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Question

CuI(s)+eCu(s)+I(aq); E=0.188 V
Cu2+(aq)+I+eCuI(s) E=0.868 V;
Ksp(CuI)=1012M2 and 298R ln 10F=0.059
If the equilibrium constant of the disproportionation reaction of Cu+ is Kc i.e.
2Cu+(aq)KcCu(s)+Cu2+(aq); then find the value of (0.59×logKc)

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Solution

Given,
CuI(s)Cu++I Ksp=1012 M2
So when [I]=1 M, then [Cu+]=1012 M
Again,
CuI(s)+eCu(s)+I(aq) E=0.188 V;
This is equivalent to
Cu+aq1012+eCu(s) E=0.188 V
So,
E=E10.0591log110120.188=E10.0591log11012
E1=0.52 V
Again,
Cu2+(aq)+I+eCuI(s) E=0.868 V
This is equivalent to
Cu2+(aq)1M+eCu+(aq)1012M E=0.868 V
So,
E=E20.0591log10121 0.868=E20.0591log10121
E2=0.16 V
Now for disproportionation of Cu+ i.e.
2Cu+(aq)Cu(s)+Cu2+(aq) Ecell=E1E2=0.520.16=0.36 V
So For equilibrium 2Cu+(aq)KcCu(s)+Cu2+(aq)
Ecell=0.0591logKc0.59logKc=3.6

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