In a certain polluted atmosphere containing `O_(3)` at a steady-state concentration of `2.0 xx 10^(-8) mol L^(-1)`, the hourly Production of `O_(3)` by all sources was estimated as `7.2 xx 10^(-15) mol L^(-1)`. If only mechanism for the destruction of `O_(3)` is the second order reaction,
`2O_(3) rarr 3O_(2)`
Calculate the rate constant for the destruction reaction defined by the rate law for `-Delta[O_(3)]//Delta t`.

Explanation

To solve the problem, we need to calculate the rate constant \( k \) for the destruction of ozone (\( O_3 \)) in a second-order reaction given the steady-state concentration and the rate of production.

### Step-by-Step Solution:

1. **Identify the Given Data:**
- Steady-state concentration of \( O_3 \):
\[
[O_3] = 2.0 \times 10^{-8} \, \text{mol L}^{-1}
...