Dynamic Equilibrium. O 2 Transport, Hg and equilibrium. Tro Chpt 14 Chemical Equilibrium
|
|
- Maximillian Simmons
- 5 years ago
- Views:
Transcription
1 Tro Chpt 14 Chemical Equilibrium The extent of chemical reactions The equilibrium constant, K Calculating equilibrium constants Predicting reaction directions Le Chatelier s Principle Suggested eoc problems for chapter 14:21, 27, 29, 31, 37, 41, 47, 51, 57, 61, 65 Tro 14.1 and 14.2 Dynamic Equilibrium Hemoglobin - a protein found in red blood cells that enhances the amount of O 2 that can be carried through the blood stream Hb + O 2 HbO 2 the concentrations of Hb, O 2, and HbO 2 are all interdependent the relative amounts of Hb, O 2, and HbO 2 at equilibrium are related to a constant called the equilibrium constant, K changing the concentration of any one of these necessitates changing the other concentrations to re-establish equilibrium O 2 Transport, Hg and equilibrium Tro 14.3 Dynamic Equilibrium and the equilibriuim constants K in the lungs, with high concentration of O 2, the equilibrium shifts to combine the Hb and O 2 together to make more HbO 2 N 2 O 4 2NO 2 (colorless) (brown) in the cells, with low concentration of O 2, the equilibrium shifts to break down the HbO 2 and increase the amount of free O 2 O 2 Hb + Oin 2 HbO 2 lungs cells
2 Dynamic Equilibrium continued The Significance of the Equilibrium constant K is small (e.g ) K is large (e.g. 50) cis-2-butene trans-2-butene K is intermediate (e.g. 1) Writing Equilibrium Constant Expressions: Relationships between K and the Chemical Equation N 2 + 3H 2 2NH 3 K expressions for individual reactions and overall reactions N 2 + O 2 2NO K c = 4.3 x NO + O 2 2NO 2 K c = 6.4 x 10 9 N 2 + 2O 2 2NO 2 K c =? NH 3 + O 2 2NO + H 2 O K c = 2.75 x 10-15
3 K and the direction of a chemical reaction 2 SO 2 + O 2 2 SO 3 vs. 2 SO 3 2 SO 2 + O 2 Tro 14.4 Expressing K in Terms of Pressure K p vs. K c Form of K and the coefficients of a chemical reaction SO 2 + 1/2O 2 SO 3 n(aa + bb cc + dd) N 2 (g) + 3H 2 (g) 2NH 3 (g) K c = 3.5 x 10 8 at 25 C K p = (3.5 x 10 8 )*(RT) (-2) = 5.8 x 10 5 Tro 14.5 Reactions involving Solids and Liquids Tro 14.6 and 14.8 Reaction tables, stoichiometry and equilibrium concentrations CaCO 3 (s) CaO (s) + CO 2 (g) Solids and pure liquids DO NOT appear in the reaction quotient or K expression In a study of the conversion of methane to other fuels, a chemical engineer mixes gaseous CH 4 and H 2 O in a 0.32 L flask at 1200 K. At equilibrium, the flask contains 0.26 mol of CO, mol of H 2 and mol of CH 4. What is [H 2 O] at equilibrium? K c = 0.26 for the reaction: CH 4 + H 2 O CO + 3H 2 Answer: [H 2 O] = 0.56 M
4 Reaction tables, stoichiometry and equilibrium concentrations Fuel engineers use the extent of the change from CO and H 2 O to CO 2 and H 2 to regulate the proportions of synthetic fuel mixtures. If mol of CO and mol of H 2 O are placed in a 125 ml flask at 900 K, what is the composition of the equilibrium mixture? By the way, at this temperature, K c is 1.56 for the reaction: CO (g) + H 2 O (g) CO 2 (g) + H 2 (g) If we have 2.00 M CO and 1.00 M H 2 O, what is the composition of the equilibrium mixture? Remember, K c is 1.56 for the reaction: CO (g) + H 2 O (g) CO 2 (g) + H 2 (g) Answer: [CO] = [H 2 O] = 0.89 M [CO 2 ] = [H 2 ] = 1.11 M Answer: [CO] = 1.27 M, [H 2 O] = 0.27 M [CO 2 ] = [H 2 ] = 0.73 M Do we ALWAYS have to use the quadratic expression? Tro 14.7 The Reaction Quotient Q: Predicting the Direction of Change Phosgene is a potential warfare agent that is now outlawed by international agreement. It decomposes by the reaction: COCl 2 (g) CO (g) + Cl 2 (g) K c = 8.3 x 10-4 at 360 C Calculate [CO], [Cl 2 ] and [COCl 2 ] when 5.00 mol of COCl 2 decomposes in a 10.0 liter flask. The reaction quotient has the same algebraic format as the equilibrium constant K N 2 O 4 2NO 2 Answer: [CO] = [Cl 2 ] = 2.0 x 10-2 M [COCl 2 ] = 0.48 M
