Home
Class 12
CHEMISTRY
Determine the equilibrium constant for t...

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`.

Promotional Banner

Similar Questions

Explore conceptually related problems

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

Calculate the equilibrium constant for the reaction. Fe(s) + Cd^(2+) (aq) hArr Fe^(2+)(aq) + Cd(s) [ Given, E_(Cd^(2+) //Cd)^(@) = - 0.40V , E_(Fe^(2+)//Fe)^(@) = - 0.44 V ]

Calculate the equilibrium constant for the reaction : Fe(s)Cd^(2+)(aq)harrFe^(2+)(aq)+Cd(s) ("Given" E_(cd^(2+)//Cd)^(@)=-0.40 V, E_(Fe^(2+)//Fe)^(@)=-0.44 V)

Calculate the equilibrium constant for the reaction 2Fe3+(aq) + 2I– (aq) → 2Fe2+(aq) + I2(s) E0cell = 0.236V

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