Announcements 1. Schedule – Chapter 19 – macroscopic view of heat (today) Chapter 20 – microscopic view of heat (Tuesday – 11/18) Review Chapters 15-20 – (Thursday – 11/20) Exam 3 – (Tuesday – 11/25) 2. Physics colloquium today – Professor Gary Pielak from UNC will speak about “Protein Biophysics in Cells”. 3. Today’s lecture – Chapter 19 Temperature Heat The first law of thermodynamics 11/13/2003 PHY 113 -- Lecture 19 1 Dictionary definition: temperature – a measure of the the warmth or coldness of an object or substance with reference to some standard value. The temperature of two systems is the same when the systems are in thermal equilibrium. Equilibrium: Not equilibrium: T1 T2 T3 “Zeroth” law of thermodynamics: If objects A and B are separately in thermal equilibrium with a third object C, then objects A and B are in thermal equilibrium with each other. 11/13/2003 PHY 113 -- Lecture 19 2 Temperature scales TF=9/5 TC + 32 500 450 400 350 Kelvin scale: 300 250 T = TC + 273.15o TF 200 T≥0 150 100 50 0 -5 0 -1 0 0 -1 5 0 -2 0 0 -1 0 0 -5 0 0 50 100 150 200 TC 11/13/2003 PHY 113 -- Lecture 19 3 There is a lowest temperature: T0 = -273.15o C = 0 K Kelvin (“absolute temperature”) scale TC = -273.15 + TK Example – Room temperature = 68o F = 20o C = 293.15 K 11/13/2003 PHY 113 -- Lecture 19 4 11/13/2003 PHY 113 -- Lecture 19 5 Effects of temperature on matter Solids and liquids Model of a solid composed of atoms and bonds Thermal exansion: ∆L = α Li ∆T ∆L 11/13/2003 Li (equilibrium bond length at Ti) PHY 113 -- Lecture 19 6 Typical expansion coefficients at TC = 20o C: Linear expansion: ∆L = α Li ∆T α = 11 x 10-6/ oC Steel: Concrete: α = 12 x 10-6/ oC Volume expansion: V=L3 Î ∆V = 3α Vi ∆T = β Vi ∆T Alcohol: Air: 11/13/2003 β = 1.12 x 10-4/ oC β = 3.41 x 10-3/ oC PHY 113 -- Lecture 19 7 Brass Steel 11/13/2003 PHY 113 -- Lecture 19 8 Heat – Q -- the energy that is transferred between a “system” and its “environment” because of a temperature difference that exists between them. Sign convention: Q<0 if T1 < T2 Q>0 if T1 > T2 T1 11/13/2003 T2 Q PHY 113 -- Lecture 19 9 Heat withdrawn from system Thermal equilibrium – no heat transfer Heat added to system 11/13/2003 PHY 113 -- Lecture 19 10 Units of heat: Joule Other units: calorie = 4.186 J Kilocalorie = 4186 J = Calorie Heat capacity: C = amount of heat which must be added to the “system” to raise its temperature by 1K (or 1o C). Q = C ∆T More generally : Tf Qi → f = ∫ C (T )dT Ti Heat capacity per mass: C=mc Heat capacity per mole (for ideal gas): C=nCv 11/13/2003 PHY 113 -- Lecture 19 C=nCp 11 Some typical specific heats Material Water (15oC) Ice (-10oC) Steam (100oC) Wood Aluminum Iron Gold 11/13/2003 J/(kg·oC) 4186 2220 2010 1700 900 448 129 PHY 113 -- Lecture 19 cal/(g·oC) 1.00 0.53 0.48 0.41 0.22 0.11 0.03 12 Heat and changes in phase of materials Example: A plot of temperature versus Q added to 1g = 0.001 kg of ice (initially at T=-30oC) Q=333J Q=2260J 11/13/2003 PHY 113 -- Lecture 19 13 Some typical latent heats Material Ice ⇒Water (0oC) Water ⇒ Steam (100oC) Solid N ⇒ Liquid N (63 K) Liquid N ⇒ Gaseous N2 (77 K) Solid Al ⇒ Liquid Al (660oC) Liquid Al ⇒ Gaseous Al (2450oC) 11/13/2003 PHY 113 -- Lecture 19 J/kg 333000 2260000 25500 201000 397000 11400000 14 Peer instruction question Suppose you have a well-insulated cup of hot coffee (m=0.25kg, T=100oC). In order to get to class on time you add 0.25 kg of ice (at 0oC). When your cup comes to equilibrium, what will be the temperature of the coffee. (A) 0oC 11/13/2003 (B) 10oC (C) 50oC PHY 113 -- Lecture 19 (D) 100oC 15 Review question Suppose you have a well-insulated cup of hot coffee (m=0.25kg, T=100oC). In order to get to class on time you add 0.25 kg of ice (at 0oC). When your cup comes to equilibrium, what will be the temperature of the coffee. Q = m cw (Tf – 100oC) + m Lice + m cw (Tf − 0oC) = 0 2 cw Tf = cw · 100 − Lice Tf = cw · 100/(2 cw ) − Lice /(2 cw ) Tf = 50 –333000/(2 · 4186) = 10oC 11/13/2003 PHY 113 -- Lecture 19 16 Energy in the form of work: Work done by the “system” due to volume change xf xf Vf F W = ∫ Fdx = ∫ Adx = ∫ PdV xi xi A Vi Sign convention: W>0 if Vf > Vi (expansion) W<0 if Vf < Vi (contraction) 11/13/2003 PHY 113 -- Lecture 19 17 Work done by a gas: P (1.013 x 105) Pa “Isobaric” (constant pressure process) Po W= Po(Vf - Vi) Vi 11/13/2003 Vf PHY 113 -- Lecture 19 18 Work done by ideal gas: “Isovolumetric” (constant volume process) P (1.013 x 105) Pa Pf W=0 Pi Vi 11/13/2003 PHY 113 -- Lecture 19 19 Work done by a gas: “Isothermal” (constant temperature process) P (1.013 x 105) Pa For ideal gas: PV = nRT Wi → f Vf Pi ⎛V f = PiVi ln⎜⎜ ⎝ Vi Vi 11/13/2003 ⎛V f nRT = ∫ PdV = ∫ dV =nRT ln⎜⎜ Vi Vi V ⎝ Vi Vf ⎞ ⎟⎟ ⎠ Vf PHY 113 -- Lecture 19 20 ⎞ ⎟⎟ ⎠ Work done by a gas: “Adiabatic” (no heat flow in the process process) Qi→f = 0 For ideal gas: P (1.013 x 105) Pa PVγ = PiViγ Pi Wi → f Vi 11/13/2003 PiVi PiVi ⎡⎛ V f = ∫ PdV = ∫ γ dV = ⎢⎜⎜ γ − 1 ⎣⎢⎝ Vi Vi Vi V Vf Vf γ ⎞ ⎟⎟ ⎠ γ −1 ⎤ − 1⎥ ⎥⎦ Vf PHY 113 -- Lecture 19 21 Thermodynamic statement of conservation of energy – First Law of Thermodynamics ∆Eint = Q - W Work done by system Heat added to system “Internal” energy of system 11/13/2003 PHY 113 -- Lecture 19 22 “Internal energy” Eint=Eint(T,V,P) (for an ideal gas, Eint=Eint(T) W Tsys “environment” can be changed by interaction with the system Q “system” Tenv 11/13/2003 ∆Eint = Q - W Note: Thermal equilibrium implies a uniform temperature. In this example, the system and the environment are presumed to be in thermal equilibrium within themselves but not in thermal equilibrium with eachother. PHY 113 -- Lecture 19 23 Examples process: Wnet=W(ABCDA)=WBC+WDA P (1.013 x 105) Pa Pf B A Pi C D =(Pf−Pi) (Vf−Vi) ∆Eint(ABCDA)= ∆Eint(AB) +∆Eint(BC) +∆Eint(CD) +∆Eint(DA)=0 ÎQnet=Q(ABCDA)=Wnet Vi 11/13/2003 Vf PHY 113 -- Lecture 19 24 6 m3 1 m3 30 Pa 10 Pa 11/13/2003 PHY 113 -- Lecture 19 25 11/13/2003 PHY 113 -- Lecture 19 26 11/13/2003 PHY 113 -- Lecture 19 27 Mechanisms of heat transfer: 1. Thermal convection Heat transmitted by heated fluid flow. (Ex. -- home heating units, stove top cooking) 2. Radiation Heat transmitted by electromagnetic radiation. (Ex. – sun, microwave cooking) 3. Thermal conduction Heat transfer from one side of a material to another due to a temperature gradient. 11/13/2003 PHY 113 -- Lecture 19 28 Quantitative statement of thermal conduction: ∆Q ∆T Units: 1 J/s = 1 Watt (W) = kA ∆t ∆x cross-sectional area thermal conductivity coefficient Material Copper Glass Water Air 11/13/2003 k (W/(m·oC)) 238 0.8 0.6 0.0234 PHY 113 -- Lecture 19 29 Examples of thermal conduction T1 T −T dQ = keff A 2 1 L2 + L1 dt T2 − T1 dQ = k2 A L2 dt keff 11/13/2003 PHY 113 -- Lecture 19 L2 + L1 = L2 / k 2 + L1 / k1 30 Example: T1=20oC, T2= 0oC Single pane glass window: A=1m2 , L2 = 0.002m, k2=0.8 W/m·oC T2 − T1 dQ = k2 A = 8000 W dt L2 Double pane glass window: L1=0.01m, k1=0.0234 W/m·oC (air) T2 − T1 dQ = keff A L2 + L1 + L0 dt keff L2 + L1 + L0 = = 46 W L2 / k 2 + L1 / k1 + L0 / k0 11/13/2003 PHY 113 -- Lecture 19 31