1. Student Learning Objectives
Heat & Temperature
Chapter 5
Student Learning Objectives
Relate kinetic energy to temperature
Compare temperature scales
Analyze systems to determine methods
& effects of heat transfer

2. What does temperature measure?
Temperature is a measure of the average kinetic energy of the atoms and molecules in a substance.
We perceive the KE of atoms and molecules as being hot or cold.
Harvards Golf Ball Atmosphere
There is No Such Thing as Cold.

3. Materials at different temperatures reach thermal equilibrium when placed in contact.
Examples
Thermometer + Person
Person + Metal Chair
Most materials expand when the temperature is increased, thermal expansion
Examples
Metal lids
Bridge Joints
Bimetallic strips
Hot Air Balloons

4. Bimetallic Strip and Thermal Expansion
Brass expands more than iron.
The degree of deflection is proportional to the temperature.
A/C thermostat and dial-type thermometers are based on bimetal coils.
Invisible Motion
Section 5.1

5. Liquid-in-glass Thermometer
Thermometers are calibrated to two reference points (ice point & steam point.)
Ice point – the temperature of a mixture of pure ice and water at normal atmospheric pressure
Steam point – the temperature at which pure water boils at normal atmospheric pressure
Usually contains either mercury or red (colored) alcohol
Section 5.1

6. Temperature Scales Celsius, Kelvin, Fahrenheit
Section 5.1

7. Temperature Scales Celsius, Kelvin, Fahrenheit
Absolute Zero
Ice Point
Steam
Point
Diff.
(Boil – Ice)
Fahrenheit
- 460o
32o
212o
180
Celsius
-273o 0o
100o
100
Kelvin
273o
373o
Section 5.1

8. Temperature Kelvin is based the average KE of atoms in a gas.
Fahrenheit is based on boiling and freezing points of water.
 freezing at sea level
212o  boiling at sea level
Celsius is based on boiling and freezing points of water.
0 o  freezing at sea level
100o  boiling at sea level
Kelvin is based the average KE of atoms in a gas.

9. F = (9/5)C + 32 C = (5/9)(F – 32) K = C + 273
0 Kelvin = ─273o C = ─460o F
Object
Kelvin
Fahrenheit
Human Body K
98.6 ºF
Sun
5800 K
9,980 ºF
Blue Star
35000 K
62,540 ºF

10. Practice
These Practice Problems are presented in class

11. What is heat?
Heat is energy that moves from one object to another if there is a temperature difference.
The larger the temperature difference, the faster heat energy flows.
These Practice Problems are presented in class
Hot → Cold

12. Heat Unit SI - Calorie
Since heat is energy, it has a unit of joules. (J)
A more common unit to measure heat is the calorie.
Calorie - the amount of heat necessary to raise one gram of pure water by one Celsius degree at normal atmospheric pressure
1 cal = J (or about 4.2 J)
Kilocalorie – heat necessary to raise 1kg water by 1oC
1 food Calorie = 1000 calories (1 kcal)
1 food Calorie = 4186 J (or about 4.2 kJ)
Section 5.2

13. Expansion/Contraction with Changes in Temperature
In general, most matter, solids, liquids, and gases will expand with an increase in temperature (and contract with a decrease in temperature.)
Water is an exception to this rule – (ice floats!)
Section 5.2

14. Thermal-Expansion Joints in a Bridge
These joints allow for the contraction and expansion of the steel girders during the winter and summer seasons.
Section 5.2

15. Behavior of Water  Strange!
The volume of a quantity of water decreases with decreasing temperature but only down to 4oC. Below this temperature, the volume increases slightly.
With a minimum volume at 4oC, the density of water is maximum at this temperature and decreases at lower temperatures.
Most dense point
Section 5.2

16. Behavior of Water: Structure of Ice Solid water takes up more volume
(Ebbing, Darrell D., General Chemistry, Sixth Edition. Copyright 1999 by Houghton Mifflin Company)
An illustration of the open hexagonal (six-sided) molecular structure of ice.
This hexagonal pattern is evident in snowflakes.
Section 5.2

