CHAPTER 6 CHEMICAL EQUILIBRIUM
|
|
- Matilda Garrison
- 5 years ago
- Views:
Transcription
1 For updated version, please click on BSK1133 PHYSICAL CHEMISTRY CHAPTER 6 CHEMICAL EQUILIBRIUM PREPARED BY: DR. YUEN MEI LIAN AND DR. SITI NOOR HIDAYAH MUSTAPHA Faculty of Industrial Sciences & Technology yuenm@ump.edu.my and snhidayah@ump.edu.my
2 Description Aims To discuss the equilibrium state of chemical and physical equilibrium. To express and calculate equilibrium constants for homogeneous equilibria, heterogeneous equilibria and multiple equilibria. To discuss the factors that may affect the position of equilibrium. To learn the Le Châtelier s principle in the prediction of changes.
3 Description Expected Outcomes Able to describe the equilibrium state of chemical and physical equilibrium. Able to express and calculate the equilibrium constants. Able to study the factors that may affect the position of an equilibrium. Able to apply the Le Châtelier s principle. References Atkins, P & Julio, D. P. (2006).Physical Chemistry (8th ed.). New York: Oxford. Chang, R. (2005).Chemistry (8th ed.). New York: McGraw Hill. Atkins, P & Julio, D. P. (2012). Elements of Physical Chemistry (sixth ed.). Freeman, Oxford. Silbey, R. J., Alberty, A. A., & Bawendi, M. G. (2005). Physical Chemistry. New York: John Wiley & Sons Mortimer R. G. (2008) Physical Chemistry, Third Edition, Elsevier Academic press, USA.
4 Contents 6.1 The Concept of Equilibrium 6.2 Relate the Kinetics in Chemical Equilibrium 6.3 Factors Conclusion
5 6.1 The Concept of Equilibrium
6 I. Introduction The Concept of Equilibrium and the Equilibrium Constant o o Chemical equilibrium can be obtained when the rates of the forward and reverse reactions must be equal. In addition, the concentrations of the reactants and products are unchanged. Example: 2NO 2 (g) N 2 O 4 (g) Physical equilibrium is referring equilibrium of two phases with the same substance. Example: H 2 O (l) H 2 O (g)
7 II. Equilibrium Constant a) Homogeneous Equilibria same phase of reacting species. N 2 O 4 (g) 2NO 2 (g) K c = [NO 2] 2 [N 2 O 4 ] K c shows the reacting species (gas) (units = molarity, moles per liter and partial pressure). Pressure of a gas is to concentration in mol/l of gas (at constant temperature) P = ( n )RT K V p = P NO 2 P N2 O 4 P NO2 and P N2 O 4 are equilibrium partial pressure (atm). K p shows equilibrium concentration expressed in terms of pressure. K c K p cause their units of expression are different. Example: H 2 (g) + Br 2 (g) 2HBr (g) Since Δ n = 2 2 = 0, therefore, K p = (0.0821T) Δn K c K p = (0.0821T) 0 K c K p = K c (Special Case for this reaction where K p = K c ) 2
8 Explanation: Assume ideal gas behaviour aa (g) bb (g) (a,b = stoichiometric coefficients) K c = [B]b [A] a P A = n ART V Substitute in K p K p = (n BRT V )b ( n A RT V )a = ( b K p = P B P B = n BRT V n B V )b ( n A n A V P A a K c K p and n B V can be replaced by [A] and [B]. (RT)b-a = [B]b V )a [A] a (RT)Δn = K c (RT) Δn K p = (0.0821T) Δn K c P A = partial pressure of A P B = partial pressure of B V = volume of the container in liters have units of mol/l. Thus, Where Δ n = b a (moles of gaseous products moles of gaseous reactants) Pressures are usually expressed in atm, hence, gas constant R is atm L/(K mol).
9 b) Heterogeneous Equilibria o Refer to a reversible reaction where different phases of reactants and products that are in. CaCO 3 (s) CaO (s) + CO 2 (g) K c = CaO [CO 2] [CaCO 3 ] K c is used as symbols to differentiate it from final equilibrium constant at the end. o SPECIAL: Concentration (means density) of a solid does not depend on how much of the substance is present. Example: [CaCO 3 ] and [CaO] are constant and combine with K c to form final equilibrium constant. [CaCO 3 ] [CaO] K c = Kc = [CO 2 ] (new equilibrium constant) In thermodynamic, concentration replace with activity of pure solid or liquid = 1. Thus, K c = [CO 2 ] or K p = P CO2
10 c) Multiple Equilibria Example: These equilibria can be split into two steps: K c = A2 H + 2 [H 2 A] K c is equal to the product of the equilibrium expressions for the two reaction steps. Thus, K c = K 1 K 2
11 d) The Form of K and the Equilibrium Equation Condition I N 2 O 4 (g) 2NO 2 (g) 2NO 2 (g) N 2 O 4 (g) K c = [NO 2] 2 = 4.63 x [N 2 O 4 ] 10-3 K c = N 2O 4 = 1 = [NO 2 ] 2 K c o K c K c = 1. (Must specify the equilibrium equation) x 10 Condition II 1 N 2 2O 4 (g) NO 2 (g) N 2 O 4 (g) 2NO 2 (g) K c = [NO 2] 1 K c = [NO 2] 2 [N 2 O 4 ] [N 2 O 4 ] 2 o K c = K c, since K c = 4.63 x 10-3, Hence, K c = = 216 SUMMARY K p = (0.0821T) Δn K c Equilibrium constant (K p or K c ) is unitless.
12 6.2 Relate the Kinetics in Chemical Equilibrium
13 Relate Kinetics and Chemical Equilibrium a) A single elementary step k f rate constant A + 2B AB k 2 Forward: r rate f = k f [A][B] 2 Reverse: rate r = k r [AB] 2 At equilibrium (no net changes): rate f = rate r K c = k f = [AB 2] k r [A][B] 2 b) More than one elementary step k f Step 1: 2B B 2 Step 2: A + B AB 2 Overall reaction: A + 2B AB 2 (Example of multiple equilibria) K = k f K = k f k r = [B 2] [B] 2 k r k f k r k = [AB 2] r A [B 2 ] Overall reaction: K c = K K = AB 2 A [B] 2
14 6.2 Relate the Kinetics in Chemical Equilibrium
15 Le Chatelier s Principle It states that if external stress is introduced to an equilibrium system, the system will adjust to offset it and achieve a new equilibrium position. It helps in prediction of the position of an equilibrium reaction when a change of conditions (concentration, pressure, volume and temperature) occurs. When a new equilibrium reaches, the concentrations of reactants and products remain constant.
16 Forward Reaction A (g) + 3B (g) C (g) + D (g) ΔH = kj/mol Factors Position of Equilibrium shift to right shift to left Concentration Increase (substance A) Decrease (substance A) Pressure Increase Decrease Temperature Decrease Increase Catalyst Unchange
17 Conclusion Chemical equilibrium is referring different substances as reactants and products in an equilibrium, whereas, physical equilibrium is equilibrium between two same phases of same composition of reactants and products. Equilibrium constants is used as an indicator to show relative amount between reactants and products. The direction where an equilibrium reaction will shift is assessed by Le Châtelier s Principle when an occurrence of varying conditions.
18 AUTHOR INFORMATION DR. YUEN MEI LIAN (SENIOR LECTURER) INDUSTRIAL CHEMISTRY PROGRAMME FACULTY OF INDUSTRIAL SCIENCES & TECHNOLOGY UNIVERSITI MALAYSIA PAHANG Tel. No. (Office): DR. SITI NOOR HIDAYAH MUSTAPHA (SENIOR LECTURER) INDUSTRIAL CHEMISTRY PROGRAMME FACULTY OF INDUSTRIAL SCIENCES & TECHNOLOGY UNIVERSITI MALAYSIA PAHANG Tel. No. (Office):
Chemical Equilibrium. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Chemical Equilibrium Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Equilibrium is a state in which there are no observable changes as time goes by. Chemical
More informationCHAPTER 3: CHEMICAL EQUILIBRIUM
CHAPTER 3: CHEMICAL EQUILIBRIUM 1 LESSON OUTCOME Write & explain the concepts of chemical equilibrium Derive the equilibrium constant Kc or Kp Solving the problem using the ICE table 2 Equilibrium is a
More informationChemical Equilibrium
Chemical Equilibrium Concept of Equilibrium Equilibrium Constant Equilibrium expressions Applications of equilibrium constants Le Chatelier s Principle The Concept of Equilibrium The decomposition of N
More informationChemical Equilibrium. Chapter
Chemical Equilibrium Chapter 14 14.1-14.5 Equilibrium Equilibrium is a state in which there are no observable changes as time goes by. Chemical equilibrium is achieved when: 1.) the rates of the forward
More informationCh 16. Chemical Equilibria. Law of Mass Action. Writing Equil Constant Expressions Homogeneous Equilibria. 2NO 2 (g) N 2 O 4 (g)
Copyright 001 by Harcourt, Inc. All rights reserved.! Ch 16. Chemical Equilibria N O 4 (g) NO (g) The concept of equilibrium and K Writing equilibrium constant expressions Relationship between kinetics
More informationCh 16. Chemical Equilibria. Law of Mass Action. Writing Equil Constant Expressions Homogeneous Equilibria. 2NO 2 (g) N 2 O 4 (g) equilibrium
Copyright 001 by Harcourt, Inc. All rights reserved.! Ch 16. Chemical Equilibria N O 4 (g) NO (g) The concept of equilibrium and K Writing equilibrium constant expressions Relationship between kinetics
More informationChemical Equilibrium. Chapter 8
Chemical Equilibrium Chapter 8 Equilibrium is a state in which there are no observable changes as time goes by. Chemical equilibrium is achieved when: the rates of the forward and reverse reactions are
More informationChapter 15. Chemical Equilibrium
Chapter 15. Chemical Equilibrium 15.1 The Concept of Equilibrium Consider colorless frozen N 2 O 4. At room temperature, it decomposes to brown NO 2. N 2 O 4 (g) 2NO 2 (g) At some time, the color stops
More informationC h a p t e r 13. Chemical Equilibrium
C h a p t e r 13 Chemical Equilibrium Chemical equilibrium is achieved when: the rates of the forward and reverse reactions are equal and the concentrations of the reactants and products remain constant
More informationThe Concept of Equilibrium
The Concept of Equilibrium Reversible reactions As the concentrations of the reactants decrease the rate of reaction in the forward direction decreases. As the concentrations of the products increase the
More information15.1 The Concept of Equilibrium
Lecture Presentation Chapter 15 Chemical Yonsei University 15.1 The Concept of N 2 O 4 (g) 2NO 2 (g) 2 Chemical equilibrium occurs when a reaction and its reverse reaction proceed at the same rate. The
More informationChemical Equilibrium. Professor Bice Martincigh. Equilibrium
Chemical Equilibrium by Professor Bice Martincigh Equilibrium involves reversible reactions Some reactions appear to go only in one direction are said to go to completion. indicated by All reactions are
More informationChapter 15. Chemical Equilibrium
Chapter 15. Chemical Equilibrium 15.1 The Concept of Equilibrium Consider colorless frozen N 2 O 4. At room temperature, it decomposes to brown NO 2. N 2 O 4 (g) 2NO 2 (g) At some time, the color stops
More informationChapter 15 Equilibrium
Chapter 15. Chemical Equilibrium 15.1 The Concept of Equilibrium Chemical equilibrium is the point at which the concentrations of all species are constant. A dynamic equilibrium exists when the rates of
More informationEquilibrium. Reversible Reactions. Chemical Equilibrium
Equilibrium Reversible Reactions Chemical Equilibrium Equilibrium Constant Reaction Quotient Le Chatelier s Principle Reversible Reactions In most chemical reactions, the chemical reaction can be reversed,
More informationChemical Equilibrium - Chapter 15
Chemical Equilibrium - Chapter 15 1. Dynamic Equilibrium a A + b B c C + d D At Equilibrium: Reaction is proceeding in both directions at the same rate. There is no net change in concentrations of reactants
More informationChemistry 123: Physical and Organic Chemistry Topic 4: Gaseous Equilibrium
Topic 4: Introduction, Topic 4: Gaseous Equilibrium Text: Chapter 6 & 15 4.0 Brief review of Kinetic theory of gasses (Chapter 6) 4.1 Concept of dynamic equilibrium 4.2 General form & properties of equilbrium
More informationThe Equilibrium State. Chapter 13 - Chemical Equilibrium. The Equilibrium State. Equilibrium is Dynamic! 5/29/2012
Chapter 13 - Chemical Equilibrium The Equilibrium State Not all chemical reactions go to completion; instead they attain a state of equilibrium. When you hear equilibrium, what do you think of? Example:
More informationCHEMISTRY. Chapter 15 Chemical Equilibrium
CHEMISTRY The Central Science 8 th Edition Chapter 15 Chemical Kozet YAPSAKLI The Concept of Chemical equilibrium is the point at which the concentrations of all species are constant. Chemical equilibrium
More informationCHEMISTRY XL-14A CHEMICAL EQUILIBRIA. August 20, 2011 Robert Iafe
CHEMISTRY XL-14A CHEMICAL EQUILIBRIA August 20, 2011 Robert Iafe Unit Overview 2 Reactions at Equilibrium Equilibrium Calculations Le Châtelier s Principle Catalysts Reactions at Equilibrium 3 Reversibility
