1. Temperature and Heat Temperature and Heat

2. Temperature Scales Water boils Water freezes 212 32 Farenheit 100 0 Celcius 273.15 373.15 Kelvin NOTE: K=0 is “absolute zero”, meaning (almost) zero KE/molecule 14

3. Temp Scales Question l Two cups of coffee are heated to 100 degrees Fahrenheit. Cup 1 is then heated an additional 20 degrees Centigrade, cup 2 is heated an additional 20 Kelvin. Which cup of coffee is hotter? A) OneB) TwoC) Same 20

4. Thermal Expansion l When temperature rises è molecules have more kinetic energy »they are moving faster, on the average è consequently, things tend to expand l amount of expansion depends on… è change in temperature è original length è coefficient of thermal expansion »L 0 +  L = L 0 +  L 0  T »  L =  L 0  T (linear expansion) »  V =  V 0  T (volume expansion) Temp: T Temp: T+  T L0L0 LL 23

5. Density Question As you heat a block of aluminum from 0 C to 100 C its density A. Increases B. Decreases C. Stays the same T = 0 C M, V 0  0 = M / V 0 T = 100 C M, V 100  100 = M / V 100 <  0 26

6. Example: concrete sidewalk A concrete (  =12x10 -6 /K) sidewalk is 10m long when poured on a cold day (0 o C) How much will the length of the sidewalk increase on a hot day (35 o C)?

7. Example: gas tank l A steel (β=36x10 -6 /K) gas tank has a volume of 75 lit. You fill it up with gasoline (β=950x10 -6 /K) early in the morning when it is cool During the day the temperature increases by 20 o C. How much gas will spill out?

8. Differential Expansion Demo A bimetallic strip is made with aluminum  =16x10 -6 /K on the left, and iron  =12x10 -6 /K on the right. At room temperature, the lengths of metal are equal. If you heat the strips up, what will it look like? A BC Aluminum gets longer, forces curve so its on outside 29

9. Amazing Water l Water is very unusual in that it has a maximum density at 4 degrees C. That is why ice floats, and we exist! 30

10. Tight Fit An aluminum plate has a circular hole cut in it. An aluminum ball (solid sphere) has exactly the same diameter as the hole when both are at room temperature, and hence can just barely be pushed through it. If both the plate and the ball are now heated up to a few hundred degrees Celsius, how will the ball and the hole fit ? A. The ball wont fit through the hole any more B. The ball will fit more easily through the hole C. Same as at room temperature 35

11. Why does the hole get bigger when the plate expands ??? Object at temp T Same object at higer T: Plate and hole both get larger Imagine a plate made from 9 smaller pieces. Each piece expands. If you remove one piece, it will leave an “expanded hole” 36

12. A glass jar (  = 3x10 -6 K -1 ) has a metal lid (  = 16x10 -6 K -1 ) which is stuck. If you heat them by placing them in hot water, the lid will be A. Easier to open B. Harder to open C. Same Stuck Lid Question 38 Copper lid expands more, making a looser fit, and easier to open!

13. Heat l Definition: Flow of energy between two objects due to difference in temperature è Note: similar to WORK è Object does not “have” heat (it has energy: temp) l Units: Joule è 4186 Joules = 1 Calorie = 1000 calories = è calorie: Amount of heat needed to raise 1g of water 1ºC 10

14. Example: Sears Tower l You decide to take the stairs to the top of the Sears tower (442m). If you have a weight of 670N and your body was 100% efficient in converting food into mechanical energy. How many Calories would you need to eat to replenish your body Whopper with Cheese: 696 Cal Big Mac with Cheese: 560 Cal

15. Specific Heat l Heat adds energy to object/system l IF system does NO work then:  Heat increases internal energy. Q =  U è Heat increases temperature! Q = c m  T è Heat required to increase Temp depends on amount of material (m) and type of material (c) l Q = cm  T : “Cause” = “inertia” x “effect” (just like F=ma) è cause = Q è effect =  T è inertia = cm (mass x specific heat capacity) l  T = Q/cm (just like a = F/m) 15

