CH341. : Physical chemistry 3

Department

Department of Chemistry

Academic Program

Bachelor in Chemistry

Type

Compulsory

Credits

02

Prerequisite

CH242.

Overview

This course aims to study:

- Metal and electrolytic conductivity.

- Comparison of galvanic cell and electrolysis.

- Electrolysis in an aqueous medium. Electrolysis with the participation of electrodes.

- Faraday Laws. Quantitative manifestations of electrolysis.

- The relationship between effort and concentration (Nernst equation).

- The relationship between the equilibrium constant and the voltage of the measuring cell.

- Molar conduction.

- Calculate the cell constant from knowing the resistance of the solution and conductivity

Intended learning outcomes

Study of molar conductivity and calculation of cell constant from knowledge of solution resistance and conductivity:

1. Enable the student to interpret metal and electrolytic conductivity.

2. Develop students' ability to know the interactions that occur at the electrodes of the cell.

3. Develop students' skills to describe the electrochemical equivalent and its relationship to Farday's law.

4. Enable students to identify the quantitative aspects of electrolysis.

5. Develop students' ability to distinguish the relationship between effort and concentration (Nernst equation).

6. Know the relationship between the equilibrium constant and the voltage of the measuring cell.

7.Demonstrates and explains metal and electrolytic conductivity.

8.Explains the reactions that occur at the electrodes of the cell.

9.Describes the electrochemical equivalent and its relationship to Farday's law. 10.Determines the quantitative manifestations of electrolysis.

11.Distinguish the relationship between effort and concentration (Nernst equation). 12.Distinguish the relationship between the equilibrium constant and the voltage of the measuring cell.

13.Recognize molar conductivity and calculate cell constant from knowledge of solution resistance and conductivity.

14.Interprets and analyzes metal and electrolytic conductivity.

15.Analyzes the reactions that occur at the electrodes of the cell.

16.Deduces the electrochemical equivalent and its relationship to Faraday's law.

17. Discusses the quantitative aspects of electrolysis.

18.Connects effort and concentration.

19.Detects the relationship between the equilibrium constant and the voltage of the measuring cell.

20.Interprets and analyzes molar conductivity and calculation of cell constant from knowledge of solution resistance and conductivity.

21. Employ his knowledge of metal and electrolytic conductivity.

22.Evaluates the reactions that occur at the electrodes of the cell.

23.Faraday Law shall apply.

24.Calculates the quantitative manifestations of electrolysis.

25. Uses his knowledge to link effort and concentration.

26.Uses the relationship between the equilibrium constant and the measuring cell voltage.

27.The cell constant is calculated from the knowledge of solution resistance and conductivity.

28. The student should be able to communicate and communicate in writing and orally.

29. The student should be able to use modern technology in searching for information.

30. The student should be able to work as a team through panel discussions.

31. Ability to self-learning and continuous.

Teaching and learning methods

1- Lecture.

2- Discussion and dialogue.

3- Collection of information.

Methods of assessments

Notes	Percentage	Evaluation weight	Evaluation duration	Evaluation methods	No.
	25%	25	Fifth week	First written test (multiple choice style and essay questions)	1
	25%	25	Tenth week	First written test (multiple choice style and essay questions)	2
	50%	50	Last week	Final Exam	3

Course Content

Week	Scientific topic	Teaching hours	Lectures	Exercises	Discussion
1-2	Metal and electrolytic conductivity	4
3-4	Comparison of galvanic cell and electrolysis	4
5	First med term exam
6	Electrolysis in an aqueous medium	2
7	Electrolysis in an aqueous medium	2
8	Faraday Rules	2
9	Quantitative manifestations of electrolysis	2
10	Second med term exam
11	The relationship between effort and concentration (Nernst equation)	2
12	Relationship between the equilibrium constant and the voltage of the measuring cell	2
13	Molar Conductance	2
14	Calculation of the cell constant from the knowledge of solution resistance and conductivity	2
15	Final exam
	Total	24

References

Reference Title	Publisher	Version	The author	Reference location
Fundamentals of Physical Chemistry			Omar Alhazazi
Physical Chemistry	Prentice-Hall	4th edition	Walter Moor	University Library

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