Unit 5
Kinetics and Equilibrium
Period 1 Unit Calendar
Period 9 Unit Calendar
Chapter 14: Chemical Kinetics
14.1 factors affecting reaction rates
14.2 reaction rates
Stoichiometrically determine the rates of (dis)appearance of substances involved in a chemical reaction.
14.3 Concentration and Rate (Rate Law)
Determine the rate law for various reactions of different reaction orders
Calculate and determine the proper units for the rate constant.
14.4 the change of concentration with time
Determine how much reactant/product remains/was produced for first and second order reactions over time.
Use the rate laws to determine the half-life of 1st and 2nd order reactions
Helpful video: Kinetics Equations; Rearranging equations with logs
14.5 temperature and rate
SW explain chemical reactions in terms of the collision model, interpret corresponding potential energy diagrams and use the arrhenius equation (k = Ae-Ea/RT AND ln(k1/k2) = (Ea/R)(1/T2 - 1/T1)
Video: Potassium Permanganate and Oxalic Acid; trials 1-3
If you are absent for the lab, you can use this video to collect the necessary data to complete the lab.
14.6 Reaction mechanisms
Objectives: Reaction Mechanisms or text
Identify catalysts, intermediates and overall reaction given elementary steps for a reaction
Describe the molecularity of chemical reactions given their elementary steps
Objectives: Reaction Mechanisms and Rate Laws or text
Determine the rate law for a reaction mechanisms with slow first elementary steps
Determine the rate law for a reaction mechanisms with fast first elementary steps
14.7 Catalysis
Describe how catalysts (and enzymes) increase the reaction rate in terms of mechanism and activation energy.
Graphically show the effect of catalysts on potential energy diagrams.
Chapter 14 Resources:
Chapter 15: Chemical Equilibrium
15.1 the concept of equilibrium
15.2 The equilibrium constant
Determine the proper equilibrium constant expression given a balanced chemical equation
Calculate the value for Keq given equilibrium values of reactants and products
Use Kp=Kc(RT)Δn to convert between the equilibrium constant in terms of molar concentration and pressure
15.3 Understanding and Working With Equilibrium Constants
Manipulate EQ and determine the resulting value for Keq (flipping the eq, doubling coefficients, combining equations)
Infer if an equilibrium lies far to the left or right based on the magnitude of the Eq Constant
15.4 heterogeneous equilibria
Accurately set up the equilibrium constant expression and calculate its value for heterogeneous equilibrium including saturated solutions
15.5 calculating eq constants
Use the equilibrium constant and stoichiometry to determine equilibrium concentrations for the compounds involved in a chemical equilibrium.
15.6 application of eq constants
Objectives: Predicting the Direction Of Reaction (Keq vs Q) or text
Use the Keq value and expression to determine which direction a system will proceed in order to reach equilibrium given initial conditions (Keq vs. Q)
Objectives: Calculating Equilibrium Concentrations or text
Calculate the equilibrium concentrations given Keq and initial conditions (Note: You may need to use the quadratic equation)
15.7 Le Chatlier’s principle
Analyze what would happen to an equilibrium that is subjected to a disturbance, such as changes in temperature, pressure, volume, concentrations and presence of a catalyst.
Chapter 15 Resources: