Faraday’s Laws of Electrolysis chapter 3 can study by students of class 12. These definitiona and formulas of Class 12 Chemistry Chapter 3: Electrochemistry is developed and witten by our expert teachers. Chemistry formulas. Faraday’s Laws of Electrolysis is prepapred and collected from varius resources to help the students.
What are the Faraday’s Laws of Electrolysis?
First law
The amount of chemical reaction which occurs at any electrode during electrolysis by a current is proportional to the quantity of electricity passed through the electrolyte (solution or melt).
Second law
The amounts of different substances liberated by the same quantity of electricity passing through the electrolytic solution are proportional to their chemical equivalent weights (Atomic Mass of Metal ÷ Number of electrons required to reduce the cation).
It is obvious that one mole of Mg2+ and Al3+ require 2 mol of electrons (2F) and 3 mol of electrons (3F) respectively. 1 F = 96487 C mol–1
Products of Electrolysis
The products of electrolysis depend on the different oxidizing and reducing species present in the electrolytic cell and their standard electrode potentials. some of the electrochemical processes although feasible, are so slow kinetically that at lower voltages these don’t seem to take place and extra potential (called overpotential) has to be applied, which makes such process more difficult to occur.
For example on electrolysis of water at anode
At higher potential we get
Cl– (aq) → ½ Cl2 (g) + e– E(cell) V= 1.36 V
At low potential
2H2O(l )→ O2(g) + 4H+(aq) + 4e– E(cell)V = +1.23 V,
