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Transcript of Chapter 13.1-13.4 AP Chem Chemical Equilibrium. 2 Chapter 13 Table of Contents Copyright © Cengage...
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Chapter 13.1-13.4AP Chem
Chemical Equilibrium
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Chapter 13
Table of Contents
Copyright © Cengage Learning. All rights reserved
13.1The Equilibrium Condition
13.2The Equilibrium Constant
13.3Equilibrium Expressions Involving Pressures
13.4Heterogeneous Equilibria
13.5Applications of the Equilibrium Constant
13.6 Solving Equilibrium Problems
13.7 Le Châtelier’s Principle
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Chapter 13
Table of Contents
Copyright © Cengage Learning. All rights reserved
• WEEK OUTLOOK• Monday - Notes 13.1-13.4 with problems w/sheet due
Tuesday - should be able to complete in class today.• *Be sure all reports are turned in and made up TODAY!• Tuesday - Notes 13.5-13.7 with emphasis on Le
Chatelier’s Principle emphasized & problems assigned due Wed. - some time in class to complete
• Kaci & Jonathan - library 2nd floor 7:30 with ACT invent.• Wednesday- Lab• Thursday - CAPS - No class• Friday - Good Friday - No school• Tuesday - April 2nd - ACT Testing 11th graders only.• Test probably next Thursday - just over ch. 13 only.
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Chapter 13
Table of Contents
Copyright © Cengage Learning. All rights reserved
• HANDOUTS - Ch. 13 NMSI Equilibrium Packet (Notes with practice problems)
• HANDOUT - Equilibrium Homework Sheet #1
• TURN IN Kinetics Lab - will go over pre-lab questions• HW: Equilibrium w/s #1 should be done today - due
Mon. for grade• HW: Notes packet #1-6 problems due next week but
keep for studying.• CW: Notes 13.1-13.4 • VOTE ON KINETICS TESTING CH. 12• Iodine Clock Rxn. Simulation Lab - as time permits
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Chapter FourteenGeneral Chemistry 4th edition, Hill, Petrucci, McCreary, PerryPrentice Hall © 2005Hall © 2005
Dynamic Nature of Equilibrium
When a system reaches equilibrium, the forward and reverse reactions continue to occur … but at equal rates.
We are usually concerned with the situation after equilibrium is reached.
After equilibrium the concentrations of reactants and products remain constant.
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Section 13.1
The Equilibrium Condition
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Chemical Equilibrium
• The state where the concentrations of all reactants and products remain constant with time.
• On the molecular level, there is frantic activity. Equilibrium is not static, but is a highly dynamic situation.
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Section 13.1
The Equilibrium Condition
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Equilibrium Is:
• Macroscopically static • Microscopically dynamic
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Section 13.1
The Equilibrium Condition
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Changes in Concentration
N2(g) + 3H2(g) 2NH3(g)
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Section 13.1
The Equilibrium Condition
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Chemical Equilibrium
• Concentrations reach levels where the rate of the forward reaction equals the rate of the reverse reaction.
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Section 13.1
The Equilibrium Condition
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The Changes with Time in the Rates of Forward and Reverse Reactions
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Section 13.1
The Equilibrium Condition
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Concept Check
Consider an equilibrium mixture in a closed vessel reacting according to the equation:
H2O(g) + CO(g) H2(g) + CO2(g)
You add more H2O(g) to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer.
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Section 13.1
The Equilibrium Condition
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Concept Check
Consider an equilibrium mixture in a closed vessel reacting according to the equation:
H2O(g) + CO(g) H2(g) + CO2(g)
You add more H2 to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer.
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Section 13.2
Atomic Masses
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The Equilibrium Constant
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Consider the following reaction at equilibrium:
jA + kB lC + mD
• A, B, C, and D = chemical species.
• Square brackets = concentrations of species at equilibrium.
• j, k, l, and m = coefficients in the balanced equation.
• K = equilibrium constant (given without units).
j
l
k
m
[B][A]
[D] [C]K =
Law of Mass ActionLaw of Mass Action
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Section 13.2
Atomic Masses
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The Equilibrium Constant
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Conclusions About the Equilibrium Expression
• Equilibrium expression for a reaction is the reciprocal of that for the reaction written in reverse.
• When balanced equation for a reaction is multiplied by a factor of n, the equilibrium expression for the new reaction is the original expression raised to the nth power;
• thus Knew = (Koriginal)n.
• K values are usually written without units.
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Conclusions about Equilibrium Conclusions about Equilibrium ExpressionsExpressions
The equilibrium expression for a reaction The equilibrium expression for a reaction is the reciprocal for a reaction written in is the reciprocal for a reaction written in reversereverse
2NO2NO22(g) (g) 2NO(g) + O 2NO(g) + O22(g(g))
2NO(g) + O2NO(g) + O22(g) (g) 2NO2NO22(g)(g)
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Conclusions about Equilibrium Conclusions about Equilibrium ExpressionsExpressions
When the balanced equation for a reaction When the balanced equation for a reaction is multiplied by a factor is multiplied by a factor nn, the equilibrium , the equilibrium expression for the new reaction is expression for the new reaction is the the original expressionoriginal expression, raised to the , raised to the nthnth power. power.
2NO2NO22(g) (g) 2NO(g) + O 2NO(g) + O22(g(g))
NONO22(g) (g) NO(g) + ½O NO(g) + ½O22(g(g))
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Section 13.2
Atomic Masses
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The Equilibrium Constant
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• K always has the same value at a given temperature regardless of the amounts of reactants or products that are present initially.
• For a reaction, at a given temperature, there are many equilibrium positions but only one value for K. Equilibrium position is a set of equilibrium
concentrations.
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Section 13.3
The Mole Equilibrium Expressions Involving Pressures
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• K involves concentrations - (also called Kc)
• Kp involves pressures for gases.
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Section 13.3
The Mole Equilibrium Expressions Involving Pressures
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Example
N2(g) + 3H2(g) 2NH3(g)
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Section 13.3
The Mole Equilibrium Expressions Involving Pressures
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Example
N2(g) + 3H2(g) 2NH3(g)
Equilibrium pressures at a certain temperature:
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Section 13.3
The Mole Equilibrium Expressions Involving Pressures
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Example
N2(g) + 3H2(g) 2NH3(g)
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Section 13.3
The Mole Equilibrium Expressions Involving Pressures
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The Relationship Between K and Kp
Kp = K(RT)Δn
• Δn = sum of the coefficients of the gaseous products minus the sum of the coefficients of the gaseous reactants.
• R = 0.08206 L·atm/mol·K• T = temperature (in kelvin)
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Section 13.3
The Mole Equilibrium Expressions Involving Pressures
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Example
N2(g) + 3H2(g) 2NH3(g)
Using the value of Kp (3.9 × 104) from the previous example, calculate the value of K at 35°C.
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Section 13.4
Heterogeneous Equilibria
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Homogeneous Equilibria
• Homogeneous equilibria – involve the same phase:
N2(g) + 3H2(g) 2NH3(g)
HCN(aq) H+(aq) + CN-(aq)
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Section 13.4
Heterogeneous Equilibria
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Heterogeneous Equilibria
• Heterogeneous equilibria – involve more than one phase:
2KClO3(s) 2KCl(s) + 3O2(g)
2H2O(l) 2H2(g) + O2(g)
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Section 13.4
Heterogeneous Equilibria
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• The position of a heterogeneous equilibrium does not depend on the amounts of pure solids or liquids present. The concentrations of pure liquids and solids
are constant.
2KClO3(s) 2KCl(s) + 3O2(g)
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Chapter FourteenGeneral Chemistry 4th edition, Hill, Petrucci, McCreary, PerryPrentice Hall © 2005Hall © 2005
Equilibria Involving PureSolids and Liquids
• The equilibrium constant expression does not include terms for pure solid and liquid phases because their concentrations do not change in a reaction.
• Although the amounts of pure solid and liquid phases change during a reaction, these phases remain pure and their concentrations do not change.
[CaO] [CO2]Kc = –––––––––– [CaCO3]
Kc = [CO2]
Example: CaCO3(s) CaO(s) + CO2(g)
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Section 13.4
Heterogeneous Equilibria
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ASSIGNMENTS - 2/20/14
• W/sheet #1 problems due Monday • This assignment should be able to be completed today
in class but is due Monday.
• Ch. 13 Equilibrium packet - #1-#6 practice problems - answers shown to see if you are doing correctly.
• Prepare for Test on Kinetics.• HW: Read chapter 13 over the next week.
• Ch. 12 Kinetics Test - VOTED for WEDNESDAY - Feb 26