + 12.096 g/mol + 194.04 g/mol
Molar mass ≈ 358.041 g/mol
Therefore, the molar mass of FeSO4·6H2O is approximately 358.041 grams per mole.