The Advanced Chemical Engineering Thermodynamics. The thermodynamics properties of fluids (II) Ji-Sheng Chang Q&A_-10-11/17/2005(10)
|
|
|
- Norman Mitchell
- 5 years ago
- Views:
Transcription
1 The Advanced Chemical Engineering Thermodynamics The thermodynamics properties of fluids (II) Q&A_-10-11/17/2005(10) Ji-Sheng Chang
2 Property relations The residual Gibbs free energy The definition of residual properties M R (T,P) = M(T,P) - M IG (T,P) R: Residual property IG : Ideal gas behavior property M R (T,P) = M(T,P) - M IG (T,P), M are the properties as V, G, H, S,
3 Property relations The residual properties V R (T,P) = V(T,P) - V IG (T,P) = V - RT/P; Basic thermodynamics relationship for calculations G R (T,P) = G(T,P) - G IG (T,P); More important in traditional Chemical Engineering Thermodynamics H R (T,P) = H(T,P) - H IG (T,P)
4 Property relations Deriving the residual properties in terms of the PVT properties. From the generating function of Gibbs free energy, V R /RT= [ (G R /RT)/ P] T, Then d(g R /RT) = (V R /RT)dP, to integrate from P=0 to P at constant T.
5 Property relations The integrated result in terms of PVT property as the formula (6.45) R G RT = P 0 ( V RT 1 ) dp, P (constant T) G R RT = P 0 ( Z 1) dp, P (constant T)
6 Property relations The residual enthalpy, H R /RT= - T [ (G R /RT)/ T]P, The integrated result in terms of PVT property as the formula (6.46) R H RT = T 0 P Z T P dp P, (constant T)
7 Property relations In previous section S = H/T - G/T, then the residual entropy S R /R = H R /RT - G R /RT The result in terms of PVT property as the formula (6.48) S R RT = T Z dp P P 0 T 0 P P ( Z 1) dp, P (constant T)
8 Property relations Using the independent property of T and V More commonly as the form P=P(V,T) of the PVT equations of state, especially the cubic equations of state. P = ZRT/V, P = ZρRT; as ρ = 1/V dp=rtd(zρ)=rt(zdρ+ρdz) at constant T
9 Property relations G R RT dp/p=dρ/ρ+dz/z, as the formula (6.58) G R RT dp ( Z 1), 0 P = P d = ρ ρ ( Z 1) + Z 0 ρ 1 the alternative form. (constant T) lnz, (constant T) G R V RT = dv ( Z 1) + Z 1 lnz, V (constant T)
10 Property relations Calculating the residual properties The PVT data, Using graphical integration method to calculate the residual Gibbs free energy from steam data. R G RT = 1 P Z dp, 0 P (constant T)
11 Phase diagram PT phase diagram of water 2. The Solid/Liquid equilibrium curve for water for most component 300 P/bar PC,TC 200 O C path Solid Liquid Gas Critical properties PC= bar T/K TC=647.1 K TTri= K
12 Vapor/Liquid equilibrium curve The Antoine equation The constant of Antoine equation for water A= B= C= ln P sat /kpa = A B T/ C+ C
13 Property Critical properties of water PC= bar TC=647.1 K PTri=0.611 kpa TTri= K Tn= K at P= bar = 1 atm
14 Property relations Problems Calculate the residual Gibbs energy of the 200 C superheat steam at 10 bar, using the PVT data from steam tables
15 Properties P/kPa P/bar V/cm 3 g -1 V/cm 3 mol -1 Z (Z-1)/P
16 Properties P/kPa P/bar V/cm 3 g -1 V/cm 3 mol -1 Z (Z-1)/P
17 Residual Gibbs free energy properties G R /RT of superheat steam 200 O C (Z -1)/P [ bar -1 ] P [ bar ]
18 Example 1 Calculating the residual properties The PVT equations of state Using the two term virial equation of states, estimate the molar volume, residual enthalpy, residual entropy, and residual Gibbs free energy of the carbon dioxide at the states of temperature of 25 C and pressure of 1 bar.
