$A$ 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 $.7$)

The number of coulombs required for the deposition of $107.870 \ g$ of silver is

How many coulombs are required to oxidise $0.1 \ mole$ of $H_2O$ to oxygen?

Faraday's laws of electrolysis will fail when

$250 \ mL$ of a waste solution obtained from the workshop of a goldsmith contains $0.1 \ M \ AgNO_3$ and $0.1 \ M \ AuCl$. The solution was electrolyzed at $2 \ V$ by passing a current of $1 \ A$ for $15 \ minutes$. The metal/metals deposited will be
$(E^0_{Ag^+/Ag} = 0.80 \ V, E^0_{Au^+/Au} = 1.69 \ V)$

In the electrolysis of acidulated water,it is desired to obtain $1.12 \ cc$ of hydrogen gas per second at $STP$ conditions. The current to be passed is: (in $A$)