1. Why were the reagents equilibrated in water bath before mixing? 2. What is the purpose of starch in the experiment? 3. What will happen to the reaction time and reaction rate if the concentration of one of the reactants is doubled while keeping everything the same?
1. Why were the reagents equilibrated in water bath before mixing? 2. What is the purpose of starch in the experiment? 3. What will happen to the reaction time and reaction rate if the concentration of one of the reactants is doubled while keeping everything the same?
Chemical Principles in the Laboratory
11th Edition
ISBN:9781305264434
Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi
Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi
Chapter21: Rates Of Chemical Reactions, Ii. A Clock Reaction
Section: Chapter Questions
Problem 2ASA
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Hello, the priority to be answered would be page 1 (1st image). However, I can put part 2 (2nd image) on a new question/post. Just wanted to include that in this post for reference to whoever will answer it. Thank you!
Transcribed Image Text:Post lab Questions:
1. Why were the reagents equilibrated in water bath before mixing?
2. What is the purpose of starch in the experiment?
3. What will happen to the reaction time and reaction rate if the concentration of one of
the reactants is doubled while keeping everything the same?
4. Cite possible sources of error in the experiment.
![Table 4-1
Volume, mL
Run
4.00 M
0.00120 M I2
1.00 м HC
Starch
dH20
acetone
solution
1
2.00
2.00
2.00
2.00
17.00
2
4.00
2.00
2.00
2.00
15.00
3
2.00
2.00
4.00
2.00
15.00
4
2.00
4.00
2.00
2.00
15.00
5
3.00
3.00
3.00
1.00
15.00
Table 4-2
Time elapsed
(sec)
Run
1
257
2
131
130
4
510
181
1. Determine the concentration of each component (C2) in the final mixture for each
run (refer to Table 4-1) for the total volume (V2) of the mixture, and the initial
concentration (C1) and volume (V1) of each component).
CiV1 = C2V2
%3D
2. Calculate for the reaction rate per run using the concentration of iodine and time
elapsed.
reaction rate = [12] in the final mixture/time elapsed
3. Determine the reaction order with respect to l2. Also determine the reaction order
with respect to C3H,O and the reaction order with respect to HCI. Round off your
answers to the nearest whole number.
4. Calculate for the rate constant for each run using the reaction orders obtained (use
rounded off values of reaction orders).
5. Take the average of the rate constants.
6. Determine the rate law of the reaction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6a43db2c-c99e-4fe2-95ba-8aac0e3febc0%2F63aed2b7-67d6-419b-ab65-cedcdcf5e103%2Fjootag_processed.png&w=3840&q=75)
Transcribed Image Text:Table 4-1
Volume, mL
Run
4.00 M
0.00120 M I2
1.00 м HC
Starch
dH20
acetone
solution
1
2.00
2.00
2.00
2.00
17.00
2
4.00
2.00
2.00
2.00
15.00
3
2.00
2.00
4.00
2.00
15.00
4
2.00
4.00
2.00
2.00
15.00
5
3.00
3.00
3.00
1.00
15.00
Table 4-2
Time elapsed
(sec)
Run
1
257
2
131
130
4
510
181
1. Determine the concentration of each component (C2) in the final mixture for each
run (refer to Table 4-1) for the total volume (V2) of the mixture, and the initial
concentration (C1) and volume (V1) of each component).
CiV1 = C2V2
%3D
2. Calculate for the reaction rate per run using the concentration of iodine and time
elapsed.
reaction rate = [12] in the final mixture/time elapsed
3. Determine the reaction order with respect to l2. Also determine the reaction order
with respect to C3H,O and the reaction order with respect to HCI. Round off your
answers to the nearest whole number.
4. Calculate for the rate constant for each run using the reaction orders obtained (use
rounded off values of reaction orders).
5. Take the average of the rate constants.
6. Determine the rate law of the reaction.
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