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]`.

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]

It the reaction, 2Ag(s)+Fe^(2+)(aq)rarr2Ag^(+)(aq)+Fe(s) possible? Given : E_(Fe^(2+)|Fe)^(@)=-0.44V and E_(Ag^(+)|Ag)^(@)=+0.80V .

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.

Will Cu dissolve as Cu^(2+) in 1 (M) HCl solution? Will it do so in 1 (M) HNO_(3) solution? ["Given : "E_(Cu^(2+)|Cu)^(@)=+0.34 and E_(NO_(3)^(-)|NO)^(@)=+0.96]

Write down the appropriate Nernst equation for the following voltaic cell and calculate the e.m.f. of the cell at 298 K. Fe(s)|Fe^(2+)(0.002M)||Ag^(+)(0.02M)|Ag(s) ["Given, "E_(Fe^(2+)|Fe)^(@)=-0.44V and E_(Ag^(+)|Ag)^(@)=+0.80V" at 298K"]

Write cell reaction and calculate electrical work obtained from the following galvanic cell at standard condition . Mg|Mg^(2+)(aq)||Ag^(+)(aq)|Ag [Given : E_(Mg^(2+)|Mg)^(0) = -2.36 volt and E_(Ag^(+)|Ag)^(0) = 0.80 volt.]

Calculate the electrical work (at standard state) obtained from galvanic cell : Mg|Mg^(2+)(aq)||Ag^(+)(aq)|Ag Given : E_(Mg^(2+)|Mg)^(@)=-2.36V and E_(Ag^(2+)|Ag)^(@)=+0.80V

Determine DeltaG^(@) and the value of the equilibrium constant for the following reaction occurring in an electrochemical cell at 25^(@)C . Cu(s)+2Ag^(+)(aq)rarr Cu^(2+)(aq)+2Ag(s) Given that, E_(Cu^(2+)|Cu)^(@)=0.34V and E_(Ag^(+)|Ag)^(@)=0.80V

Which among the following vessels is used to store CuSO_(4) solution ? a Zn vessel [ Given E_(Zn^(2+)|Zn)^(@)=-0.76V, E_(Cu^(2+)|Cu)^(@)=+0.34V and E_(Ag^(+)|Ag)^(0)=0.80V ]

Why is the value of E_(Cu^(2+)|Cu)^(0)(+0.34V) positive ?