`Zn(s)|Zn^(2+)(aq)(0.1M)||Ag^+(aq)(0.01)|Ag(s)`
Given `E_(Zn^(2+)//Zn)^@ = -0.76, E_(Ag^(+)//Ag)^@ = 0.80V`
Determine `E_(cell)` , if your answer is `Xxx10^(-2)`V then determine value of X..

For Zn^(2+) //Zn, E^(@) =- 0.76 , for Ag^(+)//Ag, E^(@) = -0.799V . The correct statement is

Find E_(cell)^(@) for the cell : Zn | Zn^(2+)(1M) || Ag^(+)(1M) | Ag [Given that : E_(Zn//Zn^(2+))^(@)=0.76" V" , E_(Ag^(+)//Ag)^(@)=0.80" V" .

For Zn^(2+) //Zn, E^@ =- 0. 76 V , for Ag^+ //Af E^@ =0.799 V . The correct statement is .

Calculate Delta_(r)G^(@) and e.m.f. (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=96500C" "mol^(-1) OR (a) Define conductivity and molar conductivity for the solution of an electrolyte. Discuss their variation with concentration. (b) Calculation the standard cell potential of the galvanic cell in which the following reaction takes place: Fe^(2+)(aq)+Ag^(+)(aq)toFe^(3+)(aq)+Ag(s) Calculate the Delta_(r)G^(@) and equilibrium constant of the reaction also. (E_(Ag^(+)//Ag)^(@)=0.80,E_(Fe^(3+)//Fe^(2+))^(@)=0.77V)

For the cell : Zn (s) |Zn^(2+)(a M)||Ag^(o+)(bM)|Ag(s) . a. Write Nernst equation to show how E_(cell) vary with concentration of Zn^(2+) and Ag^(o+) ions. Given E^(c-)._((Zn^(2+)|Zn))=0.76V,E^(-)._((Ag^(o+)|Ag))=0.80V. b. Find E_(cell) for [Zn^(2+)]=0.01M and [Ag^(c-)]=0.02M . c. For what values of Q will the cell EMF be i. 0.0V" "ii. 0.97 V

What is the cell potential for following cell Zn(s)//Zn^(2+)(0.04M||Cu^(2+)(0.02M)//Cu(s) Given E_(Zn//Zn^(2+))^@ = -0.76V & E_(Cu//Cu^(2+))^@ = 0.34V