Final answer:
The hydrocarbon in the provided combustion reaction is a compound containing only carbon and hydrogen in the ratio of 422.6g and 70.4g respectively, based on the provided product masses. It falls within classes Alkane, Alkene, or Alkyne.
Step-by-step explanation:
In order to identify the hydrocarbon in this reaction, we first need to understand the combustion reaction of hydrocarbons. In a combustion reaction, a carbon-containing compound such as a hydrocarbon combines with oxygen to form carbon dioxide (CO2) and water (H2O). Each gram of carbon in the hydrocarbon generates 44/12 grams of CO2, while each gram of hydrogen generates 18/2 grams of H2O in the reaction.
To find the chemical formula of the hydrocarbon compound, we first calculate the mass of carbon and hydrogen from the masses of CO2 and H2O respectively. In 1549g of CO2, the number of grams of carbon is (1549g x 12/44) = 422.6g. Similarly, in 633.9g of H2O, the amount of hydrogen is (633.9g x 2/18) = 70.4g.
By subtracting these from the total mass of the hydrocarbon, we can calculate the amount of any other elements present. In this case, 493g (total mass) - 422.6g (Carbon) - 70.4g (Hydrogen) = 0g. This means our hydrocarbon contains only carbon and hydrogen in the ratio of 422.6g and 70.4g, therefore, it is likely to be a compound within the Alkane, Alkene, or Alkyne classes.
Learn more about Combustion of Hydrocarbon