Course Outline
Term 1 (Term 2)
Introduction 1-3
Atomic Theory 4-6
Use of the Mole 7
Chemical Bonding 8-13
Chemical Reactions 14-15
Oxidation & REDOX 16-17
Thermochemistry 18-25
Gases 26-33
Review (Term 1) 34-35
Old Exams
Lab Videos
Thermochemistry (Lectures 18-25)
PowerPoint     Readings    Assignments
Practice Tests

18 Thermochemistry, Enthalpy
The lecture begins with an introduction to thermochemistry, the study of heat flow to or from a chemical reaction. The concepts of internal haber and of enthalpy are introduced, as well as heat capacity and the idea of a "state function". Hess' law is described (you have actually used in when we looked at the Born-Haber cycle).
ppt-18     Chap.8    A-07 Enthalpy Practice Test

19 Enthalpy
In this lecture, we introduce the concept of "heat of formation" of a compound, i.e. the heat evolved or absorbed when a compound is formed from the elements. Hand in hand with this goes the idea of a "standard state", the physical state of a compound or element at specified conditions (usually 1 atm pressure and 25oC). To explain the origin of the enthalpy of a reaction, bond dissociation energies are used.
ppt-19     Chap.8    A-07 Enthalpy Practice Test

20 Enthalpy, Energy Sources
Some of the concepts of enthalpy and energy are used in a more descriptive lecture about our usage of energy. The food Calorie is defined. Two sources of energy (coal and hydrogen) are compared. The gasification of coal to produce "Syngas" provides an interesting set of reactions whose enthalpies are important.
ppt-20     Chap.8    A-07 Enthalpy Practice Test

21 Entropy
The concept of entropy is introduced. Entropy is a measure of the "randomness" of the system being considered. For example, the molecules in a gas are more randomly arranged than those of a solid material. Thus, the gas has a higher entropy than the solid. The mathematical basis of entropy is presented (Boltzmann's law), and several examples of situations where entropy will increase or decrease are given.
ppt-21     Chap.8    A-07 Entropy Practice Test

22 Equilibrium I
An introduction to the idea of an equilibrium reaction. Formulation of the equilibrium constant. Use of the constant to infer the position of the reaction at equilibrium, and to calculate concentrations of all species at equilibrium.
ppt-22     Chap.13   A-08 Entropy Practice Test

23 Equilibrium II
Use of the equilibrium constant. Predicting the dorection that the reaction shifts if the temperature, pressure or concentration of one of the species is changed.
ppt-23     Chap.13    A-08 Entropy Practice Test

24 Free Energy, Equilibrium
In this lecture, you will learn the relationshp between the entropy change of the Universe and the spontaneity of a reaction. A simpler method for predicting the spontaneity of a reaction is to calculate the Gibbs energy change, commonly called the free energy change. 
ppt-24     Chap.16    A-08 Entropy Practice Test

25 Free Energy, Equilibrium
In this lecture, the connection between the equilibrium position of a reaction and the free energy change is made. 
ppt-25     Chap.16    A-08 Entropy Practice Test