1 Chemistry: An Introduction 2 Measurements And Calculations 3 Matter 4 Chemical Foundations: Elements, Atoms, And Ions 5 Nomenclature 6 Chemical Reactions: An Introduction 7 Reactions In Aqueous Solutions 8 Chemical Composition 9 Chemical Quantities 10 Energy 11 Modern Atomic Theory 12 Chemical Bonding 13 Gases 14 Liquids And Solids 15 Solutions 16 Acids And Bases 17 Equilibrium 18 Oxidation–reduction Reactions And Electrochemistry 19 Radioactivity And Nuclear Energy 20 Organic Chemistry 21 Biochemistry Chapter17: Equilibrium
17.1 How Chemical Reactions Occur 17.2 Conditions That Affect Reaction Rates 17.3 The Equilibrium Condition 17.4 Chemical Equilibrium: A Dynamic Condition 17.5 The Equilibrium Constant: An Introduction 17.6 Heterogeneous Equilibria 17.7 Le Châtelier’s Principle 17.8 Applications Involving The Equilibrium Constant 17.9 Solubility Equilibria Chapter Questions Section: Chapter Questions
Problem 1ALQ: Consider an equilibrium mixture of four chemicals (A. B. C. and D. all gases) reacting in a closed... Problem 2ALQ: The boxes shown below represent a set of initial conditions for the reaction: Draw a quantitative... Problem 3ALQ: For the reaction H2+I22HI, consider two possibilities: (a) you add 0.5 mole of each reactant, allow... Problem 4ALQ: Given the reaction A+BC+D, consider the following situations: a. You have 1.3 M A and 0.8 M B... Problem 5ALQ: Consider the reaction A+BC+D. A friend asks the following: “I know we have been told that if a... Problem 6ALQ Problem 7ALQ: The value of the equilibrium constant, K, is dependent on which of the following? (There may be more... Problem 8ALQ: You are browsing through the Handbook of Hypothetical Chemistry when you come across a solid that is... Problem 9ALQ: What do you suppose happens to the Ksp, value of a solid as the temperature of the solution changes?... Problem 10ALQ: . Consider an equilibrium mixture consisting of H2O(g), CO(g). H2(g), and CO2(g) reacting in a... Problem 11ALQ: . Equilibrium is microscopically dynamic but macroscopically static. Explain what this means. Problem 12ALQ: In Section 17.3 of your text, it is mentioned that equilibrium is reached in a closed system. What... Problem 13ALQ Problem 14ALQ: . Consider the figure below in answering the following questions. a. What does a catalyst do to a... Problem 1QAP: For a chemical reaction to take place, some or all chemical bonds in the reactants must break, and... Problem 2QAP: For the simple reaction 2H2(g)+O2(g)2H2O(l)list the types of bonds that must be broken and the types... Problem 3QAP: How do chemists envision reactions taking place in terms of the collision model for reactions? Give... Problem 4QAP: When molecules collide, a certain minimum energy called the _________ is needed for the reaction to... Problem 5QAP: How does a catalyst work to speed up a chemical reaction? Problem 6QAP: Why are enzymes important? For example, what is the importance of the enzyme carbonic anhydrase in... Problem 7QAP: How does equilibrium represent the balancing of opposing processes? Give an example of an... Problem 8QAP: Consider the equilibrium process depicted in Fig. 17.6. When does the equilibrium state occur? Problem 9QAP: When writing a chemical equation for a reaction that comes to equilibrium. how do we indicate... Problem 10QAP: . How do chemists recognize a system that has reached a state of chemical equilibrium? When writing... Problem 11QAP: . What does it mean to say that a state of chemical or physical equilibrium is dynamic? Problem 12QAP: . Consider an initial mixture of N2 and H2 gases that can be represented as follows: The gases react... Problem 13QAP: . In general terms. what does the equilibrium constant for a reaction represent? What is the... Problem 14QAP: . There is only one value of the equilibrium constant for a particular system at a particular... Problem 15QAP: . Write the equilibrium expression for each of the following reactions. a.... Problem 16QAP: . Write the equilibrium expression for each of the following reactions. a. N2(g)+3Cl2(g)2NCl3(g)b.... Problem 17QAP: . Write the equilibrium expression for each of the following reactions. a.... Problem 18QAP: . Write the equilibrium expression for each of the following reactions. a. CO(g)+2H2(g)CH3OH(g)b.... Problem 19QAP: . Suppose that for the reaction PCl5(g)PCl3(g)+Cl2(g)it is determined, at a particular temperature.... Problem 20QAP: . Ammonia. a very important industrial chemical. is produced by the direct combination of the... Problem 21QAP: . At high temperatures, elemental nitrogen and oxygen react with each other to form nitrogen... Problem 22QAP: . Suppose that for the reaction 2N2O(g)+O2(g)4NO((g))it is determined, at a particular temperature,... Problem 23QAP: . What is a homogeneous equilibrium system? Give an example of a homogeneous equilibrium reaction.... Problem 24QAP: . True or false? The position of a heterogeneous equilibrium does not depend on the amounts of pure... Problem 25QAP: . Write the equilibrium expression for each of the following heterogeneous equilibria. a.... Problem 26QAP: . Write the equilibrium expression for each of the following heterogeneous equilibria. a.... Problem 27QAP: . Write the equilibrium expression for each of the following heterogeneous equilibria. a.... Problem 28QAP: . Indicate whether the stated equilibrium expression is correct for each of the following... Problem 29QAP: . In your own words, describe what Le Châtelier’s principle tells us about how we can change the... Problem 30QAP: . Consider the reaction 2CO(g)+O2(g)2CO2(g)Suppose the system is already at equilibrium, and then an... Problem 31QAP: . For an equilibrium involving gaseous substances, what effect, in general terms, is realized when... Problem 32QAP: . What is the effect on the equilibrium position if an exothermic reaction is carried out at a... Problem 33QAP: . For the reaction system C(s)+H2O(g)H2(g)+CO(g)which has already reached a state of equilibrium,... Problem 34QAP: . For the reaction system P4(s)+6F2(g)4PF3(g)which has already reached a state of equilibrium,... Problem 35QAP: . Suppose the reaction system CH4(g)+2O2(g)CO2(g)+2H2O(l)has already reached equilibrium. Predict... Problem 36QAP: . Consider the general reaction 2A(g)+B(s)C(g)+3D(g)H=+115kJ/molwhich has already come to... Problem 37QAP: . Hydrogen gas and chlorine gas in the presence of light react explosively to form hydrogen chloride... Problem 38QAP: . Hydrogen gas, oxygen gas, and water vapor are in equilibrium in a closed container. Hydrogen gas... Problem 39QAP: . The reaction C2H2(g)+2Br2(g)C2H2Br4(g)is exothermic in the forward direction. Will an increase in... Problem 40QAP: . Old fashioned “smelling salts” consist of ammonium carbonate, (NH4)2CO3. The reaction for the... Problem 41QAP: . Plants synthesize the sugar dextrose according to the following reaction by absorbing radiant... Problem 42QAP: . Consider the exothermic reaction CO(g)+2H2(g)CH3OH(l)Predict three changes that could be made to... Problem 43QAP: . Suppose are action has the equilibrium constant K=1.3108. What does the magnitude of this constant... Problem 44QAP: . Suppose a reaction has the equilibrium constant K=1.7108at a particular temperature. Will there be... Problem 45QAP: . For the reaction Br2(g)+5F2(g)2BrF5(g)the system at equilibrium at a particular temperature is... Problem 46QAP: . Consider the reaction SO2(g)+NO2(g)SO3(g)+NO(g)Suppose it is found at a particular temperature... Problem 47QAP: . For the reaction 2CO(g)+O2(g)2CO2(g)it is found at equilibrium at a certain temperature that the... Problem 48QAP: . For the reaction CO2(g)+H2(g)CO(g)+H2O(g)the equilibrium constant. K, has the value 5.21103at a... Problem 49QAP: . The equilibrium constant for the reaction H2(g)+F2(g)2HF(g)has the value 2.1103at a particular... Problem 50QAP: . For the reaction 2H2O(g)2H2(g)+O2(g)K=2.4103at a given temperature. At equilibrium ills found that... Problem 51QAP: . For the reaction 3O2(g)2O3(g)The equilibrium constant, K, has the value 1.121054at a particular... Problem 52QAP: . For the reaction N2O4(g)2NO(g)the equilibrium constant K has the value 8.1103at a particular... Problem 53QAP: . Explain how the dissolving of an ionic solute in water represents