Fundamental relations: The thermodynamic functions The molecular partition function Using statistical thermodynamics Mean energies Heat capacities Equation.

Slides:



Advertisements
Similar presentations
15.5 Electronic Excitation
Advertisements

The Heat Capacity of a Diatomic Gas
The Kinetic Theory of Gases
Pressure and Kinetic Energy
Statistical Mechanics
Nankai University Song Feng Chapter 4 Boltzman Distribution in infirm-coupling system Prof. Song
CHAPTER 14 THE CLASSICAL STATISTICAL TREATMENT OF AN IDEAL GAS.
EQUILIBRIUM AND KINETICS. Mechanical Equilibrium of a Rectangular Block Centre Of Gravity Potential Energy = f(height of CG) Metastable state Unstable.
6.5.Gaseous Systems Composed of Molecules with Internal Motion Assumptions ( ideal Boltzmannian gas ) : 1. Molecules are free particles ( non-interacting).
MSEG 803 Equilibria in Material Systems 10: Heat Capacity of Materials Prof. Juejun (JJ) Hu
The entropy, S, of a system quantifies the degree of disorder or randomness in the system; larger the number of arrangements available to the system, larger.
Statistical Mechanics
Copyright 1999, PRENTICE HALLChapter 191 Chemical Thermodynamics Chapter 19 David P. White University of North Carolina, Wilmington.
Intro/Review of Quantum
CHE-20028: PHYSICAL & INORGANIC CHEMISTRY
Heat Capacity Amount of energy required to raise the temperature of a substance by 1C (extensive property) For 1 mol of substance: molar heat capacity.
15.4 Rotational modes of diatomic molecules The moment of inertia, where μ is the reduced mass r 0 is the equilibrium value of the distance between the.
Partition Functions for Independent Particles
Vibrational and Rotational Spectroscopy
Vibrational Spectroscopy
Ch 23 pages Lecture 15 – Molecular interactions.
Molecular Information Content
The Helmholtz free energyplays an important role for systems where T, U and V are fixed - F is minimum in equilibrium, when U,V and T are fixed! by using:
Physical Chemistry IV The Use of Statistical Thermodynamics
Exam I results.
Spontaneity, Entropy, and Free Energy
Chapter 20: Thermodynamics
First Law of Thermodynamics  You will recall from Chapter 5 that energy cannot be created nor destroyed.  Therefore, the total energy of the universe.
Prentice Hall © 2003Chapter 19 Chapter 19 Chemical Thermodynamics CHEMISTRY The Central Science 9th Edition David P. White.
Rate Theories of elementary reaction. 2 Transition state theory (TST) for bimolecular reactions Theory of Absolute reaction Rates Theory of activated.
Ideal diatomic gas: internal degrees of freedom
Lecture 9 Energy Levels Translations, rotations, harmonic oscillator
Diatomic and Polyatomic Gases
The Ideal Monatomic Gas. Canonical ensemble: N, V, T 2.
Prentice Hall © 2003Chapter 19 Chapter 19 Chemical Thermodynamics CHEMISTRY The Central Science 9th Edition.
Molecular Partition Function
Summary Boltzman statistics: Fermi-Dirac statistics:
Lecture 16 – Molecular interactions
Partition functions of ideal gases. We showed that if the # of available quantum states is >> N The condition is valid when Examples gases at low densities.
Chapter 14: The Classical Statistical Treatment of an Ideal Gas.
Chemistry 231 Thermodynamics in Reacting Systems.
Chapter 19 Statistical thermodynamics: the concepts Statistical Thermodynamics Kinetics Dynamics T, P, S, H, U, G, A... { r i},{ p i},{ M i},{ E i} … How.
CHE-20028: PHYSICAL & INORGANIC CHEMISTRY
Monatomic Crystals.
CHE 116 No. 1 Chapter Nineteen Copyright © Tyna L. Meeks All Rights Reserved.
Review Of Statistical Mechanics Continued
The Heat Capacity of a Diatomic Gas Chapter Introduction Statistical thermodynamics provides deep insight into the classical description of a.
The Ideal Diatomic and Polyatomic Gases. Canonical partition function for ideal diatomic gas Consider a system of N non-interacting identical molecules:
Lecture 26 — Review for Exam II Chapters 5-7, Monday March 17th
Chemistry 101 : Chap. 19 Chemical Thermodynamics (1) Spontaneous Processes (2) Entropy and The Second Law of Thermodynamics (3) Molecular Interpretation.
Prentice Hall © 2003Chapter 19 Chapter 19 Chemical Thermodynamics CHEMISTRY The Central Science 9th Edition David P. White.
Physical Behavior of Matter Review. Matter is classified as a substance or a mixture of substances.
THERMODYNAMICS – ENTROPY AND FREE ENERGY 3A-1 (of 14) Thermodynamics studies the energy of a system, how much work a system could produce, and how to predict.
Advanced Thermochemistry Mrs. Stoops Chemistry. Chapter Problems Ch 19 p742: 16, 20, 28, 34, 38, 40, 46, 52, 56, 58, 75, 93.
In the mid-1800s, Mayer, Helmholtz, and Joule discovered independently that heat is simply a form of energy. 1853: Wiedemann and Franz law (good.
MIT Microstructural Evolution in Materials 4: Heat capacity
Reaction Rate Theory D E reaction coordinate + k A B AB.
15.4 Rotational modes of diatomic molecules
Chapter 6 Applications of
Physical Behavior of Matter Review
Solution of Thermodynamics: Theory and applications
The units of g(): (energy)-1
Thermochemistry Test Review
Physical Chemistry IV The Use of Statistical Thermodynamics
Reminder: Chemical Equilibrium
Polyatomic Ideal Gases “Borrowed” from various sources on the web!
Equilibrium and Kinetics
MIT Microstructural Evolution in Materials 4: Heat capacity
Chapter 5 - Phonons II: Quantum Mechanics of Lattice Vibrations
Topics 5 & 15 Chemical Thermodynamics
Presentation transcript:

Fundamental relations: The thermodynamic functions The molecular partition function Using statistical thermodynamics Mean energies Heat capacities Equation of state Residual entropies Equilibrium constants Chapter 20 Statistical thermodynamics: the machinery

Exercises for Chapter (b), 20.3(a), 20.6(a), 20.10(b), 20.12(a), 20.15(b),20.17(a) 20.3, 20.6, 20.10, 20.16, 20.19

Fundamental relations The thermodynamic functions The molecular partition function

The thermodynamic functions: A and p The Helmholtz energy Independent molecules: (Distinguishable) (Indistinguishable) A= U - TS A(0)=U(0) The pressure

Thermodynamic Riddles (Ch.5) dU=TdS-pdV, dH=TdS+Vdp dG=Vdp-SdT, dA=-SdT-pdV Enjoy!! U=q+w, H=U+pV, G=H-TS, A=U-TS

Deriving an equation of state Derive the expression for the pressure of a gas of independent particles For a gas of independent particles: Where following relations have been used:

Classroom exercise Deriving the equation of state of a sample for which With where f depends on the volume

The thermodynamic function: H H=U+pV  For a gas of independent particles:

The thermodynamic functions: G G=H-TS=A+pV  For a gas of independent particles: G=A+pV  Or Define molar partition function

The molecular partition function Translational, Rotational, Vibrational, Electronic energies

The translational contribution At room temperature, O 2 in a vessel of 100 ml At room temperature, H 2

Independent states (  factorization of q) Three-dimensional box: Thermal wavelength (Translational partition function)

Typical Rotors

The Rotational Energy Levels Around a fixed-axis Around a fixed-point (Spherical Rotors)

Linear Rotors

The rotational contribution hcB/kT= At room temperature, for H(1)Cl(35), B= /cm kT/hc= /cm (Linear rotors)

The rotational contribution: Approximation (Linear rotors) hcB/kT<<1

Symmetric Rotors

The rotational contribution: Approximation (Symmetric rotors) hcB/kT<<1

J K J K =

The rotational contribution: Approximation (Symmetric rotors)

The rotational contribution: Approximation (Asymmetric rotors) (If you have question here, just ignore it. The detailed derivation of this equation is beyond the Scope of this course.)

Rotational temperature The ``high temperature`` approximation means From Table 20.1, it is clear that this approximation is indeed valid unless the temperature is not too low (< ~10K).

Symmetry number How to avoid overestimating the rotational partition function? Symmetrical linear rotor After deducting the indistinguishable States, In general,

Symmetry number Nonlinear molecules: General cases: the number of rotational symmetry elements.

