Course overview
Did you know that photosynthesis (the reaction of water and carbon dioxide to produce glucose and oxygen) is a redox reaction in which water becomes oxidised and carbon dioxide becomes reduced? This electrochemistry course explains redox reactions in electrolysis cells, how to measure the electrode potential and how to utilise the Nernst equation to determine the cell potential under non-standard conditions. Sign up to master electrochemistry.
Course description
This advanced chemistry course delves into electrochemistry and explains electrolysis, electrode potential, cells and batteries. We begin by discussing redox reactions found in two types: oxidation and reduction reactions. We then describe the chemical reactions influenced by a passing current (called ‘electrolysis’), the electrolysis cell with its components and reactions at the anode and cathode. We then explain how to use quantitative electrolysis to determine the amount of metal deposited when passing a specific current. The course shows you how to calculate the Avogadro constant using an electrolytic method.
The course then moves on to electrode potential and lays out the method of measuring the electrode potential of a half-cell using a reference electrode (for example, a standard hydrogen electrode with a known potential). We also investigate galvanic cells (voltaic cells), which use spontaneous redox reactions to produce electricity, and their constituent parts. We also compare electrolytic and galvanic cells. The course then examines standard cell potential, cell voltage (standard cell potential) and how temperature, pressure or concentration affect the electrode potential.
We then cover the Nernst equation, which relates the electrode potential to the temperature and concentration of an electrode. The course investigates primary batteries (non-chargeable disposable batteries), including cylindrical and button primary batteries along with their components, and some secondary batteries (rechargeable) such as lead and Lithium-ion batteries, along with their usage in cars and electronics. We also discuss hydrogen-oxygen fuel cells that power automobiles by generating energy through a redox reaction. Finally, we outline the use of molten electrolytes and aqueous electrolytes. This advanced chemistry course suits chemistry students and aspiring electrical engineers. Sign up to learn more about batteries and electrochemistry.
Entry requirements
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Learning outcome
- Define ‘electrolysis’, ‘redox reactions’, ‘standard electrode potential’, ‘redox equilibrium’, ‘half-cell’ and ‘cells and batteries’
- Describe the electrolysis cell composition, redox reactions in the electrolysis cell, the galvanic cell components and the Nernst equation formula
- Calculate the amount of a substance produced during electrolysis, the Avogadro constant by an electrolytic method and the cell potential under non-standard conditions
- Explain how to write the oxidation-reduction reaction and the half-cell
- Summarise the galvanic cell components, primary and secondary batteries and their components
- Discuss hydrogen cell components and their chemistry
- Identify the voltage measured under standard conditions using a standard hydrogen electrodes
- List the advantages and limitations of hydrogen fuel cells and the various types of half-cells
Knowledge and skills you will learn
Course options
Course Type: Online
Details
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