6. The rate law for the overall reaction 2 N2O5 (g) →4 NO2 (g) + O2 (g) is Rate = k[N2Os). a. Consider this mechanism: N2Os (g) → NO3 (g) + NO2 (g) (fast) NO2 (g) + N2Os (g)→ 3 NO2 (g) + 02 (g) (fast] i. ii. (slow] i. NO3 (g) +0 (g) – NO2 (g) + O2 (g) Is this reaction mechanism consistent with the rate law? Why or Why not? b. If the reaction mechanism is not consistent with the rate law, how would it need to change to become consistent? c. List potential reaction intermediates present in this mechanism. d. Draw a reaction energy diagram for this mechanism including any modifications you've made in a-c.

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6. The rate law for the overall reaction
2 N2Os (g) →4 NO02 (g) + O2 (g)
is Rate = k[N2Os].
a. Consider this mechanism:
i.
N2Os (g) → NO3 (g) + NO2 (g)
NO2 (g) + N2Os (g) →3 NO2 (g) + O2 (9)
NO3 (g) + 0 (g) → NO2 (g) + O2 (g)
(fast)
ii.
(slow)
ii.
[fast)
Is this reaction mechanism consistent with the rate law? Why or Why not?
b. If the reaction mechanism is not consistent with the rate law, how would it
need to change to become consistent?
c. List potential reaction intermediates present in this mechanism.
d. Draw a reaction energy diagram for this mechanism including any modifications
you've made in a-c.
Transcribed Image Text:6. The rate law for the overall reaction 2 N2Os (g) →4 NO02 (g) + O2 (g) is Rate = k[N2Os]. a. Consider this mechanism: i. N2Os (g) → NO3 (g) + NO2 (g) NO2 (g) + N2Os (g) →3 NO2 (g) + O2 (9) NO3 (g) + 0 (g) → NO2 (g) + O2 (g) (fast) ii. (slow) ii. [fast) Is this reaction mechanism consistent with the rate law? Why or Why not? b. If the reaction mechanism is not consistent with the rate law, how would it need to change to become consistent? c. List potential reaction intermediates present in this mechanism. d. Draw a reaction energy diagram for this mechanism including any modifications you've made in a-c.
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