Molar mass of iron(II) sulfide (FeS)

The molar mass of iron(II) sulfide (FeS) is 87.905 g/mol.

Step-by-step calculation

ElementAtomsAtomic massSubtotal
Iron × 1 55.845 = 55.845
Sulfur × 1 32.06 = 32.06
Total87.905 g/mol

Percent composition by element

  • Iron 63.53%
  • Sulfur 36.47%

Try another formula

H2O NaCl CO2 C6H12O6 H2SO4 Ca(OH)2 CuSO4·5H2O C8H10N4O2

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Related compounds

FeSO4 Iron(II) sulfate FeS2 Iron disulfide Fe2(SO4)3 Iron(III) sulfate FeSO4·7H2O Iron(II) sulfate heptahydrate (NH4)2Fe(SO4)2·6H2O Ammonium iron(II) sulfate hexahydrate H2SO4 Sulfuric acid

FAQ

What is the molar mass of FeS?

The molar mass of iron(II) sulfide (FeS) is 87.905 g/mol.

How do you calculate the molar mass of FeS?

Multiply the atomic mass of each element by the number of its atoms in FeS, then add the results: 1 × 55.845 (Fe) + 1 × 32.06 (S) = 87.905 g/mol.

What percentage of FeS is Iron?

Iron makes up 63.53% of the mass of iron(II) sulfide (FeS).