Calculate `DeltaG^@` in `kJmol^(2+)` and equilibrium constant for the following cell reaction: `Zn(s)+Cu^(2+)(aq)harrCu(s)+Zn^(2+)(aq)` [Give: E_(Zn^(2+)//Zn)^@=-0.76 V, E_(Cu^(2+)//Cu)^@=+0.34V,F=96500 C mol^(-1)]`

Calculate the value of equilibrium constant of the reaction occurring in Deniell cell at 25^(@)C . Given : E_(Zn^(2+)|Zn)^(@)=-0.76V and E_(Cu^(2+)|Cu)^(@)=+0.34V

Calculate Delta_(r)G^(@) and emf (E) that can be obtained from the following cell under the standard conditions at 25^(@)C? Zn(s)|Zn^(2+)(aq)||Sn^(2+)(aq)|Sn(s) ["Given : "E_(Zn^(2+)|Zn)^(@)=-0.76V , E_(Sn^(2+)|Sn)^(@)=-0.14V and F="96500 C.mol."^(-1)]

Calculate the EMF of the electrochemical cell for which the following cell reaction is given below- Zx(S) + ni^(2_+)(aq) rarr Zn^(+2)(aq) + Ni(S) Given E_(zn^2//zn)^@ = - 0.76 V E_(Ni^(2+) // Nl) = - 0.25 V.

Calculate the equilibrium constant of the reaction : Cu(s)+2Ag^(+)(aq)rarr Cu^(2+)(aq)+2Ag(s): E_("cell")^(@)=0.46V

Find the equilibrium constant for the reaction: Cu^(2+)+In^(2+)hArr Cu^(+)+In^(3+) Given : E_(Cu^(2+)|Cu^(+))^(@)=0.15V, E_(In^(2+)|In^(+))^(@)=-0.4V, E_(In^(3+)|In^(+))^(@)=-0.42V

Calculate the value of the equilibrium constant of the following reaction at 298 K: Given: E_(Cu^(2+)|Cu)^(@)=+0.34V and E_(Cl_(2)|2Cl^(-))^(@)=+1.36V

Determine the maximum amount of work that can be derived from the cell, Zn|Zn^(2+)(1M)||Cu^(2+)(1M)|Cu. Given : E_(Zn^(2+)|Zn)^(@)=-0.76V and E_(Cu^(2+)|Cu)^(@)=+0.34V

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

Determine DeltaG^@ and the value of the equlibrium 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)^@=0.34 V and E_(Ag^+//Ag)^@ =0.80V

Calculate Delta_(r)G^(@) for the reaction Mg(s)+Cu^(2+)(aq)rarrMg^(2+)(aq)+Cu(s) Given : E_("cell")^(@)=+2.71V, 1F = "96500 C.mol"^(-1)