Moles of Electron Formula:
From: | To: |
Definition: This calculator determines the number of moles of electrons transferred in an electrochemical reaction based on the charge passed and moles of analyte.
Purpose: It's essential for electrochemistry calculations, helping to understand electron transfer in redox reactions and electrolysis processes.
The calculator uses the formula:
Where:
Explanation: The charge is divided by the product of moles of analyte and Faraday's constant to determine the moles of electrons transferred.
Details: Calculating moles of electrons is crucial for understanding stoichiometry in electrochemical reactions, determining reaction yields, and designing electrochemical cells.
Tips: Enter the charge in Coulombs and moles of analyte. Both values must be positive numbers. The result shows moles of electrons transferred.
Q1: What is Faraday's constant?
A: Faraday's constant (96485.33212 C/mol) represents the charge of one mole of electrons, fundamental in electrochemistry.
Q2: How do I determine the charge passed?
A: Charge (Q) can be calculated as current (I) multiplied by time (t) in seconds (Q = I × t).
Q3: What's the relationship between moles of electrons and moles of analyte?
A: The ratio depends on the stoichiometry of the half-reaction (n in the Nernst equation).
Q4: Can this calculator be used for electrolysis calculations?
A: Yes, it's applicable to both galvanic cells and electrolysis processes.
Q5: Why is the result often very small?
A: Because Faraday's constant is large, the number of moles of electrons is typically small for practical amounts of charge.