Classical Thermodynamics of Solutions

Slides:

Advertisements

Similar presentations

Lecture 24 Chemical equilibrium Equilibrium constant Dissociation of diatomic molecule Heterophase reactions.

Advertisements

Electrolyte Solutions - Debye-Huckel Theory

We will call μ the Chemical Potential Right now we will think of it as the molar free energy, but we will refine this definition later… Free Energy.

Department of Mechanical Engineering ME 322 – Mechanical Engineering Thermodynamics Lecture 32 Ideal Gas Mixtures II.

Solutions of Nonelectrolytes

CHEMICAL AND PHASE EQUILIBRIUM (1)

Department of Civil & Environmental Engineering

Solutions Lecture 6. Clapeyron Equation Consider two phases - graphite & diamond–of one component, C. Under what conditions does one change into the other?

For a closed system consists of n moles, eq. (1.14) becomes: (2.1) This equation may be applied to a single-phase fluid in a closed system wherein no.

Advanced Thermodynamics Note 11 Solution Thermodynamics: Applications

Properties of Solutions. Concentration Terms Dilute - not a lot of solute. Concentrated - a large amount of solute. Concentration can be expressed quantitatively.

Chemical Thermodynamics 2013/ th Lecture: Thermodynamics of Simple Mixtures Valentim M B Nunes, UD de Engenharia.

Lecture 18Multicomponent Phase Equilibrium1 Theories of Solution The Gibbs energy of mixing is given by: And the chemical potential is: For ideal gases,

Thermodynamic Property Relations

System. surroundings. universe.

The Advanced Chemical Engineering Thermodynamics The variables (thermodynamic properties) and the equations in thermodynamics Q&A -2- 9/22/2005(2) Ji-Sheng.

Solution thermodynamics theory—Part IV

Chapter 19 Chemical Thermodynamics

Now we are going to start looking at models for the chemical potential mi of a given component i in a mixture The first model is the ideal gas mixture.

Chemistry Thermodynamics Lecture 13 : Non Ideal Solutions and Activity Lecture 14 : Chemical Equilibria Lecture 15 : Kinetic Coefficients & the.

Thermodynamics of Multi-component Systems Consider a binary solid solution of A and B atoms: Let n A = # of moles of A n B = # of moles of B def:mole(or.

1 The Laws of Thermodynamics in Review 1.The internal energy* of an isolated system is constant. There are only two ways to change internal energy – heat.

Notation convention Let G' stand for total free energy and in a similar fashion S', V', H', etc. Then we will let = G'/n represent the free energy per.

Chemical Thermodynamics II Phase Equilibria

Chapter 19 Chemical Thermodynamics Lecture Presentation John D. Bookstaver St. Charles Community College Cottleville, MO © 2012 Pearson Education, Inc.

Thermodynamics Basic Review of Byeong-Joo Lee Microstructure Evolution

Physical Chemistry content Physical Chemistry 1 (BSC) Thermodynamics Terms The thermodynamic system First law of thermodynamics Work, heat, internal energy,

Chapter 19 Chemical Thermodynamics. First Law of Thermodynamics Energy cannot be created nor destroyed. Therefore, the total energy of the universe is.

Thermodynamics Chapter 18.

Thermodynamics Chapter 19. First Law of Thermodynamics You will recall from Chapter 5 that energy cannot be created or destroyed. Therefore, the total.

Chapter 19 Chemical Thermodynamics HW:

Review: Expressions of the thermodynamic equilibrium constant K

Chapter 19 Chemical Thermodynamics Lecture Presentation John D. Bookstaver St. Charles Community College Cottleville, MO © 2012 Pearson Education, Inc.

1. (1.3) (1.8) (1.11) (1.14) Fundamental equations for homogeneous closed system consisting of 1 mole:

Partial Molar Quantities and the Chemical Potential Lecture 6.

ERT 206/4 THERMODYNAMICS SEM 1 (2012/2013) Dr. Hayder Kh. Q. Ali 1.

Entropy ( ) Entropy (S) is a measure of disorder in a system – Nature likes to create disorder (i.e., ΔS > 0) – Larger entropies mean that more energy.

