Abstract
This chapter presents the terminology of electrodes and electrochemical cells. It discusses Faraday's laws and the quantitative relationships in electrochemistry. The chapter describes the chemistry of some of the more common cells and batteries. It discusses fuel cells, which are still at the development stage, but may be important in the overall future energy picture. Electrochemistry deals with oxidation-reduction reactions that either produce or utilize electrical energy and electrochemical reactions take place in cells. Each cell has two electrodes, conductors through which electrons enter or leave the cell. Altogether, three things must happen in a functioning cell: (1) either oxidation or reduction occurs at each electrode, (2) electrons flow through an external conductor, and (3) ions flow in the electrolyte solution. There are two types of electrochemical cells: voltaic cell and electrolytic cell. A voltaic cell generates electrical energy from a spontaneous redox reaction. An electrolytic cell uses electrical energy from outside the cell to cause a redox reaction to occur. Electrical current is carried in the external circuit of a cell by electrons and within a cell by ions. Standard electrode potentials can be used to predict what the electrode reactions and the cell potential will be for any specific electrochemical cell. The most widely used storage cell is the lead storage cell. The chapter explains the concept of electrolysis.
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