Final Exam Information
| Date | Time | Location |
| Thursday, August 3, 2000 | 0800-1000 | GILB 124 |
Final version as of August 2, 2000
The Final Exam Objectives include those presented for Exams
1, 2, and 3
and these listed below:
Be able to
| 1 | Work problems similar to those assigned in the text book and Chem SkillBuilder and presented in the lecture, quizzes, and worksheets |
| 2 | Apply Raoult's and Henry's Laws to solutions and distinguish between them in application. |
| 3 | Discuss and calculate boiling point elevation and freezing point depression, and describe the origins of the phenomena. The expressions and constants will be provided. |
| 4 | State what is meant by terms such as colligative properties, initial reaction rate, reaction order, activation energy, transition state, homogeneous and heterogeneous catalysis, |
| 5 | Discuss the meaning of osmotic pressure and account for examples of it. |
| 6 | Describe what is meant by reaction rate, and determine reaction rate from suitable data. |
| 7 | Describe the four factors that affect reaction rate and explain qualitatively why these factors have the effect they do. |
| 8 | State what is meant by the "rate law" of a reaction and determine the rate constant and exponents to concentrations from suitable data. |
| 9 | Describe what is meant by reactions of zero, first, and second order. |
| 10 | Use the integrated rate expresssion for a first order reaction to solve problems involving reactant amounts as a function of time. |
| 11 | Use the concept of a half-life of a first order reaction to estimate reactant amounts at various times. |
| 12 | Describe the main tenents of Collision Theory and Transition State Theory, and discuss applications of those theories. |
| 13 | Obtain the activation energy of a reaction from reaction rate constants at different temperatures. |
| 14 | Describe what is meant by a Reaction Mechanism, and obtain a Rate Law for a reaction from a mechanism with a single rate-determining step. |
| 15 | Describe the role of a catalyst in speeding up a reaction for the cases of a metal surface and an enzyme. |
| 16 | Construct the equilibrium constant expression from an overall reaction, and explain why the "kinetics view" accounts for the expression. |
| 18 | Predict the direction a reaction will proceed if the computed Qc is not equal to the equilibrium constant. |
| 19 | Use LeChatlier's Principle to predict the direction an equilibrium will shift when a stress or change is imposed. The stress could be a change in volume, total pressure, moles of reactant or product, or temperature. |
http://www.chem.orst.edu/ch121-3s/ch122/exam_information/final_exam_information.htm
Last updated by M. Schuyler on September 09, 2002.
Copyright 1998 R. Nafshun
