Thermodynamics (Lecture Notes) Heat and Thermodynamics (7 th Edition) by Mark W. Zemansky & Richard H. Dittman
|
|
|
- Felicia Mills
- 6 years ago
- Views:
Transcription
1 Thermodynamics (Lecture Notes Heat and Thermodynamics (7 th Edition by Mark W. Zemansky & Richard H. Dittman
2 2
3 Chapter 1 Temperature and the Zeroth Law of Thermodynamics 1.1 Macroscopic Point of View If no matter crosses the boundary, = a closed system. If an exchange of matter, = an open system. Two points of view: Macroscopic: the human scale or larger. Microscopic: the molecular scale or smaller. Macroscopic Coordinates: (provide a macroscopic description of a system 1. No special assumptions (e.g., the structure of matter 2. Few in number (to describe the system 3. Fundamental (as suggested by our sensory perceptions 4. Directly measurable Including the macroscopic coordinate of temp. = Thermodynamics. 1.2 Microscopic Point of View A microscopic description of a system: 1. Assumptions 2. Many quantities 3. Mathematical models 4. Theoretical calculation = Statistical mechanics (Ch. 12 3
4 4 CHAPTER 1. TEMPERATURE AND THE ZEROTH LAW OF THERMODYNAMICS 1.3 Macroscopic VS. Microscopic Points of View = (Macroscopic description = Microscopic description ave 1.4 Scope of Thermodynamics Thermaodynamic systems: a gas, a vapor, a mixture (e.g., vapor and air, surface films, electric cells, wire resistors, electric capacitors, and magnetic substances. 1.5 Thermal Equilibrium and The Zeroth Law The 0 th law of thermodynamics: If A C and B C, A B. ( : thermal equilibrium 1.6 Concept of Temperature Isotherm: The locus of all points representing states in which a system is in thermal equilibrium with one state of another system. (See Fig. 1-3 = If (X 1, Y 1 (X 1, Y 1, (X 2, Y 2 (X 1, Y 1, (X 3, Y 3 (X 1, Y 1,, = Isotherm I. = If (X 1, Y 1 (X 1, Y 1, (X 2, Y 2 (X 1, Y 1, (X 3, Y 3 (X 1, Y 1,, = Isotherm I. The temperature of a system is a property that determines whether or not a system is in thermal equilibrium with other systems. 1.7 Thermometers and Measurement of Temperature (See Fig. 1-4 θ(x = a X (const. Y (1 See Fig. 1-5 (Triple-pt. cell θ T P = K (2 (1 = θ(x T P = a X T P ( = a = K X T P = θ(x = ( K X X T P # (const. Y 1.8 Comparison of Thermometers In Table 1.1, = six thermometers. For a gas, = θ(x = ( K P P T P (const. V.
5 1.9. GAS THERMOMETER 5 For a wire resistor, = θ(r = ( K R R T P For a thermocouple, = θ(e = ( K E E T P (const. tension. (const. tension. In Table 1.2, = choose a gas thermometers as the standard thermometer. 1.9 Gas Thermometer See Fig (The volume of the gas is kept constant Ideal-Gas Temperature Ideal-gas law: where P V = n R T, (1 n: the number of moles, R: the molar gas const., T : theoretical thermodynamic temp. (Sec Experiment: (T θ (1 = P V = n R θ P T P V = n R θ T P, θ T P = K = θ = ( K P P T P # (const. V (2 Measuring T : (at the normal boiling pt. of water 1. With the triple-pt. cell = P T P = 120 kpa (suppose. With steam, measure P NBP = θ(p NBP = ( K PNBP Remove some of the gas = P T P, say, 60 kpa. Measure the new P NBP = θ(p NBP = ( K PNBP Repeat the procedures 1 and Plot θ(p NBP P T P, = T = lim P T P 0 θ(p NBP = K lim P T P 0 P P T P # (const. V (See Fig. 1-7.
6 6 CHAPTER 1. TEMPERATURE AND THE ZEROTH LAW OF THERMODYNAMICS 1.11 Celsius Temp. Scale θ( 0 C = T (K e.g., θ NBP ( 0 C = T NBP (K = C }{{} # Platinum Resistance Thermometry Range: K ( C = R (T = R T P (1 + at + bt 2, a, b : consts. (empirical formula 1.13 Radiation Thermometry Blackbody radiation (> C 1.14 Vapor Pressure Thermometry Use 3 He or 4 He (isotopes of He. ( K 1.15 Thermocouple E = c 0 + c 1 θ + c 2 θ 2 + c 3 θ 3, c is : consts. ( C 1.16 International Temperature Scale of 1990 (ITS-90 (See Table 1.3 ITS-90 = a set of defining fixed points measured with the primary gas thermometer + a set of procedures for interpolation between the fixed points using secondary thermometers Rankine and Fahrenheit Temp. Scales T (R = 9 5 T (K θ( 0 F = T (R θ( 0 F = 9 5 θ(0 C + 32
7 Chapter 2 Simple Thermodynamic Systems 2.1 Thermodynamic Equilibrium mechanical equil. + chemical equil. + thermal equil. = thermodynamic equil. state 2.2 Equation of State For a closed system, the eq. of state relates the temperature to two other thermodynamic variables. e.g., (a gas = P V = nrt (very low pressure, or van der Waals eq.: P v = RT, v(= V/n: molar volume (or volume per mole, (P + a (v b = RT (higher pressure. v2 XYZ systems = Simple systems (e.g., a gas, 1-dim stretched wire, 2-dim. surface, Hydrostatic Systems E.g., a solid, a liquid, a gas, or a mixture of any two. = a P V T system The eq. of state, = V = func. of (T, P or V = V (T, P (1 or = P = func. of (T, V or P = P (T, V (2 7
