Consider the following equilibrium:N₂ (g) + 3H₂ (g) 2NH3 (g)AG=-34. KJNow suppose a reaction vessel filled with 3.73 atm of nitrogen (N₂) and 1.60 atm of ammonia (NH3) at 493. °C. Answer the following questions about thissystem:Under these conditions, will the pressure of N, tend to rise or fall?Is it possible to reverse this tendency by adding H₂?In other words, if you said the pressure of N₂ will tend to rise, can that bechanged to a tendency to fall by adding H₂? Similarly, if you said thepressure of N₂ will tend to fall, can that be changed to a tendency to riseby adding H₂?If you said the tendency can be reversed in the second question, calculatethe minimum pressure of H₂ needed to reverse it.Round your answer tosignificant digits.ⒸrisefallO yesO noatmX S ?doÄr

Answered: Image /qna-images/answer/a0f5a153-7887-43eb-84b2-3e75d09f7543.jpg

sider the following equilibrium: N₂ (g) +3H₂ (g)2NH₂ (g) AG=-34. KJ suppose a reaction vessel is filled with 3.73 atm of nitrogen (N₂) and 1.60 atm of ammonia (NH3) at 493. °C. Answer the following questions about this cem:

sider the following equilibrium: N₂ (g) +3H₂ (g)2NH₂ (g) AG=-34. KJ suppose a reaction vessel is filled with 3.73 atm of nitrogen (N₂) and 1.60 atm of ammonia (NH3) at 493. °C. Answer the following questions about this cem:

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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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