Phosgene, \(\text{COCl}_2(g)\), decomposes at elevated temperatures according to the following equation:

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

A student places \(1.6\text{ mol}\) of pure \(\text{COCl}_2(g)\) into a rigid, evacuated \(4.0\text{ L}\) container at \(400\text{ K}\). At this temperature, the equilibrium constant for the reaction is \(K_c = 1.0 \times 10^{-5}\). What is the equilibrium concentration of \(\text{CO}(g)\) in the container?