Moles of Electron Transferred given Change in Gibbs Free Energy Calculator

Formula:

\[ n = \frac{-\Delta G}{F \times E_{cell}} \]

Moles of Electron Transferred (n):

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1. What is Moles of Electron Transferred?

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

Purpose: This calculation helps in understanding electrochemical reactions and determining the stoichiometry of redox reactions.

2. How Does the Calculator Work?

The calculator uses the formula:

\[ n = \frac{-\Delta G}{F \times E_{cell}} \]

Where:

\( n \) — Moles of electron transferred
\( \Delta G \) — Gibbs Free Energy (J)
\( F \) — Faraday constant (96485.33212 C/mol)
\( E_{cell} \) — Cell Potential (V)

Explanation: The negative Gibbs free energy divided by the product of Faraday constant and cell potential gives the moles of electrons transferred.

3. Importance of This Calculation

Details: Knowing the moles of electrons transferred is crucial for understanding electrochemical cell performance, battery design, and corrosion studies.

4. Using the Calculator

Tips: Enter the Gibbs Free Energy in joules and the cell potential in volts. The Faraday constant is fixed at 96485.33212 C/mol.

5. Frequently Asked Questions (FAQ)

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

Q2: Can the cell potential be zero?
A: No, the cell potential must be non-zero to avoid division by zero in the calculation.

Q3: What units should I use for Gibbs Free Energy?
A: The calculator expects Gibbs Free Energy in joules (J).

Q4: How precise is this calculation?
A: The calculation is precise to 8 decimal places for moles of electrons.

Q5: What does a negative value for n mean?
A: The negative sign indicates the direction of electron flow in the redox reaction.