Question

a chemical compound composed of nitrogen and oxygen was carefully analyzed and found to consist of 36.8% nitrogen. determine the empirical formula of the unknown compound.
you have correctly selected 0.

Explanation:

Step1: Find oxygen percentage

Since the compound is only N and O,
$\text{Oxygen percentage} = 100\% - 36.8\% = 63.2\%$

Step2: Assume 100g sample, get masses

Mass of N: $m_N = 36.8\ \text{g}$, Mass of O: $m_O = 63.2\ \text{g}$

Step3: Calculate moles of each element

Molar mass of N: $M_N=14.01\ \text{g/mol}$, Molar mass of O: $M_O=16.00\ \text{g/mol}$
Moles of N: $n_N = \frac{36.8}{14.01} \approx 2.63\ \text{mol}$
Moles of O: $n_O = \frac{63.2}{16.00} = 3.95\ \text{mol}$

Step4: Divide by smallest mole value

Smallest mole value is $2.63\ \text{mol}$
Ratio of N: $\frac{2.63}{2.63} = 1$
Ratio of O: $\frac{3.95}{2.63} \approx 1.5$

Step5: Scale to whole numbers

Multiply both ratios by 2 to eliminate decimals:
N: $1 \times 2 = 2$, O: $1.5 \times 2 = 3$

Answer:

$\text{N}_2\text{O}_3$