The following system is at equilibrium:X(s) +3Y(g) =Z(g)Classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of the net reaction. Drag the appropriate items to their respective bins. • View Available Hint(s) Reset Help Add more X Increase the volume Remove some X Decrease the volume Leftward shift Rightward shift No shift

The following system is at equilibrium:X(s) +3Y(g) =Z(g)Classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of the net reaction. Drag the appropriate items to their respective bins. • View Available Hint(s) Reset Help Add more X Increase the volume Remove some X Decrease the volume Leftward shift Rightward shift No shift

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 12.45PAE: The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does...

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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.
Sulfur oxychloride, SO2Cl2, decomposes to sulfur dioxide and chlorine gases. SO2Cl2(g)SO2(g)+Cl2(g) At a certain temperature, the equilibrium partial pressures of SO2, Cl2, and SO2Cl2 are 1.88 atm, 0.84 atm, and 0.27 atm, respectively. (a) What is K at that temperature? (b) Enough Cl2 condenses to reduce its partial pressure to 0.68 atm. What are the partial pressures of all gases when equilibrium is reestablished?
The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does the equilibrium shift in response to each of the following stresses? (a) The quantity of solid carbon is increased. (b) A small quantity of water is added, and CO2 dissolves in it. (c) The system is cooled. (d) The volume of the container is increased.
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?
The following data are for the system A(g)2B(g) (a) How long does it take the system to reach equilibrium? (b) How does the rate of the forward reaction compare with the rate of the reverse reaction after 30 s? After 90 s?
Assume that the change in pressure of H2S is small enough to be neglected in the following problem, (a) Calculate the equilibrium pressures of all species in an equilibrium mixture that results from the decomposition of H2S with an initial pressure of 0.824 atm. 2H2S(g)2H2(g)+S2(g)Kp=2.2106 (b) Show that the change is small enough to be neglected.
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.
. Ammonia. a very important industrial chemical. is produced by the direct combination of the following elements under carefully controlled conditions: N2(g)+3H2(g)2NH3(g)Suppose. in an experiment, that the reaction mixture is analyzed after equilibrium is reached, and it is found, at a particular temperature. that [NH3]=0.25M,[H2]=3.4103M, and [N2]=5.3105M. Calculate the value of K at this temperature.
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?
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.
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?
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?