A compound is found to contain 63.52 % iron and 36.48 % sulfur. What is its empirical formula.

Asked on by mpumpkin

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jeew-m | College Teacher | (Level 1) Educator Emeritus

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Let us consider we have 100g of the compound.

So then we will have 63.52g of iron and 36.48g of sulphur.


Molic weight

Fe = 56g/mol

S = 32g/mol


Amount of Fe moles in 100g of compound `= 63.52/56 = 1.1343` mol

Amount of S moles in 100g of compound `= 36.48/32 = 1.0133` mol


So the mole ratio of


So the empirical formula of the compound is FeS.



Usually FeS is also a frequent compound between Fe and S. So the chemical formula of the compound can also be FeS.


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