Electrochemical Cells

A device that can either produce electrical energy from chemical processes or use chemical reactions to generate electrical energy is called an electrochemical cell. Voltaic or galvanic cells are electrochemical devices that produce an electric current, and electrolytic cells are devices that produce chemical processes, such as electrolysis. A typical illustration of a galvanic cell is a 1.5 volt cell intended for home usage. better source needed] One or more cells that are linked in parallel, series, or series-and-parallel make up a battery. An electrolyte, two electrodes, and an electrolytic cell make up an electrolytic cell (a cathode and an anode). The electrolyte is often a mixture of ions that have been dissolved in water or another solvent. Electrolytes include molten salts like sodium chloride. The ions in the electrolyte are drawn to an electrode with the opposite charge when an external voltage is supplied to the electrodes, which can then drive charge-transferring (also known as faradaic or redox) processes. A typically stable or inert chemical substance in the solution can only be broken down by an electrolytic cell with an external electrical potential (i.e. voltage) of the right polarity and adequate magnitude. Chemical reactions that would not normally happen spontaneously can be produced by the electrical energy used.