For Part B: Use the rate law determined above (integer values for the orders of reaction - m, n, and p – and the properly rounded average value for the rate constant, k) to predict (using equation 2) the rate of reaction for the mixture you ran in Part B. Equation 2: rate = k [acetone]" [I;]" [H°P • Then use this rate to calculate (using equation 4) how long (t) you would EXPECT it to take for the Iz color to disappear from this mixture. Equation 4: [12] - 2lo t-to All2] 0 -12]o [12 ]o rate = At t-0 t • Compare this theoretically calculated time to the time you experimentally measured in Part B as % error. %error= (standard/ average)*100%
For Part B: Use the rate law determined above (integer values for the orders of reaction - m, n, and p – and the properly rounded average value for the rate constant, k) to predict (using equation 2) the rate of reaction for the mixture you ran in Part B. Equation 2: rate = k [acetone]" [I;]" [H°P • Then use this rate to calculate (using equation 4) how long (t) you would EXPECT it to take for the Iz color to disappear from this mixture. Equation 4: [12] - 2lo t-to All2] 0 -12]o [12 ]o rate = At t-0 t • Compare this theoretically calculated time to the time you experimentally measured in Part B as % error. %error= (standard/ average)*100%
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...
Related questions
Question
Using the following information from the table and previous completed questions complete part B
![[12]o
Mixture
[Acetone],
[H.]o
[L]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](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fee47860b-51bf-4c58-a4ad-6a29df2141ce%2F8b8c7091-addf-448d-93a8-38fefa61588f%2F2ulrt7d_processed.jpeg&w=3840&q=75)
Transcribed Image Text:[12]o
Mixture
[Acetone],
[H.]o
[L]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
![For Part A: Using the data for mixtures A1-A4, calculate:
• the order of reaction with respect to acetone (i.e., the value of m in equation 2). M=1
• the order of reaction with respect to H* (i.e., the value of p in equation 2) P=0
• the order of reaction with respect to I, (i.e., the value of n in equation 2) N=1
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.
Rate law:
4.17x10^-6 =K [.8]^1[.2]^1[.001]^0
K=2.60*10^-5M^-1s^-1
For Part B:
Use the rate law determined above (integer values for the orders of reaction
the properly rounded average value for the rate constant, k) to predict (using equation 2) the rate
of reaction for the mixture you ran in Part B.
т, п, and p —and
Equation 2: rate = k [acetone]" [I;]" [H°P'
• Then use this rate to calculate (using equation 4) how long (t) you would EXPECT it to take for
the I, color to disappear from this mixture.
Equation 4:
[12] – 12]o
t-to
All2]
[12]o
t
rate =
At
t-0
=
Compare this theoretically calculated time to the time you experimentally measured in Part B as
% error.
%error= (standard/ average)*100%](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fee47860b-51bf-4c58-a4ad-6a29df2141ce%2F8b8c7091-addf-448d-93a8-38fefa61588f%2Fd5yqt86_processed.jpeg&w=3840&q=75)
Transcribed Image Text:For Part A: Using the data for mixtures A1-A4, calculate:
• the order of reaction with respect to acetone (i.e., the value of m in equation 2). M=1
• the order of reaction with respect to H* (i.e., the value of p in equation 2) P=0
• the order of reaction with respect to I, (i.e., the value of n in equation 2) N=1
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.
Rate law:
4.17x10^-6 =K [.8]^1[.2]^1[.001]^0
K=2.60*10^-5M^-1s^-1
For Part B:
Use the rate law determined above (integer values for the orders of reaction
the properly rounded average value for the rate constant, k) to predict (using equation 2) the rate
of reaction for the mixture you ran in Part B.
т, п, and p —and
Equation 2: rate = k [acetone]" [I;]" [H°P'
• Then use this rate to calculate (using equation 4) how long (t) you would EXPECT it to take for
the I, color to disappear from this mixture.
Equation 4:
[12] – 12]o
t-to
All2]
[12]o
t
rate =
At
t-0
=
Compare this theoretically calculated time to the time you experimentally measured in Part B as
% error.
%error= (standard/ average)*100%
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 3 steps
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY