OFB Chapter 7 Chemical Equilibrium
|
|
- Phillip Nelson
- 6 years ago
- Views:
Transcription
1 OFB Chapter 7 Chemical Equilibrium 7-1 Chemical Reactions in Equilibrium 7-2 Calculating Equilibrium Constants 7-3 The Reaction Quotient 7-4 Calculation of Gas-Phase Equilibrium 7-5 The effect of External Stresses on Equilibria: Le Châtelier s Principle 7-6 Heterogeneous Equilibrium 7-7 Extraction and Separation Processes 9/22/2004 OFB Chapter 7 1
2 Last Day to Drop Oct. 8 All exercises Homework: Chapter 7: -8, 14, 24, 42, 54 Mid-Term Grades Due Sept. 24 Satisfactory Note: this is all that s on WebCT Be familiar with equilibrium problems these are very important Unsatisfactory 9/24/2004 OFB Chapter 7 1
3 forward aa + bb cc + reverse dd 9/22/2004 OFB Chapter 7 3 ~220 K (-53 o C)
4 7-1 Chemical Reactions and Equilibrium The equilibrium condition for every reaction can be summed up in a single equation in which a number, the equilibrium constant (K) of the reaction, equals an equilibrium expression, a function of properties of the reactants and products. H 2 O(l) H 2 25 o C Temperature ( o C) Vapor Pressure (atm) K = H 2 O(l) H 2 30 o C K = /22/2004 OFB Chapter 7 4
5 Chemical Reactions and Equilibrium H 2 O (l) H 2 O (g) P H 2O P ref = K P ref is numerically equal to 1 The convention in the book is to express all pressures in atmospheres and to omit factors of P ref because their value is unity. An equilibrium constant K is a pure number. 9/22/2004 OFB Chapter 7 5
6 Chemical Reactions and Equilibrium 2 NO 2 (g) N 2 O 4 (g) N 2 O 4 (g) 2 NO 2 (g) An equilibrium reaction 9/22/2004 OFB Chapter 7 6
7 Chemical Reactions and Equilibrium 2 NO 2 (g) N 2 O 4 (g) N 2 O 4 (g) 2 NO 2 (g) T T P P 2 NO 2 (g) N 2 O 4 (g); K = 25 o C 9/22/2004 OFB Chapter 7 7
8 Chemical Reactions and Equilibrium As the equilibrium state is approached, the forward and backward rates of reaction approach equality. At equilibrium the rates are equal, and no further net change occurs in the partial pressures of reactants or products. Four fundamental characteristics of equilibrium states in isolated systems: 1. They display no macroscopic evidence of change. 2. They are reached through spontaneous processes. 3. They show a dynamic balance of forward and backward processes. 4. They are the same regardless of the direction from which they are approached. forward aa + bb cc + reverse dd 9/22/2004 OFB Chapter 7 8
9 The Form of Equilibrium Expressions forward aa + bb cc + reverse dd In a chemical reaction in which a moles of species A and b moles of species B react to form c moles of species C and d moles of species D, the partial pressures at equilibrium are related through provided that all species are present as low-pressure gases. 9/22/2004 OFB Chapter 7 9
10 Exercise 7-1 Write equilibrium expressions for the reactions defined by the following equations: 3 H 2 (g) + SO 2 (g) H 2 S(g) + 2 H 2 O(g) 2 C 2 F 5 Cl(g) + 4 O 2 (g) Cl 2 (g) + 4 CO 2 (g) + 5 F 2 (g) 9/22/2004 OFB Chapter 7 10
11 Example Calculating Equilibrium Constants Consider the equilibrium 4 NO 2 (g) 2 N 2 O(g) + 3 O 2 (g) The three gases are introduced into a container at partial pressures of 3.6 atm (for NO 2 ), 5.1 atm (for N 2 O), and 8.0 atm (for O 2 ) and react to reach equilibrium at a fixed temperature. The equilibrium partial pressure of the NO 2 is measured to be 2.4 atm. Calculate the equilibrium constant of the reaction at this temperature, assuming that no competing reactions occur. initial partial pressure (atm) change in partial pressure (atm) equilibrium partial pressure (atm) 4 NO 2 (g) 2 N 2 O(g) + 3 O 2 (g) 9/22/2004 OFB Chapter 7 11
12 4 NO 2 (g) 2 N 2 O(g) + 3 O 2 (g) initial partial pressure (atm) change in partial pressure (atm) equilibrium partial pressure (atm) 3.6-4x = 2.4 atm NO 2 ; x = 0.3 atm (0.3 atm) = 5.7 atm N 2 O (0.3 atm) = 8.9 atm O 2 K = (P N 2 O )2 (P O2 ) 3 (P NO2 ) 4 = (5.7)2 (8.9) 3 (2.4) 4 = 9/22/2004 OFB Chapter 7 12
13 Exercise 7-2 The compound GeWO 4 (g) forms at high temperature in the reaction 2 GeO (g) + W 2 O 6 (g) 2 GeWO 4 (g) Some GeO (g) and W 2 O 6 (g) are mixed. Before they start to react, their partial pressures both equal atm. After their reaction at constant temperature and volume, the equilibrium partial pressure of GeWO 4 (g) is atm. Assuming that this is the only reaction that takes place, (a) determine the equilibrium partial pressures of GeO and W 2 O 6, and (b) determine the equilibrium constant for the reaction. initial partial pressure (atm) change in partial pressure (atm) equilibrium partial pressure (atm) 2 GeO (g) + W 2 O 6 (g) 2 GeWO 4 (g) 9/22/2004 OFB Chapter 7 13
14 2 GeO(g) + W 2 O 6 (g) 2 GeWO 4 (g) initial partial pressure (atm) change in partial pressure (atm) equilibrium partial pressure (atm) 0 + 2x = atm GeWO 4 ; x = atm (0.490) = atm GeO = atm W 2 O 6 K = (P GeWO2 ) 2 (P GeO ) 2 (P W2 O 6 ) = (0.980) 2 (0.020) 2 (0.510) 9/22/2004 OFB Chapter 7 14
15 Relationships Among the K s of Related Reactions Rule 1: The equilibrium constant for a reverse reaction is always the reciprocal of the equilibrium constant for the corresponding forward reaction. #1 #2 2 H 2 (g) + O 2 (g) 2 H 2 O(g) 2 H 2 O(g) 2 H 2 (g) + O 2 (g) (P H 2O )2 (P H 2 )2 (P O 2 ) = K 1 (P H 2 )2 (P O 2 ) (P H 2O )2 = K 2 K 1 = 1/K 2 9/22/2004 OFB Chapter 7 15
16 Relationships Among the K s of Related Reactions Rule 2: When the coefficients in a balanced chemical equation are all multiplied by a constant factor, the corresponding equilibrium constant is raised to a power equal to that factor. #1 #3 2 H 2 (g) + O 2 (g) 2 H 2 O(g) Rxn 1 H 2 (g) + ½ O 2 (g) H 2 O(g) Rxn 3 (P H 2O ) (P H 2 )(P O2 )½ = K 3 K 3 = K 1½ = K 1 9/22/2004 OFB Chapter 7 16
17 Relationships Among the K s of Related Reactions Rule 3: when chemical equations are added to give a new equation, their equilibrium constants are multiplied to give the equilibrium constant associated with the new equation. 2 BrCl(g) Br 2 (g) + Cl 2 (g) Br 2 (g) + I 2 (g) 2 IBr(g) (P Br 2 )(P Cl2 ) (P BrCl ) 2 = K 1 = 25 o C (P IBr ) 2 (P Br 2 ) (P I2 ) = K 2 = 25o C = K 1 K 2 = (0.45)(0.051) 25 o C 9/22/2004 OFB Chapter 7 17
18 ( ) c P ( P ) D ( P ) a ( P ) 7-3 The Reaction Quotient forward aa + bb cc + reverse d C = b A B K ( ) c P ( P ) D ( P ) a ( P ) d C = b A B dd Note that K (the Equilibrium Constant) uses equilibrium partial pressures Note that Q (the reaction quotient) uses prevailing partial pressures, not necessarily at equilibrium Q 9/22/2004 OFB Chapter 7 18
19 The Reaction Quotient forward aa + bb cc + reverse c ( P ) ( PD ) a ( P ) ( P ) d C = b A B Q dd If Q < K, reaction proceeds in a forward direction (toward products); If Q > K, reaction proceeds in a backward direction (toward reactants); If Q = K, the reactions stops because the reaction is in equilibrium. 9/22/2004 OFB Chapter 7 19
20 Exercise 7-4 The equilibrium constant for the reaction P 4 (g) 2 P 2 (g) is 1.39 at 400 o C. Suppose that 2.75 mol of P 4 (g) and 1.08 mol of P 2 (g) are mixed in a closed 25.0 L container at 400 o C. Compute Q (init) (the Q at the moment of mixing) and state the direction in which the reaction proceeds. P 2 P 2 = K = 1 P4 ( ) P ( ) 1.39 K = 400 o C; n P4 (init) = 2.75 mol; n P 2 (init) P P 4(init) = n P 4(init)RT/V Q =? K PV = nrt = 1.08 mol P P 2(init) = n P 2(init)RT/V Q = (2.39) 2 /(6.08) = < 1.39; Q < K 9/22/2004 OFB Chapter 7 20
