If 965 coulombs of electricity is passed through a metal cup dipped in silver(I) salt solution, in order to plate it with silver. Then the amount of silver deposited on its surface is (Given: the molar mass of Ag = 108 g mol - 1 , 1 F = 96500 coulombs)

Step-by-step solution

The chemical equation for deposition of silver from the salt solution is Ag + ( aq ) + e - → Ag ( s ) Clearly, for deposition of one mole of silver one-mole electrons are required. Charge on one mole of the electron is equal to one Faraday or 96500 Coulombs. The mass of one mole of silver is equal to its molar mass, i.e., 108   g . Thus, we can say that 96500 coulomb charge can deposit 108   g of silver. Therefore, 965 coulomb will deposit 108 96500 × 965 = 1 . 08   g of silver.