More informationEquilibrium. What is equilibrium? Hebden Unit 2 (page 37 69) Dynamic Equilibrium
Equilibrium What is equilibrium? Hebden Unit (page 37 69) Dynamic Equilibrium Hebden Unit (page 37 69) Experiments show that most reactions, when carried out in a closed system, do NOT undergo complete
More informationChapter 15 Equilibrium
Chapter 15. Chemical Equilibrium Common Student Misconceptions Many students need to see how the numerical problems in this chapter are solved. Students confuse the arrows used for resonance ( )and equilibrium
More informationChapter 15 Chemical Equilibrium. Equilibrium
Chapter 15 Chemical The Concept of Chemical equilibrium occurs when a reaction and its reverse reaction proceed at the same rate. The Concept of As a system approaches equilibrium, both the forward and
More informationChemical Equilibrium. Foundation of equilibrium Expressing equilibrium: Equilibrium constants Upsetting equilibrium Le Chatelier
Chemical Equilibrium Foundation of equilibrium Expressing equilibrium: Equilibrium constants Upsetting equilibrium Le Chatelier Learning objectives Write equilibrium constant expressions for both solutions
More informationChemical Equilibrium
Chemical Equilibrium Chemical Equilibrium When compounds react, they eventually form a mixture of products and unreacted reactants, in a dynamic equilibrium. A dynamic equilibrium consists of a forward
More informationChapter Outline. The Dynamics of Chemical Equilibrium
Chapter Outline 14.1 The Dynamics of Chemical Equilibrium 14.2 Writing Equilibrium Constant Expressions 14.3 Relationships between K c and K p Values 14.4 Manipulating Equilibrium Constant Expressions
More information(i.e., equilibrium is established) leads to: K = k 1
CHEMISTRY 104 Help Sheet #8 Chapter 12 Equilibrium Do the topics appropriate for your lecture http://www.chem.wisc.edu/areas/clc (Resource page) Prepared by Dr. Tony Jacob Nuggets: Equilibrium Constant
More informationChapter 14 Chemical Equilibrium
Chapter 14 Chemical Equilibrium Fu-Yin Hsu Chemical reaction The speed of a chemical reaction is determined by kinetics. The extent of a chemical reaction is determined by thermodynamics. 14.1 Fetal Hemoglobin
More informationChapter 15 Equilibrium
Chapter 15. Chemical Equilibrium Common Student Misconceptions Many students need to see how the numerical problems in this chapter are solved. Students confuse the arrows used for resonance ( )and equilibrium
More information1. a. The rates of the forward and reverse reactions are equal at equilibrium.
CHATER THIRTEEN CHEMICAL EQUILIBRIUM For Review 1. a. The rates of the forward and reverse reactions are equal at equilibrium. b. There is no net change in the composition (as long as temperature is constant).
More information1301 Dynamic Equilibrium, Keq,
1301 Dynamic Equilibrium, Keq, and the Mass Action Expression The Equilibrium Process Dr. Fred Omega Garces Chemistry 111 Miramar College 1 Equilibrium Concept of Equilibrium & Mass Action Expression Extent
More informationEQUILIBRIA. e Q = a D B
I. Basis of Equilibrium. A. Q and equilibrium. EQUILIBRIA 1. Consider the general reaction bb + cc dd + ee a. Αs time elapses, [B] and [C] decrease causing the rate of the forward reaction to decrease.
More informationChapter 5. Chemistry for Changing Times, Chemical Accounting. Lecture Outlines. John Singer, Jackson Community College. Thirteenth Edition
Chemistry for Changing Times, Thirteenth Edition Lecture Outlines Chemical Accounting John Singer, Jackson Community College Chemical Sentences: Equations Chemical equations represent the sentences in
More informationChapter 13: Chemical Equilibrium
Chapter 13: Chemical Equilibrium 13.1 The Equilibrium Condition Equilibrium: a state in which no observable changes occur H 2 O (l) H 2 O (g) Physical equilibrium: no chemical change. N 2(g) + 3H 2(g)
More informationChapter 17. Equilibrium
Chapter 17 Equilibrium How Chemical Reactions Occur Chemists believe molecules react by colliding with each other. If a collision is violent enough to break bonds, new bonds can form. Consider the following
More informationTutorial 1 (not important for 2015)
Tutorial 1 (not important for 2015) 1 st Law of thermodynamics and other basic concepts Do No. 5 (05-03-2015) 1. One mole of an ideal gas is allowed to expand against a piston which supports 41 atm pressures.
