The `E^@` values corresponding to the following two reduction electrode processes are:
`Cu^(+)|Cu=0.52V`
`Cu^(2+)|Cu)=0.16V`
Formulate the galvanic cell for their combination calculate the cell potential and `Delta_rG^@` for the cell reaction.

Write each half cell reaction of the following electrochemical cell: Cu(s)|Cu^(2+)(1M)||Ag^(+)(1M)|Ag(s)

Calculate the EMF of the cell, containing nickel and copper electrodes. Given E^@(NI^(2+)|NI)=-0.25V and E^@(Cu^(2+)|Cu)=+0.34V .

Write the Nernst equation for the above cell, if E^@(Zn^(2+)|Zn)=-0.76V, E^@(Cu^(@+)|Cu)=+0.34V

1 M solution each of Cu(NO_3)_2 , AgNO_3 , Hg(NO_3)_2 and Mg(NO_3)_2 is electrolysed using Pt electrons. The values of standard reduction electrode potentials in volts are: Ag^+|Ag=+0.80V, Cu^(2+)|Cu=+0.34V Hg^(2+)|Hg=+0.79V, Mg^(2+)|Mg=-2.37V The sequence of deposition of metals on the cathode will be

Write Nernst equation and cell reaction of the following cell: Zn|Zn^(2+)||Cu^(2+)|Cu

Write the half cell reaction and the overall cell reaction for the electrochemical cell: Zn|Zn^(2+)(1.0M)||Pb^(2+)(1.0M)|Pb Calculate the standard e.m.f. for the cell if standard electrode potentials for Pb^(2+)|Pb and Zn^(2+)|Zn electrodes are -0.126V and -0.763V respectively.

Calculate the potential of the following cell reaction at 298K: Sn^(4+)(1.50M)+Zn(s)rarrSn^(2+)(0.5M)+zn^(2+)(2.0M) The standard potential of the cell is 0.89V, will the potential of the cell will increase or decrease if the concentration of Sn^(2+) is increased in the cell?

Represent the cell in which the following reaction takes place: Mg(s)+Cu^(2+)(0.0001M) to Mg^(2+)(0.1M)+Cu(s) . Calculate its E, if E^(@) is 2.71V .