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2 March, 14:44

A 10 g sample of a compound contain only carbon, hydrogen, and oxygen forms 23.98 g CO2 and 4.91 g H2O upon complete combustion. What is the empirical formula of the compound?

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  1. 2 March, 15:00
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    There are three major steps for finding an empirical formula from a combustion reaction.

    1.) Determine the grams of carbon and hydrogen from the given data.

    C: 23.98 g x (12.011 g / 44.01 g) = 6.54 g C

    H: 4.91 g x (2.0158 g / 18.02 g) = 0.55 g H

    Determine the grams of oxygen in the sample by subtracting the mass of the compound given from the total mass solved earlier.

    O: 10.0 - (6.54 + 0.55) = 2.91 g O

    2) Convert the values in step 1 to moles.

    C: 6.54 g / 12.01 g / mol = 0.54 mol

    H: 0.55 g / 1.01 g/mol = 0.54 mol

    O: 2.91 g / 16.00 g/mol = 0.18 mol

    3) Divide each by the lowest value calculated in step 2

    C: 0.54 mol / 0.18 mol = 3

    H: 0.54 mol / 0.18 mol = 3

    O: 0.18 mol / 0.18 mol = 1

    Thus, the empirical formula is C3H3O.
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