Calculate the standard cell potential of galvanic cell in which the following reaction takes place
`2Cr_(s)+3Cd_(aq)^(+2)rarr2cr_(aq)^(+3)+3Cd_(s)`
Given `E_(Cr^(+3)//Cr)=-0.74(V)E^(@)_(Cd^(+2)//Cd)=-0.04(V)`

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.

Calculate the standard cell potentials of galvanic cell in which the following reactions take place 2Cr_((s)) + 3Cd_((aq))^(2+)rarr 2Cr_(aq)^(3+) + 3Cd E_(Cr)^@ = -0.740 V, E_(Cd)^@ = -0.403 V, Calculate the Delta_rG^@ and equilibrium constant of the reactions.

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 potentials of galvanic cell in which the following reactions take place : a. Cr(s) +3Cd^(2+)(aq) rarr 2Cr^(3+)(aq)+3Cd b. Fe^(2+)(aq)+Ag^(o+)(aq)rarr Fe^(3+)(aq)+Ag(s) Calculate the Delta_(r)G^(@) and equilibrium constant of the reactions .

Calculate the standard cell potentials of galvanic cell in which the following reactions take place. (i) 2Cr(s) + 3Cd^(2+)(aq) to 2Cr^(3+) (aq) + 3Cd (ii) Fe^(2+)(aq) + Ag^(+)(aq) to Fe^(3+)(aq) + Ag(s) Calculate the ΔrG and equilibrium constant of the reactions.