elektrochemisches

Elektrochemisches, in German often used as elektrochemische or elektrochemischer, refers to processes where chemical change is coupled to electric energy, typically involving electron transfer at electrode–electrolyte interfaces. The field of electrochemistry studies these processes, including their thermodynamics, kinetics, and applications.

Core concepts include redox reactions, electrodes (anode and cathode), electrolytes, and ion transport. An electrochemical cell can operate as a voltaic (galvanic) device converting chemical energy to electrical energy, or as an electrolytic device using electrical energy to drive non-spontaneous reactions. Electrode potentials, the Nernst equation, and overpotential describe driving forces and reaction rates at surfaces.

Techniques and instrumentation: potentiometry, voltammetry, chronometry, and electrochemical impedance spectroscopy (EIS). Common setups use a working, reference, and counter electrode; reference electrodes such as Ag/AgCl or the standard hydrogen electrode provide a stable potential. Measurements are performed under defined conditions, often with specialized buffers and controlled temperature.

Applications span energy storage and conversion (batteries, fuel cells, supercapacitors), electrolysis and material synthesis (water splitting, chlorine production, electrodeposition), corrosion protection and surface finishing, and electroanalytical sensors for environmental, medical, and industrial analysis.

Historically, elektrochemische research traces to Galvani and Volta and matured through Faraday’s laws linking charge to chemical change. Today the field spans physical chemistry, materials science, and chemical engineering, integrating theory and practice to understand interfaces and to develop devices and sensors.