How much charge is required for the reduction of one mole of MnO4- to…

An electrochemical cell consists of two metallic electrodes (anode and cathode) dipping in electrolytic solutions. Oxidation takes place at the anode and reduction takes place at the cathode. These cells are of two types:

1) Galvanic cells, in which the chemical energy of a spontaneous redox reaction is converted into electrical energy. E^o_cell = E^o_cathode - E^o_anode, where E^o_cell is the standard potential of the cell, and Δ_rG^o = -nFE^o_cell, where Δ_rG^o is the standard Gibbs energy change of the cell reaction.

2) Electrolytic cells, in which electrical energy is used to carry out a non-spontaneous redox reaction. The amount of substance produced at an electrode depends on the quantity of electricity passed, Q = I × t (where I is the current in ampere and t is the time in seconds). One faraday is the charge carried by 1 mole of electrons, that is 96500 C.

The conductivity (κ) of an electrolytic solution depends on the nature and the concentration of the electrolyte. According to Kohlrausch’s law of independent migration of ions, the limiting molar conductivity of an electrolyte is the sum of the limiting molar conductivities of its cation and anion, for example Λ^o_m(NaCl) = λ^o_Na⁺ + λ^o_Cl^–, where λ^o is the limiting molar conductivity of an ion. The law can be used to calculate the limiting molar conductivity of weak electrolytes.