An electric current is passed through a silver voltameter connected to a water voltameter. The cathode of the silver voltameter weighed $0.108 \ g$ more at the end of the electrolysis. The volume of oxygen evolved at $STP$ is ............... $cm^{3}$.

In an industrial process,$40 \ kg$ of calcium is produced by electrolysis in $2 \ hours$. How much $kg$ of aluminum would be produced if the same current is passed for the same duration? (Atomic mass of $Ca = 40, Al = 27$)

When $1 \ C$ of electricity is passed through an electrolytic solution,the mass deposited on the electrode is equal to which of the following?

If in a voltaic cell $5 \ g$ of zinc is consumed,then how many ampere-hours are produced? (Given that the $E.C.E.$ of $Zn$ is $3.387 \times 10^{-7} \ kg/C$)

$4.5 \ g$ of aluminium (atomic mass $27 \ amu$) is deposited at the cathode from an $Al^{3+}$ solution by a certain quantity of electric charge. The volume of hydrogen produced at $STP$ from $H^{+}$ ions in the solution by the same quantity of electric charge will be .............. $L$.

$7.5 \ A$ current is passed for $200 \ s$ through $AgNO_3$ solution. If experimentally $1.08 \ g$ of $Ag$ is obtained,then calculate the current efficiency (cell capacity). $[Ag = 108 \ u]$