EEC 503 Spring 2009 REVIEW 1
|
|
|
- Francis Brooks
- 5 years ago
- Views:
Transcription
1 EEC 503 Spring 2009 REVIEW 1 1. Why are chemical reactions important to energy, environmental and process engineering? Name as many reasons as you can think of. 2. What is a chemical reaction? 3. What do we mean by reaction stoichiometry? What does stoichiometry represent? 4. What is a mole? What is the relationship between a kmol and mol? What is the relationship between a lbmol and a mol? 5. Progress of single reaction can be represented by a single molar extent of reaction. What is the relationship between the initial moles of reactants and products, the moles for each of the above after some reaction time, the stoichiometric coefficients and reaction extent? 6. Relate molar extent of reaction to the fractional conversion of the limiting reactant. What is the limiting reactant? 7. What is the relationship between mole fraction of various products and reactants and reaction extent? 1
2 8. Extend the relationship developed in answering question 5. to multiple reactions consisting of R independent reactions between S species? 9. What is the stoichiometric coefficient of an inert? 10. In a set of R stoichiometric reactions between S species how would you determine the set R of independent reactions? 11. What is the rate of reaction? 12. What does rate of reaction depend on? 13. What is activation energy for the reaction? Can it be defined always? 14. Which reaction rate increases more rapidly with temperature, the one with lower or higher activation energy? 15. What is the Arrhenius form of the rate constant? 16. How can an n-th order reaction rate be represented. 2
3 17. Can the temperature and composition dependence term be separated in reaction rates that follow the Langmuir-Hinshelwood (Hougen-Watson) form? Can an activation energy be defined for the rate from of that type? 18. What is molar internal energy? What is it a function of? 19. How is molar enthalpy defined? What about partial molar enthalpy? What information is needed to calculate it at a given temperature and composition? 20. What is the standard heat of reaction? 21. What is molar Gibbs free energy in terms of molar enthalpy and entropy? 22. What is the thermodynamic condition for equilibrium in a reactive system? 23. How is the thermodynamic equilibrium constant defined? 24. How is the standard Gibbs free energy for reaction calculated and how does it relate to the equilibrium constant? 25. What is Van t Hoff s equation for variation of equilibrium constant with temperature? 3
4 26. How can one calculate the heat of reaction as a function of temperature? 27. Does the equilibrium constant have units? 28. How does one relate activity to mole fraction? Activity to concentration? 29. Calculate the equilibrium conversion of SO 2 reacting with air at 25 C and at 600 C and P= 1 atm for a feed that contains 1) stoichiometric ratio of reactants 2) large excess of air 3) what would happen to the equilibrium conversion if your raised the pressure of operation to 100 atm. Would it be affected more for case 1 or case 2? Assume constant heat or reaction. 30. What is the kinetic definition of equilibrium? What constraint does that impose on the reaction forms for the reverse and forward reactions? 31. If Arrhenius form is used to represent the rate constant k c ((mol/l) 1-n s -1 ) and the rate constant for the same gas phase reaction k p (mol/l) atm -n s -1 ), what is the relationship between k co and k po and E P and E c? 32. What are the basic postulates of the transition state theory (TST)? 33. What is the universal frequency of TST equal to? 34. How does the expression for the rate constant derived by TST account for system non-ideality? 4
5 35. Using TST and Debye-Huckel theory what relation results for the dependence of the rate constant on ionic strength of the solution. 36. What is an elementary reaction? What can one say about stoichiometric coefficients for an elementary reaction? 37. What is the law of mass action? When does it apply? 38. In gas phase reactions bimolecular reactions can occur between what type of species? The rate of bimolecular reactions is of what order? 39. What gas phase trimolecular reactions do you know? What is the overall reaction order? 40. Are gas phase unimolecular reactions always first order? 41. What is the Lindemann Christansen mechanism for unimolecular reactions? 42. How do we obtain the rate forms for free radical recombination reactions? 43. What are the key differences between gas phase reactions and reactions in solution. 44. What relationship between reaction rate constant and solvent properties does TST predict? 45. What is diffusion? 46. If elementary reactions in solution involve ions or other charged species how does TST account for the effect of the electric field? 47. What dependence of the rate constant on solvent and ion properties is obtained by TST via the dual sphere and single sphere model? 5
