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?
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Answers
There are no organic compounds that contain c, h and o, since these are not chemical elements. They should be written as C, H, O. Also, co2 should be written as CO2.
Now, on to answering the question. You need to find the MOLES of C, H and O in order to find the empirical formula.
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