How do I find the empirical formula of FeSO4? Thanks!

Yes

To find the empirical formula of FeSO4, you need to determine the ratio of the atoms present in the compound. Here are the steps:

Step 1: Write down the elements present in the compound and their respective symbols. In this case, there are three elements: iron (Fe), sulfur (S), and oxygen (O).

Step 2: Determine the number of atoms of each element present in the compound. The subscript numbers in the chemical formula indicate the number of atoms of each element. In FeSO4, there is one Fe, one S, and four O atoms.

Step 3: Simplify the ratio of atoms by dividing each number of atoms by the greatest common divisor (GCD) of all the numbers. In this case, the GCD of 1, 1, and 4 is 1.

So, the simplified ratio of atoms is 1:1:4.

Step 4: Write down the final empirical formula using the simplified ratio. In this case, the empirical formula is FeSO4.

Therefore, the empirical formula of FeSO4 is FeSO4.

To find the empirical formula of FeSO4, you need to determine the ratio of the elements in the compound using their masses or percentages.

Step 1: Find the atomic masses of each element involved.
The atomic mass of iron (Fe) is approximately 55.845 g/mol.
The atomic mass of sulfur (S) is approximately 32.06 g/mol.
The atomic mass of oxygen (O) is approximately 16.00 g/mol.

Step 2: Determine the element's mass in the compound.
FeSO4 contains one iron atom (Fe), one sulfur atom (S), and four oxygen atoms (O). Therefore, you need to multiply the atomic mass of each element by the number of atoms of that element in FeSO4.
Fe: 1 x 55.845 g/mol = 55.845 g/mol
S: 1 x 32.06 g/mol = 32.06 g/mol
O: 4 x 16.00 g/mol = 64.00 g/mol

Step 3: Calculate the total mass of the compound.
Add up the masses of each element.
55.845 g/mol + 32.06 g/mol + 64.00 g/mol = 151.905 g/mol

Step 4: Find the molar ratio.
Divide each element's mass by the total mass of the compound to find the molar ratio.
Fe: 55.845 g/mol / 151.905 g/mol ≈ 0.367
S: 32.06 g/mol / 151.905 g/mol ≈ 0.211
O: 64.00 g/mol / 151.905 g/mol ≈ 0.421

Step 5: Simplify the ratio.
Divide each molar ratio by the smallest ratio.
Fe: 0.367 / 0.211 ≈ 1.74
S: 0.211 / 0.211 = 1
O: 0.421 / 0.211 ≈ 2

Step 6: Round to the nearest whole number.
Fe: 1.74 ≈ 2
S: 1
O: 2

Therefore, the empirical formula of FeSO4 is Fe2SO4.

FeSO4 is the empirical formula for iron(II) sulfate or ferrous sulfate.