A rigid, sealed \(1.0 \text{ L}\) reaction vessel contains a mixture of \(\text{NO(g)}\) and \(\text{O}_2\text{(g)}\) at a constant temperature. The system reacts and reaches equilibrium according to the balanced equation below:

\[ 2\,\text{NO(g)} + \text{O}_2\text{(g)} \rightleftharpoons 2\,\text{NO}_2\text{(g)} \]

The initial and equilibrium concentrations of the species are recorded in the table below:

Species	Initial Concentration (M)	Equilibrium Concentration (M)
\(\text{NO(g)}\)	\(0.60\)	\(?\)
\(\text{O}_2\text{(g)}\)	\(0.40\)	\(?\)
\(\text{NO}_2\text{(g)}\)	\(0.00\)	\(0.40\)

Based on the data, what is the numerical value of the equilibrium constant, \(K_c\), for the reaction at this temperature?