Question

12.78 g of an organic compound containing C,H and O and undergoes combustion to produce 25.56 g of carbon dioxide and 10.46 g of water. what is the empirical formula of the organic compound?

plz solve​

Answer 1

Here is ur solution mate....>

moles C = 25.56 g CO2 x 1 mole CO2/44 g x 1 mole C/mole CO2 = 0.581 moles C

moles H = 10.46 g H2O x 1 mole H2O/18 g x 2 moles H/mole H2O = 1.16 moles H

To find moles of O, we can find grams of C and H and subtract that from total mass of 12.78 g and then convert to moles.

mass of C = 0.581 moles C x 12 g/mole = 6.97 g

mass of H = 1.16 moles H x 1 g/mole = 1.16 g

mass of O = 12.78 g - 6.97g -1.16 g = 4.65 g

moles O = 4.65 g O x 1 mole O/16 g = 0.291 moles

So, the empirical formula has 0.581 moles C, 1.16 moles H and 0.291 moles O. To get to whole numbers divide all by 0.291 to obtain 1.99 C, 3.98 H and 1 O. This translates to an empirical formula of C2H4O

Hope it helps uh..!