The reaction NO(g) 1 O3(g) 88n NO2(g) 1 O2(g) was studied

Chapter 15, Problem 15.41

(choose chapter or problem)

The reaction NO(g) 1 O3(g) 88n NO2(g) 1 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 3 1014 molecules/cm3.) Time (ms) [NO] (molecules/cm3) 0 6.0 3 108 100 6 1 5.0 3 108 500 6 1 2.4 3 108 700 6 1 1.7 3 108 1000 6 1 9.9 3 107 In the second experiment, [NO] was held constant at 2.0 3 1014 molecules/cm3. The data for the disappearance of O3 were as follows: Time (ms) [O3] (molecules/cm3) 0 1.0 3 1010 50 6 1 8.4 3 109 100 6 1 7.0 3 109 200 6 1 4.9 3 109 300 6 1 3.4 3 109a. 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 5 k9[NO]x Rate 5 k0[O3]y d. What is the value of the rate constant for the overall rate law? Rate 5 k[NO]x[O3]y