CHEM Dr. Babb s Sections Lecture Problem Sheets
|
|
- Brianna Elliott
- 5 years ago
- Views:
Transcription
1 CHEM 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 zeroth order reaction. Is the half life constant? For a zeroth order reaction, what type of plot will yield a straight line? 62. Give the integrated form of a first order reaction. Find the half-life for a general first order reaction. Is the half-life constant? For a first order reaction, what type of plot will yield a straight line? A. A certain first order reaction has the rate law Rate = k[a] with k= sec -1. If the initial concentration of A is 0.75 M, what will be the concentration of A after 1 minute? What is the half-life for this reaction? How much time will it take for 75% of A to react? How much A will be left after the passage of three half-lives? What is the initial rate of the reaction? 63. Give the integrated form of a second order reaction. Find the half-life for a general second order reaction. Is the half-life constant? For a second order reaction, what type of plot will yield a straight line? 64. The following data were collected for the reaction: 2 HI(g) > H 2 (g) + I 2 (g) at 580K. Time (min) [HI] M M M M M Determine the reaction order and form of the rate law. (HINT: Plot [HI] vs. t, ln[hi] vs. t and 1/[HI] vs. t.) Calculate the numerical values of the specific rate constant and the halflife of the reaction. After how much time will only 20% of the original amount of HI remain? Kinetics: Elementary Reactions, Mechanisms, Catalysis and Arrhenius Equation 65. Define the terms: elementary step and reaction mechanism. Can the rate law be written directly for an elementary reaction? 66. A reaction mechanism that occurs in polluted air is the following: NO 2 + O 3 > NO 3 + O 2 SLOW NO 3 + NO 2 > N 2 O 5 FAST Write the net reaction for this process, define the molecularity of each elementary step and write the rate law for this process. What is happening to the NO 3? 67. A reaction mechanism for the destruction of ozone, O 3, in the stratosphere is: O 3 > O 2 + O FAST O 3 + O > 2 O 2 SLOW Write the net reaction, define the molecularity of each elementary step and write the rate law for this process. Identify the intermediate. 68. A reaction mechanism for the destruction of ozone by high flying aircraft is the following: O 3 > O 2 + O
2 NO + O 3 > NO 2 + O 2 NO 2 + O > NO + O 2 Write the net reaction and define the molecularity of each elementary step. Identify any reaction intermediates and catalysts. 69. Define the following terms: transition state and activation energy. On a molecular level, how does an increase in temperature lead to an increase in reaction rate? Give the Arrhenius equation. Show how the Arrhenius equation can be used to calculate the activation energy and pre-exponential factor. 70. The specific rate constant for the formation of HI was measured at two different temperatures. Calculate the numerical values of the activation energy and preexponential factor. Calculate the value of the specific rate constant at 427 C. H 2 + I 2 > 2 HI k (1/M-s) Temp (K) The following rate constants were found for the decomposition of N 2 O 5 at four different temperatures. k (1/s) Temp ( C) Make a plot of ln(k) vs. 1/T. Calculate the activation energy and pre-exponential factor from the plot. What is the value of the specific rate constant at C? 72. How does a catalyst increase the rate of a reaction? Is the reaction mechanism the same in the presence of a catalyst? Chemical Equilibrium: Introduction to K p and K c 73. Define the following terms: equilibrium, equilibrium constant expression, and equilibrium constant. 74. Do all reactions go 100 % to completion (such that all reactants react to form products)? Are the concentrations of reactants and products changing at equilibrium? In a chemical reaction, once equilibrium is established it is referred to as a dynamic equilibrium. What does this mean? 75. At equilibrium, how are the rates of the forward and reverse reactions related? 76. For the general elementary reaction below, write the rate law for the forward reaction (Forward Rate=?) and the rate law for the reverse reaction (Reverse Rate=?). Derive the equilibrium constant (K) and equilibrium constant expression (K=?) by setting the Forward Rate = Reverse Rate. aa + bb < > cc + dd 77. Does the numerical value of the equilibrium constant K depend on temperature? 78. Consider the equation below. What does the value of K c tell you about the relative values of k f and k r? What does the value of K c tell you about the concentrations of products and reactants at equilibrium? COCl 2 (g) < > CO(g) + Cl 2 (g) K c =
3 79. Consider the equation below. What does the value of K c tell you about the relative values of k f and k r? What does the value of K c tell you about the concentrations of products and reactants at equilibrium? PCl 3 (g) + Cl 2 (g) < > PCl 5 (g) K c = When K c is large (K>10 +3 ), how do the concentrations of reactants and products compare? When K c is small (K<10-3 ), how do the concentrations of reactants and products compare? When K c is intermediate (10-3 <K<10 +3 ), how do the concentrations of reactants and products compare? 81. Write the equilibrium constant expressions for the chemical reactions below. A. 4 NH 3 (g) + 5 O 2 (g) < > 4 NO (g) + 6 H 2 O(g) K c =? B. 3 Fe(s) + 4 H 2 O(g) < > Fe 3 O 4 (s) + 4 H 2 (g) K c =? C. COCl 2 (g) < > CO(g) + Cl 2 (g) K c =? D. PCl 3 (g) + Cl 2 (g) < > PCl 5 (g) K c =? E. NH 3 (aq) + H 2 O(l) < > NH + 4 (aq) + OH - (aq) K c =? F. H 2 O(s) < > H 2 O(g) K c =? G. 2 NaHCO 3 (s) < > Na 2 CO 3 (s) + H 2 O(l) + CO 2 (g) K c =? 82. Are pure solids, pure liquids and solvents included in the equilibrium constant expression? Why not? 83. Given the chemical reaction below, calculate the numerical value of the equilibrium constant for the reactions in A, B, C and D. N 2 (g) + 3 H 2 (g) < > 2 NH 3 (g) K c = at 25 C A. 2 NH 3 (g) < > N 2 (g) + 3 H 2 (g) K c =? B. 3 N 2 (g) + 9 H 2 (g) < > 6 NH 3 (g) K c =? C. ½ N 2 (g) + 3/2 H 2 (g) < > NH 3 (g) K c =? D. NH 3 (g) < > ½ N 2 (g) + 3/2 H 2 (g) K c =? 84. Write the equilibrium constant expression (K p ) in terms of partial pressures for the general reaction: aa(g) + bb(g) > cc(g) + dd(g) where a, b, c, d are coefficients 85. Write the equilibrium constant expressions (K p ) for the reactions below: A. 2 SO 2 (g) + O 2 (g) < > 2 SO 3 (g) B. N 2 (g) + 3 H 2 (g) < > 2 NH 3 (g) C. 4 NH 3 (g) + 5 O 2 (g) < > 4 NO (g) + 6 H 2 O(g) 86. For the reaction in 85A, K c = at a temperature of 727 C. What is the numerical value of K p? 87. What is the general mathematical equation that can be used to calculate K c from K p? K c from K p? 88. Calculate the equilibrium constant in terms of partial pressures (K p ) for the reaction below: CO(g) + 3 H 2 (g) < > CH 4 (g) + H 2 O(g) K c = 3.91 at 927 C 89. Calculate the equilibrium constant in terms of concentrations (K c ) for the reaction below: CO(g) + H 2 O(g) < > CO 2 (g) + H 2 (g) K p = 0.58 at 727 C Under what conditions will K c and K p be equal (have the same value)?
4 Chemical Equilibrium: Reaction Quotient and Concentration Problems 90. What is the form of the reaction quotient Q c? What concentrations are used to calculate the numerical value of the reaction quotient? 91. Consider the reaction below with the given initial concentrations of products and reactants. Is the reaction already at equilibrium? If not, which way will it proceed to attain equilibrium? (HINT: Calculate Q c and compare its value to K c ) CO(g) + 3 H 2 (g) < > CH 4 (g) + H 2 O(g) K c = 3.91 at 927 C Initial: M M M M 92. If Q c is greater than K c, which way will the reaction proceed in order to attain equilibrium (left to right or right to left)? If Q c is less than K c, which way will the reaction proceed in order to attain equilibrium (left to right or right to left)? If Q c is equal to K c, which way will the reaction proceed in order to attain equilibrium (left to right or right to left)? 93. A 10.0 L vessel contains mol CO 2 and mol of CO. Some solid carbon C(s) is added and temperature is raised to 1000 C. Will more CO(g) form? The reaction is shown below. (HINT: Calculate Q c and compare it to K c ) CO 2 (g) + C(s) < > 2 CO(g) K c =1.17 at 1000 C 94. Consider the reaction given below 2 NOBr(g) < > 2 NO(g) + Br 2 (g) K c = at 24 C For each of the following compositions, describe in which direction the reaction will go to reach equilibrium. A. [NOBr]= M C. [NOBr]=0.500 M [NO]= M [NO]= M [Br 2 ]= M [Br 2 ]= M B. [NOBr]=0.115 M [NO]= M [Br 2 ]= M 95. Calculate the missing concentrations and the numerical value of K c for the following: A. 2 ICl(g) < > I 2 (g) + Cl 2 (g) K c =? Initial: M 0.22M Change: At Eq: 0.09M B. H 2 (g) + I 2 (g) < > 2 HI(g) K c =? Initial: M Change: M At Eq: C. 3 A + 2 B < > C + 2 D K c =? Initial: 6.00M 2.00M 1.00M 0 Change: 0.50M At Eq: 96. If 0.50 mol PCl 5 is injected into a 2.0L vessel, what will be the equilibrium concentrations of all species? PCl 5 (g) < > PCl 3 (g) + Cl 2 (g) K c =1.8 at 250 C
5 97. Initially a mixture contains mol each of N 2 and O 2 in an 8.00 L vessel. Calculate the equilibrium concentration of gaseous NO. N 2 (g) + O 2 (g) < > 2 NO(g) K c = Consider the reaction below which is already at equilibrium. Calculate the partial pressures of NO 2 and N 2 O 4 when the total pressure is increased to 20 atm. 2 NO 2 (g) < > N 2 O 4 (g) At Eq: 0.25 atm 0.25 atm Chemical Equilibrium: Le Chatelier s Principle 99. State Le Chatelier s Principle. List the types of stresses that can be applied to a system at equilibrium Why does the addition of a catalyst to an equilibrium mixture not change the equilibrium? Why does an increase of pressure due to addition of an inert gas not change the equilibrium concentrations of reactants and products? 101. If the temperature is changed, does the value of K C change? Why? 102. Consider the reaction below 2 ICl(g) < > I 2 (g) + Cl 2 (g) K c =0.12 At Eq: 0.26M 0.09M 0.09M What will happen (in which direction will the reaction proceed) if the following changes occur? A M ICl is added B M I 2 is added C. All of the Cl 2 is removed 103. Consider the reaction below which is at equilibrium BaSO 4 (s) < > BaO(s) + SO 3 (g) What will happen if more solid BaSO 4 is added? more solid BaO is added? 104. For a reaction at equilibrium, the pressure is increased by decreasing the volume. Will the equilibrium concentrations of species be altered? Is the numerical value of K c or K p changed? 105. Consider the reaction below which has already attained equilibrium N 2 O(g) + NO 2 (g) < > 3 NO(g) K c = at 200 C Which way will the reaction proceed to reach equilibrium if the pressure is increased by decreasing the volume? 106. For the reaction CO(g) + H 2 O(g) < > H 2 (g) + CO 2 (g) Will a decrease in pressure by increasing volume alter the equilibrium concentrations of all species? 107. A certain reaction is exothermic ()H= negative). What happens to the numerical value of K c if the temperature is increased? if the temperature is decreased? 108. A certain reaction is endothermic ()H= positive). What happens to the numerical value of K c if the temperature is increased? if the temperature is decreased? 109. Consider the reaction below which has already attained equilibrium N 2 H 4 (g) + H 2 (g) < > 2 NH 3 (g) )H= kj In which direction will the reaction proceed if the temperature is increased? 110. Consider the reaction below which has already attained equilibrium N 2 (g) + O 2 (g) < > 2 NO(g) )H=+181 kj In which direction will the reaction proceed if the temperature is increased?
6 CHEM 116-Dr. Babb s Section Answer Key to Exam II Lecture Problem Sheet 61. Integrated form of zeroth order rate law: [A] t = -kt + [A] 0 Half-life is the time it takes for half of original amount of reactant to react such that only half remains. For zeroth order reaction, half-life equation is J = [A] 0 /2k and half-life is not constant but directly proportional to initial concentration of reactant (J%[A] 0 or as [A] 0 8, J8). For zeroth order reaction, a plot of [A] t vs. t will yield a straight line. 62. Integrated form of first order rate law: ln[a] t = -kt + ln[a] 0 For first order reaction, half-life equation is J = ln2/k and half-life is a constant and not dependent on initial concentration of reactant. For first order reaction, a plot of ln[a] t vs. t will yield a straight line. A. [A] after 1 minute is 0.50 M; Half-life (J)= sec; it will take sec for 75% of A to react; after three half-lives M of A remains; the initial rate of the reaction is M/sec. 63. Integrated form of second order rate law: 1/[A] t = kt + 1/[A] 0 For second order reaction, half-life equation is J = 1/k[A] 0 and half-life is not constant but inversely proportional to initial concentration of reactant (J%1/[A] 0 or as [A] 0 8, J9). For first order reaction, a plot of 1/[A] t vs. t will yield a straight line. 64. Reaction is second order in [HI] and Rate Law is: Rate = k[hi] 2 ; k = M -1 min -1 ; J=0.696 min; it will take 2.8 min for 20% of the original amount of HI to remain. 66. Net Rxn: 2 NO 2 + O 3 > N 2 O 5 + O 2 ; Both steps are bimolecular; Rate = k[no 2 ][O 3 ]; The NO 3 is an intermediate. 67. Net Rxn: 2 O 3 > 3 O 2 ; First elementary step is unimolecular while second is bimolecular; Rate = k[o 3 ][O]; The O is an intermediate. 68. Net Rxn: 2 O 3 > 3 O 2 ; First elementary step is unimolecular while second and third are bimolecular; the O and NO 2 are intermediates; the NO is a catalyst. 70. Activation Energy (E A )= J/mol; Pre-exponential factor (A) = M -1 sec -1 ; Specific rate constant (k) at 427 C = M -1 sec Activation Energy (E A )= J/mol; Pre-exponential factor (A) = M -1 sec -1 ; Specific rate constant (k) at 427 C = 0.17 sec Numerical value of K depends only on T but does not depend on initial concentrations of reactants or products. 78. Since K C for this reaction is less than 1 and K C =k f /k r, then k r > k f. Since K C =[Products]/[Reactants] and for this reaction K C <1, then [Reactants]>[Products]. 79. Since K C for this reaction is greater than 1 and K C =k f /k r, then k f > k r. Since K C =[Products]/[Reactants] and for this reaction K C >1, then [Products]>[Reactants]. 80. When K C > 10 3, then [Products] >> [Reactants] and reaction proceeds essentially 100% to completion. When K C < 10-3, then [Reactants] >> [Products] and reaction proceeds hardly at all to completion. When 10-3 < K C < 10 3, then [Products] ~ [Reactants] and appreciable amounts (experimentally measurable quantities) of both reactants and products are present. 81. A. K c = [NO] 4 [H 2 O] 6 /[NH 3 ] 4 [O 2 ] 5 B. K c = [H 2 ] 4 /[H 2 O] 4
7 C. K c = [CO][Cl 2 ]/[COCl 2 ] D. K c = [PCl 5 ]/[PCl 3 ][Cl 2 ] E. K c = [NH + 4 ][OH - ]/[NH 3 ] F. K c = [H 2 O] G. K c = [CO 2 ] 82. Concentrations for pure solids, pure liquids and the solvent are not included in the equilibrium constant expression because these concentrations depend only on density and don t vary (i.e. are constant). These constant concentrations are already included into the numerical value of K. 83. A B C D A. K p = (p SO3 ) 2 /(p SO2 ) 2 (p O2 ) B. K p = (p NH3 ) 2 /(p H2 ) 3 (p N2 ) C. K p = (p NO ) 4 (p H2O ) 6 /(p NH3 ) 4 (p O2 ) K p =K c (RT) )n or K c =K p (RT) -)n ; Whenever )n gas = 0, then K c =K p. 90. Reaction quotient (Q C ) has same form as K C except non-equilibrium or initial concentrations are used to calculate Q C. 91. Q C =6.25 and Q c > K c. Thus this reaction is not at equilibrium and will proceed from right to left in order to reach equilibrium. 92. If Q c > K c, reaction proceeds from right to left in order to reach eq. If Q c < K c, reaction proceeds from left to right in order to reach eq. If Q c = K c, reaction is at equilibrium and will not react in a net way in either direction. 93. Q C =0.202 and Q c < K c. Thus this reaction is not at equilibrium and will proceed from left to right in order to reach equilibrium and more gaseous CO will be formed. 94. A. Q C = and Q c > K c. Thus this reaction is not at equilibrium and will proceed from right to left in order to reach equilibrium. B. Q C = and Q c = K c. Thus this reaction is at equilibrium and will not react in a net way in either direction. C. Q C = and Q c < K c. Thus this reaction is not at equilibrium and will proceed from left to right in order to reach equilibrium. 95. A. 2 ICl(g) < > I 2 (g) + Cl 2 (g) K c =0.1 Initial: M 0.22M Change: +0.26M -0.13M -0.13M At Eq: 0.26M 0.09 M 0.09M B. H 2 (g) + I 2 (g) < > 2 HI(g) K c =137 Initial: M Change: M M M At Eq: 0.365M 0.365M 4.270M
