Simple lattice-gas model for water
|
|
- Randell Wilson
- 6 years ago
- Views:
Transcription
1 Simple lattice-gas model for water A. Ciach, W. T. Góźdź and A. Perera Motivation H-bonds and packing of molecules Construction of the lattice model Results in mean-field approximation
2 Water molecule and H-bonds
3 Water anomalies - facts: Phase diagram for p<2000 bar, dp/dt<0 at the solid-liquid coexistence
4 Increasing T) for p<2000 bar, standard behavior for p>2000bar. For p=1 bar maximum of density at T=4C Density of ice is larger than the density of liquid water Density along the phase coexistence Insert molar volume vs. temperature
5 Isothermal compressibility Specific heat Thermal expansivity
6 Motivation: Water is the main component of living matter; Water molecule is very simple, but liquid water has very peculiar properties. The role of the H-bond network in self-assembly of ionic, polar and amphiphilic solutes is not yet explained. Nature of the hydrophobic and hydrophilic interactions still open question. In order to model collective phenomena on the nano- or micrometer length scale we need a mesoscopic model for water, simple enough but capturing the essential physics. There are no simple mesocopic models for water. Advantage of simple models: If some degrees of freedom are neglected, and the predictions of the model are correct, then the origin of the observed phenomena is explained.
7 Structure of ice Crystal I h Schematic representation of the tetrahedral structure in ice
8 Structure of liquid water Cartoon showing clusters of H-bonded molecules, and close-packed regions. Confirmed neither by experiments nor by simulations Lifetime of H-bonds in liquid water ~ 0.1 ps.
9 Statistical-mechanical modeling. I. Lattice gas model for simple fluids Typical configuration for T>T c Phase diagram Empty cell Occupied cell Nearest-neighbor interaction p= e E N Probability of a configuration Grand potential = ktln
10 Low density Empty cell High density II. Lattice gas model for water Typical configurations liquid gas Interaction energies a van der Waals h - H-bond relative density difference volume of the lattice cell v = volume per molecule in ice Probability of a configuration p= e E N L N H 1 2 Density in a configuration = L N L 1 2 N H V
11 Hamiltonian Blume-Emery-Griffith model for a binary mixture H [{ s}]= 1 2 nn [ J l l s x s x ' 4J gl s2 x s 2 x ' 2Q s x s 2 x ' ] x [ s x 1 s 2 x ] s= 1,0,1 s s 2 - concentration - cell occupancy = s 1 s 2 - density { s } Probability of the configuration : J ll =a 2 h 4 p[{ s}]= e H [{ s}] grand potential H [{ s}] = { s} e = pvv = kt ln J gl =a 1 2 h 4 Q=a 1 h 4
12 Ground state (T=0K) dependence on the model parameters Simple fluid Water-like By assuming the coexistence between the high-density and the low-density phases at p=2000 bar we obtain a relation between the model parameters a,h,v,
13 Limiting cases High density Low density s=1 s= 1 s=1 s= 1 H l l [{ s }]= J l l 2 nn s x s x ' 6Q x s x H lg [{ s }]= J lg 2 s x s x' [6J nn gl 1 2 ] x s x Each limiting case is isomorphic with the Ising (lattice gas) model. In each case a critical point is expected. By equating the critical-point temperatures to 180K and 650K we obtain two relations between the model parameters.
14 The model parameters: v=35 A 3 a=3.6 kj/mol h=1.1 kj/mol =0.12 In water: v~33 A 3 a~5.5 kj/mol h= E H= kj /mol=1.2kj/mol 0.1 Mean-field (MF) approximation: each molecule is in the external field resulting from interactions with the remaining molecules in their equilibrium positions. Average values are approximated by the most probable values. In MF the critical point temperature T c is overestimated. Exact result for T c in the Ising model is T c ~4.5/6T MF MF c =0.75 T c
15 Functional of two fields, MF [s x, x ]=H [s x, x ] TS[s x, x ] On the lattice the entropy S has the ideal-mixing entropy form The fields s= s MF, = s 2 MF satisfy the minimum condition MF s =0= MF Spinodal surface: det [ 2 MF ]=0 The density: =[ 1 s] ice
16 Spinodal (dashed) and binodal lines in MF
17 Gas-liquid coexistence in experiment and in the model Anomalous density increase
18 EOS isobars P=100 bar p=1000bar p=2500bar p=10bar Critical pressure in the model is p=653 bar
19 Isothermal compressibility 0.1 kbar 1 kbar We observe minimum of the compressibility, but only for high pressures
20 Constant-pressure specific heat 0.1 kbar 1 kbar
21 Thermal expansivity 0.1 kbar 1 kbar
22 Correlation length at the critical density of the mestastable liquid-liquid critical point
23 For p<2000 bar open structure at low T. T increases mixing of the two forms of water density increases. Further increase of T mixing of the occupied and empty cells -density decreases. For p>2000bar compact structure at low T. T increases - mixing of the two forms of water density decreases.
