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 9.6 mol of nitrogen and 9.3 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) = 9.6 mol - Moles of oxygen (O) = 9.3 mol Next, we can find the simplest whole number ratio of nitrogen to oxygen by dividing both values by the smaller number of moles: 1. Divide the moles of nitrogen by the moles of oxygen: \[ \frac{9.6}{9.3} \approx 1.032 \] 2. Divide the moles of oxygen by the moles of oxygen: \[ \frac{9.3}{9.3} = 1 \] Now we have a ratio of approximately 1.032:1 for nitrogen to oxygen. To express this as whole numbers, we can round 1.032 to 1 (since it is very close to 1) and keep the ratio as 1:1. Thus, the ratio of nitrogen to oxygen is approximately 1:1, which suggests that the compound could be represented as \( \text{NO} \). Therefore, the complete chemical formula for the unknown compound is: \[ \text{NO} \]