AP Chemistry Unit 9.10 Electrolysis and Faraday’s Law

Electrolysis and Faraday’s Law

  • Electrolysis: the process of creating an electrolyte cell
    • Used for electroplating
  • Electrolyte cell: runs by running a galvanic cell backwards → the electrons are flowing in the opposite direction
    • In galvanic cells, electron flow is a spontaneous process; in electrolytic cells it is nonspontaneous
  • For electrolysis, the total cell potential (E) will be negative → ΔG° = + (Unfavorable process)

Electrolytic Cell (Electrolysis)

Stoichiometry of Electrolysis

  • Shortcut:
    • A = time in seconds
    • M = molar mass
    • Fe- = Faraday’s constant

Faraday’s Law

  • (on RFS) → the amount of charge that flows thru an electrolytic cell is a factor of the current and time that its running
    • I = current
    • Q = charge (in coulombs)
    • T = time
  • One Faraday = one mole of electrons “pushed” thru the wire
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