If the `Pb^(2+)` ion concentration is maintained at `1.0 M` , what is the `[Cu^(2+)]` concentration when the cell potential drops to zero? `E^(o) ""_(cell)= 0.473V`, and cell reaction is `Pb (s)abs(Pb^(2+ )(1.0M))abs(Cu^(2+)(1.0xx10^(-4)M)) Cu(s)`

If the Pb^(2+) concentration is maintained at 1.0M what is the [Cu^(2+)] , when the cell potential drops to zero ? E_("cell")^@ = 0.473V, Pb(s) // Pb^(2+) // Cu^(2+) // Cu(s)

A copper-silver cell is set up. The copper ion concentration in it is 0.10 M. The concentration of silver ions is not known.The cell potential measured is 0.422 V. Determine the concentration of silver ions in the cell. [Given E_(Ag^(+)//Ag)^(@)=0.80,E_(Cu^(2+)//Cu)^(@)=+0.34 V]

A copper-silver cell is set up. The copper ion concentration in it is 0.10 M. The concentration of silver ions is not known. The cell potential measured is 0.422 V. Determine the concentration of silver ions in the cell. [Given E_(Ag^(+)//Ag)^(@)=0.80,E_(Cu^(2+)//Cu)^(@)=+0.34 V]

Calculate the half cell potential at 25^@C for the cell reaction Cu^(2+)(aq)+2erarrCu , When [Cu^(2+)]=4M and E^@(Cu^(2+)//Cu)=0.34V .

What is the cell potential of the following cell ? Zn(s)|Zn^(2+)(1.0M)||Pb^(2+)(1.0M)|Pb(s) Given : E_(Pb^(2+)//Pb)^(@)=-0.12" V and " E_(Zn^(2+)//Zn)^(@)=-0.76" V"

E_(cell)^@ for Zn(s)+Pb^(2+) (1M ) to Zn^(2+) (1M) +Pb(s) is 0.66 volt. E_(cell) for the reaction Zn(s)+Pb^(2+) (0.1M) to Zn^(2+) (0.1M) +Pb(s) is

If the Zn^(2+) and Cu^(2+) concentrations are 0.1 M and 10^(-9) M respectively at 25^(@) C , the potential of the cell containing Zn//Zn^(2+) and Cu//Cu^(2+) electrodes is ___________. [Given E_(Zn//Zn^(2+))^(@)=+0.76, E_(Cu//Cu^(2+))^(@)=-0.34 V]

For the reaction Ni(s) + Cu^(2o+)(1M) rarr Ni^(2o+)(1M) + Cu (s), E^@ cell = 0.57 V DeltaG^@ of the reaction is