Consider the following electrode processes of a cell, Cl ⁻ 1 2 Cl ₂+e⁻ [ MCl +e⁻ M+ Cl ⁻ ] If EMF of this cell is -1.140 ~V and E^ value of the cell is -0.55 ~V at 298 ~K , the value of the equilibrium constant of the sparingly soluble salt M Cl is in the order of

Step-by-step solution

MCl +e⁻ M+ Cl ⁻ cathode (reduction) Cl ⁻ 1 2 Cl ₂+e⁻ anode (oxidation) MCl M + 1 2 Cl ₂ The K_C of the cell reaction is calculated from Nernst equation E_ cell =E^ cell - 0.059 n K_c aligned & -1.140=-0.55- 0.059 1 c & -0.59=-0.059 K_c & K_c= 0.59 0.059 =10 & K_C=10¹⁰ & K_ s p is for M+ 1 2 Cl ₂ M Cl M⁺+ Cl ⁻ & K_ s p = 1 K_c & = 1 10¹⁰ =10⁻¹⁰ aligned