[" Q.15.Calculate "Delta_(r)" G'and log "K_(c)" for the following reaction: "],[qquad Cd^(+2)(aq)+Zn(s)longrightarrow Zn^(2+)(aq)+Cd(s)],[" Given: "E_(cd^(2+)t_(cd))=0.403V],[E_(Zn^(2)+/2n)=-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+) (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: Cd^(2+)+Zn(s)rarrZn^(2+)(aq)+Cd(s) If E_(Cd^(2+)|Cd)=-0.403V and E_(Zn^(2+)|Zn)=-.763V

Calculate Delta_(r)G^(@) and log K_(c) for the following reaction at 298 K. 2Cr_((s))+Cd_((aq))^(3+)+33Cd_((s)){Given :E^(@)""_(Cell")=+0.34V,IF=96500Cmol^(-1)]

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)]

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

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 ]