galvaniske

Galvaniske refers to galvanic phenomena in electrochemistry. A galvanic (or voltaic) cell converts the chemical energy released by a spontaneous redox reaction into electrical energy. In such a cell, electrons flow from a more active electrode (anode) to a less active one (cathode) through an external circuit.

Two electrodes are immersed in an electrolyte, and the electrical current is completed by a salt bridge or porous separator. The anode undergoes oxidation, releasing electrons, while the cathode undergoes reduction, consuming them. The overall reaction is spontaneous, yielding a positive cell potential under standard conditions.

Cell notation (anode | electrolyte || electrolyte | cathode) summarizes the setup. The standard cell potential, E°cell, indicates spontaneity: a positive value means the reaction can run without external energy input.

Historically, the term derives from Luigi Galvani and Alessandro Volta, who studied electricity in biological and chemical contexts. The expression galvanic is used in contrast to electrolytic, where external electrical energy drives a non-spontaneous reaction.

Applications include primary and rechargeable batteries, electroplating and metal finishing, corrosion protection, and electrochemical sensors. In energy storage, galvanic cells are the core concept behind almost all modern batteries.

Galvanic corrosion occurs when two different metals are electrically connected in an electrolyte, causing accelerated deterioration of the more active metal. Mitigation includes insulation, sacrificial anodes, coatings, and choosing materials with appropriate electrochemical potentials.

Galvaniske remains a general term describing devices and processes driven by spontaneous redox reactions, distinct from electrolytic systems that require external power.