Calculate the equilibrium constant for the reaction `:`
`Fe^(2+)Ce^(4+)hArrFe^(3+)+Ce^(3+)`
Given `:E^(c-)._((Ce^(4+)|Ce^(3+)))=1.44V`
`E^(c-)._((Fe^(3+)|Fe^(2+)))=0.68V`

Calculate the equilibrium constant for the reaction : Fe^(2+)+Ce^(4+)hArr Fe^(3+)+Ce^(3+) Given, E_(Ca^(4+)//Ce^(3+))^(@)=1.44V and E_(Fe^(3+)//Fe^(2+))^(@)=0.68V

Calculate the equilibrium constant for the reaction Fe(s)+Cd2+(aq)⇔Fe2+(aq)+Cd(s) (Given : E∘Cd2+∣Cd=0.40V,E∘Fe2+∣Fe=−0.44V).

(a) Corrosion is essentially an electrochemical phenomenon. Explain the reactions occurring during corrosion of iron kept in an open atmosphere. (b) Calculate the equilibrium constant for the equilibrium reaction Fe_((s)) + Cd_((aq))^(2+) hArr Fe_((aq))^(2+) + Cd_((s)) (Given : E_(Cd^(2+)|Cd)^(@) = -0.40 V , E_(Fe^(2+)|Fe)^(@) = -0.44V ).

Calculate the equilibrium constant for the reaction Fe + CuSO_4 ⇌ FeSO_4 + Cu at 25°C. (Given E°(OP/Fe) = 0.5 V°, E°(OP/Cu) = -0.4 V)

The equilibrium constant (K) for the reaction Fe^(2+)(aq)+Ag^(+)(aq)toFe^(3+)(aq)+Ag(s) will be Given E^(@)(Fe^(3+)//Fe^(2+))=0.77V, E^(@)(Ag^(+)//Ag)=0.80V

Calculate DeltaG^(@) for the reaction : Cu^(2+)(aq) +Fe(s) hArr Fe^(2+)(aq) +Cu(s) . Given that E_(Cu^(2+)//Cu)^(@) = 0.34 V , E_(Fe^(+2)//Fe)^(@) =- 0.44 V

Calculate DeltaG^(@) for the reaction : Cu^(2+)(aq) +Fe(s) hArr Fe^(2+)(aq) +Cu(s) . Given that E^(@)Cu^(2+)//Cu = 0.34 V , E_(Fe^(+2)//Fe)^(@) =- 0.44 V

Calculate the n-factor of reactants in the given reactions. (c ) [Fe(CN)_(6)]^(4-)rarr Fe^(3+)+CO_(2)+NO_(3)^(-)

Calculate the n-factor of reactants in the given reactions. (e ) Fe_(2)(SO_(4))_(3)rarr Fe^(2+)+SO_(2)

The expression for equilibrium constant, K_(c) for the following reaction is Fe_((aq))^(3+)+3OH_((aq))^(-)hArrFe(OH)_(3(s))