Question

In: Chemistry

The estimated average concentration of NO2 in air in the United States in 2006 was 0.016...

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 ?

Solutions

Expert Solution

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).


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