a 1.000 - gram sample that contains 0.0128 moles od a hydrocarbon was burned in excess air to convert all the components to CO2 and H2O. if 3.385 grams of CO2 and 0.692 grams of H2O are produced, what is the empirical formula of the hydrocarbon? what is the molecular weight? what is the molecular formula?
2007-01-23 02:33:11 · 2 answers · asked by piangpiang 2 in Science & Mathematics ➔ Chemistry
First you can get the molecular weight of the hydrocarbon from its mass and the number of moles that you gave.
To get the moles of carbon in the compound, convert the mass of CO2 into moles. When you divide that number by the number of moles of the original compound, you'll calculate the number of carbon atoms in a single molecule.
Next, you take the mass of water formed and convert that to moles, then multiply that by 2 to get the number of moles of hydrogen in the compound. Again, divide the moles of hydrogen by the moles of the original compound to get the number of hydrogen atoms per molecule of the original hydrocarbon, and you're done!
2007-01-23 02:41:36 · answer #1 · answered by hcbiochem 7 · 0⤊ 0⤋
part A u change 1.39L to moles by dividing by 22.4. for hydrogen u do 22.3g/18.016g/mol then multiply by 2 to get mol of H. part B u do 3.13 g/L divded by the reciprocal of 22.4. part C its the answer for part B divided by molar mass of CH2. part D i have no idea.
2016-05-24 00:44:41 · answer #2 · answered by Anonymous · 0⤊ 0⤋