5 Comparing Q to K N 2 O 4 2NO 2 (K) Tro 14.9 Stressing out a happy system Le Chatelier s Principle Le Chatelier s principle: when a chemical system at equilibrium is disturbed, it re-attains equilibrium by undergoing a net reaction that reduces the effect of the disturbance
6 Predicting the effect of a change in concentration on the equilibrium position To improve air quality and obtain a useful product, sulfur is often removed from coal and natural gas by treating the fuel contaminant hydrogen sulfide with O 2 : 2H 2 S (g) + O 2 (g) 2S (s) + 2H 2 O (g) Predicting the effect of a change in concentration on the equilibrium position for reactions involving gases How could you change the volume of the reaction to increase the yield of products? CaCO 3 (s) Cl 2 (g) + I 2 (g) CaO (s) + CO 2 (g) 2ICl (g) What happens to: a) [H 2 O] is O 2 is added b) [H 2 S] if O 2 is added c) [O 2 ] if H 2 S is removed d) [H 2 S] if sulfur is added S (s) + 3F 2 (g) SF 6 (g) The effect of a change in temperature PCl 3 (g) + Cl 2 (g) PCl 5 (g) ΔH rxn = -111 kj PCl 3 (g) + Cl 2 (g) PCl 5 (g) + heat The van t Hoff Equation: Changes in K with changes in T:
7 N 2 (g) + 3H 2 (g) NH 3 (g) ΔΗ rxn = kj N 2 (g) + 3H 2 (g) NH 3 (g) ΔΗ rxn = kj N 2 (g) + 3H 2 (g) NH 3 (g) ΔΗ rxn = kj
The 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 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 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 informationEquilibrium means that the rxn rates are equal. evaporation H20(l) condensation
Reversible reactions Most chemical reactions are reversible they can occur backwards as well as forwards reactants products Consider an open container of water (non-equilibrium) A closed water bottle is
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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 informationReaction Rates & Equilibrium. What determines how fast a reaction takes place? What determines the extent of a reaction?
Reaction Rates & Equilibrium What determines how fast a reaction takes place? What determines the extent of a reaction? Reactants Products 1 Reaction Rates Vary TNT exploding. A car rusting. Dead plants
More informationChemical Equilibria & the Application of Le Châtelier s Principle to General Equilibria
Chemical Equilibria & the Application of Le Châtelier s Principle to General Equilibria CHEM 102! T. Hughbanks! Example of Equilibrium N 2 (g) + 3H 2 (g) 2 NH 3 (g) Reactions can occur, in principle, in
More informationChapter 12: Chemical Equilibrium The Extent of Chemical Reactions
Chapter 12: Chemical Equilibrium The Extent of Chemical Reactions When a system reaches equilibrium, the [products] and [reactants] remain constant. A + B C + D [5M] [2M] [3M] [1.5M] Rate fwd = Rate rev
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 12: Chemical Equilibrium The Extent of Chemical Reactions
Chapter 12: Chemical Equilibrium The Extent of Chemical Reactions When a system reaches equilibrium, the [products] and [reactants] remain constant. A + B C + D [5M] [2M] [3M] [1.5M] Rate fwd = Rate rev
More informationReaction Rates & Equilibrium. What determines how fast a reaction takes place? What determines the extent of a reaction?
