Consider the following system at equilibrium at 723 K: N₂(g) +3H₂(g)2NH3(g) + 26.6 kcal Indicate whether each individual change would favor the production of NH3(g). Evaluate each change separately, assuming that all other conditions remain constant. Decreasing the temperature. Decreasing the pressure. Increasing the volume. Removing NH3. Adding H₂. 00.00.
Consider the following system at equilibrium at 723 K: N₂(g) +3H₂(g)2NH3(g) + 26.6 kcal Indicate whether each individual change would favor the production of NH3(g). Evaluate each change separately, assuming that all other conditions remain constant. Decreasing the temperature. Decreasing the pressure. Increasing the volume. Removing NH3. Adding H₂. 00.00.
Chemistry
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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
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![**Consider the following system at equilibrium at 723 K:**
\[ \text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g) + 26.6 \text{ kcal} \]
*Indicate whether each individual change would favor the production of NH\(_3\)(g). Evaluate each change separately, assuming that all other conditions remain constant.*
1. **Decreasing the temperature.**
- [Dropdown menu]
2. **Decreasing the pressure.**
- [Dropdown menu]
3. **Increasing the volume.**
- [Dropdown menu]
4. **Removing NH\(_3\).**
- [Dropdown menu]
5. **Adding H\(_2\).**
- [Dropdown menu]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3bd4c942-9001-4b89-a982-59669ffeb7dd%2F306f6036-3ca8-4d44-8db2-bc5632b8b493%2F4skuasp_processed.png&w=3840&q=75)
Transcribed Image Text:**Consider the following system at equilibrium at 723 K:**
\[ \text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g) + 26.6 \text{ kcal} \]
*Indicate whether each individual change would favor the production of NH\(_3\)(g). Evaluate each change separately, assuming that all other conditions remain constant.*
1. **Decreasing the temperature.**
- [Dropdown menu]
2. **Decreasing the pressure.**
- [Dropdown menu]
3. **Increasing the volume.**
- [Dropdown menu]
4. **Removing NH\(_3\).**
- [Dropdown menu]
5. **Adding H\(_2\).**
- [Dropdown menu]
![Consider the following system at equilibrium at 723 K:
\[ 2 \, \text{NH}_3 \, (g) + 26.6 \, \text{kcal} \rightleftharpoons \text{N}_2 \, (g) + 3 \, \text{H}_2 \, (g) \]
Indicate whether each individual change would favor the production of \(\text{N}_2 \, (g)\). Evaluate each change separately, assuming that all other conditions remain constant.
- Decreasing the temperature:
- [Dropdown for response]
- Decreasing the pressure:
- [Dropdown for response]
- Increasing the volume:
- [Dropdown for response]
- Removing \(\text{NH}_3\):
- [Dropdown for response]
- Removing \(\text{H}_2\):
- [Dropdown for response]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3bd4c942-9001-4b89-a982-59669ffeb7dd%2F306f6036-3ca8-4d44-8db2-bc5632b8b493%2F9krmzbb_processed.png&w=3840&q=75)
Transcribed Image Text:Consider the following system at equilibrium at 723 K:
\[ 2 \, \text{NH}_3 \, (g) + 26.6 \, \text{kcal} \rightleftharpoons \text{N}_2 \, (g) + 3 \, \text{H}_2 \, (g) \]
Indicate whether each individual change would favor the production of \(\text{N}_2 \, (g)\). Evaluate each change separately, assuming that all other conditions remain constant.
- Decreasing the temperature:
- [Dropdown for response]
- Decreasing the pressure:
- [Dropdown for response]
- Increasing the volume:
- [Dropdown for response]
- Removing \(\text{NH}_3\):
- [Dropdown for response]
- Removing \(\text{H}_2\):
- [Dropdown for response]
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Step 1: Le-chatalier's principle!
VIEWStep 2: Effect of temperature change on equilibrium!
VIEWStep 3: Effect of pressure change on equilibrium!
VIEWStep 4: Effect of volume change on equilibrium!
VIEWStep 5: Effect of ammonia removal on equilibrium!
VIEWStep 6: Effect of hydrogen addition on equilibrium!
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