elektrochemin

Elektrochemin, also known as electrochemistry, is the branch of chemistry that studies chemical processes that are driven by electrical energy or involve electron transfer at interfaces between electrodes and electrolytes. It unites concepts from chemistry and electricity to understand how redox reactions occur at electrode surfaces and how electrical energy can be generated or consumed by chemical systems.

Core concepts include electrode potentials, standard reduction potentials, the Nernst equation, and Faraday's laws, which relate the amount of substance transformed to the charge passed. The basic components of electrochemical systems are electrodes, an electrolyte, and an external circuit that connects the electrodes. In galvanic (voltaic) cells, chemical reactions generate electrical energy, while in electrolysis, electrical energy drives non-spontaneous chemical reactions.

Common techniques used to study electrochemical processes include cyclic voltammetry and chronoamperometry, which provide information about reaction mechanisms, kinetics, and concentration. Applications of elektrochemin span several domains. In energy storage and conversion, batteries, fuel cells, and supercapacitors rely on electrochemical reactions. In materials processing, electroplating, electrodeposition, and electropolishing use controlled electrode reactions. Electrosynthesis leverages electrochemistry for chemical production, including chlorine and caustic alkali generation in the chlor-alkali process. Corrosion protection is enhanced by methods such as cathodic protection. Electrochemical sensors detect chemical species in environmental, medical, and industrial contexts, including glucose and other biomolecule sensors.

Historically, the field advanced with Volta’s early galvanic cells and Faraday’s laws in the 19th century, with further developments shaping modern analytical and energy technologies.