Answer:
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Step-by-step explanation:
To determine the empirical formula of the hydrocarbon, we need to determine the mass of carbon and hydrogen present in the compound. To do this, we can first convert the masses of carbon dioxide and water to the mass of carbon and hydrogen they contain.
The molecular formula of carbon dioxide is CO2, which means that each molecule of carbon dioxide contains 1 carbon atom and 2 oxygen atoms. Thus, the mass of carbon in 3.66 g of carbon dioxide is 3.66 g / (12.011 g/mol + 2*15.999 g/mol) = 0.836 g.
The molecular formula of water is H2O, which means that each molecule of water contains 2 hydrogen atoms and 1 oxygen atom. Thus, the mass of hydrogen in 1.50 g of water is 1.50 g / (2*1.008 g/mol + 15.999 g/mol) = 0.734 g.
To determine the empirical formula, we need to express the masses of carbon and hydrogen in terms of the number of moles. We can do this by dividing the mass of each element by its atomic weight. This gives us 0.836 g C / 12.011 g/mol = 0.0695 mol C and 0.734 g H / 1.008 g/mol = 0.725 mol H.
To express these amounts in terms of the smallest whole numbers, we need to divide both numbers by the smaller number. In this case, the smaller number is 0.0695 mol C, so we divide both numbers by 0.0695 to get 1 mol C and 10.5 mol H. Since we want the empirical formula to be expressed in whole numbers, we round 10.5 mol H to 11 mol H.
Thus, the empirical formula for this hydrocarbon is C1H11.
To determine the molecular formula of the compound, we need to know the molar mass of the compound. The molar mass is given as 60 g/mol, which means that the compound has a molar mass of 60 g/mol.
Since the empirical formula of the compound is C1H11, the molecular formula must be C1H11 as well, since the molar mass of the compound is equal to the molar mass of the empirical formula. Therefore, the molecular formula of the compound is also C1H11.