Nitrogen monoxide and hydrogen react to form nitrogen and water, like this: 2 NO(g) + 2H,(g) → N2(g) + 2H,O(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 65.7 atm H2 23.0 atm N2 22.5 atm H,0 70.0 atm Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits.
Nitrogen monoxide and hydrogen react to form nitrogen and water, like this: 2 NO(g) + 2H,(g) → N2(g) + 2H,O(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 65.7 atm H2 23.0 atm N2 22.5 atm H,0 70.0 atm Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits.
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 30P
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