A chemist is investigating the chemical reaction system by which nitric oxide, NO(g), is converted to nitrogen, N2(g), and oxygen, O2(g): 2 NO(g) ⇌ N2(g) + O2(g) Initially she places 1.6 mol nitric oxide, 1.6 mol nitrogen, and 0.60 mol oxygen in a 1.00 L vessel. At equilibrium, she finds that the concentration of nitric oxide is 1.4 mol/L. Calculate the equilibrium constant, K, for this chemical reaction system.
A chemist is investigating the chemical reaction system by which nitric oxide, NO(g), is converted to nitrogen, N2(g), and oxygen, O2(g): 2 NO(g) ⇌ N2(g) + O2(g) Initially she places 1.6 mol nitric oxide, 1.6 mol nitrogen, and 0.60 mol oxygen in a 1.00 L vessel. At equilibrium, she finds that the concentration of nitric oxide is 1.4 mol/L. Calculate the equilibrium constant, K, for this chemical reaction system.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter19: The Chemistry Of The Main-group Elements
Section: Chapter Questions
Problem 60QRT
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A chemist is investigating the
2 NO(g) ⇌ N2(g) + O2(g)
Initially she places 1.6 mol nitric oxide, 1.6 mol nitrogen, and 0.60 mol oxygen in a 1.00 L vessel. At equilibrium, she finds that the concentration of nitric oxide is 1.4 mol/L. Calculate the equilibrium constant, K, for this chemical reaction system.
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