How many seconds of current at $241.25 \ A$ must be passed to deposit all the silver present in $125 \ mL$ of $1 \ M \ AgNO_3$ solution? $(1 \ F = 96500 \ C)$

The amount of silver deposited on passing $2 \ F$ of electricity through an aqueous solution of $AgNO_3$ is: (in $g$)

Three voltameters containing aqueous solutions of $H_2SO_4$,$CuSO_4$,and $AgNO_3$ are connected in series as shown. $A$ current was passed for $10 \ hours$. $10.8 \ g$ of $Ag$ was deposited at the cathode in the $(III)$ electrolytic cell during electrolysis. If the current efficiency is $50\%$,what is the magnitude of the current in amperes?

In the electrolysis of an aqueous $Ni(NO_3)_2$ solution using $Ni$ electrodes,upon passing $1$ equivalent of charge,the mass of the cathode $(Ni = 59)$ changes by:

The atomic weight of $Al$ is $27$. When a current of $5$ Faradays is passed through a solution of $Al^{3+}$ ions,the weight of $Al$ deposited is ............ $g$.

$A$ dilute solution of sulphuric acid is electrolysed using a current of $0.10 \ A$ for $2 \ hours$ to produce hydrogen and oxygen gas. The total volume of gases produced at $STP$ is $...... \ cm^3$. (Nearest integer) $[$ Given : Faraday constant $F = 96500 \ C \ mol^{-1}$ at $STP$,molar volume of an ideal gas is $22.7 \ L \ mol^{-1} ]$