Calculate equilibrium constant for the reaction :
`Mg(s) |Mg^(2+)(0.001 M) || Cu^(2+)(0.0001 M)|Cu(s)`
Given `E_((Mg^(2+)//Mg))^(@)=-2.37" V " , E_((Cu^(2+)//Cu))^(@)=0.34" V "`

Calculate emf and DeltaG for the following reaction at 298 K Mg(s)|Mg^(2+)(0.01 M)||Ag^(+)(0.0001 M)|Ag(s) Given E_((Mg^(2+)//Mg))^(@)=-2.37" V ", E_((Ag^(+)//Ag))^(@)=+0.80" V "

Find the e.m.f. of the cell, Mg(s)//Mg^(2+)(0.01 M) || Cu^(2+)(aq)(0.0001 M)//Cu(s) "Given" E_(Mg^(2+)//Mg)^(@)=-2.37 " volts" , E_(Cu^(2+)//Cu)^(@)=+0.34" volts" .

Calculate e.m.f. of cell for the reaction : Mg_((s))+Cu^(2+)"(0.0001 M)"rarr Mg^(2+)"(0.001 M)"+Cu_((s)) Given that : E_(Mg^(2+)//Mg)^(@)=-2.37V E_(Cu^(2+)//Cu)^(@)=+0.34V

Calculate the equilibrium constant for the reaction at 298K. Zn(s) +Cu^(2+)(aq) hArr Zn^(2+)(aq) +Cu(s) Given, E_(Zn^(2+)//Zn)^(@) =- 0.76V and E_(Cu^(2+)//Cu)^(@) = +0.34 V

Calculate the equilibrium constant for the reaction at 298K. Zn(s) +Cu^(2+)(aq) hArr Zn^(2+)(aq) +Cu(s) Given, E_(Zn^(2+)//Zn)^(@) =- 0.76V and E_(Cu^(2+)//Cu)^(@) = +0.34 V

Calculate the equilibrium constant for the reaction at 298K. Zn(s) +Cu^(2+)(aq) hArr Zn^(2+)(aq) +Cu(s) Given, E_(Zn^(2+)//Zn)^(@) =- 0.76V and E_(Cu^(2+)//Cu)^(@) = +0.34 V

Calculate the equilibrium constant for the reaction at 298K. Zn(s) +Cu^(2+)(aq) hArr Zn^(2+)(aq) +Cu(s) Given, E_(Zn^(2+)//Zn)^(@) =- 0.76V and E_(Cu^(2+)//Cu)^(@) = +0.34 V

Calculate emf of the following cell reaction at 2968 K : Ni(s)//Ni^(2+)(0.01 M) || Cu^(2+)(0.1 M)//Cu(s) [Given E_(Ni^(2+)//Ni)^(@)=-0.25" V ",E_(Cu^(2+)//Cu)^(@)=+0.34 " V " ] Write the overall cell reaction.