- 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