The value of Faraday’s constant (F) is:

F=96485 C/molF = 96485 \text{ C/mol}

What is Faraday’s Constant?

Faraday’s constant represents the electric charge carried by one mole of electrons. It is the product of:

F=NA×eF = N_A \times e

Where:

• NA=6.022×1023N_A = 6.022 \times 10^{23} (Avogadro’s number) – number of particles per mole
• e=1.602×10−19e = 1.602 \times 10^{-19} Coulombs – charge of one electron

Multiplying these values:

F=(6.022×1023)×(1.602×10−19)F = (6.022 \times 10^{23}) \times (1.602 \times 10^{-19}) F≈96485 C/molF \approx 96485 \text{ C/mol}

Common Approximations:

• 96485 C/mol (exact value)
• 96500 C/mol (rounded for quick calculations)

Where is Faraday’s Constant Used?

1. Electrolysis Calculations
   • Used in Faraday’s laws of electrolysis to determine the amount of substance deposited or dissolved during electrolysis.

   m=QF×Mnm = \frac{Q}{F} \times \frac{M}{n}Where:

   • mm = Mass deposited (g)
   • QQ = Charge passed (Coulombs)
   • FF = 96485 C/mol
   • MM = Molar mass of substance
   • nn = Number of electrons transferred
2. Nernst Equation
   • Helps in calculating electrode potential under non-standard conditions:

   E=E∘−RTnFln⁡QE = E^\circ – \frac{RT}{nF} \ln Q

3. Gibbs Free Energy and Electrochemical Cells
   • Relates Gibbs free energy (ΔG\Delta G) to cell potential (EE):

   ΔG=−nFE\Delta G = -nFE

   • Determines the spontaneity of a redox reaction.

Key Takeaways

• Faraday’s constant = 96485 C/mol.
• Represents charge carried by one mole of electrons.
• Used in electrolysis, Nernst equation, and Gibbs free energy calculations.

Let me know if you need further clarification!