Transition Theory Abbreviated Derivation [ A - B - C] # E o. Reaction Coordinate. [ ] # æ Æ
|
|
- Diana Thompson
- 6 years ago
- Views:
Transcription
1 Transition Theory Abbreviated Derivation A + BC æ Æ AB + C [ A - B - C] # E A BC D E o AB, C Reaction Coordinate A + BC æ æ Æ æ A - B - C [ ] # æ Æ æ A - B + C The rate of reaction is the frequency of the complex crossing the barrier # -r A = r AB = u I C ABC (1) where the frequency u I can be thought of as a loose vibration. We are going to assume that the activated complex is in virtual equilibrium with the reactants Then K # C = C # ABC (2) C A C BC -r A = u I K C # C A C BC (3) From thermodynamics we know Then DG = -RT ln K (4) K = e -DG RT (5) where K is the dimensionless true equilibrium constant and related to the concentration equilibrium constant K C by K = K g K C V d m = K C V d m = e -DG RT (6) Then for the equilibrium between the reactants and the transition state K # C = V -d m e -DG # RT 1
2 Part I Relate K C # to Partition Functions We are now going use statistical mechanics to derive the equation for K C #. We start by recalling that the number of ways, W, of arranging N particles among m energy states is N! W = n 1!n 2!Kn m! where n i is the number of particles in the i th state. For a fixed total number of molecules N = Ân i and a fixed total energy E = Ân i e i the most probable distribution, the one that overwhelms all the others, is found by setting dw = 0. The result is where n i N = e -be i q q = Âe -be i, b = 1 k B T n i N = fraction of molecules that occupy energy state e i (9) q = molecular partition function The molecular partition function, q, gives a measure of how the molecules are distributed (partitioned) among the energy states. It gives an indication of the average number of states that are accessible at a particular temperature for non interacting molecules. Fundamental postulate relating t and W Sterling s approximation Using Sterling s approximation, Equation (10) becomes S = k ln W = k[ ln N!- ln n i!] (10) (7) (8) ln X!= X ln X - X (11) n i Substituting for using Equation (8) N S = -k  ln n i N 2 (12)
3 U-U 67 8 o N} S = kbâ n i e i + kâ n i ln q The sum  n i e i is the internal energy relative to the ground state, i.e. (U U o ) S = U - U o + kn ln q (13) T This result is for non interacting particles. For interacting particles, the result is S = U - U o T + k ln q N From thermodynamic we know the relationship between Combining Equations (14) and (15) N! (14) G = U - T S + PV = U - T S + nrt (15) G = U o - nrtln q N (16) We now define molar partition function, q m q N = q = q m n q m = q n (17) Dividing Equation (16) by the number of moles n when Typical units of G and U are (J/mol). G = U o - RTln q m (18) G G = n, U o = U n We now will apply Equation (18) to each species in the reaction The change in Gibbs free energy for reaction (19) is Using Equation (18) we obtain aa+ bb Æ cc + dd (19) G i = U oi - RTln q mi (20) DG = cg C + dg D - bg B - ag A (21) 3
4 where and using Equation (22) The molar partition function is DG = DE 0 - RTln q c mc a q ma d q md b q mb N -d Avo (22) DE 0 = cu C + du Do - bu Bo - au Ao (23) K = e -DE 0 RT d = d + c - b - a q c mc q mi = q i and the partition function per unit volume is then d q md b a q mb q ma n q i = q i V N -d Avo (24) V q mi = q i n = q i V m (25) K = e -DE 0 RT q C q B ( ) c ( q D ) d ( ) b ( ) a q A Recalling Equation (6) and equating it to Equation (26) K C K g V d m = K = e -DE 0 RT q C q B V m d -d ( ) c ( q D ) d ( ) b ( ) a q A V m d -d For ideal mixtures Kg = 1 and canceling the molar volumes we arrive at the main result we have been looking for K C = e -DE 0 RT q C q B ( ) c ( q D ) d ( ) b ( ) a q A N -d Avo We now apply Equation (28) to our transition state reaction (d = 1) A+ BC æ Æ ABC # æ Æ AB+ C K # C = e - ( DE 0 RT) q ABC -1 q A q BC # (26) (27) (28) (29) 4
5 Part II Partition Function We now focus on the partition function per unit volume Dividing by V q = Âe -be i = Âe -b ( e el +e T +e V +e Rot ) i = Âe -be el Âe -be T Âe -be V Âe -be Rot = q el q T q V q R (30) q T = q T V (31) q = q el q T q V q R (32) The Transitional Partition Function, q T The translational partition function is obtained by solving the wave equation for a particle in a box. q T = 1 L V 3 q T = 1 L = 2pmkT 3 h ( ) 1 2 Where L is the thermal wave length, h is Plank s constant, m = mass of the molecule and k is Boltzmann s constant. Substituting for k and h and simplifying m q T = AB m 3 1 amu T 300K 3 2 (33) The Vibrational Partition Function, q V For the harmonic oscillator For small arguments of Evaluating hu i kt q V = q V1 q V2 q V3 K (34) 1 q Vi = 1- exp - hu i kt (35) q vi = kt hu i (36) 5
6 hu k B T = hc u u = K k B T 1 cm T c = speed of light The Rotational Partition Function, q R For linear molecules we solve the wave equation for the rigid rotator model to find the rotational partition function to be where B = Rotational Constant where I = moment of inertia Evaluating k, h, c, and simplifying q R = kt 2hcB B = h 8pcI I = Â m i r i 2 c = speed of light T I q R =12.4 AB 300K 1 amu Ang 2 1 S y The overall or total partition function for the activated complex is # q ABC = q # e q # T q # # V q R We now consider the loose imaginary vibration u I. The total vibrational partition function is the product of the partition functions for each vibrational mode, i.e., 6 (37) (38) q # V = q # Vi q # # V1 q V2 = kt q # # V1 q V2 = kt q V# (39) hu I hu I where q V# is the partition function that includes the loose vibration and q V# is the vibrational partition function without the loose vibration. Similarly for the total partition function substituting into Equation (39) # q ABC = kt q ABC# (40) hu I K # C = kt e -DE o RT q ABC# (41) hu I q A q BC
7 Substituting Equation (41) into Equation (3) we note that the loose vibration frequency cancels and we obtain -r A = kt e -DE o RT q ABC# C A C BC (42) h q A q BC 43 K C# k B T T = h molecules s 300K 23 molecules = mol Note: If B and C are the same molecule, B 2, in the reaction A = kt h q ABC# N q A q Avo (43) BC A+ B 1 - B 2 Æ AB+ B There will be a factor of 2 ( 2kT h) in the rate constant because A can attach either B molecule, B 1 or B 2. It s sometimes easier to make TST calculations by taking ratios The Eyring Equation q A-B-C = q A q BC q A-B-C q A q BC Tran q A-B-C q A q BC Vib q A-B-C q A q BC Letting K C# represent the equilibrium constant with the loose vibration removed we have -r A = k B T h K C# C A C BC the true dimensionless equilibrium constant is then K = K g K C V m d Rot K C# = K # V m -d = K # V m = K # C T where C T is the total concentration 7
8 DG # = -RT ln K # -DG RT K # = e DG = DH - TDS K C# = K C# = -r A = k BT 1 h DS # # = S ABC = C T e -DG # RT C T e DS # R e DS# R e -DH # RT e -DH # RT C T C A C BC (44) -S A -S B = a negative number because we are going from a less ordered state to a more ordered state. DH # = H ABC-# - H A - H BC = a positive number e DS# R Configurations Leading to Reactions = Total Number of Configurations (45) Definitions q = overall partition function = Âe -be i, b = 1 kt q m = q n = molar partition function q = q e q Tr q Vib q Rot q T = q T V q V = q Vi q V1 q V2 q V # = vibrational partition for activated state including loose vibration q V# = vibrational partition function with loose vibration removed q # = overall partition function per unit volume with loose vibration removed 8
3. RATE LAW AND STOICHIOMETRY
Page 1 of 39 3. RATE LAW AND STOICHIOMETRY Professional Reference Shelf R3.2 Abbreviated Lecture Notes Full Lecture Notes I. Overview II. Introduction A. The Transition State B. Procedure to Calculate
More informationFoundations of Chemical Kinetics. Lecture 12: Transition-state theory: The thermodynamic formalism
Foundations of Chemical Kinetics Lecture 12: Transition-state theory: The thermodynamic formalism Marc R. Roussel Department of Chemistry and Biochemistry Breaking it down We can break down an elementary
More informationHandout 11: Ideal gas, internal energy, work and heat. Ideal gas law
Handout : Ideal gas, internal energy, work and heat Ideal gas law For a gas at pressure p, volume V and absolute temperature T, ideal gas law states that pv = nrt, where n is the number of moles and R
More informationHandout 11: Ideal gas, internal energy, work and heat. Ideal gas law
Handout : Ideal gas, internal energy, work and heat Ideal gas law For a gas at pressure p, volume V and absolute temperature T, ideal gas law states that pv = nrt, where n is the number of moles and R