24 Summary Simple model for water is developed. Water is treated as a special mixture of low and high density components with chemical potentials and. The model predicts correctly the special features of water. It may play a similar role as the lattice gas model of simple fluids. Entropy associated with mixing of closely-packed and open structures is the key reason of water anomalies Quantitative improvement can be obtained in off-lattice models, with a more realistic form of the entropy term.
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
More information2. As gas P increases and/or T is lowered, intermolecular forces become significant, and deviations from ideal gas laws occur (van der Waal equation).
A. Introduction. (Section 11.1) CHAPTER 11: STATES OF MATTER, LIQUIDS AND SOLIDS 1. Gases are easily treated mathematically because molecules behave independently. 2. As gas P increases and/or T is lowered,
More information2. As gas P increases and/or T is lowered, intermolecular forces become significant, and deviations from ideal gas laws occur (van der Waal equation).
A. Introduction. (Section 11.1) CHAPTER 11: STATES OF MATTER, LIQUIDS AND SOLIDS 1. Gases are easily treated mathematically because molecules behave independently. 2. As gas P increases and/or T is lowered,
More informationAus: Daniel Schroeder An introduction to thermal physics, Pearson Verlag
Ω A q B Ω B Ω total 0 00 8 0 8 8 0 8 00 99 9 0 80 8 0 8 0 98 0 80 0 8 00 97 0 0 80 0 8 0 8 9 0 79 0 88 9 0 8 0 8 0 0 0 9 0 0 9 0 77 0 9 9 88 0 8 0 00 7 0 9 0 7 0 9 9 0 Ω total ( 0 ) 7 0 0 0 00 N, q few
More informationStatistical Physics. Solutions Sheet 11.
Statistical Physics. Solutions Sheet. Exercise. HS 0 Prof. Manfred Sigrist Condensation and crystallization in the lattice gas model. The lattice gas model is obtained by dividing the volume V into microscopic
More informationImperfect Gases. NC State University
Chemistry 431 Lecture 3 Imperfect Gases NC State University The Compression Factor One way to represent the relationship between ideal and real gases is to plot the deviation from ideality as the gas is
More informationA Phase Transition in Ammonium Chloride. CHM 335 TA: David Robinson Office Hour: Wednesday, 11 am
A Phase Transition in Ammonium Chloride CHM 335 TA: David Robinson Email: Drobinson@chm.uri.edu Office Hour: Wednesday, 11 am Purpose Determine the critical exponent for the order to disorder transition
More informationPhenomenological Theories of Nucleation
Chapter 1 Phenomenological Theories of Nucleation c 2012 by William Klein, Harvey Gould, and Jan Tobochnik 16 September 2012 1.1 Introduction These chapters discuss the problems of nucleation, spinodal
More informationStatistical physics. Emmanuel Trizac LPTMS / University Paris-Sud
Statistical physics Emmanuel Trizac LPTMS / University Paris-Sud Outline I Introduction to phase transitions and critical phenomena 1- The problems raised by phase transitions, from a statistical mechanics
More information5.60 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
More informationPhase Transitions in Multicomponent Systems
Physics 127b: Statistical Mechanics Phase Transitions in Multicomponent Systems The ibbs Phase Rule Consider a system with n components (different types of molecules) with r s in equilibrium. The state
More informationChapter 12. Insert picture from First page of chapter. Intermolecular Forces and the Physical Properties of Liquids and Solids
Chapter 12 Insert picture from First page of chapter Intermolecular Forces and the Physical Properties of Liquids and Solids Copyright McGraw-Hill 2009 1 12.1 Intermolecular Forces Intermolecular forces
More informationChemistry 5350 Advanced Physical Chemistry Fall Semester 2013
Chemistry 5350 Advanced Physical Chemistry Fall Semester 2013 Name: Quiz 2: Chapters 3, 4, and 5 September 26, 2013 Constants and Conversion Factors Gas Constants: 8.314 J mol 1 K 1 8.314 Pa m 3 mol 1
More informationSurvey of Thermodynamic Processes and First and Second Laws
Survey of Thermodynamic Processes and First and Second Laws Please select only one of the five choices, (a)-(e) for each of the 33 questions. All temperatures T are absolute temperatures. All experiments
More informationPhases of matter and phase diagrams
Phases of matter and phase diagrams Transition to Supercritical CO2 Water Ice Vapor Pressure and Boiling Point Liquids boil when the external pressure equals the vapor pressure. Temperature of boiling
More informationPROBLEM 6.3. Using the appropriate table, determine the indicated property. In each case, locate the state on sketches of the T-v and T-s diagrams.
