# 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: