At \( 298 \, \text{K} \), the equilibrium constant is \( 2 \times 10^{15} \) for the reaction:
\( \mathrm{Cu(s)} + 2\mathrm{Ag^+(aq)} \rightleftharpoons \mathrm{Cu^{2+}(aq)} + 2\mathrm{Ag(s)} \)
The equilibrium constant for the reaction \( \dfrac{1}{2}\mathrm{Cu^{2+}(aq)} + \mathrm{Ag(s)} \rightleftharpoons \dfrac{1}{2}\mathrm{Cu(s)} + \mathrm{Ag^+(aq)} \) is \( x \times 10^{-8} \). The value of \( x \) is _______________. (Nearest Integer)
