The kinetics of the reaction between nitrogen monoxide gas and oxygen gas were investigated at \(298\text{ K}\):

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

Initial rate data were collected across three experimental trials and recorded in the table below.

Trial	\([\text{NO}]_0\text{ (M)}\)	\([\text{O}_2]_0\text{ (M)}\)	Initial rate of reaction \(\text{(M}\cdot\text{s}^{-1}\text{)}\)
1	\(0.10\)	\(0.10\)	\(2.0 \times 10^{-3}\)
2	\(0.20\)	\(0.10\)	\(8.0 \times 10^{-3}\)
3	\(0.30\)	\(0.20\)	\(3.6 \times 10^{-2}\)

Based on the data in the table, which of the following is the correct rate law and specific rate constant, \(k\), for the reaction?