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

Determine the equilibrium constant for the reaction : Fe^(2+)(aq)+Ce^(4+)(aq)rarr Fe^(3+)(aq)+Ce^(3+)(aq) Givne : E_(Ce^(4+)|Ce^(3+))^(@)=1.44V & E_(Fe^(3+)|Fe^(2+))^(@)=0.77V .

Calculate at 25^(@) C , the equilibrium constant for the reaction : 2 Fe^(3+) + Sn^(2+) hArr 2 Fe^(2+) + Sn^(4+) Given that E_((Fe^(3+)|Fe^(2+)))^(Theta) = 0.771 V , E_((Sn^(4+) |Sn^(2+)))^(Theta) = 0.150 V

What will be the standard electrode potential for the change, Fe^(3+)(aq)+e rarr Fe^(2+)(aq). Given : E_(Fe^(3+)|Fe)^(@)=-0.036V, E_(Fe^(2+)|Fe)^(@)=-0.439V

Calculate the emf of the following call at 298 K : 2Cr(s)+3Fe^(2+)(0.1M)rarr2Cr^(3+)(0.01M)+3Fe(s) ["Given : "E_((Cr^(3+)|Cr))^(@)=-0.74V, E_((Fe^(2+)|Fe))^(@)=-0.44V]