E

Electrochemistry

E° cell = E° cathode − E° anode | ΔG° = −nFE°
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Formula / NotationE° cell = E° cathode − E° anode | ΔG° = −nFE°
Also Known AsGalvanic cell, Voltaic cell, Electrolytic cell, Redox cell

What is Electrochemistry?

The branch of chemistry concerned with the relationship between chemical changes and electrical energy. It encompasses the study of electrochemical cells, electrolysis, electrode potentials, and corrosion. Applications include batteries, fuel cells, and electroplating.

Formula & Notation

E° cell = E° cathode − E° anode | ΔG° = −nFE°

Other Names / Synonyms: Galvanic cell, Voltaic cell, Electrolytic cell, Redox cell

Properties & Characteristics

Two types: (1) Galvanic/voltaic cell — spontaneous redox reaction generates electricity (battery). (2) Electrolytic cell — external electricity drives non-spontaneous reaction. Standard hydrogen electrode (SHE) reference = 0.00 V. Faraday constant F = 96,485 C/mol. Nernst equation: E = E° − (RT/nF)ln Q. At 25°C: E = E° − (0.0592/n)log Q.

Uses & Applications

Batteries (lead-acid, Li-ion, nickel-cadmium). Fuel cells (H₂/O₂). Electroplating (Cu, Au, Ni, Cr). Electrolytic refining of metals (copper, aluminum via Hall-Héroult). Chloralkali process (Cl₂ and NaOH from NaCl electrolysis). Corrosion protection. Biosensors (glucose sensors, pH electrodes). Anodizing aluminum.

Safety Information

High-voltage electrochemical cells present electrocution hazard. Hydrogen gas produced at cathode is flammable — ensure ventilation. Lead-acid batteries contain H₂SO₄ and lead (toxic). Lithium cells can undergo thermal runaway. Electrolysis of chloride solutions produces toxic chlorine gas. Always use proper electrical isolation and ventilation.

Always consult the SDS/MSDS before handling any chemical. This information is for educational purposes only.

Key Facts

Term Electrochemistry
Formula E° cell = E° cathode − E° anode | ΔG° = −nFE°
Index All "E" terms
Synonyms Galvanic cell, Voltaic cell, Electrolytic cell, Redox cell

Frequently Asked Questions

The branch of chemistry concerned with the relationship between chemical changes and electrical energy. It encompasses the study of electrochemical cells, electrolysis, electrode potentials, and corrosion. Applications include batteries, fuel cells, and electroplating.

More "E" Terms

Effective Collisions Effective Collisions E ≥ Ea (activation energy required) Effective Molality m_eff = i × m (van't Hoff factor) Effective Nuclear Charge Z_eff = Z − σ (Slater's rules) Efflorescence Hydrated salt losing water in air: M·nH₂O(s) → M·(n-x)H₂O(s) + xH₂O(g) Einsteinium Es Electrical Conductivity κ = 1/ρ; Λm = κ/c Electrochemical Cell Galvanic cell: ΔG = −nFE_cell; Electrolytic cell: ΔG = +nFE_applied Electrochemical Series Arranged by E° (standard reduction potential); SHE: E° = 0.00 V Electrochemistry Electrode Electrode Potential E = E° − (RT/nF)ln Q
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