Final answer:
The empirical formula of the compound is C₃H₄. which corresponds to option 4.
Step-by-step explanation:
The empirical formula of a compound can be determined from the masses of carbon dioxide and water produced during combustion. In this case, we have 66.0 g of CO₂ and 36.0 g of H₂O.
To find the empirical formula, we need to determine the molar amounts of carbon and hydrogen in the compound. From the mass of CO₂, we can calculate the moles of carbon present. Using the molar mass of carbon dioxide (44 g/mol), we find that there are 1.5 moles of carbon (66.0 g / 44 g/mol).
Similarly, from the mass of H₂O, we can calculate the moles of hydrogen. Using the molar mass of water (18 g/mol), we find that there are 2 moles of hydrogen (36.0 g / 18 g/mol).
Since the ratio of carbon to hydrogen in the compound is 1.5:2, we can simplify it to a ratio of 3:4. Therefore, the empirical formula of the compound is C₃H₄, which corresponds to option 4.