Formula Used:
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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.
The calculator uses the formula:
Where:
Explanation: The negative of the standard Gibbs free energy change is divided by the product of the Faraday constant and the standard cell potential.
Details: Knowing the moles of electrons transferred is crucial for understanding electrochemical reactions, designing batteries, and predicting reaction spontaneity.
Tips: Enter the standard Gibbs free energy in Joules and the standard cell potential in Volts. The standard cell potential must be non-zero.
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.