Hi please help
A 0.4647-g sample of a compound known to contain only carbon, hydrogen, and oxygen was burned in oxygen to yield 0.8635 g of CO2 and 0.1767 g of H2O. What is the empirical formula of the compound?
2007-01-28 09:53:20 · 3 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
From the mass of CO2, you can find the number of moles of C in the original compound
From the moles of water, you can calculate the number of moles of H in the original compound
Next, you'll need to find the moles of oxygen indirectly. Take the moles of C that you found and convert that to grams, and do the same with the moles of H. Add those two masses together and subtract the sum from the original mass of the compound. The difference is the mass of oxygen in the original compound. Convert that into moles of oxygen.
Finally, divide the moles of C, H and O by the smallest number of moles, and you'll have the ratios of moles of C to H to O (the empirical formula) of the original compound...
2007-01-28 10:04:08 · answer #1 · answered by hcbiochem 7 · 0⤊ 0⤋
Work out the actual mass of C in the CO2, and the actual mass of H in the H2O. These are your first two masses. The mass of O in the sample can then be found by adding them together, and subtracting from 0.4647g.
Then you do a normal empirical formula calculation.
2007-01-28 10:04:51 · answer #2 · answered by Gervald F 7 · 0⤊ 0⤋
yuo gotta find the percentages then the lowestnumbers of each you can have in a sample then find the multiple of each that multiplies the the total
2007-01-28 09:57:41 · answer #3 · answered by allottagame 2 · 0⤊ 3⤋