Determine the molecular formula of an …
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Gaurav Seth 5 years, 1 month ago
We have given,
Mass percent of iron (Fe) =69.9%
Mass percent of oxygen (O)=30.1%
Number of moles of iron present in the oxide =69.90/55.85 =1.25
Number of moles of oxygen present in the oxide=30.1/16.0
=1.88
Ratio of iron to oxygen in the oxide,
1.25:1.88
=1:1.5
=2:3
Therefore the empirical formula of the oxide is Fe2O3.
Empirical formula mass of Fe2O3= [2(55.85) +3(16)]g
Molar mass of Fe2O3=159.69g
Thus, n= Molar mass/Empirical Formula mass =159.69/159.7g
=0.999 = 1(approx.)
Molecular formula of a compound is obtained by multiplying the empirical formula with n. Thus, the empirical formula of the given oxide is Fe2O3 and n is 1.
Hence, the molecular formula of the oxide is Fe2O3.
2Thank You