8 C. 3 A + 2 B < > C + 2 D K c = Initial: 6.00M 2.00M 1.00M 0 Change: -0.75M -0.50M +0.25M 0.50M At Eq: 5.25M 1.50M 1.25M 0.50M 96. [Cl 2 ] = [PCl 3 ] = 0.22 M; [PCl 5 ]=0.03 M M 98. p NO2 =2.1 atm; p N2O4 =18 atm 102. A. reaction proceeds from left to right in order to regain eq. B. reaction proceeds from right to left in order to regain eq. C. reaction proceeds from left to right in order to regain eq Addition of more solid BaSO 4 or BaO will have no effect on the eq. because concentrations of pure solids are not included in the eq. constant expression If total pressure is altered, the numerical value of K is not changed. The only factor influencing the value of K is temperature. However, a change in the total pressure does change the partial pressures of gaseous species and may remove the reaction from eq as P increases V decreases and reaction will proceed toward side of equation that occupies less volume. This means that reaction will proceed toward side of equation that has less moles of gas. In this instance, reaction will proceed toward the reactants in order to regain eq as P decreases due to V increase reaction will proceed toward side of equation that occupies more volume (i.e. toward side of equation with more moles of gas). However, in this case both sides of equation have same # moles of gas and thus occupy same volume. As a result, the eq. of this reaction is unaffected by changes in P due to V change as T increases, K C decreases or as T decreases, K C increases for an exothermic reaction as T increases, K C increases or as T decreases, K C decreases for an endothermic reaction as T increases, Heat increases so heat on the product side is increased and reaction will proceed from right to left in order to regain eq as T increases, Heat increases so heat on reactant side is increased and reaction will proceed from left to right in order to regain eq.
(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 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. 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 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 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 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 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 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 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 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 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 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 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 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 informationSection 10. Rates of Reactions Goal: Learn how temperature, concentration, and catalysts affect the rate of reaction. Summary
Chapter 10 Reaction Rates and Chemical Equilibrium Section 10. Rates of Reactions Goal: Learn how temperature, concentration, and catalysts affect the rate of reaction. Summary The rate of a reaction is
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 informationHomework 07. Kinetics
HW07 - Kine!cs Started: Mar at 10:56am Quiz Instruc!ons Homework 07 Kinetics Question 1 Consider the reaction: O (g) 3O (g) rate = k[o ] [O ] 3 3 What is the overall order of the reaction and the order
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 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 14 Chemical Kinetics
Chapter 14 Chemical Kinetics Factors that Affect Reaction rates Reaction Rates Concentration and Rate The Change of Concentration with Time Temperature and Rate Reactions Mechanisms Catalysis Chemical
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 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 informationChapter 11: CHEMICAL KINETICS
Chapter : CHEMICAL KINETICS Study of the rate of a chemical reaction. Reaction Rate (fast or slow?) Igniting gasoline? Making of oil? Iron rusting? We know about speed (miles/hr). Speed Rate = changes
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. Chapter 14 Chemical Kinetics
CHEMISTRY The Central Science 8 th Edition Chapter 14 Kozet YAPSAKLI kinetics is the study of how rapidly chemical reactions occur. rate at which a chemical process occurs. Reaction rates depends on The
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 informationBrown et al, Chemistry, 2nd ed (AUS), Ch. 12:
Kinetics: Contents Brown et al, Chemistry, 2 nd ed (AUS), Ch. 12: Why kinetics? What is kinetics? Factors that Affect Reaction Rates Reaction Rates Concentration and Reaction Rate The Change of Concentration
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 informationChapter 13 Kinetics: Rates and Mechanisms of Chemical Reactions
Chapter 13 Kinetics: Rates and Mechanisms of Chemical Reactions 14.1 Focusing on Reaction Rate 14.2 Expressing the Reaction Rate 14.3 The Rate Law and Its Components 14.4 Integrated Rate Laws: Concentration
More informationChemical Kinetics Ch t ap 1 er
Chemical Kinetics Chapter 13 1 Chemical Kinetics Thermodynamics does a reaction take place? Kinetics how fast does a reaction proceed? Reaction rate is the change in the concentration of a reactant or
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 informationQuestions 1-3 relate to the following reaction: 1. The rate law for decomposition of N2O5(g) in the reaction above. B. is rate = k[n2o5] 2
Questions 1-3 relate to the following reaction: 2N2O5(g) 4NO2(g) + O2(g) 1. The rate law for decomposition of N2O5(g) in the reaction above A. is rate = k[n2o5] B. is rate = k[n2o5] 2 C. is rate = [NO2]
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 informationLecture 2. Review of Basic Concepts
Lecture 2 Review of Basic Concepts Thermochemistry Enthalpy H heat content H Changes with all physical and chemical changes H Standard enthalpy (25 C, 1 atm) (H=O for all elements in their standard forms
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 informationWorksheet 21 - Le Chatelier's Principle
Worksheet 21 - Le Chatelier's Principle Le Chatelier's Principle states that if a stress is applied to a system at equilibrium, the system will adjust, to partially offset the stress and will reach a new
More information(second-order kinetics)
CHEM*130 (F 01) REVIEW QUESTIONS FOR FINAL EXAM PAGE - 1 PART A QUESTION 1 Given: Reaction studied: NO 2 (g) NO(g) + O(g) Arrhenius equation: k 2.6 10 12 e! 8900 T L mol!1 s!1 (a) E a k A e! E a R T where
More informationKinetics. Chapter 14. Chemical Kinetics
Lecture Presentation Chapter 14 Yonsei University In kinetics we study the rate at which a chemical process occurs. Besides information about the speed at which reactions occur, kinetics also sheds light
More informationUseful Information is Located at the End of the Exam. 1. An Elementary Step in a reaction mechanism tells us:
CHEM 122 General Chemistry Summer 2014 Name: Midterm Examination 2 Useful Information is Located at the End of the Exam. Multiple Choice Questions 1. An Elementary Step in a reaction mechanism tells us:
More information6. Which expression correctly describes the equilibrium constant for the following reaction? 4NH 3 (g) + 5O 2 (g) 4NO(g) + 6H 2 O(g)
1. Which of the following can we predict from an equilibrium constant for a reaction? 1. The extent of a reaction 2. Whether the reaction is fast or slow 3. Whether a reaction is exothermic or endothermic
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 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 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 informationa. rate = k[no] 2 b. rate = k([no][o 2 ] c. rate = k[no 2 ] 2 [NO] -2 [O 2 ] -1/2 d. rate = k[no] 2 [O 2 ] 2 e. rate = k([no][o 2 ]) 2
General Chemistry III 1046 E Exam 1 1. Cyclobutane, C 4 H 8, decomposes as shown: C 4 H 8 (g)! 2 C 2 H 4 (g). In the course of a study of this reaction, the rate of consumption of C 4 H 8 at a certain
More informationLecture Presentation. Chapter 14. Chemical Kinetics. John D. Bookstaver St. Charles Community College Cottleville, MO Pearson Education, Inc.
