Suggest four ways in which the concentration of PH3 could be increased in an equilibrium described by the following equation: P4 (g) + 6H₂ (8)= 4PH3 (8) ΔΗ= 110 5 kJ
Suggest four ways in which the concentration of PH3 could be increased in an equilibrium described by the following equation: P4 (g) + 6H₂ (8)= 4PH3 (8) ΔΗ= 110 5 kJ
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
![**Ways to Increase the Concentration of PH₃ in an Equilibrium Reaction**
In a chemical equilibrium reaction described by the equation:
\[ \mathbf{P_4 (g) + 6H_2 (g) \leftrightarrow 4PH_3 (g)} \]
with \( \Delta H = 110.5 \text{ kJ} \),
there are several strategies to increase the concentration of phosphine (PH₃). Here are four ways to achieve this:
1. **Increase the Pressure:**
- In gaseous reactions, increasing the pressure tends to favor the side of the equilibrium with fewer gas molecules.
- Here, 7 moles of gas (1 mole of P₄ and 6 moles of H₂) turn into 4 moles of PH₃ gas. Increasing the pressure will shift the equilibrium to the right, favoring the production of PH₃.
2. **Decrease the Temperature:**
- The given reaction has a positive ΔH value, indicating that it is endothermic.
- Lowering the temperature will shift the equilibrium position to the right to counteract the removal of heat, therefore increasing the formation of PH₃.
3. **Increase the Concentration of Reactants:**
- According to Le Chatelier's Principle, increasing the concentration of the reactants (P₄ or H₂) will shift the equilibrium toward the products to counterbalance the change.
- Therefore, by adding more P₄ or H₂, the system will produce more PH₃.
4. **Remove PH₃ as it Forms:**
- Continuously removing PH₃ gas from the reaction vessel as it forms will shift the equilibrium to the right, promoting the formation of more PH₃.
- This can be done using various separation techniques such as condensation or absorption.
By employing these strategies, the concentration of PH₃ in the equilibrium system can be increased.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff90913a8-510d-485a-8226-8a0b61f2c858%2F207e99b5-2dbe-4842-bee0-b6e4ee09b899%2Fp9mxcod_processed.png&w=3840&q=75)
Transcribed Image Text:**Ways to Increase the Concentration of PH₃ in an Equilibrium Reaction**
In a chemical equilibrium reaction described by the equation:
\[ \mathbf{P_4 (g) + 6H_2 (g) \leftrightarrow 4PH_3 (g)} \]
with \( \Delta H = 110.5 \text{ kJ} \),
there are several strategies to increase the concentration of phosphine (PH₃). Here are four ways to achieve this:
1. **Increase the Pressure:**
- In gaseous reactions, increasing the pressure tends to favor the side of the equilibrium with fewer gas molecules.
- Here, 7 moles of gas (1 mole of P₄ and 6 moles of H₂) turn into 4 moles of PH₃ gas. Increasing the pressure will shift the equilibrium to the right, favoring the production of PH₃.
2. **Decrease the Temperature:**
- The given reaction has a positive ΔH value, indicating that it is endothermic.
- Lowering the temperature will shift the equilibrium position to the right to counteract the removal of heat, therefore increasing the formation of PH₃.
3. **Increase the Concentration of Reactants:**
- According to Le Chatelier's Principle, increasing the concentration of the reactants (P₄ or H₂) will shift the equilibrium toward the products to counterbalance the change.
- Therefore, by adding more P₄ or H₂, the system will produce more PH₃.
4. **Remove PH₃ as it Forms:**
- Continuously removing PH₃ gas from the reaction vessel as it forms will shift the equilibrium to the right, promoting the formation of more PH₃.
- This can be done using various separation techniques such as condensation or absorption.
By employing these strategies, the concentration of PH₃ in the equilibrium system can be increased.
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.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 1 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