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

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mpumpkin | (Level 1) Valedictorian

Posted February 3, 2013 at 6:46 PM via web

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

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

Posted February 4, 2013 at 2:42 AM (Answer #1)

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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.

 

Note

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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