2. Physics 207: Lecture 24, Pg 1 Lecture 24 Goals: Chapter 17 Chapter 17  Employ heat (Q) and energy transfer in materials  Recognize adiabatic processes (i.e., Q=0) Chapter 18 Chapter 18  Follow the connection between temperature, thermal energy, and the average translational kinetic energy molecules  Understand the molecular basis for pressure and the ideal- gas law.  To predict the molar specific heats of gases and solids. Assignment Assignment  HW11, Due Wednesday 9:00 AM  For Thursday, Read through all of Chapter 18

3. Physics 207: Lecture 24, Pg 2 1 st Law of Thermodynamics l Work W and heat Q depend on process by which the system is changed (path dependent). l The change of energy in the system, ΔE th depends only on the total energy exchanged W+Q, not on the process. ΔE th =W + Q (if  K &  U =0 ) W & Q with respect to the system

4. Physics 207: Lecture 24, Pg 3 1 st Law: Work & Heat l Work done on system (an ideal gas….notice minus sign, V is in reference to the system) l W on system V i )] l If ideal gas, pV = nRT l W by system > 0 Moving left to right

5. Physics 207: Lecture 24, Pg 4 1 st Law: Work & Heat l Work:  Depends on the path taken in the pV-diagram (It is not just the destination but the path…)  W on system > 0 Moving right to left

6. Physics 207: Lecture 24, Pg 5 1 st Law: Work (“Area” under the curve) l Work depends on the path taken in the pV-diagram : (a) W a = W 1 to 2 + W 2 to 3 (1 st p then V constant, T changes)  W a (on) = - p i (V f - V i ) + 0 > 0 (b) W b = W 1 to 2 + W 2 to 3 (1 st p then V constant, T changes)  W b (on) = 0 - p f (V f - V i ) > W a > 0 (c) Need explicit form of p versus V but W c (on) > 0 2 1 3 1 2 3 W 1  2 = -p i (V f -V i ) W 2  3 = -p f (V f -V i )

7. Physics 207: Lecture 24, Pg 6 (1) Isobaric (2) Isothermal (3) Isochoric (4) Adiabatic Paths on the pV diagram (with an idea gas) p V 3 4 2 1 T1T1 T2T2 T3T3 T4T4 W = - p  V ???? W = 0 ???? Ideal gas

8. Physics 207: Lecture 24, Pg 7 Isothermal processes (in an ideal gas) l Work done when PV = nRT = constant  P = nRT / V p V 3 T1T1 T2T2 T3T3 T4T4 For this we need access to thermal energy

9. Physics 207: Lecture 24, Pg 8 Adiabatic Processes (in an ideal gas) l An adiabatic process is process in which there is no thermal energy transfer to or from a system (Q = 0) l A reversible adiabatic process involves a “worked” expansion in which we can return all of the energy transferred. l In this case PV  = const. l All real processes are not. l We need to know C p & C V p V 2 1 3 4 T1T1 T2T2 T3T3 T4T4

10. Physics 207: Lecture 24, Pg 9 Work and Ideal Gas Processes (on system) l Isothermal l Isobaric l Isochoric FYI: Adiabatic (and reversible) PV  = const.

11. Physics 207: Lecture 24, Pg 10 Two process are shown that take an ideal gas from state 1 to state 3. (“by” means “by the system on the world”) Compare the work done by process A to the work done by process B. A. W A > W B B. W A < W B C. W A = W B = 0 D. W A = W B but neither is zero ON BY A 1  3 W 1  2 = 0 (isochoric) B 1  2 W 1  2 = -½ (p 1 +p 2 )(V 2 -V 1 ) 0 B 2  3 W 2  3 = -½ (p 2 +p 3 )(V 1 -V 2 ) > 0 -W 2  3 < 0 B 1  3 = ½ (p 3 - p 1 )(V 2 -V 1 ) > 0 < 0 p1p1 p2p2 p3p3

12. Physics 207: Lecture 24, Pg 11 Two process are shown that take an ideal gas from state 1 to state 3. Compare the work done by process A to the work done by process B. A. W A > W B B. W A < W B C. W A = W B = 0 D. W A = W B but neither is zero ON BY A 1  3 W 1  2 = 0 (isochoric) B 1  2 W 1  2 = -½ (p 1 +p 2 )(V 2 -V 1 ) 0 B 2  3 W 2  3 = -½ (p 2 +p 3 )(V 1 -V 2 ) > 0 -W 2  3 < 0 B 1  3 = ½ (p 3 - p 1 )(V 2 -V 1 ) > 0 < 0

13. Physics 207: Lecture 24, Pg 12 Both Q and W can change T l We know how work changes the mechanical energy of a solid “system” l Here our system is an ideal gas….only the temperature can change l For real materials we can change the temperature or the state l We must quantify the response of a system to thermal energy transfer (Q)

