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Nitrogen and hydrogen react to form ammonia, like this: N₂(g) + 3 H₂(g) 2 NH3(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of nitrogen, hydrogen, and ammonia has the following composition: compound pressure at equilibrium N₂ 67.1 atm H₂ NH3 Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K -0 - 43.5 atm 83.8 atm x10 X

Nitrogen and hydrogen react to form ammonia, like this: N₂(g) + 3 H₂(g) 2 NH3(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of nitrogen, hydrogen, and ammonia has the following composition: compound pressure at equilibrium N₂ 67.1 atm H₂ NH3 Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K -0 - 43.5 atm 83.8 atm x10 X

Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 15P
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Nitrogen and hydrogen react to form ammonia, like this: N₂(g) + 3 H₂(g) → 2NH3(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of nitrogen, hydrogen, and ammonia has the following composition: compound pressure at equilibrium N₂ 67.1 atm H₂ NH3 K = P 43.5 atm Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. р 0 83.8 atm x10 X Ś
Transcribed Image Text:Nitrogen and hydrogen react to form ammonia, like this: N₂(g) + 3 H₂(g) → 2NH3(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of nitrogen, hydrogen, and ammonia has the following composition: compound pressure at equilibrium N₂ 67.1 atm H₂ NH3 K = P 43.5 atm Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. р 0 83.8 atm x10 X Ś
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