Using the general properties of equilibrium constantsAt a certain temperature, the equilibrium constant K for the following reaction is 1.5:H,(g) + 1,(g) 2 HI(g)Use this information to complete the following table.Suppose a 6.0L reaction vessel is filled with 1.2 mol of H, and1.2 mol of I2. What can you say about the composition of themixture in the vessel at equilibrium?O There will be very little H2 and I2.O There will be very little HI.O Neither of the above is true.What is the equilibrium constant for the following reaction?Round your answer to 2 significant digits.K =02 HI(g)1.H,(0)+I,(0)What is the equilibrium constant for the following reaction?Round your answer to 2 significant digits.K -02 H,(G)+21,(9)4 HI(g)1.ExplanationCheck62021 McGraw-Hill Education. All Rights Reserved Terms of Lise

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At a certain temperature, the equilibrium constant K for the following reaction is 1.5: H,(g) + 1,(g) 2 HI(g) Use this information to complete the following table. Suppose a 6.0L reaction vessel is filled with 1.2 mol of H, and 1.2 mol of I2. What can you say about the composition of the mixture in the vessel at equilibrium? O There will be very little H, and I,. O There will be very little HI. O Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K -0 2 HI(g) H,(0)+I,(9) 1. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K -0 2H,(0)+21,(9) 4 HI(g) 1.

At a certain temperature, the equilibrium constant K for the following reaction is 1.5: H,(g) + 1,(g) 2 HI(g) Use this information to complete the following table. Suppose a 6.0L reaction vessel is filled with 1.2 mol of H, and 1.2 mol of I2. What can you say about the composition of the mixture in the vessel at equilibrium? O There will be very little H, and I,. O There will be very little HI. O Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K -0 2 HI(g) H,(0)+I,(9) 1. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K -0 2H,(0)+21,(9) 4 HI(g) 1.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 123CP: A sample of gaseous nitrosyl bromide (NOBr) was placed in a container tiued with a frictionless,...

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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.
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.
A sample of gaseous nitrosyl bromide (NOBr) was placed in a container tiued with a frictionless, massless piston, where it decomposed at 25C according to the following equation: 2NOBr(g)2NO(g)+Br2(g) The initial density of the system was recorded as 4.495 g/L. After equilibrium was reached, the density was noted to be 4.086 g/L. a. Determine the value of the equilibrium constant K for the reaction. b. If Ar(g) is added to the system at equilibrium at constant temperature, what will happen to the equilibrium position? What happens to the value of K? Explain each answer
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?
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 25C. Kp = 5.3 105 for the reaction N2(g)+3H2(g)2NH3(g) When a certain partial pressure of NH3(g) is put into an otherwise empty rigid vessel at 25C, equilibrium is reached when 50.0% of the original ammonia has decomposed. What was the original partial pressure of ammonia before any decomposition occurred?
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 decomposition of PCl5(g) to form PCl3(g) and Cl2(g) has Kc = 33.3 at a high temperature. If the initial concentration of PCl5 is 0.1000 M, what are the equilibrium concentrations of the reactants and products?
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?
The equilibrium constant Kc, for the reaction 2 NOCI(g) 2 NO(g) + Cl2(g) is 3.9 103 at 300 C. A mixture contains the gases at the following concentrations: [NOCl] = 5.0 103 mol/L, [NO] = 2.5 103 mol/L, and [Cl2] = 2.0 103 mol/L. Is the reaction at equilibrium at 300 C? If not, in which direction does the reaction proceed to come to equilibrium?