an equilibrium process. Problem 54QAP: . What is the special name given to the equilibrium constant for the dissolving of an ionic solute... Problem 55QAP: . Why does the amount of excess solid solute present in a solution not affect the amount of solute... Problem 56QAP: . Which of the following will affect the total amount of solute that can dissolve in a given amount... Problem 57QAP: . Write the balanced chemical equation describing the dissolving of each of the following sparingly... Problem 58QAP: . Write the balanced chemical equation describing the dissolving of each of the following sparingly... Problem 59QAP: . K for copper(II)hydroxide, Cu(OH)2, has a value 2.21020at 25 °C. Calculate the solubility of... Problem 60QAP Problem 61QAP: . A saturated solution of nickel(II) sulfide contains approximately 3.6104gof dissolved NiS per... Problem 62QAP: . Most hydroxides are not very soluble in water. For example, for nickel(II) hydroxide. Ni(OH)2, is... Problem 63QAP: . The solubility product constant, Ksp, for calcium carbonate at room temperature is approximately... Problem 64QAP: . Calcium sulfate, CaSO4, is only soluble in water to the extent of approximately 2.05 g/L at 25 °C.... Problem 65QAP: . Approximately 1.5103of iron(II) hydroxide. Fe(OH)2(s), dissolves per liter of water at 18 °C.... Problem 66QAP: . Chromiurn(III) hydroxide dissolves in water only to the extent of 8.21105M at 25 °C. Calculate... Problem 67QAP: . Magnesium fluoride dissolves in water to the extent of 8.0102g/L at 25°C. Calculate the solubility... Problem 68QAP: . Lead(II) chloride, PbCl2(s), dissolves in water to the extent of approximately 3.6102Mat 20 °C.... Problem 69QAP: . Mercury(I) chloride, Hg2Cl2, was formerly administered orally as a purgative. Although we usually... Problem 70QAP: . The solubility product of iron(III) hydroxide is very small: Ksp=41038at 25 °C. A classical method... Problem 71AP: . Before two molecules can react, chemists envision that the molecules must first collide with one... Problem 72AP: . Why does an increase in temperature favor an increase in the speed of a reaction? Problem 73AP: . The minimum energy required for molecules to react with each other is called the _______ energy. Problem 74AP: . A(n) _______ speeds up a reaction without being consumed. Problem 75AP: . Equilibrium may be defined as the ________ of two processes, one of which is the opposite of the... Problem 76AP: . When a chemical system has reached equilibrium, the concentrations of all reactants and products... Problem 77AP: . What does it mean to say that all chemical reactions are, to one extent or another, reversible? Problem 78AP: . What does it mean to say that chemical equilibrium is a dynamic process? Problem 79AP: . At the point of chemical equilibrium, the rate of the forward reaction _________ the rate of the... Problem 80AP: . Equilibria involving reactants or products in more than one state are said to be _________ . Problem 81AP: . According to Le Châtelier’s principle, when a large excess of a gaseous reactant is added to a... Problem 82AP: . Addition of an inert substance (one that does not participate in the reaction) does not change the... Problem 83AP: . When the volume of a vessel containing a gaseous equilibrium system is decreased, the _________ of... Problem 84AP: . Consider the following reaction at some temperature: H2O(g)+CO(g)H2(g)+CO2(g)K=2.0 Some molecules... Problem 85AP: . What is meant by the solubility product for a sparingly soluble salt? Choose a sparingly soluble... Problem 86AP: . For a given reaction at a given temperature, the special ratio of products to reactants defined by... Problem 87AP: . Many sugars undergo a process called mutarotation, in which the sugar molecules interconvert... Problem 88AP: . Suppose K=4.5103at a certain temperature for the reaction PCl5(g)PCl3(g)+Cl2(g)If it is found that... Problem 89AP: . For the reaction CaCO3(s)CaO(s)+CO2(g)the equilibrium constant K has the form K=[CO2]. Using a... Problem 90AP Problem 91AP: . Teeth and bones are composed, to a first approximation, of calcium phosphate. Ca3(PO4)2(s). The K... Problem 92AP: . Under what circumstances can we compare the solubilities of two salts by directly comparing the... Problem 93AP: . How does the collision model account for the fact that a react ion proceeds faster when the... Problem 94AP Problem 95AP: . Explain why the development of a vapor pressure above a liquid in a closed container represents an... Problem 96AP Problem 97AP Problem 98AP: . For the reaction N2(g)+3Cl2(g)2NCl3(g)an analysis of an equilibrium mixture at a particular... Problem 99AP: . Gaseous phosphorus pentachloride decomposes according to the reaction PCl5(g)PCl3(g)+Cl2(g)The... Problem 100AP: . Write the equilibrium expression for each of the following heterogeneous equilibria. a.... Problem 101AP: . Write the equilibrium expression for each of the following heterogeneous equilibria. a.... Problem 102AP: . Consider the following generic reaction: 2A2B(g)2A2(g)+B2(g) Some molecules of A2B are placed in a... Problem 103AP Problem 104AP: . The reaction PCl3(l)+Cl2(g)PCl5(s)liberates 124 kJ of energy per mole of PCl3reacted. Will an... Problem 105AP Problem 106AP: . For the reaction N2(g)+3H2(g)2NH3(g)K=1.3102at a given temperature. If the system at equilibrium... Problem 107AP: . The equilibrium constant for the reaction 2NOCl(g)2NO(g)+Cl2(g)has the value 9.2106at a particular... Problem 108AP Problem 109AP Problem 110AP Problem 111AP: . Mercuric sulphide, HgS, is one of the least soluble salts known, with Ksp=1.61054at 25 °C.... Problem 112AP Problem 113AP: . For the reaction N2(g)+3H2(g)2NH3(g), list the types of bonds that must be broken and the type of... Problem 114AP: . What does the activation energy for a reaction represent? How is the activation energy related to... Problem 115AP Problem 116AP Problem 117AP Problem 118AP Problem 119AP Problem 120CP Problem 121CP: . Suppose that for a hypothetical reaction: A2(g)+2B(g)2AB(g)It is determined that at a certain... Problem 122CP Problem 123CP: . The reaction H2(g)+I2(g)2HI(g)has Kp=45.9at 763 K. A particular equilibrium mixture at 763 K... Problem 124CP Problem 125CP Problem 126CP: . Consider the following exothermic reaction at equilibrium: N2(g)+3H2(g)2NH3(g)Predict how the... Problem 1CR Problem 2CR Problem 3CR Problem 4CR: How is the strength of an acid related to the position of its ionization equilibrium? Write the... Problem 5CR Problem 6CR: How is the pH scale defined? What range of pH values corresponds to acidic solutions? What range... Problem 7CR: 7. Describe a buffered solution. Give three examples of buffered solutions. For each of your... Problem 8CR Problem 9CR Problem 10CR: . Explain what it means that a reaction has reached a state of chemical equilibrium. Explain why... Problem 11CR: . Describe how we write the equilibrium expression for a reaction. Give three examples of balanced... Problem 12CR Problem 13CR Problem 14CR: . In your own words, paraphrase Le Châtelier’s principle. Give an example (including a balanced... Problem 15CR Problem 16CR Problem 17CR: . a. Write the conjugate acid for each of the following Brønsted-Lowry bases.... Problem 18CR: . Identify the Brønsted-Lowry conjugate acid-base pairs in each of the following. a.... Problem 19CR Problem 20CR Problem 21CR Problem 22CR Problem 23CR Problem 24CR: . The solubility product of magnesium carbonate, MgCO3, has the value Ksp=6.82106at 25 °C. How many... Problem 9CR
Related questions
Which statement is INCORRECT with regard to kinetics?
A. Each 10o C rise in temperature approximately doubles the rate of a reaction.
B. The rate is expressed as the change in concentration per the change in time.
C. The rate of reaction is always expressed as a positive value.
D. The presence of a catalyst decreases the rate of reaction by lowering the Ea of the reaction.
E. The effect that changing the concentration of a reactent has on the rate of a reaction must be determined experimentally.
Definition Definition Study of the speed of chemical reactions and other factors that affect the rate of reaction. It also extends toward the mechanism involved in the reaction.
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