Michael Faraday was the first scientist who described the quantitative aspects of electrolysis. Now Faraday’s laws also flow from what has been discussed earlier. Faraday’s Laws of Electrolysis After his extensive investigations on electrolysis of solutions and melts of electrolytes, Faraday published his results during 1833-34 in the form of the following well known Faraday’s two laws of electrolysis:

(i) 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).

(ii) 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).

What is the charge on 1 mole of electrons?

96500 C

The correct answer is option 3.96500 C.

The charge on one electron is a fundamental constant in physics and is denoted by \( e \).

\( e = 1.6021 \times 10^{-19} \, \text{coulombs (C)} \)

Avogadro's number (\( N_A \)) is the number of particles (atoms, molecules, or ions) in one mole of substance. It is approximately \( 6.02 \times 10^{23} \) particles/mol.

Charge on one mole of electrons (Faraday's constant, \( F \)):

Faraday's constant \( F \) represents the total charge carried by \( N_A \) electrons. This can be calculated by multiplying the charge of one electron by Avogadro's number.

\(F = N_A \times e\)

Substitute the values:

\(F = 6.02 \times 10^{23} \times 1.6021 \times 10^{-19} \, \text{C} \)

\(F = 9.65 \times 10^{4} \, \text{C}\)

Faraday's constant is commonly approximated as \( 96485 \) C/mol. This value is very close to \( 96500 \) C/mol, which is often used in practical calculations.

Therefore, the charge on one mole of electrons, known as Faraday's constant (\( F \)), is approximately \( 96500 \) C. This quantity is fundamental in electrochemistry and electrolysis calculations, where it relates the amount of substance undergoing oxidation or reduction to the amount of electric charge transferred.