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Answer in General Chemistry for Tuti #152806

Author:
March 17th, 2023

Calculate the time required to deposit 0.37g of Silver from a silver Nitrate solution using a current of 2.5A ( Charge of Ag in is AgNO 3 is +1)

If Farade constant = 96485 Cmol-1

Atomic mass of Ag = 107.5 gmol-1

  • Deposition occurs as,

Ag+(aq) + e ——> Ag(s) —- (1)

  • No of Ag moles deposited ( nAg ) = “dfrac{0.37g}{107.5gmol^{-1}}”

= “3.44times10^{-3} mol”

  • As per the equation (1),

“n_e = n_{Ag}\”

  • Using,

“Q =It,\3.44times10^{-3}mol;times ;96485; Cmol^{-1};=;2.5A;times;t\nt;=;bf132.76s”

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