1 Answer
The electrochemical equivalent refers to the amount of a substance (usually in grams) that is deposited or liberated at an electrode during the electrolysis of a solution when one coulomb of electric charge passes through the electrolyte.
In simple terms, it's a measure of how much material gets deposited or removed at the electrodes (anode or cathode) in an electrochemical process for a given amount of electrical charge.
The electrochemical equivalent is different for different substances, and it depends on factors like the substance’s chemical properties and how easily it can gain or lose electrons.
Formula:
It’s generally given by the formula:
\[
z = \frac{M}{F \times n}
\]
Where:
Example:
If you’re electroplating copper, the electrochemical equivalent tells you how much copper will be deposited at the cathode when a certain amount of electric charge passes through the electrolyte.
Does that make sense? Would you like an example calculation or more details?
In simple terms, it's a measure of how much material gets deposited or removed at the electrodes (anode or cathode) in an electrochemical process for a given amount of electrical charge.
The electrochemical equivalent is different for different substances, and it depends on factors like the substance’s chemical properties and how easily it can gain or lose electrons.
Formula:
It’s generally given by the formula:\[
z = \frac{M}{F \times n}
\]
Where:
- \( z \) is the electrochemical equivalent (in grams per coulomb),
- \( M \) is the molar mass of the substance (in grams per mole),
- \( F \) is Faraday's constant (\( 96,485 \, C/mol \)),
- \( n \) is the valency of the substance (the number of electrons involved in the reaction).
Example:
If you’re electroplating copper, the electrochemical equivalent tells you how much copper will be deposited at the cathode when a certain amount of electric charge passes through the electrolyte.Does that make sense? Would you like an example calculation or more details?