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24 February, 12:12

A 0.02877 g sample of gas occupies 10.0-ml at 289.0 k and 1.10 atm. upon further analysis, the compound is found to be 38.734% c and 61.266% f. what is the molecular formula of the compound? (order: c, x)

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  1. 24 February, 12:30
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    Assuming ideal gas, we calculate the number of moles.

    PV = nRT

    n = PV / RT

    n = (1.10 atm) (10 x 10^-3L) / [ (0.08205746 L atm / mol K) (289 K) ]

    n = 4.64 x 10^-4 mol

    SO the molar mass is:

    molar mass = 0.02877 grams / 4.64 x 10^-4 mol

    molar mass = 62.02 g/mol

    The only possible combination is:

    C2F2

    C = 12 * 2 = 24

    F = 19 * 2 = 38

    24 + 38 = 62 g/mol
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