Fundamentals of Lead—Acid Batteries

An electrochemical power source comprises two electrodes of different materials immersed in electrolyte, whereby electrode systems with different potentials are formed at the two electrodes. Electrochemical reactions proceed at the two interfaces which involve transfer of electrons between the electrode surface and ions from the solution. The difference between the potentials of the two electrodes generates the electromotive force of the electrochemical power source. When the two electrodes (anode and cathode) are connected to a conductor with a load, electric current which can do work flows between them, i.e., the chemical energy can be converted into an electrical one. Electric current flows due to changes of the valences of the materials at the two electrodes. Michael Faraday established that, when one gram equivalent of any substance takes part in an electrochemical reaction, the quantity of electricity that flows is always equal to 96,487 coulombs (C). This value is called Faraday constant, after the name of M. Faraday, and is denoted by the symbol F. The value of the constant is generally rounded to 96,5(X) C. [Pg.29]

The electric energy, Q, that an electrochemical power source can deliver when one gram mole (atom) of material takes part in the electrochemical reactions at the two electrodes is equal to [Pg.29]

Gaston Plante combined a Pb/PbS04 with a Pb02/PbS04 electrode in sulfuric acid solution and obtained an electrochemical power source with high electromotive force. In 1860, he announced the invention of this power source as an electrochemical lead—acid cell of high power at a meeting of the French Academy of Sciences. [Pg.29]

The lead—acid cell utilises the reactions of lead oxidation (Pb Pb + 2e ) and of lead [Pg.29]

Lead Acid Batteries Science and Technology. DOI 10.1016/B978-0-444-52882-7.10002-3 2011 Elsevier B.V. All rights reserved. [Pg.29]

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