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Nitrogen monoxide decomposes by the following equation: 2NO(g) + N2(g) + 02(g); Kc = 2.3 x 10^30 at 298 K. In the atmosphere, PO2 = 0.209 atm and PN2 = 0.781 atm. What is the equilibrium partial pressure of NO in the air we breathe? (Hint: You need Kp to find the partial pressure.) O P (NO) = 2.7 X 10^-15 atm O P (NO) = 2.7 X 10^-14 atm O P (NO) = 2.7 X 10^-16 atm O P (NO) = 2.7 X 10^-17 atm

Nitrogen monoxide decomposes by the following equation: 2NO(g) + N2(g) + 02(g); Kc = 2.3 x 10^30 at 298 K. In the atmosphere, PO2 = 0.209 atm and PN2 = 0.781 atm. What is the equilibrium partial pressure of NO in the air we breathe? (Hint: You need Kp to find the partial pressure.) O P (NO) = 2.7 X 10^-15 atm O P (NO) = 2.7 X 10^-14 atm O P (NO) = 2.7 X 10^-16 atm O P (NO) = 2.7 X 10^-17 atm

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter12: Gaseous Chemical Equilibrium
Section: Chapter Questions
Problem 34QAP: At 500C, k for the for the formation of ammonia from nitrogen and hydrogen gases is 1.5105....
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Nitrogen monoxide decomposes by the following equation: 2NO(g) N2(g) + 02(g); Kc = 2.3 x 10^30 at 298 K. In the atmosphere, PO2 = 0.209 atm and PN2 = 0.781 atm. What is the equilibrium partial pressure of NO in the air we breathe? (Hint: You need Kp to find the partial pressure.) P (NO) = 2.7 X 10^-15 atm P (NO) = 2.7 X 10^-14 atm O P (NO) = 2.7 X 10^-16 atm O P (NO) = 2.7 X 10^-17 atm
Transcribed Image Text:Nitrogen monoxide decomposes by the following equation: 2NO(g) N2(g) + 02(g); Kc = 2.3 x 10^30 at 298 K. In the atmosphere, PO2 = 0.209 atm and PN2 = 0.781 atm. What is the equilibrium partial pressure of NO in the air we breathe? (Hint: You need Kp to find the partial pressure.) P (NO) = 2.7 X 10^-15 atm P (NO) = 2.7 X 10^-14 atm O P (NO) = 2.7 X 10^-16 atm O P (NO) = 2.7 X 10^-17 atm
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