Chemistry: Structure and Properties (2nd Edition)
2nd Edition
ISBN: 9780134293936
Author: Nivaldo J. Tro
Publisher: PEARSON
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Chapter 15, Problem 66E
Interpretation Introduction
To determine: Predict the direction the equilibrium will shift given the changes in the concentrations.
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Chapter 15 Solutions
Chemistry: Structure and Properties (2nd Edition)
Ch. 15 - How does a developing fetus get oxygen in the...Ch. 15 - What is dynamic equilibrium? Why is it called...Ch. 15 - Give the general expression for the equilibrium...Ch. 15 - What is the significance of the equilibrium...Ch. 15 - What happens to the value of the equilibrium...Ch. 15 - If two reactions sum to an overall reaction, and...Ch. 15 - Explain the difference between Kcand Kp. For a...Ch. 15 - What units should you use when expressing...Ch. 15 - Why do we omit the concentrations of solids and...Ch. 15 - Does the value of the equilibrium constant depend...
Ch. 15 - Explain how you might deduce the equilibrium...Ch. 15 - What is the definition of the reaction quotient ()...Ch. 15 - What is the value of when each reactant and...Ch. 15 - Prob. 14ECh. 15 - Many equilibrium calculations involve finding the...Ch. 15 - In equilibrium problems involving equilibrium...Ch. 15 - What happens to a chemical system at equilibrium...Ch. 15 - What is the effect of a change in concentration of...Ch. 15 - What is the effect of a change in volume on a...Ch. 15 - What is the effect of temperature change on a...Ch. 15 - Write an expression for the equilibrium constant...Ch. 15 - Find and fix each mistake in the equilibrium...Ch. 15 - When the reaction comes to equilibrium, will the...Ch. 15 - Ethene (C2H4) can be halogenated by this reaction:...Ch. 15 - H2 and I2 are combined in a flask and allowed to...Ch. 15 - A chemist trying to synthesize a particular...Ch. 15 - This reaction has an equilibrium constant of...Ch. 15 - This reaction has an equilibrium constant of...Ch. 15 - Prob. 29ECh. 15 - Use the following reactions and their equilibrium...Ch. 15 - Calculate Kc for reaction a. I2(g)2I(g)Kp=6.261022...Ch. 15 - Calculate Kpfor each reaction. a. N2O4(g)2NO2(g)...Ch. 15 - Write an equilibrium expression for each chemical...Ch. 15 - Find and fix the mistake in the equilibrium...Ch. 15 - Consider the reaction: CO(g)+2H2(g)CH3OH(g) An...Ch. 15 - Consider the reaction: NH4HS(s)NH3(g)+H2S(g) An...Ch. 15 - Consider the reaction: N2(g)+3H2(g)2NH3(g)...Ch. 15 - Consider the reaction: H2(g)+I2(g)2HI(g) Complete...Ch. 15 - Consider the reaction: 2NO(g)+Br2(g)2NOBr(g)Kp=...Ch. 15 - Consider the reaction:...Ch. 15 - For the reaction A(g)2B(g) , a reaction vessel...Ch. 15 - For the reaction 2A(g)B(g)+2C(g) , a reaction...Ch. 15 - Consider the reaction:...Ch. 15 - Consider the reaction: SO2Cl2(g)SO2+Cl2(g) A...Ch. 15 - Consider the reaction: H2(g)+I2(g)2HI(g) A...Ch. 15 - Consider the reaction. CO(g)+2H2(g)CH3OH(g) A...Ch. 15 - Consider the reaction: NH4HS(s)NH3(g)+H2S(g) At a...Ch. 15 - Consider the reaction:...Ch. 15 - Silver sulfate dissolves in water according to the...Ch. 15 - Nitrogen dioxide reacts with itself according to...Ch. 15 - Consider the reaction and the associated...Ch. 15 - Consider the reaction and the associated...Ch. 15 - For the reaction Kc= 0.513 at 500K. N2O4(g)2NO2(g)...Ch. 15 - For the reaction, Kc= 255 at 1000 K...Ch. 15 - Consider the reaction: NiO(s)+CO(g)Ni(s)+CO2(g)...Ch. 15 - Consider the reaction: CO(g)+H2O(g)CO2(g)+H2(g)Kc=...Ch. 15 - Consider the reaction: HC 2 H 3 O 2 (aq)+ H 2 O(l)...Ch. 15 - Prob. 58ECh. 15 - Consider the