21 7-4 Calculations of Gas-Phase Equilibria Exercise 7-5 Carbon monoxide reacts with water to give hydrogen: CO (g) +H 2 O (g) CO 2 (g) + H 2 (g) At 900 K, the equilibrium constant for this reaction, the socalled shift reaction, equals suppose the partial pressures of three gases at equilibrium at 900 K are P CO = 2.00 atm, P CO2 = 0.80 atm, and P H2 =0.48 atm Calculate the partial pressure of water under these conditions. 9/22/2004 OFB Chapter 7 21
22 7-4 Calculations of Gas-Phase Equilibria Exercise 7-5 Carbon monoxide reacts with water to give hydrogen: CO (g) +H 2 O (g) CO 2 (g) + H 2 (g) At 900 K, the equilibrium constant for this reaction, the so-called shift reaction, equals suppose the partial pressures of three gases at equilibrium at 900 K are P CO = 2.00 atm, P CO2 = 0.80 atm, and P H2 =0.48 atm Calculate the partial pressure of water under these conditions. 9/22/2004 OFB Chapter 7 22
23 Solving quadratic equations 9/22/2004 OFB Chapter 7 23
24 7-5 Effects of External Stresses on Equilibria: Le Châtelier s Principle A system in equilibrium that is subjected to a stress reacts in a way that counteracts the stress. Le Châtelier s Principle provides a way to predict the response of an equilibrium system to an external perturbation, such as Effects of Adding or Removing Reactants or Products Effects of Changing the Volume of the System Effects of Changing the Temperature 9/22/2004 OFB Chapter 7 24
25 Effects of Adding or Removing Reactants or Products PCl 5 (g) PCl 3 (g) + Cl 2 (g) add extra PCl 5 (g) add extra PCl 3 (g) remove some PCl 5 (g) remove some PCl 3 (g) ( )( 1 ) P P PCl3 Cl2 ( ) 1 P PCl 5 1 = Q 9/22/2004 OFB Chapter 7 25
26 Effects of Changing the Volume of the System PCl 5 (g) PCl 3 (g) + Cl 2 (g) Let s decrease the volume of the reaction container Let s increase the volume of the reaction container 9/22/2004 OFB Chapter 7 26
27 V reactants > V products V reactants < V products V reactants = V products Volume Decreased (Pressure Increased) Equilibrium shift right (toward products) Equilibrium Shifts left (toward reactants) Equilibrium not affected Volume Increased (Pressure Decreased) Equilibrium Shifts left (toward reactants) Equilibrium shift right (toward products) Equilibrium not affected 2 P 2 (g) P 4 (g) PCl 5 (g) PCl 3 (g) + Cl 2 (g) CO (g) +H 2 O (g) CO 2 (g) + H 2 (g) 9/22/2004 OFB Chapter 7 27
28 Effects of Changing the Temperature PCl 5 (g) PCl 3 (g) + Cl 2 (g) Let s increase the temperature of the reaction Let s decrease the temperature of the reaction 9/22/2004 OFB Chapter 7 28
29 Endothermic Reaction (absorb heat) Temperature Raised Equilibrium shift right (toward products) Temperature Lowered Equilibrium Shifts left (toward reactants) Exothermic Reaction (liberate heat) Equilibrium Shifts left (toward reactants) Equilibrium shift right (toward products) If a forward reaction is exothermic, Then the reverse reaction must be endothermic 9/22/2004 OFB Chapter 7 29
30 Effects of Changing the Temperature PCl 5 (g) PCl 3 (g) + Cl 2 (g) K = 300 o C = Q Let s increase the temperature of the reaction Let s decrease the temperature of the reaction 9/22/2004 OFB Chapter 7 30
