elektrolüütrakud

Elektrolüütrakud, also known as electrolytic cells, are electrochemical devices that use an external source of electrical energy to drive a non-spontaneous redox reaction. This process is called electrolysis. Unlike galvanic cells, which produce electricity from spontaneous chemical reactions, electrolytic cells consume electricity to force chemical change.

The fundamental components of an elektrolüütrakud include an electrolyte, which is a substance containing free ions that conducts electricity, and two electrodes, typically made of conductive materials. These electrodes are immersed in the electrolyte and are connected to an external power source, such as a battery or DC power supply. One electrode serves as the anode, where oxidation occurs, and the other as the cathode, where reduction takes place.

During operation, the external power source forces electrons to flow. At the cathode, cations in the electrolyte gain electrons and are reduced. Simultaneously, at the anode, anions lose electrons and are oxidized, with the electrons then flowing through the external circuit to the cathode. This continuous flow of electrons and ions facilitates the non-spontaneous chemical transformation.

Elektrolüütrakud have a wide range of industrial and scientific applications. They are crucial for the production of many elements and compounds, including aluminum, chlorine, and sodium hydroxide, through processes like the Hall-Héroult process and the chlor-alkali process. Electrolysis is also used for electroplating, refining metals, and in some types of batteries for charging. The specific reaction occurring in an electrolytic cell depends on the nature of the electrolyte and the applied voltage.