reaction:...Ch. 15 - Consider the reaction:...Ch. 15 - Consider the reaction: A(g)B(g)+C(g) Find the...Ch. 15 - Consider the reaction: A(g)2B(g) Find the...Ch. 15 - Consider this reaction at equilibrium:...Ch. 15 - Consider this reaction at equilibrium:...Ch. 15 - Consider this reaction at equilibrium:...Ch. 15 - Prob. 66ECh. 15 - Each reaction is allowed to come to equilibrium,...Ch. 15 - Prob. 68ECh. 15 - This reaction is endothermic: C(s)+CO2(g)2CO(g)...Ch. 15 - This reaction is exothermic:...Ch. 15 - Coal, which is primarily carbon, can be converted...Ch. 15 - Coal can be used to generate hydrogen gas (a...Ch. 15 - Carbon monoxide replaces oxygen in oxygenated...Ch. 15 - Nitrogen monoxide is a pollutant in the lower...Ch. 15 - The reaction CO2(g)+C(s)2CO(g) has Kp= 5.78 at...Ch. 15 - A mixture of water and graphite is heated to 600...Ch. 15 - At 650 K, the reaction MgCO3(s)MgO(s)+CO2(g) has...Ch. 15 - A system at equilibrium contains I2(g) at a...Ch. 15 - Consider the exothermic reaction:...Ch. 15 - Consider the endothermic reaction:...Ch. 15 - Consider the reaction: H2(g)+I2(g)2HI(g) A...Ch. 15 - Prob. 82ECh. 15 - Prob. 83ECh. 15 - Prob. 84ECh. 15 - The system described by the reaction:...Ch. 15 - A reaction vessel at 27017°C contains a mixture of...Ch. 15 - At 70 K, CCl4 decomposes to carbon and chlorine....Ch. 15 - The equilibrium constant for the reaction...Ch. 15 - A sample of CaCO3(s) is introduced into a sealed...Ch. 15 - An equilibrium mixture contains N2O4, (P = O.28)...Ch. 15 - Carbon monoxide and chlorine gas react to form...Ch. 15 - Prob. 92ECh. 15 - Prob. 93ECh. 15 - Prob. 94ECh. 15 - Nitrogen monoxide reacts with chlorine gas...Ch. 15 - At a given temperature, a system containing O2(g)...Ch. 15 - A sample of pure NO2 is heated to 337 °C, at which...Ch. 15 - When N2O5(g) is heated, it dissociates into...Ch. 15 - A sample of SO3 is introduced into an evacuated...Ch. 15 - A reaction A(g)B(g) has an equilibrium constant of...Ch. 15 - The reaction A(g)2B(g) has an equilibrium constant...Ch. 15 - A particular reaction has an equilibrium constant...Ch. 15 - Consider the reaction: aA(g)bB(g) Each of the...Ch. 15 - Consider the simple one-step reaction: A(g)B(g)...Ch. 15 - Prob. 105ECh. 15 - Consider the reaction: N2(g)+3H2(g)2NH3(g). a....Ch. 15 - For the reaction AB , the ratio of products to...Ch. 15 - Solve each of the expressions for x using the...Ch. 15 - Have each group member explain to the group what...Ch. 15 - Prob. 110ECh. 15 - What is the correct expression for the equilibrium...Ch. 15 - Prob. 2SAQCh. 15 - Use the data below to find the equilibrium...Ch. 15 - The reaction shown here has a Kp = 4.5X102 AT 825...Ch. 15 - Consider the reaction between NO and Cl2 to form...Ch. 15 - Prob. 6SAQCh. 15 - Consider the reaction between iodine gas and...Ch. 15 - Prob. 8SAQCh. 15 - The decomposition of NH4HS is endothermic:...Ch. 15 - The solid XY decomposes into gaseous X and Y:...Ch. 15 - What is the effect of adding helium gas (at...Ch. 15 - Prob. 12SAQ
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- The decomposition of NH4HS NH4HS(s) NH3(g) + H2S(g) is an endothermic process. Using Le Chateliers principle, explain how increasing the temperature would affect the equilibrium. If more NH4HS is added to a flask in which this equilibrium exists, how is the equilibrium affected? What if some additional NH3 is placed in the flask? What will happen to the pressure of NH3 if some H2S is removed from the flask?arrow_forward. Consider an equilibrium mixture consisting of H2O(g), CO(g). H2(g), and CO2(g) reacting in a closed vessel according to the equation H2O(g)+CO(g)H2(g)+CO2(g)a. You add