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

The Correct Option is D

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).