The oxidation of NO (released in small amounts in the...

The oxidation of $\mathrm{NO}$ (released in small amounts in the exhaust of automobiles) produces the brownish-red gas $\mathrm{NO}_{2}$, which is a component of urban air pollution. $$2 \mathrm{NO}+\mathrm{O}_{2} \longrightarrow 2 \mathrm{NO}_{2}$$ The rate law for the reaction is rate $=k[\mathrm{NO}]^{2}\left[\mathrm{O}_{2}\right] . \mathrm{At}$ $25^{\circ} \mathrm{C}, k=7.1 \times 10^{9} \mathrm{~L}^{2} \mathrm{~mol}^{-2} \mathrm{~s}^{-1}$. What would be the rate of the reaction if $[\mathrm{NO}]=0.0010 \mathrm{~mol} \mathrm{~L}^{-1}$ and $\left[\mathrm{O}_{2}\right]$ $=0.034 \mathrm{~mol} \mathrm{~L}^{-1} ?$

The oxidation of $\mathrm{NO}$ (released in small amounts in the exhaust of automobiles) produces the brownish-red gas $\mathrm{NO}_{2}$, which is a component of urban air pollution.
$$2 \mathrm{NO}+\mathrm{O}_{2} \longrightarrow 2 \mathrm{NO}_{2}$$
The rate law for the reaction is rate $=k[\mathrm{NO}]^{2}\left[\mathrm{O}_{2}\right] . \mathrm{At}$ $25^{\circ} \mathrm{C}, k=7.1 \times 10^{9} \mathrm{~L}^{2} \mathrm{~mol}^{-2} \mathrm{~s}^{-1}$. What would be the
rate of the reaction if $[\mathrm{NO}]=0.0010 \mathrm{~mol} \mathrm{~L}^{-1}$ and $\left[\mathrm{O}_{2}\right]$
$=0.034 \mathrm{~mol} \mathrm{~L}^{-1} ?$

Key Concepts

Rate Law

The rate law is an expression that relates the rate of a chemical reaction to the concentrations of its reactants. It is determined empirically and takes the form rate = k[A]^m[B]^n, where k is the rate constant, and m and n are the orders of the reaction with respect to the individual reactants. This concept helps us predict how variations in concentration affect the reaction speed.

Reaction Order

Reaction order refers to the exponent of a reactant concentration in the rate law and indicates the dependency of the reaction rate on that concentration. The overall order of a reaction is the sum of the individual orders and provides insight into how the reaction rate responds to changes in the concentrations of all reactants combined.

Rate Constant

The rate constant, represented by k, is a proportionality factor in the rate law that is specific to a given reaction at a particular temperature. It incorporates factors like temperature and activation energy, and its units vary based on the overall order of the reaction. The rate constant quantitatively determines the speed of the reaction under set conditions.

Calculation of Reaction Rate

Calculating the reaction rate involves substituting the given reactant concentrations and the rate constant into the rate law expression. This process allows one to determine the speed at which the reactants are converted to products, and is fundamental in assessing the kinetics of a chemical reaction.

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