If `E^@(Zn//Zn^(2+))=+0.76V`, `E^@ (Ag^+//Ag) =+0.80V `, find the emf of the cell -`Zn//Zn^(2+) (0.01M)abs"Ag+(0.1M)//Ag`.

The standard oxidation potentials, E^@ for the half reactions are : ZnrarrZn^(2+) +2e ,E^@=+0.76V Ag rarr Ag^+ +e,E^@=-0.77V The standard emf of the cell, Ag^+ +Zn rarrZn^(2+)+Ag is :

Write the cell reaction and cell potential of the cell Zn//Zn^(2+)(0.01 M)abs"Ag^+(0.1M)//Ag. Given E^0(Zn^(2+)//Zn)=-0.76V E^0(Ag^+//Ag)=+0.80V .

For the reaction at 298K, Ag^+(aq)+e^- =Ag(s),E^@=+0.80V Sn^(2+)(aq) +2e^- =Sn(s),E^@=-0.14V what is the emf of the cell reprsented as Sn|Sn^(2+)||Ag^+| Ag, if each ion having unit concentration:

Describe the construction and working of Daniell cell. The following reaction occurs in a cell Zn (s) + Co^(2+) ( aq) hArr Co(s) + Zn^(2+)(aq) Write the electrode reaction and find out the emf of the cell. Given Zn(s) rarr Zn^(2+)(aq) , E^(@) = 0.76 V CO(s) rarr Co^(2+)(aq) , E^(@) = 0.28V

Calculate the cell emf and Delta_(r ) G^(@) for the cell reation at 25^(@)C . Zn(s) | Zn^(@+) ( 0.1 M )|| Cd^(2+) ( 0.01M) | Cd(s) Given, E_(Zn^(2+) //Zn)^(@) = - 0.763V , E_(Cd^(2+) //Cd) ^(@) = - 0.403 V 1F = 96500 C "mol"^(-1) R = 8.314 JK^(-1) "mol"^(-1) ], Find E_("cell")^(@) = E_("cathode")^(@) - E_("anode")^(@) then Delta _(r ) G^(@) by using formula, Delta _(r ) G^(@) = - n FE_("cell")^(@)