Ozone in the earth's atmosphere decomposes according to the equation: `2O_(3)(g) rarr 3O_(2)(g)` This reaction is thought to occur via the two-step mechanism:
Step 1:` O_(3)(g) hArr O_(2)(g) +O(g)` Fast, reversible
Step 2: `O_(3)(g) +O(g) rarr 2O_(2)(g)` slow
What rate law is consistent with this mechanism?

Options

A. `-(Delta[O_(3)])/(Delta t)=k[O_(3)]`
B. `-(Delta[O_(3)])/(Delta t)=k[O_(3)]^(2)`
C. `-(Delta[O_(3)])/(Delta t)=(k[O_(3)]^(2))/([O_(2)])`
D. `-(Delta[O_(3)])/(Delta t)=(k[O_(3)]^(2))/([O_(2)]^(3))`

Answer

C