Calculate the value of the equilibrium constant of the following reaction at 298 K:
Given: `E_(Cu^(2+)|Cu)^(@)=+0.34V and E_(Cl_(2)|2Cl^(-))^(@)=+1.36V`

Calculate the value of equilibrium constant of the reaction occurring in Deniell cell at 25^(@)C . Given : E_(Zn^(2+)|Zn)^(@)=-0.76V and E_(Cu^(2+)|Cu)^(@)=+0.34V

Can Chlorine gas be stored in Copper Cylinder ? Given E_(Cu^(+)//Cu)^(@)= 0.34V and E_(Cl_(2)//Cl)^(@)= 1.36V

Calculate the equilibrium constant of the following reaction aty 298K. Cu(s)+2Ag^+(aq) rarr Cu^(2+)(aq)2Ag(s)~ Given E_(cell)^Theta=0.46V

Calculate the value of equilibrium constant for the reaction at 298 k. Cu(s) +2Ag^+(aq)rarrCu^(2+)(aq)+2Ag(s) E^@ (Ag2+/Ag) =0.80V and E^@( Cu2+/Cu ) =0.34V

Calculate Delta G^(Theta) and the equilibrium constant for the cell reaction , Cl_2 + 2 I^(-) to 2 Cl^(-) + I_(2) Given that E_((Cl_(2) , Cl^(-)))^(Theta) = 1.36 V , E_((I_(2) , I^(-)))^(Theta) = 0.536V

Calculate DeltaG^(Theta) and the equilibrium constant for the cell reaction : Cl_(2)+2I^(-) to 2Cl^(-) +I_(2) Given that E^(Theta)(Cl_(2), Cl^(-))=1.36V, E^(Theta)(I_(2)I^(-))=0.536V