Calculate the equilibrium constant for the reaction at 298K
`Cu(s)+Cl_(2)(g)toCuCl_(2)(aq)`
Given that
`R=8.314JK^(-1)mol^(-1)`,
`E^(@)Cu^(2+)//Cu=0.34V`,
`E^(@)(1)/(2)Cl_(2)//Cl^(-)=1.36V`
`F=96500C" "mol^(-1)`

Explanation

Cell reactions are
Oxidation: `Cu(s)toCu^(2+)(aq)+2e^(-)`
Reduction: `Cl_(2)(aq)+2e^(-) to 2Cl^(-)(aq)`
Overall: `Cu(s)+Cl_(2)(g)toCu^(2+)(aq)+2Cl^(-)(aq)`
Here, n=2
Cell representation is,
`Cu|Cu^(2+)||Cl^(-)|Cl_(2),Pt`
`EMF^(@)=E_(R)^(@)-E_(L)^(@)`
`=E_(1//2Cl_(2)//Cl^(-))^(@)-E_(Cu^(2+)//Cu)^(@)`
`=(1.36-0.34)V=1.02V`
`EMF=EMF^(@)-(0.0591V)/(n)logQ_(C)`
At eqn. EMF=0 and `Q_(C)=K_(C)`
`therefore logK_(C)=(EMF^(@)xxn)/(0.0591V)=((1.02V)xx2)/(0.0591V)`
`=(2.04)/(0.0591)=34.5178`
`K_(C)`=antilog `34*5178`
`=3.295xx10^(34)`