A chemical engineer is studying the following reaction: H₂(g) + Cl₂(g) → 2 HCl (g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.39. The engineer charges ("fills") three reaction vessels with hydrogen and chlorine, 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 A B с compound H₂ Cl₂ H Cl H₂ Cl₂ H CI H₂ Cl₂ H Cl pressure 2.00 atm 2.71 atm 2.34 atm. 2.70 atm 3.41 atm 0.93 atm 2.66 atm 3.37 atm 1.00 atm expected change in pressure ↑ increase Ot increase ↑ increase Ot increase Ot increase ↑ increase Ot increase Ot increase Ot increase O decrease ↓ O↓ decrease O decrease Odecrease O decrease O decrease O decrease Odecrease Odecrease O(no change) (no change) O (no change) (no change) O(no change) O(no change) O(no change) O (no change) O (no change)

A chemical engineer is studying the following reaction: H₂(g) + Cl₂(g) → 2 HCl (g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.39. The engineer charges ("fills") three reaction vessels with hydrogen and chlorine, 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 A B с compound H₂ Cl₂ H Cl H₂ Cl₂ H CI H₂ Cl₂ H Cl pressure 2.00 atm 2.71 atm 2.34 atm. 2.70 atm 3.41 atm 0.93 atm 2.66 atm 3.37 atm 1.00 atm expected change in pressure ↑ increase Ot increase ↑ increase Ot increase Ot increase ↑ increase Ot increase Ot increase Ot increase O decrease ↓ O↓ decrease O decrease Odecrease O decrease O decrease O decrease Odecrease Odecrease O(no change) (no change) O (no change) (no change) O(no change) O(no change) O(no change) O (no change) O (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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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?
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.
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?
. Gaseous phosphorus pentachloride decomposes according to the reaction PCl5(g)PCl3(g)+Cl2(g)The equilibrium system was analyzed at a particular temperature, and the concentrations of the substances present were determined to be [PCl5]=1.1102M,[PCl3]=0.325M. and [Cl2]=3.9103M. Calculate the value of K for the reaction.
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.
For a typical equilibrium problem, the value of K and the initial reaction conditions are given for a specific reaction, and you are asked to calculate the equilibrium concentrations. Many of these calculations involve solving a quadratic or cubic equation. What can you do to avoid solving a quadratic or cubic equation and still come up with reasonable equilibrium concentrations?
The diagram represents an equilibrium mixture for the reaction N2(g) + O2(g) ⇌ 2 NO(g) Estimate the equilibrium constant.
The equilibrium constant Kc for the synthesis of methanol, CH3OH. CO(g)+2H2(g)CH3OH(g) is 4.3 at 250C and 1.8 at 275C. Is this reaction endothermic or exothermic?
Describe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium apply to the system.
Kc = 5.6 1012 at 500 K for the dissociation of iodine molecules to iodine atoms. I2(g) 2 I(g) A mixture has [I2] = 0.020 mol/Land [I] = 2.0 108 mol/L. Is the reaction at equilibrium (at 500 K)? If not, which way must the reaction proceed to reach equilibrium?
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?
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?