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23 Nov 2019
Half-life equations: 1st order = ln2/k 2nd order = 1/[A]0k rate = k[NO]2[Br2] k (rate constant) = Experiment #1 (.096), Experiment #2 (.38),Experiment #3 (.19) average rate constant = 2.22 x 10-1 (.222) *must use average rate constant for all 3 experiments Data [NO]: Exp #1 [.02], Exp. #2 [.04], Exp. #3 [.02] [Br2]: Exp #1 [.02], Exp. #2 [.02]. Exp. #3 [.04]
Half-life equations:
1st order = ln2/k
2nd order = 1/[A]0k
rate = k[NO]2[Br2]
k (rate constant) = Experiment #1 (.096), Experiment #2 (.38),Experiment #3 (.19)
average rate constant = 2.22 x 10-1 (.222)
*must use average rate constant for all 3 experiments
Data
[NO]: Exp #1 [.02], Exp. #2 [.04], Exp. #3 [.02]
[Br2]: Exp #1 [.02], Exp. #2 [.02]. Exp. #3 [.04]
Hubert KochLv2
27 Sep 2019
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Related questions
The reaction: NO (g) + O3(g) --> NO2(g) + O2 (g) was studied by performing 2 experiments. In the first experiment, the rate of disappearance of NO was measured in the presence of a large excess of O3. The results were as follows (O3 remains effectively constant at 1.0 x 1014 molecules/ cm3).
| Time (sec x 10-3) | [NO] (molecules/cm3) |
| 0 | 6.0 x 108 |
| 100 | 5.0 x 108 |
| 500 | 2.4 x 108 |
| 700 | 1.7 x 108 |
| 1000 | 9.9 x 107 |
In the second experiment [NO] was held constant at 2.00 x 1014 molecules/cm3. The data for the disappearance of O3 is in the table below.
| Time (sec x 103) | [O3] (molecules/cm3) |
| 0 | 1.0 x 1010 |
| 50 | 8.4 x 109 |
| 100 | 7.0 x 109 |
| 200 | 4.9 x 109 |
| 300 | 3.4 x 109 |
[NO] and [O3] are both first order, and overall rate law is rate = k [NO]1[O3]1
a) What is the value of the rate constant for each experiment?
Rate= k' [NO]x Rate= k'' [O3]y
b) What is the value of the rate constant for the overall rate law?
Rate= k [NO]x [O3]y
