Unit 2: Equilibrium Learning Standards

Use the following learning outcomes to keep track of your learning progress:

• 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 diagram
• 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
• 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 process
• F:     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 K_eq and vice versa
• F4.      predict the effect (or lack of effect) on the value of K_eq of changes in the following factors:
• •            temperature
• •            pressure
• •            concentration
• •            surface area
• •            catalyst
• F5.      calculate the value of K_eq given the equilibrium concentration of all species
• F6.      calculate the value of K_eq given the initial concentrations of all species and one equilibrium concentration
• F7.      calculate the equilibrium concentrations of all species given the value of K_eq 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