Reaction Rates & Equilibrium What determines how fast a reaction takes place? What determines the extent of a reaction? Reactants Products 1 Reaction Rates Vary TNT exploding. A car rusting. Dead plants
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 informationChemistry 1011 TOPIC TEXT REFERENCE. Gaseous Chemical Equilibrium. Masterton and Hurley Chapter 12. Chemistry 1011 Slot 5 1
Chemistry 1011 TOPIC Gaseous Chemical Equilibrium TEXT REFERENCE Masterton and Hurley Chapter 12 Chemistry 1011 Slot 5 1 12.4 Applications of the Equilibrium Constant YOU ARE EXPECTED TO BE ABLE TO: Determine
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 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 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 reactions with large K c (also K p) effectively go 100% to products.
th 7 Homework: Reading, M&F, ch. 13, pp. 506-524 (applications of equilibrium constants, Le Chatelier s Principle). Problems: Nakon, ch. 17, #9, 10, 12-15, 17, 24, 34; M&F, ch. 13, #41, 42, 44, 49, 51,
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 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 informationChapter 14 Lecture Lecture Presentation. Chapter 14. Chemical Equilibrium. Sherril Soman Grand Valley State University Pearson Education, Inc.
Chapter 14 Lecture Lecture Presentation Chapter 14 Chemical Equilibrium Sherril Soman Grand Valley State University Hemoglobin Hemoglobin is a protein (Hb), found in red blood cells, that reacts with O
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 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 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 informationAP Chem Chapter 12 Notes: Gaseous Equilibrium
AP Chem Chapter 12 Notes: Gaseous Equilibrium Equilibrium I. Equilibrium is reached when both the and reactions are occurring at. A. Dynamic Equilibrium: reactions are still occurring but the of reactants
More informationand mol of Cl 2 was heated in a vessel of fixed volume to a constant temperature, the following reaction reached equilibrium.
Q1. When a mixture of 0.45 mol of PCl and 0.68 mol of Cl was heated in a vessel of fixed volume to a constant temperature, the following reaction reached equilibrium. PCl + Cl PCl 5 H = 9 kj mol 1 At equilibrium,
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 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
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 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 information3. Indicate the mass action expression for the following reaction: 2X(g) + Y(g) 3W(g) + V(g) a) [X] 2 [Y][W] 3 [V] [W] 3 [V] [X] 2 [Y] [3W][V] [2X][Y]
1. Which of the following statements concerning equilibrium is not true? a) A system that is disturbed from an equilibrium condition responds in a manner to restore equilibrium. b) Equilibrium in molecular
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 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 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 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 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 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 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 information1.6 Chemical equilibria and Le Chatelier s principle
1.6 Chemical equilibria and Le Chatelier s principle Reversible reactions: Consider the reaction: Mg(s) + H2SO4(aq) MgSO4(aq) + H2(g) The reaction stops when all of the limiting reagent has been used up.
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 informationReview Unit #11. Review Unit # H 2 O (g) + CO (g) H 2(g) + CO 2(g) H>1
Review Unit #11 1. H 2 O (g) + CO (g) H 2(g) + CO 2(g) H>1 K c = 1.6 What effect would these changes have on the equilibrium position? a. Cool the mixture b. Increase the volume of the flask c. Add H 2(g)
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 informationK eq. b) 4 HCl (g) + O 2(g) 2 H 2 O (g) + 2 Cl 2(g) c) NOCl (g) NO (g) + ½ Cl 2(g) 1. d) Fe 3+ (aq) + SCN (aq) FeSCN 2+ (aq)
Name: 1 Equilibrium Worksheet SOLUTIONS Complete the following questions on a separate piece of paper. 1. Write the uilibrium epression,, for each of the following reactions: a) NO (g) + O (g) NO (g) [
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 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 informationUnit 13: Rates and Equilibrium- Guided Notes
Name: Period: What is a Chemical Reaction and how do they occur? Unit 13: Rates and Equilibrium- Guided Notes A chemical reaction is a process that involves of atoms Law of Conservation of : Mass is neither
More informationAP Chapter 14: Chemical Equilibrium & Ksp
AP Chapter 14: Chemical Equilibrium & Ksp Warm-Ups (Show your work for credit) Name Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. AP Chapter 14: Chemical Equilibrium & Ksp 2 Warm-Ups
