1. Gases
(“balloons”)

2. Essential Questions What are the properties of gases?
What does kinetic molecular theory mean to me?
How are temperature, pressure, and volume related?
How do gases affect our lives every day?

3. Properties of Gases Have mass Can be compressed
Compression: a measure of how much a volume of matter decreases under pressure.
Why can gases be compressed??
Expand to fill their containers
Diffuse
Exert pressure

4. Kinetic Molecular Theory
Kinetic = motion
Molecular = molecules
Kinetic Molecular Theory explains the motion of ideal gas particles

5. Kinetic Molecular Theory
Explains why gases act the way they do
Only works on an Ideal Gas
More to come on that…

6. Kinetic Molecular Theory
Assumption #1:
Gases are composed of a large number of tiny particles that are so far apart that individually, their volume is considered to be zero.
Volume is always the volume of the container
(“kinetictheory”)

7. Kinetic Molecular Theory
Assumption #2:
Collisions between the particles and the walls of the container cause pressure.
Small container = more collisions = more pressure
(“bikepump”)

8. Kinetic Molecular Theory
Assumption #3
Gas particles move in straight lines and have perfectly elastic collisions
Particles are not attracted or repelled by each other
Particles don’t lose any energy when they hit each other or the walls of the container.
("collision")

9. Kinetic Molecular Theory
Assumption #4:
The average kinetic energy of a number of gas particles is directly related to the temperature
If Temperature  then Energy 
More Later
("hot-thermometer")

10. Ideal Gas??
We use Kinetic Molecular Theory to describe the behavior of ideal gases only

11. Ideal Gas?
In real life:
Particles do not have perfectly elastic collisions
Particles can have some attraction/repulsion,
Because they are moving so fast, we can pretend there is no attraction/repulsion
Using real gases, there are too many variables to account for. Using ideal gases we can explain behavior to a close approximation.

12. What About Mass? Gases have mass
Very low density, so we don’t notice it
You can feel the mass of a gas when there are a LOT of gas particles in a small amount of space (ever pick up a helium tank or wonder why they are always on hand-trucks?)

13. Pressure Pressure = force per unit area Things that affect pressure
Amount of gas
Volume
Temperature
The Gas Laws will explain these relationships

14. Pressure Units Sometimes, you need to convert between them
1 atmosphere = 760 mm Hg
1 mm Hg = 1 torr
1 atm = 101,325 Pascals (Pa) = kPa

15. Pressure Calculations
What is 724 mm Hg in torr?
724 torr
In atm?
0.953 atm
In kPa?
96.5 KPa

16. Summary of Units of Pressure
Abbreviation
Unit Equivalent to 1 atm
Atmosphere
atm
1 atm
Millimeters of Hg
mm Hg
760 mm Hg
Torr
torr
760 torr
Pascal Pa
101,325 Pa
Kilopascal
kPa
kPa

17. Barometer Vacuum Measures air pressure
The pressure of the atmosphere at sea level will hold a column of mercury 760 mm Hg.
1 atm = 760 mm Hg
760 mm Hg
1 atm Pressure

18. Manometer h Gas Column of mercury to measure pressure of a gas
One end has gas, the other is open
h is how much lower the pressure of the gas is than atmosphere h
Gas

19. Manometer
h is how much higher the gas pressure is than the atmosphere. h
Gas

20. Reading a Manometer

21. Gas Laws
Occasionally, gas Laws describe the behavior of gases at Standard Temperature and Pressure (STP)
0° C
273K
1 atmosphere
1 atm = 760 torr = 760 mmHg

22. Temperature must ALWAYS be in KELVIN!
BE CAREFUL!!!!
Temperature must ALWAYS be in KELVIN!

23. Boyle’s Law Boyle’s Law – Pressure and Volume P1V1 = P2V2
One increases, the other decreases
Temperature must be constant
(“boyle_1”)

24. Try these…
A sample of gas starts out at a pressure 1.5 atm and a volume of 1.0 liter. If the pressure is increased to 2.0 atm, what is the volume of the gas?
0.75 atm
A gas occupies 16 liters and has a pressure of 875 torr. If the volume is decreased to 5.0 liters, what is the new pressure of the gas?
2800 torr

25. Charles’ Law Charles’ Law – Temperature and Volume V1 = V2 T1 T2
One increases, the other increases
Temperature must be in Kelvin, Pressure must remain constant
(“charlesballoon”)

26. Try these…
A 2.00 liter sample of gas at 298 K is heated to 320 K. Pressure is constant at 1.00 atm. What is the new volume of the gas?
2.15L
Nicholas blows a soap bubble containing air at 42°C and has a volume of 23cm3 at 1 atm. The bubble encounters a pocket of cold air at 18°C. What is the new volume of the soap bubble?
21cm3

