`Cu^(2+)+2e^(-) rarr Cu`. For this, graph between `E_(red)` versus `ln[Cu^(2+)]` is a straight line of intercept `0.34V`, then the electrode oxidation potential of the half cell `Cu|Cu^(2+)(0.1M)` will be

A reaction, Cu^(2+)+2e^(-) rarr Cu is given. For this reaction, graph between E_(red) versus ln[Cu^(2+)] is a straight line of intercept 0.34 V, then the electrode oxidation potential of the half-cell Cu//Cu^(2+) (0.1 M) will be

For the reaction, Cu^(2+)+2e^(-) to Cu , log [Cu^(2+)] vs E graph is of type as shown in figure where OA = 0.34 V,the electrode potential of the half-cell of Cu|Cu^(2+)(0.1 M) will be

Cu^(2+) +2e rarr Cu, log [Cu^(2+)] vs E_(red) .graph is of the type as shown in figure where OA =0.34 V then electrode otential of the half cell of Cu^(2+)(0.1M) will be :

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

The standard electrode potential of Cu^(2+)|Cu half cell is +0.34V . What does it mean?

The standard reduction potential for the reaction, 2Cu^(2+) + 2e^- rarr Cu is +0.34 V. the standard electrode potential for the reaction, 2Cu^(2+) + 4e rarr 2Cu will be

Given that K_(sp) of CuS=10^(-35) and E_Cu//Cu^(2+)= (-0.34V) . The standard oxidation potential of Cu|CuS|S^(2-) Half- cell is :