Consider the reaction 2NO2(.g.)+O3(.g.) arrow N2O5(.g.)+O2(.g.) The reaction of nitrogen dioxide and ozone represents is first order in NO2(.g.) and in O3(.g.) . Which of these possible reaction mechanism is consistent with the rate law?

Question

Consider the reaction 2NO2(.g.)+O3(.g.) arrow N2O5(.g.)+O2(.g.) The reaction of nitrogen dioxide and ozone represents is first order in NO2(.g.) and in O3(.g.) . Which of these possible reaction mechanism is consistent with the rate law? <img class="img-fluid question-image" alt="image" src="https://cdn.tardigrade.in/img/question/chemistry/68551bc82529bf54183be5073e03bdc6-.png" /> (A) Only I (B) Only II (C) Both I and II (D) Neither I nor II

Tardigrade Admin · Accepted Answer

Mechanism I: Rate=k[.NO2].[.O3]. Slow step is rate determining Mechanism II: textRate textRate = textk â² [ textN textO 2 ][ textO ] â¦(i) From 1st step K=([. O2 ]. [. O ]./[. O3 ].) (k = eq. constant) text[O] text= textk ([ textO text3]/[ textO text2]) ...(ii) From equation (i) and (ii) Rate = k prime[ NO 2][ O 3][ O 2]-1 So both mechanism show that reaction is first order with respect to NO 2 and O 3.

Q. Consider the reaction 2NO2​(g)+O3​(g)→N2​O5​(g)+O2​(g) The reaction of nitrogen dioxide and ozone represents is first order in NO2​(g) and in O3​(g) . Which of these possible reaction mechanism is consistent with the rate law?

Only I

Only II

Both I and II

Neither I nor II

Q. Consider the reaction

$2 N O_{2} (g) + O_{3} (g) \to N_{2} O_{5} (g) + O_{2} (g)$

The reaction of nitrogen dioxide and ozone represents is first order in $N O_{2} (g)$ and in $O_{3} (g)$ . Which of these possible reaction mechanism is consistent with the rate law?