The kinetics of a unimolecular reaction are observed and the reactant decays over time but it is not clear from the raw data whether the process is first-order or second-order. The two plots below represent fits to least-squares lines, with the equations shown. From this information, indicate the value of the rate constant. In [A]t -0.5H -net -1.5 -2.0 -2.5 -3.0 0 y = -0.00482 x - 1.11 R² = 0.894354 100 200 t (sec) 300 400 1 [A]t 20 15 10 5 0 y = 0.04039 x + 2.0267 100 200 R² = 0.999308 300 t (sec) 400

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The kinetics of a unimolecular reaction are observed and the reactant decays over time but it is not clear from the raw data whether the
process is first-order or second-order. The two plots below represent fits to least-squares lines, with the equations shown. From this
information, indicate the value of the rate constant.
1
[A]t
20
y = -0.00482 x - 1.11
y = 0.04039 x + 2.0267
15
SE
10
5
400
In [A]t
-0.5
-1
-1.5
-2.0
-2.5
-3.0
0
R² = 0.894354
100
200
t (sec)
300
0
100
200
R² = 0.999308
300
t (sec)
400
Transcribed Image Text:The kinetics of a unimolecular reaction are observed and the reactant decays over time but it is not clear from the raw data whether the process is first-order or second-order. The two plots below represent fits to least-squares lines, with the equations shown. From this information, indicate the value of the rate constant. 1 [A]t 20 y = -0.00482 x - 1.11 y = 0.04039 x + 2.0267 15 SE 10 5 400 In [A]t -0.5 -1 -1.5 -2.0 -2.5 -3.0 0 R² = 0.894354 100 200 t (sec) 300 0 100 200 R² = 0.999308 300 t (sec) 400
What is the order of this rate process?
zeroth
first
second
cannot be determined from this information
Transcribed Image Text:What is the order of this rate process? zeroth first second cannot be determined from this information
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