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Consider the following equilibrium: 2NO₂ (g)-N₂O4 (g) AG=-5.4 kJ Now suppose a reaction vessel is filled with 1.20 atm of nitrogen dioxide (NO₂) at 802. °C. Answer the following questions about this system: Under these conditions, will the pressure of NO₂ tend to rise or fall? Is it possible to reverse this tendency by adding N₂O4? In other words, if you said the pressure of NO₂ will tend to rise, can that be changed to a tendency to fall by adding N₂O? Similarly, if you said the pressure of NO₂ will tend to fall, can that be changed to a tendency to rise by adding N₂04? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂O4 needed to reverse it. Round your answer to 2 significant digits. Orise O fall O yes O no atm 0 10 X S

Consider the following equilibrium: 2NO₂ (g)-N₂O4 (g) AG=-5.4 kJ Now suppose a reaction vessel is filled with 1.20 atm of nitrogen dioxide (NO₂) at 802. °C. Answer the following questions about this system: Under these conditions, will the pressure of NO₂ tend to rise or fall? Is it possible to reverse this tendency by adding N₂O4? In other words, if you said the pressure of NO₂ will tend to rise, can that be changed to a tendency to fall by adding N₂O? Similarly, if you said the pressure of NO₂ will tend to fall, can that be changed to a tendency to rise by adding N₂04? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂O4 needed to reverse it. Round your answer to 2 significant digits. Orise O fall O yes O no atm 0 10 X S

Chemistry
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
Chapter1: Chemical Foundations
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Consider the following equilibrium: 2NO₂ (g) N₂O4 (g) Now suppose a reaction vessel is filled with 1.20 atm of nitrogen dioxide (NO₂) at 802. °C. Answer the following questions about this system: AG= = -5.4 kJ Under these conditions, will the pressure of NO₂ tend to rise or fall? Is it possible to reverse this tendency by adding N₂O4? In other words, if you said the pressure of NO₂ will tend to rise, can that be changed to a tendency to fall by adding N₂O4? Similarly, if you said the pressure of NO2 will tend to fall, can that be changed to a tendency to rise by adding N₂04? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂O4 needed to reverse it. Round your answer to 2 significant digits. Orise Ofall O yes O no atm x10 X
Transcribed Image Text:Consider the following equilibrium: 2NO₂ (g) N₂O4 (g) Now suppose a reaction vessel is filled with 1.20 atm of nitrogen dioxide (NO₂) at 802. °C. Answer the following questions about this system: AG= = -5.4 kJ Under these conditions, will the pressure of NO₂ tend to rise or fall? Is it possible to reverse this tendency by adding N₂O4? In other words, if you said the pressure of NO₂ will tend to rise, can that be changed to a tendency to fall by adding N₂O4? Similarly, if you said the pressure of NO2 will tend to fall, can that be changed to a tendency to rise by adding N₂04? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂O4 needed to reverse it. Round your answer to 2 significant digits. Orise Ofall O yes O no atm x10 X
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