`Zn|Zn_((ag))^(2+)||Cu_((ag))^(2+)| Cu E^(@)` for the cell is 1.10V at `25^(@)C`. The equilibrium constant for the cell reaction is of the order of

E^(@) for the cell Zn(s)|Zn^(2+)(aq)|Cu^(2+)(aq)|Cu(s) is 1.1V at 25^(@)C the equilibrium constant for the cell reaction is about

E^(@) for the electrochemical cell Zn(s)|Zn^(2+) 1 M (Aq.)||Cu^(2+) 1 M (aq.)|Cu(s) is 1.10 V at 25^(@)C . The equilibrium constant for the cell reaction, Zn(s) +Cu^(2+) (aq.) hArr Zn^(2+) (aq.)+Cu(s) Will be :

In the cell Zn|Zn^(2+)||Cu^(2+)|Cu , the negaitve terminal is

For the cell reaction , Ni_(s)| Ni _((aq))^(2+) | |Ag_((aq)) |Ag_((s)) Calculate the equilibrium constant at 25^(@)C . How much maximum work would be obtained by operation of this cell? E_(Zn^(2+)//Zn)^(@)=-0.25V and E_(Ag^(+)//Ag)^(@)=0.80V

For the cell Zn(s)|Zn^(2+)||Cu^(2+)|Cu(s) , the standard cell voltage, E^(c-)._(cell) is 1.10V . When a cell using these reagents was prepared in the lab, the measured cell voltage was 0.98V . One possible explanatino for the observed voltage is

Zn(s) + Cu^(2+)(aq) rarr Zn^(2+)(aq) + Cu(s) The cell representation for the above redox reaction is

The standard potential E^(@) for the half reactions are as : Zn rarr Zn^(2+) + 2e^(-), E^(@) = 0.76V Cu rarr Cu^(2+) +2e^(-) , E^(@) = -0.34 V The standard cell voltage for the cell reaction is ? Zn +Cu^(2) rarr Zn ^(2+) +Cu

The standard emf for the cell cell reaction Zn + Cu^(2+) rarr Zn^(2+) + Cu is 1.10 volt at 25^@ C . The emf for the cell reaction when 0.1 M Cu^(2+) and 0.1 M ZN^(2+) solutions are used at 25^@ =C is .

The equilibrium constant of the reaction; Cu(s)+2Ag + (aq)⟶Cu 2+ (aq)+2Ag(s) E o =0.46V at 298K

The cell , Zn | Zn^(2+) (1M) || Cu^(2+) (1M) Cu (E_("cell")^@ = 1. 10 V) , Was allowed to be completely discharfed at 298 K . The relative concentration of 2+ to Cu^(2+) [(Zn^(2=))/(Cu^(2+))] is :