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

We need to determine what quantity of silver is deposited when 1 coulomb of charge is passed through $$AgNO_3$$ solution. According to Faraday’s First Law of Electrolysis, the mass of a substance deposited at an electrode is directly proportional to the quantity of charge passed.

The mass deposited (m) is related to the charge (Q) by

where $$Z$$ is the electrochemical equivalent and $$Q$$ is the charge in coulombs. The electrochemical equivalent $$Z$$ is defined as the mass of a substance deposited when 1 coulomb of charge is passed through the solution.

Substituting $$Q = 1$$ coulomb gives

Therefore, the quantity of silver deposited is one electrochemical equivalent of silver.

The electrochemical equivalent of silver is

which shows that it is neither 1 g nor 0.1 g‐atom of silver. The chemical equivalent of silver would be deposited by one faraday (96500 C) of charge, not one coulomb.

Hence, the correct answer is Option (2): 1 electrochemical equivalent of silver.