[" 28.Calculate "_(1)G^(0)" and log "K_(c)" for the following reaction: "],[Cd^(2+)(aq)+Zn^(2)(aq)rarr Zn^(2+)(aq)+Cd(s)],[" Given: "E^(0)cd^(2+)|cd=-0.403V],[E^(0)/m^(2+)|zn=-0.763V]

Calculate Delta ,G^@ and log K_c for the following reation: Cd^(+2)(aq)+Zn^(2+)(aq)+Cd(s) Given : E_(cd^(2+)//cd)^(0)=0.403 V E_(Zn^2+//Zn)^(0)=0.763 V

Calculate Delta ,G^@ and log K_c for the following reation: Cd^(+2)(aq)+Zn^(2+)(aq)+Cd(s) Given : E_(cd^(2+)//cd)^(0)=0.403 V E_(Zn^2+//Zn)^(0)=0.763 V

Calculate the equilibrium constant for the reaction: Cd^(2+)+Zn(s)rarrZn^(2+)(aq)+Cd(s) If E_(Cd^(2+)|Cd)=-0.403V and E_(Zn^(2+)|Zn)=-.763V

Write cell representation for following cells Cd^(2+)(aq)+Zn(s)toZn^(2+)(aq)+Cd(s)

Calculate the equilibrium constant for the reaction: Cd^(2+) (aq) +Zn(s) hArr Zn^(2+) (aq) +Cd (s) If E_(Cd^(2+)//Cd)^(Theta) = -0.403V E_(Zn^(2+)//Zn)^(Theta) = -0.763 V

Calculate the equilibrium constant for the reaction : Fe(s)Cd^(2+)(aq)harrFe^(2+)(aq)+Cd(s) ("Given" E_(cd^(2+)//Cd)^(@)=-0.40 V, E_(Fe^(2+)//Fe)^(@)=-0.44 V)

Calculate the equilibrium constant for the reaction. Fe(s) + Cd^(2+) (aq) hArr Fe^(2+)(aq) + Cd(s) [ Given, E_(Cd^(2+) //Cd)^(@) = - 0.40V , E_(Fe^(2+)//Fe)^(@) = - 0.44 V ]

Calculate DeltaG^@ in kJmol^(2+) and equilibrium constant for the following cell reaction: Zn(s)+Cu^(2+)(aq)harrCu(s)+Zn^(2+)(aq) [Give: E_(Zn^(2+)//Zn)^@=-0.76 V, E_(Cu^(2+)//Cu)^@=+0.34V,F=96500 C mol^(-1)]

Calculate the equilibrium constant for the reaction at 298 K Zn(s)+Cu^(2+)(aq)harr Zn^(2+)(aq)+Cu(s) Given " " E_(Zn^(2+)//Zn)^(@)=-0.76 V 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