calculate equilibrium constant for reaction at 298 k.zn+cu2+gives zn2+ +cu given that Eo zn2+/zn=0.76v Eo cu2+/cu + 0.34v.

As we know that the free energy change in an electrochemical cell is:

∆G0 = -nFE0  --------------(1)

Also from kinetic perspective we have,

∆G0 = -RT ln K --------------(2)

Thus, from these 2 equations we get

ln K = nFE0RTThus,log K = nE00.0592

E0 = E cathode - E anode

Here Zn which has higher oxidation potential will act as anode where as Cu electrode will act as cathode

E0 = + 0.34 -(-0.76)
  = 1.1 V

Substituting values we get,log K = 2 x 1.10.0592= 37.162K = antilog 37.162K =1.44 x 1037




 

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