Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![**Consider the following equilibrium:**
\[ 2\text{NH}_3 (g) \rightleftharpoons \text{N}_2 (g) + 3\text{H}_2 (g) \quad \Delta G^0 = 34. \text{kJ} \]
Now suppose a reaction vessel is filled with 6.47 atm of ammonia (\(\text{NH}_3\)) and 9.96 atm of nitrogen (\(\text{N}_2\)) at 10. °C. Answer the following questions about this system:
1. **Under these conditions, will the pressure of \(\text{NH}_3\) tend to rise or fall?**
- [ ] rise
- [x] fall
2. **Is it possible to reverse this tendency by adding \(\text{H}_2\)?**
In other words, if you said the pressure of \(\text{NH}_3\) will tend to rise, can that be changed to a tendency to fall by adding \(\text{H}_2\)? Similarly, if you said the pressure of \(\text{NH}_3\) will tend to fall, can that be changed to a tendency to rise by adding \(\text{H}_2\)?
- [x] yes
- [ ] no
3. **If you said the tendency can be reversed in the second question, calculate the minimum pressure of \(\text{H}_2\) needed to reverse it.**
Round your answer to 2 significant digits.
\(\boxed{\phantom{0}} \, \text{atm}\)](https://content.bartleby.com/qna-images/question/ba5985c8-0471-4fef-a4a8-b2bc52598737/08712ffc-ce73-405d-a9b9-58004be7be59/hxy1inw_processed.png)
Transcribed Image Text:**Consider the following equilibrium:**
\[ 2\text{NH}_3 (g) \rightleftharpoons \text{N}_2 (g) + 3\text{H}_2 (g) \quad \Delta G^0 = 34. \text{kJ} \]
Now suppose a reaction vessel is filled with 6.47 atm of ammonia (\(\text{NH}_3\)) and 9.96 atm of nitrogen (\(\text{N}_2\)) at 10. °C. Answer the following questions about this system:
1. **Under these conditions, will the pressure of \(\text{NH}_3\) tend to rise or fall?**
- [ ] rise
- [x] fall
2. **Is it possible to reverse this tendency by adding \(\text{H}_2\)?**
In other words, if you said the pressure of \(\text{NH}_3\) will tend to rise, can that be changed to a tendency to fall by adding \(\text{H}_2\)? Similarly, if you said the pressure of \(\text{NH}_3\) will tend to fall, can that be changed to a tendency to rise by adding \(\text{H}_2\)?
- [x] yes
- [ ] no
3. **If you said the tendency can be reversed in the second question, calculate the minimum pressure of \(\text{H}_2\) needed to reverse it.**
Round your answer to 2 significant digits.
\(\boxed{\phantom{0}} \, \text{atm}\)
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