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1 December, 09:24

A 5.00 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 78./gmol, is burned completely in excess oxygen, and the mass of the products carefully measured:

product mass

carbon dioxide 16.93g

water 3.46g

Use this information to find the molecular formula of X.

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Answers (1)
  1. 1 December, 10:44
    0
    C6H6

    Explanation:

    Step 1:

    Data obtained from the question. This include the following:

    Mass of the compound = 5g

    Molar mass of the compound = 78g/mol

    Mass of CO2 = 16.93g

    Mass of H2O = 3.46g

    Step 2:

    Determination of the mass of carbon, hydrogen and oxygen present ij the compound. This can be obtained as follow:

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

    Mass of C = 12/44 x 16.93 = 4.62g

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

    Mass of H = 2/18 x 3.46 = 0.38g

    Mass of O = 5 - (4.62 + 0.38) = 0

    Step 3:

    Determination of the empirical formula of the compound.

    C = 4.62g

    H = 0.38g

    Divide by their molar mass

    C = 4.62/12 = 0.385

    H = 0.38/1 = 0.38

    Divide by the smallest

    C = 0.385/0.38 = 1

    H = 0.38/0.38 = 1

    Therefore, the empirical formula of the compound is CH.

    Step 4:

    Determination of the molecular formula of the compound.

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

    The molecular formula = > [CH]n

    [CH]n = 78

    [12 + 1]n = 78

    13n = 78

    Divide both side by 13

    n = 78/13

    n = 6

    The molecular formula = > [CH]n

    => [CH]6

    => C6H6.

    Therefore, the molecular formula of the compound is C6H6.
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