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11 February, 07:05

Analysis of a compound of sulfur, oxygen and fluorine showed that it is 31.42% S and 31.35% O, with F accounting for the remainder. In a separate experiment, the molar mass of the compound was found to be 102.1 g/mol. Determine the molecular formula of the compound.

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  1. 11 February, 07:16
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    The molecular formula is SO2F2

    Explanation:

    Step 1: Data given

    Suppose the mass of compound = 100 grams

    The compound contains:

    31.42 % S = 31.42 grams S

    31.35 % O = 31.35 grams O

    100 - 31.42 - 31.35 = 37.23 F

    Molar mass of S = 32.065 g/mol

    Molar mass F = 19.00 g/mol

    Molar mass O = 16.00 g/mol

    Step 2: Calculate moles

    Moles = mass / molar mass

    Moles S = 31.42 grams / 32.065 g/mol

    Moles S = 0.9799 moles

    Moles 0 = 31.35 grams / 16.00 g/mol

    Moles 0 = 1.959 moles

    Moles F = 37.23 grams / 19.00 g/mol

    Moles F = 1.959 moles

    Step 3: Calculate mol ratio

    We divide by the smallest amount of moles

    S: 0.9799 / 0.9799 = 1

    F: 1.959 / 0.9799 = 2

    O : 1.959 / 0.9799 = 2

    The empirical formula is SO2F2

    This formula has a molecular mass of 102.06 g/mol

    This means the empirical formula is also the molecular formula : SO2F2
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