(1.6 × 10−19)(6.022 × 1023 ) = 96,487 C/mol e−This number is called Faraday’s constant, and one Faraday (F) is equivalent to the amount of charge
contained in one mole of electrons (1 F = 96,487 coulombs, or J/V).
An example of an electrolytic cell, in which molten NaCl is electrolyzed to form Cl 2 (g) and Na(l), is
given below:
In this cell, Na+ ions migrate toward the cathode, where they are reduced to Na (l). Similarly, Cl− ions
migrate toward the anode, where they are oxidized to Cl 2 (g).
ELECTRODE CHARGE DESIGNATIONS
The anode of an electrolytic cell is considered positive, since it is attached to the positive pole of the
battery and so attracts anions from the solution. The anode of a galvanic cell, on the other hand, is
considered negative because the spontaneous oxidation reaction that takes place at the galvanic
cell’s anode is the original source of that cell’s negative charge, i.e., is the source of electrons. In
spite of this difference in designating charge, oxidation takes place at the anode in both types of
cells, and electrons always flow through the wire from the anode to the cathode.