19 Deriving the formulas The equations of residual Gibbs free energy Three type of the two term virial equation The residual Gibbs free energy for a gas at each P and T
20 Deriving the formulas Second virial coefficient From PVT data From generalized correlation equations Based molecular thermodynamic, it is integrated from potential function
21 Example 2 Calculating the residual properties The PVT equations of state Using the two term virial equation of states, estimate the molar volume, residual enthalpy, residual entropy, and residual Gibbs free energy of the methane at the states of temperature of 25 C and pressure of 1 bar.
22 Example 3 Calculating the residual properties The PVT equations of state (?) Using the two term virial equation of states, estimate the molar volume, residual enthalpy, residual entropy, and residual Gibbs free energy of the benzene at the states of temperature of 25 C and pressure of 1 bar.
23 Theorem of corresponding states Two-parameter theorem of corresponding states Given T and P Finding Tc, Pc Calculate Tr, Pr Using Tr, Pr to finding the reduced properties from Table E.1 to E.16
24 Theorem of corresponding states Three-parameter theorem of corresponding states Given T and P Finding Tc, Pc, ω Calculate Tr, Pr Using Tr, Pr, ω to finding the reduced properties from Table E.1 to E.16
25 Theorem of corresponding states Based on the corresponding states principles The Lee/Kesler generalized correlation tables, Appendix E at text books of pages from 695 to 711. The properties of some pure species tables, Appendix B at text books of pages from 679 to 682.
26 Example 4 Application of the theorem of corresponding states to estimate the thermodynamics properties of the pure components. At temperature of 25 C and pressure of 1 bar, estimate the molar volume, residual enthalpy, residual entropy, and residual Gibbs free energy of the carbon dioxide.
27 Example 5 Application of the theorem of corresponding states to estimate the thermodynamics properties of the pure components. At temperature of 25 C and pressure of 1 bar, estimate the molar volume, residual enthalpy, residual entropy, and residual Gibbs free energy of the methane.
28 Example 6 Application of the theorem of corresponding states to estimate the thermodynamics properties of the pure components. (?) At temperature of 25 C and pressure of 1 bar, estimate the molar volume, residual enthalpy, residual entropy, and residual Gibbs free energy of the benzene.
ChBE BIBLE. Robert A. Pinnick. 28 April 2006
ChBE BIBLE Robert A. Pinnick 28 April 2006 Contents 1 Thermodynamics 2 1.1 Equations of State....................................... 2 1.1.1 Ideal Gas Law..................................... 3 1.1.2 Cubic
Thermodynamic ProperDes for Fluids
SKF2213: CHEMICAL ENGINEERING THERMODYNAMICS Thermodynamic roperdes for Fluids Mohammad Fadil Abdul Wahab ObjecDves To develop fundamental property relations (FR) of U,H,S,G,A,V,,T from 1st and 2nd Law
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
ln( P vap(s) / torr) = T / K ln( P vap(l) / torr) = T / K
Chem 4501 Introduction to Thermodynamics, 3 Credits Kinetics, and Statistical Mechanics Fall Semester 2017 Homework Problem Set Number 9 Solutions 1. McQuarrie and Simon, 9-4. Paraphrase: Given expressions
Phase Diagrams. NC State University
Chemistry 433 Lecture 18 Phase Diagrams NC State University Definition of a phase diagram A phase diagram is a representation of the states of matter, solid, liquid, or gas as a function of temperature
For an incompressible β and k = 0, Equations (6.28) and (6.29) become:
Internal Energy and Entropy as Functions of T and V These are general equations relating the internal energy and entropy of homogeneous fluids of constant composition to temperature and volume. Equation
Fuel, Air, and Combustion Thermodynamics
Chapter 3 Fuel, Air, and Combustion Thermodynamics 3.1) What is the molecular weight, enthalpy (kj/kg), and entropy (kj/kg K) of a gas mixture at P = 1000 kpa and T = 500 K, if the mixture contains the
Potential Concept Questions
Potential Concept Questions Phase Diagrams Equations of State Reversible Processes Molecular Basis of Heat Capacity State Functions & Variables Temperature Joules Experiment for conversion of one form
Thermodynamic Properties
Thermodynamic Properties (TP) Thermodynamic Properties Define and articulate some of the critical language and concepts of Thermodynamics Distinguish between the universe, system, surroundings, and boundary
HOMOGENEOUS CLOSED SYSTEM
CHAE II A closed system is one that does not exchange matter with its surroundings, although it may exchange energy. W n in = 0 HOMOGENEOUS CLOSED SYSEM System n out = 0 Q dn i = 0 (2.1) i = 1, 2, 3,...
3.012 PS 7 Thermo solutions Issued: Fall 2003 Graded problems due:
3.012 PS 7 Thermo solutions 3.012 Issued: 11.17.03 Fall 2003 Graded problems due: 11.26.03 Graded problems: 1. Analysis of equilibrium phases with a binary phase diagram. Shown below is the phase diagram
We can see from the gas phase form of the equilibrium constant that pressure of species depend on pressure. For the general gas phase reaction,
Pressure dependence Equilibrium constant We can see from the gas phase form of the equilibrium constant that the equilibrium concentrations of species depend on pressure. This dependence is inside the
Physical transformations of pure substances Boiling, freezing, and the conversion of graphite to diamond examples of phase transitions changes of
Physical transformations of pure substances Boiling, freezing, and the conversion of graphite to diamond examples of phase transitions changes of phase without change of chemical composition. In this chapter
Name: Discussion Section:
CBE 141: Chemical Engineering Thermodynamics, Spring 2017, UC Berkeley Midterm 2 FORM A March 23, 2017 Time: 80 minutes, closed-book and closed-notes, one-sided 8 ½ x 11 equation sheet allowed Please show
Index to Tables in SI Units
Index to Tables in SI Units Table A-1 Atomic or Molecular Weights and Critical Properties of Selected Elements and Compounds 926 Table A-2 Properties of Saturated Water (Liquid Vapor): Temperature Table
Chapter 17.3 Entropy and Spontaneity Objectives Define entropy and examine its statistical nature Predict the sign of entropy changes for phase
Chapter 17.3 Entropy and Spontaneity Objectives Define entropy and examine its statistical nature Predict the sign of entropy changes for phase changes Apply the second law of thermodynamics to chemical
Application of Thermodynamics in Phase Diagrams. Today s Topics
Lecture 23 Application of Thermodynamics in Phase Diagrams The Clausius Clapeyron Equation A. K. M. B. Rashid Professor, Department of MME BUET, Dhaka Today s Topics The Clapeyron equation Integration
Ph.D. Qualifying Examination In Thermodynamics
Ph.D. Qualifying Examination In Thermodynamics May 2014 University of Texas at Austin Department of Chemical Engineering The exam is a closed book examination. There are five equally weighed problems on
Pressure Volume Temperature Relationship of Pure Fluids
Pressure Volume Temperature Relationship of Pure Fluids Volumetric data of substances are needed to calculate the thermodynamic properties such as internal energy and work, from which the heat requirements
The Chemical Potential
CHEM 331 Physical Chemistry Fall 2017 The Chemical Potential Here we complete our pivot towards chemical thermodynamics with the introduction of the Chemical Potential ( ). This concept was first introduced
Thermodynamic condition for equilibrium between two phases a and b is G a = G b, so that during an equilibrium phase change, G ab = G a G b = 0.
CHAPTER 5 LECTURE NOTES Phases and Solutions Phase diagrams for two one component systems, CO 2 and H 2 O, are shown below. The main items to note are the following: The lines represent equilibria between
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
Ch. 19 Entropy and Free Energy: Spontaneous Change
Ch. 19 Entropy and Free Energy: Spontaneous Change 19-1 Spontaneity: The Meaning of Spontaneous Change 19-2 The Concept of Entropy 19-3 Evaluating Entropy and Entropy Changes 19-4 Criteria for Spontaneous
ME 201 Thermodynamics
Spring 01 ME 01 Thermodynamics Property Evaluation Practice Problems II Solutions 1. Air at 100 K and 1 MPa goes to MPa isenthapically. Determine the entropy change. Substance Type: Ideal Gas (air) Process:
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
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.
Can hematite nanoparticles be an environmental indicator?
Can hematite nanoparticles be an environmental indicator? Haibo Guo, a Huifang Xu, b and Amanda S. Barnard a 1 Chemical potential of water vapour At low temperatures and under high pressures, water vapour
Chapter 3. Property Relations The essence of macroscopic thermodynamics Dependence of U, H, S, G, and F on T, P, V, etc.
Chapter 3 Property Relations The essence of macroscopic thermodynamics Dependence of U, H, S, G, and F on T, P, V, etc. Concepts Energy functions F and G Chemical potential, µ Partial Molar properties
Solutions to Problem Set 9
Solutions to Problem Set 9 1. When possible, we want to write an equation with the quantity on the ordinate in terms of the quantity on the abscissa for each pf the labeled curves. A B C p CHCl3 = K H
Thermodynamics I. Properties of Pure Substances
Thermodynamics I Properties of Pure Substances Dr.-Eng. Zayed Al-Hamamre 1 Content Pure substance Phases of a pure substance Phase-change processes of pure substances o Compressed liquid, Saturated liquid,
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
General Chemistry I Concepts
Thermodynamics Thermodynamics The Three Laws of Thermodynamics (18.1) Spontaneous Processes (18.2) Entropy (18.3) The Second Law of Thermodynamics (18.4) Gibbs Free Energy (18.5) Free Energy and Chemical
CALCULATION OF THE COMPRESSIBILITY FACTOR AND FUGACITY IN OIL-GAS SYSTEMS USING CUBIC EQUATIONS OF STATE
CALCULATION OF THE COMPRESSIBILITY FACTOR AND FUGACITY IN OIL-GAS SYSTEMS USING CUBIC EQUATIONS OF STATE V. P. de MATOS MARTINS 1, A. M. BARBOSA NETO 1, A. C. BANNWART 1 1 University of Campinas, Mechanical
MS212 Thermodynamics of Materials ( 소재열역학의이해 ) Lecture Note: Chapter 7
2017 Spring Semester MS212 Thermodynamics of Materials ( 소재열역학의이해 ) Lecture Note: Chapter 7 Byungha Shin ( 신병하 ) Dept. of MSE, KAIST Largely based on lecture notes of Prof. Hyuck-Mo Lee and Prof. WooChul
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
download instant at 2 Phase Diagrams of Pure Fluids
2 Phase Diagrams of Pure Fluids 13 2. PHASE DIAGRAMS OF PURE FLUIDS Problem 2.1 Solution a) 25 ı C, 1 bar: liquid, because the temperature is below the saturation temperature at 1 bar (99.63 ı C). 10 bar,
Phase Diagrams. Department of Mechanical Engineering Indian Institute of Technology Kanpur Kanpur India
Phase Diagrams 1 Increasing the temperature isobarically T-v diagram of constant-pressure phase-change processes of a pure substance at various pressures numerical values are for water. 2 Temperature -
Name: Discussion Section:
CBE 141: Chemical Engineering Thermodynamics, Spring 2017, UC Berkeley Midterm 2 FORM B March 23, 2017 Time: 80 minutes, closed-book and closed-notes, one-sided 8 ½ x 11 equation sheet allowed lease show
Solutions to Problem Set 6
Solutions to Problem Set 6 1. non- ideal gas, 1 mol 20.0 L 300 K 40.0 L 300 K isothermal, reversible Equation of state: (a)b is a constant independent of T Given du = ( U/ T) V dt + ( U/ V) T dv U = U(T,V)
Practice Examinations Chem 393 Fall 2005 Time 1 hr 15 min for each set.
Practice Examinations Chem 393 Fall 2005 Time 1 hr 15 min for each set. The symbols used here are as discussed in the class. Use scratch paper as needed. Do not give more than one answer for any question.
Mixtures. Partial Molar Quantities
CHEM 331 Physical Chemistry Fall 2017 Mixtures Our current discussion takes up some general results for systems that are mixtures and/or open. The former involve systems that contain multiple components;
Chapter Eighteen. Thermodynamics
Chapter Eighteen Thermodynamics 1 Thermodynamics Study of energy changes during observed processes Purpose: To predict spontaneity of a process Spontaneity: Will process go without assistance? Depends
CHEMISTRY 443, Fall, 2014 (14F) Section Number: 10 Examination 2, November 5, 2014
NAME: CHEMISTRY 443, Fall, 2014 (14F) Section Number: 10 Examination 2, November 5, 2014 Answer each question in the space provided; use back of page if extra space is needed. Answer questions so the grader
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
You MUST sign the honor pledge:
CHEM 3411 MWF 9:00AM Fall 2010 Physical Chemistry I Exam #2, Version B (Dated: October 15, 2010) Name: GT-ID: NOTE: Partial Credit will be awarded! However, full credit will be awarded only if the correct
Exam Thermodynamics 12 April 2018
1 Exam Thermodynamics 12 April 2018 Please, hand in your answers to problems 1, 2, 3 and 4 on separate sheets. Put your name and student number on each sheet. The examination time is 12:30 until 15:30.
Chapter 8 Phase Diagram, Relative Stability of Solid, Liquid, and Gas
Chapter 8 Phase Diagram, Relative Stability of Solid, Liquid, and Gas Three states of matter: solid, liquid, gas (plasma) At low T: Solid is most stable. At high T: liquid or gas is most stable. Ex: Most
Name: Discussion Section:
CBE 141: Chemical Engineering Thermodynamics, Spring 2018, UC Berkeley Midterm 2 March 22, 2018 Time: 80 minutes, closed-book and closed-notes, one-sided 8 ½ x 11 equation sheet allowed Please show all
S A 0.6. Units of J/mol K S U /N
Solutions to Problem Set 5 Exercise 2. Consider heating a body A, of constant heat capacity J/ C and initially at temperature K, to a nal temperature of 2K. The heating takes place by sequentially placing
Name: Discussion Section:
CBE 141: Chemical Engineering Thermodynamics, Spring 2018, UC Berkeley Midterm 2 March 22, 2018 Time: 80 minutes, closed-book and closed-notes, one-sided 8 ½ x 11 equation sheet allowed Please show all
CHEM-UA 652: Thermodynamics and Kinetics
1 CHEM-UA 652: Thermodynamics and Kinetics Notes for Lecture 13 I. PHASE DIAGRAMS The different phases of substances are characterized by different ranges of thermodynamic variables in which these phasesarethestablephases.
Chemistry 2000 Fall 2017 Test 2 Version A Solutions
Chemistry 2000 Fall 207 Test 2 Version A Solutions. Start with a balanced reaction: (a) liquid water: C 2 H 4(g) + 3 O 2(g) 2 CO 2(g) + 2 H 2 O r S = 2S (CO 2 ) + 2S (H 2 O, l) [S (C 2 H 4 ) + 3S (O 2
3.012 PS 7 3.012 Issued: 11.05.04 Fall 2004 Due: 11.12.04 THERMODYNAMICS 1. single-component phase diagrams. Shown below is a hypothetical phase diagram for a single-component closed system. Answer the
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.
