An unknown compound has the following chemical formula: where \( x \) stands for a whole number. Measurements also show that a certain sample of the unknown compound contains 5.4 mol of nitrogen and 10.84 mol of oxygen. Write the complete chemical formula for the unknown compound.

To determine the complete chemical formula for the unknown compound, we need to find the ratio of nitrogen (N) to oxygen (O) in the sample. Given: - Moles of nitrogen (N) = 5.4 mol - Moles of oxygen (O) = 10.84 mol Next, we can find the simplest whole number ratio of nitrogen to oxygen by dividing both quantities by the smaller number of moles, which is 5.4 mol. 1. Calculate the ratio of nitrogen: \[ \text{Ratio of N} = \frac{5.4 \, \text{mol}}{5.4 \, \text{mol}} = 1 \] 2. Calculate the ratio of oxygen: \[ \text{Ratio of O} = \frac{10.84 \, \text{mol}}{5.4 \, \text{mol}} \approx 2.009 \] Since we need whole numbers, we can round 2.009 to the nearest whole number, which is 2. Thus, the ratio of nitrogen to oxygen is approximately 1:2. This means the empirical formula of the compound is \( \text{NO}_2 \). Therefore, the complete chemical formula for the unknown compound is: \[ \text{NO}_2 \]