Represent the cell in which the following reaction takes place.The value of `E^@` for the cell is 1.260 V. What is the value of Ecell ?
`2Al(s) + 3Cd^(2+) (0.1M) rarr 3Cd(s)+2Al^(3+) (0.01M)`

What is the value fo DeltaG^(@0 for the reactions? 2Al(s) + 3Cu^(2+)(aq) rightarrow + 3Cu(s) E^(@) = 2.02V

Represent the cell in which following reaction takes place : Mg(s)+2Ag^(o+)(0.0001M)rarr Mg^(2+)(0.130M)+2Ag(s) calculate its E_(cell) if E^(c-)._(cell)=3.17V.

Calculate the e.m.f. of the cell in which the following reaction takes place : Ni(s) +2Ag^(+)(0.002 M)to Ni^(2+)(0.160 M)+2Ag(s) Given E_(cell)^(@) =1.05 v

Calculate the standard cell potential of galvanic cell in which the following reaction take place : (Given E_(OP)^(@)Cr, Cd, Fe^(2+), Ag are 0.74V, 0.40V, -0.77V and -0.80V respectively) (a) 2Cr_((s))+3Cd_((aq.))^(2+) rarr 2Cr_((aq.))^(3+)+3Cd (b) Fe_((aq.))^(2+)+Ag_((aq.))^(+) rarr Fe_((aq.))^(3+)+Ag_((s)) Calculate the Delta_(r)G^(@) and equilibrium constant of the reactions.

Calculate the emf of the cell in which the following reaction takes place Ni(s) + 2Ag_((0.002M))^(+) rarr Ni_((0.160M))^(2+) + 2Ag_((s)) Given E_("Cell")^(@) = 1.07V

Calculate the standard cell potentials of the galvanic cells in which the following reactions take place. (a) " " 2Cr(s)+3Cd^(2+) to 2Cd^(3+)(aq)+3Cd(s) Given E_(Cr^(3+)//Cr)^(@)=-0.74" V" , E_(Cd^(2+)//Cd)^(@)=-0.40" V" (b) " " Fe^(2+)(aq)+Ag^(+)(aq) to Fe^(3+)(aq)+Ag(s) Gievn E_(Ag^(+)//Ag)^(@)=0.80" V" ,E_(Fe^(3+)//Fe^(2+))^(@)=0.77 " V" Also calculate DeltaG^(@) and equilibrium constant for the reaction.