Nitrogen dioxide (46.0 g/mol) forms from nitric oxide (28.0 g/mol) and oxygen (32.0 g/mol):2 NO(g) + O2(g) → 2 NO2(g)What is the volume change of the system when 36.0 g of NO2 is formed at a pressure of 1 atm and 300 K, assuming ideal gas behavior?

Calculate the initial and final moles of gas in the system. Initially, you have moles of NO and O2. Finally, you have moles of NO2. Use the stoichiometry from the previous step to determine these values.

Apply the ideal gas law to find the change in volume. The ideal gas law is \( PV = nRT \), where \( P \) is pressure, \( V \) is volume, \( n \) is the number of moles, \( R \) is the ideal gas constant (0.0821 L·atm/mol·K), and \( T \) is temperature. Calculate the initial and final volumes using the initial and final moles of gas.