Final answer:
The rate law for the reaction H2(g) + 2NO(g) → N2O(g) + H2O(g) is second order in NO and first order in H2, making it third order overall. Without experimental data, the rate constant k cannot be accurately determined from the given options.
Step-by-step explanation:
To determine the rate constant (k) for the reaction H2(g) + 2NO(g) → N2O(g) + H2O(g), we need to look at the experimentally determined rate law. The given reaction has a rate law expressed as rate = k[NO]2[H2]. This indicates that the reaction is second order with respect to NO and first order with respect to H2. The overall order of the reaction is the sum of the individual orders, which is 3 (second order + first order).
While the question provides options for the rate constant value of k, without additional experimental data such as concentration, time, or actual rate of reaction, it would be impossible to accurately provide a definitive value for k. Therefore, based on the information provided, we cannot determine the correct rate constant from among the given options.