The formation of small amounts of nitric oxide, NO, in automobile engines is the first step in t

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The formation of small amounts of nitric oxide, NO, in...

The formation of small amounts of nitric oxide, $\mathrm{NO}$, in automobile engines is the first step in the formation of smog. As noted in Problem $14.56$, nitric oxide is readily oxidized to nitrogen dioxide by the reaction $$2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{NO}_{2}(g)$$ The following data were collected in a study of the rate of this reaction: What is the rate law for the reaction? What is the rate constant with its correct units?

The formation of small amounts of nitric oxide, $\mathrm{NO}$, in automobile engines is the first step in the formation of smog. As noted in Problem $14.56$, nitric oxide is readily oxidized to nitrogen dioxide by the reaction
$$2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{NO}_{2}(g)$$
The following data were collected in a study of the rate of this reaction:
What is the rate law for the reaction? What is the rate constant with its correct units?

Key Concepts

Experimental Determination of Kinetics

Experimental methods such as the initial rates method are used to determine the form of the rate law and the numerical value of the rate constant. By measuring how the reaction rate varies with differing initial reactant concentrations, the individual orders and the overall kinetics of the process can be established.

Rate Constant

The rate constant is a proportionality factor in the rate law that encapsulates the intrinsic reactivity of the chemical species and the effect of temperature. Its units depend on the overall order of the reaction so that the rate, which is generally expressed in terms of concentration per time, has the correct units.

Rate Law

The rate law is an empirical expression that relates the rate of a chemical reaction to the concentrations of its reactants. It typically takes the form rate = k[A]^m[B]^n, where k is the rate constant and m and n are the orders with respect to each reactant, respectively. This form is determined based on experimental observations and not simply by examining the stoichiometry of the reaction.

Reaction Order

The reaction order refers to the sum of the exponents in the rate law expression and indicates how sensitive the reaction rate is to changes in reactant concentrations. It is determined experimentally and helps in understanding the kinetics of the reaction, including which steps may be rate-limiting.

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