CHEMISTRY:MOLECULAR NATURE (LL)W/ACCESS
7th Edition
ISBN: 9781119497325
Author: JESPERSEN
Publisher: WILEY
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 14, Problem 25RQ
Equilibrium and Le Châtelier's Principle
Why doesn’t a catalyst affect the position of equilibrium in a
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Chapter 14 Solutions
CHEMISTRY:MOLECULAR NATURE (LL)W/ACCESS
Ch. 14 - In what way dots the chapter-opening photo...Ch. 14 - Write the equilibrium law for each of the...Ch. 14 - The equilibrium law for a reaction is...Ch. 14 - At25C,Kc=7.01025forthereaction2SO2(g)+O2(g)2SO3(g)...Ch. 14 - At 25C, the following reactions have the...Ch. 14 - Write the equilibrium law in terms of partial...Ch. 14 - Using partial pressures, write the equilibrium law...Ch. 14 - Nitrous oxide, , is a gas used as an anesthetic;...Ch. 14 - Methanol, CH5OH, is a promising fuel that can be...Ch. 14 - Write the equilibrium law for the following...
Ch. 14 - Write the equilibrium law for each of the...Ch. 14 - Suppose a mixture contained equal concentrations...Ch. 14 - Arrange the following reactions in order of their...Ch. 14 - Consider the equilibrium...Ch. 14 - Consider the equilibrium PCl3(g)+Cl2(g)PCl5(g) for...Ch. 14 - In a particular experiment, it was found that when...Ch. 14 - An equilibrium was established for the reaction...Ch. 14 - A student placed 0.200 mol of PCl3(g) and 0.100...Ch. 14 - The decomposition of ,
has vessel contained...Ch. 14 - Prob. 20PECh. 14 - During an experiment, 0.200molofH2and0.200molofI2...Ch. 14 - In an experiment, were placed in a 1.00 L vessel...Ch. 14 - At 25C, the reaction...Ch. 14 - In air at and 1.00 atm, the concentration is...Ch. 14 - Dynamic Equilibrium in Chemical Systems 14.1...Ch. 14 - Dynamic Equilibrium in Chemical Systems
14.2 Using...Ch. 14 - Dynamic Equilibrium in Chemical Systems Repeat the...Ch. 14 - Dynamic Equilibrium in Chemical Systems
14.4 Using...Ch. 14 - 14.5 What meanings do the terms reactants and...Ch. 14 - Equilibrium Laws
14.6 What is an equilibrium law?....Ch. 14 - Equilibrium Laws
14.7 How is the term reaction...Ch. 14 - Equilibrium Laws
14.8 When a chemical equation and...Ch. 14 - Equilibrium Laws 14.9 Under what conditions does...Ch. 14 - Equilibrium Laws
14.10 Describe in words how the...Ch. 14 - Equilibrium Laws Based on Pressures or...Ch. 14 - Equilibrium Laws Based on Pressures or...Ch. 14 - Equilibrium Laws Based on Pressures or...Ch. 14 - Equilibrium Laws Based on Pressures or...Ch. 14 - Equilibrium Laws for Heterogeneous Reactions 14.15...Ch. 14 - Equilibrium Laws for Heterogeneous Reactions 14.16...Ch. 14 - Position of Equilibrium and the Equilibrium...Ch. 14 - Position of Equilibrium and the Equilibrium...Ch. 14 - Position of Equilibrium and the Equilibrium...Ch. 14 - Position of Equilibrium and the Equilibrium...Ch. 14 - Equilibrium and Le Chtelier's Principle State Le...Ch. 14 - Equilibrium and Le Chtelier's Principle Explain,...Ch. 14 - Equilibrium and Le Chteliers Principle Halving the...Ch. 14 - Equilibrium and Le Chteliers Principle How will...Ch. 14 - Equilibrium and Le Châtelier's Principle
14.25 Why...Ch. 14 - Equilibrium and Le Chtelier's Principle Why doesnt...Ch. 14 - Equilibrium Laws
14.27 Write the equilibrium law...Ch. 14 - Equilibrium Laws
14.28 Write the equilibrium law...Ch. 14 - Write the equilibrium law for the following...Ch. 14 - Write the equilibrium law for the following...Ch. 14 - At 25C,Kc=11085 for the reaction...Ch. 14 - Use the following equilibria...Ch. 14 - Write the equilibrium law for each of the...Ch. 14 - 14.34 Write the equilibrium law for the...Ch. 14 - Equilibrium Laws Based on Pressures and...Ch. 14 - 14.36 Write the equilibrium law for the reactions...Ch. 14 - Prob. 37RQCh. 14 - Prob. 38RQCh. 14 - For which of the following reactions does Kp=Kc?...Ch. 14 - For which of the following reactions does KpKc?...Ch. 14 - 14.41 The reaction has a . What is the value of ...Ch. 14 - 14.42 The reaction has a . What is the value of ...Ch. 14 - 14.43 The reaction has a . What is the value of ...Ch. 14 - One possible way of removing NO from the exhaust...Ch. 14 - At 773C the reaction CO(g)+2H2(g)CH3OH(g) has...Ch. 14 - The reaction...Ch. 14 - Equilibrium Laws for Heterogeneous Reactions...Ch. 14 - Equilibrium Laws for Heterogeneous Reactions The...Ch. 14 - Equilibrium Laws for Heterogeneous Reactions
14.49...Ch. 14 - Equilibrium Laws for Heterogeneous Reactions
14.50...Ch. 14 - The heterogeneous reaction...Ch. 14 - At 25C,Kc=360 for the reaction...Ch. 14 - Equilibrium and Le Chtelier's Principle The...Ch. 14 - Equilibrium and Le Chtelier's Principle How will...Ch. 14 - 14.55 Consider the equilibrium
In which direction...Ch. 14 - Consider the equilibrium 2NO(g)+Cl2(g)2NOCl(g) for...Ch. 14 - Calculating Equilibrium Constants At 773C, a...Ch. 14 - Calculating Equilibrium Constants Ethylene, C2H4,...Ch. 14 - At high temperature, 2.00 mol of HBr was placed in...Ch. 14 - A 0.050 mol sample of formaldehyde vapor, CH2O,...Ch. 14 - The reaction NO2(g)+NO(g)N2O(g)+O2(g) reached...Ch. 14 - At 25C,0.0560molO2and0.020molN2O were placed in a...Ch. 14 - Using Equilibrium Constants to Calculate...Ch. 14 - Using Equilibrium Constants to Calculate...Ch. 14 - 14.65 At a certain temperature, the reaction
has...Ch. 14 - 14.66 for the reaction
at a certain temperature....Ch. 14 - At 25C,Kc=0.145 for the following reaction in the...Ch. 14 - At 25C,Kc=0.145 for the following reaction in the...Ch. 14 - 14.69 The equilibrium constant, Kc, for the...Ch. 14 - For the reaction in Problem 14.69, a reaction...Ch. 14 - 14.71 At a certain temperature the reaction
has ....Ch. 14 - At 25C,Kc=0.145 for the following reaction in the...Ch. 14 - The reaction...Ch. 14 - 14.74 At for the reaction
If and are placed in...Ch. 14 - 14.75 At , the decomposition of , has . If a 1.00...Ch. 14 - At 500C, the decomposition of water into hydrogen...Ch. 14 - 14.77 At a certain temperature, for the...Ch. 14 - At 460C, the reaction SO2(g)+NO2(g)NO(g)+SO3(g)...Ch. 14 - 14.79 At a certain temperature, for the...Ch. 14 - At 25C,Kc=0.145 for the following reaction in the...Ch. 14 - *14.81 At a certain temperature, for the...Ch. 14 - The reaction...Ch. 14 - 14.83 The reaction at
. In a reaction vessel...Ch. 14 - 14.84 At , the following concentrations were found...Ch. 14 - The following reaction in aqueous solution has...Ch. 14 - At a certain temperature, Kc=0.914 for the...Ch. 14 - At 27C,Kc=1.51018 for the reaction...Ch. 14 - Consider the equilibrium...Ch. 14 - At a certain temperature, Kc=0.914 for the...Ch. 14 - At a certain temperature, Kc=0.914 for the...Ch. 14 - 14.91 Two 1.00 L bulbs are filled with 0.500 atm...Ch. 14 - For the equilibrium 3NO2(g)N2O5(g)+NO(g)...Ch. 14 - To study the following reaction at 20C,...Ch. 14 - Describe in words how the mass action expression...Ch. 14 - *14.95 For the reaction below,
A mixture of was...Ch. 14 - At 2000C, the decomposition of CO2,...Ch. 14 - *14.97 At , the reaction
has are placed in a...Ch. 14 - At 200.0C,Kc=1.410-10 for the reaction...Ch. 14 - At 400C,Kc=2.9104 for the reaction:...Ch. 14 - *14.100 The reaction . Into a 4.50 L reaction...Ch. 14 - 14.101 In an equilibrium law, coefficients in the...Ch. 14 - Why are equilibrium concentrations useful to know?Ch. 14 - 14.103 Suppose we set up a system in which water...Ch. 14 - 14.104 Do equilibrium laws apply to other systems...Ch. 14 - What might prevent a system from reaching dynamic...Ch. 14 - 14.106 After many centuries the earth’s atmosphere...Ch. 14 - 14.107 If a mixture consisting of many small...Ch. 14 - Why doesnt Le Chteliers principle apply to the...Ch. 14 - 14.109 Le Châtelier’s principle qualitatively...
Additional Science Textbook Solutions
Find more solutions based on key concepts
What two body structures contain flexible elastic cartilage?
Anatomy & Physiology (6th Edition)
DRAW IT Pea plants heterozygous for flower position and stem length (AaTt) are allowed to self-pollinate, and ...
Campbell Biology (11th Edition)
4. Two of these organ system bear the major responsibility for ensuring homeostasis of the internal environment...
Human Anatomy & Physiology (Marieb, Human Anatomy & Physiology) Standalone Book
Choose the best answer to each of the following. Explain your reasoning. Based on computer models, when is plan...
Cosmic Perspective Fundamentals
The data were obtained from a use-dilution test comparing four disinfectants against Salmonella choleraesuis. G...
Microbiology: An Introduction
A piston motion moves a 25kg hammerhead vertically 1m from rest to a ve1oci of 50m/s in a stamping machine. Wha...
Fundamentals Of Thermodynamics
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
- Suppose you have two identical unopened bottles of carbonated beverage. The contents of both bottles appear to be perfectly clear. You loosen the cap of one of the bottles and hear a hiss as gas escapes, and at the same time gas bubbles appear in the liquid. The liquid in the unopened bottle still appears to be perfectly clear. Explain these observations using the concept of equilibrium and Le Chteliers principle. Remember, a carbonated beverage contains carbon dioxide gas dissolved in a liquid under pressure.arrow_forwardWrite a balanced chemical equation for a totally gaseous equilibrium system that would lead to the following equilibrium constant expression. Keq=[N2]2[H2O]6[NH3]4[O2]3arrow_forwardThe equilibrium constant expression for a given reaction depends on how the equilibrium equation is written. Explain the meaning of that statement. You may, if you wish, use the equilibrium equation N2(g)+3H2(g)2NH3(g) to illustrate your explanation.arrow_forward
- Use Le Chteliers principle to predict the direction of equilibrium shift in the following equilibria when the indicated stress is applied: a. 2A+B+heatC; some A is removed. b. 2A+B+heatC+D; the system is cooled. c. N2O42NO2; some NO2 is removed.arrow_forwardIndicate whether or not each of the following changes would affect the value of a systems equilibrium constant. a. Removal of a reactant from the equilibrium mixture b. Decrease in the systems total pressure c. Decrease in the systems temperature d. Addition of a catalyst to the equilibrium mixturearrow_forward. Explain what it means that a reaction has reached a state of chemical equilibrium. Explain why equilibrium is a dynamic state: Does a reaction really “stop” when the system reaches a state of equilibrium? Explain why, once a chemical system has reached equilibrium, the concentrations of all reactants remain constant with time. Why does this constancy of concentration not contradict our picture of equilibrium as being dynamic? What happens to the rates of the forward and reverse reactions as a system proceeds to equilibrium from a starting point where only reactants are present?arrow_forward
- Indicate whether or not each of the following changes would affect the value of a systems equilibrium constant. a. Addition of a product to the equilibrium mixture b. Increase in the systems total pressure c. Increase in the systems temperature d. Addition of both a reactant and a product to the equilibrium mixturearrow_forwardFor the generalized chemical reaction A(g)+B(g)C(g)+D(g) determine whether the concentration of D in an equilibrium mixture will (1) increase, (2) decrease, or (3) not change when each of the following changes is effected. a. concentration of A is increased b. concentration of B is decreased c. concentration of C is increased d. concentration of C is decreasedarrow_forwardFor the generalized chemical reaction A(g)+B(g)C(g)+D(g) determine whether the concentration of A in an equilibrium mixture will (1) increase, (2) decrease, or (3) not change when each of the following changes is effected. a. concentration of B is increased b. concentration of C is decreased c. concentration of D is increased d. concentration of D is decreasedarrow_forward
- Classify each of the following statements as true or false. aSome equilibria depend on a steady supply of a reactant in order to maintain the equilibrium. bBoth forward and reverse reactions continue after equilibrium is reached. cEvery time reactant molecules collide, there is a reaction. dPotential energy during a collision is greater than potential energy before or after the collision. eThe properties of a transition state are between those of the reactants and products. fActivation energy is positive for both the forward and reverse reactions. gKinetic energy is changed to potential energy during a collision. hAn increase in temperature speeds the forward reaction but slows the reverse reaction. iA catalyst changes the steps by which a reaction is completed. jAn increase in concentration of a substance on the right-hand side of an equation speeds the reverse reaction rate. kAn increase in the concentration of a substance in an equilibrium increases the reaction rate in which the substance is a product. lReducing the volume of a gaseous equilibrium shifts the equilibrium in the direction of fewer gaseous molecules. mRaising temperature results in a shift in the forward direction of an endothermic equilibrium. nThe value of an equilibrium constant depends on temperature. oA large K indicates that an equilibrium is favored in the reverse direction.arrow_forwardTell what will happen to each equilibrium concentration in the following when the indicated stress is applied and a new equilibrium position is established. a. LiOH(s)+CO2(g)LiHCO3(s)+heat; CO2 is removed. b. 2NaHCO3(s)+heatNa2O(s)+2CO2(g)+H2O(g); The system is cooled. c. CaCO3(s)+heatCaO(s)+CO2(g); The system is cooled.arrow_forward
arrow_back_ios
arrow_forward_ios
Recommended textbooks for you
Introductory Chemistry: An Active Learning Approa...ChemistryISBN:9781305079250Author:Mark S. Cracolice, Ed PetersPublisher:Cengage Learning
Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co
World of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage Learning
General, Organic, and Biological ChemistryChemistryISBN:9781285853918Author:H. Stephen StokerPublisher:Cengage Learning
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry for Today: General, Organic, and Bioche...ChemistryISBN:9781305960060Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. HansenPublisher:Cengage Learning
Introductory Chemistry: An Active Learning Approa...
Chemistry
ISBN:9781305079250
Author:Mark S. Cracolice, Ed Peters
Publisher:Cengage Learning
Chemistry: Matter and Change
Chemistry
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Glencoe/McGraw-Hill School Pub Co
World of Chemistry, 3rd edition
Chemistry
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Brooks / Cole / Cengage Learning
General, Organic, and Biological Chemistry
Chemistry
ISBN:9781285853918
Author:H. Stephen Stoker
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry for Today: General, Organic, and Bioche...
Chemistry
ISBN:9781305960060
Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen
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