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]

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

Answer 1

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