Final answer:
The molar mass of Fe(NH₄)₂(SO₄)₂·6H₂O is calculated by summing the atomic masses of iron, ammonium, sulfate, and water based on their quantity in the formula.
Step-by-step explanation:
Determining the Molar Mass of Fe(NH₄)₂(SO₄)₂·6H₂O
To find the molar mass of Fe(NH₄)₂(SO₄)₂·6H₂O, we must calculate the sum of the atomic masses of all atoms in the formula. This is a compound with a complex composition including iron (Fe), ammonium (NH₄), sulfate (SO₄), and water molecules (H₂O). The molar mass is calculated by adding together the masses of the individual atoms in the formula, considering their respective quantities. The compound includes one iron atom, two ammonium groups, two sulfate groups, and six water molecules. Using the periodic table, we find the mass of each atom and multiply it by the number of times it appears in the chemical formula. Then, we sum these values to obtain the molar mass.
To help you understand, let's work out an example for ammonium (NH₄). The atomic mass for nitrogen (N) is approximately 14.00 amu, and for hydrogen (H), it's approximately 1.00 amu. Ammonium has one nitrogen atom and four hydrogen atoms. Therefore, the mass of an ammonium ion is (1 x 14.00) + (4 x 1.00) = 18.00 amu.
If we follow this method for the entire compound Fe(NH₄)₂(SO₄)₂·6H₂O, we'd calculate the molar mass by adding the masses of iron, ammonium, sulfate, and water, each multiplied by the number of times they appear in the formula.