Question

27-11. Consider the decomposition reaction of N?O?(g) 2N?O?(g) \stackrel{k_{obs}}{\longrightarrow} 4NO?(g) + O?(g) A proposed mechanism for this reaction is N?O?(g) \stackrel{k?}{\rightleftharpoons} NO?(g) + NO?(g) NO?(g) + NO?(g) \stackrel{k?}{\longrightarrow} NO(g) + NO?(g) + O?(g) NO?(g) + NO(g) \stackrel{k?}{\longrightarrow} 2NO?(g) Assume that the steady-state approximation applies to both the NO(g) and NO?(g) reaction intermediates to show that this mechanism is consistent with the experimentally observed rate law \frac{d[O?]}{dt} = k_{obs}[N?O?] Express $k_{obs}$ in terms of the rate constants for the individual steps of the reaction mechanism.

          27-11. Consider the decomposition reaction of N?O?(g)

2N?O?(g) \stackrel{k_{obs}}{\longrightarrow} 4NO?(g) + O?(g)
A proposed mechanism for this reaction is

N?O?(g) \stackrel{k?}{\rightleftharpoons} NO?(g) + NO?(g)

NO?(g) + NO?(g) \stackrel{k?}{\longrightarrow} NO(g) + NO?(g) + O?(g)

NO?(g) + NO(g) \stackrel{k?}{\longrightarrow} 2NO?(g)

Assume that the steady-state approximation applies to both the NO(g) and NO?(g) reaction
intermediates to show that this mechanism is consistent with the experimentally observed
rate law

\frac{d[O?]}{dt} = k_{obs}[N?O?]

Express $k_{obs}$ in terms of the rate constants for the individual steps of the reaction mechanism.

27-11. Consider the decomposition reaction of N?O?(g)

2N?O?(g) kobs⟶ 4NO?(g) + O?(g)
A proposed mechanism for this reaction is

N?O?(g) k?⇌ NO?(g) + NO?(g)

NO?(g) + NO?(g) k?⟶ NO(g) + NO?(g) + O?(g)

NO?(g) + NO(g) k?⟶ 2NO?(g)

Assume that the steady-state approximation applies to both the NO(g) and NO?(g) reaction
intermediates to show that this mechanism is consistent with the experimentally observed
rate law

(d[O?])/(dt) = kobs[N?O?]

Express kobs in terms of the rate constants for the individual steps of the reaction mechanism.

Added by Monica T.

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