Final answer:
To find the masses of CO₂ and H₂O produced from the combustion of a compound with empirical formula C3H8O, we must use the combustion stoichiometry and molar masses of CO₂ and H₂O, adjusting for the empirical formula to get the correct masses of each compound produced.
Step-by-step explanation:
Combustion Analysis of C3H8O
To determine the masses of CO₂ and H₂O produced by the combustion of 0.986 g of a compound with the empirical formula C3H8O, we must first understand the stoichiometry of the combustion reaction. One mole of carbon yields one mole of CO₂, and two moles of hydrogen yield one mole of H₂O upon complete combustion. The molar mass of CO₂ (44.01 g/mol) and H₂O (18.016 g/mol) are needed for these calculations.
For carbon: The mass of carbon in CO₂ can be calculated by dividing the mass of CO₂ produced by its molar mass and multiplying by the molar mass of carbon (12.01 g/mol).
For hydrogen: The mass of hydrogen in H₂O can be calculated similarly by dividing the mass of H₂O produced by its molar mass and multiplying by the molar mass of hydrogen (1.008 g/mol).
Oxygen is present in both CO₂ and H₂O, and its mass in the original compound can be determined by difference from the total mass of the compound.
The molar masses of carbon, hydrogen, and oxygen must be considered to properly balance the chemical reaction and accurately account for all atoms in the compound. Using this information, the empirical formula of C3H8O can guide us in determining the correct ratio of CO₂ and H₂O produced.