1. Chlorine dioxide, C1O2, is a reddish-yellow gas that is soluble in water. In basic solution, it gives ClO3 and ClO₂ ions: 2C102(aq) + 2 OH (aq) → ClO3(aq) + ClO2 (aq) + H₂0(1) To obtain the rate law for this reaction, the following experiments were run and, for each, the initial rate of reaction of ClO2 was determined. Obtain the rate law and the value of the rate constant. Experiment # Exp. 1 Exp. 2 Exp. 3 Initial Concentrations (M) CIO2 OH. 0.060 0.030 0.020 0.030 0.020 0.090 Initial Rate (mol/L-s) 0.0248 0.00276 0.00828
1. Chlorine dioxide, C1O2, is a reddish-yellow gas that is soluble in water. In basic solution, it gives ClO3 and ClO₂ ions: 2C102(aq) + 2 OH (aq) → ClO3(aq) + ClO2 (aq) + H₂0(1) To obtain the rate law for this reaction, the following experiments were run and, for each, the initial rate of reaction of ClO2 was determined. Obtain the rate law and the value of the rate constant. Experiment # Exp. 1 Exp. 2 Exp. 3 Initial Concentrations (M) CIO2 OH. 0.060 0.030 0.020 0.030 0.020 0.090 Initial Rate (mol/L-s) 0.0248 0.00276 0.00828
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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 answer the following with equations used and calculations.
Transcribed Image Text:Prelab questions:
Iodine Clock Reaction
1. Chlorine dioxide, ClO2, is a reddish-yellow gas that is soluble in water. In basic solution,
it gives ClO3 and ClO₂ ions:
2C102(aq) + 2 OH (aq) → ClO3 (aq) + ClO2 (aq) + H₂0(1)
To obtain the rate law for this reaction, the following experiments were run and, for each,
the initial rate of reaction of ClO2 was determined. Obtain the rate law and the value of the
rate constant.
Experiment #
Exp. 1
Exp. 2
Exp. 3
Initial Concentrations (M)
CIO2
OH-
0.060
0.030
0.020
0.030
0.020
0.090
Initial Rate
(mol/L-s)
0.0248
0.00276
0.00828
![Data Sheet:
Part 1: Effect of Concentration Data
Table 1. Raw experimental data.
Run # [103] (M) [1] (M) [103]. (M) [1] (M) [H]. (M) Time (s)
1
17.7
2
3
4
1
2
لیا
3
4
0.010
a
5
0.020
0.010
Table 2. Calculated individual orders and rate constant.
Overall
order
0.010
b
Rate Law:
Part 2: Temperature Effect Data
Table 3. Data for the effect of temperature experiment.
Run # T (°C)
tc (s) Rate (M/S) k (
5.0
58.3
22.4
8.6
4.1
2.1
15.0
25.0
35.0
0.10
с
45.0
0.10
0.20
Iodine Clock Reaction
0.10
k
4.9
4.6
k units
) (1/T) (S-¹)
Ln (k)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcb6117a0-75b4-4432-9d67-32f0c54d9830%2Fc1fe7815-ccf0-46fb-ad03-0c8af5b4aed0%2Fzni1bwbs_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Data Sheet:
Part 1: Effect of Concentration Data
Table 1. Raw experimental data.
Run # [103] (M) [1] (M) [103]. (M) [1] (M) [H]. (M) Time (s)
1
17.7
2
3
4
1
2
لیا
3
4
0.010
a
5
0.020
0.010
Table 2. Calculated individual orders and rate constant.
Overall
order
0.010
b
Rate Law:
Part 2: Temperature Effect Data
Table 3. Data for the effect of temperature experiment.
Run # T (°C)
tc (s) Rate (M/S) k (
5.0
58.3
22.4
8.6
4.1
2.1
15.0
25.0
35.0
0.10
с
45.0
0.10
0.20
Iodine Clock Reaction
0.10
k
4.9
4.6
k units
) (1/T) (S-¹)
Ln (k)
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