Text Box: Physical Chemistry 2, BSc Course

Course Prerequisites:

Physical Chemistry 1

Course Description:

This course is an introduction to chemical thermodynamics and chemical kinetics with applications to gases, solutions, and phase equilibrium to provide a firm foundation for understanding the physical principles that govern chemical and biochemical systems.

Part 1: Physical change of pure substances

· Clapeyron and Clausius Clapeyron Equations

· First and higher-order phase transformation

· Phase, number of components, degree of freedom

· Lever rule, one, two, and three-component phase diagrams

Part 2: Nonelectrolyte solutions

· Molar fractional quantities

· Phase diagram of multi-component systems

· Vapor pressure of solution and Raoult's and Henry's laws

· Dependency of vapor pressure on the component of the system

· Solutions and saturated solutions

· Solubility of gases

· Thermodynamics of ideal solutions

· Real solutions

· Activity and activity coefficients, standard states and methods for investigation of the activity of solution components

· Fractional distillation and distillation with water vapor

· Colligative properties of ideal solutions

Part 3: Electrolyte solutions

· Activity and standard states of ions in solutions

· Average activity coefficient

· Debye–Hückel theory

· Electrochemical potential

· Interface potential difference

· Electrochemical cell

· The standard potential of cell

· Temperature and concentration dependency of electrochemical potential difference

· Calculating thermodynamics quantities of a cell by potential difference

· Conductivity of electrolyte solutions

· Special conductivity

· Molar conductivity

· Ostwald's law

· Ion mobility and transport numbers and methods of measuring them

Part 4: Chemical kinetics

· Difference between thermodynamics and kinetics investigation of chemical phenomena

· Importance of reaction path in kinetics

· Rate equations for simple and complex reactions

· Elementary reactions

· Order and molecularity of a reaction

· Chemical and physical methods for investigation of rate law

· Half-life and its dependency on the initial concentration of reactants

· The rate constant of a reaction

· Investigation of a reaction mechanism

· Parallel reactions

· Series reactions

· Reversible reactions

· Effect of temperature on reaction rate

· Collision and absolute rate theory

· Solution phase reactions and comparison with gas-phase reactions

· Diffusion controlled reactions

· Effect of catalysts on chemical reactions

· Homogeneous catalysis – Enzyme catalysis

· Inhomogeneous catalysis and adsorption

· Auto catalysis reactions

Course Materials:

Ira. N. Levine, Physical Chemistry: The molecular nature of matter and change, 6th Edition, McGraw Hill, 2009

Share box link: https://drive.google.com/drive/folders/1ES08xSmRSovCCAPuQYeehKkx4MDU_7Nh?usp=sharing

Department of Chemistry, Faculty of Science, University of Kurdistan

Mehdi Irani

Teaching duties

Physical Chemistry II

Chemical Kinetics

Computer in Chemistry

Methods

	Weekly Schedule
Session	Subject
1	7.1 The Phase Rule
2	7.2 One-Component Phase Equilibrium 7.3 The Clapeyron Equation
3	7.4 Solid–Solid Phase Transitions 7.5 Higher-Order Phase Transitions
4	Solving problems of Chapter 7
5	9.1 Solution Composition 9.2 Partial Molar Quantities
6	9.3 Mixing Quantities 9.4 Determination of Partial Molar Quantities 9.5 Ideal Solutions
7	9.6 Thermodynamic Properties of Ideal Solutions 9.7 Ideally Dilute Solutions 9.8 Thermodynamic Properties of Ideally Dilute Solutions
8	Solving problems of Chapter 9
9	Midterm examination
10	10.1 Activities and Activity Coefficients 10.2 Excess Functions 10.3 Determination of Activities and Activity Coefficients
11	10.4 Activity Coefficients on the Molality and Molar Concentration Scales 10.5 Solutions of Electrolytes 10.6 Determination of Electrolyte Activity Coefficients
12	10.7 The Debye–Hückel Theory of Electrolyte Solutions 10.8 Ionic Association 10.10 Nonideal Gas Mixtures
13	Solving problems of Chapter 10
14	12.1 Colligative Properties 12.2 Vapor-Pressure Lowering 12.3 Freezing-Point Depression and Boiling-Point Elevation 12.4 Osmotic Pressure
15	12.5 Two-Component Phase Diagrams 12.6 Two-Component Liquid–Vapor Equilibrium
16	12.7 Two-Component Liquid–Liquid Equilibrium 12.8 Two-Component Solid–Liquid Equilibrium 12.9 Structure of Phase Diagrams
17	12.10 Solubility 12.12 Three-Component Systems
18	Solving problems of Chapter 12
19	13.1 Electrostatics 13.2 Electrochemical Systems 13.3 Thermodynamics of Electrochemical Systems
20	13.4 Galvanic Cells 13.5 Types of Reversible Electrodes 13.6 Thermodynamics of Galvanic Cells 13.7 Standard Electrode Potentials
21	15.1 Kinetics 15.2 Thermal Conductivity
22	15.3 Viscosity 15.4 Diffusion and Sedimentation
23	15.5 Electrical Conductivity 15.6 Electrical Conductivity of Electrolyte Solutions
24	Solving problems of Chapter 13 and Chapter 15
25	Second midterm examination.
26	16.1 Reaction Kinetics 16.2 Measurement of Reaction Rates
27	16.3 Integration of Rate Laws
28	16.4 Finding the Rate Law 16.5 Rate Laws and Equilibrium Constants for Elementary Reactions 16.6 Reaction Mechanisms
29	16.8 Temperature Dependence of Rate Constants 16.9 Relation Between Rate Constants and Equilibrium Constants for Composite Reactions
30	16.11 Unimolecular Reactions 16.12 Trimolecular Reactions 16.13 Chain Reactions and Free-Radical Polymerizations 16.14 Fast Reactions
31	Solving problems of Chapter 16
32	16.16 Catalysis 16.17 Enzyme Catalysis 16.18 Adsorption of Gases on Solids