More informationOCN 623: Thermodynamic Laws & Gibbs Free Energy. or how to predict chemical reactions without doing experiments
OCN 623: Thermodynamic Laws & Gibbs Free Energy or how to predict chemical reactions without doing experiments Definitions Extensive properties Depend on the amount of material e.g. # of moles, mass or
More informationStatistical 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
More informationEquations: q trans = 2 mkt h 2. , Q = q N, Q = qn N! , < P > = kt P = , C v = < E > V 2. e 1 e h /kt vib = h k = h k, rot = h2.
Constants: R = 8.314 J mol -1 K -1 = 0.08206 L atm mol -1 K -1 k B = 0.697 cm -1 /K = 1.38 x 10-23 J/K 1 a.m.u. = 1.672 x 10-27 kg 1 atm = 1.0133 x 10 5 Nm -2 = 760 Torr h = 6.626 x 10-34 Js For H 2 O
More informationME 501. Exam #2 2 December 2009 Prof. Lucht. Choose two (2) of problems 1, 2, and 3: Problem #1 50 points Problem #2 50 points Problem #3 50 points
1 Name ME 501 Exam # December 009 Prof. Lucht 1. POINT DISTRIBUTION Choose two () of problems 1,, and 3: Problem #1 50 points Problem # 50 points Problem #3 50 points You are required to do two of the
More informationExpress the transition state equilibrium constant in terms of the partition functions of the transition state and the
Module 7 : Theories of Reaction Rates Lecture 33 : Transition State Theory Objectives After studying this Lecture you will be able to do the following. Distinguish between collision theory and transition
More informationIntro/Review of Quantum
Intro/Review of Quantum QM-1 So you might be thinking I thought I could avoid Quantum Mechanics?!? Well we will focus on thermodynamics and kinetics, but we will consider this topic with reference to the
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 informationThermodynamics and Kinetics
Thermodynamics and Kinetics C. Paolucci University of Notre Dame Department of Chemical & Biomolecular Engineering What is the energy we calculated? You used GAMESS to calculate the internal (ground state)
More informationProblem #1 30 points Problem #2 30 points Problem #3 30 points Problem #4 30 points Problem #5 30 points
Name ME 5 Exam # November 5, 7 Prof. Lucht ME 55. POINT DISTRIBUTION Problem # 3 points Problem # 3 points Problem #3 3 points Problem #4 3 points Problem #5 3 points. EXAM INSTRUCTIONS You must do four
More informationrate of reaction forward conc. reverse time P time Chemical Equilibrium Introduction Dynamic Equilibrium Dynamic Equilibrium + RT ln f p
Chemical Equilibrium Chapter 9 of Atkins: Sections 9.1-9.2 Spontaneous Chemical Reactions The Gibbs Energy Minimum The reaction Gibbs energy Exergonic and endergonic reactions The Description of Equilibrium
More informationwhere R = universal gas constant R = PV/nT R = atm L mol R = atm dm 3 mol 1 K 1 R = J mol 1 K 1 (SI unit)
Ideal Gas Law PV = nrt where R = universal gas constant R = PV/nT R = 0.0821 atm L mol 1 K 1 R = 0.0821 atm dm 3 mol 1 K 1 R = 8.314 J mol 1 K 1 (SI unit) Standard molar volume = 22.4 L mol 1 at 0 C and
More information5.62 Physical Chemistry II Spring 2008
MIT OpenCourseWare http://ocw.mit.edu 5.62 Physical Chemistry II Spring 2008 For information about citing these materials or our Terms of Use, visit: http://ocw.mit.edu/terms. 5.62 Spring 2007 Lecture
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 informationIntro/Review of Quantum
Intro/Review of Quantum QM-1 So you might be thinking I thought I could avoid Quantum Mechanics?!? Well we will focus on thermodynamics and kinetics, but we will consider this topic with reference to the
More informationChapter 15 Thermal Properties of Matter
Chapter 15 Thermal Properties of Matter To understand the mole and Avogadro's number. To understand equations of state. To study the kinetic theory of ideal gas. To understand heat capacity. To learn and
More informationLecture 6 Free energy and its uses
Lecture 6 Free energy and its uses dg = VdP G - G o = PoP VdP G = G o (T) + RT ln P/P o for gases and G = G o (T) + V (P-P o ) for solids and liquids µ = µ o + RT ln P (for one mole) G = G o + RT ln Q
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 informationModule 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.
