The reduction potential diagram for 'Cu' in acid solution is as follows. Calculate 'X. Cut2 → Cut → Cu +0.15 V +0.5 V E°=X volts 0.325 V 0.35 V 0.34 V 0.345 V

Latimer diagram for Cu in an acidic solution is: Cu^(+2) overset(+0.15V)toCu^(+) overset(+0.50)toCu,

Calculate the reduction potentials for the following half cells: Cu|Cu^(2+)(0.2M), E_(Cu^(2+),Cu)^@=0.34V

The standard reduction potential of Zn is -0.76V and that of Cu is +0.34V . What do they indicate?

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

What is the reduction electrode potential (in volts) of copper electrode, when [Cu^(2+)] = 0.01 M is in a solution at 25^@ C? ( E^@ of Cu^(2+)//Cu electrode is + 0.34 V.)

Calculate the electrode potential of copper electrode in a 0.1 M copper sulphate solution at 25^(@) C. (E^(@)(Cu^(2+)|Cu) = 0.34V) .