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(C) According to Faraday's law of electrolysis,the mass of a substance deposited is given by $m = \frac{M 	imes Q}{n 	imes F}$,where $M$ is the mola

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$AgNO_3$

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(C) According to Faraday's law of electrolysis,the mass of a substance deposited is given by $m = \frac{M 	imes Q}{n 	imes F}$,where $M$ is the molar mass,$n$ is the valency factor,and $Q$ is the charge passed.Since $Q$ is constant,the mass deposited is proportional to the equivalent mass,which is $\frac{M}{n}$.For $Zn^{2+}$ $(ZnSO_4)$: Equivalent mass = $\frac{65.4}{2} = 32.7 \ g$.For $Fe^{3+}$ $(FeCl_3)$: Equivalent mass = $\frac{56}{3} \approx 18.67 \ g$.For $Ag^+$ $(AgNO_3)$: Equivalent mass = $\frac{108}{1} = 108 \ g$.For $Ni^{2+}$ $(NiCl_2)$: Equivalent mass = $\frac{58.7}{2} = 29.35 \ g$.Comparing the equivalent masses,$Ag$ has the highest value $(108 \ g)$.Therefore,$Ag$ will be deposited in the maximum amount.

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?

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