A possible mechanism for the reaction 2NO(g) + O₂(g)$\rightarrow$2NO₂(g) Is: 2NO(g) $f$ N₂O₂(g) K₁,K₁',Fast N₂O₂(g)+ O₂(g)$\rightarrow$ 2NO₂(g) K₂,Slow Application of the steady-state approximation gives A) [N₂O₂] = 0. B) k₁[NO]² - k₂[N₂O₂][O₂] = 0. C) [N₂O₂] = (k₁/k₂)[NO]². D) k₁[NO]² - k₁'[N₂O₂] -k₂[N₂O₂][O₂] = 0. E) [N₂O₂] = (k₁/k₁')[NO]².

Question

Quizplus · Accepted Answer

The steady-state approximation assumes that the concentration of the intermediate (N2O2) remains constant, leading to the equation for its formation and consumption rates being equal.

A Possible Mechanism for the Reaction 2NO(g) + O2(g) →\rightarrow→ 2NO2(g) Is: 2NO(g)

A Possible Mechanism for the Reaction 2NO(g) + O₂(g) $\rightarrow$ 2NO₂(g)
Is:
2NO(g)