14. Physics 207: Lecture 24, Pg 13 What about Q? What are the relationships between  E Th and T. Latent Heat Specific Heat

15. Physics 207: Lecture 24, Pg 14 Heat and Latent Heat l Latent heat of transformation L is the energy required for 1 kg of substance to undergo a phase change. (J / kg) Q = ±ML l Specific heat c of a substance is the energy required to raise the temperature of 1 kg by 1 K. (Units: J / K kg ) Q = M c ΔT l Molar specific heat C of a gas at constant volume is the energy required to raise the temperature of 1 mol by 1 K. Q = n C V ΔT If a phase transition involved then the heat transferred is Q = ±ML+M c ΔT

16. Physics 207: Lecture 24, Pg 15 Q : Latent heat and specific heat l The molar specific heat of gasses depends on the process path l C V = molar specific heat at constant volume l C p = molar specific heat at constant pressure l C p = C V +R (R is the universal gas constant)

17. Physics 207: Lecture 24, Pg 16 Q : Latent heat and specific heat l The molar specific heat of gasses depends on the process path l C V = molar specific heat at constant volume l C p = molar specific heat at constant pressure l C p = C V +R (R is the universal gas constant)

18. Physics 207: Lecture 24, Pg 17 Latent Heat l Most people were at least once burned by hot water or steam. l An equal amount (by mass) of boiling water and steam contact your skin. l Which is more dangerous, the water or the steam?

19. Physics 207: Lecture 24, Pg 18 Mechanical equivalent of heat l Heating liquid water:  Q = amount of heat that must be supplied to raise the temperature by an amount  T.  [Q] = Joules or calories.  calorie: energy to raise 1 g of water from 14.5 to 15.5 °C (James Prescott Joule found the mechanical equivalent of heat.) 1 cal = 4.186 J 1 kcal = 1 cal = 4186 J Sign convention: +Q : heat gained - Q : heat lost

20. Physics 207: Lecture 24, Pg 19 Exercise l The specific heat (Q = M c ΔT) of aluminum is about twice that of iron. Consider two blocks of equal mass, one made of aluminum and the other one made of iron, initially in thermal equilibrium. l Heat is added to each block at the same constant rate until it reaches a temperature of 500 K. Which of the following statements is true? (a) The iron takes less time than the aluminum to reach 500 K (b) The aluminum takes less time than the iron to reach 500 K (c) The two blocks take the same amount of time to reach 500 K

21. Physics 207: Lecture 24, Pg 20 Exercise l The specific heat (Q = M c ΔT) of aluminum is about twice that of iron. Consider two blocks of equal mass, one made of aluminum and the other one made of iron, initially in thermal equilibrium. l Heat is added to each block at the same constant rate until it reaches a temperature of 500 K. Which of the following statements is true? (a) The iron takes less time than the aluminum to reach 500 K (b) The aluminum takes less time than the iron to reach 500 K (c) The two blocks take the same amount of time to reach 500 K

22. Physics 207: Lecture 24, Pg 21 Heat and Ideal Gas Processes (on system) l Isothermal Expansion/Contraction l Isobaric l Isochoric l Adiabatic

23. Physics 207: Lecture 24, Pg 22 Combinations of Isothermal & Adiabatic Processes All engines employ a thermodynamic cycle W = ± (area under each pV curve) W cycle = area shaded in turquoise Watch sign of the work!

24. Physics 207: Lecture 24, Pg 23 l Most people were at least once burned by hot water or steam. l Assume that water and steam, initially at 100°C, are cooled down to skin temperature, 37°C, when they come in contact with your skin. Assume that the steam condenses extremely fast, and that the specific heat c = 4190 J/ kg K is constant for both liquid water and steam. l Under these conditions, which of the following statements is true? (a) Steam burns the skin worse than hot water because the thermal conductivity of steam is much higher than that of liquid water. (b) Steam burns the skin worse than hot water because the latent heat of vaporization is released as well. (c) Hot water burns the skin worse than steam because the thermal conductivity of hot water is much higher than that of steam. (d) Hot water and steam both burn skin about equally badly. Exercise Latent Heat

25. Physics 207: Lecture 24, Pg 24 Exercise Latent Heat l Most people were at least once burned by hot water or steam. Assume that water and steam, initially at 100°C, are cooled down to skin temperature, 37°C, when they come in contact with your skin. Assume that the steam condenses extremely fast, and that the specific heat c = 4190 J/ kg K is constant for both liquid water and steam. l Under these conditions, which of the following statements is true? (b) Steam burns the skin worse than hot water because the latent heat of vaporization is released as well. l How much heat H 1 is transferred to the skin by 25.0 g of steam? l The latent heat of vaporization for steam is L = 2256 kJ/kg. H 1 = 0.025 kg x 2256 kJ/kg = 63.1 kJ l How much heat H 2 is transferred to the skin by 25.0 g of water? H 2 = 0.025 kg x 63 K x 4190 J/ kg K = 6.7 kJ

