1. Temperature, Heat and Energy
It’s Hot, Hot, Hot!

2. Remember Conservation of Energy?
We have been ignoring the non-mechanical or “lost” energy.

3. Energy, Work and Heat
Energy is the property that enables a body to do work.
Work can transfer mechanical energy into or out of a substance.
Heat is the transfer of thermal energy into or out of a substance.

4. Mechanical Energy Potential Energy – results from changing position.
Kinetic Energy – results from motion.

5. Thermal Energy – results from the motion of atoms (thermal motion).
Internal Energy
Internal energy is the total energy of all of the molecules in a substance. (This is not mechanical energy; you can’t see this.)
Thermal Energy – results from the motion of atoms (thermal motion).

6. Internal Energy Suppose you put a block of metal into hot water.
What happens to the energy of the block?
Does the kinetic energy of the block change?
NO!
Does the potential energy change?
Does the mechanical energy change?
Does the thermal energy change?
Yes!
Does the internal energy change?

7. First Law of Thermodynamics
(Conservation of Energy Applied to Heat)
Heat added to a system transforms to an equal amount of another form of energy.
Heat added =
Increase in internal energy +
External work done by the system

8. First Law of Thermodynamics
Examples of
First Law of Thermodynamics
Heat added =
Increase in internal energy +
External work done by the system
Heat added to table by rubbing hand on the surface =
Table gets warmer +
Table does no work
Heat added to balloon by placing it in a hot car =
Balloon gets warmer +
Balloon expands and does work by pushing air in the car aside

9. Conservation of Energy Applied to Heat
Second Law of Thermodynamics
When energy is transferred some of the energy can not be used to do work.
Or …Natural systems tend toward a state of greater disorder.

10. Second Law of Thermodynamics
Example of
Second Law of Thermodynamics
Waterfalls are used to generate electricity.
The electricity that it generates is not enough to pump all of the water back up to the top of the waterfall.
(Can’t have perpetual motion because we always lose usable energy.)

11. Entropy How’s this for a little chaos?
Entropy is the measure of the amount of disorder in a system.
Which picture shows greater entropy?

12. Temperature or Heat
Temperature is the result of the average kinetic energy of the atoms and molecules in motion.
Think of the block in the water.
The block is not moving, KE = 0 J
The molecules in the block are moving (vibrating), KE >0. This is thermal energy.
Thermal Energy is the total KE of the atoms.

13. Heat
Energy that flows from one object to another. It is the transfer of energy.
It flows from higher temperature to lower temperature.
It is measured in joules in the SI system.
It is thermal energy in transit.

14. Heat Transfer Transfer of heat depends on temperature difference.
Heat stops flowing when the temperatures are equal – Thermal equilibrium is reached.
heat lost by one object = heat gained by the other

15. Heat Equation Q – heat transferred to an object m – mass
c – specific heat
DT – temperature change

16. c = Specific Heat
The amount of energy that needs to be added to raise the temperature of a unit of mass (1kg) one degree.
This means an object with a large specific heat will require a larger amount of heat to change the temperature.
Examples : Water c = 4186 J/kgoC
Copper c = 386 J/kgoC