elektroosissilises

Elektroosissilises refers to the process of using electricity to drive a non-spontaneous chemical reaction. It is the reverse of a galvanic cell, where a spontaneous reaction produces electricity. In an electrolytic cell, an external power source, such as a battery or DC power supply, is used to force electrons to flow through a circuit containing an electrolyte.

The electrolyte is a substance that contains free ions and can conduct electricity. These ions are typically dissolved in a solvent or are molten. When an electric current is applied, the positive ions (cations) in the electrolyte migrate towards the negative electrode (cathode), where they gain electrons and are reduced. Simultaneously, the negative ions (anions) migrate towards the positive electrode (anode), where they lose electrons and are oxidized.

Common applications of electrolysis include electroplating, where a thin layer of metal is deposited onto another object for decorative or protective purposes. It is also used in the purification of metals, such as copper and aluminum. The production of chemicals like chlorine gas and sodium hydroxide is another significant industrial application. Electrolysis plays a crucial role in the refining of metals, the production of essential industrial chemicals, and the creation of protective coatings. The fundamental principle involves the decomposition of substances through the passage of electric current.