The reaction NO(g) + O3(g) → NO2(g) + O2(g) was studied by performing two experiments. In the first experiment the rate of disappearance of NO was followed in the presence of a large excess of O3. The results were as follows ([O3] remains effectively constant at 1.0x1014 molecules/cm3): Time (ms) [NO] (molecules/cm3) 0 6.0x108 100. 5.0x108 500. 2.4x108 700. 1.7x108 1000. 9.9x107 In the second experiment [NO] was held constant at 2.0x1014 molecules/cm3. The data for the disappearance of O3 are as follows: Time (ms) [NO] (molecules/cm3) 0 1.0x1010 50. 8.4x109 100. 7.0x109 200. 4.9x109 300. 3.4x109 (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 from each set of experiments? Rate = k’[NO]^x Rate = k”[O3]^y
The reaction
NO(g) + O3(g) → NO2(g) + O2(g)
was studied by performing two experiments. In the first experiment the rate of disappearance of NO was followed in the presence of a large excess of O3. The results were as follows ([O3] remains effectively constant at 1.0x1014 molecules/cm3):
Time (ms) [NO] (molecules/cm3)
0 6.0x108
100. 5.0x108
500. 2.4x108
700. 1.7x108
1000. 9.9x107
In the second experiment [NO] was held constant at 2.0x1014 molecules/cm3. The data for the disappearance of O3 are as follows:
Time (ms) [NO] (molecules/cm3)
0 1.0x1010
50. 8.4x109
100. 7.0x109
200. 4.9x109
300. 3.4x109
(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 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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