Use your experiment rate law and the average value for k to predict how long (in seconds)it would take for the acetone iodination reaction to finish for the initial conditions givenbelow. Note that you are solving for Δt in the average reaction rate.initial concentrations: [acetone] = 0.850 M[H+] = 0.320 M[I2] = 0.00150 Mreaction time (seconds): ______________How precise were the experimental measurements of the reaction time for each reactionmixture? How precise were the measurements of the value of the rate constant, k? Explain your answers. Determining the Rate Law for the Iodination of Acetone• the volumes used for all eight reaction trials (two trials for each reaction mixture) match the volumesgiven in Table 2 below:Table 2. Reaction mixtures for the iodination of acetone trials.Volume (mL)Mixture4.0 M acetone1.0 M HCI0.0050 M I2DI H2O15.05.05.010.0210.05.05.05.035.010.05.05.045.05.010.05.0Table 3. Iodination of acetone reaction times.Reaction TimeMixtureTrial 1Trial 2182 s75 s235 s35 s344 s46 s4139 s151 sinclude the above reaction times in your Data and Calculation pageseach reaction time represents the time needed for the yellow color of the iodine to just disappearfrom the reaction solution

Answered: Use your experiment rate law and the…

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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Use your experiment rate law and the average value for k to predict how long (in seconds)
it would take for the acetone iodination reaction to finish for the initial conditions given
below. Note that you are solving for Δt in the average reaction rate.
initial concentrations: [acetone] = 0.850 M
[H+] = 0.320 M
[I2] = 0.00150 M
reaction time (seconds): ______________

How precise were the experimental measurements of the reaction time for each reaction
mixture? How precise were the measurements of the value of the rate constant, k? Explain your answers.

Determining the Rate Law for the Iodination of Acetone
• the volumes used for all eight reaction trials (two trials for each reaction mixture) match the volumes
given in Table 2 below:
Table 2. Reaction mixtures for the iodination of acetone trials.
Volume (mL)
Mixture
4.0 M acetone
1.0 M HCI
0.0050 M I2
DI H2O
1
5.0
5.0
5.0
10.0
2
10.0
5.0
5.0
5.0
3
5.0
10.0
5.0
5.0
4
5.0
5.0
10.0
5.0
Table 3. Iodination of acetone reaction times.
Reaction Time
Mixture
Trial 1
Trial 2
1
82 s
75 s
2
35 s
35 s
3
44 s
46 s
4
139 s
151 s
include the above reaction times in your Data and Calculation pages
each reaction time represents the time needed for the yellow color of the iodine to just disappear
from the reaction solution

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