A sample of an iron sulfide contains $2.561*g$ of metal, and $2.206*g$ of sulfur. What is the empirical formula of iron sulfide?

Md Ariful Islam

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$"Moles of iron"$ $=$ $(2.561*g)/(55.85*g*mol^-1)$ $=$ $0.0459*mol$

$"Moles of sulfur"$ $=$ $(2.206*g)/(32.06*g*mol^-1)$ $=$ $0.0688*mol$

If we divide thru by the lower molar quantity, we get, $FeS_(1.5)$. However, by definition, the empirical formula is the simplest WHOLE number that defines constituent in a species, so we double the formula to get WHOLE numbers:

$Fe_2S_3$.

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