31 Driving Reactions to Completion Industrial Synthesis of Ammonia N 2 (g) + 3H 2 (g) 2NH 3 (g) Forward reaction exothermic V reactants > V products Volume Decreased (Pressure Increased) Equilibrium shift right (toward products) Volume Increased (Pressure Decreased) Equilibrium Shifts left (toward reactants) Exothermic Reaction (liberate heat) Temperature Raised Equilibrium Shifts left (toward reactants) Temperature Lowered Equilibrium shift right (toward products) 9/22/2004 OFB Chapter 7 31
32 ( ) c P ( P ) D ( P ) a ( P ) A Review: Chemical Equilibrium forward aa + bb cc + reverse B d b ( ) c P ( P ) D ( P ) a ( P ) d C = b A B Q dd C = K Q =? K 1. Effects of Adding or Removing Reactants or Products 2. Effects of Changing the Volume (or Pressure) of the System 3. Effects of Changing the Temperature 9/22/2004 OFB Chapter 7 32
33 Exercise 7-10 State the effect of an increase in temperature and also of a decrease in volume on the equilibrium yield of the products in each of the following reactions. a) CH 3 OCH 3 (g) + H 2 O (g) 2 CH 4 (g) + O 2 (g) Increase Temp? Decrease Volume? b) H 2 O (g) + CO (g) HCOOH (g) Increase Temp? Decrease Volume? 9/22/2004 OFB Chapter 7 33
34 Heterogeneous Equilibrium Solids CaCO 3 (s) CaO(s) + CO 2 (g) Liquids H 2 O(l) H 2 O(g) Dissolved species I 2 (s) I 2 (aq) 9/22/2004 OFB Chapter 7 34
35 Law of Mass Action 1. Gases enter equilibrium expressions as partial pressures, in atmospheres. E.g., P CO2 2. Dissolved species enter as concentrations, in moles per liter. E.g., [Na + ] 3. Pure solids and pure liquids are represented in equilibrium expressions by the number 1 (unity); a solvent taking part in a chemical reaction is represented by unity, provided that the solution is dilute. E.g., I 2 K ( s) = [ I [ I 2 ( aq)] ( s)] 2 I 2 ( aq) = [ I ( aq)] 1 9/22/2004 OFB Chapter = [ I 2 ]
36 Law of Mass Action 4. Partial pressures and concentrations of products appear in the numerator and those of the reactants in the denominator. Each is raised to a power equal to its coefficient in the balanced chemical equation. aa + bb cc + dd 9/22/2004 OFB Chapter 7 36
37 Exercise 7-11 Write equilibrium-constant equations for the following Equilibria: (a) Si 3 N 4 (s) + 4 O 2 (g) 3 SiO 2 (s) + 2 N 2 O(g) (b) O 2 (g) + 2 H 2 O(l) 2 H 2 O 2 (aq) (c) CaH 2 (s) + 2 C 2 H 5 OH(l) Ca(OC 2 H 5 ) 2 (s) + 2 H 2 (g) 9/22/2004 OFB Chapter 7 37
38 Exercise 7-12 A vessel holds pure CO (g) at a pressure of atm and a temperature of 354K. A quantity of nickel is added, and the partial pressure of CO (g) drops to an equilibrium value of atm because of the reaction Ni (s) + 4CO (g) Ni(CO) 4 (g) Compute the equilibrium constant for this reaction at 354K. 9/22/2004 OFB Chapter 7 38
39 Exercise 7-12 A vessel holds pure CO (g) at a pressure of atm and a temperature of 354K. A quantity of nickel is added, and the partial pressure of CO (g) drops to an equilibrium value of atm because of the reaction Ni (s) + 4CO (g) Ni(CO) 4 (g) Compute the equilibrium constant for this reaction at 354K. P Ni(CO) 4 Ni(CO) 4 K = = 4 4 (PCO) [Ni(s)] (PCO) P (1) initial partial pressure (atm) change in partial pressure (atm) equilibrium partial pressure (atm) P CO (atm) P Ni(CO)4 (atm) 9/22/2004 OFB Chapter 7 39
40 7-7 Extraction and Separation Processes Extraction Partitioning of a solute between two immiscible solvents Chromatography Solute is partitioned between a mobile phase and a stationary phase Column Chromatography Gas-liquid Chromatography 9/22/2004 OFB Chapter 7 40
Chapter 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 informationCHAPTER 7: Chemical Equilibrium
CHAPTER 7: Chemical Equilibrium Chemical Reactions and Equilibrium Calculating Equilibrium Constants The Reaction Quotient Calculation of Gas-Phase Equilibria The effect of External Stresses: Le Châtelier
