Calculate the standard free energy change of the reaction taking place in the cell `Z_n(s)+Cu^2+(aq) overset(rightarrow)(leftarrow)Z_n^2+(aq)+Cu(s).(Given E^0 Z_n^2+//Z_n=0.76v` and `E^0C_u^2+//C_u=+0.34V, F=96500)`

Calculate the standard emf of the cell having the cell reaction. Zn(s) + Co^(2+) ( aq) rarr Zn^(2+) ( aq) + Co(s) E_(Zn//Zn^(2+)) ^(@) = 0.76V, E_(Co//Co^(2+))^(@) = 0.25V

What is meant by electrode potential? Explain in the half cell reactions of Zn(s) + Cu^(2+) ( aq) rarr Zn^(2+) (aq) + Cu(s)

Derive Nerst equation for EMF of the following cell. Zn (s) + Cu^2+ (aq) rarr Zn^2+ (aq) + Cu(s)

Represent the galvanic cell in which the reaction, Zn(s) + Cu^(2+) (aq) rarr Zn^(2+) (aq) + Cu(s) take place.

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")^(@)

For the Daniel Cell derive the relation E_(cell) =E_(cell)^0-0.0591/(2) log [Z_n^2+(aq)]/[Cu^2+(aq)]