What is the time (in seconds) required for depositing all the silver present in 125ml of 1M ${\text{AgNO}}_{\text{3}}$ solution by passing a current of 241.25 amperes ?

number of moles =

$\frac{\text{M}\times {\text{V}}_{\text{ml}}}{\text{1000}}=\frac{\text{1}\times \text{125}}{\text{1000}}=\text{0}\text{.125}\text{moles}$

${\text{Ag}}^{+}+{\text{e}}^{-}\underset{}{\overset{}{\to }}\text{Ag}$

1 F $\underset{}{\overset{}{\leftarrow }}$ 1 mole of Ag

    ?  $\underset{}{\overset{}{\leftarrow }}$ 0.125 moles of Ag

$\text{Q}=0.125\text{F}=0.125\times 96500$

$\text{c}\times \text{t}=0.125\times 96500$

$241.25\times \text{t}=0.125\times 96500$,  t = 50 seconds