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 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 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 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 9. Chemical Equilibrium
Chapter 9. Chemical Equilibrium 9.1 The Nature of Chemical Equilibrium -Approach to Equilibrium [Co(H 2 O) 6 ] 2+ + 4 Cl- [CoCl 4 ] 2- + 6 H 2 O Characteristics of the Equilibrium State example) H 2 O(l)
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 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. 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 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 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 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 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 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 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. 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 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 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 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 informationEquilibrium and Reversible Rxns. CHAPTER 14 Chemical Equilibrium. What happens? Stoichiometry
CHAPTER 14 Chemical Equilibrium 17-1 What happens? Stoichiometry How Fast? Kinetics applies to the speed of a reaction, the concentration of product that appears (or of reactant that disappears) per unit
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 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 informationChapter 6: Chemical Equilibrium
Chapter 6: Chemical Equilibrium 6.1 The Equilibrium Condition 6.2 The Equilibrium Constant 6.3 Equilibrium Expressions Involving Pressures 6.4 The Concept of Activity 6.5 Heterogeneous Equilibria 6.6 Applications
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 informationChemical Equilibria 2
Chemical Equilibria 2 Reading: Ch 14 sections 6-9 Homework: Chapter 14: 27*, 29*, 31, 33, 41, 43, 45, 51*, 55, 61*, 63, 67*, 69* * = important homework question Review A chemical equilibrium and its respective
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 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. 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 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 13. The Concept of Equilibrium. A System at Equilibrium. The Concept of Equilibrium. Chemical Equilibrium. N 2 O 4 (g) 2 NO 2 (g)
PowerPoint to accompany The Concept of Equilibrium Chapter 13 Chemical Equilibrium Figure 13.1 Chemical equilibrium occurs when a reaction and its reverse reaction proceed at the same rate. The Concept
More informationLe Châtelier's Principle. Chemical Equilibria & the Application of Le Châtelier s Principle to General Equilibria. Using Le Châtelier's Principle
Chemical Equilibria & the Application of Le Châtelier s Principle to General Equilibria CHEM 107 T. Hughbanks Le Châtelier's Principle When a change is imposed on a system at equilibrium, the system will
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 informationUnit 2 Pre-Test Reaction Equilibrium
Unit 2 Pre-Test Reaction Equilibrium Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Consider the following equilibrium system: 2HF(g) F 2(g) + H 2 (g)
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 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 informationLecture Presentation. Chapter 15. Chemical Equilibrium. James F. Kirby Quinnipiac University Hamden, CT Pearson Education
