Electrolytic Cells
Galvanic
cells have Eºcell
positive – they go in whatever direction is natural for them.
Electrolytic cells have Eºcell negative – they are forced to go backwards using a battery or some other source of electricity.
Electrolytic cells are, basically, galvanic cells that are forced to go in reverse.
Recall the reaction and Eºcell from the galvanic cell example:
Electrolytic cells have Eºcell negative – they are forced to go backwards using a battery or some other source of electricity.
Electrolytic cells are, basically, galvanic cells that are forced to go in reverse.
Recall the reaction and Eºcell from the galvanic cell example:
If
the reaction is allowed to go naturally, Cl2
will be consumed, Br2
will be produced, and 0.292 V of potential difference will be
produced between the two beakers.
OR, we could create an electrolytic cell, and APPLY a voltage of 0.292 V (or more). This would force the reaction to go backwards, so we'll consume Br2 and produce Cl2.
Note: oxidation still occurs at the “anode” and reduction still occurs at the “cathode” ... but now the anode and cathode have switched!
OR, we could create an electrolytic cell, and APPLY a voltage of 0.292 V (or more). This would force the reaction to go backwards, so we'll consume Br2 and produce Cl2.
Note: oxidation still occurs at the “anode” and reduction still occurs at the “cathode” ... but now the anode and cathode have switched!
