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1)

 Consider the following electrode processes of a cell

 Cl12Cl2+e

                                      [MCl+eM+Cl]

If EMF of this cell is -1.140 V and E0 value of the cell is -0.55 V  at 298 K, the value of the equilibrium constant of the sparingly soluble salt MCl is in the order of 


A) 1010

B) 108

C) 107

D) 1011

Answer:

Option A

Explanation:

MCl+eM+Cl cathode (reduction)

 Cl12Cl2+e   anode (oxidation)

  MClM+12Cl2

  The Kc of the cell reaction is calculated  from 

Nernst equation    Ecell=E0cell0.059nlogKc

 1.140=0.550.0591logc

 0.59=0.059logKc

 logKc=0.590.059=10

Kc=1010

 Ksp is for  M+12Cl2MClM++Cl

    Ksp=1Kc

 =11010=1010