1. State the two things that Kinetics explain in a chemical reaction if you assume that Thermodynamics explains if the reaction occurs or not.

2. Explain the collision theory including the two factors for an effective collision (i.e. correct orientation and energy (activation energy, E_{ac} or greater).

3. Using the collision theory and the Kinetic Molecular Theory, explain reaction mechanism including determining rate limiting/determining steps, which species is a catalyst/intermediate, and the relationship between the number of reactant particles and the rate of the reaction. (i.e. making products). Also be able to determine the rate of reaction for these chemical reactions (see rate law objectives below).

4. Using the Kinetic Energy graph, explain the factors for increasing the rate of reaction including temperature, more particle able to collide (i.e concentration change, surface area, pressure & volume changes, and stirring). Need to explain via the Kinetic Energy graph

5. Draw a Potential Energy diagram for both an exothermic and endothermic reaction and identify the heat of reaction, potential energy of product/reactant/activated complex/activation energy. Student need to define the role of activation energy and activated complex in reacting reactants into products. Also change the above Potential Energy diagram for the addition of the catalysts and how it affect the rate of reaction.

6. Explain what the Rate Law is how it is related to the concentrations of the reactant. Be able to define each of the components of the equation.

7. Be able to recognize and solve Methods of Initial Rate problems to determine the complete Rate law (including order of each reactant(s), k (rate constant) and the overall rate of the chemical reaction.

8. Be able to recognize and solve for Integrated Rate Law problems including determine the appropriate order of the reactant via generating [A] vs. t graph or ln[A] vs. t graph or 1/[A] vs. t graph. In addition, be able to look at these graphs and determine which would be the correct order of the reactant. Also be able to convert the graphical information (slope, y-intercept) into the Rate Law "equation".

9. Be to explain half-live and to solve "simple" problems of complete half live calculations. Also, using your know of specific half-live equations for the zero order, first order and second order, determine half-live problems.