Chemistry 360 Spring 2017 Dr. Jean M. Standard April 19, Exam points
Chemistry 360 pring 2017 Dr. Jean M. tandard April 19, 2017 Name Exam 3 100 points Note: You must show your work on problems in order to receive full credit for any answers. You must turn in your equation
Chemistry 192 Problem Set 7 Spring, 2018
Chemistry 192 Problem Set 7 Spring, 2018 1. Use Table D2 to calculate the standard enthalpy change for the combustion of liquid benzene (C 6 H 6 ) in pure oxygen gas to produce gas phase carbon dioxide
WEEK 6. Multiphase systems
WEEK 6 Multiphase systems Multiphase systems P 237. Processes usually deal with material being transferred from one phase (gas, liquid, or solid) to another. 6.1a Phase diagrams F = force on piston Water
General Physical Chemistry I
General Physical Chemistry I Lecture 13 leksey Kocherzhenko pril 7, 2015" Last time " Phase diagrams" Maps showing the thermodynamically stable phases for each and," phase regions in a phase diagram are
PREDICTION OF SATURATED LIQUID VOLUMES FROM A MODIFIED VAN DER WAALS EQUATION. By Charles R. Koppany
PREDICTION OF SATURATED LIQUID VOLUMES FROM A MODIFIED VAN DER WAALS EQUATION Part 1 By Charles R. Koppany Introduction Over the past 40 years or so, closed cubic (in volume) equations of state have been
Exam 3, Chemistry 481, 8 December 2017
1 Exam 3, Chemistry 481, 8 December 2017 Show all work for full credit Useful constants: k B = 1.3807 10 23 J K 1 ; R (molar gas constant) = 8.314 J K 1 mol 1 Helmholz free energy: A = U S, so that da
m m 3 mol Pa = Pa or bar At this pressure the system must also be at approximately 1000 K.
5. PHASES AND SOLUTIONS n Thermodynamics of Vapor Pressure 5.. At equilibrium, G(graphite) G(diamond); i.e., G 2 0. We are given G 2900 J mol. ( G/ P) T V V 2.0 g mol.95 0 6 m 3 mol Holding T constant
From what we know now (i.e, ΔH and ΔS) How do we determine whether a reaction is spontaneous?
pontaneous Rxns A&G-1 From what we know now (i.e, Δ and Δ) ow do we determine whether a reaction is spontaneous? But Δ and Δ are not enough... here is competition between lowering energy and raising entropy!
Although the molar volumes of liquids can be calculated by means of generalized cubic equations of state, the results are often not of high accuracy.
3.7 GENERALIZED CORRELATIONS FOR LIQUIDS Although the molar volumes of liquids can be calculated by means of generalized cubic equations of state, the results are often not of high accuracy. In addition,
Phase Equilibrium: Preliminaries
Phase Equilibrium: Preliminaries Phase diagrams for two one component systems, CO 2 and H 2 O, are shown below. The main items to note are the following: The lines represent equilibria between two phases.
CHAPTER SIX THERMODYNAMICS Vapor-Liquid Equilibrium in a Binary System 6.2. Investigation of the Thermodynamic Properties of Pure Water
CHAPTER SIX THERMODYNAMICS 6.1. Vapor-Liquid Equilibrium in a Binary System 6.2. Investigation of the Thermodynamic Properties of Pure Water 2 6.1. VAPOR-LIQUID EQUILIBRIUM IN A BINARY SYSTEM Keywords:
More on phase diagram, chemical potential, and mixing
More on phase diagram, chemical potential, and mixing Narayanan Kurur Department of Chemistry IIT Delhi 13 July 2013 Melting point changes with P ( ) Gα P T = V α V > 0 = G α when P Intersection point
Appendix F. Steam Tables
Appendix F Steam Tables F.1 INTERPOLATION When a value is required from a table at conditions which lie between listed values, interpolation is necessary. If M, the quantity sought, is a function of a
pv m = RT + Bp The simplest equation for calculating fugacity, given an equation of state, is Z=1 + B RT p
Chem 42/523 Chemical hermodynamics Homework Assignment # 5 1. *Assume O 2 gas obeys the virial equation pv m = R + Bp with B = 12.5 cm 3 mol 1 at 298.15 K. Calculate the fugacity of oxygen at p = 1. MPa
Chem 112 Dr. Kevin Moore
Chem 112 Dr. Kevin Moore Gas Liquid Solid Polar Covalent Bond Partial Separation of Charge Electronegativity: H 2.1 Cl 3.0 H Cl δ + δ - Dipole Moment measure of the net polarity in a molecule Q Q magnitude
Chemical Equilibria. Chapter Extent of Reaction
Chapter 6 Chemical Equilibria At this point, we have all the thermodynamics needed to study systems in ulibrium. The first type of uilibria we will examine are those involving chemical reactions. We will
General Physical Chemistry I
General Physical Chemistry I Lecture 11 Aleksey Kocherzhenko March 12, 2015" Last time " W Entropy" Let be the number of microscopic configurations that correspond to the same macroscopic state" Ø Entropy
Thermodynamics is the study of the relationship between heat and other forms of energy that are involved in a chemical reaction.
Ch 18 Thermodynamics and Equilibrium Thermodynamics is the study of the relationship between heat and other forms of energy that are involved in a chemical reaction. Internal Energy (U) Internal energy
AAE COMBUSTION AND THERMOCHEMISTRY
5. COMBUSTIO AD THERMOCHEMISTRY Ch5 1 Overview Definition & mathematical determination of chemical equilibrium, Definition/determination of adiabatic flame temperature, Prediction of composition and temperature
4.1 Constant (T, V, n) Experiments: The Helmholtz Free Energy
Chapter 4 Free Energies The second law allows us to determine the spontaneous direction of of a process with constant (E, V, n). Of course, there are many processes for which we cannot control (E, V, n)
Chapter 5. Simple Mixtures Fall Semester Physical Chemistry 1 (CHM2201)
Chapter 5. Simple Mixtures 2011 Fall Semester Physical Chemistry 1 (CHM2201) Contents The thermodynamic description of mixtures 5.1 Partial molar quantities 5.2 The thermodynamic of Mixing 5.3 The chemical
Chapter 11 Spontaneous Change and Equilibrium
Chapter 11 Spontaneous Change and Equilibrium 11-1 Enthalpy and Spontaneous Change 11-2 Entropy 11-3 Absolute Entropies and Chemical Reactions 11-4 The Second Law of Thermodynamics 11-5 The Gibbs Function
Thermodynamic Third class Dr. Arkan J. Hadi
5.5 ENTROPY CHANGES OF AN IDEAL GAS For one mole or a unit mass of fluid undergoing a mechanically reversible process in a closed system, the first law, Eq. (2.8), becomes: Differentiation of the defining
Thermodynamics 1 Lecture Note 1
Thermodynamics 1 Lecture Note 1 March 02, 2015 Kwang Kim Yonsei University kbkim@yonsei.ac.kr 39 8 7 34 53 Y O N Se I 88.91 16.00 14.01 78.96 126.9 Scientific Thinking - System under investigation - Description
Chemistry 123: Physical and Organic Chemistry Topic 2: Thermochemistry
Recall the equation. w = -PΔV = -(1.20 atm)(1.02 L)( = -1.24 10 2 J -101 J 1 L atm Where did the conversion factor come from? Compare two versions of the gas constant and calculate. 8.3145 J/mol K 0.082057
The underlying prerequisite to the application of thermodynamic principles to natural systems is that the system under consideration should be at equilibrium. http://eps.mcgill.ca/~courses/c220/ Reversible
Liquids and Solids. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Liquids and Solids Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Gases, Liquids and Solids Gases are compressible fluids. They have no proper volume and proper
Figure Q3. Boundary conditions for a tubular reactor.
