The quantity of silver deposited when one coulomb charge is passed through\(AgNO_3\)solution:
- 0.1 g atom of silver
- 1 chemical equivalent of silver
- 1 g of silver
- 1 electrochemical equivalent of silver
The Correct Option is D
Approach Solution - 1
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).
Approach Solution -2
The mass of a substance deposited or liberated during electrolysis is directly proportional to the quantity of electricity (charge) passed through the solution.
According to Faraday’s first law of electrolysis:
\[ m = ZQ \] where:
m = mass of the substance deposited (in grams)
Z = electrochemical equivalent (in g/C)
Q = total charge passed (in coulombs)
Step 2: Given data.
Charge passed, Q = 1 coulomb
Step 3: Substitute in the formula.
\[ m = Z \times Q = Z \times 1 = Z \]
Therefore, the mass of silver deposited = 1 electrochemical equivalent of silver.
Step 4: Final Answer.
The quantity of silver deposited is:
\[ \boxed{1 \, \text{electrochemical equivalent of silver}} \]
Final Answer: 1 electrochemical equivalent of silver
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