27. Gay-Lussac’s Law Gay-Lussac’s Law – Pressure and Temperature P1 = P2
T1 T2
One increases, the other increases
Volume must remain constant

28. Try these…
If a 3.00L container contains a gas at 1.00 atm of pressure at 298 K, and the temperature is increased to 460 K, what is the pressure the gas exerts on the container?
1.54 atm
If a 2L container starts out having a pressure of 870. torr at a temperature of 350. K, what is the temperature if the pressure decreases to 600. torr?
241 K

29. COMBINE them all together…
Combined Gas Law
P1V1 = P2V2
T1 T2
Most useful, because it brings all the other gas laws we’ve talked about together

30. Try these…
If I have a gas at a pressure of 12.0 atm, a volume of 23.0 liters, and a temperature of 200. K, and I raise the pressure to 14.0 atm and increase the temperature to 300. K, what is the new volume of the gas?
29.6 L
A gas takes up 17.0 liters, has a pressure of 2.30 atm, and a temperature of 299 K. If I raise the temperature to 300. K and lower the pressure to 1.50 atm, what is the new volume of the gas?
26.2 L

31. Let’s get moles involved… Avogadro’s Law
At a constant temperature and pressure, volume relates directly to the number of moles
More gas = more volume
V1 = V2
n n2

32. Let’s put more stuff together…
Ideal Gas Law
If you know 3 pieces of information about your gas you can calculate the fourth
R is the ideal gas constant
What is R?
R = (L·atm)/(mol·K)
With different units:
R = 8.31 (L·kPa)/(mol·K)

33. Try these…
If I have a 6.7mol of a gas at 350 K and 12 atm of pressure, what is the volume of the gas?
16L
How many moles of gas will occupy 14 liters at 298 K and 2.0 atm of pressure?
1.1 mol
At what pressure will 6.02 moles of gas occupy 3.14 liters at 98.0°C?
58.4 atm

34. Dalton’s Law
The total pressure in a container is the sum of the pressure each gas would exert if it were alone in the container.
The total pressure is the sum of the partial pressures.
PTotal = P1 + P2 + P3 + P4 + P5 ...
For each P = nRT/V

35. Dalton's Law PTotal = n1RT + n2RT + n3RT +... V V V
In the same container R, T and V are the same.
PTotal = (n1+ n2 + n3+...) RT V
PTotal = (nTotal) RT V

36. Dalton’s Law of Partial Pressure

37. Dalton’s Law Examples
Air contains oxygen, nitrogen, carbon dioxide, and trace amounts of other gases. What is the partial pressure of oxygen at kPa of total pressure if the partial pressures of nitrogen, carbon dioxide, and other gases are kPa, kPa, and 0.94 kPa, respectively?
21.22kPa

38. The mole fraction Ratio of moles of the substance to the total moles.
Symbol is Greek letter chi c
c1 = n1 = P nTotal PTotal

39. Examples
The partial pressure of nitrogen in air is 592 torr. Air pressure is 752 torr, what is the mole fraction of nitrogen?
0.787
What is the partial pressure of nitrogen if the container holding the air is compressed to 5.25 atm?
4.13 atm

40. Review Properties of gases Kinetic Molecular Theory Boyle’s Law
Charles’s Law
Gay-Lussac’s Law
Combined Gas Law
Ideal Gas Law
Dalton’s Law of Partial Pressures
Mole Fraction

41. Stoichiometry Our old friend…
When you calculate volume in a stoichiometry problem using 22.4 L/mol, we are getting the volume at STP
We will do all our stoichiometry problems at STP
You can use gas laws to find the volume of product at different temperatures/pressures

42. Examples
Sulfur trioxide is produced in enormous quantities each year for use in the synthesis of sulfuric acid
S(s) + O2(g)  SO2(g)
2SO2(g) + O2(g)  2SO3(g)
What volume of O2(g) at 350°C and a pressure of 5.25atm is needed to completely convert 5.00g or sulfur to sulfur trioxide?

43. 4NH3(g) + 5O2(g) ® 4NO(g) +6H2O(g)
Examples
Consider the following reaction:
4NH3(g) + 5O2(g) ® 4NO(g) +6H2O(g)
What volume of NO at STP will be produced from 23.7L of NH3?
23.7L
What volume of O2 measured at STP will be consumed when 10.0L NH3 is reacted?
12.5L

44. Examples Mercury can be produced by the following reaction:
2HgO ® 2Hg +O2
What volume of oxygen gas can be produced from 4.10 g of mercury (II) oxide at STP?
0.212L
At 400.ºC and 740 torr?
0.537L