16. Question l After a grueling work out, you drink a liter of cold water (0 C). How many Calories does it take for your body to raise the water up to body temperature of 36 C? 1) 36 2) 360 3) 3,600 4) 36,000 1 liter = 1,000 grams of H 2 0 1000 g x 1 calorie/(gram degree) x (36 degree) = 36,000 calories 36,000 calories = 36 Calories! 18

17. Question Suppose you have two insulated buckets containing the same amount of water at room temperature. You also happen to have two blocks of metal of the same mass, both at the same temperature, warmer than the water in the buckets. One block is made of aluminum and one is made of copper. You put the aluminum block into one bucket of water, and the copper block into the other. After waiting a while you measure the temperature of the water in both buckets. Which is warmer? 1. The water in the bucket containing the aluminum block 2. The water in the bucket containing the copper block 3. The water in both buckets will be at the same temperature Since aluminum has a higher specific heat than copper, you are adding more heat to the water when you dump the aluminum in the bucket (q=mc  T). 20 Substance c in J/(kg-C) aluminum900 copper387

18. Specific Heat Question Suppose you have equal masses of aluminum and copper at the same initial temperature. You add 1000 J of heat to each of them. Which one ends up at the higher final temperature A) aluminum B) copper C) the same  T = Q/cm 23 Substance c in J/(kg-C) aluminum900 copper387 iron452 lead128 human body 3500 water 4186 ice 2000

19. Latent Heat L l As you add heat to water, the temperature increases for a while, then it remains constant, despite the additional heat! l Latent Heat L [J/kg] is heat which must be added (or removed) for material to change phase (liquid- gas). 28 T Q added to water water temp rises water changes to steam (boils) steam temp rises 100 o C Latent Heat Substance L f (J/kg) L v (J/kg) water33.5 x 10 4 22.6 x 10 5

20. Ice Question l Which will do a better job cooling your soda, a “cooler” filled with water at 0C, or a cooler filled with ice at 0 C. A) WaterB) About SameC) Ice T Q added to water ice temp rises ice changes to water (melts) water temp rises 0 o C Latent Heat Substance L f (J/kg) L v (J/kg) water33.5 x 10 4 22.6 x 10 5 Latent Heat L [J/kg] is heat which must be added (or removed) for material to change phase (liquid- gas). 30

21. Example: sweat l During a tough work out, your body sweats (and evaporates) 1 liter of water to keep cool (37 C). How much water would you need to drink (at 2C) to achieve the same thermal cooling? (recall C V = 4.2 J/g for water, L v =2.2x10 3 J/g) 33

22. Question Summers in Phoenix Arizona are very hot (125 F is not uncommon), and very dry. If you hop into an outdoor swimming pool on a summer day in Phoenix, you will probably find that the water is too warm to be very refreshing. However, when you get out of the pool and let the sun dry you off, you find that you are quite cold for a few minutes (yes...you will have goose-bumps on a day when the air temperature is over 120 degrees). How can you explain this? 35

23. Example: ice and water l How much ice (at 0 C) do you need to add to 0.5 liters of a water at 25 C, to cool it down to 10 C? (L = 80 cal/g, c = 1 cal/g C, c ice = 0.5 cal/g C)

24. Example: ice and water 2 l 0.8kg of ice (at -10 o C) is added to 1.4kg of water at 20 o C, How much of the ice will melt? (L f = 33.5x10 4 J/kg, c water = 4186 J/kg C, c ice = 2000 J/kg C)

25. Summary l Temperature measure of average Kinetic Energy of molecules l Thermal Expansion è  L =  L 0  T (linear expansion) è  V =  L 0  T (volume expansion) l Heat is FLOW of energy è Flow of energy may increase temperature l Specific Heat   t = Q / (c m) è Monatomic IDEAL Gas C V = 3/2 R è Diatomic IDEAL Gas C V = 5/2 R l Latent Heat è heat associated with change in phase