Assertion : In electrolysis, the quantity of electricity needed for depositing 1 mole silver is different from that required for 1 mole of copper.
Reason : The molecular weights of silver and copper are different.

Options

A. If both assertion and reason are true and reason is the correct explanation of assertion .
B. If both assertion and reason are true but reason is not the correct explanation of assertion .
C. If assertion is true but reason is false .
D. If both assertion and reason are false .

Explanation

To solve the assertion and reason question regarding electrolysis and the quantities of electricity needed for depositing silver and copper, we can follow these steps:

### Step 1: Understand the Assertion
The assertion states that in electrolysis, the quantity of electricity needed for depositing 1 mole of silver is different from that required for 1 mole of copper.

### Step 2: Understand the Reason
The reason provided is that the molecular weights of silver (Ag) and copper (Cu) are different.

### Step 3: Apply Faraday's Second Law of Electrolysis
Faraday's second law states that the amount of substance deposited at an electrode is directly proportional to the quantity of electricity passed and inversely proportional to the equivalent weight of the substance.

### Step 4: Calculate the Equivalent Weights
The equivalent weight (EW) can be calculated using the formula:
\[ \text{Equivalent Weight} = \frac{\text{Molecular Weight}}{n} \]
where \( n \) is the number of electrons transferred in the reaction.

- For silver (Ag):
- Molecular Weight of Ag = 108 g/mol
- \( n \) factor of Ag = 1 (since Ag+ gains 1 electron)
- Equivalent Weight of Ag = \( \frac{108}{1} = 108 \) g/equiv

- For copper (Cu):
- Molecular Weight of Cu = 63.5 g/mol
- \( n \) factor of Cu = 2 (since Cu2+ gains 2 electrons)
- Equivalent Weight of Cu = \( \frac{63.5}{2} = 31.75 \) g/equiv

### Step 5: Compare the Equivalent Weights
Since the equivalent weight of silver (108 g/equiv) is different from that of copper (31.75 g/equiv), it indicates that the quantity of electricity required to deposit 1 mole of each metal will also be different.

### Step 6: Conclusion
Both the assertion and the reason are correct. The assertion is true because the quantity of electricity needed for depositing 1 mole of silver is indeed different from that required for 1 mole of copper due to their differing equivalent weights, which arise from their differing molecular weights.

### Final Answer
Both the assertion and the reason are correct, and the reason is a correct explanation of the assertion.

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