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[E(Cu^(2)+/Cu)=0.34V],[E(Cu^(+)/Cu)=0.52...

[E_(Cu^(2)+/Cu)=0.34V],[E_(Cu^(+)/Cu)=0.522V],[E_(Cu^(2)+/Cu^(+))=]

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E_(Cu^(2+)//Cu)^(@) =0.43V E_(Cu^(+)//Cu)^(@)=0.55V E_(Cu^(2+)//Cu^(+))^(@) =

Cu^(+) ion is not stable in aqueous solution because because of dispropotionation reaction. E^(@) value of disproportionation of Cu^(+) is [E_(Cu^(2+)//Cu^(+))^(@)=+ 0.15 V, E_(Cu^(2+)//Cu)^(@)=0.34 V]

Cu^(+) ion is not stable in aqueous solution because because of dispropotionation reaction. E^(@) value of disproportionation of Cu^(+) is [E_(Cu^(2+)//Cu^(+))^(@)=+ 0.15 V, E_(Cu^(2+)//Cu)^(@)=0.34 V]

Given the standard electrod potentials E_(Cu^(2+)//Cu)^(@)=0.34v and E_(Cu^(+)//Cu)^(@)=0.52V . What is K_(c) for the disproportion 2Cu^(+)toCu+Cu^(2+)

Explain why the stability of Cu^(+) io in aqueous solution is lower Cu^(2+) ion . E_(Cu^(2+)|Cu)^(@)= +0.34 "V & "E_(Cu^(+)|Cu)^(@)= +0.52 V

(CU^(+) ((aq)) is unstable in solution and undergoes simultaneous oxidation and reduction, according to the reaction 2Cu_((aq))^(+) Cu_((aq))^(2+) +Cu_((s)) choose E^(@) for the above reaction if E_(Cu^(2+)//Cu^(@))= 0.34V and E_(Cu^(2+)//Cu^(+) )= 0.15V