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The Experimental Rate Law for the Decomposition of Nitrous Oxide

Question 11

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. 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.

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