The rate law for the following mechanism is NO₂(g)+ F₂(g)$\rightarrow$NO₂F(g)+ F(g) K₁, Slow F(g)+ NO₂(g)$\rightarrow$NO₂F(g) K₂, Fast A) rate = k₂[NO₂]². B) rate = k₂[NO₂][F]. C) rate = k₁[NO₂][F₂]. D) rate = k₁k₂[NO₂]². E) rate = k₁[NO₂F][F].

Question

Quizplus · Accepted Answer

The rate law is determined by the slow step of the reaction mechanism, which involves both $NOS$ and $F$ as reactants.

The Rate Law for the Following Mechanism Is NO2(g)+ F2(g) →\rightarrow→

The Rate Law for the Following Mechanism Is
NO₂(g)+ F₂(g) $\rightarrow$