Formula:
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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.
The calculator uses the formula:
Where:
Explanation: The negative Gibbs free energy divided by the product of Faraday constant and cell potential gives the moles of electrons transferred.
Details: Knowing the moles of electrons transferred is crucial for understanding electrochemical cell performance, battery design, and corrosion studies.
Tips: Enter the Gibbs Free Energy in joules and the cell potential in volts. The Faraday constant is fixed at 96485.33212 C/mol.
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.