A chem ngineer is studying the following reaction:4 HCl(g) + O₂(g) → 2H₂O(g) + 2Cl₂(g)At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.17.PThe engineer charges ("fills") four reaction vessels with hydrogen chloride and oxygen, and lets the reaction begin. She then measures the composition of themixture inside each vessel from time to time. Her first set of measurements are shown in the table below.Predict the changes in the compositions the engineer should expect next time she measures the compositions.reactionvesselABCcompoundHCl02H₂OC1₂H CIH₂OC1₂H Cl0₂H₂OC12pressure6.10 atm5.69 atm9.07 atm4.08 atm6.65 atm5.36 atm7.21 atm2.91 atm4.19 atm4.74 atm8.43 atm4.13 atmexpected change in pressure↑ increase↑ increase↑ increase↑ increase↑ increase↑ increase↑ increase↑ increase↑ increase↑ increase↑ increase↑ increase↓ decreasedecreasedecreasedecrease↓ decrease↓ decrease↓ decrease↓ decrease↓ decrease↓ decrease↓ decrease↓ decrease(no change)(no change)(no change)(no change)(no change)(no change)(no change)(no change)(no change)(no change)(no change)(no change)

A chem ngineer is studying the following reaction: 4 HCl(g) + O₂(g) → 2 H₂O(g) +2C1₂(g) At the temperature the engineer picks, the equilibrium constant Kp for this reaction is 0.17. The engineer charges ("fills") four reaction vessels with hydrogen chloride and oxygen, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction vessel A B U с compound H CI 0₂ H₂O C1₂ H CI 0₂ H₂O C1₂ H CI 0₂ H₂O C1₂ pressure 6.10 atm 5.69 atm 9.07 atm 4.08 atm. 6.65 atm. 5.36 atm 7.21 atm 2.91 atm 4.19 atm. 4.74 atm 8.43 atm. 4.13 atm expected change in pressure Ot increase Ot increase ↑ Ot increase Ot increase Ot increase Ot increase Ot increase Ot increase ↑ increase Ot increase Ot increase Ot increase decrease O decrease O decrease Odecrease decrease Odecrease Odecrease Odecrease Odecrease Odecrease decrease Odecrease O(no change) O(no change) O(no change) O(no change) (no change) O(no change) O (no change) (no change) O (no change) O(no change) O(no change) (no change)

A chem ngineer is studying the following reaction: 4 HCl(g) + O₂(g) → 2 H₂O(g) +2C1₂(g) At the temperature the engineer picks, the equilibrium constant Kp for this reaction is 0.17. The engineer charges ("fills") four reaction vessels with hydrogen chloride and oxygen, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction vessel A B U с compound H CI 0₂ H₂O C1₂ H CI 0₂ H₂O C1₂ H CI 0₂ H₂O C1₂ pressure 6.10 atm 5.69 atm 9.07 atm 4.08 atm. 6.65 atm. 5.36 atm 7.21 atm 2.91 atm 4.19 atm. 4.74 atm 8.43 atm. 4.13 atm expected change in pressure Ot increase Ot increase ↑ Ot increase Ot increase Ot increase Ot increase Ot increase Ot increase ↑ increase Ot increase Ot increase Ot increase decrease O decrease O decrease Odecrease decrease Odecrease Odecrease Odecrease Odecrease Odecrease decrease Odecrease O(no change) O(no change) O(no change) O(no change) (no change) O(no change) O (no change) (no change) O (no change) O(no change) O(no change) (no change)

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.101PAE: 12.101 An engineer working on a design to extract petroleum from a deep thermal reservoir wishes to...

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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?
At room temperature, the equilibrium constant Kc for the reaction 2 NO(g) ⇌ N2(g) + O2(g) is 1.4 × 1030. Is this reaction product-favored or reactant-favored? Explain your answer. In the atmosphere at room temperature the concentration of N2 is 0.33 mol/L, and the concentration of O2 is about 25% of that value. Calculate the equilibrium concentration of NO in the atmosphere produced by the reaction of N2 and O2. How does this affect your answer to Question 11?
Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?
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?
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?
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.
12.103 Methanol, CH3OH, can be produced by the reaction of CO with H2, with the liberation of heat. All species in the reaction are gaseous. What effect will each of the following have on the equilibrium concentration of CO? (a) Pressure is increased, (b) volume of the reaction container is decreased, (c) heat is added, (d) the concentration of CO is increased, (e) some methanol is removed from the container, and (f) H2 is added.
A solution is prepared by dissolving 0.050 mol of diiodocyclohexane, C5H10I2, in the solvent CCl4.The total solution volume is 1.00 L When the reaction C6H10I2 C6H10 + I2 has come to equilibrium at 35 C, the concentration of I2 is 0.035 mol/L. (a) What are the concentrations of C6H10I2 and C6H10 at equilibrium? (b) Calculate Kc, the equilibrium constant.
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?
Nitrosyl chloride, NOC1, decomposes to NO and Cl2 at high temperatures. 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g) Suppose you place 2.00 mol NOC1 in a 1.00–L flask, seal it, and raise the temperature to 462 °C. When equilibrium has been established, 0.66 mol NO is present. Calculate the equilibrium constant Kc for the decomposition reaction from these data.
The diagram represents an equilibrium mixture for the reaction N2(g) + O2(g) ⇌ 2 NO(g) Estimate the equilibrium constant.
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?