Find the empirical formula of a compound that is 53.7% iron and 46.3% sulfur.What is the empirical mass of the said compound in g/mol?Use:Fe = 56 amuS = 32 amu

Step 1: Assume you have 100g of the compound. This means you have 53.7g of iron (Fe) and 46.3g of sulfur (S).

Step 2: Convert the mass of each element to moles.

For iron: 53.7g Fe * (1 mol Fe / 56g Fe) = 0.96 mol Fe

For sulfur: 46.3g S * (1 mol S / 32g S) = 1.45 mol S

Step 3: Write the ratio of the moles of each element to the smallest number of moles calculated.

For iron: 0.96 mol Fe / 0.96 = 1 mol Fe

For sulfur: 1.45 mol S / 0.96 = 1.51 mol S

Step 4: Since the empirical formula is the simplest whole number ratio of atoms in a compound, we round 1.51 to the nearest whole number, which is 2.

So, the empirical formula of the compound is FeS2.

Step 5: To find the empirical mass of the compound, add the atomic masses of all atoms in the empirical formula.

For FeS2: (1 * 56g/mol Fe) + (2 * 32g/mol S) = 56g/mol + 64g/mol = 120g/mol

So, the empirical mass of the compound is 120g/mol.