Question

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)

Answer 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 ( n_Ag ) = $\dfrac{0.37g}{107.5gmol^{-1}}$

= $3.44\times10^{-3} mol$

• As per the equation (1),

$n_e = n_{Ag}\\$

• Using,

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