Symmetry Group and Symmetry Numbers C1C1 CICI CS:CS:1 D2D2 D2dD2d D2h:D2h:4 C : 1 C2C2 C2vC2v C2h:C2h:2 D3D3 D3dD3d D3h:D3h:6 D : 2 C3C3 C3vC3v C3h:C3h:3 D4D4 D4dD4d D4h:D4h:8 T, T h T d :12 C4C4 C4vC4v C4h:C4h:4 D5D5 D5dD5d D5h:D5h:10 O, O h :24 C5C5 C5vC5v C5h:C5h:5 D6D6 D6dD6d D6h:D6h:12 I, I h :60 C6C6 C6vC6v C6h:C6h:6 D7D7 D7dD7d D7h:D7h:14 S4:S4:2 C7C7 C7vC7v C7h:C7h:7 D8D8 D8dD8d D8h:D8h:16 S6:S6:3 C8C8 C8vC8v C8h:C8h:8 S8:S8:4

A= /cm, B= /cm, C= /cm, T=298 K ABC= /cm

Classroom exercise N A= /cm, B= /cm, C= /cm, T=298 K ABC= /cm

Quantum mechanical interpretation The wavefunction of fermions changes sign when exchanged whereas the wavefunction of bosons does not change sign when exchanged.

(for even J) (for odd J)

CO 2 Nuclear spin = 0 Only even J-states are admissible CO 2  Boson

Quantum mechanical interpretation There are 8 nuclear spin states:

Quantum mechanical interpretation

Generally, for a molecule with N R rotational elements (including the identity operation), the symmetry number Quantum mechanical interpretation

Symmetry Group and Symmetry Numbers C1C1 CICI CS:CS:1 D2D2 D2dD2d D2h:D2h:4 C : 1 C2C2 C2vC2v C2h:C2h:2 D3D3 D3dD3d D3h:D3h:6 D : 2 C3C3 C3vC3v C3h:C3h:3 D4D4 D4dD4d D4h:D4h:8 T, T h T d :12 C4C4 C4vC4v C4h:C4h:4 D5D5 D5dD5d D5h:D5h:10 O, O h :24 C5C5 C5vC5v C5h:C5h:5 D6D6 D6dD6d D6h:D6h:12 I, I h :60 C6C6 C6vC6v C6h:C6h:6 D7D7 D7dD7d D7h:D7h:14 S4:S4:2 C7C7 C7vC7v C7h:C7h:7 D8D8 D8dD8d D8h:D8h:16 S6:S6:3 C8C8 C8vC8v C8h:C8h:8 S8:S8:4

10 points!! Derive from quantum mechanics the symmetry number of benzene:

The vibrational contribution v = 0, 1, 2,

Normal modes 3N-6 vibrational degrees of freedom For a nonlinear molecule of N atoms, there are 3N degrees of freedom: 3 translatinal, 3 rotational and For a linear molecule of N atoms, there are 3N degrees of freedom: 3 translatinal, 2 rotational and 3N-5 vibrational degrees of freedom The total vibrational partition function is:

Exercise The wave number of the three vibrational modes of H 2 O /cm, /cm, and /cm. Calculate vibrational partition function at 1500 K. The total vibrational partition function then is: 1.031x1.276x1.028=1.353 At 1500 K, most molecules are at their vibrational ground state!

Classroom exercise The three vibrational normal modes of CO 2 are /cm, /cm (doubly degenerate), /cm. Calculate the vibrational partition function at 1500K.

Low temperature approximation High temperature approximation Only the zero-point level is occupied.

The electronic contribution For most cases, the excited energy is much larger than kT and the electronic energy level of the ground is not degenerate:

Degenerate case: NO

The overall partition function elec vib rot (Linear rotor, Single vib mode) (Nonlinear rotor, multiple vib mode)

m M=N A *m

Exercise Calculate the value of molar Gibbs energy for H2O(g) at 1500 K given that A= /cm, B= /cm, and C= /cm and the information of normal modes given in last exercise.

Classroom Exercise Calculate the value of molar Gibbs energy for CO2(g) at 1500 K given that B= /cm. The three vibrational normal modes of CO2 are /cm, /cm (doubly degenerate), /cm

Classroom Exercise Calculate the value of molar Gibbs energy for CO2(g) at 1500 K given that B= /cm. The three vibrational normal modes of CO2 are /cm, /cm (doubly degenerate), /cm

II. Using statistical thermodynamics Mean energies Heat capacities Equation of state Residual entropies Equilibrium constants

Mean energies M=T,R,V,orE The mean translational energy 1D case: 3D case:

The mean rotational energy (Linear rotors)

The mean rotational energy At high temperature, the partition function of a linear rotor: Classroom exercise: the mean rotational energy of an asymmetric rotor at high temperature:

The mean vibrational energy

Heat capacities Translational contribution:

The rotational contribution: At high temperature: Common cases

At low temperature: The vibrational contribution: Common cases Rare cases: Cv,m  R

