Elektrolysen

Elektrolyse is a process that uses an electric current to drive an otherwise non-spontaneous chemical reaction. This is achieved by passing an electric current through a substance, typically an ionic compound in a molten state or dissolved in a suitable solvent, known as an electrolyte. The electrolyte contains ions that can move and conduct electricity. The electric current is supplied by electrodes, usually made of metal or graphite, inserted into the electrolyte. These electrodes are connected to a direct current power source.

The electrode connected to the positive terminal of the power source is called the anode, and the electrode connected to the negative terminal is called the cathode. At the cathode, reduction occurs, where positive ions (cations) gain electrons and become neutral atoms or molecules. At the anode, oxidation occurs, where negative ions (anions) lose electrons and become neutral atoms or molecules, or other oxidized species. These chemical changes at the electrodes are the result of the applied electric potential overcoming the inherent stability of the chemical bonds.

Common applications of electrolysis include the production of metals like aluminum and copper, the purification of metals, the production of chlorine gas and sodium hydroxide, and electroplating, where a thin layer of one metal is deposited onto another. It is also used in water splitting to produce hydrogen and oxygen gas. The efficiency and outcome of electrolysis depend on factors such as the nature of the electrolyte, the electrode material, the current density, and the temperature.