4/17/2014PHY 770 Spring Lecture 231 PHY Statistical Mechanics 12:00 * - 1:45 PM TR Olin 107 Instructor: Natalie Holzwarth (Olin 300) Course.

Solution thermodynamics theory—Part I

Lecture 6. NONELECTROLYTE SOLUTONS. NONELECTROLYTE SOLUTIONS SOLUTIONS – single phase homogeneous mixture of two or more components NONELECTROLYTES –

Chemical-Reaction Equilibra ERT 206: Thermodynamics Miss Anis Atikah Ahmad Tel: anis

Chapter 14: The Classical Statistical Treatment of an Ideal Gas.

Multi-component Homogeneous System: Solution Thermodynamics

Chemical Equilibrium By Doba Jackson, Ph.D.. Outline of Chpt 5 Gibbs Energy and Helmholtz Energy Gibbs energy of a reaction mixture (Chemical Potential)

Solution thermodynamics theory—Part IV

ACTIVITY AND ACTIVITY COEFFICIENT

42C.1 Non-Ideal Solutions This development is patterned after that found in Molecular Themodynamics by D. A. McQuarrie and John D. Simon. Consider a molecular.

Introduction to phase equilibrium

Solution thermodynamics theory

Ideal and Dilute Solutions 2/21/2016. Master Thermodynamics Equations.

General Phase Equilibrium

Thermodynamics Chemical-reaction Equilibria

Clapeyron and Clausius Clapeyron Equations

SOLUTION THERMODYNAMICS:

Now we are going to start looking at models for the chemical potential  i of a given component i in a mixture The first model is the ideal gas mixture.

Chemical Thermodynamics  2009, Prentice-Hall, Inc. First Law of Thermodynamics You will recall that energy cannot be created nor destroyed. Therefore,

Solution thermodynamics theory—Part III

Gibbs-Duhem and the Chemical Potential of Ideal Solutions

Solution thermodynamics theory—Part IV

SUBJECT:-CHEMICAL ENGINEERING THERMODYNAMICS 2 TOPIC:- DISCUSS GIBSS DUHEM EQUATION. - CALCULATION OF PARTIAL PROPERTIES FROM.

Solution of Thermodynamics: Theory and applications

Chemical and Phase Equilibrium (2)

Chapter 13 Macromolecules in Solution: Thermodynamics and Equilibria

Classical Thermodynamics of Multicomponent Systems

Classical description of a single component system

Don’t be in a such a hurry to condemn a person because he doesn’t do what you do, or think as you think. There was a time when you didn’t know what you.

Free Energy and Pressure

How Free Energy Depends on P

Phase diagrams and phase transitions of unary systems

Presentation transcript:

Classical Thermodynamics of Solutions Lecture 17 Classical Thermodynamics of Solutions Gibbs free energy of formation of solution Ideal gas mixtures Ideal, dilute and concentrated solutions Excess functions

Gibbs free energy of mixing, GM XA mol of A + XB mol of B Since Therefore But Thus finally or

Ideal gas activity and GM Activity for a gas is Where is arbitrary. We can choose For which And the Gibbs free energy of mixing

Ideal gas - HM, and SM Since X is independent from temperature. From this the entropy of mixing of an ideal solution

Multicomponent condensed phases Chemical potential of a vapor For the solid In equilibrium, distributive equilibrium From which since in equilibrium

Ideal solution For ideal solution From which And

Dilute solution Pressure above dilute solute is proportional to its concentration From which Where Is the activity coefficient can be greater or smaller than one. It is 1 for ideal solutions.

Dilute solution - II Gibbs Duhem At constant T and P In terms of molar properties Thus for dilute solution of B in A

Dilute solution - III Recalling that And with Since activity coefficient is constant

Dilute solution - IV After differentiating the second term After integration since

Concentrated solutions Activity coefficient is not a constant any more However, for so-called regular solutions we still assume entropy of mixing same as for the ideal solution But the enthalpy of mixing will be not zero.

Excess functions Chemical potential of mixing For an ideal solution Which defines excess chemical potential of mixing Or in terms of partial molar from which