Answer:
We can use the ideal gas law, PV = nRT, to solve for the density at STP (standard temperature and pressure). At STP, the temperature is 273.15 K and the pressure is 1 atm. We know the molar mass of NO2 is 46.01 g/mol. We also know that 1 mole of any gas at STP occupies a volume of 22.4 L.
First, we can calculate the number of moles of NO2 at STP:
n = PV/RT = (1 atm)(22.4 L)/(0.08206 L·atm/mol·K)(273.15 K) = 1.00 mol
Next, we can calculate the mass of 1 mole of NO2:
46.01 g/mol
Finally, we can calculate the density of NO2 at STP:
density = mass/volume = (46.01 g/mol)/(22.4 L) = 2.054 g/L
Therefore, the density at STP of NO2 gas (molar mass = 46.01 g/mol) in grams per liter is 2.054 g/L.
Step-by-step explanation: