Li + + e – ® Li(s) – . Table . : Standard Electrode Potentials at K Ions are present as aqueous species and H O as liquid; gases and solids are shown by g and s. Reaction (Oxidised form + ne – ® ® ® ® ® Reduced form) E o /V Increasing strength of oxidising agent Increasing strength of reducing agent .
A negative E o means that the redox couple is a stronger reducing agent than the H + /H couple. . A positive E o means that the redox couple is a weaker reducing agent than the H + /H couple. In Daniell cell, the electrode potential for any given concentration of Cu + and Zn + ions, we write For Cathode: /Cu /Cu – RT F ln aq ( .
) For Anode: /Zn / Zn – RT F ln aq ( . ) The cell potential, E (cell) = /Cu /Zn / Cu – RT F ln + (aq) / Zn + RT F ln + (aq) / Cu / Zn – RT F + + ln – ln aq