1. Chpt 5 - Gases Gas Law Development Dalton’s Partial pressure law
Graham’s effusion
Kinetic Theory
Root-mean-square velocity
van der Waals equation of state
HW: Chpt 5 - pg , #s 5, 22, 23, 25, 31, 32, 35, 39, 41, 46, 55, 64, 66, 71, 75, 77, 81, 91, 95, 97, 101, Due Mon 10/4

2. Torricelli barometer Pressure is? Units? The height in mm of mercury
above the surface of the resevoir
of mercury determines the pressure.
The units are mmHg.
mmHg is also the same unit as
Torr. i.e. standard pressure is 760 mmHg and 760 Torr

3. Simple Manometer Similar to the barometer,
the height difference of the Hg relates the pressure difference in the unknown gas bulb side to the current atmospheric pressure.
The higher Hg side has the _____ pressure.
(higher/lower)

4. Boyle’s Law
Constant temperature experiments demonstrated the PV=constant graphing this yields an inverse relationship
Thus if the pressure of volume changes at a constant temperature
P1V1 = P2V2

5. Plot of PV vs. P for Several Gases
This graph shows Boyles linear relationship for the PxV. The constant depends on the gas

6. Charles’s Law
Constant pressure experiments demonstrated that Volume is directly proportional to Temperature (Kelvin)
V1 = V2
T T2
Several gases were used & all extrapolate to zero volume and the same temperature at negative 273oC

7. Plots of V vs. T(ºC) Charles’s Law Experiment results
Demonstrates a unique absolute zero at oC

8. Combined Gas Law P1V1 = P2V2 T1 T2
Avogadro’s Law - equal volumes of gas contain equal particles of gas
V = k n
At constant temperature and pressure the volume is directly proportional to the number of moles of gas.

9. Ideal Gas Law
Putting it all together, we can calculate that constant now. The universal gas constant R.
PV=R or PV=nRT
nT R = l *atm/mol*K
= l *kpa/mol*K

10. Density / Molar Mass with Ideal gas law
Molar mass, MM = ? What are the units?
So, moles = ?
Density, d = ? Use L for density since gas
So, mass = ?
Combine and get expression for moles n=
N= PV = dV Thus MM = dRT volume will be in Liters
RT MM P

11. Dalton’s Law of Partial Pressures
The gases in a mixture act independently and thus the forces (and pressures) are additive.
Ptotal = P1 + P2 + P3 + …

12. Kinetic Molecular Theory
Ideal Gas Behavior
Particles assumed to have zero volume
Particles in constant motion
Particles exert no forces on each other
KEave is directly proportional to T (K)
Check out Appendix 2 to see derivation of ideal gas law PV=nRT

13. Kinetic Theory also KEave = 3/2 RT Root square mean velocity
urms = sqrt(3RT/M)
Where M is mass of a mole in kg
So now we can calculate ave velocities of gases

14. Effusion of Gas into Evacuated Chamber
If more than one type of gas or more than one isotope, which gas effuses faster?
Lighter gas moves
Faster!!
KE = 1/2 mv2

15. Relative Molecular Speed Distribution of H2 and UF6

16. Diffusion Rates of NH3 and HCl Molecules Through Air
Relative diffusion/effusion rate pg. 213 textbook
rate1 = Sqrt(M2)
rate2 Sqrt(M1) lighter gas is faster

17. Ideal vs. Real Gases
All of the gases are real!!! They just behave “ideally” at certain temperatures and pressures.
Think of the KMT assumptions, what conditions would gases “fail” to act ideally.
Low temperatures (gases condense) & High pressures (force the gases together so they have to interact)

18. Plots of PV/nRT vs. P for Several Gases

19. Plot of PV/nRT vs. P for N2 Gas
This graph shows that at higher temperatures gases behave closer to ideal even at high pressures.
Recall that gases behave “ideally” at low pressures and high temperatures.

20. van der Waals Equation
van der Waals equation is entire gas law relationship with corrections for real volume and molecular attractions. pg.216 textbook with Table 5.3 for some common gases
(Pobs + correction) x ( V - nb) = nRT
This formula is also given on AP exam sheet.

21. Values of the van der Waals Constants for Common Gases
a is a measure of intermolecular attractions (it is the correction to the pressure to account for attractions for each other)
b is a measure of size of the molecule (it is the volume correction)