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The forward reaction rate for the nitric...

The forward reaction rate for the nitric oxide-oxygen reaction
`2NO+O_(2) rarr 2NO_(2)` has the rate law as:
`Rate = k[NO]^(2)[O_(2)]`.
If the mechanism is assumed to be:
`2NO+O overset(k_(eq))hArr` , (rapid equilibration)
`N_(2)O_(2) + O_(2) overset(k_(2))rarr 2NO_(2)` (slow step),
then which of the following is (are) correct?
(I) Rate constant `= k_(eq)k_(2)` , (II) `[N_(2)O_(2)] = k_(eq)[NO]^(2)`
(III) `[N_(2)O_(2)] = k_(eq)[NO]` , (IV) Rate constant `= k_(2)`
The correct option is

A

I, II

B

III, IV

C

I, III

D

None of these

Text Solution

Verified by Experts

The correct Answer is:
D
`k_(eq) = ([N_(2)O_(2)])/([NO]^(2)) rArr [N_(2)O_(2)] = k_(eq)[NO]^(2)` and `RDS : Rate = k_(2)[N_(2)O_(2)][O_(2)]`
`= k_(2)k_(eq)[NO]^(2)[O_(2)] = k [NO]^(2)[O_(2)]`
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