EBK GENERAL CHEMISTRY
11th Edition
ISBN: 9780134419022
Author: Bissonnette
Publisher: PEARSON CUSTOM PUB.(CONSIGNMENT)
expand_more
expand_more
format_list_bulleted
Question
Chapter 15, Problem 91IAE
Interpretation Introduction
Interpretation:
Equilibrium amount of each gas should be calculated in moles.
Concept introduction:
Equilibrium constant of a reaction can be expressed in terms of KP or KC.
Binomial theorem can apply to solve higher order terms.
To solve polynomial equations can numerical methods, Newton − Raphson method is a one method. Other than that, methods can use scientific calculator and computational methods to solve polynomial equations.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionChapter 15 Solutions
EBK GENERAL CHEMISTRY
Ch. 15 - Based on these descriptions, write a balanced...Ch. 15 - Based on these descriptions, write a balanced...Ch. 15 - Write equilibrium constant expressions, Kg , for...Ch. 15 - Write equilibrium constant expressions, Kg for the...Ch. 15 - Write an equilibrium constant, Kg1 for the...Ch. 15 - Write an equilibrium constant Kg for the formation...Ch. 15 - Determine values of Ks from the Kg values given....Ch. 15 - Determine the values of Kg from the Kg values...Ch. 15 - The vapor pressure of water at 25C is 238 mmHg....Ch. 15 - If Kg=5.12102 for the equilibrium established...
Ch. 15 - Determine Kz for the reaction...Ch. 15 - Given the equilibrium constant values...Ch. 15 - Use the following data to estimate a value of Kg...Ch. 15 - Determine Kg for the reaction...Ch. 15 - An important environmental and physiological...Ch. 15 - Rust Fe2O2(s) , is caused by the oxidation of iron...Ch. 15 - 1.00102 mol PCl3 is introduced into a 250.0 mL...Ch. 15 - A mixture of 1.00gH2 and 1.06gH2S in a 0.500 L...Ch. 15 - The two common chlorides of phosphorus, PCl2 and...Ch. 15 - A 0.682 g sample of ICI(g) is placed in a 625 mL...Ch. 15 - Write the equilibrium constant expression for the...Ch. 15 - Write the equilibrium constant expression for the...Ch. 15 - Equilibrium is established at 1000 K, where Ke=281...Ch. 15 - For the dissociation o l2(g)t about...Ch. 15 - In the Ostwald process for oxidizing ammonia, a...Ch. 15 - At 2000K, Kx=0.154 for the reaction...Ch. 15 - An equilibrium mixture at 1000 K contains 0.276...Ch. 15 - For the reaction CO(g)+H2O(g)CO2(g)+H2(g),Kc=23.2...Ch. 15 - Can a mixture of 2.2 mol O2 , 3.6 mol SO2 , and...Ch. 15 - Is a mixture of 0.0205 mol NO2(g) and...Ch. 15 - In the reaction 2SO2(g)+O2(g)2SO2(g) , 0.455 mol...Ch. 15 - In the reaction CO(g)+H2O(g)CO2(g)+H2(g),Kc=31.4...Ch. 15 - A mixture consisting of 0.150molH2 and 0.150moll2...Ch. 15 - Stating with 0.280 mol Sbcl2 and 0.160mol Cl2 ,...Ch. 15 - Starting with 0.3500 mo CO(g) and 0.05500 mol...Ch. 15 - g each of CO, H2O , and H2 are sealed in a 1.41L...Ch. 15 - Eqilibrium is established in a 2.50 L flask at...Ch. 15 - For the following reaction, Kg=2.00 at 100C ....Ch. 15 - The substances involved in the following in the...Ch. 15 - The N2O4-NO2 equilibrium mixture in the flask on...Ch. 15 - Formamide, used in the manufacture of...Ch. 15 - A mixture of 1.00 mol NaHCO2 (s) and 1.00 mol...Ch. 15 - Cadmium metal is added to 0.350 L of an aqueous...Ch. 15 - Lead metal is added to 0.100 M Cr2+(aq) . What are...Ch. 15 - One sketch below represents an initial...Ch. 15 - One sketch below represents an initial...Ch. 15 - One important reaction in the citric acid cycle is...Ch. 15 - The following reaction is an important reaction in...Ch. 15 - Refer to Example 15-2 H2S(g) at 747.6 mmHg...Ch. 15 - A sample of NH4HS(s) is placed in a 2.58L flask...Ch. 15 - The following reaction is used self-contained...Ch. 15 - Prob. 52ECh. 15 - Exactly 1.00 mol each of CO and Cl2 are introduced...Ch. 15 - For the reaction 2NO2(g)2NO(g)+O2(g),Kg=1.8108 at...Ch. 15 - Continuous removal of one of the products of a...Ch. 15 - We can represent the freezing of H2O(l) at 0C as...Ch. 15 - Explain how each of the following affects the...Ch. 15 - In the gas phase, iodine reacts with cyclopentene...Ch. 15 - The reaction N2(g)+O2(g)2NO(g),rH=+181kJmol-1 ,...Ch. 15 - Use data from Appendix D to determine whether the...Ch. 15 - If the volume of an equilibrium mixture of...Ch. 15 - For the reaction A(s)B(s)+2C(g)+12D(g)tH=0 Will Kc...Ch. 15 - What effect does increasing the volume of the...Ch. 15 - For which of the following reaction would you...Ch. 15 - The following reaction represents the binding of...Ch. 15 - In human body, the enzyme carbon anahydrase...Ch. 15 - A crystal of dinitrogen tetroxide (melting point,...Ch. 15 - When hydrogen iodide is heated, the degree...Ch. 15 - The standard enthalpy of reaction lot the...Ch. 15 - Would you expect at the amount of N2 to increase,...Ch. 15 - The equilibrium constant for the following...Ch. 15 - For the reaction C2H2(g)+3H2(g)2CH4(g) , the...Ch. 15 - The equilibrium constant for the following...Ch. 15 - The equilibrium constant for the following...Ch. 15 - Explain why the percent of molecules that...Ch. 15 - Prob. 76IAECh. 