Elektrolízises

Elektrolízises is a chemical process that uses direct electric current to drive an otherwise non-spontaneous chemical reaction. In this process, an electrolyte, which is a substance containing free ions, is decomposed. Electrolysis is a method of using electricity to break down compounds. The word "electrolysis" was coined by Oliver Wolcott Gibbs in 1856, derived from the Greek words "electro" meaning electricity and "lysis" meaning to split.

The process requires an electrolytic cell, which consists of an electrolyte and two electrodes. The electrodes are typically made of inert materials like platinum or graphite, or they can be reactive. A direct current power source is connected to the electrodes. The negative electrode is called the cathode, and the positive electrode is called the anode. During electrolysis, positively charged ions (cations) in the electrolyte migrate towards the cathode, where they gain electrons and are reduced. Negatively charged ions (anions) migrate towards the anode, where they lose electrons and are oxidized.

Common applications of electrolysis include the production of aluminum metal from its ore, the refining of copper, and the electroplating of metals. It is also used in the production of chlorine and sodium hydroxide through the electrolysis of brine. The principles of electrolysis are fundamental to electrochemistry and have significant industrial and scientific importance.