Calculate the equilibrium constant for the reactant at 298 K
Cu (s) `+ 2 Ag^(+) (aq) to Cu^(2+) (aq) + 2 Ag (s)`
Given that `E_((Ag^(+) |Ag))^(Theta) = 0.80 V ` and `E_((Cu^(2+) |Cu))^(Theta) = 0.34` V .

Explanation

`E_(cell)^(Theta)` is related to equilibrum constant `K_(e)` as : 298 K as:
`E_(cell)^(Theta) = (0.059)/(n) log K_(c) ` or `log K_(c) = (n E_(cell)^(Theta))/(0.059)`
`E_(cell)^(Theta) = E_((Ag^(+) | Ag))^(Theta) - E_((Cu^(2+) |Cu))^(Theta)`
`= 0.80 - 0.34 = 0.46` V
or log `K_(c) = (2 xx 0.46)/(0.059) = 15.59`
`therefore " " K_(c) = 3.92 xx 10^(15)` .