Complete combustion of 3.20g of a hydrocarbon produced 9.69g of co2 and 4.96g of h2o. what is the empirical formula for the hydrocarbon?

The empirical formula for the hydrocarbon : C₂H₅

Complete combustion of Hydrocarbons with Oxygen will be obtained by CO₂ and H₂O compounds.

If O₂ is insufficient there will be incomplete combustion produced by CO and H and O

Hydrocarbon combustion reactions (specifically alkanes)

Complete combustion of 3.20g of a hydrocarbon produced 9.69g of CO₂ and 4.96g of H₂O

Then the mass of C in CO₂: (molar mass of CO₂ = 44 g / mol, atomic mass C = 12 g / mol)

mass H in H2O (molar mass H2O = 18 g / mol, atomic mass H = 1 g / mol)

For example the hydrocarbons: CxHy

x and y are the mole ratio of C and H atoms

the mole ratio of C: H (from CO₂ and H₂O) is the same as the ratio of C and H in hydrocarbon compounds then:

mol C: mol H = 0.22: 0.5511 = 0.4 = 4: 10

So that the compound molecular formula: C₄H₁₀ or can be simplified in the form of the empirical formula C₂H₅

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