Consider the following equilibrium: N₂O4 (8)2NO₂ (8) AG = 5.4 kJ Now suppose a reaction vessel is filled with 0.399 atm of dinitrogen tetroxide (N₂O4) at 588. °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

Consider the following equilibrium: N₂O4 (8)2NO₂ (8) AG = 5.4 kJ Now suppose a reaction vessel is filled with 0.399 atm of dinitrogen tetroxide (N₂O4) at 588. °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

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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