14.16 Consider the following equilibrium process at 700°C: 2H2 (g) + S2(g)= 2H2S(g) Analysis shows that there are 2.50 moles of H2, 1.35 × 10 mole of S2, and 8.70 moles of H2S present in a 12.0-L flask. Calculate the equilibrium constant K. for the reaction. Pag

14.16 Consider the following equilibrium process at 700°C: 2H2 (g) + S2(g)= 2H2S(g) Analysis shows that there are 2.50 moles of H2, 1.35 × 10 mole of S2, and 8.70 moles of H2S present in a 12.0-L flask. Calculate the equilibrium constant K. for the reaction. Pag

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter15: Principles Of Chemical Reactivity: Equilibria

Section: Chapter Questions

Problem 7PS: The reaction PCl5(g) PCl3(g) + Cl2(g) was examined at 250 C. At equilibrium, [PCl5] = 4.2 105...

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In the contact process, sulfuric acid is manufactured by first oxidizing SO2 to SO3, which is then reacted with water The reaction of SO2 with O2 is 2SO2(g)+O22SO3(g) A 2.000-L flask was filled with 0.0400 mol SO2 and 0.0200 mol O2. At equilibrium at 900 K, the flask contained 0.0296 mol SO3 How many moles of each substance were in the flask at equilibrium?
Consider the following reaction at some temperature: H2O(g)+CO(g)H2(g)+CO2(g)K=2.0 Some molecules of H2O and CO are placed in a 1.0-L container as shown below. When equilibrium is reached, bow many molecules of H2O, CO, H2, and CO2 are present? Do this problem by trial and error-that is, if two molecules of CO react, is this equilibrium; if three molecules of CO react, is this equilibrium; and so on.
In a 3.0-L vessel, the following equilibrium partial pressures are measured: N2, 190 torr; H2, 317 torr; NH3, 1.00103 torr. N2(g)+3H2(g)2NH3(g) (a) How will the partial pressures of H2, N2, and NH3 change if H2 is removed from the system? Will they increase, decrease, or remain the same? (b) Hydrogen is removed from the vessel until the partial pressure of nitrogen, at equilibrium, is 250 torr. Calculate the partial pressures of the other substances under the new conditions.
Chemical Equilibrium I Part 1: You run the chemical reaction C(aq)+D(aq)2E(aq) at 25C. The equilibrium constant Kc for the reaction at this temperature is 2.0. a Write the equilibrium-constant expression for the reaction. b Can you come up with some possible concentrations of C, D, and E that you might observe when the reaction has reached equilibrium at 25C? What are these values? c A student says that only a very limited number of concentrations for C, D, and E are possible at equilibrium. Is this true? State why you think this is true or is not true. d If you start with 1.0 M concentrations of both C and D and allow the reaction to come to equilibrium, would you expect the concentration of C to have decreased to zero? If not, what would you expect for the concentration of C? (An approximate value is fine.) Part 2: Consider the reaction A(aq)F(aq)+G(aq), whose equilibrium constant is 1.0 105 at 20C. For each of the situations described below, indicate whether any reaction occurs. If reaction does occur, then indicate the direction of that reaction and describe how the concentrations of A, B, F, and G change during this reaction. a A(aq) and B(aq) are mixed together in a container. b F(aq) and G(aq) are mixed together in a container. c A(aq) and F(aq) are mixed together in a container. d B(aq) and G(aq) are mixed together in a container. e Just B(aq) is placed into a container. f Just G(aq) is placed into a container. Consider any one of these situations in which a reaction does occur. At equilibrium, does the reaction mixture have appreciably more products than reactants? If not, how would you describe the equilibrium composition of the reaction mixture? How did you arrive at this answer?
Methanol, CH3OH, formerly known as wood alcohol, is manufactured commercially by the following reaction: CO(g)+2H2(g)CH3OH(g) A 1.500-L vessel was filled with 0.1500 mol CO and 0.3000 mol H2. When this mixture came to equilibrium at 500 K. the vessel contained 0.1187 mol CO. How many moles of each substance were in the vessel?
Suppose sulfur dioxide reacts with oxygen at 25C. 2SO2(g)+O2(g)2SO3(g) The equilibrium constant Kc equals 8.0 1035 at this temperature From the magnitude of Kc, do you think this reaction occurs to any great extent when equilibrium is reached at room temperature? If an equilibrium mixture is 1.0 M SO3 and has equal concentrations of SO2 and O2, what is the concentration of SO2 in the mixture? Does this result agree with what you expect from the magnitude of Kc?
A mixture of 0.0565 mol phosphorus pentachloride, PCl5, and 0.0800 mol helium gas, He, was placed in a 1.000-L flask and heated to 250.0C. The phosphorus pentachloride decomposes at this temperature to give phosphorus trichloride, PCl3, and chlorine gas, Cl2. The helium gas is inert. PCl5(g)PCl3(g)+Cl2(g) What is the partial pressure of helium in this equilibrium mixture at 250.0C? At equilibrium, the total pressure is found to be 6.505 atm. What is Kc for the dissociation of PCl5?
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The reaction 2 NO2(g) N2O4(g) has an equilibrium constant, Kc, of 170 at 25 C. If 2.0 103 mol of NO2 is present in a 10.-L. Flask along with 1.5 103 mol of N2O4, is the system at equilibrium? If it is not at equilibrium, does the concentration of NO2 increase or decrease as the system proceeds to equilibrium?
For the equilibrium 2 SO2(g) + O2(g) 2 SO3(g) Kc = 245 (at 1000 K) the equilibrium concentrations are [SO2] = 0.102, [O2] = 0.0132, and [SO3] = 0.184. The concentration of SO2 is suddenly doubled. Show that the forward reaction takes place to reach a new equilibrium.
Iodine monobromide, IBr, occurs as brownish-black crystals that vaporize with decomposition: 2IBR(g)I2(g)+Br2(g) The equilibrium constant Kc at 100C is 0.026. If 0.010 mol IBr is placed in a 1.0-L vessel at 100C, what are the moles of substances at equilibrium in the vapor?
Molecular bromine, Br2, dissociates at elevated temperatures into bromine atoms, Br. Br2(g)2Br(g) A 3.000-L flask initially contains pure molecular bromine. The temperature is then raised to 1600 K. If the total pressure of this equilibrium mixture at this elevated temperature is 1.000 atm, what are the total moles of gas in the container? A spectroscopic analysis of this mixture showed that it contained 1.395 g of Br atoms. What is the partial pressure of Br? What is Kp for the dissociation of molecular bromine to bromine atoms?