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Category: Thermodynamics

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Presentation on theme: "Category: Thermodynamics"— Presentation transcript:

1 Category: Thermodynamics
1 Category: Thermodynamics II. Heat and Phase changes Updated: 2014March13

2 Outline Heat Capacity (Storage of Heat) Heat Flow Phases of Matter
2 Outline Heat Capacity (Storage of Heat) Heat Flow Phases of Matter References

3 A. Heat Capacity Heat is Energy Storage of Energy: Heat Capacity
3 Heat is Energy Storage of Energy: Heat Capacity Atomic Theory of Specific Heats

4 1. Heat is Energy Caloric Theory Friction creates heat
4 Caloric Theory Friction creates heat Equivalence of heat and energy

5 Antoine Lavoisier 1743-1794 (beheaded-French Revolution)
1a. Caloric Theory (1783) 5 “Caloric”: the substance of heat It flows like a fluid from hot to cold objects until “level” (same temperature) It is conserved (heat cannot be created, only moved around) 1 calorie raises 1 gm of water by 1C (Nicolas Clement 1824) Antoine Lavoisier (beheaded-French Revolution)

6 1b. Mechanical Equivalence of Heat
6 Count Rumford: Inventor of the “drip” coffee pot 1798 shows that heat is NOT conserved (boring a cannon creates enough heat via friction to boil water) Sir Benjamin Thompson Count Rumford

7 1c. Heat is Energy (Joule experiment)
7 experiment, dropping weight drives paddlewheel that heats fluid. 1 calorie of heat is equivalent to Joules of work 1847 Helmholtz states principle of conservation of total energy James Prescott Joule

8 2. Storage of Heat 8 Heat Capacity Specific Heat Calorimetery

9 2a. Heat Capacity Heat is a form of energy that can be stored
9 Heat is a form of energy that can be stored Heat Capacity: the amount of heat Q required to raise temperature of system by T=1 SI Units: Joule/C Extensive quantity

10 2b. Specific Heat 10 Specific Heat is the (intensive) measure of heat capacity per unit (thermal) mass Joseph Black (1760s) shows materials have different values of specific heat Joseph Black Material J/kg °C cal/gm °C Copper 386 0.092 Aluminum 900 0.215 Air 1050 0.251 Ice 2220 0.530 Water 4186 1.000

11 2c. Calorimetry First calorimeter used by Lavoisier & Laplace 1782
11 First calorimeter used by Lavoisier & Laplace 1782 Measure specific heat “c” of block of metal (mass M) by heating it to temperature Th, drop into mass “m” of cold water (Tc), measure final temperature T

12 3. Atomic Theory of Specific Heat
12 Specific Heat of Gas Specific Heat of Solids, Dulong-Petit Law Low Temperature Behavior

13 3a. Specific Heat of a Gas 13 At constant volume*, heat added to a monatomic gas goes into random kinetic energy of molecules. All monatomic gasses have same specific heat per mole (R=gas constant) ! For diatomic gasses, heat also goes into two axes of rotational kinetic energy. Each mode contributes (1/2)R per mole *If instead measured at constant pressure, the specific heat is more because energy goes into work of expanding the gas.

14 3b. Specific Heats of Solids
14 Dulong & Petit Law (1819) show that many solids have the same specific heat if measured per mole (instead of per mass) of 25 J/mol C Later it was realized this is related to gas constant c=3R Material J/kg °C gm/mol J/mol °C Aluminum 900 26.98 24.3 Copper 386 63.55 24.5 Silver 236 107.87 25.5 Tungsten 134 183.84 24.6 Lead 128 207.2 26.5

15 3c. Einstein and Debye Models
15 Einstein (1907) and Debye (1912) show that specific heats all approach 3R at high enough temperature At low temperature go to zero (this prevents being able to go below absolute zero!)

16 3d. Einstein and Debye Models
16 Einstein’s Model (1907) works well at intermediate and high temperatures, but not at low temperature. Debye’s Model (1912) works well at low temperature and high, but not in the middle. The Debye Temperature: TD At low temperatures Debye shows that the specific heat increases with the cube of the temperature.

17 B. Heat Flow There are three mechanisms by which heat flows:
17 There are three mechanisms by which heat flows: Convection Conduction Radiation

18 1. Convection 18 Heat moved by physical flow of gas/liquid. Often creates “convection cells” (can be seen on surface of sun!). No good formula!

19 2. Conduction 19 (a) Phenomena: Heat in a solid is transported by collisions between electrons. Generally good conductors of electricity are also good conductors of heat because the electrons are free to move. Newton’s Law of Cooling Loss of heat is proportional to the difference in temperature of system to environment [R=thermal resistance] Temperature of system will follow an exponential decay law [C=heat capacity]

20 2c. Law of Thermal Conduction
20 (c) Fourier’s Theory of thermal conduction Heat Flux: heat flow per time (Watts)=Q/t Amount of heat flow is inversely proportional to the “Thermal Resistance R” of the system (units of degree per Watt). Thermal resistance “R” depends upon geometry (length L, area A, hence its “extensive”) and the thermal conductivity “k” of the material Th Tc

21 2c. Thermal Conductivity
21 Thermal conductivity (intensive quantity!) of solids are better than liquids or gasses. In the latter, convection will usually dominate. Aluminum 240 Water 0.57 Air Vacuum 0

22 3. Radiation 22 (a) Stefan’s Law Emissivity Black Body Radiation Curve

23 3a. Josef Stefan’s Law 1879 Power (watts)=AT4
23 Experimentally shows total output of light of a hot dense (black) body is proportional to 4th power of the temperature (in Kelvin) Power (watts)=AT4 =5.67x10-8 Watts/(m2-K4) A=surface area 1884 Ludwig Boltzmann (former student of Stefan) derives formula from thermodynamics. I was a guest speaker (Sept 2005) at the Josef Stefan Institute in Slovenia.

24 3a ii Measure Temperature of Sun
24 1604 Kepler proposes intensity of light drops of with square of distance (?) Charles Soret measures solar flux to be about 1400 Watts/m2 at surface of the earth. Stefan uses this to estimate temperature of sun to be 5700 K.

25 3b Leslie Cube Experiment (1804)
25 A cube with different emissitivites on different faces. One usually shows that the “black” surface radiates better than “white” surface.

26 3bii Emissivity 26 A perfect “black body” will radiate according to Stefan’s law. Most systems are not perfect, and so we include a “fudge factor” called the “emissivity”: 0<e<1 Further, the environment at temperature Te will radiate energy back into the system, so the rate at which system loses heat is:

27 3c.i. Wien’s Displacement Law
27 1893 shows that the “color” of black body is inversely proportional to temperature Wien’s constant =2,898,000 nm-K So T=6000K gives =483 nm

28 3c.ii. Black Body Curve Willhelm Wien gets Nobel Prize 1911
28 Willhelm Wien gets Nobel Prize 1911 1894 coins term “black body” The black body emits all colors, but where it peaks is described by Wien’s law

29 3.c.iii. Black Body Theory 29 Maxwell: hot atoms vibrate, acting like small antennas, radiating electromagnetic waves Wien tries to give theory to explain shape of curve, but it fails in IR Rayleigh (1900) & Jeans (1905) have another theory, but it fails in UV, blowing up to infinite energy (the “ultraviolet catastrophe”).

30 3c.iv. Max Planck’s Theory
30 1900 Max Planck ad-hoc proposes that vibrations are “quantized”, i.e. come in steps of n=1, 2, 3, rather than continuous. Energy: E=nhf n=integer quantum number f=frequency of oscillation h is “Planck’s Constant h=6.626x10-34 Joule-Sec

31 3cv. Planck Radiation Law
31 His theory exactly matched the experimental measurements of the black body radiation curve k = Boltzmann Constant (1.3810-23 Joule/Kelvin)

32 C. Phases of Matter Phases of matter Latent Heats of Phase Change
32 Phases of matter Latent Heats of Phase Change Phase Diagrams (PVT diagrams)

33 1. Phases There are 4 states of matter (called “Phases”) Solid Liquid
33 There are 4 states of matter (called “Phases”) Solid Liquid Gas Plasma (hot gas ionizes)

34 1b. Plasma 34 Superheating a gas, it will ionize (electrons separate from rest of atom) into a 4th state of matter called a “plasma”.

35 1c. Van der Waals equation
35 Why are there phases of matter? Van der Waals (Nobel Prize 1910) modified gas equation predicts solid, liquid and gas phases. “a” represents attractive forces between molecules and “b” the volume of a mole of molecules. Johannes van der Waals

36 2. Latent Heats 36 Joseph Black Black (1761) measures the amount of heat it takes to change phase of water. Defines: Latent Heat of fusion (melt ice) is 80 cal/gm Latent Heat of vaporization (boil) 597 cal/gm

37 2b. Latent Heats-continued
37 Some substances, n.b. dry ice (CO2), go straight from solid to gas, so we have a latent heat of “sublimation” (opposite process is “deposition”) Dry ice latent heat of sublimation is: 571 J/gm Much better than using water ice (no melted water!)

38 3(a) PT Diagram for Pure Substance
38 Triple Point: all 3 phases coexist. Above critical point it’s a “supercritcal fluid”, no distinction between gas and liquid Clausius-Clapeyron equation tells us the slope of the phase change curve, where “L” is the latent heat, and v is change in volume per mole of phase transition.

39 PT Diagram for Water 39 Expands when freezes, hence ice under pressure will melt (ice skates!) Note from A to D the slope is negative!

40 PT Diagram for Helium 40 Helium: Has two different liquid states, hence two “triple points”

41 PVT diagram 41 Van der Waals equation PVT diagrams

42 PVT diagram 42

43 Misc Notes 43 MCAT includes Van der Waals equation.
Condensation vs evaporation Evaporation takes place at surface, boiling is throughout fluid. Regelation (melting under pressure of ice) Heat released by freezing, e.g. center of earth. Change of phase of hydrogen to a metal in jupiter and saturn (liquid or solid?) Ice III (what happened to Ice II ?), what conditions for change, glaciers?


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