Electrochemical cell in which spontaneous redox drives electron flow through an external circuit, producing useful electrical work. Two half-cells (anode oxidation, cathode reduction) connected by a salt bridge.
Galvanic cell
Related concepts
- Oxidation-reduction (redox)
- Standard electrode potential (E°)
- Battery
- Fuel cell
- Anode and cathode
- Standard hydrogen electrode (SHE)
- Nernst equation: E = E° − (RT/nF) ln Q (equilibrium-potentiometry backbone)
- Butler-Volmer: i = i₀ [exp(αFη/RT) − exp(−(1−α)Fη/RT)] (symmetric α=1/2 ⇒ 2 i₀ sinh)
- Nernst: Q=1 ⇒ E = E°; log(1) = 0; E − E° = 0 at standard state
- α=1/2 BV: i = 2 i₀ sinh(Fη/(2RT)); rewrite(exp) residual 0; i(η=0)=0