Match the items of column I with column II on the basis of data given below:
`E_(F_2|F^-)^@=2.87V, E_(Li^+|Li)^@=-3.5V`
`E_(Au^(3+)|Au)^@=1.4V, E_(Br_2|Br^-)^@=1.09V`

An aqueous solution containing 1M each of Au^(3+),Cu^(2+),Ag^(+),Li^(+) is being electrolysed by using inert electrodes. The value of standard potentials are : E_(Ag^(+)//Ag)^(@)=0.80 V,E_(Cu^(+)//Cu)^(@)=0.34V and E_(Au^(+3)//Au)^(@)=1.50,E_(Li^(+)//Li)^(@)=-3.03V will increasing voltage, the sequence of deposition of metals on the cathode will be :

Which of the following statements is correct? If E_(Cu^(2+)|Cu)^(@)=0.34V, E_(Sn^(2+)|Sn)^(@)=-0.136V "and"E_(H^+|H_2)^(@)=-0.0V

When a solution of AgNO_3 (1 M) is electrolysed using platinum anode and copper cathode, what are the products obtained at two electrodes? Given : E_(cu^(2+)|cu)^(@)=+0.34 V , E_(H_2O|O_2,H^+)^(@)=-1.23 V E_(H^+|H_2)^(@)=+0.0V , E_(ag^+|Ag)^(@)=+0.8 V

Can Fe^(3+) oxidise Br^- to Br_2 under standard conditions? E_(Fe^(3+)|Fe^(2+))=0.771V , E_(Br_2|Br^-)=1.09V .

Can a zinc spoon be used to stir a solution of copper sulphate? Support your answer with reason E_(Zn^(2+)|Zn)^@=-0.76V , E_(Cu^(2+)|Cu)^@=+0.34V

Based on the data, arrange Fe^(2+), Mn^(2+) and Cr^(2+) in the increasing order of stability of +2 oxidation state: E_(Cr^(3+)//Cr^(2+))^0= -0.4V, E_(Mn^(3+)//Mn^(2+))^0= 1.5V, E_(Fe^(3+)//Fe^(2+))^0= 0.8V

The calculate the e.mf. Of the following cell at 298: Fe|Fe^(2+)(0.1M)||Ag^(2+)(0.1M)|Ag E_((Fe^(2+)//Fe))^(@)=-0.44V,E_((Ag^(+)//Ag))^(@)=0.80V .