More informationChapter 19 Chemical Thermodynamics Entropy and free energy
Chapter 19 Chemical Thermodynamics Entropy and free energy Learning goals and key skills: Explain and apply the terms spontaneous process, reversible process, irreversible process, and isothermal process.
More informationThe 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
More informationaa + bb ---> cc + dd
17 Chemical Equilibria Consider the following reaction: aa + bb ---> cc + dd As written is suggests that reactants A + B will be used up in forming products C + D. However, what we learned in the section
More informationThe mathematical description of the motion of Atoms, Molecules & Other Particles. University of Rome La Sapienza - SAER - Mauro Valorani (2007)
The mathematical description of the motion of Atoms, Molecules Other Particles Particle Dynamics Mixture of gases are made of different entities: atoms, molecules, ions, electrons. In principle, the knowledge
More informationThermodynamics. Chem 36 Spring The study of energy changes which accompany physical and chemical processes
Thermodynamics Chem 36 Spring 2002 Thermodynamics The study of energy changes which accompany physical and chemical processes Why do we care? -will a reaction proceed spontaneously? -if so, to what extent?
More informationChemistry 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
More informationGeneral Chemistry revisited
General Chemistry revisited A(g) + B(g) C(g) + D(g) We said that G = H TS where, eg, H = f H(C) + f H(D) - f H(A) - f H(B) G < 0 implied spontaneous to right G > 0 implied spontaneous to left In a very
More informationPhysical Chemistry Chapter 6 Chemical Kinetics
Physical Chemistry Chapter 6 Chemical Kinetics by Azizul Helmi Sofian Faculty of Chemical & Natural Resources Engineering azizulh@ump.edu.my Chapter Description Aims To define rate laws accordingly To
More informationStatistical thermodynamics for MD and MC simulations
Statistical thermodynamics for MD and MC simulations knowing 2 atoms and wishing to know 10 23 of them Marcus Elstner and Tomáš Kubař 22 June 2016 Introduction Thermodynamic properties of molecular systems
More informationGherman Group Meeting. Thermodynamics and Kinetics and Applications. June 25, 2009
Gherman Group Meeting Thermodynamics and Kinetics and Applications June 25, 2009 Outline Calculating H f, S, G f Components which contribute to H f, S, G f Calculating ΔH, ΔS, ΔG Calculating rate constants
More informationChpt 19: Chemical. Thermodynamics. Thermodynamics
CEM 152 1 Reaction Spontaneity Can we learn anything about the probability of a reaction occurring based on reaction enthaplies? in general, a large, negative reaction enthalpy is indicative of a spontaneous
More informationPractice Questions Placement Exam for Entry into Chemistry 120
Practice Questions Placement Exam for Entry into Chemistry 120 Potentially Useful Information Avogadro's number = 6.0221420 10 23 h = 6.6260688 10 34 J s c = 2.9979246 10 8 m/s 1amu = 1.6605387 10 27 kg
More informationStatistical Mechanics
Statistical Mechanics Newton's laws in principle tell us how anything works But in a system with many particles, the actual computations can become complicated. We will therefore be happy to get some 'average'
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 informationChapter 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
More informationEffect 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
More informationChapter 3 - First Law of Thermodynamics
Chapter 3 - dynamics The ideal gas law is a combination of three intuitive relationships between pressure, volume, temp and moles. David J. Starling Penn State Hazleton Fall 2013 When a gas expands, it
More informationRate of Heating and Cooling
Rate of Heating and Cooling 35 T [ o C] Example: Heating and cooling of Water E 30 Cooling S 25 Heating exponential decay 20 0 100 200 300 400 t [sec] Newton s Law of Cooling T S > T E : System S cools
More informationExam 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.
More informationEntropy, Free Energy, and Equilibrium
Entropy, Free Energy, and Equilibrium Chapter 17 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Spontaneous Physical and Chemical Processes A waterfall runs
More informationUNIT 15: THERMODYNAMICS
UNIT 15: THERMODYNAMICS ENTHALPY, DH ENTROPY, DS GIBBS FREE ENERGY, DG ENTHALPY, DH Energy Changes in Reactions Heat is the transfer of thermal energy between two bodies that are at different temperatures.
More informationCHAPTER 9 LECTURE NOTES
CHAPTER 9 LECTURE NOTES 9.1, 9.2: Rate of a reaction For a general reaction of the type A + 3B 2Y, the rates of consumption of A and B, and the rate of formation of Y are defined as follows: Rate of consumption
More informationChemical Kinetics. Chapter 13. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Chemical Kinetics Chapter 13 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Chemical Kinetics Thermodynamics does a reaction take place? Kinetics how fast does
More informationChemistry 1A, Fall 2003 Midterm 1 Sept 16, 2003 (90 min, closed book)
Name: SID: TA Name: Chemistry 1A, Fall 2003 Midterm 1 Sept 16, 2003 (90 min, closed book) This exam has 38 multiple choice questions. Fill in the Scantron form AND circle your answer on the exam. Each
More informationReaction Dynamics (2) Can we predict the rate of reactions?
Reaction Dynamics (2) Can we predict the rate of reactions? Reactions in Liquid Solutions Solvent is NOT a reactant Reactive encounters in solution A reaction occurs if 1. The reactant molecules (A, B)
More informationCharacteristics of Chemical Equilibrium. Equilibrium is Dynamic. The Equilibrium Constant. Equilibrium and Catalysts. Chapter 14: Chemical Equilibrium
Characteristics of Chemical Equilibrium Chapter 14: Chemical Equilibrium 008 Brooks/Cole 1 008 Brooks/Cole Equilibrium is Dynamic Equilibrium is Independent of Direction of Approach Reactants convert to
More informationEnergy Barriers and Rates - Transition State Theory for Physicists
Energy Barriers and Rates - Transition State Theory for Physicists Daniel C. Elton October 12, 2013 Useful relations 1 cal = 4.184 J 1 kcal mole 1 = 0.0434 ev per particle 1 kj mole 1 = 0.0104 ev per particle
More informationChemical Thermodynamics. Chapter 18
Chemical Thermodynamics Chapter 18 Thermodynamics Spontaneous Processes Entropy and Second Law of Thermodynamics Entropy Changes Gibbs Free Energy Free Energy and Temperature Free Energy and Equilibrium
More informationTODAY 0. Why H = q (if p ext =p=constant and no useful work) 1. Constant Pressure Heat Capacity (what we usually use)
361 Lec 7 Fri 9sep15 TODAY 0. Why H = q (if p ext =p=constant and no useful work) 1. Constant Pressure Heat Capacity (what we usually use) 2. Heats of Chemical Reactions: r H (mechanics of obtaining from
More informationUnusual Entropy of Adsorbed Methane on Zeolite Templated Carbon. Supporting Information. Part 2: Statistical Mechanical Model
Unusual Entropy of Adsorbed Methane on Zeolite Templated Carbon Supporting Information Part 2: Statistical Mechanical Model Nicholas P. Stadie*, Maxwell Murialdo, Channing C. Ahn, and Brent Fultz W. M.
More informationStatistical thermodynamics L1-L3. Lectures 11, 12, 13 of CY101
Statistical thermodynamics L1-L3 Lectures 11, 12, 13 of CY101 Need for statistical thermodynamics Microscopic and macroscopic world Distribution of energy - population Principle of equal a priori probabilities
More informationMolar Specific Heat of Ideal Gases
Molar Specific Heat of Ideal Gases Since Q depends on process, C dq/dt also depends on process. Define a) molar specific heat at constant volume: C V (1/n) dq/dt for constant V process. b) molar specific
More informationSome properties of the Helmholtz free energy
Some properties of the Helmholtz free energy Energy slope is T U(S, ) From the properties of U vs S, it is clear that the Helmholtz free energy is always algebraically less than the internal energy U.
More informationFoundations of Chemical Kinetics. Lecture 30: Transition-state theory in the solution phase
Foundations of Chemical Kinetics Lecture 30: Transition-state theory in the solution phase Marc R. Roussel Department of Chemistry and Biochemistry Transition-state theory in solution We revisit our original
More informationThermochemistry in Gaussian
Thermochemistry in Gaussian Joseph W. Ochterski, Ph.D. help@gaussian.com c 2000, Gaussian, Inc. June 2, 2000 Abstract The purpose of this paper is to explain how various thermochemical values are computed
More informationCh 17 Free Energy and Thermodynamics - Spontaneity of Reaction
Ch 17 Free Energy and Thermodynamics - Spontaneity of Reaction Modified by Dr. Cheng-Yu Lai spontaneous nonspontaneous Spontaneous Processes Processes that are spontaneous in one direction are nonspontaneous
More informationExam 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
More informationLecture 6 Free Energy
Lecture 6 Free Energy James Chou BCMP21 Spring 28 A quick review of the last lecture I. Principle of Maximum Entropy Equilibrium = A system reaching a state of maximum entropy. Equilibrium = All microstates
More informationChemical Kinetics and Equilibrium
Chemical Kinetics and Equilibrium Part 1: Kinetics David A. Katz Department of Chemistry Pima Community College Tucson, AZ USA Chemical Kinetics The study of the rates of chemical reactions and how they
More informationPhysical Chemistry I CHEM 4641 Final Exam 13 questions, 30 points
Physical Chemistry I CHEM 4641 Final Exam 13 questions, 30 points Name: KEY Gas constant: R = 8.314 J mol -1 K -1 = 0.008314 kj mol -1 K -1. Boltzmann constant k = 1.381 10-23 J/K = 0.6950 cm -1 /K h =
More informationME 262A - Physical Gas Dynamics 1996 Final Exam: Open Book Portion. h = 6.62 x J s Energy conversion factor: 1 calorie = 4.
Name: ME 262A - Physical Gas Dynamics 1996 Final Exam: Open Book Portion Useful data and information: k = 1.38 x 10-23 J/K h = 6.62 x 10-34 J s Energy conversion factor: 1 calorie = 4.2 J 1. (40 points)
More informationChemistry 1A, Fall 2003 Midterm 2 Oct 14, 2003 (90 min, closed book)
Name: SID: TA Name: Chemistry 1A, Fall 2003 Midterm 2 Oct 14, 2003 (90 min, closed book) This exam has 45 multiple choice questions. Fill in the Scantron form AND circle your answer on the exam. Each question
More informationLecture 20. Chemical Potential
Lecture 20 Chemical Potential Reading: Lecture 20, today: Chapter 10, sections A and B Lecture 21, Wednesday: Chapter 10: 10 17 end 3/21/16 1 Pop Question 7 Boltzmann Distribution Two systems with lowest
More informationStatistical and Thermal Physics. Problem Set 5
Statistical and Thermal Physics xford hysics Second year physics course Dr A. A. Schekochihin and Prof. A. T. Boothroyd (with thanks to Prof. S. J. Blundell Problem Set 5 Some useful constants Boltzmann
More informationPractice Questions Placement Exam for Exemption from Chemistry 120
Practice Questions Placement Exam for Exemption from Chemistry 120 Potentially Useful Information Avogadro's number = 6.0221420 10 23 h = 6.6260688 10 34 J s c = 2.9979246 10 8 m/s 1amu = 1.6605387 10
More informationTHERMODYNAMICS I. TERMS AND DEFINITIONS A. Review of Definitions 1. Thermodynamics = Study of the exchange of heat, energy and work between a system
THERMODYNAMICS I. TERMS AND DEFINITIONS A. Review of Definitions 1. Thermodynamics = Study of the exchange of heat, energy and work between a system and its surroundings. a. System = That part of universe
More informationDisorder and Entropy. Disorder and Entropy
Disorder and Entropy Suppose I have 10 particles that can be in one of two states either the blue state or the red state. How many different ways can we arrange those particles among the states? All particles
More informationWhat s free about Gibbs free energy?
