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Nitrogen monoxide and hydrogen react to form nitrogen and water, like this: 2 NO(g) + 2 H₂(g) → N₂(g) + 2H₂O(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of nitrogen monoxide, hydrogen, nitrogen, and water has the following composition: compound pressure at equilibrium NO 66.9 atm 58.6 atm H₂ N₂ H₂O 7.70 atm K₂ = 0 51.0 atm Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. X 3

Nitrogen monoxide and hydrogen react to form nitrogen and water, like this: 2 NO(g) + 2 H₂(g) → N₂(g) + 2H₂O(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of nitrogen monoxide, hydrogen, nitrogen, and water has the following composition: compound pressure at equilibrium NO 66.9 atm 58.6 atm H₂ N₂ H₂O 7.70 atm K₂ = 0 51.0 atm Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. X 3

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter12: Gaseous Chemical Equilibrium
Section: Chapter Questions
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Nitrogen monoxide and hydrogen react to form nitrogen and water, like this: 2 NO(g) + 2 H₂(g) → N₂(g) + 2 H₂O(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of nitrogen monoxide, hydrogen, nitrogen, and water has the following composition: compound pressure at equilibrium NO 66.9 atm H₂ N₂ H₂O K 58.6 atm 0 7.70 atm Calculate the value of the equilibrium constant for this reaction. Round your answer to 2 significant digits. P 51.0 atm 0 x10 X
Transcribed Image Text:Nitrogen monoxide and hydrogen react to form nitrogen and water, like this: 2 NO(g) + 2 H₂(g) → N₂(g) + 2 H₂O(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of nitrogen monoxide, hydrogen, nitrogen, and water has the following composition: compound pressure at equilibrium NO 66.9 atm H₂ N₂ H₂O K 58.6 atm 0 7.70 atm Calculate the value of the equilibrium constant for this reaction. Round your answer to 2 significant digits. P 51.0 atm 0 x10 X
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