1 Answer
The electrochemical equivalent of a substance refers to the amount of that substance (usually in grams) that is deposited or liberated at an electrode during the process of electrolysis when a current of one ampere flows for one second. It is a measure of how much of a substance is chemically changed when a specific amount of electric charge passes through the electrolyte.
In simple terms, it tells you how much of a substance you can get from an electrode for a given amount of electric current over time.
Formula:
The electrochemical equivalent \( z \) can be calculated using the formula:
\[
z = \frac{M}{n \cdot F}
\]
Where:
Example:
For the electrolysis of water, hydrogen (H₂) and oxygen (O₂) are produced. The electrochemical equivalent of hydrogen would tell you how much hydrogen gas is liberated for a given current.
In short, it connects the physical change of a substance with the amount of electrical energy supplied in the form of current.
In simple terms, it tells you how much of a substance you can get from an electrode for a given amount of electric current over time.
Formula:
The electrochemical equivalent \( z \) can be calculated using the formula:\[
z = \frac{M}{n \cdot F}
\]
Where:
- \( M \) is the molar mass of the substance (in grams per mole).
- \( n \) is the valency (the number of electrons required to deposit or dissolve one mole of the substance).
- \( F \) is Faraday’s constant (approximately 96,485 C/mol), which represents the charge on one mole of electrons.
Example:
For the electrolysis of water, hydrogen (H₂) and oxygen (O₂) are produced. The electrochemical equivalent of hydrogen would tell you how much hydrogen gas is liberated for a given current.In short, it connects the physical change of a substance with the amount of electrical energy supplied in the form of current.