According to Faraday's second law of electrolysis

Options

A. `M_1/M_2 = E_1/E_2 `
B. `m = Z xx C xx t`
C. `Z = (m)/(C xx t)`
D. `E_1/E_2 = Z_2/Z_1`

Explanation

### Step-by-Step Solution:

1. **Understanding Faraday's Second Law of Electrolysis**:
Faraday's second law states that the mass of different ions liberated at the electrodes when the same amount of electricity is passed through different electrolytes is directly proportional to their chemical equivalents.

2. **Mathematical Representation**:
The law can be expressed mathematically as:
\[ \frac{m_1}{m_2} = \frac{E_1}{E_2} \]
where \( m_1 \) and \( m_2 \) are the masses of the substances deposited at the electrodes, and \( E_1 \) and \( E_2 \) are their chemical equivalents.

3. **Relating Mass to Charge**:
The mass of a substance deposited during electrolysis can also be expressed using the formula:
\[ m = zct \]
where \( z \) is the electrochemical equivalent, \( c \) is the current, and \( t \) is the time.

4. **Understanding Electrochemical Equivalent**:
The electrochemical equivalent \( z \) can be defined as:
\[ z = \frac{m}{ct} \]
This shows how the mass is related to the charge passed through the electrolyte.

5. **Comparing Two Electrolytes**:
By comparing two different electrolytes, we can derive that:
\[ \frac{E_1}{E_2} = \frac{z_2}{z_1} \]
This means that the ratio of their chemical equivalents is equal to the ratio of their electrochemical equivalents.

6. **Conclusion**:
Therefore, the correct interpretation of Faraday's second law of electrolysis is:
\[ \frac{m_1}{m_2} = \frac{E_1}{E_2} \]
This confirms that the mass of ions liberated is directly proportional to their chemical equivalents when the same amount of electricity is passed through different electrolytes.