Calculate the equilibrium constant for the following reaction at 298 K:
`Cu(s) + Cl_(2) (g) to CuCl_(2) (aq)`
Given: `R =8.314 J K^(-1) mol^(-1) , E_(Cu^(2+)//Cu)^(@) = 0.34 V, E_(1/2Cl_(2)//Cl^(-))^(@) =1.36 V, 1 F = 96500 C mol^(-1)`

Explanation

`E_("cell")^(@) =E_(1/2Cl_(2)//Cl^(-))^(@) - E_(Cu^(2+)//Cu)^(@) = +1.36 V - 0.34 V = 1.02 V`
Applying the following relation and substituting the values, we get
`log K = (nE^(@))/(0.0591) = (2 xx 1.02)/(0.0591) = 2.04/(0.0591) = 34.5177`
K = Antilog `34.5177 = 3.294 xx 10^(34)`
Thus, equilibrium constant `=3.294 xx 10^(34)`