more H2O to the flask. How does the new equilibrium concentration of each chemical compare to its origin al equilibrium concentration after equilibrium is re-established? Justify your answer. b. You add more H2to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer.arrow_forward. Consider the reaction 2CO(g)+O2(g)2CO2(g)Suppose the system is already at equilibrium, and then an additional mole of CO 2(g) is injected into the system at constant temperature. Does the amount of O2(g) in the system increase or decrease? Does the value of K for the reaction change?arrow_forward
- For the reactionH2(g)+I2(g)2HI(g), consider two possibilities: (a) you mix 0.5 mole of each reactant. allow the system to come to equilibrium, and then add another mole of H2 and allow the system to reach equilibrium again. or (b) you mix 1.5 moles of H2 and 0.5 mole of I2 and allow the system to reach equilibrium. Will the final equilibrium mixture be different for the two procedures? Explain.arrow_forwardAt 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?arrow_forward12.103 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.arrow_forward
- . For the reaction 3O2(g)2O3(g)The equilibrium constant, K, has the value 1.121054at a particular temperature. a. What does the very small equilibrium constant indicate about the extent to which oxygen gas, O2(g), is converted to ozone gas, O3(g), at this temperature? b. If the equilibrium mixture is analyzed and [O2(g)]is found to be 3.04102M, what is the concentration of O3(g) in the mixture’?arrow_forwardHydrogen and carbon dioxide react at a high temperature to give water and carbon monoxide. H2(g) + CO2(g) H2O(g) + CO(g) (a) Laboratory measurements at 986 C show that there are 0.11 mol each of CO and H2O vapor and 0.087 mol each of H2 and CO2 at equilibrium in a 50.0-L container. Calculate the equilibrium constant for the reaction at 986 C. (b) Suppose 0.010 mol each of H2 and CO2 are placed in a 200.0-L container. When equilibrium is achieved at 986 C, what amounts of CO(g) and H2O(g), in moles, would be present? [Use the value of Kc from part (a).]arrow_forwardIn Section 13.1 of your text, it is mentioned that equilibrium is reached in a closed system. What is meant by the term closed system. and why is it necessary to have a closed system in order for a system to reach equilibrium? Explain why equilibrium is not reached in an open system.arrow_forward
- A mixture of SO2, O2, and SO3 at 1000 K contains the gases at the following concentrations: [SO2] = 5.0 103 mol/L, [O2] = 1.9 103 mol/L, and [SO3] = 6.9 103 mol/L. Is the reaction at equilibrium? If not, which way will the reaction proceed to reach equilibrium? 2 SO2(g) + O2(g) 2 SO3(g) Kc = 279arrow_forwardConsider the system 4 NH3(g) + 3 O2(g) ⇌ 2 N2(g) + 6 H20(ℓ) ΔrH° = −1530.4 kJ/mol How will the amount of ammonia at equilibrium be affected by removing O2(g) without changing the total gas volume? adding N2(g) without changing the total gas volume? adding water without changing the total gas volume? expanding the container? increasing the temperature? Which of these changes (i to v) increases the value of K? Which decreases it?arrow_forwardThe decomposition of NH4HS, NH 4 HS( s )NH3( g )+ H 2 S( g ) is an endothermic process. Using Le Chatelier's principle, explain how increasing the temperature would affect the equilibrium. If more NH4HS is added to a flask in which this equilibrium exists, how is the equilibrium affected? What if some additional NH3 is placed in the flask? What will happen to the pressure of NH3 if some H2S is removed from the flask?arrow_forward
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