Lecture Presentation Chapter 15 Chemical James F. Kirby Quinnipiac University Hamden, CT The Concept of N 2 O 4 (g) 2 NO 2 (g) Chemical equilibrium occurs when a reaction and its reverse reaction proceed
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 informationChemical 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 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 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 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. 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 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 informationChemical & Solubility Equilibrium (K eq, K c, K p, K sp )
Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Unit 8 (Chp 15,17): Chemical & Solubility (K eq, K c, K p, K sp ) John D. Bookstaver St. Charles
More informationJanuary 03, Ch 13 SB equilibrium.notebook
Ch 13: Chemical Equilibrium exists when 2 opposing reactions occur simultaneously at the same rate (dynamic rather than static) Forward rate = reverse rate https://www.youtube.com/watch?v=wld_imyqagq The
More informationChapter 1 The Atomic Nature of Matter
Chapter 1 The Atomic Nature of Matter 1-1 Chemistry: Science of Change 1-2 The Composition of Matter 1-3 The Atomic Theory of Matter 1-4 Chemical Formulas and Relative Atomic Masses 1-5 The Building Blocks
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 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 information(g) + 3 H 2. (g) 2 NH 3. 1) Only gases and dissolved species appear in an equilibrium expression. 4 NH 3. O(g) K c = (s) + 2N 2.
Chapter 16: Chemical Equilibrium What is meant by an equilibrium system? What is an equilibrium expression? N 2 +3 H 2 2 NH 3 1) Only gases and dissolved species appear in an equilibrium expression. 4
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 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 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 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 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 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 informationHomework 03. Chemical Equilibria
HW03 - Chemical Equilibria! This is a preview of the published version of the quiz Started: Feb 14 at 9:1am Quiz Instruc!ons Homework 03 Chemical Equilibria Question 1 When the chemical reaction A + B
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 informationCollision Theory. Collision theory: 1. atoms, ions, and molecules must collide in order to react. Only a small number of collisions produce reactions
UNIT 16: Chemical Equilibrium collision theory activation energy activated complex reaction rate reversible reaction chemical equilibrium law of chemical equilibrium equilibrium constant homogeneous equilibrium
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 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 equilibrium. As you read ask yourself
Chemical equilibrium Reading: Chapter 15 (omit 15.7) As you read ask yourself What is meant by chemical equilibrium? How does the equilibrium constant expression depend on the nature of the species (liquids,
More informationChem chemical reactions can go forward as well as in the reverse direction. concentrations of reactants and products become constant over time
Chemical equilibrium Reading: Chapter 15 (omit 15.7) As you read ask yourself What is meant by chemical equilibrium? How does the equilibrium constant expression depend on the nature of the species (liquids,
More informationK P VERSUS K C PROPERTIES OF THE EQUILIBRIUM CONSTANT
