The following system obeys second-order kinetics. 2 NO2→NO3+NO NO3+CO→NO2+CO2 What

step 1 When we're given a mechanism for a reaction, which is what we are given in this problem, we can

The following system obeys second-order kinetics. 2...

The following system obeys second-order kinetics. \[ \begin{array}{l} 2 \mathrm{NO}_{2} \rightarrow \mathrm{NO}_{3}+\mathrm{NO} \\ \mathrm{NO}_{3}+\mathrm{CO} \rightarrow \mathrm{NO}_{2}+\mathrm{CO}_{2} \end{array} \] What is the rate law for this reaction? (A) rate $=k\left[\mathrm{NO}_{2}\right][\mathrm{CO}]$ (B) rate $=k\left[\mathrm{NO}_{2}\right]^{2}[\mathrm{CO}]$ (C) rate $=k\left[\mathrm{NO}_{2}\right]\left[\mathrm{NO}_{3}\right]$ (D) rate $=k\left[\mathrm{NO}_{2}\right]^{2}$

The following system obeys second-order kinetics.
\[
\begin{array}{l}
2 \mathrm{NO}_{2} \rightarrow \mathrm{NO}_{3}+\mathrm{NO} \\
\mathrm{NO}_{3}+\mathrm{CO} \rightarrow \mathrm{NO}_{2}+\mathrm{CO}_{2}
\end{array}
\]
What is the rate law for this reaction?
(A) rate $=k\left[\mathrm{NO}_{2}\right][\mathrm{CO}]$
(B) rate $=k\left[\mathrm{NO}_{2}\right]^{2}[\mathrm{CO}]$
(C) rate $=k\left[\mathrm{NO}_{2}\right]\left[\mathrm{NO}_{3}\right]$
(D) rate $=k\left[\mathrm{NO}_{2}\right]^{2}$

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Key Concepts

Elementary Reaction

An elementary reaction is a single step in a reaction mechanism that occurs in one event and in which the rate law can be directly derived from the stoichiometry of that step. In such reactions, the molecularity (i.e., the number of molecules colliding) directly determines the order of that step.

Reaction Mechanism

A reaction mechanism is the sequence of elementary steps by which a chemical reaction occurs. Understanding the mechanism is crucial because it helps in deriving the rate law, especially when intermediates are formed. The mechanism shows how the kinetics of the overall reaction can be influenced by the slow (rate-determining) step or by steady-state levels of reactive intermediates.

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 by the specific steps of a reaction mechanism rather than merely the overall stoichiometric equation, and it indicates how the reaction rate depends on the concentrations involved.

Reaction Order

Reaction order refers to the sum of the exponents of the concentration terms in the rate law. For a reaction that is second order overall, the combined powers on the reactant concentrations add up to two, which directly affects how changes in concentration influence the reaction rate.

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