Consider the following chemiluminescent (gives off light) chemical reaction between the pollutant nitric oxide and the photochemical pollutant ozone: O3+NO-> NO2+O2

In one laboratory experiment the rate of disappearance of ozone (O3) was measured to be 6 x 10-4 M/s. Simultaneously, the concentration of ozone was measured to be 9 x 10-6 M and the concentration of nitric oxide (NO) was measured to be 2.5 x 10-6 M. Given that this chemiluminescent chemical reaction follows the following rate law:  Rate=k[O3][NO]

calculate the rate constant k.