Electrochemical Cell
| Formula / Notation | Galvanic cell: ΔG = −nFE_cell; Electrolytic cell: ΔG = +nFE_applied |
|---|---|
| Also Known As | Galvanic cell, electrolytic cell, voltaic cell, Daniell cell (example) |
What is Electrochemical Cell?
A device that either converts chemical energy into electrical energy (galvanic cell) or uses electrical energy to drive a chemical reaction (electrolytic cell). All electrochemical cells consist of two electrodes and an electrolyte through which ions can flow.
Formula & Notation
Other Names / Synonyms: Galvanic cell, electrolytic cell, voltaic cell, Daniell cell (example)
Properties & Characteristics
Uses & Applications
Safety Information
Always consult the SDS/MSDS before handling any chemical. This information is for educational purposes only.
Key Facts
Frequently Asked Questions
A device that either converts chemical energy into electrical energy (galvanic cell) or uses electrical energy to drive a chemical reaction (electrolytic cell). All electrochemical cells consist of two electrodes and an electrolyte through which ions can flow.
Electrochemical cells are the basis of batteries (galvanic), fuel cells (galvanic), electrolysis (industrial electrolytic), electroplating (electrolytic), corrosion protection (galvanic/electrolytic), and analytical electrochemistry (potentiometry, voltammetry, coulometry).
Electrochemical cells can generate flammable or toxic gases (H₂, Cl₂, O₂). Electrolytes may be corrosive (H₂SO₄) or toxic (KCN). High currents cause heat and fire hazards. Lithium batteries can undergo thermal runaway with fire and toxic gas release if damaged or improperly charged.
The formula or notation for Electrochemical Cell is: Galvanic cell: ΔG = −nFE_cell; Electrolytic cell: ΔG = +nFE_applied