Select two trials that can be used to determine the reaction order with respect to A. [A], mol/L [B], mol/L rate, mol/(L-min) Trial 1 0.443 0.459 0.0824 Trial 2 0.886 0.459 0.165 Trial 3 0.443 0.918 0.0824 Trial 4 0.429 0.938 0.0798 Rate = k[A]orderA[B]orderB (Select all that apply.) O Trial 1 O Trial 2 O Trial 3 O Trial 4
Select two trials that can be used to determine the reaction order with respect to A. [A], mol/L [B], mol/L rate, mol/(L-min) Trial 1 0.443 0.459 0.0824 Trial 2 0.886 0.459 0.165 Trial 3 0.443 0.918 0.0824 Trial 4 0.429 0.938 0.0798 Rate = k[A]orderA[B]orderB (Select all that apply.) O Trial 1 O Trial 2 O Trial 3 O Trial 4
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions
Section14.3: Effect Of Concentration On Reaction Rate
Problem 14.3CYU: The initial rate ( [NO]/ t] of the reaction of nitrogen monoxide and oxygen NO(g) + 2O2(g) NO2(g)...
Related questions
Question
3
![A general reaction is the formation of molecule C from two reactant molecules, A and B.
A + B C
The reaction was run multiple times at constant temperature using different initial concentrations of the two reactants. The initial rates
obtained are included in the table below.
The rate equation is of the form:
mol
1orderB
rate = k[A]orderA [B]
%3D
L• min
[A], mol/L [B], mol/L rate, mol/(L-min)
Trial 1
0.443
0.459
0.0824
Trial 2
0.886
0.459
0.165
Trial 3
0.443
0.918
0.0824
Trial 4
0.429
0.938
0.0798](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F783d260a-ea1c-402a-b0ab-7a62c96d7cdd%2F238175a3-3cde-49cb-a3ef-2652ac423490%2Fp3v1amm_processed.jpeg&w=3840&q=75)
Transcribed Image Text:A general reaction is the formation of molecule C from two reactant molecules, A and B.
A + B C
The reaction was run multiple times at constant temperature using different initial concentrations of the two reactants. The initial rates
obtained are included in the table below.
The rate equation is of the form:
mol
1orderB
rate = k[A]orderA [B]
%3D
L• min
[A], mol/L [B], mol/L rate, mol/(L-min)
Trial 1
0.443
0.459
0.0824
Trial 2
0.886
0.459
0.165
Trial 3
0.443
0.918
0.0824
Trial 4
0.429
0.938
0.0798
![Select two trials that can be used to determine the reaction order with respect to A.
[A], mol/L [B], mol/L rate, mol/(L-min)
Trial 1
0.443
0.459
0.0824
Trial 2
0.886
0.459
0.165
Trial 3
0.443
0.918
0.0824
Trial 4
0.429
0.938
0.0798
K[A]orderA[B]
31orderB
Rate =
(Select all that apply.)
O Trial 1
O Trial 2
O Trial 3
O Trial 4](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F783d260a-ea1c-402a-b0ab-7a62c96d7cdd%2F238175a3-3cde-49cb-a3ef-2652ac423490%2Fso5v0d6_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Select two trials that can be used to determine the reaction order with respect to A.
[A], mol/L [B], mol/L rate, mol/(L-min)
Trial 1
0.443
0.459
0.0824
Trial 2
0.886
0.459
0.165
Trial 3
0.443
0.918
0.0824
Trial 4
0.429
0.938
0.0798
K[A]orderA[B]
31orderB
Rate =
(Select all that apply.)
O Trial 1
O Trial 2
O Trial 3
O Trial 4
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 2 steps with 1 images
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 & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:
9781337398909
Author:
Lawrence S. Brown, Tom Holme
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:
9781337398909
Author:
Lawrence S. Brown, Tom Holme
Publisher:
Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781133949640
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning