Calculations – Rate Constant (M*s4) Using the measured reaction rate and the calculated [S,0,²], [S;O,²], and [1), calcuate the value of the rate constant, k, for Exp. 1-3 using the experimentally determined rate law (from last week): (first order with respect to S,0," and I) Record the rate constant, k, in Table 3 for Exp. 1-3. Show your work for the calculation of k for Exp. 3 (where indicated) in your lab report. Table 3: Calculation of k from the Rate Law (S,0,) -5.0 * 10 M Exp. (5,0 (M) Rxn Rate (M/s) 3.1 10 1.5 10* 8.3* 10 T'C ( (M) 1.2 10 1.2* 10 1.2 10 k (M*s4) 3.0* 10 3.0* 10 3.0* 10 1 25 3 45
Calculations – Rate Constant (M*s4) Using the measured reaction rate and the calculated [S,0,²], [S;O,²], and [1), calcuate the value of the rate constant, k, for Exp. 1-3 using the experimentally determined rate law (from last week): (first order with respect to S,0," and I) Record the rate constant, k, in Table 3 for Exp. 1-3. Show your work for the calculation of k for Exp. 3 (where indicated) in your lab report. Table 3: Calculation of k from the Rate Law (S,0,) -5.0 * 10 M Exp. (5,0 (M) Rxn Rate (M/s) 3.1 10 1.5 10* 8.3* 10 T'C ( (M) 1.2 10 1.2* 10 1.2 10 k (M*s4) 3.0* 10 3.0* 10 3.0* 10 1 25 3 45
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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please help me calculate for the rate constant
![Calculations – Rate Constant (M's)
Using the measured reaction rate and the calculated [S20, ], [S:0,2], and [1], calcuate the value of the rate
constant, k, for Exp. 1-3 using the experimentally determined rate law (from last week):
rate = k [S,0,P 11) (first order with respect to $,0 and 1)
Record the rate constant, k, in Table 3 for Exp. 1-3.
Show your work for the calculation of k for Exp. 3 (where indicated) in your lab report.
Table 3: Calculation of k from the Rate Law
=_5.0* 104
M
k (Ms+)
[S:0,1 (M)
3.0* 10
3.0* 10
[1 (M)
1.2 101
Exp.
T'C
Rxn Rate (M/s)
3.1 10
1.5 10
8.3 10
1
5
1.2 101
1.2 101
2
25
3
45
3.0* 10 2](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F23029c3f-32e4-4946-9f07-7f9c026ab9f8%2F59e88d2c-379d-40bc-aced-10de8d3e1f4e%2Fnucdozg_processed.png&w=3840&q=75)
Transcribed Image Text:Calculations – Rate Constant (M's)
Using the measured reaction rate and the calculated [S20, ], [S:0,2], and [1], calcuate the value of the rate
constant, k, for Exp. 1-3 using the experimentally determined rate law (from last week):
rate = k [S,0,P 11) (first order with respect to $,0 and 1)
Record the rate constant, k, in Table 3 for Exp. 1-3.
Show your work for the calculation of k for Exp. 3 (where indicated) in your lab report.
Table 3: Calculation of k from the Rate Law
=_5.0* 104
M
k (Ms+)
[S:0,1 (M)
3.0* 10
3.0* 10
[1 (M)
1.2 101
Exp.
T'C
Rxn Rate (M/s)
3.1 10
1.5 10
8.3 10
1
5
1.2 101
1.2 101
2
25
3
45
3.0* 10 2
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