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Electrochemistry
Electrochemical cells, Nernst equation, conductance
Key Concepts
- Galvanic (voltaic) cell: spontaneous redox reaction generates electricity
- Electrolytic cell: non-spontaneous reaction driven by external electricity
- Standard hydrogen electrode (SHE): E° = 0 V (reference)
- Higher reduction potential → stronger oxidising agent
- Faraday's laws: mass deposited proportional to charge passed and equivalent weight
Important Formulae
| Cell EMF | E_cell = E°_cathode − E°_anode |
| Nernst equation | E = E° − (RT/nF) ln Q |
| ΔG and EMF | ΔG° = −nFE° |
| Faraday's first law | m = (M/nF) × Q = (M/nF) × It |
| Kohlrausch's law | Λ°_m = Σ(λ° ions) |
Quick Tips
- Faraday constant F = 96,485 C/mol ≈ 96,500 C/mol.
- At equilibrium: E_cell = 0; ΔG = 0; Nernst gives E° = (RT/nF) ln K.
- Specific conductance decreases on dilution; molar conductance increases.
Practice Questions
Practice 20 randomly selected NEET questions on Electrochemistry. Answers are revealed after each question.
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