Multiple Choice
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 ![The experimental rate law for the decomposition of nitrous oxide (N<sub>2</sub>O) to N<sub>2</sub> and O<sub>2</sub> is Rate = k[N<sub>2</sub>O]<sup>2</sup>. Two mechanisms are proposed: I. N<sub>2</sub>O → N<sub>2</sub> + O N<sub>2</sub>O + O → N<sub>2</sub> + O<sub>2</sub><sub></sub><sub></sub> II. 2N<sub>2</sub>O N<sub>4</sub>O<sub>2</sub><sub></sub> N<sub>4</sub>O<sub>2</sub> → 2N<sub>2</sub> + O<sub>2</sub><sub></sub> Which of the following could be a correct mechanism? A) Mechanism I with the second step as the rate-determining step. B) Mechanism II with the second step as the rate-determining step. C) Mechanism I with the first step as the rate-determining step. D) Two of these could be correct. E) None of these could be correct.](https://d2lvgg3v3hfg70.cloudfront.net/TB6422/11eaaf91_9dee_2506_892c_6fea6fc7fd80_TB6422_11.jpg)
N4O2
N4O2 → 2N2 + O2
Which of the following could be a correct mechanism?
A) Mechanism I with the second step as the rate-determining step.
B) Mechanism II with the second step as the rate-determining step.
C) Mechanism I with the first step as the rate-determining step.
D) Two of these could be correct.
E) None of these could be correct.
Correct Answer:
Verified
Correct Answer:
Verified
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