elektrochimische

Elektrochimische (electrochemical) refers to processes, phenomena, or devices that involve the interconversion of chemical energy and electrical energy, typically through redox reactions at interfaces between an electrode and an electrolyte. The term is used in German and in English texts to describe electrochemical reactions and systems.

In an electrochemical system, reactions occur at electrodes immersed in an electrolyte. An anode is where oxidation takes place and electrons leave the species, while a cathode is where reduction occurs and electrons arrive. The electrolyte conducts ions but is not conductive to electrons. The potential difference between the electrodes drives current and determines reaction rates, often described by principles such as the Nernst equation and overpotential considerations.

Common electrochemical configurations include galvanic (voltaic) cells, which generate electrical energy from chemical reactions; and electrolytic cells, which use electrical energy to drive non-spontaneous chemical processes. Key concepts in electrochemistry include electrode potentials, charge transfer at the electrode–electrolyte interface, double-layer structure, and diffusion of species to and from the electrode surfaces.

Techniques used to study electrochemical systems include voltammetry, chronoamperometry, chronopotentiometry, and impedance spectroscopy. These methods help reveal reaction mechanisms, kinetics, diffusion behavior, and the properties of materials used as electrodes and electrolytes.

Applications span energy storage and conversion (batteries, supercapacitors, fuel cells), electroplating and electroforming, corrosion protection and monitoring, electrochemical sensors, and processes such as water splitting and chlorine production. The field underpins both fundamental science and a wide range of technologies driving modern industry.