The standard potentials of some electrodes are as follows. Arrange the metals in an increasing order of their reductiong power.
`1)K^(+)//K=-2.93V" "2)Ag^(+)//Ag =0.80V" "3) Cu^(2+)//Cu=0.34V`
`4)Mg^(2+)//Mg =-2.37V" "5)Cr^(3+)//Cr =-0.74C" "6)Fe^(+)//Fe =-0.44V`

Standard reduction electrode potential of three metals A, B and C are respectively +0.05 V, -3.0 and -1.2 V. The reducing powers of

Standard oxidation potential of iron electrode is + 0.44 V. Calculate the potential of Fe, FeSO_4(0.1 M) at 25^@C .

If the standard electrode protential of Cu^(2+)// Cu electrode is 0.34 V , what is the electrode potential at 0.01 M concentration of Cu^(2+) ? (T = 298^(@) K)

The emf of galvanic cell of the reaction Zn+Cu^(2+)rarr Zn^(2+) + Cu is (E^(@)Zn^(2+)//Zn " is" -0.76V " and " Cu^(2+)//Cu " is " +0.34V)

E.M.F of the cell reaction , 2Ag^(+) + Cu to 2Ag + Cu^(2+) is 0.46 V . If E_(Cu^(2+) // Cu)^(0) is | 0.34 V , E_(Ag^(+)//Ag)^(0) is

Given the standard electrode potentials K^(+)//K=-2.93V.Ag^(+)//Ag=0.80V . Which among them has greater reducing power ?

An aqueous solution containing one mole per litre of each Cu(NO_3)_2 , AgNO_3 . Hg(NO_3)_(2), Mg(NO_3)_2 is being electrolysed using inert electrodes. The values of standard electrode potential (reduction potential) in volts are Ag//Ag^(+) = + 0.80 V " "Hg//Hg^(2+) = + 0.79V " " Cu//Cu^(2+) = +0.34 V " " Mg//Mg^(2+) = -2.37 V With increasing voltage, the sequence of deposition of metals on cathode will be

At what concentration of copper sulphate solution, the potential of Cu^(2+) , Cu becomes zero? The standard reduction potential of Cu^(2+) , Cu is 0.34 V.