Hydrogen reacts with nitrogen monoxide to form dinitrogen monoxide (laughing gas) according to the equation: H2O(g) + 2NO(g) rightarrow O + H2O(g)NO (M) 0.30 0.60 0.60H2 (M) 0.35 0.35 0.70Rate (M/L/s) 3.822 x 103 1.529 x 10-2 3.058 x 10-2 A) Determine the rate law according to the following data. B) Determine the rate constant (in mol-2. L2. s-1).C) Determine the orders with respect to each reactant.

A.

B.

C. Second-order with respect to NO and first-order with respect to H₂

Explanation:

Hello,

In this case, for the reaction:

The rate law is determined by writing the following hypothetical rate laws:

Whereas we can compute m as follows:

Therefore, the reaction is second-order with respect to NO. Thus, for hydrogen, we find n:

A) Therefore, the reaction is first-order with respect to H₂. In such a way, we conclude that that the rate law is:

B) Rate constant is computed from one kinetic data:

C. As mentioned before, reaction is second-order with respect to NO and first-order with respect to H₂.

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