Elektrokemisk

Elektrokemisk, or electrochemistry, is a field of chemistry that studies chemical reactions driven by electrical energy or that produce electrical energy through redox processes. At its core are electrodes, an electrolyte, and a driving potential: oxidation reactions occur at the anode, reduction at the cathode, with ion movement in the electrolyte maintaining charge balance. The potential difference between electrodes is described by electrode potentials and, under standard conditions, by standard reduction potentials. The Nernst equation relates cell potential to concentrations.

Electric charge transfer adheres to Faraday's laws: the amount of substance transformed is proportional to the total electric charge passed. This underpins quantitative electrochemistry and electrolysis. Electrochemical cells are broadly categorized as galvanic (voltaic) cells, which generate electrical energy from chemical reactions, and electrolytic cells, which drive non-spontaneous reactions with external power. Modern electrochemistry includes techniques such as potentiometry, voltammetry, chronometry, and electrochemical impedance spectroscopy for analysis and sensing.

Key applications include energy storage and conversion (batteries, fuel cells, and supercapacitors); electroplating and refining of metals; corrosion prevention and protection; electroanalysis and biosensing; and electrosynthesis for chemical manufacturing. Historical developments trace to pioneers such as Volta, Galvani, Faraday, and Nernst, whose work established fundamental concepts of cell potentials, charge transfer, and reaction kinetics. The field continues to advance in materials science, renewable energy, and environmental monitoring, linking fundamental redox chemistry with practical technologies.