When the same quantity of electricity is passed through the aqueous solutions of the given electrolytes for the same amount of time, which metal will be deposited in maximum amount on the cathode?

By Faraday's law of electrolysis:

Equal amount of charge causes deposition of equal number of equivalents of different metals. eg. $1\mathrm{F}$ charge  will deposit one equivalent of any metal.

Discharged mass of one equivalent of $\mathrm{Zn} \mathrm{from} {\mathrm{ZnCl}}_2= \frac{65.4}{2}=32.7 \mathrm{g}$

Discharged mass of one equivalent of $\mathrm{Fe} \mathrm{from} {\mathrm{FeCl}}_3=\frac{56}{3}=18.67 \mathrm{g}$

Discharged mass of one equivalent of $\mathrm{Ag} \mathrm{from} {\mathrm{AgNO}}_3=\frac{108}{1}=108 \mathrm{g}$

Discharged mass of one equivalent of $\mathrm{Ni} \mathrm{from} {\mathrm{NiCl}}_2=\frac{58.7}{2}=29.35 \mathrm{g}$ 

So, Silver metal will be deposited in maximum amount on the cathode.