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23 September, 08:55

A 8.00g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 44./gmol, is burned completely in excess oxygen, and the mass of the products carefully measured: product mass carbon dioxide 24.01g water 13.10g Use this information to find the molecular formula of X.

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  1. 23 September, 09:18
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    C3H6.

    Explanation:

    Data obtained from the question:

    Mass of the compound = 8g

    Mass of CO2 = 24.01g

    Mass of H2O = 13.10g

    Next, we shall determine the mass of C, H and O present in the compound. This is illustrated below:

    Molar Mass of CO2 = 12 + (2x16) = 44g/mol

    Molar Mass of H2O = (2x1) + 16 = 18g/mol

    Mass of C in compound = Mass of C/Molar Mass of CO2 x 24.01

    => 12/44 x 24.01 = 6.5g

    Mass of H in the compound = Mass of H/Molar Mass of H2O x 13.1

    => 2x1/18 x 13.1 = 1.5g

    Mass of O in the compound = Mass of compound - (mass of C + Mass of H)

    => 8 - (6.5 + 1.5) = 0

    Next, we shall determine the empirical formula of the compound. This is illustrated below:

    C = 6.5g

    H = 1.

    Divide by their molar mass

    C = 6.5/12 = 0.54

    H = 1.4/1 = 1.

    Divide by the smallest

    C = 0.54/0.54 = 1

    H = 1/0.54 = 2

    Therefore, the empirical formula is CH2

    Finally, we shall determine the molecular formula as follow:

    The molecular formula of a compound is a multiple of the empirical formula.

    Molecular formula = [CH2]n

    [CH2]n = 44

    [12 + (2x1) ]n = 44

    14n = 44

    Divide both side by 14

    n = 44/14

    n = 3

    Molecular formula = [CH2]n = [CH2]3 = C3H6

    Therefore, the molecular formula of the compound is C3H6
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