Part B Consider the second-order reaction: 2HI(g) →H₂(g) + I₂(g) Ise the simulation to find the initial concentration [HI], and the rate constant k for the eaction. What will be the concentration of HI after t = 2.93×10¹0 s ([HI]t) for a reaction tarting under the condition in the simulation?
Part B Consider the second-order reaction: 2HI(g) →H₂(g) + I₂(g) Ise the simulation to find the initial concentration [HI], and the rate constant k for the eaction. What will be the concentration of HI after t = 2.93×10¹0 s ([HI]t) for a reaction tarting under the condition in the simulation?
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
4
![▼
Part B
Consider the second-order reaction:
2HI(g) →H₂(g) + I₂(g)
Use the simulation to find the initial concentration [HI], and the rate constant k for the
reaction. What will be the concentration of HI after t = 2.93×10¹0 s ([HI]t) for a reaction
starting under the condition in the simulation?
Express your answer in moles per liters to three significant figures.
► View Available Hint(s)
[HI] =
Submit
VE ΑΣΦ
Ć
******
www
?
mol
L](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F17d691f6-c15c-4493-a453-5eef977b8b22%2Fb70c55ee-b49d-470f-b718-4cc7d4adfd49%2Fw55qypz_processed.png&w=3840&q=75)
Transcribed Image Text:▼
Part B
Consider the second-order reaction:
2HI(g) →H₂(g) + I₂(g)
Use the simulation to find the initial concentration [HI], and the rate constant k for the
reaction. What will be the concentration of HI after t = 2.93×10¹0 s ([HI]t) for a reaction
starting under the condition in the simulation?
Express your answer in moles per liters to three significant figures.
► View Available Hint(s)
[HI] =
Submit
VE ΑΣΦ
Ć
******
www
?
mol
L
![Most of the time, the rate of a reaction depends on
the concentration of the reactant. In the case of
second-order reactions, the rate is proportional to
the square of the concentration of the reactant.
Select the image to explore the simulation, which
will help you to understand how second-order
reactions are identified by the nature of their plots.
You can also observe the rate law for different
reactions.
3-
**NAME
PERCK
In the simulation, you can select one of the three
different kinds of plots. You may use the Start
Stop, and Reset buttons to observe the
corresponding changes in the plot for different
kinds of reactions. You can also select six different
reactions using the drop-down menu and observe
three different types of plots for each reaction.
Relating plots to the order of a reaction
Consider the following reaction:
A-products
The plot of [A] versus t is linear for the zero-order reaction, the plot of In/A) versus t is linear for the first-order
reaction, and the plot of versus f is linear for the second-order reaction. (A) represents the concentration of the
reactant A
Part A
(A)
The linearity of each graph can be used to identify the order of a reaction.
View Available Hint(s)
C₂H2CH₂
2NO₂-2NO+O₂
2N₂O-2N₂+O₂
2N₂O₁-4NO₂ +0₂
2H1 H₂ +1₂
Reaction order Linear plot
[A] vs. t
In A) vs. t
Submit Previous Answers
zero
first
second
There are six different reactions you can access in the simulation using the drop-down menu. Which of the
following are second-order reactions?
Check all that apply.
Correct
vs. t
Review | Constants | Periodic Table](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F17d691f6-c15c-4493-a453-5eef977b8b22%2Fb70c55ee-b49d-470f-b718-4cc7d4adfd49%2F4r3cn6b_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Most of the time, the rate of a reaction depends on
the concentration of the reactant. In the case of
second-order reactions, the rate is proportional to
the square of the concentration of the reactant.
Select the image to explore the simulation, which
will help you to understand how second-order
reactions are identified by the nature of their plots.
You can also observe the rate law for different
reactions.
3-
**NAME
PERCK
In the simulation, you can select one of the three
different kinds of plots. You may use the Start
Stop, and Reset buttons to observe the
corresponding changes in the plot for different
kinds of reactions. You can also select six different
reactions using the drop-down menu and observe
three different types of plots for each reaction.
Relating plots to the order of a reaction
Consider the following reaction:
A-products
The plot of [A] versus t is linear for the zero-order reaction, the plot of In/A) versus t is linear for the first-order
reaction, and the plot of versus f is linear for the second-order reaction. (A) represents the concentration of the
reactant A
Part A
(A)
The linearity of each graph can be used to identify the order of a reaction.
View Available Hint(s)
C₂H2CH₂
2NO₂-2NO+O₂
2N₂O-2N₂+O₂
2N₂O₁-4NO₂ +0₂
2H1 H₂ +1₂
Reaction order Linear plot
[A] vs. t
In A) vs. t
Submit Previous Answers
zero
first
second
There are six different reactions you can access in the simulation using the drop-down menu. Which of the
following are second-order reactions?
Check all that apply.
Correct
vs. t
Review | Constants | Periodic Table
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 2 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