A chemical engineer is studying the following reaction:4 HCl(g)+O2(9) →2 H,O(g)+2Cl,(9)At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.072.рThe engineer charges ("fills") four reaction vessels with hydrogen chloride and oxygen, and lets the reaction begin. He thenmeasures 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.Arreactioncompoundpressureexpected change in pressurevesselHCl10.82 atmf increaseI decrease(no change)O22.66 atmO f increaseI decrease(no change)АH,03.92 atmO f increaseI decrease(no change)Cl,6.44 atmO f increaseO I decreaseO (no change)HCl10.92 atmf increaseI decrease(no change)O22.69 atmf increaseI decrease(no change)ВH,O3.87 atmO f increaseI decrease(no change)Cl,6.39 atmO f increaseI decrease(no change) oloHCl10.92 atmf increasedecrease(no change)O22.69 atmArf increaseI decrease(no change)ВH,O3.87 atmO t increaseI decrease(no change)Cl,6.39 atmf increaseI decrease(no change)HCl10.22 atmO f increaseI decrease(no change)O22.50 atmO f increaseI decrease(no change)H,05.37 atmf increaseI decrease(no change)Cl,8.23 atmf increaseO I decreaseO (no change)

Equilibrium constant ( K) and reaction quotient (Q ) is the ratio of concentration of products to…

A chemical engineer is studying the following reaction: 4 HCl(9)+O,(9) → 2 H,0(9)+2Cl,(9) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.072. 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 HCl 10.82 atm f increase I decrease O (no change) O2 2.66 atm O t increase O I decrease O (no change) A H,O 3.92 atm O f increase I decrease (no change) Cl, 6.44 atm O t increase I decrease (no change) HCI 10.92 atm O t increase I decrease (no change) 02 2.69 atm O t increase I decrease (no change) В H,O 3.87 atm O f increase I decrease (no change) Cl, 6.39 atm O t increase I decrease (no change)

A chemical engineer is studying the following reaction: 4 HCl(9)+O,(9) → 2 H,0(9)+2Cl,(9) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.072. 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 HCl 10.82 atm f increase I decrease O (no change) O2 2.66 atm O t increase O I decrease O (no change) A H,O 3.92 atm O f increase I decrease (no change) Cl, 6.44 atm O t increase I decrease (no change) HCI 10.92 atm O t increase I decrease (no change) 02 2.69 atm O t increase I decrease (no change) В H,O 3.87 atm O f increase I decrease (no change) Cl, 6.39 atm O t increase I decrease (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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Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?
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?
Consider 0.200 mol phosphorus pentachloride sealed in a 2.0-L container at 620 K. The equilibrium constant, Kc, is 0.60 for PCl5(g) PCl3(g) + Cl2(g) Calculate the concentrations of all species after equilibrium has been reached.
During an experiment with the Haber process, a researcher put 1 mol N2 and 1 mol H2 into a reaction vessel to observe the equilibrium formation of ammonia, NH3. N2(g)+3H2(g)2NH3(g) When these reactants come to equilibrium, assume that x mol H2 react. How many moles of ammonia form?
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12.101 An engineer working on a design to extract petroleum from a deep thermal reservoir wishes to capture toxic hydrogen sulfide gases present by reaction with aqueous iron(II) nitrate to form solid iron(II) sulfide. (a) Write the chemical equation for this process, assuming that it reaches equilibrium. (b) What is the equilibrium constant expression for this system? (c) How can the process be manipulated so that it does not reach equilibrium, allowing the continuous removal of hydrogen sulfide?
Describe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium apply to the system.
The experiment in Exercise 12.33 was redesigned so that the reaction started with 0.15 mol each of N2 and O2 being injected into a 1.0-L container at 2500 K. The equilibrium constant at 2500 K is 3.6 X 10“’. What was the composition of the reaction mixture after equilibrium was attained? The following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) *2 2 NO K = 4.1 X IO-4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L-’ ofO2, what were the equilibrium concentrations of all species?