In: Chemistry
The estimated average concentration of NO2 in air in the United States in 2006 was 0.016 ppm.
Calculate the partial pressure of the NO2 in a sample of this air when the atmospheric pressure is 748 torr (99.7 kPa ).
How many molecules of NO2 are present under these conditions at 17 ∘C in a room that measures 16 × 11 × 6 ft ?
Concentration of a gas in ppm is also equal to µmol/mol of the gas in the atmosphere. Therefore, the partial pressure of NO2 is given as
P(NO2) = (ppm concentration)*10-6*(atmospheric pressure) = (0.016)*10-6*(99.7 kPa)*(1000 Pa/1 kPa) = 0.0015952 Pa = 1.5952*10-3 Pa (ans).
Volume of the room = (16*11*6) ft3 = 1056 ft3 = (1056 cu.ft)*(28.3168 L/1 cu.ft) = 29902.5408 L (ans).
We know that 1 Pa = 9.8692*10-6 atm.
Use the ideal gas law to calculate the number of moles of NO2.
P*V = n*R*T
===> (1.5952*10-3 Pa)*(9.8692*10-6 atm/1 Pa)*29902.5408 L = n*(0.082 L-1tm/mol.K)*(273 + 17) K
===> n = 1.97967*10-5 mol.
We know that 1 mole of an ideal gas = 6.023*1023 molecules; therefore,
1.97967*10-5 mol NO2 = (6.023*1023*1.96967*10-5) molecules = 1.19235*1019 molecules ≈ 1.20*1019 molecules (ans).