A chemical engineer is studying the following reaction: 4 HCl(9)+0,(9) 2H,0(9)+2Cl,(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.68. The engineer charges ("fills") four reaction vessels with hydrogen chloride and oxygen, and lets the reaction begin. He then measures the composition 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 HCI 4.20 atm O1 increase OI decrease (no change) 3.82 atm O 1 increase O I decrease O (no change) H,0 2.45 atm O t increase OI decrease O (no change) Cl, 2.58 atm 1 increase OI decrease O (no change) HCI 1.12 atm O t increase 0I decrease e (no change) 3.06 atm O 1 increase OI decrease e (no change) H,0 3.99 atm O t increase OI decrease (no change) Cl, 4.12 atm et increase OI decrease O (no change) HCI 2.94 atm O t increase OI decrease O (no change) 3.81 atm O 1 increase O I decrease O (no change) C. H,0 3.65 atm O 1 increase OI decrease O (no change) Cl, 3.80 atm O t increase OI decrease O (no change) 1目|目目目|

A chemical engineer is studying the following reaction: 4 HCl(9)+0,(9) 2H,0(9)+2Cl,(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.68. The engineer charges ("fills") four reaction vessels with hydrogen chloride and oxygen, and lets the reaction begin. He then measures the composition 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 HCI 4.20 atm O1 increase OI decrease (no change) 3.82 atm O 1 increase O I decrease O (no change) H,0 2.45 atm O t increase OI decrease O (no change) Cl, 2.58 atm 1 increase OI decrease O (no change) HCI 1.12 atm O t increase 0I decrease e (no change) 3.06 atm O 1 increase OI decrease e (no change) H,0 3.99 atm O t increase OI decrease (no change) Cl, 4.12 atm et increase OI decrease O (no change) HCI 2.94 atm O t increase OI decrease O (no change) 3.81 atm O 1 increase O I decrease O (no change) C. H,0 3.65 atm O 1 increase OI decrease O (no change) Cl, 3.80 atm O t increase OI decrease O (no change) 1目|目目目|

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 ×...

See similar textbooks

Similar questions

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.
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?
You place 0.600 mol of nitrogen, N2, and 1.800 mol of hydrogen, H2, into a reaction vessel at 450C and 10.0 atm. The reaction is N2(g)+3H2(g)2NH3(g) What is the composition of the equilibrium mixture if you obtain 0.048 mol of ammonia, NH3, from it?
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.
At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s), to chlorine and iodine gases. The partial pressure of chlorine gas at equilibrium is three times that of iodine gas. What are the partial pressures of iodine and chlorine at equilibrium?
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?
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.
Describe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium apply to the system.
For the reaction N2(g)+3H2(g)2NH3(g) show that Kc = Kp(RT)2 Do not use the formula Kp = Kc(RT)5n given in the text. Start from the fact that Pi = [i]RT, where Pi is the partial pressure of substance i and [i] is its molar concentration. Substitute into Kc.
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.
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.
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?