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Ammonia is synthesized from nitrogen and hydrogen in the reaction:  N2(g)  +  3H2(g)  <-->  2NH3(g). At 500oC, the equilibrium constant for this reaction is 0.080.  Given that you have reacted 2.5 moles of Nitrogen gas with 1.75 moles of hydrogen gas, and you produced 1 mole of ammonia gas in a 2.5L flask, is the reaction at equilibrium? If not, in what direction will it tend?

Ammonia is synthesized from nitrogen and hydrogen in the reaction:  N2(g)  +  3H2(g)  <-->  2NH3(g). At 500oC, the equilibrium constant for this reaction is 0.080.  Given that you have reacted 2.5 moles of Nitrogen gas with 1.75 moles of hydrogen gas, and you produced 1 mole of ammonia gas in a 2.5L flask, is the reaction at equilibrium? If not, in what direction will it tend?

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.18PAE: The reaction, 3 H2(g) + N2(g) (g), has the fol lowing equilibrium constants at the temperatures...
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Ammonia is synthesized from nitrogen and hydrogen in the reaction:  N2(g)  +  3H2(g)  <-->  2NH3(g). At 500oC, the equilibrium constant for this reaction is 0.080.  Given that you have reacted 2.5 moles of Nitrogen gas with 1.75 moles of hydrogen gas, and you produced 1 mole of ammonia gas in a 2.5L flask, is the reaction at equilibrium? If not, in what direction will it tend? 

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