`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

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

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

The emf of the cell, Zn|Zn^(2+) (0.01 M)||Fe^(2+) (0.001 M)|Fe at 298 K is 0.2905 V then the value of equilibrium constant for the cell reaction is :

The emf of the cell, Zn|Zn^(2+)(0.01M)|| Fe^(2+)(0.001M) | Fe at 298 K is 0.2905 then the value of equilibrium constant for the cell reaction is:

The standard e.m.f. of the cell Zn| Zn^(2+) (0.01 M) || Fe^(2+) (0.001 M) | Fe at 298 K is 0.02905 then the value of equilibrium constant for the cell reaction 10^(x) . Find x.