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`.

Calculate the emf of the following cell. Zn(s)|Zn^(2+) (0.01M)|| Ag^+ (0.001M) | Ag(s) Given E_(Zn|Zn^(2+))^@ = 0.76V and E_(Ag|Ag^+)^@ = -0.80V

The standard cell potential for the cell is , Zn|Zn^(2+)(1M)||Cu^(2+)(1M)|Cu [E^@ for Zn^(2+)//Zn=-0.76V, E^@ for Cu^(2+)//Cu=+0.34V]

Write the cell reaction and calculate the emf of the Cell Zn|Co^2+(aq)|| Zn^2+(aq)| Co (Given E_(Zn|Zn^2+)^@=+0.76V and E_(Co|Co^2+)^@=+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")^(@)

The emf of a cell corresponding to the reaction, Zn(s) + 2H^(+) ( aq) rarr Zn^(2+) ( 0.1 M ) + H_(2) ( g , 1 atm) is 0.28 V at 25^(@)C . Write the half-cell reaction and calculate the pH of the solution at the hydrogen electrode. E_(Zn^(2+)//Zn)^(@) = - 0.76V, E_(H^(+) //H_(2))^(@) = 0

A cell is set up between ‘Zn’ and ‘Cu’ electrode. If the two half cells work under standard condition, calculate the cell potential. Given E^@(Zn^(2+)//Zn)=-0.76V and E^@(Cu^(2+)//Cu)=+0.34V .

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