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19 October, 22:12

Combustion of 28.30 g of a compound containing only carbon, hydrogen, and oxygen produces 32.75 gco2 and 13.41 gh2o. What is the empirical formula of the compound?

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  1. 19 October, 22:34
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    The empirical formula is C₂H₄O₃.

    We must calculate the masses of C, H, and O from the masses given.

    Mass of C = 32.75 g CO₂ * (12.01 g C/44.01 g CO₂) = 8.9372 g C

    Mass of H = 13.4 g H₂O * (2.016 H/18.02 g H₂O) = 1.5067 g H

    Mass of O = Mass of compound - Mass of C - Mass of H

    = (28.30 - 8.9372 - 1.5067) g = 17.856 g

    Now, we must convert these masses to moles and find their ratios. If the ratios are not integers, we multiply them by a number to make them close to integers.

    From here on, I like to summarize the calculations in a table.

    Element m/g n/mol Ratio * 2 Integers

    C 8.9372 0.74415 1 2 2

    H 1.5067 1.4948 2.0086 4.0174 4

    O 17.856 1.1160 1.4997 2.9994 3

    The empirical formula is C₂H₄O₃.
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