Question

For the chemical reaction, \(2\text{O}_3\rightleftharpoons 3\text{O}_2\), the reaction proceeds as follows:
\[\text{O}_3\rightleftharpoons \text{O}_2 + \text{O} \, \text{(fast)}\]
\[\text{O} + \text{O}_3 \rightarrow 2\text{O}_2 \, \text{(slow)}\]
The rate law expression will be:

• A. \( r = k'[\text{O}_3]^2 \)
• B. \( r = k'[\text{O}_3]^2[\text{O}_2]^{-1} \)
• C. \( r = k'[\text{O}_3][\text{O}_2] \)
• D. Unpredictable

Answer 1

The Correct Option is B

The correct option is (B): \( r = k'[\text{O}_3]^2[\text{O}_2]^{-1} \)