1. Chapter 23: Change of Phase Chapter 24: Thermodynamics
Chapters 23 & 24
Chapter 23: Change of Phase
Chapter 24: Thermodynamics

2. 3 Common Phases of Matter
A fourth phase, plasma--ionized gas (not shown), is the most common phase of matter in the universe. 

3. 2 Changes of Phase From solid → liquid From liquid → gas
Depends on temperature & pressure.
Usually involves a transfer of energy.

4. Change of Phase- Energy

5. Evaporation Liquid to Gas Takes place at the surface of a liquid.
Molecules at the surface are being bumped from below & given enough energy to break free.

6. Evaporation is “COOL”
Because energy was lost when the molecule broke free, the avg. KE left in the container is lowered.
EVAPORATION = COOLING!!!
Shower, dog’s tongues, swimming, etc…

7. Condensation is “HOT” Gas to Liquid. CONDENSATION = WARMING!
Fast gas molecules collide with slow ones and loose energy. They don’t have enough energy to stay as a gas. (Not fast enough.)

8. De-Foggers. How do they work?
Prevent condensation.
Clear, thin film.
Takes the water formed & immediately spreads it out evenly.
You can’t see the water!

9. Evaporation & Condensation
Greater evaporation = COOLING
Equal = No net change
Greater condensation = WARMING

10. Condensation in the Atmosphere
At each temp, there is a limit to the amount of water vapor in the air.
Limit reached = saturation
Called “humidity”

11. Saturation
100% humidity
More water vapor needed to saturate high temp. air than low temp. air.
Condensation must be happening in the air. (water sticks to itself)

12. Boiling
Liquid to gas
Question: Is boiling a cooling process or a warming process????
Answer: It is a COOLING process!!! 
As faster molecules with a larger KE leave…
the avg. KE left lowers = cooling!

13. Pressure Cooker Question: How does it cook so darn fast???????
Answer: Increases the boiling temp so food cooks at a higher temperature!

14. Boiling occurs at different temps…
At higher altitudes, pressure is less, so water needs less KE to fight against the force of the air on their way off the surface of the liquid.
Did you know…At the ocean floor (approx. 2 miles down) water won’t boil until it is ~700 ºF!!

15. Freezing When energy is withdrawn from a liquid.
It slows down until it’s a solid.

16. Change of Phase Equation
Q = mL
Heat energy = (mass)(heat of fusion or vaporization) “lost or gained” “latent heat”
J = (kg)(J/kg)

17. Thermodynamics
The study of heat & it’s ability to transform into mechanical energy.
Power plants, cars, etc…
There are 3 Laws.

18. Thermodynamics
The study of heat & it’s ability to transform into mechanical energy.
Power plants, cars, etc…
There are 3 Laws.

19. 1st Law of Thermodynamics
When heat is added to a system, it transforms to an EQUAL amount of some other form of energy.
…because energy is ALWAYS conserved

20. 1st Law Example…
A battery powered light is switched on and heat is produced.
That heat energy actually already existed inside the system as chemical energy inside the battery.
So no energy is either gained or lost as a result of switching on the light!

21. 1st Law Equation
Q = ΔE + W
Heat added = change of internal E + external work
J = J + J

22. 2nd Law of Thermodynamics
Heat will NEVER, by itself, flow from cold to hot.
It will flow from hot to cold until equilibrium has been reached.

23. IE = Thot – Tcold Thot 2nd Law Equation
Ideal Efficiency
IE = Thot – Tcold
Thot
No SI unit label for ideal efficiency.
Temperature is measured in K. (Remember your conversion equations for the test!)

24. It’s impossible…
Question: To produce usable energy with ZERO impact to the environment… WHY?
Answer: Because heat (waste) will always be given off!
(It will warm air, rivers, etc…)

25. 3rd Law of Thermodynamics
You can’t reach absolute zero.

26. The End. Any questions?