Mixture [Acetone], [H.], [IL]o Rate = avg. time A1 .8 .2 .001 4.17*10^-6 A2 1.6 .2 .001 8.5*10^-6 АЗ .8 .4 .001 8.16*10^-6 A4 .8 .2 .0005 4.17*10^-6 1.2 .3 .001 8.33*10^-6 Calculations to do: For Part A: Using the data for mixtures Al-A4, calculate: the order of reaction with respect to acetone (i.e., the value of m in equation 2). • the order of reaction with respect to H* (i.e., the value of p in equation 2) • the order of reaction with respect to I, (i.e., the value of n in equation 2) Note: Calculate each order of reaction to +0.01, and also the value rounded to an integer. Use the integer value in all subsequent calculations. Once you have the rate law calculate the value of the rate constant, k, for each of your four mixtures (and round each properly). And then calculate the average value for the rate constant. Include the units for k.
Mixture [Acetone], [H.], [IL]o Rate = avg. time A1 .8 .2 .001 4.17*10^-6 A2 1.6 .2 .001 8.5*10^-6 АЗ .8 .4 .001 8.16*10^-6 A4 .8 .2 .0005 4.17*10^-6 1.2 .3 .001 8.33*10^-6 Calculations to do: For Part A: Using the data for mixtures Al-A4, calculate: the order of reaction with respect to acetone (i.e., the value of m in equation 2). • the order of reaction with respect to H* (i.e., the value of p in equation 2) • the order of reaction with respect to I, (i.e., the value of n in equation 2) Note: Calculate each order of reaction to +0.01, and also the value rounded to an integer. Use the integer value in all subsequent calculations. Once you have the rate law calculate the value of the rate constant, k, for each of your four mixtures (and round each properly). And then calculate the average value for the rate constant. Include the units for k.
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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Question
Complete Part A using the given table and equation 2 which is;
rate = k [acetone]^m [I2]^n [H+]^p
![12].
Mixture
[Acetone],
[H,]o
[I]o
Rate =
avg. time
A1
.8
.2
.001
4.17*10^-6
A2
1.6
.2
.001
8.5*10^-6
АЗ
.8
.4
.001
8.16*10^-6
A4
.8
.2
.0005
4.17*10^-6
В
1.2
.3
.001
8.33*10^-6
Calculations to do:
For Part A:
Using the data for mixtures Al-A4, calculate:
• the order of reaction with respect to acetone (i.e., the value of m in equation 2).
• the order of reaction with respect to H* (i.e., the value of p in equation 2)
the order of reaction with respect to I, (i.e., the value of n in equation 2)
Note: Calculate each order of reaction to +0.01, and also the value rounded to an integer. Use
the integer value in all subsequent calculations.
Once you have the rate law calculate the value of the rate constant, k, for each of your four
mixtures (and round each properly). And then calculate the average value for the rate constant.
Include the units for k.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fee47860b-51bf-4c58-a4ad-6a29df2141ce%2F7e4df79b-5ebc-48ae-ad03-8f46c988aa02%2Fox5juhn_processed.jpeg&w=3840&q=75)
Transcribed Image Text:12].
Mixture
[Acetone],
[H,]o
[I]o
Rate =
avg. time
A1
.8
.2
.001
4.17*10^-6
A2
1.6
.2
.001
8.5*10^-6
АЗ
.8
.4
.001
8.16*10^-6
A4
.8
.2
.0005
4.17*10^-6
В
1.2
.3
.001
8.33*10^-6
Calculations to do:
For Part A:
Using the data for mixtures Al-A4, calculate:
• the order of reaction with respect to acetone (i.e., the value of m in equation 2).
• the order of reaction with respect to H* (i.e., the value of p in equation 2)
the order of reaction with respect to I, (i.e., the value of n in equation 2)
Note: Calculate each order of reaction to +0.01, and also the value rounded to an integer. Use
the integer value in all subsequent calculations.
Once you have the rate law calculate the value of the rate constant, k, for each of your four
mixtures (and round each properly). And then calculate the average value for the rate constant.
Include the units for k.
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