A complex chemical reaction takes place in two steps. Step I: NO(g) + O3(g) → NO3(g) + O(g) Step II: NO3(g) + O(g) → NO2(g) + O2(g) The predicted rate law is rate = k[NO][O3] Identify the rate determining step. Name the reaction intermediate/s. Why is/are it/these intermediate/s?

Rate law is rate = K[NO] [O3]. &there4; step I is rate determining step. NO3(g) and O(g) are reaction intermediates. These are reaction intermediates because they are formed in step I and consumed in step II.

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A complex chemical reaction takes place in two steps. Step I: NO(g) + O3(g) → NO3(g) + O(g) Step II: NO3(g) + O(g) → NO2(g) + O2(g) The predicted rate law is rate = k[NO][O3] -

Question

A complex chemical reaction takes place in two steps.

Step I: NO(g) + O₃(g) → NO₃(g) + O(g)

Step II: NO₃(g) + O(g) → NO₂(g) + O₂(g)

The predicted rate law is rate = k[NO][O₃]

Identify the rate determining step.
Name the reaction intermediate/s. Why is/are it/these intermediate/s?

Answer in Brief

Solution

Rate law is rate = K[NO] [O₃]. ∴ step I is rate determining step.
NO₃(g) and O(g) are reaction intermediates. These are reaction intermediates because they are formed in step I and consumed in step II.

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Molecularity of Elementary Reactions

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