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N2(g) + O2(g) ⇌ 2NO(g) If N2(g) and O2(g) are placed in a flask at a constant temperature with the initial pressures of PN2 = 0.78 atm and PO2 = 0.21 atm, the equilibrium pressure of NO(g) that forms is PNO = 1.7 x 10-2 atm. What is the value of Kp?

N2(g) + O2(g) ⇌ 2NO(g) If N2(g) and O2(g) are placed in a flask at a constant temperature with the initial pressures of PN2 = 0.78 atm and PO2 = 0.21 atm, the equilibrium pressure of NO(g) that forms is PNO = 1.7 x 10-2 atm. What is the value of Kp?

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 36QAP: At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s),...
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N2(g) + O2(g) ⇌ 2NO(g)

If N2(g) and O2(g) are placed in a flask at a constant temperature with the initial pressures of PN2 = 0.78 atm and PO2 = 0.21 atm, the equilibrium pressure of NO(g) that forms is PNO = 1.7 x 10-2 atm. What is the value of Kp?

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