A proposed mechanism for one of the pathways for the destruction of ozone in the atmosphere is:

step $1$ slow: $O_3+NOlongrightarrowN{O}_2+O_2$

step $2$ fast: $N{O}_2+$OlongrightarrowNO$+O_2$

$(1)$ Which species acts as a catalyst? Enter formula. If none, leave box blank:

$(2)$ Which species acts as a reaction intermediate? Enter formula. If none, leave box blank:

$(\frac{A^2}{A_2})$

$(3)$ Complete the rate law for the overall reaction that is consistent with this mechanism. Use the form $k[A{]}^m[B{]}^n$dots, where $\text{'}1\text{'}$ is understood $($so don't write it$)$ for $m,n$ etc.

Rate $=$

$A_2\sqrt[\phantom{2}]{A^2}$

Submit

Submit and Next

Mark this question for later review.

Skip to Previous

Skip to Next