If 50.0 g of CO2 (g) and 12.0g H2O (g) are formed when a hydrocarbon compound is burned in excess O2. What is the mass?
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When hydrocarbons are burned in a limited amount of air, both CO and CO2 form. When 0.450 g of a particular hydrocarbon was burned in air, 0.467 g of CO, 0.733 g of CO2, and 0.450 g of H2O were formed. (a) What is the empirical formula of the compound? (b) How many grams of O2 were used in the reaction? (c) How many grams would have been required for complete combustion?
A certain hydrocarbon that has a molar mass of is combusted. After the reaction, of this hydrocarbon yielded of and of . Determine the molecular formula of the compound.
19. When 1.125 g of a liquid hydrocarbon, CxHy, was burned, 3.447 g CO2 and 1.647 g H2O were produced. The molar mass of the compound was found to be 86.2 g/mol in a separate experiment. Determine the empirical and molecular formulas for the unknown hydrocarbon, CxHy.