1. Temperature and Ideal Gas
Everything is made of atoms
In gases the molecules don’t interact with each other. Simple
How does the atomic (molecular) nature of a gas explain its properties?
Air in your tires?
How hot is hot?
How cold is cold?

2. Temperature
The quantity indicating how warm or cold an object is relative to some standard is TEMPERATURE (T).
T does not depend on quantity of a substance. A cup and a thimble of boiling water both have same T.
When two objects have the same temperature, they are in thermal equilibrium.
Heat is the flow of energy due to a temperature difference. Heat always flows from objects at high temperature to objects at low temperature.

3. There is no heat flow between objects in thermal equilibrium
The Zeroth Law of Thermodynamics:
If two objects are each in thermal equilibrium with a third object, then the two objects are in thermal equilibrium with each other.
There is no heat flow between objects in thermal equilibrium

4. Temperature Scales (*) Values given at 1 atmosphere of pressure.
Fahrenheit scale
Water boils*
212 F
Water freezes*
32 F
Absolute zero
 F
Could incorporate personal response system questions from the College Physics by G/R/R 2E ARIS site ( Instructor Resources: CPS by eInstruction, Chapter 13, Questions 1, 2, and 3.
(*) Values given at 1 atmosphere of pressure.

5. Temperature Scales (*) Values given at 1 atmosphere of pressure.
Fahrenheit scale
Celsius scale
Water boils*
212 F
100 C
Water freezes*
32 F
0 C
Absolute zero
 F
273.15C
Could incorporate personal response system questions from the College Physics by G/R/R 2E ARIS site ( Instructor Resources: CPS by eInstruction, Chapter 13, Questions 1, 2, and 3.
(*) Values given at 1 atmosphere of pressure.

6. Temperature Scales (*) Values given at 1 atmosphere of pressure.
Absolute or Kelvin scale
Fahrenheit scale
Celsius scale
Water boils* K
212 F
100 C
Water freezes* K
32 F
0 C
Absolute zero
0 K
 F
273.15C
Could incorporate personal response system questions from the College Physics by G/R/R 2E ARIS site ( Instructor Resources: CPS by eInstruction, Chapter 13, Questions 1, 2, and 3.
(*) Values given at 1 atmosphere of pressure.

7. The temperature scales are related by:
Fahrenheit/Celsius
Absolute/Celsius

8. Example (text problem 13.3): (a) At what temperature (if any) does the numerical value of Celsius degrees equal the numerical value of Fahrenheit degrees?
(b) At what temperature (if any) does the numerical value of kelvins equal the numerical value of Fahrenheit degrees?

9. Question Which is smaller, a change of 1oF or 1oC? A) 1oF B) 1oC
C) they are the same

10. Molecular Picture of a Gas
Atoms and molecules are
the basic units of matter
We want to explain thermal
Properties in terms of atoms
and molecules.
How many atoms?

11. Molecular Picture of a Gas
We can specify the amount of a substance by giving its mass or by the number of molecules (or atoms) it has.
If we know the mass of a molecule we can go from one description to the other
A golf ball weighs 1.6 ounces.
I have a 20 lb box of golf balls
I have a box of 200 golf balls
Totally equivalent

12. Molecular Picture of a Gas
If a sample contains a single substance (element or compound) the number of particles in the sample is
N = M/m.
N equals the total mass of the sample (M) divided by the mass (m) of the atom (or molecule)
The number density of particles is N/V where N is the total number of particles contained in a volume V.

13. It is convenient to have a standard number to facilitate this going back and forth from the two descriptions.
Since we deal with human size numbers (gms) this will involve a very large number of atoms
One mole of a substance contains the same number of particles as there are atoms in 12 grams of 12C. The number of atoms in 12 grams of 12C is Avogadro’s number.

