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Definition: This calculator determines the amount of electrons (in moles) taking part in an electrochemical cell reaction based on the work done and cell potential.
Purpose: It helps chemists and electrochemists understand the stoichiometry of electron transfer in redox reactions.
The calculator uses the formula:
Where:
Explanation: The work done is divided by the product of Faraday constant and cell potential to determine the moles of electrons transferred.
Details: Calculating moles of electrons transferred is crucial for understanding reaction stoichiometry, battery performance, and electrolysis processes.
Tips: Enter the work done in joules and the cell potential in volts. Both values must be positive numbers.
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: How is work related to electron transfer?
A: The work done in an electrochemical cell is directly proportional to the number of electrons transferred.
Q3: What units should I use for inputs?
A: Work should be in joules (J) and cell potential in volts (V).
Q4: Can this be used for battery calculations?
A: Yes, this calculation is fundamental for understanding battery capacity and performance.
Q5: Why might my result be very small?
A: Since we're dealing with individual electrons, the number of moles is typically very small (often in the range of 10^-6 to 10^-3).