What is the molar mass of iron(II) chloride tetrahydrate? The error interval is +/- 2 g/mol.

Add the atomic masses of the atoms in FeCl2.4H2O.

I don't know the connection to the error interval with this question but +/- 2 g/mol sounds large to me.

Chemical Formula: FeCl₂ * H₂O

55.85 + 2(35.45) + 2(1.01) + 16.00 = 144.77 g/mol

To calculate the molar mass of iron(II) chloride tetrahydrate, we need to determine the molar mass of each individual element and then sum them up.

Iron(II) chloride contains two elements: iron (Fe) and chlorine (Cl). The molar mass of iron is 55.85 g/mol, and the molar mass of chlorine is 35.45 g/mol. Since there are two chlorine atoms in iron(II) chloride, we multiply the molar mass of chlorine by 2.

Molar mass of Fe: 55.85 g/mol
Molar mass of Cl: 35.45 g/mol x 2 = 70.90 g/mol

Now let's consider tetrahydrate. The prefix "tetra" indicates that there are four water molecules (H2O) associated with the iron(II) chloride. The molar mass of water is 18.02 g/mol. Since there are four water molecules, we multiply the molar mass of water by 4.

Molar mass of H2O: 18.02 g/mol x 4 = 72.08 g/mol

To calculate the molar mass of iron(II) chloride tetrahydrate, we add the molar masses of iron(II) chloride and tetrahydrate together.

Molar mass of iron(II) chloride tetrahydrate = Molar mass of FeCl2 + Molar mass of 4H2O
= 55.85 g/mol + 70.90 g/mol + 72.08 g/mol
= 198.83 g/mol

Therefore, the molar mass of iron(II) chloride tetrahydrate is 198.83 g/mol.

Considering the error interval of +/- 2 g/mol, we can state that the molar mass of iron(II) chloride tetrahydrate with the error margin is between 196.83 g/mol and 200.83 g/mol.