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Electrochemistry & Solid State

Electrochemical cells, electrolysis, Nernst equation, and crystal structures

Key Concepts
  • Galvanic cells convert spontaneous redox reactions into electricity
  • Electrolytic cells use external electricity to drive non-spontaneous reactions
  • The Nernst equation links cell potential to concentration
  • Faraday's laws relate deposited mass to charge passed
  • Solid state: unit cells (SC, BCC, FCC), packing efficiency and defects
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) × It
FCC / BCC edge FCC: 4r = a√2 · BCC: 4r = a√3
Crystal density ρ = ZM/(N_A·a³)
Quick Tips
  • Faraday constant F = 96,500 C/mol.
  • Packing efficiency: FCC/HCP = 74%, BCC = 68%, SC = 52%.
  • Schottky defect lowers density; Frenkel defect leaves density unchanged.
Sample Practice Questions

  1. In a galvanic cell, oxidation takes place at the:

    • Cathode
    • Anode
    • Salt bridge
    • Electrolyte
    Show answer

    Answer: Anode

  2. The value of the Faraday constant is approximately:

    • 6.022×10²³ C/mol
    • 96500 C/mol
    • 8.314 C/mol
    • 9×10⁹ C/mol
    Show answer

    Answer: 96500 C/mol

  3. The packing efficiency of a face-centred cubic (FCC) unit cell is:

    • 52%
    • 68%
    • 74%
    • 100%
    Show answer

    Answer: 74%

  4. The standard electrode potential of the standard hydrogen electrode is:

    • 0 V
    • 1 V
    • −1 V
    • 0.76 V
    Show answer

    Answer: 0 V

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