8 8 CHAPTER 2. SIMPLE THERMODYNAMIC SYSTEMS or Exact differentials: = T = func. of (P, V or T = T (P, V (3 If dz is an exact differential of a func. of x and y, then ( ( z z dz = dx + dy, x y y x If P =const, (1 = dv = ( V T P ( V dt + P T dp, (4 = β = ( V/V T (coeff. of volume expansion, = β = 1 V If T =const, ( V T P (coeff. of volume expansion = B = P ( V/V (isothermal bulk modulus, = B = V ( P V T = κ = 1 V ( V P (2 = dp = ( P T (3 = dt = ( T P T (isothermal bulk modulus (isothermal compressibility V dt + ( P V V dp + ( T V T P dv, (5 dv, (6 (4 (6 = The dv, dp, and dt are differentials of actual functions. = exact differentials #. 2.4 Mathematical Theorems ( x 1 = ; y z ( y/ x z ( x y z ( y z x ( z = 1. x y e.g., a PVT system, ( = ( ( P V ( T V T T P P V = 1, = β = 1 V ( P = V T ( V T P & κ = 1 V ( V T ( T P P V = β κ # ( V P T,
9 2.5. STRETCHED WIRE 9 Therefore, (5 = dp = ( P T V dt + ( P V T dv = β κ dt 1 κv dv. If V = const, = dp = β κ dt, = P f P i dp = T f T i 2.5 Stretched Wire β κ, dt, = P f P i = β κ (T f T i # (V = const = a FLT system, F: tension (in N, L: length (in m, T : temp. (in K. If T = const, (within the limit of elasticity = F = k(l L 0, L 0 : the length at zero tension. (Hooke s law Since L = L(T, F, = dl = ( L T F dt + ( T F T df, If F = const, = α = 1 T ( L L (linear coeff. of exansion, = α = 1 L ( L T F (linaer coeff. of expansion If T =const, = Y = ( F/A ( L/L (Young s modulus, = Y = L A Since ( F L T = ( F T ( L T F ( F L T ( T F L = ( F L 2.6 Surfaces T (isothermal Young s mdulus = 1 L ( L T F = α A Y # = a γat system, γ: surface tension (in N/m, A: area (in m 2, T : temp. (in K. e.g., (1 For most pure liquids in equil. with their vapor phase,
10 10 CHAPTER 2. SIMPLE THERMODYNAMIC SYSTEMS = γ = γ 0 (1 T/T c n, γ 0 : the surface tension at 20 0 C, T c : critical temp., n: betw (2 A thin filem of oil on water, = (γ γ w A = a T, γ w : the surface tension of a clean water surface, a: a const. 2.7 Electrochemical Cell = a EZT system, E: emf (in Volts, Z: charge (in coulombs C, T : temp. (in K. Eq. of state, (by Exp. = E = E 20 + α(θ β(θ γ(θ , where E 20 : the emf at 20 0 C, θ: temp. in Celsius, α, β, γ: consts. 2.8 Dielectric Slab = an E PT system, where E: electric field (in V/m, P: tot. polarization emf (in C m, T : temp. (in K. Eq. of state, = P V = (a + b/t, a, b: consts. (for T > 10 K 2.9 Paramagnetic Rod = a HMT system, where H: magnetic field (in A/m, M: tot. magnetization (in A m 2, T : temp. (in K. Eq. of state, = M = CcH T, C c: Curie const Intensive and Extensive Coordinates Intensive coords. (indept of the mass:
11 2.10. INTENSIVE AND EXTENSIVE COORDINATES 11 e.g., P, F, γ, E, E, H, T, density(ρ,... Extensive coords. (propotional to the mass: e.g., V, L, A, Z, E, P, M, mass(m, U, S,... = extensive intensive = extensive
12 12 CHAPTER 2. SIMPLE THERMODYNAMIC SYSTEMS
13 Chapter 3 Work 3.1 Work If work is done on the system, = W > 0. If work is done by the system, = W < Quasi-Static Process quasi-static process (thermodynamics:: massless springs (mechanics or wires with no resistance (circuit 3.3 Work in Changing the Volume of a Hydrostatic System See Fig. 3-1 (quasi-static compression dw = F dx = P A dx, dv = A dx dw = P dv = W if = V f V i P dv (a quasi-static path i f i f, = W fi = V i V f P dv (a quasi-static path f i = W if # 13
14 14 CHAPTER 3. WORK 3.4 P V Diagram See Fig. 3-2 (a, (b, and (c. 3.5 Hydrastatic Work Depends on the Path See Fig. 3-3, i a f : W = 2P 0 V 0 i b f : W = P 0 V 0 i f : W = 3 2 P 0 V 0 = W is path-dependent. = W is not a state function. = W is an exact differential. 3.6 Calculation of P dv for Quasi-Static Processes Quasi-static isothermal expansion or compression of an ideal gas: = W = V f V i P dv, P V = nrt = V f V i nrt V dv = nrt V f V i dv V = nrt ln V f V i # Quasi-static isothermal increase of pressure on a solid: = W = P dv, dv = ( V P dp + ( V T T dt = κv dp P = P f P i κv P dp = κv P f P i P dp = κv 2 (P 2 f P 2 i #
15 3.7. WORK IN CHANGING THE LENGTH OF A WIRE Work in Changing the Length of a wire dw = F dl, F = F(L, T, = W = L f L i F dl# 3.8 Work in Changing the Area of a Surface Film dw = γ da, = W = A f A i γ da# 3.9 Work in Moving Charge with an Electrochemical Cell dw = E dz, = W = Z f Z i E dz# 3.10 Work in Changing the Total Polarization of a Dielectric Solid dw = E dp, = W = P f P i E dp # 3.11 Work in Changing the Total Magnetization of a Paramagnetic Solid dw = µ 0 H dm, = W = µ 0 Mf M i H dm#
16 16 CHAPTER 3. WORK 3.12 Generalized Work See Table 3.1 (Work of simple systems 3.13 Composite Systems See Figs. 3-8 & 3-9. In general, a five-coords. system (Y, X, Y, X, and T, = dw = Y dx + Y dx = Choose T, X, and X as indept coords.
