Application of Faraday's Laws-2

Two cells containing $\mathrm{Ni}(\mathrm{NO}{\phantom{A}}_3){\phantom{A}}_2$‍ and $\mathrm{AgNO}{\phantom{A}}_3$‍ electrolytic solutions respectively, are connected in series.

A steady current is passed through these cells until $11.72\mathrm{g}$‍ of $\mathrm{Ni}$‍ is deposited.

Calculate the amount of $\mathrm{Ag}$‍ obtained. Given: Molar mass of $\mathrm{Ni}$‍ is $58.6\text{g/mol}$‍
Molar mass of $\mathrm{Ag}$‍ is $108\text{g/mol}$‍.

$\mathrm{g}$‍.