PROBLEM 63 Using the appropriate table, determine the indicated property In each case, locate the state on sketches of the -v and -s diagrams (a) water at p = 040 bar, h = 147714 kj/kg K Find s, in kj/kg
More informationChapter 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
More informationCH.7 Fugacities in Liquid Mixtures: Models and Theories of Solutions
CH.7 Fugacities in Liquid Mixtures: Models and Theories of Solutions The aim of solution theory is to express the properties of liquid mixture in terms of intermolecular forces and liquid structure. The
More informationChapter 10. Lesson Starter. Why did you not smell the odor of the vapor immediately? Explain this event in terms of the motion of molecules.
Preview Lesson Starter Objectives The Kinetic-Molecular Theory of Gases The Kinetic-Molecular Theory and the Nature of Gases Deviations of Real Gases from Ideal Behavior Section 1 The Kinetic-Molecular
More informationChapter 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
More informationMonte Carlo simulation of confined water
Monte Carlo simulation of confined water Author: Guillermo Cámbara Ruiz Advisor: Giancarlo Franzese Facultat de Física, Universitat de Barcelona, Diagonal 645, 08028 Barcelona, Spain. Abstract: In living
More informationLattice protein models
Lattice protein models Marc R. Roussel epartment of Chemistry and Biochemistry University of Lethbridge March 5, 2009 1 Model and assumptions The ideas developed in the last few lectures can be applied
More informationPhysics 404: Final Exam Name (print): "I pledge on my honor that I have not given or received any unauthorized assistance on this examination.
Physics 404: Final Exam Name (print): "I pledge on my honor that I have not given or received any unauthorized assistance on this examination." May 20, 2008 Sign Honor Pledge: Don't get bogged down on
More informationChem 112 Exam 1 Version A Spring /16/ :00am/Odago, M. O.
Chem 112 Exam 1 Version A Spring 2011 02/16/2011 10:00am/Odago, M. O. 1. The pressure of a certain gas is measured to be 25.1 mmhg. What is this pressure expressed in units of pascals? (1 atm=1.0125 x10
More informationChapter 17. Free Energy and Thermodynamics. Chapter 17 Lecture Lecture Presentation. Sherril Soman Grand Valley State University
Chapter 17 Lecture Lecture Presentation Chapter 17 Free Energy and Thermodynamics Sherril Soman Grand Valley State University First Law of Thermodynamics You can t win! The first law of thermodynamics
More informationChapter-2 (Page 22-37) Physical and Chemical Properties of Water
Chapter-2 (Page 22-37) Physical and Chemical Properties of Water Introduction About 70% of the mass of the human body is water. Water is central to biochemistry for the following reasons: 1- Biological
More informationThe 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
More informationLiquids and Solids Chapter 10
Liquids and Solids Chapter 10 Nov 15 9:56 AM Types of Solids Crystalline solids: Solids with highly regular arrangement of their components Amorphous solids: Solids with considerable disorder in their
More information12. Heat of melting and evaporation of water
VS 12. Heat of melting and evaporation of water 12.1 Introduction The change of the physical state of a substance in general requires the absorption or release of heat. In this case, one speaks of a first
More informationChapter 11. Intermolecular Forces and Liquids & Solids
Chapter 11 Intermolecular Forces and Liquids & Solids The Kinetic Molecular Theory of Liquids & Solids Gases vs. Liquids & Solids difference is distance between molecules Liquids Molecules close together;
More informationWeek 11/Th: Lecture Units 28 & 29
Week 11/Th: Lecture Units 28 & 29 Unit 27: Real Gases Unit 28: Intermolecular forces -- types of forces between molecules -- examples Unit 29: Crystal Structure -- lattice types -- unit cells -- simple
More informationPhase transitions and critical phenomena
Phase transitions and critical phenomena Classification of phase transitions. Discontinous (st order) transitions Summary week -5 st derivatives of thermodynamic potentials jump discontinously, e.g. (
More informationLectures 16: Phase Transitions
Lectures 16: Phase Transitions Continuous Phase transitions Aims: Mean-field theory: Order parameter. Order-disorder transitions. Examples: β-brass (CuZn), Ferromagnetic transition in zero field. Universality.
More informationP(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
More informationChapter 2 Experimental sources of intermolecular potentials
Chapter 2 Experimental sources of intermolecular potentials 2.1 Overview thermodynamical properties: heat of vaporization (Trouton s rule) crystal structures ionic crystals rare gas solids physico-chemical
More informationIdeal Gas Behavior. NC State University
Chemistry 331 Lecture 6 Ideal Gas Behavior NC State University Macroscopic variables P, T Pressure is a force per unit area (P= F/A) The force arises from the change in momentum as particles hit an object
More informationChem 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
More informationTable 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]
More informationFor more info visit
Basic Terminology: Terms System Open System Closed System Isolated system Surroundings Boundary State variables State Functions Intensive properties Extensive properties Process Isothermal process Isobaric
More informationvan der Waals Isotherms near T c
van der Waals Isotherms near T c v d W loops are not physical. Why? Patch up with Maxwell construction van der Waals Isotherms, T/T c van der Waals Isotherms near T c Look at one of the van der Waals isotherms
More informationPH4211 Statistical Mechanics Brian Cowan
PH4211 Statistical Mechanics Brian Cowan Contents 1 The Methodology of Statistical Mechanics 1.1 Terminology and Methodology 1.1.1 Approaches to the subject 1.1.2 Description of states 1.1.3 Extensivity
More information(b) The measurement of pressure
(b) The measurement of pressure The pressure of the atmosphere is measured with a barometer. The original version of a barometer was invented by Torricelli, a student of Galileo. The barometer was an inverted
More informationSpontaneous Change.! Although exothermic processes tend to be spontaneous, spontaneous reactions can be exothermic or endothermic:
Spontaneous Change! Any process, once initiated, that continues without further intervention is spontaneous.! Although exothermic processes tend to be spontaneous, spontaneous reactions can be exothermic
More informationThe broad topic of physical metallurgy provides a basis that links the structure of materials with their properties, focusing primarily on metals.
Physical Metallurgy The broad topic of physical metallurgy provides a basis that links the structure of materials with their properties, focusing primarily on metals. Crystal Binding In our discussions
More informationThermal and Statistical Physics Department Exam Last updated November 4, L π
Thermal and Statistical Physics Department Exam Last updated November 4, 013 1. a. Define the chemical potential µ. Show that two systems are in diffusive equilibrium if µ 1 =µ. You may start with F =
More informationLecture 20: Spinodals and Binodals; Continuous Phase Transitions; Introduction to Statistical Mechanics
Lecture 20: 11.28.05 Spinodals and Binodals; Continuous Phase Transitions; Introduction to Statistical Mechanics Today: LAST TIME: DEFINING METASTABLE AND UNSTABLE REGIONS ON PHASE DIAGRAMS...2 Conditions
More informationWhat determines the phase of a substance? Temperature Pressure Interparticle Forces of Attraction
Liquids and Solids What determines the phase of a substance? Temperature Pressure Interparticle Forces of Attraction Types of Interparticle Forces Ionic Bonding Occurs between cations and anions Metallic
More informationCHEM-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.
