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
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ISBN:9781305957404
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Chapter1: Chemical Foundations
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![2. 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 to come to equilibrium, and the partial pressures of the gases are: Pₙ₂ = 0.12 atm, Pₕ₂ₒ = 0.082 atm, Pₙₒ = 0.55 atm, and Pₕ₂ = 0.76 atm. Another system contains the same reactants and products at the following pressures: Pₙ₂ = 0.15 atm, Pₕ₂ₒ = 0.12 atm, 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?
\[ N_2(g) + 2 \, H_2O(g) \rightleftharpoons 2 \, NO(g) + 2 \, H_2(g) \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb4bda451-1bcc-473c-9a91-77116df85d00%2F6e7ebb1c-db3e-4322-9029-8981c470a3dc%2Fdv2ts8a_processed.jpeg&w=3840&q=75)
Transcribed Image Text:2. 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 to come to equilibrium, and the partial pressures of the gases are: Pₙ₂ = 0.12 atm, Pₕ₂ₒ = 0.082 atm, Pₙₒ = 0.55 atm, and Pₕ₂ = 0.76 atm. Another system contains the same reactants and products at the following pressures: Pₙ₂ = 0.15 atm, Pₕ₂ₒ = 0.12 atm, 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?
\[ N_2(g) + 2 \, H_2O(g) \rightleftharpoons 2 \, NO(g) + 2 \, H_2(g) \]
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