To succeed in this topic, you need to:
• Be familiar with redox chemistry involving the loss of electrons (oxidation) and gain of electrons (reduction).
• Be familiar with chemical species having different oxidation states, i.e. oxidation numbers.
• Be familiar with electrochemical half-cells, including the standard hydrogen electrode, and the standard electrode potential for any given half-cell.

After working through this Chemistry Factsheet, you will:

• Be aware that redox reactions create an electromotive force (emf), due to the electrical potential formed between two different electrochemical half-cells.
• Be aware of methods for calculating the electrode potential between two different electrochemical half-cells.
• Be aware of the Nernst equation and its use in determining the electrode potential between half-cells with non-standard concentrations.

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Publication Date

January 2019


ISSN: 1351-5136

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288 Electrochemical Calculations

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