Standard oxidation potential of iron electrode is `+ `0.44V. Calculate the potential of Fe, `FeSO_(4) ` ( 1M ) at `25^(@)C`.

The oxidation potential of a hydrogen electrode at pH =10 and P_(H_2) = 1 atm

Calculate the standard reduction potential of (Ag^+)/ (Ag) electrode when the cell potential for the cell Cu | Cu^2+ (1M) | | Ag^+(1M) | Ag is 0.46 V .

E^(@) of Ag electrode is 0.8 V and solubility product of AgI is 1 xx 10^(-16) . Calculate the potential of Ag electrode at 25^(@)C in a saturated AgI solution in water.

The standard electrode potential ( E^(@) ) for Daniel cell is + 1.1 V. Calculate, the Delta G^(@) for the reaction, Zn(s) + Cu^(2+) ( aq) rarr Zn^(2+) ( aq) + Cu(s) 1F = 96500 C "mol"^(-1))

Calculate the equilibrium constant for the reaction. 2Fe^(2+) + 3I^(-) hArr 2Fe^(3+) + I_(3)^(-) The standard reduction potential in acidic condition is 0.78 V and 0.54 V , respectively . For Fe^(3+) //Fe^(2+) and I_(3)^(-) //I couples.

Calculate the standard electrode potential of Ni^(2+) | Ni electrode if emf of the cell, Ni(s) | Ni^(2+) ( 0.01 M ) || Cu^(2+) ( 0.1M) | Cu(s) is 0.059 V. [ Given E_(Cu^(2+) //Cu) ^(@) = + 0.34V

The standard reduction potential for the reaction, 2Cu^(2+) + 2e^- rarr Cu is +0.34 V. the standard electrode potential for the reaction, 2Cu^(2+) + 4e rarr 2Cu will be

Copper from copper sulphate solution can be displaced by ………….The standared reduction potentials of some electrodes are given below: E^@(Fe^(2+),Fe) =-0.44V E^@(Zn^(2+),Zn)=-0.76 V E^@(Cu^(2+),Cu) =+0.34V E^@(Cr^(3+),Cr)=-0.74V E^@(H^+,1/2 H_2)=-0.00 V