• 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)

              ○ The E°cell will be the amount of energy supplied

  • Which reaction to flip? flip the sign of the reaction that leads to a E° when both are summed

Electrolytic Cell (Electrolysis)

Stoichiometry of Electrolysis

  •  Shortcut:

           ○ A = amperes

           ○ t = time in seconds

           ○ M = atomic mass of the metal

           ○ F = Faraday’s constant (in Joules)

          ○ e- = number of electrons in half-reaction

Faraday’s Law

(on RFS) → use this equation for electroplating questions

           ○ I = current required for electroplating

                  ■ More e- in half-reaction (q) and shorter time = requires more current for electroplating

            ○ Q = (moles of sample)(e- in half reaction)(Faraday’s constant)

            ○ T = time

  • One Faraday = one mole of electrons “pushed” thru the wire

             ○ When given Faraday’s → easier to use dimensional analysis