2N₂O5 (aq) → 4NO₂(aq) + O₂(g) What is the rate of disappearance of N2O5 from 200 to 400 seconds? Time [N₂05] [NO₂] [0₂] 0 1.00 0 0 200 0.88 0.24 0.12 400 0.78 ? ? 600 0.69 0.62 0.16 800 0.61 0.78 0.20 RateN₂05 [?] × 10⁰?¹ M/s = x Coefficient (green) Exponent (yellow) Enter
2N₂O5 (aq) → 4NO₂(aq) + O₂(g) What is the rate of disappearance of N2O5 from 200 to 400 seconds? Time [N₂05] [NO₂] [0₂] 0 1.00 0 0 200 0.88 0.24 0.12 400 0.78 ? ? 600 0.69 0.62 0.16 800 0.61 0.78 0.20 RateN₂05 [?] × 10⁰?¹ M/s = x Coefficient (green) Exponent (yellow) Enter
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
![**Chemistry: Understanding Reaction Rates**
**Reaction:**
\[ 2N_2O_5 (aq) \rightarrow 4NO_2 (aq) + O_2 (g) \]
**Problem Statement:**
What is the rate of disappearance of \( N_2O_5 \) from 200 to 400 seconds?
**Data Table:**
| Time (s) | \([N_2O_5]\) | \([NO_2]\) | \([O_2]\) |
|----------|--------------|------------|-----------|
| 0 | 1.00 | 0 | 0 |
| 200 | 0.88 | 0.24 | 0.12 |
| 400 | 0.78 | ? | ? |
| 600 | 0.69 | 0.62 | 0.16 |
| 800 | 0.61 | 0.78 | 0.20 |
**Explanation:**
The table above represents the concentration of \( N_2O_5 \), \( NO_2 \), and \( O_2 \) at various times during the reaction.
**Rate Calculation:**
To find the rate of disappearance of \( N_2O_5 \) from 200 to 400 seconds:
\[ \text{Rate}_{N_2O_5} = -\frac{[\text{N}_2\text{O}_5]_{400} - [\text{N}_2\text{O}_5]_{200}}{400\text{s} - 200\text{s}} \]
\[ \text{Rate}_{N_2O_5} = -\frac{0.78 - 0.88}{400 - 200} \]
\[ \text{Rate}_{N_2O_5} = -\frac{-0.10}{200} \]
\[ \text{Rate}_{N_2O_5} = 0.0005 \text{ M/s } \]
Thus, the rate of disappearance of \( N_2O_5 \) is \( 0.0005 \text{ M/s } \).
**Enter the Coefficient and Exponent:**
\[ \text{Rate}_{N_2O_](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdfd84302-10e6-446d-ac4f-33b2622f5f16%2F5d93aabb-ea5e-44c7-aaeb-9609537a6b70%2Fq3edfq_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Chemistry: Understanding Reaction Rates**
**Reaction:**
\[ 2N_2O_5 (aq) \rightarrow 4NO_2 (aq) + O_2 (g) \]
**Problem Statement:**
What is the rate of disappearance of \( N_2O_5 \) from 200 to 400 seconds?
**Data Table:**
| Time (s) | \([N_2O_5]\) | \([NO_2]\) | \([O_2]\) |
|----------|--------------|------------|-----------|
| 0 | 1.00 | 0 | 0 |
| 200 | 0.88 | 0.24 | 0.12 |
| 400 | 0.78 | ? | ? |
| 600 | 0.69 | 0.62 | 0.16 |
| 800 | 0.61 | 0.78 | 0.20 |
**Explanation:**
The table above represents the concentration of \( N_2O_5 \), \( NO_2 \), and \( O_2 \) at various times during the reaction.
**Rate Calculation:**
To find the rate of disappearance of \( N_2O_5 \) from 200 to 400 seconds:
\[ \text{Rate}_{N_2O_5} = -\frac{[\text{N}_2\text{O}_5]_{400} - [\text{N}_2\text{O}_5]_{200}}{400\text{s} - 200\text{s}} \]
\[ \text{Rate}_{N_2O_5} = -\frac{0.78 - 0.88}{400 - 200} \]
\[ \text{Rate}_{N_2O_5} = -\frac{-0.10}{200} \]
\[ \text{Rate}_{N_2O_5} = 0.0005 \text{ M/s } \]
Thus, the rate of disappearance of \( N_2O_5 \) is \( 0.0005 \text{ M/s } \).
**Enter the Coefficient and Exponent:**
\[ \text{Rate}_{N_2O_
Expert Solution
![](/static/compass_v2/shared-icons/check-mark.png)
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 with 2 images
![Blurred answer](/static/compass_v2/solution-images/blurred-answer.jpg)
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](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781259911156/9781259911156_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
![Principles of Instrumental Analysis](https://www.bartleby.com/isbn_cover_images/9781305577213/9781305577213_smallCoverImage.gif)
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781259911156/9781259911156_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
![Principles of Instrumental Analysis](https://www.bartleby.com/isbn_cover_images/9781305577213/9781305577213_smallCoverImage.gif)
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
![Organic Chemistry](https://www.bartleby.com/isbn_cover_images/9780078021558/9780078021558_smallCoverImage.gif)
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
![Chemistry: Principles and Reactions](https://www.bartleby.com/isbn_cover_images/9781305079373/9781305079373_smallCoverImage.gif)
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
![Elementary Principles of Chemical Processes, Bind…](https://www.bartleby.com/isbn_cover_images/9781118431221/9781118431221_smallCoverImage.gif)
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY