Question

The quantity of silver deposited when one coulomb charge is passed through$AgNO_3$solution:

• A. 0.1 g atom of silver
• B. 1 chemical equivalent of silver
• C. 1 g of silver
• D. 1 electrochemical equivalent of silver

Answer 1

Answer: (D)

1 electrochemical equivalent of silver

Answer 2

The amount of a substance deposited during electrolysis is determined using Faraday’s laws of electrolysis. The formula is:
$W = ZIt,$
where:
- $W$ is the mass of the substance deposited,
- $Z$ is the electrochemical equivalent of the substance,
- $I$ is the current passed, and
- $t$ is the time for which the current is passed.
Step 1: Relating charge to electrochemical equivalent
We know that:
$Q = It,$
where $Q$ is the total charge passed through the solution. Substituting this into the equation for $W$, we get:
$W = ZQ$
Step 2: Deposition of silver
For one coulomb of charge ($Q = 1 \, \text{C}$), the mass of silver deposited is directly proportional to the electrochemical equivalent ($Z$) of silver. Thus:
$W = ZQ = (\text{electrochemical equivalent of silver}).$
Step 3: Conclusion
The quantity of silver deposited when one coulomb of charge is passed is equal to the electrochemical equivalent of silver. This matches the given option.
Final Answer: (4).