1. Temperature and Heat

2. What are temperature and heat?
Are they the same? What causes heat?

3. What Is Temperature? How do we measure temperature?
What are we actually measuring?

4. Temperature and Its Measurement
How do we measure temperature?
Thermometer: Device with a physical property that changes with temperature and can be easily measured quantitatively.
If two objects are in contact with one another long enough, the two objects have the same temperature (thermal equilibrium).
Two or more objects in thermal equilibrium have the same temperature.
Zeroth law of thermodynamics.

5. Temperature Scales
The first widely used temperature scale was devised by Gabriel Fahrenheit.
Water freezing point: 32F
Water boiling point: 212F
Another widely used scale was devised by Anders Celsius.
Water freezing point: 0C.
Water boiling point: 100C

6. Temperature Scales Conversion between two scales:
E1. An object has a temperature of 45C. What is its temperature in degree Fahrenheit?
E2. The temperature of a winter day is 14F. What is the temperature in degree Celsius?

7. Zero Temperature
The zero point on the Fahrenheit scale was based on the temperature of a mixture of salt and ice in a saturated salt solution.
The zero point on the Celsius scale is the freezing point of water.
Both scales go below zero.
Is there an absolute zero?

8. What is absolute zero?
If the volume of a gas is kept constant while the temperature is different, the pressure will be different.

9. The Third Temperature Scale
Absolute Temperature Scale (Kelvin Scale)
Example
Water freezing point: 0C =273.2 K.
Water boiling point: 100C = K

10. Heat and Specific Heat Capacity
Steel has a lower specific heat capacity than water.

11. Specific Heat Capacity
specific heat capacity (c): the quantity of heat needed to change a unit mass (1 g) of the material by a unit amount in temperature (1 C).
It is a property of the material, determined by experiment.
The specific heat capacity of water is 1 cal/gC
Table 10.1 Specific capacity of some common substances
Substance Specific Heat Capacity (in Cal/g/C)
Water 1.0
Ice
Steam
Ethyl alcohol 0.58
Glass
Aluminum

12. When a material’s temperature is changed, we can calculate how much heat absorbed/released by the material:
Q = mcT
where Q = quantity of heat
m = mass
c = specific heat capacity
T = change in temperature
Example: E6
How much heat is required to raise the temperature of 70g of water from 20C to 80C

13. Heat and Temperature Heat:
Heat is the energy that flows from one object to another when there is a difference in temperature between the objects. Heat is the average kinetic energy of atoms or molecules making up the system.
Temperature:
Temperature is an indication
of whether or not and in which
direction, the heat will flow
(Temperature is an indication
of the average of kinetic energy
of atoms or molecules).

14. Phase Change and Latent Heat
When an object goes through a change of phase or state, heat is added or removed without changing the temperature. Instead, the state of matter changes: solid to liquid, for example.
The amount of heat needed per unit mass to produce a phase change is called the latent heat (L)
The latent heat of fusion of water is 80 cal/g (Lf = 80 cal/g is 80 cal/g): it takes 80 calorie of heat the melt 1 g of ice at 0C to become water at 0C.
The latent heat of vaporization of water is 540 cal/g (Lv = 540 cal/g): it takes 540 calories of heat to turn one gram of water at 100 C into steam at 100 C.

15. Example Box 10.1
If the specific heat capacity of ice is 0.5 cal/gC°, how much heat would have to be added to 200 g of ice, initially at a temperature of -10°C, to (a) raise the ice to the melting point? (b) complete melt the ice?

16. Heat and Mechanic Energy
Benjamin Thompson ( ) noticed that cannon barrels and drill bits became hot during drilling.
Joule performed a series of experiments showing that mechanical work could raise the temperature of a system.
1 cal = 4.19 J
First law of Thermodynamics.
Energy Conservation - In an isolated system, the total amount of energy, including heat, is conserved.

17. Applying the First Law of Thermodynamics
Example (Box 10.2) :A hot plate is used to transfer 400 cal of heat to a beaker containing ice and water. 500 J of work are also done on the contents of the beaker by stirring.
a) What is the increase in
internal energy of the
ice-water mixture?
b) How much ice melts in
this process?

18. Counting Food Calories
Calories in Physics and in food:
In Physics: 1 calories is the amount of energy needed to raise the temperature of 1 g of water 1 C.
In food: 1 Calories is the amount of energy needed to raise the temperature of 1 kg water 1 C
1 Cal =1,000 cal
Normal body maintenance uses up about 15 calories per day for each pound of body weight.
You must consume about 3500 calories to gain a pound of weight.
To burn off 500 calories you would have to run 5 miles, bike 15 miles, or swim for an hour.

19. The Flow of Heat Three basic processes for heat flow: Conduction
Convection
Radiation

20. Conduction: heat flow when in contact
The rate of heat flow depends on:
a) the temperature difference between the objects.
b) the thermal conductivity of the materials, a measure of how well the materials conduct heat.
A metal block at room temperature will feel colder than a wood block of the exact same temperature. Why?

21. Convection: heat is transferred by the motion of a fluid containing thermal energy.
Radiation, heat energy is transferred by electromagnetic waves.
can take place across a vacuum.

22. What heat-flow processes are involved in the greenhouse effect?

23. Lab T4. Measurement of the specific heat
Example: Suppose that you have 100 g of water at
the temperature of 20 C, and you have 50 g of a
metal at the temperature of 100 C. If you put the
metal into the water, and the final temperature is
30 C when the mix of water and aluminum reaches
a thermal equilibrium, what is the specific capacity
of the metal?