Complete combustion of 4.20 g of a hydrocarbon produced 13.4 g of co2 and 4.81 g of h2o. what is the empirical formula for the hydrocarbon?

There is a complete combustion of the hydrocarbon.
13.4 g CO2 is produced
The number of moles of carbon is
13.4 g CO2(1 mol CO2/ 44 g CO2) (1 mol C/1 mol CO2) = 0.3045 mol C
4.81 g of H2O is produced
The number of moles of H is
4.81 g H2O (1 mol H2O/18 g H2O) (2 mol H/1 mol H2O) = 0.2672 mol H
Dividing greater number by the smaller number
0.3045 / 0.2672 = 1.14
The empirical formula is
CH

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