14. Why 12 gm of Carbon? u = 1g/(6x1023) =1.66x10-24g =1.66x10-27kg
A carbon-12 atom by definition has a mass of exactly 12 atomic mass units (12 u or 12 amu).
12g = 12u NA
u = 1g/(6x1023) =1.66x10-24g =1.66x10-27kg
Problem
This is the conversion factor between the atomic mass unit and kg (1 u = 1.661027 kg). NA and the mole are defined so that a 1 gram sample of a substance with an atomic mass of 1 u contains exactly NA particles.
A mole of O2 has mass 32 gm., of water m=18 gm

15. Example (text problem 13.37): Air at room temperature and atmospheric pressure has a mass density of 1.2 kg/m3. The average molecular mass of air is 29.0 u. How many air molecules are there in 1.0 cm3 of air?
The total mass of air in the given volume is:

16. Example continued:

17. Question Which contains more atoms, 5 mol. of helium
(mass He =4amu) or 1 mol of neon (m Ne =20amu)
A) Helium
B) Neon
C) both have same number of atoms

18. Question Which contains more atoms, 1 mol of helium
or 1 mol of Steam (water)
A) Helium
B) water
C) both have same number of atoms

19. Decrease the volume Increase the pressure
Constant T: P ~1/V

20. Increase the number of molecules Increase the pressure
Constant V,T: P ~ N

21. We also know that, as you drive, tire pressure increases with T
Constant V,N: P ~ T

22. Absolute Temperature and the Ideal Gas Law
Could incorporate personal response system questions from the College Physics by G/R/R 2E ARIS site ( Instructor Resources: CPS by eInstruction, Chapter 13, Questions 8, 9, 10, 11, 12, 13, 14, and 15.
Constant P: V ~T

23. Absolute Temperature and the Ideal Gas Law
Experiments done on dilute gases (a gas where interactions between molecules can be ignored) show that:
Could incorporate personal response system questions from the College Physics by G/R/R 2E ARIS site ( Instructor Resources: CPS by eInstruction, Chapter 13, Questions 8, 9, 10, 11, 12, 13, 14, and 15.
For constant pressure
Charles’ Law
For constant volume
Gay-Lussac’s Law

24. For constant temperature
Boyle’s Law
For constant pressure and temperature
Avogadro’s Law

25. What Temperature do we use?
Could incorporate personal response system questions from the College Physics by G/R/R 2E ARIS site ( Instructor Resources: CPS by eInstruction, Chapter 13, Questions 8, 9, 10, 11, 12, 13, 14, and 15.
There is a lowest possible T
V→0

26. Absolute Temperature
There is a coldest possible temperature Absolute zero.
All objects will transfer heat to an object at absolute 0.
Experiment show (e.g. V→0 ) that the coldest possible T is oC.
Kelvin scale measures T from Absolute 0 in units of 1oC
TK=Tc+273o

27. The ideal gas law can also be written as (macroscopic form):
Putting all of these statements together gives the ideal gas law (microscopic form):
k = 1.381023 J/K is Boltzmann’s constant
The ideal gas law can also be written as (macroscopic form):
R = NAk = 8.31 J/K/mole is the universal gas constant and n is the number of moles.

28. Here, Vf = Vi/9, Pf = 20.0Pi, and Ti = 30 C = 303 K.
Example (text problem 13.41): A cylinder in a car engine takes Vi = 4.50102 m3 of air into the chamber at 30 C and at atmospheric pressure. The piston then compresses the air to one-ninth of the original volume and to 20.0 times the original pressure. What is the new temperature of the air?
Here, Vf = Vi/9, Pf = 20.0Pi, and Ti = 30 C = 303 K.
The ideal gas law holds for each set of parameters (before compression and after compression).

29. The final temperature is
Example continued:
Take the ratio:
The final temperature is
The final temperature is 673 K = 400 C.

30. The ideal gas law can also be written as (macroscopic form):
Putting all of these statements together gives the ideal gas law (microscopic form):
k = 1.381023 J/K is Boltzmann’s constant
The ideal gas law can also be written as (macroscopic form):
R = NAk = 8.31 J/K/mole is the universal gas constant and n is the number of moles.

31. Question When the temperature of a quantity of gas is increased
A) the pressure must increase.
B) the volume must increase.
C) the pressure and/or the volume must increase.
D) none of the above

32. Question
A pot of water on the stove is heated from 25oC to 100oC. By what factor does the
temperature in Kelvin change?
A) T2 = 4T1
B) T2 = 1.25T1
C) T2 = 0.80T1
D) T2 = 0.20T1

33. Question
Inside your air-conditioned apartment, you blow up a balloon as large as possible and then take it outside on a hot summer day. The balloon is most likely to then
A) shrink.
B) remain the same size.
C) expand and pop.

