Consider the following equilibrium: 2NO(g) + Cl₂ (g) → 2NOCI (g) AGO = -41. KJ Now suppose a reaction vessel is filled with 7.97 atm of nitrogen monoxide (NO) and 9.76 atm of nitrosyl chloride (NOCI) at 1094. °C. Answer the following questions about this system: Under these conditions, will the pressure of NOCI tend to rise or fall? Is it possible to reverse this tendency by adding Cl₂? In other words, if you said the pressure of NOCI will tend to rise, can that be changed to a tendency to fall by adding Cl₂? Similarly, if you said the pressure of NOCI will tend to fall, can that be changed to a tendency to rise by adding Cl₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of Cl, needed to reverse it. Round your answer to 2 significant digits. rise O fall O yes O no atm Ox X
Consider the following equilibrium: 2NO(g) + Cl₂ (g) → 2NOCI (g) AGO = -41. KJ Now suppose a reaction vessel is filled with 7.97 atm of nitrogen monoxide (NO) and 9.76 atm of nitrosyl chloride (NOCI) at 1094. °C. Answer the following questions about this system: Under these conditions, will the pressure of NOCI tend to rise or fall? Is it possible to reverse this tendency by adding Cl₂? In other words, if you said the pressure of NOCI will tend to rise, can that be changed to a tendency to fall by adding Cl₂? Similarly, if you said the pressure of NOCI will tend to fall, can that be changed to a tendency to rise by adding Cl₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of Cl, needed to reverse it. Round your answer to 2 significant digits. rise O fall O yes O no atm Ox X
Consider the following equilibrium: 2NO(g) + Cl₂ (g) → 2NOCI (g) AGO = -41. KJ Now suppose a reaction vessel is filled with 7.97 atm of nitrogen monoxide (NO) and 9.76 atm of nitrosyl chloride (NOCI) at 1094. °C. Answer the following questions about this system: Under these conditions, will the pressure of NOCI tend to rise or fall? Is it possible to reverse this tendency by adding Cl₂? In other words, if you said the pressure of NOCI will tend to rise, can that be changed to a tendency to fall by adding Cl₂? Similarly, if you said the pressure of NOCI will tend to fall, can that be changed to a tendency to rise by adding Cl₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of Cl, needed to reverse it. Round your answer to 2 significant digits. rise O fall O yes O no atm Ox X
Answer the following questions about the system given the chemical reaction below.
Transcribed Image Text:## Equilibrium Analysis
Consider the following equilibrium reaction:
\[
2 \text{NO (g)} + \text{Cl}_2 \text{(g)} \rightleftharpoons 2 \text{NOCl (g)} \quad \Delta G^0 = -41. \text{kJ}
\]
A reaction vessel is filled with 7.97 atm of nitrogen monoxide (NO) and 9.76 atm of nitrosyl chloride (NOCl) at 1094°C. Analyze the system with the following questions:
### Questions to Consider:
1. **Tendency of NOCl Pressure:**
- Under these conditions, will the pressure of NOCl tend to rise or fall?
- [X] rise
- [ ] fall
2. **Reversal with Cl₂ Addition:**
- Is reversing this tendency possible by adding Cl₂?
- In other words, if the pressure of NOCl tends to rise, can it be changed to a fall by adding Cl₂? Conversely, if NOCl tends to fall, can it be reversed to rise by adding Cl₂?
- [ ] yes
- [X] no
3. **Calculation (if applicable):**
- If you determined that the tendency can be reversed in the second question, calculate the minimum pressure of Cl₂ needed to reverse it. (Round your answer to 2 significant digits.)
- \[ \boxed{\phantom{0} } \text{ atm} \]
### Checkbox Legend:
- Small checkbox, unchecked.
- Circle checkbox as selected in "rise" for the tendency of NOCl to rise.
- Small "x" and reload icon indicating calculation options (irrelevant to the transcription focus).
Definition Definition Transformation of a chemical species into another chemical species. A chemical reaction consists of breaking existing bonds and forming new ones by changing the position of electrons. These reactions are best explained using a chemical equation.
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![## Equilibrium Analysis
Consider the following equilibrium reaction:
\[
2 \text{NO (g)} + \text{Cl}_2 \text{(g)} \rightleftharpoons 2 \text{NOCl (g)} \quad \Delta G^0 = -41. \text{kJ}
\]
A reaction vessel is filled with 7.97 atm of nitrogen monoxide (NO) and 9.76 atm of nitrosyl chloride (NOCl) at 1094°C. Analyze the system with the following questions:
### Questions to Consider:
1. **Tendency of NOCl Pressure:**
- Under these conditions, will the pressure of NOCl tend to rise or fall?
- [X] rise
- [ ] fall
2. **Reversal with Cl₂ Addition:**
- Is reversing this tendency possible by adding Cl₂?
- In other words, if the pressure of NOCl tends to rise, can it be changed to a fall by adding Cl₂? Conversely, if NOCl tends to fall, can it be reversed to rise by adding Cl₂?
- [ ] yes
- [X] no
3. **Calculation (if applicable):**
- If you determined that the tendency can be reversed in the second question, calculate the minimum pressure of Cl₂ needed to reverse it. (Round your answer to 2 significant digits.)
- \[ \boxed{\phantom{0} } \text{ atm} \]
### Checkbox Legend:
- Small checkbox, unchecked.
- Circle checkbox as selected in "rise" for the tendency of NOCl to rise.
- Small "x" and reload icon indicating calculation options (irrelevant to the transcription focus).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F87896b23-33e0-4e58-a967-e6f5a2b8fe91%2F8c5bacf7-ea6f-4072-b5a3-7d3dfc84b295%2Fjsqmndt_processed.png&w=3840&q=75)
