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20. Nitrogen monoxide can be synthesized by combining nitrogen and oxygen under certain conditions: N2(g) + O2(g) 2NO(g) At 1500K, the reaction has an equilibrium constant of 1.10x10-5. If air is pumped into a reaction vessel up to a pressure of 85.0 atm, what will be the partial pressure of NO at equilibrium? (Assume that air is 80% nitrogen and 20% oxygen). 2 PN²

20. Nitrogen monoxide can be synthesized by combining nitrogen and oxygen under certain conditions: N2(g) + O2(g) 2NO(g) At 1500K, the reaction has an equilibrium constant of 1.10x10-5. If air is pumped into a reaction vessel up to a pressure of 85.0 atm, what will be the partial pressure of NO at equilibrium? (Assume that air is 80% nitrogen and 20% oxygen). 2 PN²

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section: Chapter Questions
Problem 5PS: A mixture of SO2, O2, and SO3 at 1000 K contains the gases at the following concentrations: [SO2] =...
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20. Nitrogen monoxide can be synthesized by combining nitrogen and oxygen under certain conditions: N2(g) + O2(g) 2NO(g) At 1500K, the reaction has an equilibrium constant of 1.10x10-5. If air is pumped into a reaction vessel up to a pressure of 85.0 atm, what will be the partial pressure of NO at equilibrium? (Assume that air is 80% nitrogen and 20% oxygen). 2 PN²
Transcribed Image Text:20. Nitrogen monoxide can be synthesized by combining nitrogen and oxygen under certain conditions: N2(g) + O2(g) 2NO(g) At 1500K, the reaction has an equilibrium constant of 1.10x10-5. If air is pumped into a reaction vessel up to a pressure of 85.0 atm, what will be the partial pressure of NO at equilibrium? (Assume that air is 80% nitrogen and 20% oxygen). 2 PN²
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