Chemistry

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a compound of nitrogen and oxygen is 30.46% by mass N and 69.54% by mass O.
the molar mass if the compound was determined to be 92g/mol.

What is the empirical formula of the compound?

What is the molecular formula of the compound?

  • Chemistry -

    Take a 100 g sample which gives you
    30.46% N
    69.54% O

    Convert to mols.
    30.46/atomic mass N - about 2.2 but you can do it more accurately.
    69.54/atomic mass O = about 4.4

    Now find the ratio of the two to each other with the smaller number being no less than 1.00. You can see from the numbers that N1.00O2.00 is the ratio but you don't see that the easy way to do it is to divide the smaller number by itself then divide the other number by the same small number.
    2.2/2.2 = 1.00
    4.4/2.2 = 2.00
    empirical formula is NO2

    The molecular formula is some multiple of the empirical formula; i.e.
    (NO2)x = (14+32)x = 92 where x is the multile. 46*x = 92 and x = 2 so the molecular formula is (NO2)2 or N2O4.

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