Consider the following equilibrium: N₂O4 (8) 2NO₂ (g) AGⓇ = 5.4 kJ = Now suppose a reaction vessel is filled with 9.54 atm of dinitrogen tetroxide (N₂04) at 858. °C. Answer the following questions about this s Under these conditions, will the pressure of N₂O4 tend to rise or fall? Is it possible to reverse this tendency by adding NO₂? In other words, if you said the pressure of N₂O4 will tend to rise, can that be changed to a tendency to fall by adding NO₂? Similarly, if you said the pressure of N₂O4 will tend to fall, can that be changed to a tendency to rise by adding NO₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO₂ needed to reverse it. Round your answer to 2 significant digits. Orise O fall O yes O no atm 0 x10 X
Consider the following equilibrium: N₂O4 (8) 2NO₂ (g) AGⓇ = 5.4 kJ = Now suppose a reaction vessel is filled with 9.54 atm of dinitrogen tetroxide (N₂04) at 858. °C. Answer the following questions about this s Under these conditions, will the pressure of N₂O4 tend to rise or fall? Is it possible to reverse this tendency by adding NO₂? In other words, if you said the pressure of N₂O4 will tend to rise, can that be changed to a tendency to fall by adding NO₂? Similarly, if you said the pressure of N₂O4 will tend to fall, can that be changed to a tendency to rise by adding NO₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO₂ needed to reverse it. Round your answer to 2 significant digits. Orise O fall O yes O no atm 0 x10 X
Consider the following equilibrium: N₂O4 (8) 2NO₂ (g) AGⓇ = 5.4 kJ = Now suppose a reaction vessel is filled with 9.54 atm of dinitrogen tetroxide (N₂04) at 858. °C. Answer the following questions about this s Under these conditions, will the pressure of N₂O4 tend to rise or fall? Is it possible to reverse this tendency by adding NO₂? In other words, if you said the pressure of N₂O4 will tend to rise, can that be changed to a tendency to fall by adding NO₂? Similarly, if you said the pressure of N₂O4 will tend to fall, can that be changed to a tendency to rise by adding NO₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO₂ needed to reverse it. Round your answer to 2 significant digits. Orise O fall O yes O no atm 0 x10 X
Answer the following questions based on the given information about this chemical reaction.
Transcribed Image Text:**Consider the following equilibrium:**
\[ \text{N}_2\text{O}_4 (g) \rightleftharpoons 2\text{NO}_2 (g) \quad \Delta G^0 = 5.4 \, \text{kJ} \]
Now suppose a reaction vessel is filled with 9.54 atm of dinitrogen tetroxide (\(\text{N}_2\text{O}_4\)) at 858°C. Answer the following questions about this system:
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**Under these conditions, will the pressure of \(\text{N}_2\text{O}_4\) tend to rise or fall?**
- Rise (selected)
- Fall
---
**Is it possible to reverse this tendency by adding \(\text{NO}_2\)?**
In other words, if you said the pressure of \(\text{N}_2\text{O}_4\) will tend to rise, can that be changed to a tendency to fall by adding \(\text{NO}_2\)? Similarly, if you said the pressure of \(\text{N}_2\text{O}_4\) will tend to fall, can that be changed to a tendency to rise by adding \(\text{NO}_2\)?
- Yes
- No
---
**If you said the tendency can be reversed in the second question, calculate the minimum pressure of \(\text{NO}_2\) needed to reverse it.**
Round your answer to 2 significant digits.
\[\_\_\_\_\] atm
---
**Additional Diagram:**
There is a small interactive calculator box on the right with options for numerical input and basic operations like clear and reset. This implies students are expected to calculate values actively as part of the exercise.
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.
Expert Solution
Step 1
Here the equilibrium reaction is dissociation of N2O4 to NO2 at 858°C. The initial pressure of N2O4 is 9.54 atm .we have to predict whether the pressure of N2O4 will increase or decrease and what minimum pressure the reaction will reverse its direction.
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![**Consider the following equilibrium:**
\[ \text{N}_2\text{O}_4 (g) \rightleftharpoons 2\text{NO}_2 (g) \quad \Delta G^0 = 5.4 \, \text{kJ} \]
Now suppose a reaction vessel is filled with 9.54 atm of dinitrogen tetroxide (\(\text{N}_2\text{O}_4\)) at 858°C. Answer the following questions about this system:
---
**Under these conditions, will the pressure of \(\text{N}_2\text{O}_4\) tend to rise or fall?**
- Rise (selected)
- Fall
---
**Is it possible to reverse this tendency by adding \(\text{NO}_2\)?**
In other words, if you said the pressure of \(\text{N}_2\text{O}_4\) will tend to rise, can that be changed to a tendency to fall by adding \(\text{NO}_2\)? Similarly, if you said the pressure of \(\text{N}_2\text{O}_4\) will tend to fall, can that be changed to a tendency to rise by adding \(\text{NO}_2\)?
- Yes
- No
---
**If you said the tendency can be reversed in the second question, calculate the minimum pressure of \(\text{NO}_2\) needed to reverse it.**
Round your answer to 2 significant digits.
\[\_\_\_\_\] atm
---
**Additional Diagram:**
There is a small interactive calculator box on the right with options for numerical input and basic operations like clear and reset. This implies students are expected to calculate values actively as part of the exercise.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F87896b23-33e0-4e58-a967-e6f5a2b8fe91%2F22edef10-02b9-4cb9-80db-126476aa5ecf%2Fs8kza8i_processed.png&w=3840&q=75)