Lecture Presentation Chapter 14 John D. Bookstaver St. Charles Community College Cottleville, MO In kinetics we study the rate at which a chemical process occurs. Besides information about the speed at
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 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 12. Kinetics. Factors That Affect Reaction Rates. Factors That Affect Reaction Rates. Chemical. Kinetics
PowerPoint to accompany Kinetics Chapter 12 Chemical Kinetics Studies the rate at which a chemical process occurs. Besides information about the speed at which reactions occur, kinetics also sheds light
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 informationChemical Kinetics. Rate = [B] t. Rate = [A] t. Chapter 12. Reaction Rates 01. Reaction Rates 02. Reaction Rates 03
Chapter Chemical Kinetics Reaction Rates 0 Reaction Rate: The change in the concentration of a reactant or a product with time (M/s). Reactant Products aa bb Rate = [A] t Rate = [B] t Reaction Rates 0
More informationCh 6 Practice Problems
Ch 6 Practice Problems 1. Which of the following statements is true? A) When two opposing processes are proceeding at identical rates, the sstem is at equilibrium. B) Catalsts are an effective means of
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 informationC H E M I C N E S C I
C H E M I C A L K I N E T S C I 4. Chemical Kinetics Introduction Average and instantaneous Rate of a reaction Express the rate of a reaction in terms of change in concentration Elementary and Complex
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 informationEXAM 3 REVIEW LBS 172 REACTION MECHANISMS
EXAM 3 REVIEW LBS 172 REACTION MECHANISMS GENERAL -Step by step process of bond making and breaking by which reactants become products -Summation of steps must be equal to overall reaction -Example: NO
More informationChemical Kinetics AP Chemistry Lecture Outline
Chemical Kinetics AP Chemistry Lecture Outline Name: Factors that govern rates of reactions. Generally... (1)...as the concentration of reactants increases, rate (2)...as temperature increases, rate (3)...with
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 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 informationWksht Rate Laws
Wksht 1.1 - Rate Laws Iowa State University Leader: Deborah Course: CHEM 178 Instructor: Bonaccorsi/Vela Date: 1/16/18 1. Describe the difference between average rate and instantaneous rate. Average rate-
More informationCH1810-Lecture #8 Chemical Equilibrium: LeChatlier s Principle and Calculations with K eq
CH1810-Lecture #8 Chemical Equilibrium: LeChatlier s Principle and Calculations with K eq LeChatlier s Principle A system at equilibrium responds to a stress in such a way that it relieves that stress.
More informationCHEM Chapter 14. Chemical Kinetics (Homework) Ky40
CHEM 1412. Chapter 14. Chemical Kinetics (Homework) Ky40 1. Chlorine dioxide reacts in basic water to form chlorite and chlorate according to the following chemical equation: 2ClO 2 (aq) + 2OH (aq) ClO
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 informationCHEM 102 Winter 10 Exam 2(a)
CHEM 102 Winter 10 Exam 2(a) On the answer sheet (scantron) write your Name, Student ID Number, and Recitation Section Number. Choose the best (most correct) answer for each question AND ENTER IT ON YOUR
More informationChapter 12. Chemical Kinetics
Chapter 12 Chemical Kinetics Chapter 12 Table of Contents 12.1 Reaction Rates 12.2 Rate Laws: An Introduction 12.3 Determining the Form of the Rate Law 12.4 The Integrated Rate Law 12.5 Reaction Mechanisms
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 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 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 informationExam 2 Sections Covered: (the remaining Ch14 sections will be on Exam 3) Useful Information Provided on Exam 2:
Chem 101B Study Questions Name: Chapters 12,13,14 Review Tuesday 2/28/2017 Due on Exam Thursday 3/2/2017 (Exam 2 Date) This is a homework assignment. Please show your work for full credit. If you do work
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 informationCalculating Rates of Substances. Rates of Substances. Ch. 12: Kinetics 12/14/2017. Creative Commons License
Ch. 2: Kinetics An agama lizard basks in the sun. As its body warms, the chemical reactions of its metabolism speed up. Chemistry: OpenStax Creative Commons License Images and tables in this file have
More information14.1 Factors That Affect Reaction Rates
14.1 Factors That Affect Reaction Rates 1) 2) 3) 4) 14.2 Reaction Rates How does increasing the partial pressures of the reactive components of a gaseous mixture affect the rate at which the compounds
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 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 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 informationBCIT Winter Chem Exam #1
BCIT Winter 2014 Chem 0012 Exam #1 Name: Attempt all questions in this exam. Read each question carefully and give a complete answer in the space provided. Part marks given for wrong answers with partially
More informationCh 13 Rates of Reaction (Chemical Kinetics)
Ch 13 Rates of Reaction (Chemical Kinetics) Reaction Rates and Kinetics - The reaction rate is how fast reactants are converted to products. - Chemical kinetics is the study of reaction rates. Kinetics
More informationChemical Kinetics -- Chapter 14
Chemical Kinetics -- Chapter 14 1. Factors that Affect Reaction Rate (a) Nature of the reactants: molecular structure, bond polarity, physical state, etc. heterogeneous reaction: homogeneous reaction:
More informationEquilibrium and Reaction Rate
Equilibrium and Reaction Rate Multiple Choice Questions - Answers 1. Activation energy could be considered as the minimum energy required to do which of these? A. change the orientation of the reactant
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 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 informationAP Chapter 13: Kinetics Name
AP Chapter 13: Kinetics Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. AP Chapter 13: Kinetics 2 Warm-Ups (Show your work for credit) Date 1.