15 - Refer to Example 15-13g. Suppose that 0100 L of...Ch. 15 - In the equilibrium described in Example 15-12, the...Ch. 15 - Starting with SO2(g) at 1.00 atm, what will be the...Ch. 15 - A sample of a with a mole ratio of N2 to O2 , of...Ch. 15 - Derive, by calculation, the equilibrium amounts of...Ch. 15 - The decomposition of salicylic acid to phenol and...Ch. 15 - One of the key reaction in the gasification of...Ch. 15 - A sample of pure PCl2(g) is introduced into an...Ch. 15 - Prob. 85IAECh. 15 - Prob. 86IAECh. 15 - Show that in terms of mole fractions of gases and...Ch. 15 - For the synthesis of ammonia at 500 K,...Ch. 15 - Prob. 89IAECh. 15 - Prob. 90IAECh. 15 - Prob. 91IAECh. 15 - Concerning me reaction in Exercise 26 and the...Ch. 15 - For the reaction 2NO(g)+Cl2(g)2NOCl(g),Kz=3.7108...Ch. 15 - Prob. 94IAECh. 15 - Prob. 95IAECh. 15 - Prob. 96IAECh. 15 - Prob. 97IAECh. 15 - Prob. 98IAECh. 15 - Prob. 99FPCh. 15 - The decomposition of Hl(g) is represented by the...Ch. 15 - Prob. 101FPCh. 15 - Prob. 102FPCh. 15 - Prob. 103FPCh. 15 - Prob. 104SAECh. 15 - Prob. 105SAECh. 15 - Explain the important distinctions between each...Ch. 15 - In the reversible reaction H2(g)+l2(g)2Hl(g) , a...Ch. 15 - Equilibrium is established the reaction...Ch. 15 - The volume of the reaction vessel containing an...Ch. 15 - For the reaction 2NO2(g)=2NO(g)+O2(g),Kg=1.8108 at...Ch. 15 - For the dissociation reaction...Ch. 15 - The following data are given at...Ch. 15 - Equilibrium is established in the reversible...Ch. 15 - The Deacon process for producing chlorine gas fro,...Ch. 15 - For the reaction SO2(g)SO2(aq),K=1.25 at 25C ....Ch. 15 - In the reaction H2O2(g)H2O2(aq),K=1.0104 at 25C ....Ch. 15 - An equilibrium mixture of SO2 , SO2 , and O2 gases...Ch. 15 - Prob. 118SAE
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- . What does it mean to say that a state of chemical or physical equilibrium is dynamic?arrow_forward5.2. What is the difference between a static equilibrium and a dynamic equilibrium? Give examples difference from the examples in the text. What is similar for the two types of equilibria?arrow_forwardDuring an experiment with the Haber process, a researcher put 1 mol N2 and 1 mol H2 into a reaction vessel to observe the equilibrium formation of ammonia, NH3. N2(g)+3H2(g)2NH3(g) When these reactants come to equilibrium, assume that x mol H2 react. How many moles of ammonia form?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_forwardShow that the complete chemical equation, the total ionic equation, and the net ionic equation for the reaction represented by the equation KI(aq)+I2(aq)KI3(aq) give the same expression for the reaction quotient. KI3 is composed of the ions K+ and I3-.arrow_forwardAt 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?arrow_forward
- In 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_forwardA 4.72-g sample of methanol (CH3OH) was placed in an otherwise empty 1.00-L flask and heated to 250.C to vaporize the methanol. Over time, the methanol vapor decomposed by the following reaction: CH3OH(g)CO(g)+2H2(g) After the system has reached equilibrium, a tiny hole is drilled in the side of the flask allowing gaseous compounds to effuse out of the flask. Measurements of the effusing gas show that it contains 33.0 times as much H2(g) as CH3OH(g). Calculate K for this reaction at 250.C.arrow_forwardIn Section 17.3 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 for a system to reach equilibrium? Explain why equilibrium is not reached in an open system.arrow_forward
- Mustard gas, used in chemical warfare in World War I, has been found to be an effective agent in the chemotherapy of Hodgkin's disease. It can be produced according to the following reaction: SCl2(g)+2C2H4(g)S(CH2CH2Cl)2(g)An evacuated 5.0-1- flask at 20.0C is filled with 0.258 mol SCl2 and 0.592 mol C2H4. After equilibrium is established, 0.0349 mol mustard gas is present. (a) What is the partial pressure of each gas at equilibrium? (b) What is K at 20.0C?arrow_forward5.19. Assume that a reaction exists such that equilibrium occurs when the partial pressures of the reactants and products are all . If the volume of the system were doubled, all of the partial pressures would be . Would the system still be at equilibrium? Why or Why not?arrow_forwardA gaseous material XY(g) dissociates to some extent to produce X(g) and Y(g): XY(g)X(g)+Y(g) A 2.00-g sample of XY (molar mass = 165 g/mol) is placed in a container with a movable piston at 25C. The pressure is held constant at 0.967 atm. As XY begins to dissociate, the piston moves until 35.0 mole percent of the original XY has dissociated and then remains at a constant position. Assuming ideal behavior, calculate the density of the gas in the container after the piston has stopped moving, and determine the value of K for this reaction of 25C.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Chemical Equilibria and Reaction Quotients; Author: Professor Dave Explains;https://www.youtube.com/watch?v=1GiZzCzmO5Q;License: Standard YouTube License, CC-BY