The gas-phase synthesis of nitrosyl chloride proceeds according to the balanced chemical equation below:

\[ 2\,\text{NO(g)} + \text{Cl}_2\text{(g)} \rightarrow 2\,\text{NOCl(g)} \]

Under a specific set of reaction conditions, the experimentally determined rate law is:

\[ \text{Rate} = k\,[\text{NO}]^2\,[\text{Cl}_2] \]

In an initial trial, the reaction begins with initial concentrations \([\text{NO}]_1\) and \([\text{Cl}_2]_1\), yielding an initial rate of \(r_1\). In a second trial conducted at the same temperature, the initial concentration of \(\text{NO(g)}\) is increased by a factor of \(1.50\) (such that \([\text{NO}]_2 = 1.50\,[\text{NO}]_1\)) while the initial concentration of \(\text{Cl}_2\text{(g)}\) is decreased by half (such that \([\text{Cl}_2]_2 = 0.500\,[\text{Cl}_2]_1\)). Which of the following expressions correctly represents the initial reaction rate, \(r_2\), in the second trial in terms of \(r_1\)?