Electrochemistry (Undergraduate Foundation)

This course provides a complete guide to electrochemistry, the study of the relationship between chemical reactions and electrical energy. It covers the principles of oxidation-reduction (redox) reactions and their application in electrochemical cells. The material details the structure and function of both galvanic (voltaic) cells, which produce electricity, and electrolytic cells, which use electricity to drive non-spontaneous reactions. Electrochemistry is the science behind all modern portable energy storage and industrial metal production. The principles covered are the basis for batteries, fuel cells, and rechargeable power sources. This knowledge is also critical for understanding corrosion, electroplating, and the industrial-scale electrolysis used to produce fundamental materials like aluminium and chlorine. By the end of this course, you will be able to identify the components of any electrochemical cell and predict the direction of electron flow. You will also be able to calculate standard cell potentials using a table of standard reduction potentials, apply Faraday's laws to electrolytic calculations, and use the Nernst equation to determine cell potential under non-standard conditions. This course is for students who have a solid foundation in stoichiometry and redox reactions. It is a mandatory course for all students of chemistry and chemical engineering and is a direct prerequisite for the study of analytical chemistry, materials science, and electrical engineering.

Payment required for enrolment
Enrolment valid for 12 months
This course is also part of the following learning track. You may join the track to gain comprehensive knowledge across related courses.
[NUC Core] CHM 101: General Chemistry I
[NUC Core] CHM 101: General Chemistry I
This learning track delivers the complete NUC CCMAS curriculum for General Chemistry I. It is a comprehensive programme designed to build a robust, university-level foundation in modern chemistry. The track systematically covers all essential topics, from atomic theory, chemical bonding, and the states of matter, to the quantitative principles of stoichiometry, equilibrium, thermodynamics, and kinetics. This programme is for first-year undergraduates in science, technology, engineering, and mathematics (STEM) faculties who are required to take CHM 101. It is also essential for any student or professional globally who needs a rigorous and complete foundation in first-year university chemistry for further study or career development. This track delivers a full skill set in chemical theory and quantitative problem-solving. Graduates will be able to determine molecular structures, calculate reaction quantities, analyse the energetics and rates of reactions, and solve complex equilibrium problems. This programme provides the non-negotiable prerequisite knowledge for all subsequent chemistry courses and for any degree in the physical sciences, engineering, or medicine.

This learning track delivers the complete NUC CCMAS curriculum for General Chemistry I. It is a comprehensive programme designed to build a robust, university-level foundation in modern chemistry. The track systematically covers all essential topics, from atomic theory, chemical bonding, and the states of matter, to the quantitative principles of stoichiometry, equilibrium, thermodynamics, and kinetics. This programme is for first-year undergraduates in science, technology, engineering, and mathematics (STEM) faculties who are required to take CHM 101. It is also essential for any student or professional globally who needs a rigorous and complete foundation in first-year university chemistry for further study or career development. This track delivers a full skill set in chemical theory and quantitative problem-solving. Graduates will be able to determine molecular structures, calculate reaction quantities, analyse the energetics and rates of reactions, and solve complex equilibrium problems. This programme provides the non-negotiable prerequisite knowledge for all subsequent chemistry courses and for any degree in the physical sciences, engineering, or medicine.

Course Chapters

1. Introduction
1

This chapter provides the roadmap for the course. It introduces electrochemistry as the study of the interplay between chemical reactions and electrical energy, outlining the key topics of galvanic and electrolytic cells. Key learning objectives include: understanding the overall course structure and appreciating the role of electrochemistry in energy storage and industrial processes.

Chapter lessons

1-1. Welcome

This lesson provides a brief overview of the course, outlining the key topics of electrochemical cells, cell potentials, and electrolysis.

2. Galvanic Cells
3
4

This chapter covers galvanic (or voltaic) cells, which use spontaneous redox reactions to generate electrical energy. It details the components of these cells and the principles of cell potential. Key learning objectives include: identifying the anode, cathode, and salt bridge in a galvanic cell; and calculating the standard cell potential (E°cell) using standard reduction potentials.

Chapter lessons

2-1. Cell components

This lesson defines the components of a galvanic cell: the anode (oxidation), the cathode (reduction), the salt bridge, and the external circuit.

2-2. Cell notation

This lesson introduces the standard line notation used to represent electrochemical cells in a concise format.

2-3. Standard cell potential

This lesson defines standard reduction potentials and explains how to use them to calculate the standard cell potential (E°cell) for any galvanic cell.

3. Thermodynamics and Cell Potential
2
4

This chapter connects electrochemistry to thermodynamics. It explores the relationship between cell potential, Gibbs free energy, and the equilibrium constant. Key learning objectives include: calculating the change in Gibbs free energy from the cell potential; and using the Nernst equation to find the cell potential under non-standard conditions.

Chapter lessons

3-1. Free energy link

This lesson introduces the equation ΔG° = -nFE°cell, which directly relates the standard cell potential to the standard change in Gibbs free energy.

3-2. The Nernst equation

This lesson introduces the Nernst equation, which is used to calculate the cell potential under non-standard conditions of concentration or pressure.

4. Electrolytic Cells
2
4

This chapter covers electrolytic cells, which use an external source of electrical energy to drive non-spontaneous chemical reactions. The focus is on the quantitative aspects of electrolysis as described by Faraday's laws. Key learning objectives include: distinguishing between galvanic and electrolytic cells; and applying Faraday's laws to perform stoichiometric calculations for electrolysis.

Chapter lessons

4-1. Defining electrolysis

This lesson defines an electrolytic cell and explains how it differs from a galvanic cell in both function and construction.

4-2. Faraday's laws

This lesson introduces Faraday's laws of electrolysis, which quantitatively relate the amount of substance produced or consumed to the total electric charge passed through the cell.

5. Conclusion
2

This concluding chapter summarises the key concepts of electrochemistry. It reinforces the understanding of how chemical and electrical energy are interconverted in electrochemical cells. This summary prepares the student for the final course, 'Radioactivity', which explores reactions that occur within the atomic nucleus itself.

Chapter lessons

5-1. Course summary

This lesson consolidates knowledge by reviewing the principles of galvanic cells, electrolytic cells, cell potentials, and the quantitative laws of electrolysis.

5-2. Next steps

This final lesson looks ahead, explaining how the principles of electron transfer in electrochemistry are a conceptual bridge to the study of subatomic particles in nuclear chemistry.