17 17
18 18 CHAPTER 4. HEAT AND THE FIRST LAW OF THERMODYNAMICS Chapter 4 Heat and the First Law of Thermodynamics 4.1 Work and Heat 4.2 Adiabatic Work 4.3 Internal-Energy Function 4.4 Mathematical Formulation of the First Law 4.5 Concept of Heat 4.6 Difference Form of the Firat Law 4.7 Heat Capacity and its Measurement 4.8 Specific Heat of Water; the Calorie 4.9 Equation for a Hydrostatic System 4.10 Quasi-Static Flow of Heat; Heat Reservoir 4.11 Heat Conduction 4.12 Thermal Conductivity and its Measurement 4.13 Heat Convection 4.14 Thermal Radiation; Blackbody 4.15 Kirchhoff s Law; Radiation Heat 4.16 Stefan-Boltzmann Law
19 Chapter 5 Ideal Gas 5.1 Equation of State of a Gas 5.2 Internal Energy of a Real Gas 5.3 Ideal Gas 5.4 Experimental Determination of Heat Capacities 5.5 Quasi-Static Adiabatic Process 5.6 Rüchhardt s Method of Measuring γ 5.7 Velocity of a Logitudinal Wave 5.8 The Microscopic Point of View 5.9 Kinetic Theory of the Ideal Gas 19
20 20 CHAPTER 5. IDEAL GAS
21 21
22 22 CHAPTER 6. THE SECOND LAW OF THE THERMODYNAMICS Chapter 6 The Second Law of the Thermodynamics 6.1 Conversion of Work into Heat and Vice Versa 6.2 The Gasoline Engine 6.3 The Diesel Engine 6.4 The Steam Engine 6.5 The Stirling Engine 6.6 Heat Engine; Kelvin-Planck Statement of the Second Law 6.7 Refrigerator; Clausius Statement of the Second Law 6.8 Equivalence of the Kelvin-Planck and Clausius Statements 6.9 Reversibility and Irreversibility 6.10 External Mechanical Irreversibility 6.11 Internal Mechanical Irreversibility 6.12 External and Internal Thermal Irreversibility 6.13 Chemical Irreversibility 6.14 Conditions for Reversibility
23 Chapter 7 The Carnot Cycle and the Thermodynamic Temperature Scale 7.1 Carnot Cycle 7.2 Examples of Carnot Cycles 7.3 Carnot Refrigerator 7.4 Carnot s Theorem and Corollary 7.5 The Thermodynamic Temperature Scale 7.6 Absolute Zero and Carnot Efficiency 7.7 Equality of Ideal-Gas and Thermodynamic Temperatures 23
24 24CHAPTER 7. THE CARNOT CYCLE AND THE THERMODYNAMIC TEMPERATURE SCALE
25 Chapter 8 Entropy 8.1 Reversible Part of the Second Law 8.2 Entropy 8.3 Principle of Carathéodory 8.4 Entropy of the Ideal Gas 8.5 T S Diagram 8.6 Entropy and Reversibility 8.7 Entropy and Irreversibility 8.8 Irreversible Part of the Second Law 8.9 Heat and Entropy in Irreversible Processes 8.10 Entropy and Nonequilibrium States 8.11 Principle of Increase of Entropy 8.12 Application of the Entropy Principle 8.13 Entropy and Disorder 8.14 Exact Differentials 25
26 26 CHAPTER 8. ENTROPY
27 Chapter 9 Pure Substances 9.1 P V Diagram for a Pure Substance 9.2 P T Diagram for a Pure Substance; Phase Diagram 9.3 P V T Surface 9.4 Equation of State 9.5 Molar Heat Capacity at Constant Pressure 9.6 Volume Expansivity; Cubic Expansion Coefficient 9.7 Compressibility 9.8 Molar Heat Capacity at Constant Volume 9.9 T S Diagram for a Pure Substance 27
28 28 CHAPTER 9. PURE SUBSTANCES
29 Chapter 10 Mathematical Methods 10.1 Characteristic Functions 10.2 Enthalpy 10.3 Helmholtz and Gibbs Functions 10.4 Two Mathematical Theorems 10.5 Maxwell s Relations 10.6 T ds Equations 10.7 Internal-Energy Equations 10.8 Heat-Capacity Equations 29
30 30 CHAPTER 10. MATHEMATICAL METHODS
31 Chapter 11 Open Systems 11.1 Joule-Thomson Expansion 11.2 Liquefaction of Gases by the Joule-Thomson Expansion 11.3 First-Order Phase Transitions: Clausius-Clapeyron Equation 11.4 Clausius-Clapeyron Equation and Phase Diagrams 11.5 Clausius-Clapeyron Equation and the Carnot Engine 11.6 Chemical Potential 11.7 Open Hydrostatic Systems in Thermodynamic Equilibrium 31
32 32 CHAPTER 11. OPEN SYSTEMS
33 Chapter 12 Statistical Mechanics 12.1 Fundamental Principles 12.2 Equilibrium Distribution 12.3 Significance of Lagrangian Multipliers λ and β 12.4 Partition Function for Canonical Ensemble 12.5 Partition Function of an Ideal Monatomic Gas 12.6 Equipartition of Energy 12.7 Distribution of Speeds in an Ideal Monatomic Gas 12.8 Statistical Interpretation of Work and Heat 12.9 Entropy and Information 33
34 34 CHAPTER 12. STATISTICAL MECHANICS
35 Chapter 13 Thermal Properties of Solids 13.1 Statistical Mechanics of a Nonmetallic Crystal 13.2 Frequency Spectrum Crystals 13.3 Thermal Properties of Nonmetals 13.4 Thermal Properties of Metals 35
18.13 Review & Summary
5/2/10 10:04 PM Print this page 18.13 Review & Summary Temperature; Thermometers Temperature is an SI base quantity related to our sense of hot and cold. It is measured with a thermometer, which contains
fiziks Institute for NET/JRF, GATE, IIT-JAM, JEST, TIFR and GRE in PHYSICAL SCIENCES
Content-Thermodynamics & Statistical Mechanics 1. Kinetic theory of gases..(1-13) 1.1 Basic assumption of kinetic theory 1.1.1 Pressure exerted by a gas 1.2 Gas Law for Ideal gases: 1.2.1 Boyle s Law 1.2.2
Introduction. Statistical physics: microscopic foundation of thermodynamics degrees of freedom 2 3 state variables!
Introduction Thermodynamics: phenomenological description of equilibrium bulk properties of matter in terms of only a few state variables and thermodynamical laws. Statistical physics: microscopic foundation
1. Thermodynamics 1.1. A macroscopic view of matter
1. Thermodynamics 1.1. A macroscopic view of matter Intensive: independent of the amount of substance, e.g. temperature,pressure. Extensive: depends on the amount of substance, e.g. internal energy, enthalpy.
Chemistry. Lecture 10 Maxwell Relations. NC State University
Chemistry Lecture 10 Maxwell Relations NC State University Thermodynamic state functions expressed in differential form We have seen that the internal energy is conserved and depends on mechanical (dw)
MACMILLAN PHYSICAL SCIENCE
Thermal physics MACMILLAN PHYSICAL SCIENCE Series advisers Physics titles: Dr R L Havill, University of Sheffield Dr A K Walton, University of Sheffield Chemistry titles: Dr D M Adams, University of Leicester
Thermodynamics 2013/2014, lecturer: Martin Zápotocký
Thermodynamics 2013/2014, lecturer: Martin Zápotocký 2 lectures: 1. Thermodynamic processes, heat and work, calorimetry, 1 st and 2 nd law of thermodynamics 2. Entropy, thermodynamic potentials, nonequilibrium
Thermodynamics. 1.1 Introduction. Thermodynamics is a phenomenological description of properties of macroscopic systems in thermal equilibrium.
1 hermodynamics 1.1 Introduction hermodynamics is a phenomenological description of properties of macroscopic systems in thermal equilibrium. Imagine yourself as a post-newtonian physicist intent on understanding
Table of Contents [ttc]
![Table of Contents [ttc]](/thumbs/89/97960614.jpg "Table of Contents [ttc]")
Table of Contents [ttc] 1. Equilibrium Thermodynamics I: Introduction Thermodynamics overview. [tln2] Preliminary list of state variables. [tln1] Physical constants. [tsl47] Equations of state. [tln78]
5.60 Thermodynamics & Kinetics Spring 2008
MIT OpenCourseWare http://ocw.mit.edu 5.60 Thermodynamics & Kinetics Spring 2008 For information about citing these materials or our Terms of Use, visit: http://ocw.mit.edu/terms. 5.60 Spring 2008 Lecture
Thermodynamics 2018/2019, lecturer: Martin Zápotocký
Thermodynamics 2018/2019, lecturer: Martin Zápotocký 2 lectures: 1. Thermodynamic processes, heat and work, calorimetry, 1 st and 2 nd law of thermodynamics 2. Entropy, thermodynamic potentials, nonequilibrium
Thermodynamic system is classified into the following three systems. (ii) Closed System It exchanges only energy (not matter) with surroundings.
1 P a g e The branch of physics which deals with the study of transformation of heat energy into other forms of energy and vice-versa. A thermodynamical system is said to be in thermal equilibrium when
UNIVERSITY OF SOUTHAMPTON
UNIVERSITY OF SOUTHAMPTON PHYS1013W1 SEMESTER 2 EXAMINATION 2014-2015 ENERGY AND MATTER Duration: 120 MINS (2 hours) This paper contains 8 questions. Answers to Section A and Section B must be in separate
Physics 53. Thermal Physics 1. Statistics are like a bikini. What they reveal is suggestive; what they conceal is vital.
Physics 53 Thermal Physics 1 Statistics are like a bikini. What they reveal is suggestive; what they conceal is vital. Arthur Koestler Overview In the following sections we will treat macroscopic systems
Part II Statistical Physics
Part II Statistical Physics Theorems Based on lectures by H. S. Reall Notes taken by Dexter Chua Lent 2017 These notes are not endorsed by the lecturers, and I have modified them (often significantly)
01. Equilibrium Thermodynamics I: Introduction
University of Rhode Island DigitalCommons@URI Equilibrium Statistical Physics Physics Course Materials 2015 01. Equilibrium Thermodynamics I: Introduction Gerhard Müller University of Rhode Island, gmuller@uri.edu
Chapter 18 Temperature, Heat, and the First Law of Thermodynamics. Thermodynamics and Statistical Physics
Chapter 18 Temperature, Heat, and the First Law of Thermodynamics Thermodynamics and Statistical Physics Key contents: Temperature scales Thermal expansion Temperature and heat, specific heat Heat and
Thermodynamics & Statistical Mechanics SCQF Level 9, U03272, PHY-3-ThermStat. Thursday 24th April, a.m p.m.
College of Science and Engineering School of Physics H T O F E E U D N I I N V E B R U S I R T Y H G Thermodynamics & Statistical Mechanics SCQF Level 9, U03272, PHY-3-ThermStat Thursday 24th April, 2008
CHEMICAL ENGINEERING THERMODYNAMICS. Andrew S. Rosen
CHEMICAL ENGINEERING THERMODYNAMICS Andrew S. Rosen SYMBOL DICTIONARY 1 TABLE OF CONTENTS Symbol Dictionary... 3 1. Measured Thermodynamic Properties and Other Basic Concepts... 5 1.1 Preliminary Concepts
THERMODYNAMICS CONTENTS
1. Introduction HERMODYNAMICS CONENS. Maxwell s thermodynamic equations.1 Derivation of Maxwell s equations 3. Function and derivative 3.1 Differentiation 4. Cyclic Rule artial Differentiation 5. State
Unit 7 (B) Solid state Physics
Unit 7 (B) Solid state Physics hermal Properties of solids: Zeroth law of hermodynamics: If two bodies A and B are each separated in thermal equilibrium with the third body C, then A and B are also in
Thermodynamics of solids 5. Unary systems. Kwangheon Park Kyung Hee University Department of Nuclear Engineering
Thermodynamics of solids 5. Unary systems Kwangheon ark Kyung Hee University Department of Nuclear Engineering 5.1. Unary heterogeneous system definition Unary system: one component system. Unary heterogeneous
More Thermodynamics. Specific Specific Heats of a Gas Equipartition of Energy Reversible and Irreversible Processes
More Thermodynamics Specific Specific Heats of a Gas Equipartition of Energy Reversible and Irreversible Processes Carnot Cycle Efficiency of Engines Entropy More Thermodynamics 1 Specific Heat of Gases
Module 5 : Electrochemistry Lecture 21 : Review Of Thermodynamics
Module 5 : Electrochemistry Lecture 21 : Review Of Thermodynamics Objectives In this Lecture you will learn the following The need for studying thermodynamics to understand chemical and biological processes.
Temperature Thermal Expansion Ideal Gas Law Kinetic Theory Heat Heat Transfer Phase Changes Specific Heat Calorimetry Heat Engines
Temperature Thermal Expansion Ideal Gas Law Kinetic Theory Heat Heat Transfer Phase Changes Specific Heat Calorimetry Heat Engines Zeroeth Law Two systems individually in thermal equilibrium with a third
Atkins / Paula Physical Chemistry, 8th Edition. Chapter 3. The Second Law
Atkins / Paula Physical Chemistry, 8th Edition Chapter 3. The Second Law The direction of spontaneous change 3.1 The dispersal of energy 3.2 Entropy 3.3 Entropy changes accompanying specific processes
Chemical Engineering Thermodynamics
Chemical Engineering Thermodynamics P Liquid P x 1 sat P 1 T sat T 2 T x 1 T x 1 T y 1 Liquid Vapour sat P 2 P x 1 P y 1 P y 1 Vapour sat T 1 x, y 1 1 x, y 1 1 Pradeep Ahuja Contents CHEMICAL ENGINEERING
General Physics I. Lecture 23: Basic Concepts of Thermodynamics
General Physics I Lecture 23: Basic Concepts of Thermodynamics Prof. WAN, Xin xinwan@zju.edu.cn http://zimp.zju.edu.cn/~xinwan/ Temperature [Operational definition] Temperature is what you measure with
Thermodynamics! for Environmentology!
1 Thermodynamics! for Environmentology! Thermodynamics and kinetics of natural systems Susumu Fukatsu! Applied Quantum Physics Group! The University of Tokyo, Komaba Graduate School of Arts and Sciences
Chapter 3. The Second Law Fall Semester Physical Chemistry 1 (CHM2201)
Chapter 3. The Second Law 2011 Fall Semester Physical Chemistry 1 (CHM2201) Contents The direction of spontaneous change 3.1 The dispersal of energy 3.2 The entropy 3.3 Entropy changes accompanying specific
Chapter 1 Introduction and Basic Concepts
Chapter 1 Introduction and Basic Concepts 1-1 Thermodynamics and Energy Application Areas of Thermodynamics 1-2 Importance of Dimensions and Units Some SI and English Units Dimensional Homogeneity Unity
Introduction to Chemical Thermodynamics. D. E. Manolopoulos First Year (13 Lectures) Michaelmas Term
Introduction to Chemical Thermodynamics D. E. Manolopoulos First Year (13 Lectures) Michaelmas Term Lecture Synopsis 1. Introduction & Background. Le Chatelier s Principle. Equations of state. Systems
Chapter 2 Carnot Principle
Chapter 2 Carnot Principle 2.1 Temperature 2.1.1 Isothermal Process When two bodies are placed in thermal contact, the hotter body gives off heat to the colder body. As long as the temperatures are different,
(Heat capacity c is also called specific heat) this means that the heat capacity number c for water is 1 calorie/gram-k.
Lecture 23: Ideal Gas Law and The First Law of Thermodynamics 1 (REVIEW) Chapter 17: Heat Transfer Origin of the calorie unit A few hundred years ago when people were investigating heat and temperature
Chapter 1. The Properties of Gases Fall Semester Physical Chemistry 1 (CHM2201)
Chapter 1. The Properties of Gases 2011 Fall Semester Physical Chemistry 1 (CHM2201) Contents The Perfect Gas 1.1 The states of gases 1.2 The gas laws Real Gases 1.3 Molecular interactions 1.4 The van
S = S(f) S(i) dq rev /T. ds = dq rev /T
In 1855, Clausius proved the following (it is actually a corollary to Clausius Theorem ): If a system changes between two equilibrium states, i and f, the integral dq rev /T is the same for any reversible
UBMCC11 - THERMODYNAMICS. B.E (Marine Engineering) B 16 BASIC CONCEPTS AND FIRST LAW PART- A
UBMCC11 - THERMODYNAMICS B.E (Marine Engineering) B 16 UNIT I BASIC CONCEPTS AND FIRST LAW PART- A 1. What do you understand by pure substance? 2. Define thermodynamic system. 3. Name the different types
R13. II B. Tech I Semester Regular Examinations, Jan THERMODYNAMICS (Com. to ME, AE, AME) PART- A
SET - 1 II B. Tech I Semester Regular Examinations, Jan - 2015 THERMODYNAMICS (Com. to ME, AE, AME) Time: 3 hours Max. Marks: 70 Note 1. Question Paper consists of two parts (Part-A and Part-B) 2. Answer
Fundamentals. Statistical. and. thermal physics. McGRAW-HILL BOOK COMPANY. F. REIF Professor of Physics Universüy of California, Berkeley
Fundamentals of and Statistical thermal physics F. REIF Professor of Physics Universüy of California, Berkeley McGRAW-HILL BOOK COMPANY Auckland Bogota Guatemala Hamburg Lisbon London Madrid Mexico New
INDEX 481. Joule-Thomson process, 86, 433. Kosterlitz-Thouless transition, 467
Index accessible microstates, 173 183, 185, 196, 200, 201 additive random process, 146 adiabatic demagnetization, 235 expansion, 52, 61 process, 43 quasistatic, 49, 50 wall, 34 anharmonic oscillator, 349
UNIVERSITY OF SOUTHAMPTON
UNIVERSITY OF SOUTHAMPTON PHYS1013W1 SEMESTER 2 EXAMINATION 2014-2015 ENERGY AND MATTER Duration: 120 MINS (2 hours) This paper contains 8 questions. Answers to Section A and Section B must be in separate
THERMODYNAMICS SSC-JE STAFF SELECTION COMMISSION MECHANICAL ENGINEERING STUDY MATERIAL THERMODYNAMICS THERMODYNAMICS THERMODYNAMICS
1 SSC-JE STAFF SELECTION COMMISSION MECHANICAL ENGINEERING STUDY MATERIAL 2 Syllabus: Thermal Engineering (Thermodynamics) Properties of Pure Substances : p-v & P-T diagrams of pure substance like H 2
MME 2010 METALLURGICAL THERMODYNAMICS II. Fundamentals of Thermodynamics for Systems of Constant Composition
MME 2010 METALLURGICAL THERMODYNAMICS II Fundamentals of Thermodynamics for Systems of Constant Composition Thermodynamics addresses two types of problems: 1- Computation of energy difference between two
CHEM 231. Physical Chemistry I NJIT Fall Semester, Prerequisites: Chem 126 or 123, Phys 111 Co requisite: Math 211
CHEM 231 Physical Chemistry I NJIT Fall Semester, 2017 Prerequisites: Chem 126 or 123, Phys 111 Co requisite: Math 211 Textbook: Chapters to be covered: Instructor: Goals: Prerequisites: Course Outline:
Lecture 44: Review Thermodynamics I
ME 00 Thermodynamics I Lecture 44: Review Thermodynamics I Yong Li Shanghai Jiao Tong University Institute of Refrigeration and Cryogenics 800 Dong Chuan Road Shanghai, 0040, P. R. China Email : liyo@sjtu.edu.cn
Thermodynamics B Test
Northern Regional: January 19 th, 2019 Thermodynamics B Test Name(s): Team Name: School Name: Team Number: Rank: Score: Science Olympiad North Florida Regional at the University of Florida Thermodynamics
Part1B(Advanced Physics) Statistical Physics
PartB(Advanced Physics) Statistical Physics Course Overview: 6 Lectures: uesday, hursday only 2 problem sheets, Lecture overheads + handouts. Lent erm (mainly): Brief review of Classical hermodynamics:
Suggestions for Further Reading
Contents Preface viii 1 From Microscopic to Macroscopic Behavior 1 1.1 Introduction........................................ 1 1.2 Some Qualitative Observations............................. 2 1.3 Doing
Outline Review Example Problem 1. Thermodynamics. Review and Example Problems: Part-2. X Bai. SDSMT, Physics. Fall 2014
Review and Example Problems: Part- SDSMT, Physics Fall 014 1 Review Example Problem 1 Exponents of phase transformation : contents 1 Basic Concepts: Temperature, Work, Energy, Thermal systems, Ideal Gas,
THERMODYNAMICS THERMOSTATISTICS AND AN INTRODUCTION TO SECOND EDITION. University of Pennsylvania
THERMODYNAMICS AND AN INTRODUCTION TO THERMOSTATISTICS SECOND EDITION HERBERT B. University of Pennsylvania CALLEN JOHN WILEY & SONS New York Chichester Brisbane Toronto Singapore CONTENTS PART I GENERAL
Basic Thermodynamics
Basic Thermodynamics Ramesh.K 2/08/2012 1 Syllabus Subject BASIC THERMODYNAMICS Sub. Code 09 ME 3DC BTD Credits 04 L-T-P 3-1-0 1. Introduction: History of Thermodynamics, Macroscopic V/s Microscopic View
Test Exchange Thermodynamics (C) Test Answer Key
1 Test Exchange Thermodynamics (C) Test Answer Key Made by Montgomery High School montyscioly@gmail.com 2 Questions are worth between 1 to 3 points. Show calculations for all open-ended math questions
Chapter 20 Entropy and the 2nd Law of Thermodynamics
Chapter 20 Entropy and the 2nd Law of Thermodynamics A one-way processes are processes that can occur only in a certain sequence and never in the reverse sequence, like time. these one-way processes are
Introduction to thermodynamics
Chapter 6 Introduction to thermodynamics Topics First law of thermodynamics Definitions of internal energy and work done, leading to du = dq + dw Heat capacities, C p = C V + R Reversible and irreversible
PY2005: Thermodynamics
ome Multivariate Calculus Y2005: hermodynamics Notes by Chris Blair hese notes cover the enior Freshman course given by Dr. Graham Cross in Michaelmas erm 2007, except for lecture 12 on phase changes.
