Given : `E_(cu^(+2)//cu)^0=0.34 V`
`E_(Cl_2//Cl^(-))^0`=1.36 V
`E_(Br_2//Br^(-))^0=1.08 V`
`E_(l_2//l^(-))^0=0.54 V`
`{:("Column-I","Column-II"),((A)Cu^(+2)+2Cl to Cu+Cl_2, (p)"Can produce electricity in the galvanic cell"),((B)Cl_2+CutoCu^(+2)+2Cl^(-),(q)"Can be made to occur in electrolysis cell"),((C )2I^(-)+"starch solution + chlorine water",(r)"Appearance of brown colour"),((D)2Br^(-)+C Cl_4+"Chlorine water",(s)"Appearance of violet colour"):}`

Answer

A`to`q , B`to`q , C-`to` s , D`to`r

Explanation

`(A)toq " " (E_("red")^(@))Cl_2//Cl^(-) gt (E_("red")^(@))Cu^(+2)//cu`
so reduction of `Cl_2` to `Cl^(-)` will occur at cathode and oxidation of Cu to `Cu^(+2)` will occur at anode.So reverse reaction is possible it means such reverse reaction can be made to occur in an electrolysis cell.
`(B)to p`
As mentioned in (a) the reaction is feasible and hence can produce electricity in the galvanic cell
`( C)tos " " 2I^(-)toCl_2 to I_2 ("violet")+2Cl^(-)`
`(E_("red")^@)_(Cl_2//Cl^(-)) gt (E_("red")^@)_(l_2//l^(-))`
`(D)to r " " 2Br^(-)toCl_2 to Br_2 ("Brown")+2Cl^(-)`
`(E_("red")^@)_(Cl_2//Cl^(-)) gt (E_("red")^@)_(Br_2//Br^(-))`