When 3.949 grams of a hydrocarbon,
CxHy, were burned in a combustion analysis
apparatus, 12.39 grams of CO2 and
5.073 grams of H2O were produced.
In a separate experiment, the molar mass of the compound was found
to be 56.11g/mol. Determine the empirical formula
and the molecular formula of the hydrocarbon.
| empirical formula = |
| molecular formula = |
Convert moles to grams by dividing by the Molecular weight:
Moles CO2=12.39/44.01=0.2815
Moles H2O=5.073/18.01=0.0.2815
Moles C=0.2815
Moles H = 0.2815×2= 0.563
Ratio C:H by moles = 0.2815 : 0.563⇒
1:2
So the empirical formula is CH2
Molecular weight of the compound is 56.11g/mol
Empirical formula molecular weight = 14
Thus Molecular formula = empirical formula * 4
= CH2 * 4 = C4H8
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