An electrochemical cell has two half cell reaction as, `A^(2+)+2e^-,E^0=0.34V`
`XtoX^(2+)+2e^-,E^0=+2.37V`. The cell voltage will be

An electrochemical cell has two half cell reaction as, A^(2+)+2e^-toA,E^0=0.34V XtoX^(2+)+2e^-,E^0=+2.37V . The cell voltage will be

An electrochemical cell has two half cell reactions as A^(2+) + 2e^(-) rarr A ; E^(0) =0.63V ; X rarr X^(2+)+2e^(-) ; E^(0) =2.37V The cell voltage will be

The standard electrode potentials E^(@) for the half cell reactions are as : ZntoZn^(2+)+2e^(-),E^(@)=0.76V FetoFe^(2+)+2e^(-),E^(@)=041V The EMF of the cell reaction Fe^(2+)+ZntoZn^(2+)+Fe is :

The standard electrode potential of the htwo half cells are given below Ni^(+2) + 2e^(-) to Ni , E^(@) = -0.25 V , Zn^(+2) + 2e^(-) to Zn , E^(0) = -0.77 V The voltage of cell formed by combining the two half cells would be

The standard potential (E^(0)) for the half reaction are as Zn to Zn^(2+) + 2e^(-) , E^(0) = + 0.76 V Fe to Fe^(2+) + 2e^(-) , E^(0) = + 0.41 V . The emf for the cell reaction Fe^(2+) + Zn to Zn^(2+) + Fe is

The standard oxidation potential E^@ for the half cell reaction are Zn rarr Zn^2+2e^- E^@=+ 0.76 V Fe rarr Fe^2+ + 2e^- E^@=+ 0.41 V EMF of the cell rection is Zn+Fe^(2+) rarr Zn^(2+)+Fe