By virtue of Faraday's second law of electrolysis, the electrochemical equivalent of the two metals liberated at the electrodes has the same ratio as that of their

Options

A. Atomic masses
B. Molecular masses
C. Equivalent masses
D. Any of three

Explanation

To solve the question regarding Faraday's second law of electrolysis and the relationship between the electrochemical equivalents of two metals, we can follow these steps:

### Step-by-Step Solution:

1. **Understand Faraday's Second Law of Electrolysis**:
Faraday's second law states that the mass of a substance deposited or liberated at an electrode during electrolysis is directly proportional to the quantity of electricity passed through the electrolyte and is also directly proportional to the equivalent mass of the substance.

2. **Define Electrochemical Equivalent**:
The electrochemical equivalent (E) of a substance is defined as the mass of the substance deposited or liberated by the passage of one coulomb of electric charge. According to Faraday's second law, the electrochemical equivalent is related to the equivalent mass of the substance.

3. **Set Up the Relationship**:
If we have two metals (let's call them Metal 1 and Metal 2) and their respective electrochemical equivalents are E1 and E2, the masses deposited (W1 and W2) when the same amount of electricity (Q) is passed can be expressed as:
\[ W1 \propto E1 \quad \text{and} \quad W2 \propto E2 \]

4. **Express the Ratio**:
Since the mass deposited is proportional to the electrochemical equivalent, we can write:
\[ \frac{W1}{W2} = \frac{E1}{E2} \]

5. **Relate to Equivalent Masses**:
The equivalent mass (E) of a substance is defined as the molar mass (M) divided by the number of electrons (n) transferred in the reaction:
\[ E = \frac{M}{n} \]
Therefore, the ratio of the electrochemical equivalents of the two metals is equivalent to the ratio of their equivalent masses.

6. **Conclusion**:
Thus, according to Faraday's second law, the electrochemical equivalents of the two metals liberated at the electrodes have the same ratio as that of their equivalent masses.

### Final Answer:
The answer is **equivalent masses**.

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