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5 June, 13:30

A compound consists of 65.45% C, 5.492% H, and 29.06% O on a mass basis and has a molar mass of 110 g/mol. Determine the molecular formula of the compound.

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  1. 5 June, 13:50
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    The molecular formula is C6H6O2

    Explanation:

    Step 1: Data given

    Suppose the mass of the compound = 100 grams

    The compound has:

    65.45 % C = 65.45 grams

    5.492 % H = 5.49 grams

    29.06 % O = 29.06 grams

    Molar mass C = 12.01 g/mol

    Molar mass H = 1.01 g/mol

    Molar mass O = 16.00 g/mol

    Molar mass = 110 g/mol

    Step 2: Calculate moles

    Moles = mass / molar mass

    Moles C = 65.45 grams / 12.01 g/mol

    Moles C = 5.450 moles

    Moles H = 5.49 grams / 1.01 g/mol

    Moles H = 5.44 moles

    Moles O = 29.06 grams / 16.00 g/mol

    Moles O = 1.816 moles

    Step 3: Calculate mol ratio

    We divide by the smallest amount of moles

    Moles C = 5.450 moles / 1.816 = 3

    Moles H = 5.44 moles / 1.816 = 3

    Moles O = 1.816/1.816 = 1

    The empirical formula is C3H3O

    The molar mass of this formula is 55 g/mol

    We have to multiply the empirical formula by n

    n = 110/55 = 2

    2 * (C3H3O) = C6H6O2

    The molecular formula is C6H6O2
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