34. Question
The Kelvin temperature of an ideal gas is doubled and the volume is halved. How is the pressure affected?
A) increases by a factor of 2
B) increases by a factor of 4
C) stays the same
D) decreases by a factor of 2
E) decreases by a factor of 4

35. Kinetic Theory of the Ideal Gas
An ideal gas is a dilute gas where the particles act as point particles with no interactions except for elastic collisions.
Point particles can have only KE, no internal PE
Add heat (energy) to gas, energy increases
KE increases.
But if we add heat, temperature also increases.
T depends on KE
Could incorporate personal response system questions from the College Physics by G/R/R 2E ARIS site ( Instructor Resources: CPS by eInstruction, Chapter 13, Questions 16 and 18.

36. Kinetic Theory of Ideal Gas
T~ KEav/molecule
if T =absolute 0, molecules don’t move.
T T T
More total energy, but same T, same average KE

37. Temperature is related to average KE
This is true even for liquids and solids

38. Pressure is caused by collisions
Gas particles have random motions. Each time a particle collides with the walls of its container there is a force exerted on the wall. The force per unit area on the wall is equal to the pressure in the gas.

39. The pressure will depend on:
The number of gas particles ~N
Frequency of collisions with the walls ~ v
Amount of momentum transferred during each collision ~ mv
P~ Nmv2 ~N KEmol

40. The pressure in the gas is
Where <Ktr> is the average translational kinetic energy of the gas particles; it depends on the temperature of the gas.

41. Typical air molecule is moving more than
1,000 Miles/hr. Some move faster some slower

42. The average kinetic energy also depends on the rms speed of the gas
Problem
where the rms speed is

43. What is rms? root mean square
v2 rms is the average of the square of the velocities. It is not the square of the average
Average
of squares
rms

44. What is rms? root mean square
vrms is the average of the square of the velocities. It is not the square of the average

45. rms Example
v1 = v2 = vav = 6
v12 = v22 = 64

46. The distribution of speeds in a gas is given by the Maxwell-Boltzmann Distribution.

47. Example (text problem 13.60): What is the temperature of an ideal gas whose molecules have an average translational kinetic energy of 3.201020 J?

48. On the Kelvin scale T = 25 C = 298 K. Element Mass (kg)
Example (text problem 13.70): What are the rms speeds of helium atoms, and nitrogen, hydrogen, and oxygen molecules at 25 C?
On the Kelvin scale T = 25 C = 298 K.
Element
Mass (kg)
rms speed (m/s) He
6.641027
1360 H2
3.321027
1930 N2
4.641026
515 O2
5.321026
482
In atomic mass units, the masses used are 4u for He, 2u for H2, 14u for N2, and 16u for O2.

49. Question
At a given temperature, a hydrogen molecule has a speed of 800 m/s. At the same
temperature, an oxygen molecule has a speed of
A) m/s.
B) m/s.
C) m/s.
D) 100 m/s.

51. Question When will a real gas behave most like an ideal gas?
A) at high temperatures and high pressures
B) at low temperatures and high pressures
C) at low temperatures and low pressures
D) at high temperatures and low pressures

52. Question
The rms speed of a box of molecules which are moving at non uniform speeds is
greater than the average speed.
A) always
B) sometimes
C) never

53. Thermal expansion
Most objects including liquids and solids expand when their Temperature increases

54. An object’s length after its temperature has changed is
 is the coefficient of linear expansion
where T = TT0 and L0 is the length of the object at a temperature T0.

55. Example (text problem 13.84): An iron bridge girder
(Y = 2.01011 N/m2) is constrained between two rock faces whose spacing doesn’t change. At 20.0 C the girder is relaxed. How large a stress develops in the iron if the sun heats the girder to 40.0 C?
 = 12106 K1 (from Table 13.2)
Using Hooke’s Law:

56. How does the area of an object change when its temperature changes?L0
L0+L
The blue square has an area of L02.
With a temperature change T each side of the square will have a length change of L = TL0.

57. The fractional change in area is:

58. The fractional change in volume due to a temperature change is:
For solids  = 3

59. Question
A metal plate with a hole cut in it is heated. As the plate expands,
A) the hole expands.
B) the hole shrinks.
C) the hole stays the same size.

60. Question
You can loosen the metal lid on a glass jar by running it under hot water. Given that the lid and the jar have roughly the same diameter, compare the expansion of the diameter of the lid to that of the jar. (asteel = 12 x 10-6 K-1, aglass = 3.25 x 10-6 K-1)
A) DLlid = 3.7 DLjar
B) DLlid = 0.27DLjar
C) DLlid = 7.4 DLjar
D) DLlid = 1.9 DLjar