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19 June, 13:45

Nitrogen and oxygen form an extensive series of oxides with the general formula NxOy. One of them is a blue solid that comes apart, reversibly, in the gas phase. It contains 36.84% N. What is the empirical formula of this oxide?

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  1. 19 June, 17:09
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    Work out the number of moles in

    100.00 grams of the oxide.

    For nitrogen: The atomic mass of N is 14.0067, and we have 36.84 g N:

    36.84 g N14.0067 g N/mol N=2.630 mol N

    For oxygen: The atomic mass of O is

    15.9994, and we have

    100.00-36.84=63.16 g O:

    63.16 g N 15.9994 g N/mol N=3.948 mol N

    Now the ratio 3.958 2.630 is very close to

    1.5=32

    . So we conclude that the gas has three moles

    O to two moles N making the empirical formula

    N2O3.

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