6 48. What is Ficks First Law of diffusion? 49. What is Ficks Second Law of diffusion? 50. What is the RMS displacement equal to according to the diffusion equation? 51. What is the meaning of a diffusion limited reaction in the liquid state? What is the value of the rate constant? 52. What is the expression for the apparent rate constant for a bimolecular liquid phase reaction that is controlled both by kinetics (i.e transition state complex transformation) and diffusion. 53. What is a reaction mechanism? 54. What is the difference between an open and closed reaction mechanism sequence? 55. What is the relationship between the stoichiometry of individual mechanistic steps and the overall stoichiometry for mechanisms containing a closed sequence? 56. What are the steps for deriving an overall rate expression in terms of the concentrations of stable species only when applying PSSA to a postulated mechanism? 57. What are the key features in deriving a rate form based on RLSA application to a postulated mechanism? 58. What is characteristic reaction time? Reaction half life? 59. How is quantum yield defined? 6
7 60. What is the maximum ozone concentration proportional to if one considers only NO, NO 2, and O 3? 61. What are the NO x and CO roles in ozone formation? 62. Where does sulfur conversion occur in the atmosphere, in the gas phase or liquid phase? 63. What are the key reactions in oxidation of S(IV) to S(VI)? 64. What are the key five characteristic times for reaction of a gas phase reactant in a liquid droplet? 65. Which of the characteristic times are most likely to be rate controlling for a: a) highly soluble gas, b) slightly soluble gas. 66. Write the basic conservation law for a chemical species j in a single phase well mixed system that is: a) closed, b) open. Identify all the terms. 67. Write the basic conservation law for a chemical species j in a two phase well mixed system that is : a) closed, b) open. Identify all the terms. Do not assume that the system is equilibrated. 68. Modify the equations developed in answering question 67 to the form appropriate when all species are equilibrated between the two phases. 69. Explain the meaning of the modified Henry s constant for a soluble gas that upon dissolution dissociates. Use ammonia as a n example. 70. Illustrate the use of equations developed to treat sulfur dioxide oxidation in ar that contains L volume fraction of water in droplets form. Assuming that the only species originally present in the gas phase are nitrogen, oxygen, carbon dioxide, sulfur dioxide, ozone show which equations would need to be solved to monitor the evolution of ph, S(VI) concentration in the liquid phase. Use information provided in the notes. Do not forget to specify the electroneutrality equation. Assume a closed system. 7
8 8
1. Why are chemical reactions important to energy, environmental and process engineering? Name as many reasons as you can think of.
EEC 503 Spring 2013 REVIEW 1: BASIC KINETIC CONCEPTS 1. Why are chemical reactions important to energy, environmental and process engineering? Name as many reasons as you can think of. 2. What is a chemical
CHAPTER 4 Chemical Kinetics: Rate and Mechanistic Models. 4.1 Introduction
CHAPE 4 Chemical Kinetics: ate and Mechanistic Models 4. Introduction By listing the plausible reaction stoichiometries, we can calculate the composition of the system in its final state, i.e. at equilibrium,
CHEMICAL KINETICS. LECTURE Introduction
LECTURE-2. 2. Introduction CHEMICAL KINETICS 09//03 We have shown in the previous chapter that upon listing of the plausible reaction stoichiometries we can calculate the composition of the system in its
Reactors. Reaction Classifications
Reactors Reactions are usually the heart of the chemical processes in which relatively cheap raw materials are converted to more economically favorable products. In other cases, reactions play essential
Reaction rate. reaction rate describes change in concentration of reactants and products with time -> r = dc j
Reaction rate ChE 400 - Reactive Process Engineering reaction rate describes change in concentration of reactants and products with time -> r = dc j /dt r is proportional to the reactant concentrations
Fundamentals of Combustion
Fundamentals of Combustion Lec 3: Chemical Thermodynamics Dr. Zayed Al-Hamamre Content Process Heat Transfer 1-3 Process Heat Transfer 1-4 Process Heat Transfer 1-5 Theoretical and Excess Air Combustion
Review of differential and integral calculus and introduction to multivariate differential calculus.
