Products of electrolysis depend on the nature of material being electrlysed and the type of electrodes being used. If the electrode is inert (e.g., platinum or gold), it does not participate in the chemical reaction and acts only as source or sink for electrons. On the other hand, if the electrode is reactive, it participates in the electrode reaction. thus, the products of electrolysis may be different for reactive and inert electrodes.
Aqueous copper sulphate solution and aqueous silver nitrate solution are electrolysed by 1 ampere current for 10 minutes in separate electrolytic cells.
In these question, a statement of assertion followed by a statement of reason. choose the correct answer out of the following choices.
Q. Assertion (A): The mass of copper and silver, deposited on the cathode be same.
Reason (R): Copper and silver have different equivalent masses.

Options

A. Assertion and Reason both are correct statements and reason is correct explanation for assertion.
B. Assertion and reason both are correct statements but reason is not correct explanation for assertion.
C. Assertion is correct statement butreason is wrong statement.
D. Assertion is wrong statement but reason is correct statement.

Explanation

To solve the question regarding the assertion and reason about the electrolysis of aqueous copper sulfate and silver nitrate solutions, we will analyze both statements step by step.

### Step-by-Step Solution:

1. **Understand the Assertion (A)**:
- The assertion states that "The mass of copper and silver deposited on the cathode be the same."
- To evaluate this, we need to consider the electrolysis process and how mass is deposited at the cathode.

2. **Understand the Reason (R)**:
- The reason states that "Copper and silver have different equivalent masses."
- This is a factual statement. The equivalent mass of a substance is calculated as its molar mass divided by its valency.
- For copper (Cu), the molar mass is approximately 63.5 g/mol and its valency (n-factor) is 2, giving an equivalent mass of 31.75 g/equiv.
- For silver (Ag), the molar mass is approximately 108 g/mol and its valency is 1, giving an equivalent mass of 108 g/equiv.

3. **Calculate the Mass Deposited**:
- According to Faraday's laws of electrolysis, the mass (W) of a substance deposited at an electrode is given by the formula:
\[ W = \frac{Q \cdot E}{F} \]
where \( Q \) is the total charge (in coulombs), \( E \) is the equivalent mass, and \( F \) is Faraday's constant (approximately 96500 C/equiv).
- Given that the current (I) is 1 ampere and time (t) is 10 minutes (600 seconds), the total charge \( Q \) can be calculated as:
\[ Q = I \cdot t = 1 \, \text{A} \cdot 600 \, \text{s} = 600 \, \text{C} \]

4. **Mass of Copper Deposited**:
- For copper:
\[ W_{\text{Cu}} = \frac{600 \cdot 31.75}{96500} \approx 0.197 \, \text{g} \]

5. **Mass of Silver Deposited**:
- For silver:
\[ W_{\text{Ag}} = \frac{600 \cdot 108}{96500} \approx 0.673 \, \text{g} \]

6. **Comparison of Masses**:
- From the calculations, the mass of copper deposited is approximately 0.197 g, while the mass of silver deposited is approximately 0.673 g.
- Therefore, the assertion that the masses of copper and silver deposited on the cathode are the same is **false**.

7. **Conclusion**:
- The assertion (A) is false because the masses of copper and silver deposited are not the same.
- The reason (R) is true as copper and silver have different equivalent masses.
- Thus, the correct answer is that the assertion is false, and the reason is true.

### Final Answer:
- The assertion is false, and the reason is true.