The overall heat capacity At fairly high temperature, the vibrational contribution Is cloase to zero: Common cases: θ R <<T<<θ V

The overall heat capacity (diatomic molecules) Common cases

Exercise Estimate the molar constant-volume heat capacity of water vapor at 100C. The wave number of the three vibrational modes of H 2 O: /cm, /cm, and /cm. The rotational constants of H2O: A=27.9 1/cm, B=14.5 1/cm And C=9.3 1/cm. Common cases: θ R <<T<<θ V Experimental value: 26.1 J/mol/K

Classroom Exercise Estimate the molar constant-volume heat capacity of gaseous I 2 at 25C. The rotational constants of I 2 : B= /cm. A rare case: θ V ~ T

Classroom Exercise Estimate the molar constant-volume heat capacity of gaseous I 2 at 25C. The rotational constants of I 2 : B= /cm. A rare case: θ V ~ T, C v,m  R Experimental value: J/mol/K

Equations of state Equation of state of perfect gas: For real gases, The purpose: to find expressions for B and C in terms of the intermolecular interactions. For perfect gases, N! should be dropped for systems of distinguishable particles.

Deriving an equation of state Derive the expression for the pressure of a gas of independent particles For a gas of independent particles: Where following relations have been used:

Pair interactions Further approximation:

Mayer function

Second virial coefficient B

Second virial coefficient B (spherical potential) The interaction potential depends on distance only.

Second virial coefficient B (Hard sphere potential) when r ≦ σ, E p = ∞: when r ≧ σ,E p = 0: σ

Application of virial coefficient B For perfect gases, all virial coefficients except the first one are zero. The thermodynamic properties that depend on intermolecular interactions are determined by second and higher order virial coefficients. (Classroom Exercise)

Answer

Residual entropy The entropy (disorder) at temperature zero. AB BAAB BA S=0 S>0 There are 2^N microscopic states for N molecules with two equally possible orientations at T=0 

General cases ABC ACBABC BAC There are s equally possible orientations at T=0:

The residual entropy of ice HOH H2O is nonlinear Hydrogen bonds are oriented. The acceptable arrangement: Out of the four hydrogen atoms around an oxygen atom, two are close and two are far.

There are sixteen (2^4) equally possible configurations for ice, but only six of them are allowed.

Equilibrium constants (gas-phase reactions) For species J, aA+bB+ …  cC+dD+ …

Standard reaction Gibbs energy G(0)=U(0) 

X 2 (g)→2X(g) A dissociation equilibrium (dissociation energy of bond X-X)

Equilibrium constant: an example Evaluate the equilibrium constant for the dissociation Na 2 (g)  2Na(g) at 1000 K with data: B= /cm, v= /cm, D 0 =70.4 kJ/mol. The Na atoms have doublet ground terms.

Classroom exercise Evaluate the equilibrium constant for the dissociation Na 2 (g)  2K(g) at 1500 K with data: B= /cm, v= /cm, D 0 =70.4 kJ/mol. The Na atoms have doublet ground terms.

Contributions to the equilibrium constant: density of states Gas-phase reaction: The density of states== The number of states in a given range of energy:

Similar densities of states for products and reactants The equilibrium is dominated by the species with lower zero- point energy.

Very different densities of states The equilibrium is dominated by the species with larger density of states.

Contributions to the equilibrium constant The number ratio of product to reactant molecules: which leads to the equilibrium constant:

Proof

Energy separation and state density on equilibria Gibss energy, rather than enthalpy, controls position of equilibrium.

Helix structure of polypeptides (proteins)

Helix-coil transition h c

The statistical physics of helix-coil transition: a tetrapeptide hhhh hhch hchh chhh hhhc cchh chch hchc hcch chhc hhcc cchc chcc hccc ccch cccc (stability parameter)

Helix-coil transition of proteins with n amino acid residues hhhhhchhchhh … hhhhhchhchhhhhhhcchhcchhhhhhhchcchhhhhhhhchhchhh Zipper model:

Zipper model hhhhhchhhchhhhhhhchhcchhhhhchchhcchhhccchchhcchh The coils are necessarily in a contiguous region.

Zipper model hhhhhchhhhhhhhhhhchhchhh Nucleation with equilibrium constant σ<<1. The number of possibilities of placing a coil with i amino acids In a peptide of n amino acids: n-i+1 cchhhchhhhhhhcchhchhhhhhhhcchchhhhhh

Degree of conversion (Classroom exercise)

Zimm-Bragg model hhcchchhhhcc Separate coil regions are considered