# Nitrogen and oxygen extensive series of oxides with the general formula N_xO_x. 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?

Dec 4, 2016

${\text{N"_2"O}}_{3}$.

#### Explanation:

Work out the number of moles in $100.00$ grams of the oxide.

For nitrogen: The atomic mass of $\text{N}$ is $14.0067$, and we have $36.84 \text{ g N}$:

(36.84" g N")/(14.0067" g N/mol N") = 2.630" mol N"

For oxygen: The atomic mass of $\text{O}$ is $15.9994$, and we have $100.00 - 36.84 = 63.16 \text{ g O}$:

(63.16" g N")/(15.9994" g N/mol N") = 3.948" mol N"

Now the ratio $\frac{3.958}{2.630}$ is very close to $1.5 = \frac{3}{2}$. So we conclude that the gas has three moles $\text{O}$ to two moles $\text{N}$ making the empirical formula $\textcolor{b l u e}{{\text{N"_2"O}}_{3}}$.