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Hydrogen lodide decomposes to form hydrogen and lodine, like this: 2 HI(g) → H₂(g) + L₂(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen iodide, hydrogen, and lodine has the following composition: ? compound pressure at equilibrium HI 31.0 atm H₂ 20.7 atm 12 58.5 atm Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K₁ = 0 0.0 X 3 ol Ar

Hydrogen lodide decomposes to form hydrogen and lodine, like this: 2 HI(g) → H₂(g) + L₂(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen iodide, hydrogen, and lodine has the following composition: ? compound pressure at equilibrium HI 31.0 atm H₂ 20.7 atm 12 58.5 atm Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K₁ = 0 0.0 X 3 ol Ar

Chemistry
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
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Hydrogen lodide decomposes to form hydrogen and lodine, like this: 2 HI(g) → H₂(g) + L₂(g) - Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen iodide, hydrogen, and lodine has the following composition: ? compound pressure at equilibrium HI 31.0 atm H₂ 20.7 atm 12₂2 58.5 atm Calculate the value of the equilibrium constant. K, = 0 nstant K for this reaction. Round your answer to 2 significant digits. 0.0 X 5 FEED ola Ar
Transcribed Image Text:Hydrogen lodide decomposes to form hydrogen and lodine, like this: 2 HI(g) → H₂(g) + L₂(g) - Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen iodide, hydrogen, and lodine has the following composition: ? compound pressure at equilibrium HI 31.0 atm H₂ 20.7 atm 12₂2 58.5 atm Calculate the value of the equilibrium constant. K, = 0 nstant K for this reaction. Round your answer to 2 significant digits. 0.0 X 5 FEED ola Ar
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