During a 45-minute road trip, a vehicle emitted 16.7 g of nitrogen dioxide (NO2). What is the mass of nitrogen atoms in this amount of NO2?

To determine the mass of nitrogen atoms contained in 16.7 g of nitrogen dioxide (NO2), we first need to understand the molar mass of NO2 and how it relates to its components.

Nitrogen dioxide is composed of one nitrogen atom and two oxygen atoms. The molar masses of these elements are approximately:

• Nitrogen (N): 14.01 g/mol
• Oxygen (O): 16.00 g/mol

To calculate the molar mass of NO2, we can use the formula: Molar mass of NO2 = (1 × molar mass of N) + (2 × molar mass of O) = (1 × 14.01 g/mol) + (2 × 16.00 g/mol) = 14.01 g/mol + 32.00 g/mol = 46.01 g/mol

Now, we can find the number of moles of NO2 in the 16.7 grams emitted by using the relation: Number of moles = mass / molar mass = 16.7 g / 46.01 g/mol ≈ 0.363 moles of NO2

Since there is one nitrogen atom per molecule of NO