At \(400\text{ K}\), the equilibrium constant \(K_c\) for the reaction represented below is \(5.0\).

\[\text{CO(g)} + \text{Cl}_2\text{(g)} \rightleftharpoons \text{COCl}_2\text{(g)}\]

A student injects \(0.20\text{ mol}\) of \(\text{CO(g)}\), \(0.20\text{ mol}\) of \(\text{Cl}_2\text{(g)}\), and \(0.40\text{ mol}\) of \(\text{COCl}_2\text{(g)}\) into an evacuated, rigid \(1.0\text{ L}\) container at \(400\text{ K}\). Which of the following correctly predicts the direction the reaction will proceed to reach equilibrium, and provides the correct justification?