Question

State Faraday's laws of electrolysis.

Answer 1

Faraday's first law of electrolysis:
The amount of the substance that undergoes oxidation or reduction at each electrode during electrolysis is directly proportional to the amount of electricity that passes through the cell.
Thus mass of the substance produced
$=\frac{\text{I(A)}\times \text{t(s)}}{{\text{96500 C/mol e}}^{-}}\times \text{mole ratio}\times \text{molar mass}$
Here I(A) is current in ampere and t(s) is time in second.
Faraday's second law of electrolysis:
When the same amount of electricity is passed through different cells containing different electrolytes and arranged in series, the amounts of substances oxidized or reduced at the respective electrodes are directly proportional to their chemical equivalent masses.
$\frac{\text{moles of A produced}}{\text{moles of B produced}}=\frac{\text{mole ratio of A half reaction}}{\text{mole ratio of B half reaction}}$