The reaction NO(g) + O3(g) †’ NO2(g) + O2(g) was studied by performing two experiments. In the first experiment (results shown in following table), the rate of disappearance of NO was followed in a large excess of O3. (The [O3] remains effectively constant at 1.0 × 1014 molecules/cm3.)

In the second experiment, [NO] was held constant at 2.0 × 1014 molecules/cm3. The data for the disappearance of O3 were as follows:

a. What is the order with respect to each reactant?
b. What is the overall rate law?
c. What is the value of the rate constant obtained from each set of experiments?
Rate = k€™[NO]x Rate = k€™[O3]y
d. What is the value of the rate constant for the overall rate law? Rate = k[NO]x[O3]y

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Time (ms) INOj molecules/cm3) 100±1 500 ± 1 700 ± 1 1000 ± 1 6.0× 10° 5.0 × 108 2.4 × 108 1.7× 108 9.9 × 107 IO 1 lime (ms) (moleculescm) 50 ± 1 100 ± 1 200 ± 1 300 1 1.0 × 1010 8.4 X 10 7.0 x 10 4.9 x 109 3.4 x 10