More informationEQUILIBRIUM GENERAL CONCEPTS
017-11-09 WHEN THE REACTION IS IN EQUILIBRIUM EQUILIBRIUM GENERAL CONCEPTS The concentrations of all species remain constant over time, but both the forward and reverse reaction never cease When a system
More informationChapter Fifteen. Chemical Equilibrium
Chapter Fifteen Chemical Equilibrium 1 The Concept of Equilibrium Dynamic Equilibrium Opposing processes occur at equal rates Forward and reverses reaction proceed at equal rates No outward change is observed
More informationCHEMICAL EQUILIBRIUM Chapter 13
1 CHEMICAL EQUILIBRIUM Chapter 13 Pb 2+ (aq) + 2 Cl (aq) PbCl 2 (s) 1 Objectives Briefly review what we know of equilibrium Define the Equilibrium Constant (K eq ) and Reaction Quotient (Q) Determining
More information15/04/2018 EQUILIBRIUM- GENERAL CONCEPTS
15/04/018 EQUILIBRIUM- GENERAL CONCEPTS When a system is at equilibrium, the forward and reverse reactions are proceeding at the same rate. The concentrations of all species remain constant over time,
More informationCharacteristics of Chemical Equilibrium. Equilibrium is Dynamic. The Equilibrium Constant. Equilibrium and Catalysts. Chapter 14: Chemical Equilibrium
Characteristics of Chemical Equilibrium Chapter 14: Chemical Equilibrium 008 Brooks/Cole 1 008 Brooks/Cole Equilibrium is Dynamic Equilibrium is Independent of Direction of Approach Reactants convert to
More informationChapter 15 Chemical Equilibrium
Chapter 15 Chemical Chemical 15.1 The Concept of 15.2 The Constant (K) 15.3 Understanding and Working with Constants 15.4 Heterogeneous Equilibria 15.5 Calculating Constants 15.6 Applications of Constants
More informationAP* Chapter 13. Chemical Equilibrium
AP* Chapter 13 Chemical Equilibrium Section 13.1 The Equilibrium Condition Chemical Equilibrium The state where the concentrations of all reactants and products remain constant with time. On the molecular
More informationReaction Rate. Products form rapidly. Products form over a long period of time. Precipitation reaction or explosion
Reaction Rate Products form rapidly Precipitation reaction or explosion Products form over a long period of time Corrosion or decay of organic material Chemical Kinetics Study of the rate at which a reaction
More informationWrite a balanced reaction.. then write the equation.. then solve for something!!
Chapter 13 - Equilibrium Study Guide Purpose: This is a guide for your as you work through the chapter. The major topics are provided so that you can write notes on each topic and work the corresponding
More informationThe. Equilibrium. Constant. Chapter 15 Chemical Equilibrium. The Concept of Equilibrium. The Concept of Equilibrium. A System at Equilibrium
The Concept of Chapter 15 Chemical AP Chemistry 12 North Nova Education Centre 2017 Chemical equilibrium occurs when a reaction and its reverse reaction proceed at the same rate. The Concept of As a system
More informationFor the reaction: A B R f = R r. Chemical Equilibrium Chapter The Concept of Equilibrium. The Concept of Equilibrium
Chemical Equilibrium Chapter 15.1-4 This is the last unit of the year, and it contains quite a lot of material. Do not wait until the end of the unit to begin studying. Use what you have learned about
More informationChemical Equilibrium
Chemical Equilibrium Many reactions are reversible, i.e. they can occur in either direction. A + B AB or AB A + B The point reached in a reversible reaction where the rate of the forward reaction (product
More informationChemical Equilibria. OCR Chemistry A H432
Chemical Equilibria Chemical equilibrium is a dynamic equilibrium. Features of a dynamic equilibrium, which can only be established in a closed system (nothing added or removed): - rates of forward and
More informationc) Explain the observations in terms of the DYNAMIC NATURE of the equilibrium system.
Chemical Equilibrium - Part A: 1. At 25 o C and 101.3 kpa one mole of hydrogen gas and one mol of chlorine gas are reacted in a stoppered reaction vessel. After a certain time, three gases are detected
More informationAP CHEMISTRY NOTES 8-1 CHEMICAL EQUILIBRIUM: AN INTRODUCTION
AP CHEMISTRY NOTES 8-1 CHEMICAL EQUILIBRIUM: AN INTRODUCTION Chemical Equilibrium a dynamic state in which the rate of the forward reaction and the rate of the reverse reaction in a system are equal (the
More informationChemical Equilibrium. Many reactions are, i.e. they can occur in either direction. A + B AB or AB A + B
Chemical Equilibrium Many reactions are, i.e. they can occur in either direction. A + B AB or AB A + B The point reached in a reversible reaction where the rate of the forward reaction (product formation,
More informationCollision Theory. Unit 12: Chapter 18. Reaction Rates. Activation Energy. Reversible Reactions. Reversible Reactions. Reaction Rates and Equilibrium
Collision Theory For reactions to occur collisions between particles must have Unit 12: Chapter 18 Reaction Rates and Equilibrium the proper orientation enough kinetic energy See Both In Action 1 2 Activation
More informationChapter 13. Chemical Equilibrium
Chapter 13 Chemical Equilibrium Section 13.1 The Equilibrium Condition Chemical Equilibrium The state where the concentrations of all reactants and products remain constant with time. On the molecular
More informationGas Phase Equilibrium
Gas Phase Equilibrium Chemical Equilibrium Equilibrium Constant K eq Equilibrium constant expression Relationship between K p and K c Heterogeneous Equilibria Meaning of K eq Calculations of K c Solving
More informationChemical Equilibrium. Chemical Equilibrium
Chemical Equilibrium When some types of chemical reactions occur in the gas or solution phases, these reaction attain chemical equilibrium, i.e., the reaction does not go to completion, but the reaction
More informationCHAPTER 13 CHEMICAL EQUILIBRIUM. Questions. The Equilibrium Constant
CHATER 1 CHEMICAL EQUILIBRIUM Questions 10. a. This experiment starts with only H and N, and no NH present. From the initial mixture diagram, there is three times as many H as N molecules. So the green
More informationUNIT #10: Reaction Rates Heat/Energy in Chemical Reactions Le Chatlier s Principle Potential Energy Diagrams
UNIT #10: Reaction Rates Heat/Energy in Chemical Reactions Le Chatlier s Principle Potential Energy Diagrams NAME: 1. REACTION RATES a) The speed of a chemical reaction determined by the change in concentration
More informationChemical Equilibrium: Ch Dynamic Equilibrium. Dynamic Equilibrium. Three Approaches to Equilibrium The Equilibrium Constant Expression
Chemical Equilibrium: Ch. 15 15-1 Dynamic Equilibrium 15- The Equilibrium Constant Expression 15- Relationships Involving Equilibrium Constants 15-4 The Magnitude of an Equilibrium Constant 15-5 The Reaction
More informationChem 116 POGIL Worksheet - Week 7 Kinetics to Equilibrium
Chem 116 POGIL Worksheet - Week 7 Kinetics to Equilibrium Why? Most chemical reactions are reversible. This means that once products are formed, they can react to reform the reactants. If we allow a reaction
More informationChapter 14: Chemical Equilibrium. Mrs. Brayfield
Chapter 14: Chemical Equilibrium Mrs. Brayfield 14.2: Dynamic Equilibrium Remember from chapter 13 that reaction rates generally increase with increasing concentration of the reactions and decreases with
More informationChemical Kinetics and
Chemical Kinetics and Equilibrium Part 2: Chemical Equilibrium David A. Katz Department of Chemistry Pima Community College Tucson, AZ USA The Concept of Equilibrium Kinetics applies to the speed of a
More informationREACTION EQUILIBRIUM
REACTION EQUILIBRIUM A. REVERSIBLE REACTIONS 1. In most spontaneous reactions the formation of products is greatly favoured over the reactants and the reaction proceeds to completion (one direction). In
More informationChapter 15 Chemical Equilibrium
Equilibrium To be in equilibrium is to be in a state of balance: Chapter 15 Chemical Equilibrium - Static Equilibrium (nothing happens; e.g. a tug of war). - Dynamic Equilibrium (lots of things happen,
More information1.0 L container NO 2 = 0.12 mole. time
CHEM 1105 GAS EQUILIBRIA 1. Equilibrium Reactions - a Dynamic Equilibrium Initial amounts: = mole = 0 mole 1.0 L container = 0.12 mole moles = 0.04 mole 0 time (a) 2 In a 1.0 L container was placed 4.00
More informationChapter 6: Chemical Equilibrium
Chapter 6: Chemical Equilibrium 6.1 The Equilibrium Condition 6. The Equilibrium Constant 6.3 Equilibrium Expressions Involving Pressures 6.4 The Concept of Activity 6.5 Heterogeneous Equilibria 6.6 Applications
More informationChapter 13: Chemical Equilibrium
Chapter 13: Chemical Equilibrium May 5 2:04 PM 13.1 The Equilibrium Condition When you finish this section you will be able to list some characteristics of reactions at equilibrium. Chemical equilibrium
More informationChemical Equilibrium. A state of no net change in reactant & product concentrations. There is a lot of activity at the molecular level.
Chemical Equilibrium A state of no net change in reactant & product concentrations. BUT There is a lot of activity at the molecular level. 1 Kinetics Equilibrium For an elementary step in the mechanism:
More informationChapter Seven. Chemical Reactions: Energy, Rates, and Equilibrium
Chapter Seven Chemical Reactions: Energy, Rates, and Equilibrium Endothermic vs. Exothermic 2 Endothermic: A process or reaction that absorbs heat and has a positive ΔH. Exothermic: A process or reaction
More informationThe Extent of Chemical Reactions
Equilibrium: The Extent of Chemical Reactions The Equilibrium State and the Equilibrium Constant The Reaction Quotient and the Equilibrium Constant Equilibrium: The Extent of Chemical Reactions Expressing
More informationChemical Equilibrium-A Dynamic Equilibrium
CHAPTER 14 Page 1 Chemical Equilibrium-A Dynamic Equilibrium When compounds react, they eventually form a mixture of products and (unreacted) reactants, in a dynamic equilibrium Much like water in a U-shape
More informationExperiment #14 Virtual Chemistry Laboratory (Chemical Equilibrium) Le-Chatelier s principle
Experiment #14 Virtual Chemistry Laboratory (Chemical Equilibrium) Le-Chatelier s principle I. PURPOSE OF THE EXPERIMENT (i) To understand the basic concepts of chemical equilibrium (ii) To determine the
More informationChapter 8: Reaction Rates and Equilibrium
Chapter 8: Reaction Rates and Equilibrium ACTIVATION ENERGY In some reaction mixtures, the average total energy of the molecules is too low at the prevailing temperature for a reaction to take place at
More information1B Equilibrium. 3) Equilibrium is a dynamic state At equilibrium the rate in both directions must be the same.
1B Equilibrium The equilibrium constant, K c Characteristics of the equilibrium state 1) Equilibrium can only be established in a closed system. Matter cannot be exchanged with the surroundings (this will
More informationUnit 7 Kinetics and Thermodynamics
17.1 The Flow of Energy Heat and Work Unit 7 Kinetics and Thermodynamics I. Energy Transformations A. Temperature 1. A measure of the average kinetic energy of the particles in a sample of matter B. Heat
More informationUNIT 9 IB MATERIAL KINETICS & THERMODYNAMICS
UNIT 9 IB MATERIAL KINETICS & THERMODYNAMICS Name: ESSENTIALS: Know, Understand, and Be Able To State that combustion and neutralization are exothermic processes. Calculate the heat energy change when
More informationb. There is no net change in the composition (as long as temperature is constant).
CHAPTER THIRTEEN Questions 9. a. The rates of the forward and reverse reactions are equal at equilibrium. b. There is no net change in the composition (as long as temperature is constant). 10. False. Equilibrium
More informationCHEMICAL EQUILIBRIUM. Chapter 15
Chapter 15 P a g e 1 CHEMICAL EQUILIBRIUM Examples of Dynamic Equilibrium Vapor above a liquid is in equilibrium with the liquid phase. rate of evaporation = rate of condensation Saturated solutions rate
More informationChemical Reaction Engineering. Lecture 2
hemical Reaction Engineering Lecture 2 General algorithm of hemical Reaction Engineering Mole balance Rate laws Stoichiometry Energy balance ombine and Solve lassification of reactions Phases involved:
More informationEnergy Changes, Reaction Rates and Equilibrium. Thermodynamics: study of energy, work and heat. Kinetic energy: energy of motion
Energy Changes, Reaction Rates and Equilibrium Thermodynamics: study of energy, work and heat Kinetic energy: energy of motion Potential energy: energy of position, stored energy Chemical reactions involve
More informationChemical Kinetics. Chapter 13. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Chemical Kinetics Chapter 13 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Chemical Kinetics Thermodynamics does a reaction take place? Kinetics how fast does
More informationEntropy, Free Energy, and Equilibrium
Entropy, Free Energy, and Equilibrium Chapter 17 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Spontaneous Physical and Chemical Processes A waterfall runs
More informationChapter 18. Reversible Reactions. A chemical reaction in which the products can react to re-form the reactants is called a reversible reaction.
Section 1 The Nature of Chemical Equilibrium Reversible Reactions A chemical reaction in which the products can react to re-form the reactants is called a reversible reaction. Section 1 The Nature of Chemical
More information7/19/2011. Models of Solution. State of Equilibrium. State of Equilibrium Chemical Reaction
Models of Solution Chemistry- I State of Equilibrium A covered cup of coffee will not be colder than or warmer than the room temperature Heat is defined as a form of energy that flows from a high temperature
More informationRevision Notes on Chemical and Ionic Equilibrium
Revision Notes on Chemical and Ionic Equilibrium Equilibrium Equilibrium is the state of a process in which the properties like temperature, pressure, and concentration etc of the system do not show any
More informationQ.1 Write out equations for the reactions between...
1 CHEMICAL EQUILIBRIUM Dynamic Equilibrium not all reactions proceed to completion some end up with a mixture of reactants and products this is because some reactions are reversible; products revert to
More informationEnergy Diagram Endothermic Reaction Draw the energy diagram for exothermic and endothermic reactions. Label each part.
CP Chapter 18 Notes A Model for Reaction Rates Expressing Reaction Rates Average Rate = Δquantity Δtime The amount of increase or decrease depends on their mole ratios Units = or mol/ls Expressing Reaction
More informationThe Concept of Equilibrium
Chemical Equilibrium The Concept of Equilibrium Sometimes you can visually observe a certain chemical reaction. A reaction may produce a gas or a color change and you can follow the progress of the reaction
More informationEquilibrium Basics. The Reaction Quotient
Equilibrium Basics Any process which occurs in both directions necessarily has a point where the opposing rates will become equal. Why? From there on, there will be no further change in the macroscopic
More informationChemical Kinetics. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Chemical Kinetics Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Chemical Kinetics Thermodynamics does a reaction take place? Kinetics how fast does a reaction
More information2nd- Here's another example of a reversible reaction - dissolving salt in a beaker of water, described by the following reaction: NaCl (s)
CHEMICAL EQUILIBRIUM AP Chemistry (Notes) Most chemical processes are reversible. Reactants react to form products, but those products can also react to form reactants. Examples of reversible reactions:
More informationChemical Equilibrium. Equilibrium Constant
Chemical Equilibrium When some types of chemical reactions occur in the gas or solution phases, these reaction attain chemical equilibrium, i.e., the reaction does not go to completion, but the reaction
More informationAll reversible reactions reach an dynamic equilibrium state.
11. Equilibrium II Many reactions are reversible + 3 2 All reversible reactions reach an dynamic equilibrium state. Dynamic equilibrium occurs when forward and backward reactions are occurring at equal
More informationChapter 15. Chemical Equilibrium
1 Chapter 15. 15.1 The Concept of Equilibrium 1,2,3 Consider colorless frozen N 2 O 4. At room temperature, it decomposes to brown NO 2. N 2 O 4 (g) 2NO 2 (g) At some time, the color stops changing and
More informationEQUILIBRIUM. Opposing reactions proceed at equal rates Concs. of reactants & products do not change over time
EQUILIBRIUM Opposing reactions proceed at equal rates Concs. of reactants & products do not change over time Examples: vapor pressure above liquid saturated solution Now: equilibrium of chemical reactions
More informationChemical Equilibrium
Chemical Equilibrium Chemical Equilibrium The Concept of Equilibrium (15.1) Ways of Expressing Equilibrium Constants (15.2) What Does the Equilibrium Constant Tell Us? (15.3) Factors that Affect Chemical
More informationThermodynamics II. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Thermodynamics II Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Spontaneous Physical and Chemical Processes A waterfall runs downhill A lump of sugar dissolves
More information2.0 Equilibrium Constant
2.0 Equilibrium Constant When reactions are reversible and chemical equilibrium is reached, it is important to recognize that not all of the reactants will be converted into products. There is a mathematical
More informationChemical Equilibrium Basics
Chemical Equilibrium Basics Reading: Chapter 16 of Petrucci, Harwood and Herring (8th edition) Problem Set: Chapter 16 questions 25, 27, 31, 33, 35, 43, 71 York University CHEM 1001 3.0 Chemical Equilibrium
More informationCh14 Chemical Equilibrium. Modified by Dr. Cheng-Yu Lai
Ch14 Chemical Equilibrium Modified by Dr. Cheng-Yu Lai CHEMICAL EQUILIBRIUM Chemical Equilibrium: Chemical Equilibrium When the rate of the forward reaction equals the rate of the reverse reaction and
More information