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25 January, 07:54

The molar mass of a compound is 92 g/mol. Analysis of a sample of the compound indicates that it contains 0.606g of N and 1.390g of O. Find its molecular formula.

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Answers (2)
  1. 25 January, 08:07
    0
    N2O4

    Explanation:

    To obtain the molecular formula of the compound, first, let us calculate the empirical formula for the compound. This is illustrated below:

    N = 0.606g

    O = 1.390g

    Next, we divide the above by their molar masses

    N = 0.606/14 = 0.0432

    O = 1.390/16 = 0.0869

    Next, we divide by the smallest

    N = 0.0432/0.0432 = 1

    O = 0.0869/0.0432 = 2

    The empirical formula is NO2

    The molecular formula is given by:

    [NO2]n = 92

    [14 + (16x2) ]n = 92

    [14 + 32]n = 92

    46n = 92

    Divide both side by the coefficient of n i. e 46

    n = 92/46

    n = 2

    The molecular formula = [NO2]n = [NO2]2 = N2O4
  2. 25 January, 10:36
    0
    N2O4

    Explanation:

    Empericial formula

    N=0.606/14

    N=0.043

    O=1.390/16

    O=0.087

    Divide both N and O by the smallest number which is 0.043

    N=1

    O=2

    (NO2) n=92

    (14 + (16*2)) n=92

    (14+32) n=92

    46n=92

    Divide both sides by 46

    n=2

    Substitute n=2 in (NO2) n

    = (NO2) 2

    =N2O4
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