17. Lakes freeze from the top down – Yellowstone Lake
Photo Source: Copyright © Bobby H. Bammel. All rights reserved.
Section 5.2

18. Specific Heat
If equal quantities of heat are added to equal masses of two metals (iron and aluminum, for example) – would the temperature of each rise the same number of degrees? -- NO!
Different substances have different properties.
Specific Heat – the amount of heat necessary to raise the temperature of one kilogram of the substance 1oC
Section 5.3

19. The amount of heat it takes to increase the temperature of a material by 1o C is the specific heat capacity of the material.
c=specific heat capacity, m=mass, T=temperature (K or C)
A substance with a high specific heat capacity will resist changes in temperature.
See page 117 for different specific heat capacities
Q = cmDT

20. Practice
These Practice Problems are presented in class

21. More Practice
These Practice Problems are presented in class

22. What is the greenhouse effect? What is global warming?
The greenhouse effect traps heat near the surface of a planet.
Greenhouse gasses in the atmosphere do not create heat. Greenhouse gasses slow heat loss to space.
These Practice Problems are presented in class

23. What happens to temperature & energy during a phase change?
A substance that has reached the temperature required for a phase change maintains its temperature during the phase change.
All energy lost or gained is used to change the phase of the substance.
Evaporation (Liquid to gas)
Sublimation (Solid to gas)
Condensation (Gas to liquid)

24. The amount of heat energy per kilogram that must be added or removed for a substance to change phase is called latent heat (L).
IceWaterSteam
Q = mL
T (°C)
100
Joules

25. Graph of Temperature vs. Heat for Water
Latent heat of fusion – heat necessary to go from A to B
Latent heat of vaporization – heat necessary to go from C to D
Section 5.3

26. Graph of Temperature vs. Heat for Water
A=100% solid at 0oC B=100% liquid at 0oC C=100% liquid at 100oC D=100% gas at 100oC
Section 5.3

27. Graph of Temperature vs. Heat for 1 kg of Pure Water
0.5kcal
kg.Co
80 kcal
1.0 kcal/kg.Co
540 kcal
0.5 kcal/kg.Co
Section 5.3

28. Other phase changes
Sublimation – when a substance changes directly from solid to gas (dry ice  CO2 gas, mothballs, solid air fresheners)
Deposition – when a substance changes directly from gas to solid (ice crystals that form on house windows in the winter)
Section 5.3

29. Practice
These Practice Problems are presented in class

30. Heat Transfer Occurs by Conduction, Convection, and Radiation
Section 5.4

31. What are the three methods of heat transfer?
Conduction is the transfer of heat energy from one place to another by direct collisions.
Solids tend to conduct heat better than liquids or gases. Why?
Insulators slow or impede the rate of heat flow.
Styrofoam
Fiberglass
Freely moving electrons = High thermal conductivity

32. Convection is the transfer of heat energy from one place to another by the bulk motion of groups of molecules in a fluid. (sinking/floating)
Radiation is the transfer of heat energy from one place to another by electromagnetic waves (light).

33. Practice
These Practice Problems are presented in class

34. How are temperature and pressure related in a gas?
In a gas, pressure is determined by temperature, volume, and number of particles.
Boyle's Law: P1V1 = P2V2
Charles, Law: P1/T1 = P2/T2
PV = nkT

35. Practice
These Practice Problems are presented in class

36. What are the 3 laws of thermodynamics?
1st Law: The amount of heat energy transferred is equal to the change in internal energy plus work.
Heat Energy  DIE + Work
2nd Law: Heat cannot flow spontaneously from a cold substance to a hot substance. Entropy (disorder) cannot spontaneously decrease.
What is Entropy?

37. Laws of Thermodynamics Song
3rd Law: The entropy of a perfect crystal is zero when the temperature of the crystal is equal to absolute zero. KE → 0
Hero's Engine
Laws of Thermodynamics Song
Practice
These Practice Problems are presented in class