UDC 004 THE CONCEPT OF ELECTROLYSIS CHARACTERISTICS OF ELECTROCHEMICAL PROCESS Orynbek A. – students of ХТ-20-14к Seitmagzimova G. – senior teacher Electrochemical reaction, any process either caused or accompanied by the passage of an electric current and involving in most cases the transfer of electrons between two substances—one a solid and the other a liquid. Under ordinary conditions, the occurrence of a chemical reaction is accompanied by the liberation or absorption of heat and not of any other form of energy; but there are many chemical reactions that—when allowed to proceed in contact with two electronic conductors, separated by conducting wires—liberate what is called electrical energy, and an electric current is generated. Conversely, the energy of an electric current can be used to bring about many chemical reactions that do not occur spontaneously. A process involving the direct conversion of chemical energy when suitably organized constitutes an electrical cell. A process whereby electrical energy is converted directly into chemical energy is one of electrolysis; i.e., an electrolytic process. By virtue of their combined chemical energy, the products of an electrolytic process have a tendency to react spontaneously with one another, reproducing the substances that were reactants and were therefore consumed during the electrolysis. If this reverse reaction is allowed to occur under proper conditions, a large proportion of the electrical energy used in the electrolysis may be regenerated. This possibility is made use of in accumulators or storage cells, sets of which are known as storage batteries. The charging of an accumulator is a process of electrolysis; a chemical change is produced by the electric current passing through it. In the discharge of the cell, the reverse chemical change occurs, the accumulator acting as a cell that produces an electric current. Finally, the passage of electricity through gases generally causes chemical changes, and this kind of reaction forms a separate branch of electrochemistry that will not be treated here. Substances that are reasonably good conductors of electricity may be divided into two groups: the metallic, or electronic, conductors and the electrolytic conductors. The metals and many nonmetallic substances such as graphite, manganese dioxide, and lead sulfide exhibit metallic conductivity; the passage of an electric current through them produces heating and magnetic effects but no chemical changes. Electrolytic conductors, or electrolytes, comprise most acids, bases, and salts, either in the molten condition or in solution in water or other solvents. Plates or rods composed of a suitable metallic conductor dipping into the fluid electrolyte are employed to conduct the current into and out of the liquid; i.e., to act as electrodes. When a current is passed between electrodes through an electrolyte, not only are heating and magnetic effects produced but also definite chemical changes occur. At or in the neighbourhood of the negative electrode, called the cathode, the chemical change may be the deposition of a metal or the liberation of hydrogen and formation of a basic substance or some other chemical reduction process; at the positive electrode, or anode, it may be the dissolution of the anode itself, the liberation of a nonmetal, the production of oxygen and an acidic substance, or some other chemical oxidation process. An electrolyte, prepared either by the melting of a suitable substance or by the dissolving of it in water or other liquid, owes its characteristic properties to the presence in it of electrically charged atoms or groups of atoms produced by the spontaneous splitting up or dissociation of the molecules of the substance. In solutions of the so-called strong electrolytes, most of the original substance, or in some solutions perhaps all of it, has undergone this process of electrolytic dissociation into charged particles, or ions. When an electrical potential difference (i.e., a difference in degree of electrification) is established between electrodes dipping into an electrolyte, positively charged ions move toward the cathode and ions bearing negative charges move toward the anode. The electric current is carried through the electrolyte by this migration of the ions. When an ion reaches the electrode of opposite polarity, its electrical charge is donated to the metal, or an electric charge is received from the metal. The ion is thereby converted into an ordinary neutral atom or group of atoms. It is this discharge of ions that gives rise to one of the types of chemical changes occurring at electrodes. The study of electrochemistry began in the 18th century, bloomed until the early 20th century, and then faded, owing to an excessive use of thermodynamic principles in analyzing the processes that take place at points in the system where the various parts form interfaces. Since about 1950 electrochemistry has undergone a change. The study of processes in solutions has been less stressed, but the study of the transfer of electrons between metals and solution has increased explosively. With this new emphasis electrochemistry is becoming a core science. It promises to be an important part of the foundation of the ecology-oriented society of the future, because electricity is not a pollutant. The pollution associated with some methods of generating electricity must, however, be reduced. Alkali metal hydroxides are manufactured in the United States to the extent of approximately 36,500 tons/day, almost entirely by the electrolysis of aqueous brine solutions. In addition to sodium hydroxide the electrochemical synthesis results in the co-production of chlorine. Unlike alkali metal hydroxides, chlorine produced at the anode of an electrolytic cell in stoichiometric quantities to sodium hydroxide has experienced a declining market because of environmental problems. For example, use of chlorine by the pulp and paper industry has been declining because of traces of dioxin formed in paper products; chlorine in the treatment of sewage and water has been shown to lead to the production of toxic organo-chlorine compounds; compounds like the chlorofluorocarbons and methyl chloroform have been found to be destructive to the earth's protective ozone layer, and certain chlorine-containing pesticides have been shown to be toxic to biological systems. Consequently, it is expected that the declining demand for chlorine will continue to weaken in the approaching decades. By contrast, the demand for alkali metal hydroxides, like caustic soda is expected to remain strong. Accordingly, in view of the declining demand for chlorine and the absence of economical routes for its destruction or safe storage there is a growing need for new and more economical processes for the manufacture of high purity alkali metal hydroxides which do not also produce halogens. A number of methods have been developed for the production of alkali metal hydroxides without the simultaneous production of chlorine. While most methods are effective in eliminating the problems associated with the co-production of chlorine most have not been viewed as commercially acceptable because of various shortcomings, e.g. inefficient consumption of power, inability to produce a sufficiently pure grade of caustic soda and/or co- production of other less desirable products. The lime-soda process has several shortcomings. It is difficult to carry out to full conversion; the caustic soda is impure and the process is energy inefficient, particularly if there is any attempt to recycle the calcium by thermal decomposition of the carbonate to oxide. References: 1. Oesper, Ralph; Speter, Max (1937). "The Faraday-Whewell correspondence concerning electro-chemical terms". The Scientific Monthly. 45 (6): 535–546. 2. ^ Fabbri, Emiliana; Schmidt, Thomas J. (5 October 2018). "Oxygen Evolution Reaction—The Enigma in Water Electrolysis". ACS Catalysis. 8 (10): 9765–9774. doi:10.1021/acscatal.8b02712. 3. ^ Ashworth, William (20 March 2015). "Martinus van Marum - Scientist of the Day". Linda Hall Library. 4. ^ Ihde, Aaron J. (1964). The Development of Modern Chemistry. Harper & Row. pp. 125–127. 5. ^ Jump up to:a b "The History of Electrochemistry: From Volta to Edison". ECS. Retrieved 11 October 2019. 6. ^ Thorpe, Thomas (1896). Humphry Davy, Poet and Philosopher. New York: Macmillan & Co., Limited.
