The electrochemical cell shown below is a concentration cell. `M|M^(2+)(` saturated solution of sparingly soluble salt, `MX_(2))||M^(2+)(0.001 mol dm^(-3))|M`
The `emf` of the cell depends on the difference in the concentration of `M^(2+)` ions at the two electrodes. The `emf` of the cell at `298` is `0.059V`.
The solubility product `(K_(sp),mol^(3) dm^(-9))` of `MX_(2)` at 298 based on the information available the given concentration cell is `(` Take `2.303xxRxx298//F=0.059V)`

The electrochemical cell shown below is a concentration cell. M|M^(2+) (("Saturated solution"),("of sparingly soluble"),("salt, "MX_(2)))||M^(2+) (0.001" mol dm"^(-3))|M The emf of the cell depends on the difference in concentrations of M^(2+) ions at the two electrodes. The emf of the cell at 298 K is 0.059 V. The solubility product (K_(sp), mol^(3) dm^(-9)) of MX_(2) at 298 K based on the information available for the given concentration cell is ("take "2.303xxRxx298//F=0.059 V) :

The electrochemical cell shown below is a concentration cell. M|M^(2+) (saturated solution of a sparingly soluble salt, MX_2 || M^(2+) (0.001 mol dm^(-3) ) |M The emf of the cell depends on the difference in concentration of M^(2+) ions at the two electrode The emf of the cell at 298 is 0.059 V The solubility product (K_(sp) , mol^(3) dm^(-9)) of MX_2 at 298 based on the information available the given concentraiton cell is (take 2.303 xx R xx 298 // F = 0.059 V )

The electrochemical cell shown below is a concentrstion cell. M|M^(2+) (saturated solution of a sparingly soluble salt, Mx_2 )|| M^(2+)(0.001 mol dm^3)|M The emf of the cell depends on the difference in concentrations of M^(2+) ions at the two electrods. The emf of the cell at 298K is 0.059V. The value of /_\G(kJ mol^-1) for the given cell is (take 1F = 96500Cmol^-1 )

The electrochemical cell shown below is a concentration cell M//M^(2+) (saturated solution of a sparingly soluble salt, MX_(2))||M^(2+)(0.001 mol dm^(-3))|M The emf of the cell depends on the difference in concentrations of Mn^(2+) ions at the two electrodes. The emf of the cell at 298 K is 0.059 V . The value of DeltaG ( kJ "mol"^(-1)) for the given cell is : (take 1 F = 96500 C "mol"^(-1) )