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 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 informationReaction Rates and Chemical Equilibrium
Reaction Rates and Chemical Equilibrium 12-1 12.1 Reaction Rates a measure of how fast a reaction occurs. Some reactions are inherently fast and some are slow 12-2 12.2 Collision Theory In order for a
More informationReaction Rates and Chemical Equilibrium
Reaction Rates and Chemical Equilibrium : 12-1 12.1 Reaction Rates : a measure of how fast a reaction occurs. Some reactions are inherently fast and some are slow: 12-2 1 12.2 Collision Theory In order
More informationCalculations Involving the Equilibrium Constant K eq )
Calculations Involving the Equilibrium Constant K eq ) 1. Given the equilibrium equation below: A 2(g) + B 2(g) 2AB (g) If, at equilibrium, the concentrations are as follows: [A 2 ] = 3.45 M, [B 2 ] =
More informationChemistry 12 Unit 2: Dynamic Equilibrium. KEY Unit 2 Problem Set A KEY
Chemistry 12 Unit 2: Dynamic Equilibrium KEY Unit 2 Problem Set A KEY 1. Water is boiling in a kettle at 100 C. Is the system at equilibrium? Explain. No. The system is not closed. 2. Ice and water are
More informationEquilibrium point of any reaction is characterized by a single number: K eq is the equilibrium constant for the reaction
Lecture 19 Equilibrium Constant Equilibrium oint of any reaction is characterized by a single number: K eq is the equilibrium constant for the reaction In general: ja + kb R + qs K eq [ R] [ S] [ A] [
More informationChemistry 12: Dynamic Equilibrium Practice Test
Chemistry 12: Dynamic Equilibrium Practice Test A. Multiple Choice: For each question, select the best answer and record your choice on the answer key provided. /25 1) A system at equilibrium is said to
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 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 informationa) Write the expression for the equilibrium constant, K eq
Chemistry 12 K eq Calculations Worksheet Name: Date: Block: 1. Given the equilibrium equation below: A 2(g) + B 2(g) 2AB (g) If, at equilibrium, the concentrations are as follows: [A 2] = 3.45 M, [B 2]
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 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 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 information3 A (aq) + 2 D (aq) 4 C (g) + B (s) + 2 E (l)
AP Chemistry Test (Chapter 13) Multiple Choice (20%) 1) Which one best describes the K C for this reaction? 3 A (aq) + 2 D (aq) 4 C (g) + B (s) + 2 E (l) A) K c = [A] 3 [D] 2 B) K c = [C] 4 [B][E] 2 [C]
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 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 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 informationChemistry 1A Fall Midterm Exam 3
Chemistry 1A Fall 2017 Name Student ID Midterm Exam 3 You will have 120 minutes to complete this exam. Please fill in the bubble that corresponds to the correct answer on the answer sheet. Only your answer
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 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 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 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 informationGASEOUS EQUILIBRIUM CH. 12 EQUILIBRIUM
EQUILIBRIUM I. EQUILIBRIUM IS REACHED WHEN BOTH THE FORWARD AND REVERSE REACTIONS ARE OCCURRING AT THE SAME RATE. A. DYNAMIC EQUILIBRIUM: BOTH REACTIONS ARE STILL OCCURRING BUT THE CONCENTRATION OF REACTANTS
More informationChemical Kinetics and Equilibrium
Chemical Kinetics and Equilibrium 1 Which statement incorrectly describes a chemical reaction approaching equilibrium? As a chemical reaction approaches equilibrium, the net change in the amount of reactants
More informationCHEMICAL EQUILIBRIUM. Chapter 16. Pb 2+ (aq) + 2 Cl (aq) e PbCl 2 (s) PLAY MOVIE Brooks/Cole - Cengage
1 CHEMICAL EQUILIBRIUM Chapter 16 PLAY MOVIE Pb 2+ (aq) + 2 Cl (aq) e PbCl 2 (s) Properties of an Equilibrium Equilibrium systems are DYNAMIC (in constant motion) REVERSIBLE can be approached from either
More informationName: Unit!!: Kinetics and Equilibrium REGENTS CHEMISTRY
Name: Unit!!: Kinetics and Equilibrium REGENTS CHEMISTRY 1 Name: Unit!!: Kinetics and Equilibrium Collision theory states that a reaction is most likely to occur if reactant particles collide with the
More informationSurface Area (not in book) Reality Check: What burns faster, large or small pieces of wood?
Concentration Flammable materials burn faster in pure oxygen than in air because the of O 2 is greater. Hospitals must make sure that no flames are allowed near patients receiving oxygen. Surface Area
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 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 information