The experimental rate law for the decomposition of nitrous oxide (N2O) to N2 and

Question

The experimental rate law for the decomposition of nitrous oxide (N2O) to N2 and O2 is rate = k[N2O]^2. Two mechanisms are proposed: I. N2O ? N2 + O N2O + O ? N2 + O2 II. 2N2O <===> N4O2 N4O2 ? 2N2 + O2 Which of the following could be a correct mechanism? (show all works) A) Mechanism I with the first step as the rate-determining step. B) Mechanism II with the second step as the rate-determining step if the first step is a fast equilibrium step. C) Mechanism I with the second step as the rate-determining step as long as the first step is a fast equilibrium step. D) At least two of the above choices (a-c) could be correct. E) None of the choices (a-c) could be correct.

Explanation / Answer

answer is option D

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.