ECE = (Molar Mass of the Substance) / (Faraday's Constant * Number of Electrons Transferred)
Where:
* ECE: Electrochemical equivalent (in grams per coulomb, g/C)
* Molar Mass: The molar mass of the substance (in grams per mole, g/mol)
* Faraday's Constant: The charge of one mole of electrons (approximately 96,485 coulombs per mole, C/mol)
* Number of Electrons Transferred: The number of electrons involved in the half-reaction of the substance during electrolysis.
Example:
Let's calculate the ECE of copper (Cu).
* Molar Mass of Cu: 63.55 g/mol
* Faraday's Constant: 96,485 C/mol
* Number of Electrons Transferred: 2 (Cu²⁺ + 2e⁻ → Cu)
ECE of Cu = (63.55 g/mol) / (96,485 C/mol * 2) = 0.000329 g/C
Therefore, the electrochemical equivalent of copper is 0.000329 grams per coulomb.
Important Notes:
* The number of electrons transferred in the half-reaction is crucial for determining the ECE.
* The electrochemical equivalent is a fundamental constant for a given substance and is independent of the current, time, or other factors.
* ECE can be used to calculate the amount of substance deposited or liberated during electrolysis.