26. Physics 207: Lecture 24, Pg 25 Energy transfer mechanisms l Thermal conduction (or conduction) l Convection l Thermal Radiation

27. Physics 207: Lecture 24, Pg 26 Energy transfer mechanisms l Thermal conduction (or conduction):  Energy transferred by direct contact.  e.g.: energy enters the water through the bottom of the pan by thermal conduction.  Important: home insulation, etc. l Rate of energy transfer ( J / s or W )  Through a slab of area A and thickness  x, with opposite faces at different temperatures, T c and T h Q /  t = k A (T h - T c ) /  x  k :Thermal conductivity ( J / s m °C)

28. Physics 207: Lecture 24, Pg 27 Thermal Conductivities Aluminum238Air0.0234Asbestos0.25 Copper397Helium0.138Concrete1.3 Gold314Hydrogen0.172Glass0.84 Iron79.5Nitrogen0.0234Ice1.6 Lead34.7Oxygen0.0238Water0.60 Silver427Rubber0.2Wood0.10 J/s m °C

29. Physics 207: Lecture 24, Pg 28 (B) T top = T bottom (A) T top > T bottom (C) T top < T bottom 100 C T joint l Two identically shaped bars (one blue and one green) are placed between two different thermal reservoirs. The thermal conductivity coefficient k is twice as large for the blue as the green. l You measure the temperature at the joint between the green and blue bars. Which of the following is true? Home Exercise Thermal Conduction 300 C (D) need to know k

30. Physics 207: Lecture 24, Pg 29 l Two identically shaped bars (one blue and one green) are placed between two different thermal reservoirs. The thermal conductivity coefficient k is twice as large for the blue as the green. Home Exercise Thermal Conduction 100 C T joint 300 C Top: P green = P blue = Q /  t = 2 k A (T high - T j ) /  x= k A (T j - T low ) /  x 2 (T high - T j ) = (T j - T low )  3 T j(top) = 2 T high – T low By analogy for the bottom: 3 T j(bottom) = 2 T low – T high 3 (T j(top) - T j(bottom ) = 3 T high – 3 T low > 0 (A) T top > T bottom

31. Physics 207: Lecture 24, Pg 30 100 C l Two thermal conductors are butted together and in contact with two thermal reservoirs held at the temperatures shown. l Which of the temperature vs. position plots below is most physical? Exercise Thermal Conduction 300 C Position Temperature Position Temperature (B) (C) Position Temperature (A)

32. Physics 207: Lecture 24, Pg 31 100 C l Two thermal conductors are butted together and in contact with two thermal reservoirs held at the temperatures shown. l Which of the temperature vs. position plots below is most physical? Exercise Thermal Conduction 300 C Position Temperature (B) (C) Position Temperature (A) Position Temperature

33. Physics 207: Lecture 24, Pg 32 Energy transfer mechanisms l Convection:  Energy is transferred by flow of substance 1. Heating a room (air convection) 2. Warming of North Altantic by warm waters from the equatorial regions  Natural convection: from differences in density  Forced convection: from pump of fan l Radiation:  Energy is transferred by photons e.g.: infrared lamps  Stefan’s Law   = 5.7  10 -8 W/m 2 K 4, T is in Kelvin, and A is the surface area  e is a constant called the emissivity P =  A e T 4 (power radiated)

34. Physics 207: Lecture 24, Pg 33 Minimizing Energy Transfer l The Thermos bottle, also called a Dewar flask is designed to minimize energy transfer by conduction, convection, and radiation. The standard flask is a double-walled Pyrex glass with silvered walls and the space between the walls is evacuated. Vacuum Silvered surfaces Hot or coldliquid

35. Physics 207: Lecture 24, Pg 34 Anti-global warming or the nuclear winter scenario Assume P/A = P = 1340 W/m 2 from the sun is incident on a thick dust cloud above the Earth and this energy is absorbed, equilibrated and then reradiated towards space where the Earth’s surface is in thermal equilibrium with cloud. Let e (the emissivity) be unity for all wavelengths of light. l What is the Earth’s temperature?   P =  A T 4 =  (4  r 2 ) T 4 = P  r 2  T = [ P / (4 x  )] ¼    = 5.7  10 -8 W/m 2 K 4  T = 277 K (A little on the chilly side.)

36. Physics 207: Lecture 24, Pg 35 Lecture 24 Assignment Assignment  HW11, Due Wednesday (9:00 AM)  Tuesday review  Reading assignment through all of Chapter 18