Molecular nitrogen (N2) reacts with water vapor to form nitrogen monoxide (NO) and molecular hydrogen (H2). At some temperature a reaction system containing all four gases has been allowed come to equilibrium and the partial pressures of the gases are: PN2 = 0.12 atm, PH20 = 0.082, PNO = 0.55 atm, and PH2 = 0.76 atm. %3D Another system contains the same reactants and products at the following pressures: PN2 = 0.15 atm, PH20 = 0.12, PNO = 0.87 atm, and PH2 = 0.76 atm. Is this second system at equilibrium? If not, how will the reaction shift to reach equilibrium? N2(g) + 2 H20(g)= 2 NO(g) + 2 H2(g)

Molecular nitrogen (N2) reacts with water vapor to form nitrogen monoxide (NO) and molecular hydrogen (H2). At some temperature a reaction system containing all four gases has been allowed come to equilibrium and the partial pressures of the gases are: PN2 = 0.12 atm, PH20 = 0.082, PNO = 0.55 atm, and PH2 = 0.76 atm. %3D Another system contains the same reactants and products at the following pressures: PN2 = 0.15 atm, PH20 = 0.12, PNO = 0.87 atm, and PH2 = 0.76 atm. Is this second system at equilibrium? If not, how will the reaction shift to reach equilibrium? N2(g) + 2 H20(g)= 2 NO(g) + 2 H2(g)

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 56QAP: Sulfur oxychloride, SO2Cl2, decomposes to sulfur dioxide and chlorine gases. SO2Cl2(g)SO2(g)+Cl2(g)...

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