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At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.54. The engineer charges ("fills") four reaction vessels with nitrogen monoxide and hydrogen, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions.

At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.54. The engineer charges ("fills") four reaction vessels with nitrogen monoxide and hydrogen, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions.

Introduction to General, Organic and Biochemistry
Introduction to General, Organic and Biochemistry
11th Edition
ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Chapter7: Reaction Rates And Chemical Equilibrium
Section: Chapter Questions
Problem 7.81P
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equation is 2NO(g)+2H2----> N2(g)+2H2O(g)

¹1₂(9) N₂(9)+2₂0 1₂0(9) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.54. The engineer charges ("fills") four reaction vessels with nitrogen monoxide and hydrogen, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction vessel compound pressure expected change in pressure NO 6.99 atm ↑ increase O↓ decrease O (no change) H₂ 4.60 atm ↑ increase decrease O (no change) A N₂ 3.93 atm O † increase O decrease O (no change) H₂O 7.46 atm ↑ increase O decrease O (no change) NO 6.86 atm O ↑ increase O decrease O (no change) H₂ 4.47 atm O ↑ increase O decrease O (no change) B N₂ 4.00 atm O † increase O decrease O (no change) H₂O 7.59 atm O ↑ increase O decrease O (no change) NO 5.37 atm O ↑ increase O (no change) O decrease decrease H₂ 2.98 atm ↑ increase (no change) C N₂ 4.75 atm ↑ increase O decrease (no change) H₂O 9.08 atm O † increase ↑ O↓ decrease O (no change)
Transcribed Image Text:¹1₂(9) N₂(9)+2₂0 1₂0(9) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.54. The engineer charges ("fills") four reaction vessels with nitrogen monoxide and hydrogen, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction vessel compound pressure expected change in pressure NO 6.99 atm ↑ increase O↓ decrease O (no change) H₂ 4.60 atm ↑ increase decrease O (no change) A N₂ 3.93 atm O † increase O decrease O (no change) H₂O 7.46 atm ↑ increase O decrease O (no change) NO 6.86 atm O ↑ increase O decrease O (no change) H₂ 4.47 atm O ↑ increase O decrease O (no change) B N₂ 4.00 atm O † increase O decrease O (no change) H₂O 7.59 atm O ↑ increase O decrease O (no change) NO 5.37 atm O ↑ increase O (no change) O decrease decrease H₂ 2.98 atm ↑ increase (no change) C N₂ 4.75 atm ↑ increase O decrease (no change) H₂O 9.08 atm O † increase ↑ O↓ decrease O (no change)
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