Chemistry 12
UNIT THREE -
EquilibriumD: Dynamic Equilibrium (Introduction)
D1. describe the reversible nature of most chemical reactions
D2. identify the reversible pathways of a chemical reaction on the PE diagramD3. relate the changes in rates of the forward and reverse reactions to the changing concentrations of the reactants and products as equilibrium is established
D4. describe chemical equilibrium as a closed system at constant temperature:
- whose macroscopic properties are constant
- where the forward and reverse reaction rates are equal
- that can be achieved from either direction
- where the concentrations of reactants and products are constant
D5. describe the dynamic nature of chemical equilibrium
D6. infer that a system not at equilibrium will tend to move toward a position of equilibrium
D7. determine entropy and enthalpy changes from a chemical equation (qualitatively)
D8. state that systems tend toward a position of minimum enthalpy and maximum randomness (entropy)
D9. predict the result when enthalpy and entropy factors:
- both favour the products
- both favour the reactants
- oppose one another
E: Dynamic Equilibrium (Le Châtelier's Principle)
E1. describe the term shift as it applies to equilibria
E2. apply Le Châtelier's principle to the shifting of equilibrium involving the following:
- temperature change
- concentration change
- volume change of gaseous systems
E3. explain the above shifts using the concepts of reaction kinetics
E4. identify the effect of a catalyst on dynamic equilibrium
E5. apply the concept of equilibrium to a commercial or industrial processF: Dynamic Equilibrium (The Equilibrium Constant)
F1. gather and interpret data on the concentration of reactants and products of a system at equilibrium
F2. write the expression for the equilibrium constant when given the equation for either a homogeneous or heterogeneous equilibrium system
F3. relate the equilibrium position to the value of Keq and vice versa
F4. predict the effect (or lack of effect) on the value of Keq of changes in the following factors: temperature, pressure, concentration, surface area, and catalyst
F5. calculate the value of Keq given the equilibrium concentration of all species
F6. calculate the value of Keq given the initial concentrations of all species and one equilibrium concentration
F7. calculate the equilibrium concentrations of all species given the value of Keq and the initial concentrations
F8. determine whether a system is at equilibrium, and if not, in which direction it will shift to reach equilibrium when given a set of concentrations for reactants and products
Lesson Plan - Unit Two
Period #7 - Unit Two Review & Intro To Equilibrium
Materials : Textbook : Chemistry 12 - Hebden
Assignment #1
Unit Review Questions
Review : Go over questions from Homework
Objectives : students should be able to :
Meet all the learning outcomes for Unit Two
D: Dynamic Equilibrium (Introduction)
D1. describe the reversible nature of most chemical reactions
D2. identify the reversible pathways of a chemical reaction on the PE diagramD3. relate the changes in rates of the forward and reverse reactions to the changing concentrations of the reactants and products as equilibrium is established
D4. describe chemical equilibrium as a closed system at constant temperature:
- whose macroscopic properties are constant
- where the forward and reverse reaction rates are equal
- that can be achieved from either direction
- where the concentrations of reactants and products are constant
D5. describe the dynamic nature of chemical equilibrium
Part I - Reaction Kinetics - Unit Review and Assignment #1
Students will complete the Unit Review and work on Assignment #1, due at the beginning of the period that the Unit Test is written.
If finished early, start introduction to Equilibrium - Unit 3.
Exercise :
Unit Review Package
Assignment #1
Evaluation :
Unit Two Exam
Assignment #1
Part II - Intro To Dynamic Equilibrium - Introduction :
Give notes on page 3-1 on the "Introduction to Dynamic Equilm." To explain the following :
The reversible nature of most chemical reactions (D1)
Show overhead of PE diagram to identify the reversible pathways of a chemical reaction on the PE diagram (D2)
D3. relate the changes in rates of the forward and reverse reactions to the changing concentrations of the reactants and products as equilibrium is established
D4. describe chemical equilibrium as a closed system at constant temperature:
- whose macroscopic properties are constant
- where the forward and reverse reaction rates are equal
- that can be achieved from either direction
- where the concentrations of reactants and products are constant
D5. describe the dynamic nature of chemical equilibrium
Exercise :
Questions 20-22 page 12 of Hebden.
Questions 24-28 page 16 of Hebden
Prep for lab 18 C
Evaluation :
Unit One Exam
Homework Checks
Lab 18 C
Assignment #1
Lesson Plan - Unit Two
Period #8 - Unit Two Exam & Intro To Dynamic Equilibrium
Materials : Textbook : Chemistry 12 - Hebden
Unit Test
Review :
Objectives : students should be able to :
D: Dynamic Equilibrium (Introduction)
D1. describe the reversible nature of most chemical reactions
D2. identify the reversible pathways of a chemical reaction on the PE diagramD3. relate the changes in rates of the forward and reverse reactions to the changing concentrations of the reactants and products as equilibrium is established
D4. describe chemical equilibrium as a closed system at constant temperature:
- whose macroscopic properties are constant
- where the forward and reverse reaction rates are equal
- that can be achieved from either direction
- where the concentrations of reactants and products are constant
D5. describe the dynamic nature of chemical equilibrium
D6. infer that a system not at equilibrium will tend to move toward a position of equilibrium
D7. determine entropy and enthalpy changes from a chemical equation (qualitatively)
D8. state that systems tend toward a position of minimum enthalpy and maximum randomness (entropy)
D9. predict the result when enthalpy and entropy factors:
- both favour the products
- both favour the reactants
- oppose one another
Part I - Kinetics - Unit Exam
Students write the Unit Exam on Kinetics
Part II - Reaction Kinetics - Collision Theory :
Give notes on page 2-5 on the "Kinetic Collision Theory of Reaction Rates." Explain the following statements (B1)
- reactions are the result of collisions between reactant particles
- not all collisions are successful
- sufficient kinetic energy (KE) and favorable geometry are required
- to increase the rate of a reaction one must increase the frequency of successful collision
- energy changes are involved in reactions as bonds are broken and formed
Define Kinetic Energy and Potential Energy as related to particles in a system, and review Endothermic and Exothermic reactions (give handout of definitions and summary). (B7), (B8)
Discuss Kinetic Energy Distributions and how they relate to temperature. Show overhead. Give notes on page 2-5, "Kinetic Energy Distributions".
Describe the activated complex in terms of its potential energy ,stability, and structure and define activation energy, give notes on page 2-5, and show Orientation Overhead.
Exercise :
Questions 20-22 page 12 of Hebden.
Questions 24-28 page 16 of Hebden
Prep for lab 18 C
Evaluation :
Unit One Exam
Homework Checks
Lab 18 C
Assignment #1