Nitrogen dioxide and water react to form nitric acid and nitrogen monoxide, like this: 3 NO₂(g) + H₂O(1)→ 2 HNO3(aq) + NO(g) At a certain temperature, a chemist finds that a 6.2 L reaction vessel containing a mixture of nitrogen dioxide, water, nitric acid, and nitrogen monoxide at equilibrium has the following composition: amount 20.9 g 235.2 g 6.6 g 16.7 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. compound NO₂ H₂O HNO 3 NO K = D x10
Nitrogen dioxide and water react to form nitric acid and nitrogen monoxide, like this: 3 NO₂(g) + H₂O(1)→ 2 HNO3(aq) + NO(g) At a certain temperature, a chemist finds that a 6.2 L reaction vessel containing a mixture of nitrogen dioxide, water, nitric acid, and nitrogen monoxide at equilibrium has the following composition: amount 20.9 g 235.2 g 6.6 g 16.7 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. compound NO₂ H₂O HNO 3 NO K = D x10
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 60QRT
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