We think you have liked this presentation. If you wish to download it, please recommend it to your friends in any social system. Share buttons are a little bit lower. Thank you!
Presentation is loading. Please wait.
Published byAriana Ball
Modified over 4 years ago
Lecture 24 Chemical equilibrium Equilibrium constant Dissociation of diatomic molecule Heterophase reactions
Gibbs free energy change Chemical reaction Gibbs free energy change In equilibrium the Gibbs free energy change is zero, therefore
Activity Chemical potential with gives
Equilibrium constant Defining standard free energy change for the reaction And equilibrium constant for the reaction gives
Diatomic molecule Equilibrium constant for the reaction Chemical potential for monoatomic and diatomic gas
Diatomic molecule - equilibrium constant
Equilibrium pressure expression Equilibrium constant for the reaction Increasing temperature increasing dissociation The major parameter controlling dissociation is D e /kT
Heterophase reactions Consider a C =1 (activity of the pure solid phase) K a can be obtained from statistical mechanics (e.q., Einstein model of C solid) or from experiment via
Properties of a Pure Substance
Electrolyte Solutions - Debye-Huckel Theory
1 Chapter 6 Chemical Equilibrium. 2 Spontaneous Chemical Reactions The Gibbs Energy Minimum Consider the simple equilibrium reaction: A B The equilibrium.
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.
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?
CHAPTER 14 THE CLASSICAL STATISTICAL TREATMENT OF AN IDEAL GAS.
Chemical Equilibrium Basic Skills: Students should be able: To explain the dynamic nature of equilibrium. To be able to write the equilibrium constant.
Properties of Reservoir Fluids Fugacity and Equilibrium Fall 2010 Shahab Gerami 1.
Three Laws of Thermodynamics 1. ΔE univ = 0 For the system: ΔE = q + w 2. ΔS univ ≥ 0 For the system: ΔS ≥ q/T, where the “=“ applies to reversible processes.
Physical Transformations of Pure Substances
Equilibrium Le Chatelier’s Principle. Equilibrium Brown gasColourless gas.
Unit 4: Chemical Reactions
Thermo & Stat Mech - Spring 2006 Class 20 1 Thermodynamics and Statistical Mechanics Heat Capacities.
Thermo & Stat Mech - Spring 2006 Class 14 1 Thermodynamics and Statistical Mechanics Kinetic Theory of Gases.
Thermo & Stat Mech - Spring 2006 Class 13 1 Thermodynamics and Statistical Mechanics Open Systems and Chemical Potential.
Thermodynamic Property Relations
System. surroundings. universe.
© 2018 SlidePlayer.com Inc. All rights reserved.