[" Given "Fe^(+2)+2e^(-)rarr Fe(s),E^(@)=-0.447V],[Fe^(+2)rarr Fe^(+3)+e^(-),E^(@)=-0.771V],[" Find "E^(@)" for the reaction "Fe^(+3)+3e^(-)rarr Fe(s)]

{:(Given Fe^(+2)+2e^(-)toFe(s),,,,E^(@)=-0.447V),(Fe^(+2)toFe^(+3)+e^(-),,,,E^(@)=-0.771V):} Find E^(@) for the reaction Fe^(+3)+3e^(-)toFe(s)

{:(Given Fe^(+2)+2e^(-)toFe(s),,,,E^(@)=-0.447V),(Fe^(+2)toFe^(+3)+e^(-),,,,E^(@)=-0.771V):} Find E^(@) for the reaction Fe^(+3)+3e^(-)toFe(s)

Given, standard electrode potentials Fe^(2+) +2e^(-) rarr Fe, E^(@)=-0.440 V Fe^(3+)+3e^(-) rarr Fe, E^(@)=- 0.036 V The standarde potential (E^(@)) for Fe^(2+)+e^(-) rarr Fe^(2+) , is

Electrode potential for the following half-cell reactions are Zn rarr Zn^(2+)+2e^(-), E^(@)=+0.76V, Fe rarr Fe^(2+)+2e^(-), E^(@)=+0.44V The EMF for the cell reaction Fe^(2+)+Zn rarr Zn^(2+)+Fe will be

If E_(Fe^(2+))^(@)//Fe = -0.441 V and E_(Fe^(3+))^(@)//Fe^(2+) = -0.771 V The standard EMF of the reaction Fe+2Fe^(3+) rarr 3Fe^(2+) will be: