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11 May, 02:32

A sample of a compound contains 3.21 g of sulfur and 11.4 g of fluorine. Which of the following represents the empirical formula of the compound?

(A) SF2 (B) SF3 (C) SF4 (D) SF5 (E) SF6

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  1. 11 May, 03:03
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    The empirical formula is SF6 (option E)

    Explanation:

    Step 1: Data given

    Mass of sulfur = 3.21 grams

    Mass of fluorine = 11.4 grams

    Molar mass sulfur = 32.065 g/mol

    Molar mass fluorine = 19.00 g/mol

    Step 2: Calculate moles

    Moles = mass / molar mass

    Moles sulfur = 3.21 grams / 32.065 g/mol

    Moles sulfur = 0.100 moles

    Moles fluorine = 11.4 grams / 19.00 g/mol

    Moles fluorine = 0.600 moles

    Step 3: Calculate mol ratio

    We divide by the smallest amount of moles

    S: 0.100 / 0.100 = 1

    F : 0.600 / 0.100 = 6

    The empirical formula is SF6 (option E)
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