Nitrogen monoxide, NO, is formed in automobile exhaust by the reaction of N₂ and O2 (from air). N₂(g) + O2(g) → 2NO(g) The equilibrium constant (K) is 0.0025 at 2127°C. If an equilibrium mixture at this temperature contains 0.019 mol N₂ and 0.013 mol O₂ per liter, what is the concentration of NO? Concentration = M
Nitrogen monoxide, NO, is formed in automobile exhaust by the reaction of N₂ and O2 (from air). N₂(g) + O2(g) → 2NO(g) The equilibrium constant (K) is 0.0025 at 2127°C. If an equilibrium mixture at this temperature contains 0.019 mol N₂ and 0.013 mol O₂ per liter, what is the concentration of NO? Concentration = M
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
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 14.86QE
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![Nitrogen monoxide, NO, is formed in automobile exhaust by the reaction of N₂ and O₂ (from air).
N2 (9) + O2(g) 2NO(g)
The equilibrium constant (Kc) is 0.0025 at 2127°C. If an equilibrium mixture at this temperature contains 0.019 mol N₂
and 0.013 mol O₂ per liter, what is the concentration of NO?
Concentration =
M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Faf922873-5540-4481-ab4e-e86a6105bdb6%2Fc47f4942-9cae-4f80-9a27-9d6213bacbde%2Ffstgiv_processed.png&w=3840&q=75)
Transcribed Image Text:Nitrogen monoxide, NO, is formed in automobile exhaust by the reaction of N₂ and O₂ (from air).
N2 (9) + O2(g) 2NO(g)
The equilibrium constant (Kc) is 0.0025 at 2127°C. If an equilibrium mixture at this temperature contains 0.019 mol N₂
and 0.013 mol O₂ per liter, what is the concentration of NO?
Concentration =
M
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