More informationName Chem 6 Section #
Equilibrium Constant and its Meaning 1. Write the expressions for K eq for the following reactions. a) CH 4 (g) + 2 H 2 S(g) CS 2 (g) + 4 H 2 (g) b) 2 N 2 O 5 (g) 4 NO 2 (g) + O 2 (g) c) 3 O 2 (g) 2 O
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
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 informationB. The rate will increase by a factor of twelve. C. The rate will increase by a factor of twenty-four. D. The rate will decrease by a factor of six.
1. If O 2 (g) disappears at a rate of 0.250 M/s at a particular moment in the reaction below, what is the rate of appearance of H 2 O(g) at the same time? C 3 H 8 (g) + 5 O 2 (g) 3 CO 2 (g) + 4 H 2 O(g)
More informationChapter 14, Chemical Kinetics
Last wee we covered the following material: Review Vapor Pressure with two volatile components Chapter 14, Chemical Kinetics (continued) Quizzes next wee will be on Chap 14 through section 14.5. 13.6 Colloids
More informationb. Free energy changes provide a good indication of which reactions are favorable and fast, as well as those that are unfavorable and slow.
Chem 130 Name Exam 3, Ch 7, 19, 14 November 9, 2018 100 Points Please follow the instructions for each section of the exam. Show your work on all mathematical problems. Provide answers with the correct
More informationChapter 14: Chemical Kinetics
Chapter 14: Chemical Kinetics NOTE THIS CHAPTER IS #2 TOP TOPICS ON AP EXAM!!! NOT ONLY DO YOU NEED TO FOCUS ON THEORY (and lots of MATH) BUT YOU MUST READ THE FIGURES TOO!!! Ch 14.1 ~ Factors that Affect
More informationKinetics. 1. Consider the following reaction: 3 A 2 B How is the average rate of appearance of B related to the average rate of disappearance of A?
Kinetics 1. Consider the following reaction: 3 A 2 B How is the average rate of appearance of B related to the average rate of disappearance of A? A. [A]/ t = [B]/ t B. [A]/ t = (2/3)( [B]/ t) C. [A]/
More informationwhich has an equilibrium constant of Which of the following diagrams represents a mixture of the reaction at equilibrium?
Chapter 9 Quiz: Chemical Equilibria 1. Which of the following statements is true regarding chemical equilibrium? I. The concentrations of reactants and products at equilibrium are constant, which means
More informationLeader: Deborah Course: CHEM 178 Instructor: Bonaccorsi/Vela Date: 2/6/18 + H 2 CHF 3. a. Express the rate law in terms of m, n, and k.
EXAM I REVIEW KEY Leader: Deborah Course: CHEM 178 Instructor: Bonaccorsi/Vela Date: 2/6/18 1. Given the following reaction: CF 4 + H 2 CHF 3 + HF a. Express the rate law in terms of m, n, and k. Rate
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 informationChapter 14. Chemical Kinetics
Chapter 14. Chemical Kinetics Common Student Misconceptions It is possible for mathematics to get in the way of some students understanding of the chemistry of this chapter. Students often assume that
More informationChapter 13 Lecture Lecture Presentation. Chapter 13. Chemical Kinetics. Sherril Soman Grand Valley State University Pearson Education, Inc.
Chapter 13 Lecture Lecture Presentation Chapter 13 Chemical Kinetics Sherril Soman Grand Valley State University Ectotherms Lizards, and other cold-blooded creatures, are ectotherms animals whose body
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. Kinetics is the study of how fast chemical reactions occur. There are 4 important factors which affect rates of reactions:
Chemical Kinetics Kinetics is the study of how fast chemical reactions occur. There are 4 important factors which affect rates of reactions: reactant concentration temperature action of catalysts surface
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 informationName AP CHEM / / Chapter 12 Outline Chemical Kinetics
Name AP CHEM / / Chapter 12 Outline Chemical Kinetics The area of chemistry that deals with the rate at which reactions occur is called chemical kinetics. One of the goals of chemical kinetics is to understand
More information