$A$ current of $0.5 \ A$ is passed through molten $AlCl_3$ for $96.5 \ s$. The mass of aluminium deposited at cathode is $x \ mg$ and volume of chlorine liberated (at $STP$) at anode is $y \ mL$. $x$ and $y$ are respectively

The number of moles of electrons passed when a current of $2 \ A$ is passed through a solution of electrolyte for $20 \ minutes$ is

The quantity of electricity (in $C$) required to oxidize $1 \ mol$ of $H_2O$ to $O_2$ is approximately ..................... $\times 10^5 \ C$.

In a certain electrolysis experiment,$0.650 \ g$ of zinc is deposited in a cell having $ZnSO_4$ solution. Calculate the mass of $Cu$ deposited in another cell having $CuSO_4$ solution arranged in series with the first cell (in $g$)? (Molar mass of $Zn = 65 \ g \ mol^{-1}$,$Cu = 63.5 \ g \ mol^{-1}$)

When a copper voltameter is connected with a battery of $e.m.f.$ $12 \ V$,$2 \ g$ of copper is deposited in $30 \ minutes$. If the same voltameter is connected across a $6 \ V$ battery,then the mass of copper deposited in $45 \ minutes$ would be ............. $g$.

$0.066 \ g$ of metal was deposited when a current of $2 \ A$ is passed through a metal ion solution for $100 \ s$. What is the electrochemical equivalent (in $g \ C^{-1}$) of the metal?