The magnitude of the equilibrium constant `(K_(eq))` for a cell reaction is related to the magnitude of the standard Gibbs energy change for cell reaction by.

If the equilibrium constant of a reaction is 2×10^3 at 25°C then the standard Gibbs free energy change for the reaction will be

If the equilibrium constant of a reaction is 2×10^3 at 25°C then the standard Gibbs free energy change for the reaction will be

Knowing the equilibrium constant value of a cell reaction at a particular temperature, how will you calculate the standard Gibbs free energy change for the reaction?

The EMF of a cell is related to the equilibrium constant of the cell reaction as

Calculate the standard Gibbs energy change for the redox reaction of Daniel cell .

The equilibrium constant for certain reaction is 100 . If the value R is given to be 2 cal K^(-1) mol^(-1) , then standard Gibb's free energy change will be

The equilibrium constant K_(p) for a homogeneous gaseous reaction is 10^(-8) . The standard Gibbs free energy change DeltaG^(ɵ) for the reaction ("using" R=2 cal K^(-1) mol^(-1)) is

The equilibrium constant K_(p) for a homogeneous gaseous reaction is 10^(-8) . The standard Gibbs free energy change DeltaG^(ɵ) for the reaction ("using" R=2 cal K^(-1) mol^(-1)) is