Abstract
Electrochemistry is concerned with the effect of electrical voltages and currents on chemical reactions (ionics) and chemical changes which produce the voltages and currents (electrodics). This is illustrated in Table 9.1 where ionics is governed by Faraday’s laws, whereas electrodics is determined by the Nernst equation.
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Notes
- 1.
The ground state electronic configuration of Al is 1s22s22p63s23p1, and it would be expected for Al to have a (+1) oxidation state. This is in fact the case, and at high temperatures, the reaction.
$$ {{ AlC}}{{{ l}}_{{{3}({\rm{g}})}}} + {{ 2A}}{{{ l}}_{{({3})}}} = {{ 3AlC}}{{{ l}}_{{\left( {\rm{g}} \right)}}} $$occurs. However, attempts to electrolyze A1C1 have so far proved to be unsuccessful.
- 2.
The standard potential of the hydrogen electrode (SHE) is defined as zero at all temperatures for [H+]aq = 1 M and P(H2) = 1 atm.
Further Reading
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Electrochemistry lecture notes
http://www.chem.ualberta.ca/courses/plambeck/pl02/p0209x.htm
http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch20/electroframe.html
http://www.chem 1.com/CB l.htm
Help files for Electrochemistry http://www.learn.chem.vt.edu/tutorials/electrochem/
Batteries http://www.panasonic.com/
Batteries http://www.varta.com/
All about batteries http://www.howstuffworks.com/battery.htm
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Roussak, O.V., Gesser, H.D. (2012). Electrochemistry, Batteries, and Fuel Cells. In: Applied Chemistry. Springer, Boston, MA. https://doi.org/10.1007/978-1-4614-4262-2_9
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