More informationContents. 1 Introduction and guide for this text 1. 2 Equilibrium and entropy 6. 3 Energy and how the microscopic world works 21
Preface Reference tables Table A Counting and combinatorics formulae Table B Useful integrals, expansions, and approximations Table C Extensive thermodynamic potentials Table D Intensive per-particle thermodynamic
More informationSurface chemistry. Liquid-gas, solid-gas and solid-liquid surfaces. Levente Novák István Bányai
Surface chemistry. Liquid-gas, solid-gas and solid-liquid surfaces. Levente Novák István Bányai Surfaces and Interfaces Defining of interfacial region Types of interfaces: surface vs interface Surface
More informationChapter 2 - Water 9/8/2014. Water exists as a H-bonded network with an average of 4 H-bonds per molecule in ice and 3.4 in liquid. 104.
Chapter 2 - Water Water exists as a -bonded network with an average of 4 -bonds per molecule in ice and 3.4 in liquid. 104.5 o -bond: An electrostatic attraction between polarized molecules containing
More informationThe Equilibrium State
Materials Science & Metallurgy Part III Course M16 Computation of Phase Diagrams (Revision) H. K. D. H. Bhadeshia The Equilibrium State Equilibrium is a state in which no further change is perceptible,
More informationAdsorption from a one-dimensional lattice gas and the Brunauer Emmett Teller equation
Proc. Natl. Acad. Sci. USA Vol. 93, pp. 1438 1433, December 1996 Chemistry Adsorption from a one-dimensional lattice gas and the Brunauer Emmett Teller equation (Ising modelreference systemgibbs ecess
More informationDownloaded from
THERMODYNAMICS Thermodynamics: is the branch of science which deals with deals with the study of different forms of energy and the quantitative relationship between them. Significance of Thermodynamics:
More information5.60 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
More informationAt this point, we've developed the tools and basic concepts necessary to apply
18 Lecture 0 At this point, we've developed the tools and basic concepts necessary to apply thermodynamics to a number of different systems, with the ultimate goal of describing chemically reacting systems.
More information18:00-21:00, 13 January, 2017 (Total Score: 118 points)
Chemistry I Final Exam 18:00-21:00, 13 January, 2017 (Total Score: 118 points) R = 8.314 J K -1 mol -1 1. The ionic character of the bond in a diatomic molecule can be estimated by the formula: ( /ed )
More informationCritical Exponents. From P. Chaikin and T Lubensky Principles of Condensed Matter Physics
Critical Exponents From P. Chaikin and T Lubensky Principles of Condensed Matter Physics Notice that convention allows for different exponents on either side of the transition, but often these are found
More informationMASSACHUSETTS INSTITUTE OF TECHNOLOGY Physics Department Statistical Physics I Spring Term 2013
MASSACHUSETTS INSTITUTE OF TECHNOLOGY Physics Department 8.044 Statistical Physics I Spring Term 2013 Problem 1: Ripplons Problem Set #11 Due in hand-in box by 4:00 PM, Friday, May 10 (k) We have seen
More informationThe lattice model of polymer solutions
The lattice model of polymer solutions Marc R. Roussel Department of Chemistry and Biochemistry University of Lethbridge February 25, 2009 1 The lattice model of polymer solutions In the last note, we
More informationC a h p a t p er 3 The Importance of State Functions: Internal Energy and Enthalpy
Chapter 3 he Importance of State Functions: Internal Energy and Enthalpy Engel & Reid 1 Outline 3.1 he Mathematical roperties of State Functions 3.2 he Dependence of U on and 3.3 Does he Internal Energy
More informationGeneral 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
More informationChem Hughbanks Exam 3, April 19, 2012
Chem 107 - Hughbanks Exam 3, April 19, 2012 Name (Print) UIN # Section 503 Exam 3, Version # A On the last page of this exam, you ve been given a periodic table and some physical constants. You ll probably
More informationLiquids, Solids and Phase Changes
Chapter 10 Liquids, Solids and Phase Changes Chapter 10 1 KMT of Liquids and Solids Gas molecules have little or no interactions. Molecules in the Liquid or solid state have significant interactions. Liquids
More informationThermodynamic 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
More informationThermodynamics. Fill in the blank (1pt)
Fill in the blank (1pt) Thermodynamics 1. The Newton temperature scale is made up of different points 2. When Antonine Lavoisier began his study of combustion, he noticed that metals would in weight upon
More informationHomework 01. Phase Changes and Solutions
HW01 - Phase Changes and Solu!ons! This is a preview of the published version of the quiz Started: Jan 16 at 1:pm Quiz Instruc!ons Homework 01 Phase Changes and Solutions Question 1 Given that you have
More informationPhase 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
More informationStates of matter Part 2
Physical Pharmacy Lecture 2 States of matter Part 2 Assistant Lecturer in Pharmaceutics Overview The Liquid State General properties Liquefaction of gases Vapor pressure of liquids Boiling point The Solid
More informationGeneral 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
More informationVirial Expansion. Silicon Valley FIG March 24, Chen-Hanson Ting
Virial Expansion Silicon Valley FIG March 24, 2018 Chen-Hanson Ting Virial Expansion This paper was uploaded to Wikipedia. Google virial expansion and you will find it. Let s first scan through it on Wiki.
More informationAppendix 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
More informationPhysics 563 Term Paper Liquid-Liquid Phase Transition
Physics 563 Term Paper Liquid-Liquid Phase Transition Kuei Sun December 10, 2005 kueisun2@uiuc.edu Department of Physics, University of Illinois at Urbana- Champaign, 1110 W. Green St., Urbana, IL 61801,
More information2. WATER : THE SOLVENT FOR BIOCHEMICAL REACTIONS
2. WATER : THE SOLVENT FOR BIOCHEMICAL REACTIONS 2.1 Water and Polarity Both geometry and properties of molecule determine polarity Electronegativity - The tendency of an atom to attract electrons to itself
More information= 1906J/0.872deg = 2186J/deg
Physical Chemistry 2 2006 Homework assignment 2 Problem 1: he heat of combustion of caffeine was determined by first burning benzoic acid and then caffeine. In both cases the calorimeter was filled with
More informationConcepts of Thermodynamics
Thermodynamics Industrial Revolution 1700-1800 Science of Thermodynamics Concepts of Thermodynamics Heavy Duty Work Horses Heat Engine Chapter 1 Relationship of Heat and Temperature to Energy and Work
More informationChem Hughbanks Exam 3A, Solutions
Chem 107 - Hughbanks Exam 3A, Solutions Name (Print) UIN # Section 503 Exam 3, Version # A On the last page of this exam, you ve been given a periodic table and some physical constants. You ll probably
More informationCHEM Thermodynamics. Work. There are two ways to change the internal energy of a system:
There are two ways to change the internal energy of a system: Thermodynamics Work 1. By flow of heat, q Heat is the transfer of thermal energy between and the surroundings 2. By doing work, w Work can
More informationMSE 201A Thermodynamics and Phase Transformations Fall, 2008 Problem Set No. 8. Given Gibbs generals condition of equilibrium as derived in the notes,
MSE 201A hermodynamics and Phase ransformations Fall, 2008 Problem Set No. 8 Problem 1: (a) Let a homogeneous fluid with composition, {x}, be surrounded by an impermeable wall and in contact with a reservoir
More informationa) 1.3 x 10 3 atm b) 2.44 atm c) 8.35 atm d) 4.21 x 10-3 atm e) 86.5 atm
1. (6 pts) A sample of gas with a volume of 750 ml exerts a pressure of 756 mm Hg at 30.0 0 C. What pressure (atm) will the sample exert when it is compressed to 250 ml and cooled to -25.0 0 C? a) 1.3
More informations i s j µ B H Figure 3.12: A possible spin conguration for an Ising model on a square lattice (in two dimensions).
s i which can assume values s i = ±1. A 1-spin Ising model would have s i = 1, 0, 1, etc. We now restrict ourselves to the spin-1/2 model. Then, if there is also a magnetic field that couples to each spin,
More informationClusters and Percolation
Chapter 6 Clusters and Percolation c 2012 by W. Klein, Harvey Gould, and Jan Tobochnik 5 November 2012 6.1 Introduction In this chapter we continue our investigation of nucleation near the spinodal. We
More informationChap. 2. Polymers Introduction. - Polymers: synthetic materials <--> natural materials
Chap. 2. Polymers 2.1. Introduction - Polymers: synthetic materials natural materials no gas phase, not simple liquid (much more viscous), not perfectly crystalline, etc 2.3. Polymer Chain Conformation
More informationLecture 8. Polymers and Gels
Lecture 8 Polymers and Gels Variety of polymeric materials Polymer molecule made by repeating of covalently joint units. Many of physical properties of polymers have universal characteristic related to
More informationChapter 10. Liquids and Solids
Chapter 10 Liquids and Solids Chapter 10 Table of Contents 10.1 Intermolecular Forces 10.2 The Liquid State 10.3 An Introduction to Structures and Types of Solids 10.4 Structure and Bonding in Metals 10.5
More informationCHAPTER 10. States of Matter
CHAPTER 10 States of Matter Kinetic Molecular Theory Kinetikos - Moving Based on the idea that particles of matter are always in motion The motion has consequences Explains the behavior of Gases, Liquids,
More informationCHAPTER 10. Kinetic Molecular Theory. Five Assumptions of the KMT. Atmospheric Pressure
Kinetic Molecular Theory CHAPTER 10 States of Matter Kinetikos - Moving Based on the idea that particles of matter are always in motion The motion has consequences Explains the behavior of Gases, Liquids,
More informationSome properties of water
Some properties of water Hydrogen bond network Solvation under the microscope 1 Water solutions Oil and water does not mix at equilibrium essentially due to entropy Substances that does not mix with water
More informationMaterials at Equilibrium. G. Ceder Fall 2001 COURSE 3.20: THERMODYNAMICS OF MATERIALS. FINAL EXAM, Dec 18, 2001
NAME: COURSE 3.20: THERMODYNAMICS OF MATERIALS FINAL EXAM, Dec 18, 2001 PROBLEM 1 (15 POINTS) PROBLEM 2 (15 POINTS) PROBLEM 3 (10 POINTS) PROBLEM 4 (20 POINTS) PROBLEM 5 (14 POINTS) PROBLEM 6 (14 POINTS)
More informationPractice 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.
More informationSUPeR Chemistry CH 222 Practice Exam
SUPeR Chemistry CH 222 Practice Exam This exam has been designed to help you practice working multiple choice problems over the material that will be covered on the first CH 222 midterm. The actual exams
More informationIntermolecular Forces and Liquids and Solids Chapter 11
Intermolecular Forces and Liquids and Solids Chapter 11 A phase is a homogeneous part of the system in contact with other parts of the system but separated from them by a well defined boundary. Phases
More informationChemistry 2000 Lecture 9: Entropy and the second law of thermodynamics
Chemistry 2000 Lecture 9: Entropy and the second law of thermodynamics Marc R. Roussel January 23, 2018 Marc R. Roussel Entropy and the second law January 23, 2018 1 / 29 States in thermodynamics The thermodynamic
More informationChapter 7 PHASE EQUILIBRIUM IN A ONE-COMPONENT SYSTEM
Chapter 7 PHASE EQUILIBRIUM IN A ONE-COMPONENT SYSTEM 7.1 INTRODUCTION The intensive thermodynamic properties of a system are temperature, pressure, and the chemical potentials of the various species occurring
More informationCh. 11: Liquids and Intermolecular Forces
Ch. 11: Liquids and Intermolecular Forces Learning goals and key skills: Identify the intermolecular attractive interactions (dispersion, dipole-dipole, hydrogen bonding, ion-dipole) that exist between
More informationHomework Week 8 G = H T S. Given that G = H T S, using the first and second laws we can write,
Statistical Molecular hermodynamics University of Minnesota Homework Week 8 1. By comparing the formal derivative of G with the derivative obtained taking account of the first and second laws, use Maxwell
More information1. 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.
More informationfiziks 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
More informationChapter 13 States of Matter Forces of Attraction 13.3 Liquids and Solids 13.4 Phase Changes
Chapter 13 States of Matter 13.2 Forces of Attraction 13.3 Liquids and Solids 13.4 Phase Changes I. Forces of Attraction (13.2) Intramolecular forces? (forces within) Covalent Bonds, Ionic Bonds, and metallic
More informationEquations of State. Equations of State (EoS)
Equations of State (EoS) Equations of State From molecular considerations, identify which intermolecular interactions are significant (including estimating relative strengths of dipole moments, polarizability,
More information