13.2 Farady's Second Law

2.1 Difference between metallic conduction and electrolytic conduction

3.1 Difference Between Electrolytic Cell and Galvanic Cell

5.1 Salt Bridge

9.1 Characteristics of electrochemical series
9.2 Applications of electrochemical series

10.1 Reducing power of Metals
10.2 Oxidising Nature of Non-metals

13.1 Faraday's first law
13.2 Farady's Second Law

15.1 Condition of Equilibrium
15.2 Spontaneity of the Reaction

17.1 Primary Battery or Voltaic Cells (Dry Cells):
17.2 Secondary Cells

When same amount of electricity is passed through different electrolytes, the masses of different ions deposited or liberated at the electrolytes are directly proportional to electrochemical equivalent( or equivalent weights). Suppose ${W_1}$ and ${W_2}$ are weights of elements deposited by passing a certain quantity of electricity through their salt solutions and ${{E_1}}$ and ${{E_2}}$ are their respective weights, then

$$\begin{equation} \begin{aligned} \frac{{{W_1}}}{{{W_2}}} = \frac{{{E_1}}}{{{E_2}}} \\ \frac{{{Z_1}It}}{{{Z_2}It}} = \frac{{{E_1}}}{{{E_2}}}...(W = ZIt) \\ \frac{{{Z_1}}}{{{Z_2}}} = \frac{{{E_1}}}{{{E_2}}} \\\end{aligned} \end{equation} $$

Thus electrochemical equivalent $(Z)$ is directly proportional to its equivalent weights $(E)$

so we can say that $Z$ is directly proportional to the equivalent weight ($E$)

$$\begin{equation} \begin{aligned} E \propto Z \\ E = FZ \\\end{aligned} \end{equation} $$

Here $F$ is proportionality constant which is equal to the $96500C$. It is called Faraday constant. Thus, $$E = 96500 \times Z$$.

So we can say that when $96500C$ of electricity is passed through an electrolyte, one gram equivalent ions gets deposited on it