Fe is reacted with `1.0M HCI.E^(@)` for `Fe//Fe^(2+) = +0.34` volt. The correct observation (s) regarding this reaction is/are:

Will Fe be oxidised to Fe^(2+) by reaction with 1.0 M HCl? E^(@) for Fe//Fe^(2+)=+0.44 volt.

E^(@) of Fe^(2 +) //Fe = - 0.44 V, E^(@) of Cu //Cu^(2+) = -0.34 V . Then in the cell

E^(@) of Fe^(2 +) //Fe = - 0.44 V, E^(@) of Cu //Cu^(2+) = -0.34 V . Then in the cell

The standard reduction for the following reactions are : Fe^(3+) + 3e^(-) rarr Fe with E^(@) = - 0.036 V Fe^(2+) + 2e^(-) rarr Fe with E^(@) = - 0.44 V What would be the standard electrode potential for the reaction Fe^(3+) + e^(-) rarr Fe^(2+) ?

At equimolar concentration of Fe^(+2)//Fe^(+3) , what must [Ag^(+)] be so that voltage of the galvanic cell made from Ag^(+)//Ag and Fe^(3+)//Fe^(2+) electrodes equals zero ? The reaction is Fe^(+2)+Ag hArr Fe^(3+)+Ag . Determine the equilibrium constant at 25^(@)C for the reaction. Given E_(Ag^(+)//Ag)^(@)=0.799 volt and E_(Fe^(3+)//Fe^(2+))^(@)=0.771 volt.

For the reaction, Fe^(3+)+3e^(-) hArr Fe, E^(@) is -0.036 volt and the standard electrode potential for Fe^(3+)+e^(-) hArr Fe^(2+) is 0.771 volt. Calculate the E^(@) for Fe^(2+)+2e^(-) hArr Fe .

If E_(1)^(0) is standard electron potential for Fe//Fe^(+2) and E_(2)^(0) is for Fe^(+2)//Fe^(+3) and E_(3)^(0) for Fe//Fe^(+3) which of the following relation is correct?

If e_(Fe^(2+) //Fe)^@ =- 0. 44 1V . And E_(Fe^(3+)//Fe^(2+))^(o) = 0. 771 V . The standard emf of the reaction Fe +2 Fe^(3+) rarr 3Fe^(2+) will be .