What is the quantity of electricity (in Coulombs) required to deposit all the silver from $250 \text{ mL}$ of $1 \text{ M AgNO}_3$ solution?

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?

The atomic weights of silver and copper are $108$ and $64$ respectively. $A$ silver voltameter and a copper voltameter are connected in series,and when current is passed,$10.8 \ g$ of silver is deposited. The mass of copper deposited will be ............. $g$.

The unit of electrochemical equivalent is

Calculate the current in ampere required to deposit $4.8 \ g$ of $Cu$ from its salt solution in $30 \ minutes$. $\left[ \text{Molar mass of } Cu = 63.5 \ g \ mol^{-1} \right]$ (in $A$)

The amount of charge required to liberate $11.5 \ g$ of sodium is .....