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20 December, 10:11

What is the empirical formula of an oxide of nitrogen containing 63.61% by mass of nitrogen and 36.69% by mass of oxygen?

A. NO

B. N2O3

C. NO2

D. N2O

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Answers (1)
  1. 20 December, 10:18
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    D. N₂O

    Explanation:

    Let's assume we have 100 g of the compound. That means it consists of 63.61 grams of nitrogen and 36.69 grams of oxygen.

    Converting masses to moles:

    63.61 g N * (1 mol N / 14.01 g N) = 4.540 mol N

    36.69 g O * (1 mol O / 16.00 g O) = 2.293 mol O

    Normalize by dividing by the smallest:

    4.540 / 2.293 = 1.980 mol N

    2.293 / 2.293 = 1.000 mol O

    So there is approximately twice as many N atoms as O atoms. The empirical formula is therefore N₂O.
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