At 298K, the equilibrium constant is $2\times {10}^{-1}$ for the reaction: ${\mathrm{Cu}}_{\left(\mathrm{s}\right)}+2{{\mathrm{Ag}}^{+}}_{\left(\mathrm{aq}\right)}\underset{ }{\overset{ }{\rightleftharpoons }} {{\mathrm{Cu}}^{2+}}_{\left(\mathrm{aq}\right)}+2{\mathrm{Ag}}_{\left(\mathrm{s}\right)}$
 The equilibrium constant for the reaction

$\frac{1}{2}{\mathrm{Cu}}_{\left(aq\right)}^{2+}+{\mathrm{Ag}}_{\left(s\right)}\rightleftharpoons \frac{1}{2}{\mathrm{Cu}}_{\left(s\right)}+{\mathrm{Ag}}_{\left(aq\right)}^{+}$

is x$\times$10^-8. The value of x is ______.(Nearest Integer)