What s free about Gibbs free energy? The change in free energy for a process equals the maximum work that can be done by the system on the surroundings in a spontaneous process occurring at constant temperature
More informationThermodynamics: Entropy, Free Energy, and Equilibrium
Chapter 16 Thermodynamics: Entropy, Free Energy, and Equilibrium spontaneous nonspontaneous In this chapter we will determine the direction of a chemical reaction and calculate equilibrium constant using
More informationAP CHEMISTRY SCORING GUIDELINES
Mean 5.64 out of 9 pts AP CHEMISTRY Question 1 CO(g) + 1 2 O 2 (g) CO 2 (g) 1. The combustion of carbon monoxide is represented by the equation above. (a) Determine the value of the standard enthalpy change,
More informationChapter 4 Rigid Models and Angular Momentum Eigenstates Homework Solutions
Capter 4 Rigid Models and Angular Momentum Eigenstates Homework Solutions 1. A i j k B i 4j k AB AB AB AB()() ( 1)(4) ()( ) 4 x x y y z z i j k i j k AxB A A A 1 x y z Bx By Bz 4 i j k 5i 1 j 14k ( 1)(
More informationPreliminary Examination - Day 2 August 16, 2013
UNL - Department of Physics and Astronomy Preliminary Examination - Day August 16, 13 This test covers the topics of Quantum Mechanics (Topic 1) and Thermodynamics and Statistical Mechanics (Topic ). Each
More informationCHEMICAL THERMODYNAMICS
DEPARTMENT OF APPLIED CHEMISTRY LECTURE NOTES 6151- ENGINEERING CHEMISTRY-II UNIT II CHEMICAL THERMODYNAMICS Unit syllabus: Terminology of thermodynamics - Second law: Entropy - entropy change for an ideal
More information09 Intro to Mass Dependent Fractionation
09 Intro to Mass Dependent Fractionation Reading: White #26 Valley and Cole, Chapter 1 Guide Questions: 1) In a general sense why do heavier isotopes of an element behave differently from lighter isotopes?
More informationCH1101 Physical Chemistry Tutorial 1. Prof. Mike Lyons.
CH111 Physical Chemistry Tutorial 1. Prof. Mike Lyons. CH111 Section A Annual 1 Internal Energy Units: Joules J Internal Energy (U) : total kinetic & potential energy of system. e.g. Gas in container with
More informationIT IS THEREFORE A SCIENTIFIC LAW.
Now we talk about heat: Zeroth Law of Thermodynamics: (inserted after the 3 Laws, and often not mentioned) If two objects are in thermal equilibrium with a third object, they are in thermal equilibrium
More informationWorkshop 4: Diatomic molecule vibrational and rotational spectra CH351 Physical Chemistry, Fall 2004
Workshop 4: Diatomic molecule vibrational and rotational spectra CH35 Physical Chemistry, Fall 004 http://quantum.bu.edu/courses/ch35/pltl/4.pdf Last updated Monday, November 9, 004 6:59:3-05:00 Copyright
More informationA.P. Chemistry Rates of Reaction Chapter 12 : page 526
A.P. Chemistry Rates of Reaction Chapter 12 : page 526 I. Chemical Kinetics A. Definition- B. Requirements for a chemical reaction 1. 2. 3. II. Reaction Rates A. Rate of a reaction- B. Example: 2 N 2 O
More informationCY T. Pradeep. Lectures 11 Theories of Reaction Rates
CY1001 2015 T. Pradeep Lectures 11 Theories of Reaction Rates There are two basic theories: Collision theory and activated complex theory (transition state theory). Simplest is the collision theory accounts
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 informationADIABATIC PROCESS Q = 0
THE KINETIC THEORY OF GASES Mono-atomic Fig.1 1 3 Average kinetic energy of a single particle Fig.2 INTERNAL ENERGY U and EQUATION OF STATE For a mono-atomic gas, we will assume that the total energy
More informationSupplementary Online Materials: Formation of Stoichiometric CsF n Compounds
1 2 3 4 5 6 7 8 9 1 11 12 13 Supplementary Online Materials: Formation of Stoichiometric CsF n Compounds Qiang Zhu, 1, a) Artem R. Oganov, 1, 2, 3 and Qingfeng Zeng 4 1) Department of Geosciences, Stony
More informationCHAPTER 21: Reaction Dynamics
CHAPTER 21: Reaction Dynamics I. Microscopic Theories of the Rate Constant. A. The Reaction Profile (Potential Energy diagram): Highly schematic and generalized. A---B-C B. Collision Theory of Bimolecular
More information5.62 Physical Chemistry II Spring 2008
MIT OpenCourseWare http://ocw.mit.edu 5.6 Physical Chemistry II Spring 8 For information about citing these materials or our Terms of Use, visit: http://ocw.mit.edu/terms. 5.6 Lecture #17: Chemical Equilibrium.
More informationAn Aside: Application of Rotational Motion. Vibrational-Rotational Spectroscopy
An Aside: Application of Rotational Motion Vibrational-Rotational Spectroscopy Rotational Excited States of a Diatomic Molecule are Significantly Populated at Room Temperature We can estimate the relative
More informationMME 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
More informationAdvanced Physical Chemistry CHAPTER 18 ELEMENTARY CHEMICAL KINETICS
Experimental Kinetics and Gas Phase Reactions Advanced Physical Chemistry CHAPTER 18 ELEMENTARY CHEMICAL KINETICS Professor Angelo R. Rossi http://homepages.uconn.edu/rossi Department of Chemistry, Room
More informationC h a p t e r 13. Chemical Equilibrium
C h a p t e r 13 Chemical Equilibrium Chemical equilibrium is achieved when: the rates of the forward and reverse reactions are equal and the concentrations of the reactants and products remain constant
More informationChemical Kinetics. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Chemical Kinetics Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Chemical Kinetics Thermodynamics does a reaction take place? Kinetics how fast does a reaction
More informationPreliminary Examination - Day 2 August 15, 2014
UNL - Department of Physics and Astronomy Preliminary Examination - Day 2 August 15, 2014 This test covers the topics of Thermodynamics and Statistical Mechanics (Topic 1) and Mechanics (Topic 2). Each
More informationChapter 19. Entropy, Free Energy, and Equilibrium
Chapter 19 Entropy, Free Energy, and Equilibrium Spontaneous Physical and Chemical Processes A waterfall runs downhill A lump of sugar dissolves in a cup of coffee At 1 atm, water freezes below 0 0 C and
More informationChapter: Chemical Kinetics
Chapter: Chemical Kinetics Rate of Chemical Reaction Question 1 Nitrogen pentaoxide decomposes according to equation: This first order reaction was allowed to proceed at 40 o C and the data below were
More informationChemistry 431. Lecture 27 The Ensemble Partition Function Statistical Thermodynamics. NC State University
Chemistry 431 Lecture 27 The Ensemble Partition Function Statistical Thermodynamics NC State University Representation of an Ensemble N,V,T N,V,T N,V,T N,V,T N,V,T N,V,T N,V,T N,V,T N,V,T N,V,T N,V,T N,V,T
More informationMS212 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
More informationAP Chemistry. Free-Response Questions
2018 AP Chemistry Free-Response Questions College Board, Advanced Placement Program, AP, AP Central, and the acorn logo are registered trademarks of the College Board. AP Central is the official online
More informationLecture 28 Thermodynamics: Gibbs Free Energy, Equilibrium Constants and the Entropy Change for a Bimolecular Reaction
Physical Principles in Biology Biology 3550 Fall 2017 Lecture 28 Thermodynamics: Gibbs Free Energy, Equilibrium Constants and the Entropy Change for a Bimolecular Reaction Monday, 6 November c David P.
More information1 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 =
More informationThe 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
More information