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The reaction order with respect to a reactant can be negative, as demonstrated in the following scenario: 2O3 -> 3O2 with the rate law given by Rate = k[O3]^2[O2]^-1.

1. Rate = k[A]^0 with the unit of k being mol L^−1 sec^−1
2. Rate = k[O3]^2[O2]^-1
3. Rate = k[A]^1[B]^2
4. For cases II and III, if [A] is held constant and [B] is doubled, the rate increases fourfold, indicating second-order dependence on B. For cases I and IV, if [B] is held constant and [A] is quadrupled, the rate also quadruples, showing first-order dependence on A.

Correct answer: Rate = k[O3]^2[O2]^-1

Solution

The given rate law matches option B, where the rate is proportional to [O3]^2 and inversely proportional to [O2]. This demonstrates that the order with respect to O2 is negative (-1).

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