Combustion of a 0.9835g sample of a compound containing only carbon, hydrogen, and oxygen produced 1.900g of CO2 and 1.070g of H2O. What is the empirical formula of the compound?

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23-07-2016
Chemistry

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Combustion of a 0.9835g sample of a compound containing only carbon, hydrogen, and oxygen produced 1.900g of CO2 and 1.070g of H2O. What is the empirical formula of the compound?

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meerkat18 meerkat18 · Answer 1 · 2016-07-27T13:33:40+02:00

the combustion reaction is CHO + O2 = H20 + CO2
The amount of carbon can be determined by the amount of carbon dioxide.
moles C = 1.90 g CO2 / 44 g/mol CO2 = 0.0432 moles C = 0.5182 g C
The amount of H can be derived from the amount of water
mole H = 1.070 g H2O / 18 g / mol H2O = 0.0594 g H

grams O is 0.9835 - 0.5182 g C - 0.0594 g H = 0.4059 g O.

transforming the determined masses to moles and dividing each to the least among the three, the empirical formula is C2H2O