Question

If an oxide of nitrogen contains 25.9% by mass of nitrogen, what is its empirical formula? * 1 point Captionless Image A B C D E

Answer 1

Step-by-step explanation:

Assuming that we have 100 g of the sample, then we have 25.9 g of nitrogen and 100-25.9 or 74.1 g of oxygen.

Dividing by the molar mass, we get
`(25.9)/(14)` moles of N and
`(74.1)/(16)` moles of O (1.85 moles of N and 4.63125 moles of O).

Dividing we get the simplified formula as
`N_(1) O_(2.5)`.

Multiplying by 2, we get the empirical and molecular formula as
`N_(2) O_(5)`.