K P VERSUS K C 1. What are the units of K p and K c for each of the following? a) 2H 2 S(g) 2H 2 (g) + S 2 (g) b) 4NH 3 (g) + 3O 2 (g) 2N 2 (g) + 6H 2 O(g) 2. What are the units of K p and K c for each
More informationLe Châtelier s Principle. 19 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. Equilibrium: Le Châtelier s Principle
Factors Affecting : Le Châtelier s Principle Pressure Factors Affecting : Le Châtelier s Principle Pressure When volume decreases, the pressure increases. systems in which some reactants and products are
More informationEquilibrium. Forward and Backward Reactions. Hydrogen reacts with iodine to make hydrogen iodide: H 2 (g) + I 2 (g) 2HI(g)
Equilibrium Forward and Backward Reactions Hydrogen reacts with iodine to make hydrogen iodide: H 2 (g) + I 2 (g) 2HI(g) forward rate = k f [H 2 ][I 2 ] 2HI(g) H 2 (g) + I 2 (g) backward rate = k b [HI]
More informationThe N 2 O 4 -NO 2 Equilibrium
Chemical Equilibria William L Masterton Cecile N. Hurley Edward J. Neth cengage.com/chemistry/masterton Chapter 1 Gaseous Chemical Equilibrium For a gaseous chemical equilibrium, more than one gas is present:
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 informationThe Equilibrium State
15.1 The Equilibrium State All reactions are reversible and under suitable conditions will reach a state of equilibrium. At equilibrium, the concentrations of products and reactants no longer change because
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
Chemical Equilibrium What is equilibrium? Expressions for equilibrium constants, K eq ; Calculating K eq using equilibrium concentrations; Factors that affect equilibrium; Le Chatelier s Principle What
More informationDr. Valverde s AP Chemistry Class
AP* Chemistry Dr. Valverde s AP Chemistry Class Chapter CHEMICAL 13 Review: EQUILIBRIA: Chemical Equilibrium GENERAL CONCEPTS THE NATURE OF THE EQUILIBRIUM STATE: Equilibrium is the state where the rate
More informationCHEMICAL EQUILIBRIUM. 6.3 Le Chatelier s Principle
CHEMICAL EQUILIBRIUM 6.3 Le Chatelier s Principle At the end of the lesson, students should be able to: a) State Le Chatelier s principle b) Explain the effect of the following factors on a system at equilibrium
More informationChapter 16 - Principles of Chemical Equilibrium
Chapter 16 - Principles of Chemical Equilibrium -allreactions are "reversible" - principle of micro-reversibility - the "committed step" - much theory - not always obvious - for some the reverse reaction
More informationCHEMICAL EQUILIBRIA: GENERAL CONCEPTS
CHEMICAL EQUILIBRIA: GENERAL CONCEPTS THE NATURE OF THE EQUILIBRIUM STATE: Equilibrium is the state where the concentrations of all reactants and products remain constant with time. (in stoichiometry,
More informationChapter 17: Spontaneity, Entropy, and Free Energy
Chapter 17: Spontaneity, Entropy, and Free Energy Review of Chemical Thermodynamics System: the matter of interest Surroundings: everything in the universe which is not part of the system Closed System:
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 informationDynamic Equilibrium Illustrated
שו וי מ שק ל Equilibrium Reactants Products In an equilibrium, the forward and reverse processes continue to occur but at equal rates! The reactant and product concentrations remain constant We are usually
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 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 informationCHEM J-8 June /01(a) With 3 C-O bonds and no lone pairs on the C atom, the geometry is trigonal planar.
