Given electrode potentials asre
`Fe^(3+)+e^(-) rarr Fe^(2+)," "E^(c-)=0.771V`
I_(2)+2e^(-) rarr 2I^(c-)," "E^(c-)=0.536V`
`E^(c-)._(cell)` for the cell reaction,
`Fe^(3+)+2I^(c-) rarr Fe^(2+)+I_(2)` is

Given electrode potentials: Fe^(3+) + e^(-) rarr Fe^(2+) : E^(o) =0.771 V and I_(2) 2e^(-) rarr 2I^(-), E^(o) = 0.556 V then E^(o) for the cell reaction 2 Fe^(3+) 2I ^(-) rarr 2 Fe^(2+) + l_(2) will be:

Given electrode potentials are , Fe^(3+) + e to Fe^(2+), E^@ = 0.771V " " I_2 + 2e to 2I^(-), E^@ = 0.536 V , E^@ cell for the cell reaction, 2Fe^(3+) + 2I^(-) to 2Fe^(2+) + I_2 is

Given electrode potentials are: Fe^(3+) +e rarrFe^(2+) ,E^@=0.771V I_2 +2e rarr 2I^- ,E^@=0.536V E^@ cell for the cell reaction, 2Fe^(3+) +2I^- rarr2Fe(2+) +I_2 is:

Given standard E^(c-): Fe^(3+)+3e^(-)rarrFe," "E^(c-)=-0.036 Fe^(2+)+2e^(-)rarr Fe," "E^(c-)=-0.440V The E^(c-) of Fe^(3+)+e^(-) rarr Fe^(2+) is

Given standard E^(c-): Fe^(3+)+3e^(-)rarrFe," "E^(c-)=-0.036 Fe^(2+)+2e^(-)rarr Fe," "E^(c-)=-0.440V The E^(c-) of Fe^(3+)+e^(-) rarr Fe^(2+) is

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

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+) ?