January 2009




Course code: Campus MB 1112/3 (U of Wpg Code: CHEM-1112/3)

INTRODUCTION: This 3 credit course includes an introduction to chemical kinetics, chemical thermodynamics and equilibrium, and to acid/base and oxidation/reduction chemical reactions. The laboratory component will introduce students to some of the basic techniques of practical chemistry. The fundamental concepts of chemical reactivity covered in this course provide the essential foundation for students who wish to continue with Chemistry or Biochemistry as a major, and for students of Biology, Physics, Physical Geography, Environmental Studies, and Experimental Psychology.

PREREQUISITES: CampusMB 1111/3 (U of Wpg Code: CHEM-111/3 or 08.1111/3) or equivalent from another university.



1. Textbook:   General Chemistry: Principles and Modern Applications - Ninth Edition; Authors- Ralph H Petrucci, William S Harwood, Geoff E Herring, Jeffry D Madura;  Publisher: Pearson Prentice Hall Copyright: 2007


2. Chemistry 1112/3 Laboratory Manual


3. Scientific Calculator (but not a graphing calculator or a programmable type)


4. Other booklets will be distributed to you from time to time


COURSE DELIVERY: This is a synchronous distributed learning distance education course utilizing the Learnlinc (iLinc) system. We “meet” on Thursday evenings from 6 pm till 9 pm.


The class schedule follow:


Thursday, January 8, 2009 – Lecture #1

January 15 – Lecture #2

January 22 – Lecture #3

January 29 – Lecture #4

February 5 – Lecture #5 including Term Test ONE (50 min.)

February 12 – Lecture #6

February 19 – No lecture - Reading Week Feb.16-20

February 26 – Lecture #7

March 5 – Lecture #8

March 6 –Final date to withdraw without academic penalty.

March 12 – Lecture #9 including Term Test TWO (50 min.)

March 19 – Lecture #10

March 26 – Lecture #11

April 2 - Lecture #12 (last lecture)

April 20 – Final Exam: 1:30 pm - 4:30 pm 


Course Grading:                    Term Test #1     20%

Term Test #2     20%

Laboratory         20%

Final Exam         40%

Total               100%






Instructor: Dr. Marshall Carroll (that’s me). My email is m.carroll@uwinnipeg.ca and my phone number is 204-453-8023.  If you have any concerns, do not hesitate to contact me.





(NOTE: The html and powerpoint files and end-of-chapter exercises that we will use to help learn the topics below can be accessed by clicking HERE )



14      Chemical Kinetics  

14-1    Rate of a Chemical Reaction 

14-2    Measuring Reaction Rates 

14-3    Effect of Concn on Rxn Rates:Rate Law 

14-4    Zero-Order Reactions 

14-5    First-Order Reactions 

14-6    Second-Order Reactions 

14-7    Reaction Kinetics: A Summary 

14-8    Theoretical Models for Chemical Kinetics 

14-9    The Effect of Temperature on Rxn Rates 

14-10   Rxn Mechanisms 

14-11   Catalysis   


15      Principles of Chemical Equilibrium  

15-1    Dynamic Equilibrium 

15-2    The Equilibrium Constant Expression 

15-3    Relationships Involving Eqm Constants 

15-4    The Magnitude of an Equilibrium Constant 

15-5    The Reaction Quotient   

15-6    Le Châtelier’s Principle 

15-7    Equilibrium Calcns: Illustrative Examples 


16      Acids and Bases  

16-1    Arrhenius Theory: A Brief Review 

16-2    Brønsted—Lowry Theory of Acids and Bases 

16-3    Self-Ionization of Water and the pH Scale 

16-4    Strong Acids and Strong Bases 

16-5    Weak Acids and Weak Bases 

16-6    Polyprotic Acids 

16-7    Ions as Acids and Bases 

16-8    Molecular Structure and Acid—Base Behavior 


17      Additional Aspects of Acid—Base Equilibria 

17-1    The Common-Ion Effect

17-2    Buffer Solutions 

17-3    Acid—Base Indicators 

17-4    Neutralization Rxns and Titration Curves


7       Thermochemistry

7-1     Getting Started: Some Terminology 

7-2     Heat 

7-3     Heats of Reaction and Calorimetry

7-4     Work 

7-5     The First Law of Thermodynamics 

7-6     Heats of Reaction: delta U and delta H 

7-7     Hess’s Law   

7-8     Standard Enthalpies of Formation 



19      Spontaneous Change: Entropy and Free Energy  

19-1    Spontaneity

19-2    The Concept of Entropy 

19-3    Evaluating Entropy and Entropy Changes 

19-4    Second Law of Thermodynamics

19-5    Standard Free Energy Change, delta G° 

19-6    Free Energy Change and Equilibrium 

19-7    delta G° and K as Functions of Temperature 


20      Electrochemistry

20-1    Electrode Potentials and Their Measurement

20-2    Standard Electrode Potentials

20-3    Ecell, delta G, and  K

20-4    Ecell as a Function of Concentrations 

20-5    Batteries

20-7    Electrolysis