9. a compound consists of 17.6% hydrogen and 82.4% nitrogen. determine the empirical formula of the compound.

Explanation:

Step1: Assume 100g of the compound

This allows us to convert percentages to grams. So we have 17.6 g of hydrogen (H) and 82.4 g of nitrogen (N).

Step2: Calculate the number of moles of each element

The molar mass of H is approximately 1 g/mol and of N is approximately 14 g/mol. For hydrogen: $n_{H}=\frac{17.6\ g}{1\ g/mol}=17.6\ mol$ For nitrogen: $n_{N}=\frac{82.4\ g}{14\ g/mol}\approx5.89\ mol$

Step3: Find the mole - ratio of the elements

Divide the number of moles of each element by the smallest number of moles among them. Here, the smallest is approximately 5.89 mol. For hydrogen: $\frac{17.6\ mol}{5.89\ mol}\approx3$ For nitrogen: $\frac{5.89\ mol}{5.89\ mol}=1$

Answer:

$NH_{3}$