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 9.5 mol of oxygen and 4.66 mol of nitrogen. 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 oxygen (O) = 9.5 mol - Moles of nitrogen (N) = 4.66 mol Next, we can find the ratio of nitrogen to oxygen by dividing the number of moles of each element by the smallest number of moles present: 1. Identify the smallest number of moles: - The smallest number of moles is 4.66 mol (for nitrogen). 2. Calculate the ratio: - For nitrogen: \[ \frac{4.66 \, \text{mol N}}{4.66 \, \text{mol}} = 1 \] - For oxygen: \[ \frac{9.5 \, \text{mol O}}{4.66 \, \text{mol}} \approx 2.03 \] 3. Since we need whole numbers for the chemical formula, we can round 2.03 to the nearest whole number, which is 2. Thus, the ratio of nitrogen to oxygen is approximately 1:2. Therefore, the empirical formula for the compound is \( \text{N}_1\text{O}_2 \) or simply \( \text{NO}_2 \). If \( x \) stands for a whole number, the complete chemical formula for the unknown compound is: \[ \text{N}_x\text{O}_2 \quad \text{where } x = 1 \] So, the complete chemical formula is: \[ \text{NO}_2 \]