1. Gas Mixtures--Partial Pressure
So far: pure gases
Many gases are actually mixtures of two or more gases:
air: O2, N2 , H2O, etc
How do mixtures of gases behave?
Gas Mixtures--Partial Pressure

2. Gas Mixtures--Partial Pressure
P= 6 psi
P= 8 psi
P= 9 psi
O2 (g)
N2 (g)
CO2 (g)

3. Gas Mixtures--Partial Pressure
What happens when you put all three samples of gas together into one container (the same size container as each was in alone)?
The gases form a homogeneous mixture.
The pressure in the container increases, V and T stay the same
How do you know what the new pressure will be? P

4. Gas Mixtures--Partial Pressure
Each gas in a mixture behaves independently of the other gases present.
Each gas exerts its own pressure on the container.
PO = pressure exerted by O2
PN = pressure exerted by N2
PCO = pressure exerted by CO2 2 2 2

5. Gas Mixtures--Partial Pressure
Partial pressure: the pressure exerted by a particular gas present in a mixture
Dalton's Law of Partial Pressure: The total pressure of a mixture of gases equals the sum of the pressures that each would exert if it were present alone.
Ptotal = P1 + P2 + P3 + ………

6. Gas Mixtures--Partial Pressure
Ptotal = PO PN + PCO
So for this example:
Ptotal = 6 psi + 8 psi + 9 psi
= 23 psi 2 2 2

7. Partial Pressure In other words, at constant T and V,
Ptotal depends only on the total number of moles of gas present
Ptotal is independent of the type (or types) of gases present.

8. Partial Pressure-Mole Fraction
When describing a mixture of gases, it is useful to know the relative amount of each type of gas.
Mole fraction (X): a dimensionless number that expresses the ratio of the number of moles of one component compared to the total number of moles in a mixture.

9. Mole Fraction
If a gas mixture contains 5.0 mol O2 (g), 3.0 mol H2O (g), and 12.0 mol N2 (g),
XO=
On the exam, you must be able to calculate the mole fraction of each component of a gas mixture.
nO2
5.0 mol
= 0.25 = nt
20.0 mol

10. Partial Pressure
The partial pressure of a gas in a mixture can be found:
PA = XA Ptotal
where PA = partial pressure of gas A
XA = mole fraction of gas A
Ptotal = total pressure of mixture

11. Partial Pressure Calculation
A mixture of gases contains 0.51 mol N2, 0.28 mol H2, and 0.52 mol NH3. If the total pressure of the mixture is 2.35 atm, what is the partial pressure of H2?
PH2 = XH2 Ptotal
0.28 mol
XH2=
= 0.21
0.28 mol mol mol
PH2 = 0.21 x 2.35 = 0.50 atm

12. In the lab Chemical reaction producing gas
eg: NH4NO2 (s)  N2(g) + H2O (l)
Determine number of moles (amount) of gas collected?

13. Partial Pressures
When one collects a gas over water, there is water vapor mixed in with the gas. Ptotal = Pgas + PH2O
To find only the pressure of the desired gas, one must subtract the vapor pressure of water from the total pressure.
Table p1111 shows water vapor pressure (T dep)

14. Gas Mixtures--Partial Pressure
What is the partial pressure of O2 in a sample of gas collected over water if the total pressure was 745 torr at 25oC?
Given: Ptotal = 745 torr
T = 25oC
Find: Poxygen
Ptotal = PO2 + PH2O
Must find Pwater first.

15. Ptotal = Poxygen + Pwater
Partial Pressure
Ptotal = Poxygen + Pwater
To find Pwater, look in Appendix (p 1111):
At 25C, Pwater = torr
So:
745 torr = PO torr
PO2 = 745 torr torr = 721 torr

16. What is happening?

17. Effusion
Effusion is the escape of gas molecules through a tiny hole into an evacuated space.

18. Diffusion
Diffusion is the spread of one substance throughout a space or throughout a second substance.

19. Molecular Effusion & Diffusion
The rate of effusion (r) of a gas is inversely proportional to the square root of its molar mass, M.  1
rA = MA

21. Molecular Effusion & Diffusion
What does this all mean?
“Lighter” molecules will escape faster than “heavier” molecules.
If you want your balloons to stay inflated longer, use N2 instead of He because N2 has a higher molar mass.

22. Real Gases Real gases do not completely follow the ideal gas law.
In kinetic molecular theory, the following assumptions are made:
gas molecules occupy no space
gas molecules have no attraction for each other

23. Real Gases Neither assumption is correct.
Real gas molecules have a finite volume.
Real gas molecules do attract each other.

24. Real Gases The greatest deviation from ideal gas behavior occurs at:
high pressure
higher density of gas molecules
Molecules are closer together so:
finite volume of gas molecules more important
attraction between molecules more important

25. Real Gases
In the real world, the behavior of gases only conforms to the ideal-gas equation at relatively high temperature and low pressure.
Curves for 1 mol of gas

26. Real Gases Low temperature
Attractive forces between molecules becomes more important.
Average kinetic energy decreases.
Gas molecules have less energy to overcome attractive forces.

27. Real Gases
Even the same gas (e.g. nitrogen) will show wildly different behavior under high pressure at different temperatures.