The initial rates of the reaction represented below were measured at \(298\text{ K}\) for several different initial concentrations of \(\text{NO}(g)\) and \(\text{Br}_2(g)\).

\[ 2\text{NO}(g) + \text{Br}_2(g) \rightarrow 2\text{NOBr}(g) \]

Trial	Initial \([\text{NO}]\) (\(\text{M}\))	Initial \([\text{Br}_2]\) (\(\text{M}\))	Initial rate of formation of \(\text{NOBr}\) (\(\text{M}\cdot\text{s}^{-1}\))
\(1\)	\(0.10\)	\(0.20\)	\(2.4 \times 10^{-3}\)
\(2\)	\(0.20\)	\(0.20\)	\(9.6 \times 10^{-3}\)
\(3\)	\(0.10\)	\(0.40\)	\(4.8 \times 10^{-3}\)

Based on the experimental data, what is the value of the rate constant, \(k\), for the reaction at \(298\text{ K}\)?