1. Please illustrate or explain the meaning the following questions: (a) (10%) Please proof the five dimensionless numbers in fluid transport by Buckingham method as Eu=f(Re, Fr, We, Ma). (b) (10%) Please
Chemical and Engineering Thermodynamics
Chemical and Engineering Thermodynamics Third Edition Stanley I. Sandler University of Delaware John Wiley & Sons, Inc. New York Chichester Weinheim Brisbane Singapore Toronto Contents NOTATION xv CHAPTER1
Statistical Thermodynamics. Lecture 8: Theory of Chemical Equilibria(I)
Statistical Thermodynamics Lecture 8: Theory of Chemical Equilibria(I) Chemical Equilibria A major goal in chemistry is to predict the equilibria of chemical reactions, including the relative amounts of
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
Chapter 3 PROPERTIES OF PURE SUBSTANCES
Thermodynamics: An Engineering Approach Seventh Edition Yunus A. Cengel, Michael A. Boles McGraw-Hill, 2011 Chapter 3 PROPERTIES OF PURE SUBSTANCES Copyright The McGraw-Hill Companies, Inc. Permission
CHEMISTRY Topic #2: Thermochemistry and Electrochemistry What Makes Reactions Go? Fall 2018 Dr. Susan Findlay See Exercises in Topic 8
CHEMISTRY 2000 Topic #2: Thermochemistry and Electrochemistry What Makes Reactions Go? Fall 208 Dr. Susan Findlay See Exercises in Topic 8 Vapour Pressure of Pure Substances When you leave wet dishes on
State Polytechnic of Malang Malang Heat Effect. Thermodynamics Course Chapter 4 Agung Ari Wibowo S.T., M.Sc
State Polytechnic of Malang Malang 217 Heat Effect Thermodynamics Course Agung Ari Wibowo S.T., M.Sc Learning Objective Sensible Heat Heat Capacity & Integral Evaluation of Sensible Heat Laten Heat of
7 Simple mixtures. Solutions to exercises. Discussion questions. Numerical exercises
7 Simple mixtures Solutions to exercises Discussion questions E7.1(b For a component in an ideal solution, Raoult s law is: p xp. For real solutions, the activity, a, replaces the mole fraction, x, and
[S R (U 0 ɛ 1 ) S R (U 0 ɛ 2 ]. (0.1) k B
![[S R (U 0 ɛ 1 ) S R (U 0 ɛ 2 ]. (0.1) k B](/thumbs/72/67524544.jpg "[S R (U 0 ɛ 1 ) S R (U 0 ɛ 2 ]. (0.1) k B")
Canonical ensemble (Two derivations) Determine the probability that a system S in contact with a reservoir 1 R to be in one particular microstate s with energy ɛ s. (If there is degeneracy we are picking
Effect of adding an ideal inert gas, M
Effect of adding an ideal inert gas, M Add gas M If there is no change in volume, then the partial pressures of each of the ideal gas components remains unchanged by the addition of M. If the reaction
PETE 310 Lectures # 36 to 37
PETE 310 Lectures # 36 to 37 Cubic Equations of State Last Lectures Instructional Objectives Know the data needed in the EOS to evaluate fluid properties Know how to use the EOS for single and for multicomponent
Basic Thermodynamics Module 1
Basic Thermodynamics Module 1 Lecture 9: Thermodynamic Properties of Fluids Thermodynamic Properties of fluids Most useful properties: Properties like pressure, volume and temperature which can be measured
Appendix 4. Appendix 4A Heat Capacity of Ideal Gases
Appendix 4 W-143 Appendix 4A Heat Capacity of Ideal Gases We can determine the heat capacity from the energy content of materials as a function of temperature. The simplest material to model is an ideal
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
First Law of Thermodynamics. Example of Spontaneous Rxns. Reversible and Irreversible 8/2/2016
First Law of Thermodynamics The first law of thermodynamics states that the energy of the universe is conserved. If one object loses energy, another has to gain that energy. The mathematical relationship
The View Data module
The module Use to examine stored compound data (H, S, C p (T), G, etc.) in Compound type databases and list solutions and their constituents in Solution type databases. Table of contents Section 1 Section
PVTpetro: A COMPUTATIONAL TOOL FOR ISOTHERM TWO- PHASE PT-FLASH CALCULATION IN OIL-GAS SYSTEMS
PVTpetro: A COMPUTATIONAL TOOL FOR ISOTHERM TWO- PHASE PT-FLASH CALCULATION IN OIL-GAS SYSTEMS A. M. BARBOSA NETO 1, A. C. BANNWART 1 1 University of Campinas, Mechanical Engineering Faculty, Energy Department
MME 2010 METALLURGICAL THERMODYNAMICS II. Partial Properties of Solutions
MME 2010 METALLURGICAL THERMODYNAMICS II Partial Properties of Solutions A total property of a system consisting of multiple substances is represented as nm = n i M i If the system consists of a liquid
Non-Newtonian fluids is the fluids in which shear stress is not directly proportional to deformation rate, such as toothpaste,
CHAPTER1: Basic Definitions, Zeroth, First, and Second Laws of Thermodynamics 1.1. Definitions What does thermodynamic mean? It is a Greeks word which means a motion of the heat. Water is a liquid substance