how long it will take to remove 1/2 silver from 200cm ^₃ of 0.1 molar AgNo₃ solution with current of 1 amphere

Molarity of silver nitrate solution = 0.1 M

Volume of solution =200 cm³​ =0.2 L
No. of moles silver nitrate present = 0.1 moles/L  x 0.2 L  =0.02 moles
 
1 Mole of silver nitrate contains = 1 mole of Ag⁺ ion.
Therefore
0.02 moles of AgNO₃ contains = 0.02 moles of Ag⁺ 

Reaction involved :
$A{g}^{+} + e^{-} \to Ag$
1 mole of Ag⁺ is reduced by = 1 mole of electrons

Since we need to calculate the time for reduction of half silver ion.
Therefore

(0.01) mole of Ag⁺ is reduced by = 0.01 mole of electrons
 
Charge on 1 mole of electrons = 96500 C

Charge produced by 0.01 moles of electrons = 0.01 x 96500 = 965 C

Charge = Current (A) x Time(s)

965 C = 1 A x t
t in seconds = 965 C/ 1 A = 965 seconds
 
Time in minutes  = 965/60 = 16.083 minutes