A complex reaction takes place in two steps:

i) $\mathrm{NO(g) + O_3(g) \longrightarrow NO_3(g) + O(g)}$

ii) $\mathrm{NO_3(g) + O(g) \longrightarrow NO_2(g) + O_2(g)}$

The predicted rate law is rate = $k$[NO][O$_3$]. Identify the rate determining step. Write the overall reacti

Question

A complex reaction takes place in two steps:

i) $\mathrm{NO(g) + O_3(g) \longrightarrow NO_3(g) + O(g)}$

ii) $\mathrm{NO_3(g) + O(g) \longrightarrow NO_2(g) + O_2(g)}$

The predicted rate law is rate = $k$[NO][O$_3$]. Identify the rate determining step. Write the overall reaction. Which is the reaction intermediate? Why?

Accepted Answer

**Step 1.** The two steps are: (i) NO(g)+O3(g) -> NO3(g)+O(g); (ii) NO3(g)+O(g) -> NO2(g)+O2(g).
**Step 2.** The predicted (observed) rate law is rate = k[NO][O3], which matches the stoichiometry of step (i) exactly (one NO, one O3). This confirms step (i) is the slow, rate-determining step.
**Step 3.** Adding steps (i) and (ii): NO+O3+NO3+O -> NO3+O+NO2+O2. Cancelling the species NO3 and O that appear on both sides gives the overall reaction NO(g)+O3(g) -> NO2(g)+O2(g). …

Q.A complex reaction takes place in two steps:

Concept understanding — Molecularity

Q.A complex reaction takes place in two steps:

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