1 Answer
The electrochemical equivalent refers to the amount of a substance (usually a metal) that gets deposited or dissolved at an electrode during electrolysis when one coulomb of charge passes through the electrolyte. It’s essentially a measure of how much material is involved in the chemical reaction at the electrodes for a given amount of electric charge.
In simpler terms:
For example, if you pass a certain amount of electricity through a copper sulfate solution, the electrochemical equivalent will tell you how much copper will be deposited on the cathode for that amount of electricity.
The formula for it is:
\[
Z = \frac{M}{nF}
\]
Where:
It’s useful in electrolysis and electroplating processes! Does that clear it up?
In simpler terms:
- It tells you how much of a substance will be deposited or removed when a certain amount of electric current flows through a solution.
- It is specific to the substance involved, because different substances have different electrochemical properties.
For example, if you pass a certain amount of electricity through a copper sulfate solution, the electrochemical equivalent will tell you how much copper will be deposited on the cathode for that amount of electricity.
The formula for it is:
\[
Z = \frac{M}{nF}
\]
Where:
- \(Z\) = electrochemical equivalent (in grams per coulomb)
- \(M\) = molar mass of the substance
- \(n\) = number of electrons involved in the reaction
- \(F\) = Faraday constant (about 96,500 C/mol)
It’s useful in electrolysis and electroplating processes! Does that clear it up?