Part III: Planes, Trains, and Automobiles: Making Heat Work for You
Contents at a Glance Introduction... 1 Part I: Covering the Basics in Thermodynamics... 7 Chapter 1: Thermodynamics in Everyday Life...9 Chapter 2: Laying the Foundation of Thermodynamics...15 Chapter
The Second Law of Thermodynamics (Chapter 4)
The Second Law of Thermodynamics (Chapter 4) First Law: Energy of universe is constant: ΔE system = - ΔE surroundings Second Law: New variable, S, entropy. Changes in S, ΔS, tell us which processes made
dv = adx, where a is the active area of the piston. In equilibrium, the external force F is related to pressure P as
Chapter 3 Work, heat and the first law of thermodynamics 3.1 Mechanical work Mechanical work is defined as an energy transfer to the system through the change of an external parameter. Work is the only
Outline Review Example Problem 1 Example Problem 2. Thermodynamics. Review and Example Problems. X Bai. SDSMT, Physics. Fall 2013
Review and Example Problems SDSMT, Physics Fall 013 1 Review Example Problem 1 Exponents of phase transformation 3 Example Problem Application of Thermodynamic Identity : contents 1 Basic Concepts: Temperature,
THE SECOND LAW OF THERMODYNAMICS. Professor Benjamin G. Levine CEM 182H Lecture 5
THE SECOND LAW OF THERMODYNAMICS Professor Benjamin G. Levine CEM 182H Lecture 5 Chemical Equilibrium N 2 + 3 H 2 2 NH 3 Chemical reactions go in both directions Systems started from any initial state
ME6301- ENGINEERING THERMODYNAMICS UNIT I BASIC CONCEPT AND FIRST LAW PART-A
ME6301- ENGINEERING THERMODYNAMICS UNIT I BASIC CONCEPT AND FIRST LAW PART-A 1. What is meant by thermodynamics system? (A/M 2006) Thermodynamics system is defined as any space or matter or group of matter
Introduction to Chemical Thermodynamics. (10 Lectures) Michaelmas Term
Introduction to Chemical Thermodynamics Dr. D. E. Manolopoulos First Year (0 Lectures) Michaelmas Term Lecture Synopsis. Introduction & Background. Le Chatelier s Principle. Equations of state. Systems
Engineering Thermodynamics
Basic Engineering Thermodynamics A Venkatesh Professor Emeritus, Mechanical Engineering Department East West Institute of Technology, Bangalore, India (Formerly Professor of Mechanical Engineering, IIT
3. First Law of Thermodynamics and Energy Equation
3. First Law of Thermodynamics and Energy Equation 3. The First Law of Thermodynamics for a ontrol Mass Undergoing a ycle The first law for a control mass undergoing a cycle can be written as Q W Q net(cycle)
2. Under conditions of constant pressure and entropy, what thermodynamic state function reaches an extremum? i
1. (20 oints) For each statement or question in the left column, find the appropriate response in the right column and place the letter of the response in the blank line provided in the left column. 1.
EQUILIBRIUM IN CHEMICAL REACTIONS
EQUILIBRIUM IN CHEMICAL REACTIONS CHAPTER 12 Thermodynamic Processes and Thermochemistry CHAPTER 13 Spontaneous Processes and Thermodynamic Equilibrium CHAPTER 14 Chemical Equilibrium CHAPTER 15 Acid-Base
Final Examination. Multiple Choice Questions. 1. The Virial expansion of the Compressibility Factor for a van der Waals gas is:
CHEM 331 Physical Chemistry I Fall 2013 Name: Final Examination Multiple Choice Questions 1. The Virial expansion of the Compressibility Factor for a van der Waals gas is: Z = 1 + + The Boyle Temperature
MAHALAKSHMI ENGINEERING COLLEGE
MAHALAKSHMI ENGINEERING COLLEGE TIRUCHIRAPALLI 621 213. Department: Mechanical Subject Code: ME2202 Semester: III Subject Name: ENGG. THERMODYNAMICS UNIT-I Basic Concept and First Law 1. What do you understand
Chapter 7. Entropy. by Asst.Prof. Dr.Woranee Paengjuntuek and Asst. Prof. Dr.Worarattana Pattaraprakorn
Chapter 7 Entropy by Asst.Prof. Dr.Woranee Paengjuntuek and Asst. Prof. Dr.Worarattana Pattaraprakorn Reference: Cengel, Yunus A. and Michael A. Boles, Thermodynamics: An Engineering Approach, 5th ed.,
Part I. Temperature Measurements in the Range from 0.1 K to 300 K
Part I Temperature Measurements in the Range from 0.1 K to 300 K Introduction Part I describes modem methods for measuring temperatures lower than O C based on the use of substances that are gaseous at
Thermodynamics. Basic concepts. Thermal equilibrium and temperature
hermodynamics Basic concepts hermodynamics is a phenomenological description of macroscopic systems with many degrees of freedom. Its microscopic justication is provided by statistical mechanics. Equilibrium
CHAPTER 3 LECTURE NOTES 3.1. The Carnot Cycle Consider the following reversible cyclic process involving one mole of an ideal gas:
CHATER 3 LECTURE NOTES 3.1. The Carnot Cycle Consider the following reversible cyclic process involving one mole of an ideal gas: Fig. 3. (a) Isothermal expansion from ( 1, 1,T h ) to (,,T h ), (b) Adiabatic
Physics 115. Specific heats revisited Entropy. General Physics II. Session 13
Physics 115 General Physics II Session 13 Specific heats revisited Entropy R. J. Wilkes Email: phy115a@u.washington.edu Home page: http://courses.washington.edu/phy115a/ 4/22/14 Physics 115 1 Lecture Schedule
Physics 123 Thermodynamics Review
Physics 3 Thermodynamics Review I. Definitions & Facts thermal equilibrium ideal gas thermal energy internal energy heat flow heat capacity specific heat heat of fusion heat of vaporization phase change
Stuff. ---Tonight: Lecture 3 July Assignment 1 has been posted. ---Presentation Assignment on Friday.
Stuff ---Tonight: Lecture 3 July 0 ---Assignment 1 has been posted. Work from gravitational forces: h F gravity dx = h 0 0 mgh mg dx Where m (kg) and g is gravitational constant 9.8 m/s ---Presentation
P(N,V,T) = NRT V. = P(N,V,T) dv
CHEM-443, Fall 2016, Section 010 Student Name Quiz 1 09/09/2016 Directions: Please answer each question to the best of your ability. Make sure your response is legible, precise, includes relevant dimensional
Basic Thermodynamics Module 1
Basic Thermodynamics Module 1 Lecture 1: Introduction Introduction The most of general sense of thermodynamics is the study of energy and its relationship to the properties of matter. All activities in
Chapter 20. Heat Engines, Entropy and the Second Law of Thermodynamics. Dr. Armen Kocharian
Chapter 20 Heat Engines, Entropy and the Second Law of Thermodynamics Dr. Armen Kocharian First Law of Thermodynamics Review Review: The first law states that a change in internal energy in a system can
Version 001 HW 15 Thermodynamics C&J sizemore (21301jtsizemore) 1
Version 001 HW 15 Thermodynamics C&J sizemore 21301jtsizemore 1 This print-out should have 38 questions. Multiple-choice questions may continue on the next column or page find all choices before answering.
