For the cell `Cu//Cu^(2+)//Hg^(2+)//Hg`, `E_(cell)^(6) = 0.45 V`. Find the standard reduction potential of `Hg^(2+)//Hg` electrode. Given `E^@ cu^(2+)//cu = 0.34`.

For the cell, Cu|Cu^(2+)||Hg^(2+)|Hg, E_("cell")^(@)=+0.45V . Find the standard reduction potential of Hg^(2+)|Hg electrode. Given : 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?

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

The positive value of the standard electrode potential of Cu^(2+)|Cu indicates that -

For the given cell, Mg|Mg^(2+)||Cu^(2+)|Cu -

Consider the galvanic cell Cu|Cu^(2+)(0.13M)||Ag^(+)(0.01M)|Ag (i) Calculate the reduction potential of each electrode and EMF of the cell (ii) Is is reaction representing the cell spontaneous ? ["Given : "E_(Cu^(2+)|Cu)^(@)=+0.34V and E_(Ag^(+)|Ag)^(@)=+0.80V]

Determine reduction potential of the given electrode reaction at 25^(@)Cl Cu^(2+)(0.1M, aq)+2erarrCu(s). The standard reduction potential of Cu^(2+)|Cu system =+0.34V .

In the cell Zn//Zn^(2+)//Cu^(2+)//Cu the negative terminal is.

Which one of Sn, Cu, Cr, Al can reduce Fe^(2+) ion in aqueous medium? Explain. The standard reduction potential of Sn^(2+)|Sn, Cu^(2+)|Cu, Al^(3+)|Al, Cu^(3+)|Cr and Fe^(2+)|Fe electrodes are -0.14,+0.34, -1.66, -0.74 and -0.44V repectively.

For the galvanic cell, Cu|Cu^(2+)(0.13M)||Ag^(+)(0.01M)|Ag (ii) Is the cell reaction spontaneous ? ["Given : "E_(Cu^(2+)|Cu)^(@)=+0.34V and E_(Ag^(+)|Ag)^(@)=+0.80V] .