Nitric oxide, an important pollutant in air, is formed from the elements nitrogen and oxygen at high temperatures, such as those obtained when gasoline burns in an automobile engine. At 2000°C, K for the reaction N2(g) + O2(g) ⇆ 2NO(g) is 0.010. If 0.40 moles of N2, 0.10 moles of O2, and 0.080 moles of NO are placed in a 1.0-liter container, what will be the concentration of O2 at equilibrium?
Nitric oxide, an important pollutant in air, is formed from the elements nitrogen and oxygen at high temperatures, such as those obtained when gasoline burns in an automobile engine. At 2000°C, K for the reaction N2(g) + O2(g) ⇆ 2NO(g) is 0.010. If 0.40 moles of N2, 0.10 moles of O2, and 0.080 moles of NO are placed in a 1.0-liter container, what will be the concentration of O2 at equilibrium?
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter17: Chemcial Thermodynamics
Section: Chapter Questions
Problem 17.20QE: The equilibrium constant for a reaction decreases as temperature increases. Explain how this...
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Nitric oxide, an important pollutant in air, is formed from the elements nitrogen and oxygen at high temperatures, such as those obtained when gasoline burns in an automobile engine.
At 2000°C, K for the reaction N2(g) + O2(g) ⇆ 2NO(g) is 0.010. If 0.40 moles of N2, 0.10 moles of O2, and 0.080 moles of NO are placed in a 1.0-liter container, what will be the concentration of O2 at equilibrium?
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