Consider the following equilibrium: N₂O4 (g)2NO₂ (g) AG=5.4 kJ Now suppose a reaction vessel is filled with 4.22 atm of dinitrogen tetroxide (N₂O4) at 725. °C. Answer the following questions about this system: 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 X
Consider the following equilibrium: N₂O4 (g)2NO₂ (g) AG=5.4 kJ Now suppose a reaction vessel is filled with 4.22 atm of dinitrogen tetroxide (N₂O4) at 725. °C. Answer the following questions about this system: 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 X
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
Chapter13: Chemical Equilibrium
Section: Chapter Questions
Problem 23Q: Consider the reaction 2N2O(g) + O2(g) 4NO(g) Suppose the system is at equilibrium, and then an...
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Ll.64.
![Consider the following equilibrium:
N₂O4 (g) → 2NO₂ (8)
AG = 5.4 kJ
Now suppose a reaction vessel is filled with 4.22 atm of dinitrogen tetroxide (N₂O4) at 725. °C. Answer the following questions about this system:
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.
rise
O
O fall
O yes
O no
atm
04.0
X
S](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0ac4d88e-5f8e-43f5-ab0c-487ee1683169%2F0b8b1a72-bfbd-4ab8-b71c-78f0ef4f08a7%2F31dl1j7_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Consider the following equilibrium:
N₂O4 (g) → 2NO₂ (8)
AG = 5.4 kJ
Now suppose a reaction vessel is filled with 4.22 atm of dinitrogen tetroxide (N₂O4) at 725. °C. Answer the following questions about this system:
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.
rise
O
O fall
O yes
O no
atm
04.0
X
S
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