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

How much charge in Coulombs is required for the oxidation of $1 \ mol$ of $H_2O$ to $O_2$?

$A$ solution of $Fe_{2}(SO_{4})_{3}$ is electrolyzed for '$x$' min with a current of $1.5 \ A$ to deposit $0.3482 \ g$ of $Fe$. The value of $x$ is $.......$. [nearest integer]
Given : $1 \ F = 96500 \ C \ mol^{-1}$
Atomic mass of $Fe = 56 \ g \ mol^{-1}$

$7.5 \ A$ 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). $[Ag = 108 \ u]$

Aqueous copper sulphate solution and aqueous silver nitrate solution are electrolysed by $1 \ A$ current for $10 \ minutes$ in separate electrolytic cells. Will the mass of copper and silver deposited on the cathode be same or different? Explain your answer.

Same amount of electricity is passed through aqueous solutions of $AgNO_3$ and $CuSO_4$. The number of $Ag$ and $Cu$ atoms deposited are $x$ and $y$ respectively. The correct relationship between $x$ and $y$ is