If `-Delta G^(o)` is zero for a cell, the equilibrium constant for cell reaction is

The value of equilibrium constant for a feasible cell reaction is :

For a cell involving one electron E_(cell)^(0)=0.59V and 298K, the equilibrium constant for the cell reaction is: [Given that (2.303RT)/(F)=0.059V at T=298K ]

The cell potential for the unbalanced chemical reaction: Hg_(2)^(2+)+NO_(3)^(-)+H_(3)O^(+) to Hg^(2+) +HNO_(2)+H_(2)O+e^(-) Is measured under standard conditions in the electrochemical sell shown in the diagram were Equilibrium constant for cell reaction is :

E^(@) for the cell Zn(s)|Zn^(2+)(aq)|Cu^(2+)(aq)|Cu(s) is 1.1V at 25^(@)C the equilibrium constant for the cell reaction is about

Zn|Zn^(2+)(a=0.1M)||Fe^(2+)(a=0.01M)Fe. The EMF of the above cell is 0.2905 . The equilibrium constant for the cell reaction is

Derive an expression relating standard e.m.f. of the cell with the equilibrium constant of the cell reaction.

Given that equilibrium constant for the reaction 2SO_(2)(g) + O_(2)(g)hArr2SO_(3)(g) has a value of 278 at a particular temperature. What is the value of the equilibrium constant for the following reaction at the same temperature ? SO_(3)(g)hArrSO_(2)(g) + (1)/(2)O_(2)(g)

The E_("cell") of the reaction MnO_(4)^(-)+Fe^(+2)+H^(+)rarrMn^(2+)+H_(2)O is 0.59 V at 25^(@)C The equilibrium constant for the reaction is

The cell in which the following reaction occurs 2Fe^(3+)(aq)+2I^(-)(aq)to2Fe^(2+)(aq)+I_(2)(aq)+I_(2)(s) has E_(cell)^(0)=0.236V at 298 K. Calculate the standard gibbs energy and the equilibrium constant of the cell reaction.

For the reaction 2NO_(2)(g)+(1)/(2)O_(2)(g)hArrN_(2)O_(5)(g) if the equilibrium constant is K_(p) , then the equilibrium constant for the reaction 2N_(2)O_(5)(g)hArr4NO_(2)(g)+O_(2)(g) would be :