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

The relation between Faraday constant $(F)$,chemical equivalent $(E)$,and electrochemical equivalent $(Z)$ is

One Faraday of electricity liberates $x \times 10^{-1}$ gram atom of copper from copper sulphate,$x$ is . . . . . . .

$A$ current of $15.0 \ A$ is passed through a solution of $CrCl_2$ for $45 \ min$. The volume of $Cl_2$ (in $L$) obtained at the anode at $1 \ atm$ and $273 \ K$ is around ($1 \ F = 96500 \ C \ mol^{-1}$,At. wt. of $Cl=35.5$,$R=0.082 \ L \ atm \ K^{-1} \ mol^{-1}$) (in $.7$)

$0.50 \, L$ of a $0.60 \, M$ $CuSO_4$ solution is electrolyzed for a period of $30.0 \, min$ using a current of $4.60 \, A$. If inert electrodes are used,what is the final concentration of $Cu^{2+}$ remaining in the solution? $M$

Passage of a current for $548 \, s$ through a silver coulometer results in the deposition of $0.746 \, g$ of silver. What is the current (in $A$)?