CHEM1001 2014-J-8 June 2014 22/01(a) What is the molecular geometry of the formate ion? Marks 7 With 3 C-O bonds and no lone pairs on the C atom, the geometry is trigonal planar. Write the equilibrium
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 informationA.P. Chemistry. Unit #11. Chemical Equilibrium
A.P. Chemistry Unit #11 Chemical Equilibrium I. Chemical Equilibrium the point in a reaction at which the concentrations of products and reactants remain constant Dynamic Equilibrium the equilibrium condition
More informationaa + bb ---> cc + dd
17 Chemical Equilibria Consider the following reaction: aa + bb ---> cc + dd As written is suggests that reactants A + B will be used up in forming products C + D. However, what we learned in the section
More informationCHEM Dr. Babb s Sections Lecture Problem Sheets
CHEM 116 - Dr. Babb s Sections Lecture Problem Sheets Kinetics: Integrated Form of Rate Law 61. Give the integrated form of a zeroth order reaction. Define the half-life and find the halflife for a general
More informationWhat does the magnitude of the equilibrium constant tell us? N2(g) + O2(g) N2 O2(g) N2(g) + 3H2(g) 2NH3(g) In Short
What does the magnitude of the equilibrium constant tell us? N2(g) + O2(g) N2 O2(g) N2(g) + 3H2(g) 2NH3(g) In Short 1 D. Altering Chemical Equations and the Effect on the Equilibrium Constant What is the
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 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 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 informationChapter 15: Chemical Equilibrium. Chem 102 Dr. Eloranta
Chapter 15: Chemical Equilibrium Chem 102 Dr. Eloranta Equilibrium State in which competing processes are balanced so that no observable change takes place as time passes. Lift Gravity Sometimes called
More informationUnit 5: Spontaneity of Reaction. You need to bring your textbooks everyday of this unit.
Unit 5: Spontaneity of Reaction You need to bring your textbooks everyday of this unit. THE LAWS OF THERMODYNAMICS 1 st Law of Thermodynamics Energy is conserved ΔE = q + w 2 nd Law of Thermodynamics A
More informationChemical Equilibrium
Chemical Equilibrium 1 Equilibrium We ve already used the phrase equilibrium when talking about reactions. In principle, every chemical reaction is reversible... capable of moving in the forward or backward
More informationChapter 15 Equilibrium
Chapter 15. Chemical Equilibrium Sample Exercise 15.1 (p. 632) Write the equilibrium expression for K eq for these three reactions: a) 2 O 3(g) 3 O 2(g) b) 2 NO (g) + Cl 2(g) 2 NOCl (g) c) Ag + (aq) +
More informationChapter 15: Chemical Equilibrium: How Much Product Does a Reaction Really Make?
Chapter 15: Chemical Equilibrium: How Much Product Does a Reaction Really Make? End-of-Chapter Problems: 15.1-15.10, 15.13-15.14, 15.17-15.91, 15.94-99, 15.10-15.103 Example: Ice melting is a dynamic process:
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 8 Thermochemistry: Chemical Energy. Chemical Thermodynamics
Chapter 8 Thermochemistry: Chemical Energy Chapter 8 1 Chemical Thermodynamics Chemical Thermodynamics is the study of the energetics of a chemical reaction. Thermodynamics deals with the absorption or
More informationChem 1B Dr. White 1 Chapter 13: Chemical Equilibrium Outline Chemical Equilibrium. A. Definition:
Chem 1B Dr. White 1 Chapter 13: Chemical Equilibrium Outline 13.1. Chemical Equilibrium A. Definition: B. Consider: N 2 O 4 (g, colorless) 2NO 2 (g, brown) C. 3 Main Characteristics of Equilibrium 13.2-13.4.
More informationShifting Equilibrium. Section 2. Equilibrium shifts to relieve stress on the system. > Virginia standards. Main Idea. Changes in Pressure
Section 2 Main Ideas Equilibrium shifts to relieve stress on the system. Some ionic reactions seem to go to completion. Common ions often produce precipitates. > Virginia standards CH.3.f The student will
More informationENTHALPY, ENTROPY AND FREE ENERGY CHANGES
ENTHALPY, ENTROPY AND FREE ENERGY CHANGES Refer to the following figures for Exercises 1-6. The lines on the vertical axis represent the allowed energies. Assume constant spacing between levels to determine
More informationChapter 6 General Concepts of Chemical Equilibrium
Chapter 6 General Concepts of Chemical Equilibrium Introduction Chemical Equilibrium Ø The state where the concentrations of all reactants and products remain constant with time. Ø Equilibrium is not static,
More information