The equillibrium constant for thefollowing general reaction is `10^(30)`. Calculate `E^(@)` for the cell at 298 K.
`2X_(2)(s)+3Y^(2+)(aq)to2X_(2)^(3+)(aq)+3Y(s)`

The equilibrium constant for the following general reaction is 10^(@). Calculate E^(@) for the cell at 298 K. 2X_2(s) + 3Y^(2+)(aq) to 2X_(2)^(3+)(aq) + 3Y (s)

The equilibrium constant for the reaction Cu_(s) + 2Ag^+ _ (aq) rarr Cu^2+ _ (aq) +2Ag at 298 k is Given E^@cell=0.46v

The equilibrium constant of the reaction : Zn(s)+2Ag^(+)(aq)toZn(aq)+2Ag(s),E^(@)=1.50V at 298 K is

The equilibrium constant of the reaction : Zn(s)+2Ag^(+)(aq)toZn(aq)+2Ag(s),E^(@)=1.50V at 298 K is

The equilibrium constant of the reaction; Cu(s)+2Ag + (aq)⟶Cu 2+ (aq)+2Ag(s) E o =0.46V at 298K

Calculate the equilibrium constant for the reaction 2Fe3+(aq) + 2I– (aq) → 2Fe2+(aq) + I2(s) E0cell = 0.236V

Answer any three of the following questions. b. Calculate the value of Delta r G^(0) at 298K for the cell reaction 3Mg(s) + 2AI^(+3) to 3Mg^(+) (aq) + 2AI(s)

The equilibrium constant for the reaction : Fe^(3+)(aq)+SCN^(-)(aq)hArr Fe SCN^(2+)(aq) is 140 at 298 K. The equilibrium constant for the reaction : 2Fe^(3+)(aq)+2SCN^(-)(aq)hArr 2Fe SCN^(2+)(aq) is :

The equivalent constant of the reaction: Cu(s)+2Ag^(+)(aq.) rarr Cu^(2+)(aq.)+2Ag(s) E^(@)=0.46 V at 298 K ,is: