A chemical engineer is studying the following reaction: 4 HCl(g)+O,(g) –→ 2 H,O(g)+2Cl,(9) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.22. The engineer charges ("fills") four reaction vessels with hydrogen chloride and oxygen, 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 compound pressure expected change in pressure vessel HCI 4.88 atm Olt increase O Į decrease O (no change) O2 0, 8.21 atm O t increase O I decrease O (no change) A H,0 5.94 atm O t increase O I decrease O (no change) Cl, 5.44 atm O f increase O Į decrease O (no change) HCI 6.03 atm O t increase O Į decrease O (no change) 7.78 atm O t increase O I decrease O (no change) В H,0 4.37 atm O t increase O I decrease O (no change) CL, 3.93 atm O t increase O I decrease O (no change)

A chemical engineer is studying the following reaction: 4 HCl(g)+O,(g) –→ 2 H,O(g)+2Cl,(9) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.22. The engineer charges ("fills") four reaction vessels with hydrogen chloride and oxygen, 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 compound pressure expected change in pressure vessel HCI 4.88 atm Olt increase O Į decrease O (no change) O2 0, 8.21 atm O t increase O I decrease O (no change) A H,0 5.94 atm O t increase O I decrease O (no change) Cl, 5.44 atm O f increase O Į decrease O (no change) HCI 6.03 atm O t increase O Į decrease O (no change) 7.78 atm O t increase O I decrease O (no change) В H,0 4.37 atm O t increase O I decrease O (no change) CL, 3.93 atm O t increase O I decrease O (no change)

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 51QRT: At room temperature, the equilibrium constant Kc for the reaction 2 NO(g) ⇌ N2(g) + O2(g) is 1.4 ×...

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At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g) (a) Analysis shows that the concentrations of N2 and O2 are both 0.25 M, and that of NO is 0.0042 M under certain conditions. Is the system at equilibrium? (b) If the system is not at equilibrium, in which direction does the reaction proceed? (c) When the system is at equilibrium, what are the equilibrium concentrations?
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Consider the equilibrium N2(g)+O2(g)2NO(g) At 2300 K the equilibrium constant Kc = 1.7 103. If 0.15 mol NO(g) is placed into an empty, sealed 10.0-L flask and heated to 2300 K, calculate the equilibrium concentrations of all three substances at this temperature.
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