1. What is Moles of Electron Transferred?

Definition: The moles of electrons transferred (n) is the amount of electrons taking part in the cell reaction.

Purpose: This calculation is essential in electrochemistry for determining the stoichiometry of redox reactions and calculating cell potentials.

2. How Does the Calculator Work?

The calculator uses the formula:

Where:

• \( n \) — Moles of electron transferred (dimensionless)
• \( \Delta G° \) — Standard Gibbs Free Energy (Joules)
• \( F \) — Faraday constant (96485.33212 C/mol)
• \( E°_{cell} \) — Standard cell potential (Volts)

Explanation: The negative of the standard Gibbs free energy change is divided by the product of the Faraday constant and the standard cell potential.

3. Importance of This Calculation

Details: Knowing the moles of electrons transferred is crucial for understanding electrochemical reactions, designing batteries, and predicting reaction spontaneity.

4. Using the Calculator

Tips: Enter the standard Gibbs free energy in Joules and the standard cell potential in Volts. The standard cell potential must be non-zero.

5. Frequently Asked Questions (FAQ)

Q1: What is the Faraday constant?
A: The Faraday constant represents the electric charge carried by one mole of electrons (approximately 96485 C/mol).

Q2: Why is the Gibbs free energy negative in the formula?
A: The negative sign accounts for the fact that a spontaneous reaction has negative ΔG°.

Q3: What units should I use for Gibbs free energy?
A: The calculator expects Gibbs free energy in Joules (J). If you have kJ, multiply by 1000 before entering.

Q4: Can the cell potential be negative?
A: Yes, but it cannot be zero as that would make the denominator zero.

Q5: How precise is this calculation?
A: Very precise, as it uses the exact value of the Faraday constant to 8 decimal places.