Module Catalogues, Xi'an Jiaotong-Liverpool University   
Module Code: CHE202
Module Title: Intermediate Physical Chemistry
Module Level: Level 2
Module Credits: 5.00
Academic Year: 2017/18
Semester: SEM2
Originating Department: Chemistry
Pre-requisites: N/A
This module covers several subject areas of physical chemistry: thermodynamics, kinetics, quantum mechanics, spectroscopy, and photochemistry. The aims are to

1. revised and extend the study of the 1st and 2nd laws of thermodynamics to chemical reactions,

2. study the basic ideas and factors affecting the rates of chemical reactions.

3. give an more advanced coverage in quantum mechanics.

4. reinforce some aspects of molecular spectroscopy.
Learning outcomes 
By the end of the module, students should be able to:

A. effectively apply thermodynamic principles.

B. discuss the rate of reaction and reaction mechanisms through studying kinetics of reactions.

C. demonstrate an understanding of the basic concepts of quantum mechanics.

D. apply Schrodinger equation to for translational, vibrational, and rotational motions.

E. apply molecular orbital (MO) theory to rationalise and make predictions of the bonding in molecules.

F. discuss spectroscopy as a result of energy transitions between atomic/molecular energy levels.

G. describe different decay processes of photo excited states and use the phenomena as quantitative analysis methods.

Method of teaching and learning 
The material presented at the lectures and its application for solving problems is supported by work in small group tutorials and interactive events. Students are expected to prepare the answers to tutorial problem questions and submit them before tutorials. Discussions during tutorials will focus on problems caused the most difficulties. Two summative tests will be introduced to monitor continuously student’s learning progress.

1. Revision of materials taught in CHE106:

- Ideal gas equation, first law of thermodynamics, heat & work, enthalpy, Hess' law cycles, entropy, Gibbs energy, equilibrium constant. Examples of calculations using tables of thermodynamic data. Use of bond energies to predict U and H for chemical reactions.

- Second law of thermodynamics, statistical description of entropy. Dependence of entropy on temperature and pressure, third law of thermodynamics.

- Gibbs free energy, changes at constant temperature or pressure. Equilibrium constant K, relation to Gibbs free energy, variation with temperature.

- Chemical potential, equilibrium and the extent of reaction. Standard States. Effect of temperature and pressure on equilibria. Extension from gas phase reactions to all reactions.

2. Heat capacity at constant volume or pressure, temperature dependence of internal energy and enthalpy.

3. Real gases, deviations from ideal behaviour, virial and van der Waals equations of state.

4. Ideal liquids and solutions. Raoult's law. The chemical potential of components in ideal mixtures: standard and reference states. Colligative properties. Deviations from ideality.


1. Revision of materials taught in CHE106:

- Chemical reaction rates, rate equation, reaction orders, integrated rate equations, half life, activation energy barriers and Arrhenius equation.

- Derivation of zero-, first- and second order integrated rate eqns. Determination of reaction order and rate constant: straight plots. Half-life time of a reaction.

- Consecutive reactions. The rate determining step.

- Pre-equilibrium; steady state approximation. Diffusion controlled reactions.

- Michaelis-Menten Mechanism. Lindemann-Hinshelwood mechanism. Chain reactions.

2. Kinetic gas model, collision rates. Simple collision theory (SCT). Potential energy barriers. Reactive Encounters. Comparison of SCT with experimental
Delivery Hours  
Lectures Seminars Tutorials Lab/Prcaticals Fieldwork / Placement Other(Private study) Total
Hours/Semester 26     13      111  150 


Sequence Method % of Final Mark
1 Test1 15.00
2 Test2 15.00
3 Coursework Linked To Tutorials 10.00
4 Final Exam 60.00

Module Catalogue generated from SITS CUT-OFF: 10/22/2017 10:42:49 AM