Define standard emf of a cell.

Define standard mass.

The relationship between equilibrium constant and standard emf of a cell is

Calculate the standard emf of the cell having the standard free energy change of the cell reaction is -64.84 kJ for 2 electrons transfer.

The standard free energy change of the reaction M_((aq))^(+)+e rarrr M_((s)) is -23.125kJ . Calculate the standard emf of the half cell.

The emf of the half cell Cu_((aq))^(2+)//Cu_((s)) containing "0.01 M Cu"^(2+) solution is +0.301 V . Calculate the standard emf of the half cell.

For a cell reaction involving two electron changes the standard emf of the cell is found to be 0.295V at 25C. The equilibrinm constant of the reaction at 25^@C will be?

The equilibrium constant of cell reaction : Ag_((s))+Fe^(3+)hArr Fe^(2+)+Ag^(+) is 0.335, at 25^(@)C . Calculate the standard emf of the cell Ag//Ag^(+), Fe^(3+), Fe^(2+)//Pt . Calculate E^(@) of Fe^(3+), Fe^(2+)//Pt half cell. (Given - E^@ of Ag^+//Ag = 0.8)

Given the standard half - cell potentials (E^(@)) of the following as : Zn rarr Zn^(2+)+2e , E^(@)=+0.76V Fe rarr Fe^(2+)+2e, E^(@)=0.41V The the standard EMF of the cell with the reaction Fe^(2+)+Zn rarr Zn^(2+)+Fe is -

See whether the cell representation given below is in accordance with the conventation or not. If it is not, then write the correct representation and reaction of the cell. Calculate the standard EMF of the cell: Cu|Cu^(2+)||Zn|Zn^(2+) . ["Given : "E_(Cu^(2+)|Cu)^(@)=+0.34V, E_(Zn^(2+)|Zn)^(@)=-0.76V]

Under what condition will the terminal potential difference be more than the emf of a cell?