Calculate the standard cell potentials of the galvanic cells in which the following reactions take place :
`2Cr(s)+3Cd^(2+)(aq)rarr 2Cr^(3+)(aq)+3Cd`
Calculate `Delta_(r )G^(0)`, equilibrium constant of the reactions.

Calculate the standard cell potentials of the galvanic cells in which the following reactions take place : Fe^(2+)(aq)+Ag^(+)(aq)rarr Fe^(3+)(aq)+Ag(s) Calculate Delta_(r )G^(0) , equilibrium constant of the reactions.

Calculate the standard cell potential of the Galvanic cell in which the following reaction takes place: 2Cr(s) + 3Cd^(2+)(aq) rarr 2Cr^(3+)(aq) + 3Cd(s) . Also calculate the Delta_rG and equilibrium constant of the reaction.

Calculate the standard cell potential of a galvanic cell in which the following reaction takes place 2Cr(s) + 3Cd^(2+) ( aq) rarr 2Cr^(3+) ( aq) + 3Cd(s) Calculate Delta_( r) G^(@) and equilibrium constant K of the above reaction at 25^(@)C . [Given, E_(Cr^(3+) //Cr)^(@) = - 0.74 V, E_(Cd^(2+)//Cd)^(@) = - 0.40V, 1F = 96500 C "mol"^(-1)]

Calculate the standard cell potential of the Galvanic cell in which the following reaction takes place: Fe^(2+)(aq) + Ag^+(aq) rarr Fe^(3+)(aq) + Ag(s) . Calculate the Delta_rG and equilibrium constant of the reactions.

Calculate the standard cell potential of the galvanic cell in which the following reaction takes place: Fe%(2+)(aq)+Ag^(+)(aq)rarrFe^(3+)(aq)+Ag(s) Calculate the Delta_(r)G^(@) and equilibrium constant of the reaction also. (E_(Ag^(+)|Ag)^(@)=0.80V, E_(Fe^(3+)|Fe^(2+))^(@)=0.77V)

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)

Calculate the standard cell potential of the Galvanic cell in which the following reaction takes place: 2Cr(s) + 3Cd^(2+)(aq) rarr 2Cr^(3+)(aq) + 3Cd(s) Also calculate the DeltarG^@ value of the reaction. (Given: E_(Cr^(3+)//Cr) = -0.74V , E_(Cd^(2+)//Cd) = -0.40V and F =96500C//mol )

Calculate the standard cell potential of the galvanic cell in which the following reaction takes place: 2Cr(s)+3Cd^(2+)(aq)to2Cr^(3+)(aq)+3Cd(s) Also calcuate the triangle_(r)G^(ɵ) value of the reaction (given E_(cr^(3+)//Cr)^(ɵ)=-0.74V,E_(Cd^(3+)//Cd)^(ɵ)=-0.40V and F=96500Cmol^(-1)