What is the empirical formula for a compound that contains 53.70% iron and 46.30% sulfur

Molar mass:

iron = 55.8 g/mol

Sulfur = 32.0 g/mol

Number of moles

53.70 / 55.8 = 0.96 moles 

46.30 / 32.0 = 1.44 moles

Using the values determines the entire lower proportion in moles of the elements, just divide by the smaller one

Fe = 0.96 / 0.96

Fe = 1 mole

S = 1.4 / 0.96

S = 1.5  moles 

 multiply them by 2.

iron : 2 * 1 = 2

Sulfur : 1.5 * 2 = 3

 the empirical formula is Fe₂S₃

hope this helps!