At 298 K, the equilibrium constant is 2 × 10^15 for the reaction: Cu ( s )+2 Ag^+( aq ) ⇌ Cu^2+( aq )+2 Ag ( s ) The equilibrium constant for the…

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