If the total electricity required to deposit $1$ mole of a metal $M$ is equal to that of $10.7$ amperes of current for $10$ hours,the equivalent weight of the metal is (atomic weight $= M \ u$):

$6.5 \, g$ of $Mg$ is deposited during the electrolysis of fused $MgCl_2$. What will be the volume of chlorine gas (in $L$) discharged at the electrode at $STP$?

$A$ current of strength $2.5 \ A$ was passed through $CuSO_4$ solution for $6 \ \text{minutes} \ 26 \ \text{seconds}$. The amount of copper deposited is .............. $g$ (Atomic weight of $Cu = 63.5$) $(1 \ F = 96500 \ C)$

What amount of electricity can deposit $1 \ mole$ of $Al$ metal at cathode when passed through molten $AlCl_3$?

By passing electric current,$NaClO_{3}$ is converted into $NaClO_{4}$ according to the following equation:
$NaClO_{3} + H_{2}O \rightarrow NaClO_{4} + H_{2}$
How many moles of $NaClO_{4}$ will be formed when $3 \ F$ of charge is passed through $NaClO_{3}$?

During the electrolysis of a solution of $AgNO_3$,$9650 \ C$ of charge passes through the electroplating bath. The mass of silver deposited at the cathode will be .............. $g$.