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An iron sulfide compound is analyzed, and found to contain 11.26 g iron and 9.70 g sulfur. Determine the molar ratio of sulfur to iron in this compound, and hence its chemical formula.

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Answer:

  • Molar ratio = 1.5
  • Chemical formula = Fe₂S₃

Explanation:

First we convert the given masses of each element into moles, using their respective molar masses:

  • Fe ⇒ 11.26 g ÷ 55.845 g/mol = 0.202 mol Fe
  • S ⇒ 9.70 g ÷ 32.065 g/mol = 0.302 mol S

Now we divide them in order to calculate the molar ratio of S to Fe:

  • 0.302 / 0.202 = 1.5

Meaning that for each 1 Fe mol, there's 1.5 S moles. We can write that as Fe₁S₁.₅

Finally we double those subscripts so that they become the lowest possible integers: Fe₂S₃.

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