At $298 \ K$,the $K_c$ of the reaction $Cu(s) + 2Ag^+(aq) \rightleftharpoons Cu^{2+}(aq) + 2Ag(s)$ is $3.0 \times 10^{14}$. In a reaction mixture at a certain temperature,$[Cu^{2+}] = 1.8 \times 10^{-2} \ M$ and $[Ag^+] = 3.0 \times 10^{-9} \ M$. Is this reaction in equilibrium? In which direction will the reaction proceed?

(B) The reaction quotient $Q_c$ is calculated as: $Q_c = \frac{[Cu^{2+}]}{[Ag^+]^2} = \frac{1.8 \times 10^{-2}}{(3.0 \times 10^{-9})^2} = \frac{1.8 \times 10^{-2}}{9.0 \times 10^{-18}} = 2.0 \times 10^{15}$.
Since $Q_c = 2.0 \times 10^{15}$ and $K_c = 3.0 \times 10^{14}$,we observe that $Q_c > K_c$.
Because $Q_c > K_c$,the reaction is not in equilibrium.
Since $Q_c > K_c$,the reaction will proceed in the reverse direction to reach equilibrium.