1. What is Moles of Electron Transferred?

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.

2. How Does the Calculator Work?

The calculator uses the formula:

Where:

• \( n \) — Moles of electrons transferred (mol)
• \( w \) — Work done by/on the system (J)
• \( F \) — Faraday constant (96485.33212 C/mol)
• \( E_{cell} \) — Cell potential (V)

Explanation: The work done is divided by the product of Faraday constant and cell potential to determine the moles of electrons transferred.

3. Importance of Electron Transfer Calculation

Details: Calculating moles of electrons transferred is crucial for understanding reaction stoichiometry, battery performance, and electrolysis processes.

4. Using the Calculator

Tips: Enter the work done in joules and the cell potential in volts. Both values must be positive numbers.

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: 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).