According to Faraday's laws of electrolysis, the discharge of one electrochemical equivalent of ions should involve

Options

A. 1 mole of electrons
B. 96500 moles of electrons
C. `1/(96500)` mole of electrons
D. none of these

Answer

To solve the question regarding Faraday's laws of electrolysis and the discharge of one electrochemical equivalent of ions, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding Faraday's Laws of Electrolysis**:
- Faraday's first law states that the amount of substance discharged at an electrode during electrolysis is directly proportional to the quantity of electricity passed through the electrolyte.
- The second law states that the amount of different substances discharged by the same quantity of electricity is proportional to their equivalent weights.

2. **Electrochemical Equivalent**:
- The electrochemical equivalent (E) of an ion is defined as the mass of the substance that is deposited or liberated at an electrode when one coulomb of electric charge is passed through the electrolyte.
- Mathematically, it can be expressed as:
\[ E = \frac{m}{Q} \]
where \( m \) is the mass of the substance and \( Q \) is the total electric charge in coulombs.

3. **Discharge of One Electrochemical Equivalent**:
- According to Faraday's first law, to discharge one electrochemical equivalent of ions, a specific amount of charge must be passed through the electrolyte.
- The charge required to discharge one electrochemical equivalent of ions can be calculated using Faraday's constant (F), which is approximately 96500 coulombs per mole of electrons.
- The relationship can be expressed as:
\[ Q = n \cdot F \]
where \( n \) is the number of moles of electrons required to discharge one equivalent of the ion.

4. **Conclusion**:
- Therefore, to discharge one electrochemical equivalent of ions, a quantity of electricity equal to one Faraday (96500 coulombs) must be passed through the electrolyte.

### Final Answer:
According to Faraday's laws of electrolysis, the discharge of one electrochemical equivalent of ions should involve passing one Faraday (96500 coulombs) of electric charge.