Nitric oxide reacts hydrogen to give nitrogen and water(2no+2h2_n2+2h2o).the kinetics of this rxn is explained byfollowing zteps:(1)2no+h2_n2+h2o2(slow)( 2) h2o2+h2_2h2o(fast).

To better understand the kinetics of the reaction between nitric oxide (NO) and hydrogen (H2) to form nitrogen (N2) and water (H2O), we can examine the given reaction steps:

(1) 2NO + H2 ⟶ N2 + 2H2O (slow)
(2) H2O2 + H2 ⟶ 2H2O (fast)

The first step is the slow step, which means that it is the rate-determining step of the overall reaction. This step involves the reaction of two NO molecules with one H2 molecule to produce one N2 molecule and two H2O molecules.

The second step is the fast step, which means it occurs relatively quickly compared to the slow step. In this step, hydrogen peroxide (H2O2) reacts with hydrogen (H2) to form two water (H2O) molecules.

The overall reaction can be thought of as the combination of these two steps:

2NO + H2 ⟶ N2 + 2H2O2 (slow)
H2O2 + H2 ⟶ 2H2O (fast)

To determine the overall rate of the reaction, we need to look at the rate-determining step (slow step). The rate of the reaction will be directly proportional to the concentration of the reactants involved in this step.

The rate law for the given reaction can be expressed as:

Rate = k[NO]^2[H2]

Here, k is the rate constant and [NO] and [H2] represent the concentrations of nitric oxide and hydrogen, respectively.

By studying the kinetic behavior of this reaction, scientists can determine the rate constant (k) and understand how factors such as temperature and concentration affect the rate of the reaction.

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