`Fe^(2+)+Ag^(+)toFe^(3+)+Ag` if `E^(@)` of `Ag^(+)//Ag=x` `E^(@)` of `Fe^(@+)//Fe=y` `E^(@)` of `Fe^(3+)//Fe=z` Determine std. EMF of given cell reaction.
Calculate the standard cell potential (in V) of the cell in which following reaction takes place: Fe ^( 2 + ) ( aq ) + A g^ + ( aq ) to Fe ^( 3 + ) ( aq ) + Ag (s ) Given that E _ (Ag ^ + // Ag ) ^ 0 = x V , E _ ( Fe^( 2+ ) // Fe ) ^0 = yV , E _ (Fe^(3+)//F e )^0 = z V
Calculate the standard cell potentials of the galvanic cells in which the following reactions take place. (a) " " 2Cr(s)+3Cd^(2+) to 2Cd^(3+)(aq)+3Cd(s) Given E_(Cr^(3+)//Cr)^(@)=-0.74" V" , E_(Cd^(2+)//Cd)^(@)=-0.40" V" (b) " " Fe^(2+)(aq)+Ag^(+)(aq) to Fe^(3+)(aq)+Ag(s) Gievn E_(Ag^(+)//Ag)^(@)=0.80" V" ,E_(Fe^(3+)//Fe^(2+))^(@)=0.77 " V" Also calculate DeltaG^(@) and equilibrium constant for the reaction.
The standard reduction for the following reactions are : Fe^(3+) + 3e^(-) rarr Fe with E^(@) = - 0.036 V Fe^(2+) + 2e^(-) rarr Fe with E^(@) = - 0.44 V What would be the standard electrode potential for the reaction Fe^(3+) + e^(-) rarr Fe^(2+) ?
Show that E_(Fe^(+3)//Fe^(+2))^(@) =3E_(Fe^(+3)//Fe)^(@)-2E_(Fe^(+2)//Fe)^(@)
At equimolar concentration of Fe^(+2)//Fe^(+3) , what must [Ag^(+)] be so that voltage of the galvanic cell made from Ag^(+)//Ag and Fe^(3+)//Fe^(2+) electrodes equals zero ? The reaction is Fe^(+2)+Ag hArr Fe^(3+)+Ag . Determine the equilibrium constant at 25^(@)C for the reaction. Given E_(Ag^(+)//Ag)^(@)=0.799 volt and E_(Fe^(3+)//Fe^(2+))^(@)=0.771 volt.
Calculate the standard reduction potentials of galvanic cells in which reaction are Fe^(2+) (aq) + Ag^(+) (aq) to Fe^(3+) (aq) + Ag (s) Given that E^(Theta) (Cr^(3+) //Cr) = -0.74 V , E^(Theta) (Cd^(2+) // Cd) = -0.40 V , E^(Theta) (Fe^(3+) // Fe^(2+)) = 0.77 V , E^(Theta) (Ag^(+) // Ag) = 0.80 V
