CHEM 1523: Principles of Chemistry

Upon the successful completion of the course, students will be able to demonstrate a working knowledge of:

• The microscopic differences between solids, liquids and gases
• The origins, definition of and measurement of gas pressure
• The relationship between macroscopic gas properties, the Ideal Gas equation
• Calculations and stoichiometry involving gases
• Mixtures of gases and the relationship between mole fraction and partial pressure
• The distribution of speeds for a gas sample and the effect of mass
• The postulates of the Kinetic Molecular theory of gases
• The terms effusion and diffusion of gases and their applications
• The reasons for the corrections applied in the van der Waals equation for gases
• The microscopic and macroscopic equilibrium state and the equilibrium constant and reaction quotient
• The algebraic manipulations of a chemical reaction and its equilibrium constant
• Le Chatelier's Principle and its application to a chemical system at equilibrium
• Solving equilibrium problems, given either initial concentrations and the equilibrium constant and finding equilibrium amounts, or given equilibrium amounts and inding the equilibrium constant
• The Bronsted acid and base definitions and the relationship between conjugate acid-base pairs and their equilibrium constants for reaction with water
• The relative strengths of acids and bases determined by their equilibrium constants, including polyprotic acids
• Solving weak acid-weak base equilibrium problems
• The pH scale and the acidity or basicity of aqueous solutions
• The acid-base properties of salt solutions
• The common ion effect and buffer solutions, buffer capacity and buffer pH range, how to prepare buffer solutions, and how buffer solutions react to additions of acid or base
• The general form of acid-base titration curves, the significant regions, including indicator selection
• The acid-base properties of amino acids
• The fundamental processes involved in oxidation-reduction reactions
• The concept of half-cell reduction potentials, the standard hydrogen electrode, and cell potentials
• Standard conditions and the cell potential under non-standard conditions, the Nernst equation
• Fundamental properties of batteries
• Heat capacity, the first law of thermodynamics and calorimetry; exothermic or endothermic reactions
• The application of Hess' Law to chemical systems
• The use of enthalpies of formation to predict enthalpy changes for other reactions
• The concept of spontaneous reactions and the importance of entropy
• The second and third laws of thermodynamics

• Unit 1: Gases
• Unit 2: Kinetics
• Unit 3: Equilibrium
• Unit 4: Acid Bases and Solubility Equilibria
• Unit 5: Thermodynamics
• Unit 6: Electrochemistry

The following Open Education Resource (OER) textbook, free of charge, is required for this course:

1. TRU Open Learning Principles of Chemistry. Thompson Rivers University. https://principlesofchemistryopencourse.pressbooks.tru.ca/

• Computer with Internet is required.
• Non-programmable, single numeric line calculator such as the Casio fx-260 is required.

To successfully complete this course, students must achieve a passing grade of 50% or higher on the overall course, and 50% or higher on the mandatory final exam. 

Note: The final exam for this course is only available as a in-person exam and must be taken at an approved Testing Centre. Please email exams@tru.ca with any questions.

An Open Learning Faculty Member is available to assist students. Students will receive the necessary contact information at the start of the course.