Concentrating on the system
Concentrating on the system Entropy is the basic concept for discussing the direction of natural change, but to use it we have to analyze changes in both the system and its surroundings. We have seen that
Chapter One Reviews of Thermodynamics Update on 2013/9/13
Chapter One Reviews of Thermodynamics Update on 2013/9/13 (1.1). Thermodynamic system An isolated system is a system that exchanges neither mass nor energy with its environment. An insulated rigid tank
Thermal & Statistical Physics Study Questions for the Spring 2018 Department Exam December 6, 2017
Thermal & Statistical Physics Study Questions for the Spring 018 Department Exam December 6, 017 1. a. Define the chemical potential. Show that two systems are in diffusive equilibrium if 1. You may start
CHAPTER 4 Physical Transformations of Pure Substances.
I. Generalities. CHAPTER 4 Physical Transformations of Pure Substances. A. Definitions: 1. A phase of a substance is a form of matter that is uniform throughout in chemical composition and physical state.
Last Name or Student ID
10/06/08, Chem433 Exam # 1 Last Name or Student ID 1. (3 pts) 2. (3 pts) 3. (3 pts) 4. (2 pts) 5. (2 pts) 6. (2 pts) 7. (2 pts) 8. (2 pts) 9. (6 pts) 10. (5 pts) 11. (6 pts) 12. (12 pts) 13. (22 pts) 14.
1 mol ideal gas, PV=RT, show the entropy can be written as! S = C v. lnt + RlnV + cons tant
1 mol ideal gas, PV=RT, show the entropy can be written as! S = C v lnt + RlnV + cons tant (1) p, V, T change Reversible isothermal process (const. T) TdS=du-!W"!S = # "Q r = Q r T T Q r = $W = # pdv =
Statistical Mechanics
Franz Schwabl Statistical Mechanics Translated by William Brewer Second Edition With 202 Figures, 26 Tables, and 195 Problems 4u Springer Table of Contents 1. Basic Principles 1 1.1 Introduction 1 1.2
Fig Note the three different types of systems based on the type of boundary between system and surroundings.
CHAPTER 1 LECTURE NOTES System, Surroundings, and States Fig. 1.4 Note the three different types of systems based on the type of boundary between system and surroundings. Intensive and Extensive Properties
Thermodynamics of phase transitions
Thermodynamics of phase transitions Katarzyna Sznajd-Weron Department of Theoretical of Physics Wroc law University of Science and Technology, Poland March 12, 2017 Katarzyna Sznajd-Weron (WUST) Thermodynamics
Lecture 2: Zero law of thermodynamics
Lecture 2: Zero law of thermodynamics 1. Thermometers and temperature scales 2. Thermal contact and thermal equilibrium 3. Zeroth law of thermodynamics 1. Thermometers and Temperature scales We often associate
Physical Chemistry Physical chemistry is the branch of chemistry that establishes and develops the principles of Chemistry in terms of the underlying concepts of Physics Physical Chemistry Main book: Atkins
Physics 4230 Final Examination 10 May 2007
Physics 43 Final Examination May 7 In each problem, be sure to give the reasoning for your answer and define any variables you create. If you use a general formula, state that formula clearly before manipulating
Reversible Processes. Furthermore, there must be no friction (i.e. mechanical energy loss) or turbulence i.e. it must be infinitely slow.
Reversible Processes A reversible thermodynamic process is one in which the universe (i.e. the system and its surroundings) can be returned to their initial conditions. Because heat only flows spontaneously
Chap. 3 The Second Law. Spontaneous change
Chap. 3 The Second Law Spontaneous change Some things happen naturally; some things don t. the spontaneous direction of change, the direction of change that does not require work to be done to bring it
II/IV B.Tech (Regular) DEGREE EXAMINATION. (1X12 = 12 Marks) Answer ONE question from each unit.
Page 1 of 8 Hall Ticket Number: 14CH 404 II/IV B.Tech (Regular) DEGREE EXAMINATION June, 2016 Chemical Engineering Fourth Semester Engineering Thermodynamics Time: Three Hours Maximum : 60 Marks Answer
CHEMISTRY DEPARTMENT, PORTLAND STATE UNIVERSITY
CHEMISTRY DEPARTMENT, PORTLAND STATE UNIVERSITY CHEMISTRY 440/540, PHYSICAL CHEMISTRY. FALL, 2014 Venue: CR 250 Instructor: R. H. Simoyi (SB2 372) Syllabus: The chapters and page numbers referred to in
Lecture Ch. 2a. Lord Kelvin (a.k.a William Thomson) James P. Joule. Other Kinds of Energy What is the difference between E and U? Exact Differentials
Lecture Ch. a Energy and heat capacity State functions or exact differentials Internal energy vs. enthalpy st Law of thermodynamics Relate heat, work, energy Heat/work cycles (and path integrals) Energy
Section 3 Entropy and Classical Thermodynamics
Section 3 Entropy and Classical Thermodynamics 3.1 Entropy in thermodynamics and statistical mechanics 3.1.1 The Second Law of Thermodynamics There are various statements of the second law of thermodynamics.
Chapter 6 Thermodynamic Properties of Fluids
Chapter 6 Thermodynamic Properties of Fluids Initial purpose in this chapter is to develop from the first and second laws the fundamental property relations which underlie the mathematical structure of
Dr.Salwa Alsaleh fac.ksu.edu.sa/salwams
Dr.Salwa Alsaleh Salwams@ksu.edu.sa fac.ksu.edu.sa/salwams What is Temperature? It is the measurement of the AVERAGE kinetic energy of the particles of matter. Temperature We associate the concept of temperature
Chapter 18. Temperature, Heat, and the First Law of Thermodynamics Temperature
Chapter 18 Temperature, Heat, and the First Law of Thermodynamics 18.2 Temperature 18.3: The Zeroth aw of Thermodynamics If bodies A and B are each in thermal equilibrium with a third body T, then A and