Calculate the equilibrium constant of the reaction:
`Cu_((s))+2Ag_((ag))^(+)toCu_((aq))^(2+)+2Ag_((s))" "[E_(cell)^(Theta)=0.46V]`

Explanation

Electron change in this reaction =2=n
`E_((cell))^(Theta)=0.46V`
`K_(C)=`equilibrium constant
`E_((cell))^(Theta)=(0.059V)/(n)"log "K_(C)=0.46V`
`therefore logK_(C)=(0.46Vxx2)/(0.059)=15.5932`
`therefore K_(C)=`Antilog 15.5932
`=3.9194xx10^(15)=3.92xx10^(15)`.