A sample of N2O4 gas with a pressure of 1.00 atm is placed in a flask. When equilibrium is achieved, 20.0% of the N₂O4 has been converted to NO₂ gas. (a) Calculate Kp. (b) If the original pressure of N₂O4 is 0.10 atm, what is the percent dissociation of the gas? Is the result in agreement with Le Chatelier's principle?
A sample of N2O4 gas with a pressure of 1.00 atm is placed in a flask. When equilibrium is achieved, 20.0% of the N₂O4 has been converted to NO₂ gas. (a) Calculate Kp. (b) If the original pressure of N₂O4 is 0.10 atm, what is the percent dissociation of the gas? Is the result in agreement with Le Chatelier's principle?
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
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section: Chapter Questions
Problem 40GQ: Consider the following equilibrium: COBr2(g) CO(g) + Br2(g)Kc = 0.190 at 73 C (a) A 0.50 mol sample...
Related questions
Question
![### Equilibrium and Le Chatelier’s Principle: Sample Problem
**Problem Statement:**
A sample of \( \text{N}_2\text{O}_4 \) gas with a pressure of 1.00 atm is placed in a flask. When equilibrium is achieved, 20.0% of the \( \text{N}_2\text{O}_4 \) has been converted to \( \text{NO}_2 \) gas.
#### Questions:
(a) Calculate \( K_p \).
(b) If the original pressure of \( \text{N}_2\text{O}_4 \) is 0.10 atm, what is the percent dissociation of the gas? Is the result in agreement with Le Chatelier’s principle?
---
**Detailed Explanation:**
There are no graphs or diagrams in the provided image, only text. Therefore, we'll proceed directly with the text transcription suitable for an educational website.
### Solution:
#### (a) Calculate \( K_p \).
1. **Initial Information:**
- Initial pressure of \( \text{N}_2\text{O}_4 \): 1.00 atm
- Percent dissociation to \( \text{NO}_2 \): 20.0%
2. **Write the dissociation reaction:**
\[
\text{N}_2\text{O}_4 (g) \leftrightarrow 2 \text{NO}_2 (g)
\]
3. **Establish equilibrium pressures:**
Since 20.0% of \( \text{N}_2\text{O}_4 \) dissociates:
- Pressure of \( \text{N}_2\text{O}_4 \) at equilibrium: \( 1.00 \text{ atm} \times (1 - 0.20) = 0.80 \text{ atm} \)
- Pressure of \( \text{NO}_2 \) at equilibrium: \( 1.00 \text{ atm} \times 0.20 \times 2 = 0.40 \text{ atm} \)
\[
\text{NO}_2 = 2 \times (\text{0.20 atm}) = 0.40 \text{ atm}
\]
4. **Calculate \( K_p \):**
\[
K_p = \frac{{(\](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7f1e4f7e-3ee3-4328-9071-c5dd7af83341%2Fcf1c04cf-dfc4-429f-8858-c29ce8d106d8%2Ffssem2u_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Equilibrium and Le Chatelier’s Principle: Sample Problem
**Problem Statement:**
A sample of \( \text{N}_2\text{O}_4 \) gas with a pressure of 1.00 atm is placed in a flask. When equilibrium is achieved, 20.0% of the \( \text{N}_2\text{O}_4 \) has been converted to \( \text{NO}_2 \) gas.
#### Questions:
(a) Calculate \( K_p \).
(b) If the original pressure of \( \text{N}_2\text{O}_4 \) is 0.10 atm, what is the percent dissociation of the gas? Is the result in agreement with Le Chatelier’s principle?
---
**Detailed Explanation:**
There are no graphs or diagrams in the provided image, only text. Therefore, we'll proceed directly with the text transcription suitable for an educational website.
### Solution:
#### (a) Calculate \( K_p \).
1. **Initial Information:**
- Initial pressure of \( \text{N}_2\text{O}_4 \): 1.00 atm
- Percent dissociation to \( \text{NO}_2 \): 20.0%
2. **Write the dissociation reaction:**
\[
\text{N}_2\text{O}_4 (g) \leftrightarrow 2 \text{NO}_2 (g)
\]
3. **Establish equilibrium pressures:**
Since 20.0% of \( \text{N}_2\text{O}_4 \) dissociates:
- Pressure of \( \text{N}_2\text{O}_4 \) at equilibrium: \( 1.00 \text{ atm} \times (1 - 0.20) = 0.80 \text{ atm} \)
- Pressure of \( \text{NO}_2 \) at equilibrium: \( 1.00 \text{ atm} \times 0.20 \times 2 = 0.40 \text{ atm} \)
\[
\text{NO}_2 = 2 \times (\text{0.20 atm}) = 0.40 \text{ atm}
\]
4. **Calculate \( K_p \):**
\[
K_p = \frac{{(\
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 6 steps with 6 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 & Chemical Reactivity
Chemistry
ISBN:
9781133949640
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781133949640
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:
9781337399425
Author:
Steven S. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning