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12.12: Reaction Intermediate
https://chem.libretexts.org/Courses/Fullerton_College/Beginning_Chemistry_(Chan)/12%3A_Kinetics/12.12%3A_Reaction_Intermediate
\[\begin{align*} 2 \ce{NO} \left( g \right) &\rightarrow \cancel{\ce{N_2O_2} \left( g \right)} \\ \cancel{\ce{N_2O_2} \left( g \right)} + \ce{O_2} \left( g \right) &\rightarrow 2 \ce{NO_2} \left( g \r... $\begin{align*} 2 \ce{NO} \left( g \right) &\rightarrow \cancel{\ce{N_2O_2} \left( g \right)} \\ \cancel{\ce{N_2O_2} \left( g \right)} + \ce{O_2} \left( g \right) &\rightarrow 2 \ce{NO_2} \left( g \right) \\ \hline 2 \ce{NO} \left( g \right) + \ce{O_2} \left( g \right) &\rightarrow 2 \ce{NO_2} \left( g \right) \end{align*}\nonumber$ An intermediate is a species which appears in the mechanism of a reaction, but not in the overall balanced equation.

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