Chemistry 2301 Introduction: Review of terminology used in thermodynamics Review of differential and integral calculus and introduction to multivariate differential calculus. The properties of real gases:
Reavis High School AP Chemistry Curriculum Snapshot
Reavis High School AP Chemistry Curriculum Snapshot Unit 1: Science Fundamentals 5 Students will learn the saftey rules and laboratory equipment of the science laboratory and demonstrate their competence
OCR Chemistry A H432
All the energy changes we have considered so far have been in terms of enthalpy, and we have been able to predict whether a reaction is likely to occur on the basis of the enthalpy change associated with
AP Chemistry - Notes - Chapter 12 - Kinetics Page 1 of 7 Chapter 12 outline : Chemical kinetics
AP Chemistry - Notes - Chapter 12 - Kinetics Page 1 of 7 Chapter 12 outline : Chemical kinetics A. Chemical Kinetics - chemistry of reaction rates 1. Reaction Rates a. Reaction rate- the change in concentration
(g) + 2H 2. (g) CH [1] (g) H 2. Explain, with a calculation, whether this reaction is feasible at 25 C [3]
![(g) + 2H 2. (g) CH [1] (g) H 2. Explain, with a calculation, whether this reaction is feasible at 25 C [3]](/thumbs/94/119401233.jpg "(g) + 2H 2. (g) CH [1] (g) H 2. Explain, with a calculation, whether this reaction is feasible at 25 C [3]")
1 This question looks at two reactions involving sulfur compounds (a) Hydrogen reacts with carbon disulfide as shown below 4H 2 + CS 2 CH 4 + 2H 2 S For this reaction, ΔH = 234 kj mol 1 and ΔS = 164 J
A First Course on Kinetics and Reaction Engineering Example 1.2
Example 1.2 Problem Purpose This example shows how to determine when it is permissible to choose a basis for your calculations. It also illustrates how to use reaction progress variables and the initial
Chemical Equilibrium
Chemical Equilibrium Chemical Equilibrium The Concept of Equilibrium (15.1) Ways of Expressing Equilibrium Constants (15.2) What Does the Equilibrium Constant Tell Us? (15.3) Factors that Affect Chemical
Quantity Relationships in Chemical Reactions
Chapter 10 Relationships in Chemical Reactions Section 10.1 Conversion Factors from a Chemical Equation Goal 1 The coefficients in a chemical equation give us the conversion factors to get from the number
Module 5: Combustion Technology. Lecture 32: Fundamentals of thermochemistry
1 P age Module 5: Combustion Technology Lecture 32: Fundamentals of thermochemistry 2 P age Keywords : Heat of formation, enthalpy change, stoichiometric coefficients, exothermic reaction. Thermochemistry
Chemistry 2000 Lecture 11: Chemical equilibrium
Chemistry 2000 Lecture 11: Chemical equilibrium Marc R. Roussel February 4, 2019 Marc R. Roussel Chemical equilibrium February 4, 2019 1 / 27 Equilibrium and free energy Thermodynamic criterion for equilibrium
c) Explain the observations in terms of the DYNAMIC NATURE of the equilibrium system.
Chemical Equilibrium - Part A: 1. At 25 o C and 101.3 kpa one mole of hydrogen gas and one mol of chlorine gas are reacted in a stoppered reaction vessel. After a certain time, three gases are detected
2.0 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
General Chemistry I Concepts
Thermodynamics Thermodynamics The Three Laws of Thermodynamics (18.1) Spontaneous Processes (18.2) Entropy (18.3) The Second Law of Thermodynamics (18.4) Gibbs Free Energy (18.5) Free Energy and Chemical
Chemistry 192 Problem Set 7 Spring, 2018
Chemistry 192 Problem Set 7 Spring, 2018 1. Use Table D2 to calculate the standard enthalpy change for the combustion of liquid benzene (C 6 H 6 ) in pure oxygen gas to produce gas phase carbon dioxide
Chapter 2: Equilibrium Thermodynamics and Kinetics
Chapter 2: Equilibrium Thermodynamics and Kinetics Equilibrium Thermodynamics: predicts the concentrations (or more precisely, activities) of various species and phases if a reaction reaches equilibrium.
Chemical Reactions. Writing chemical reactions Types of chemical reactions Reactions in aqueous solutions. (ionic equations and solubility rules)
Chemical Reactions Writing chemical reactions Types of chemical reactions Reactions in aqueous solutions (ionic equations and solubility rules) Writing Equations REACTANTS PRODUCTS gold (III) sulfide is
A.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
Multiple Choice Identify the letter of the choice that best completes the statement or answers the question.
CP Chem Review 2 Matching Match each item with the correct statement below. a. activated complex d. activation energy b. reaction rate e. free energy c. inhibitor 1. the minimum energy colliding particles
Express the transition state equilibrium constant in terms of the partition functions of the transition state and the
Module 7 : Theories of Reaction Rates Lecture 33 : Transition State Theory Objectives After studying this Lecture you will be able to do the following. Distinguish between collision theory and transition
The 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
Chapter 7 Chemical Reactions: Energy, Rates, and Equilibrium
Chapter 7 Chemical Reactions: Energy, Rates, and Equilibrium Introduction This chapter considers three factors: a) Thermodynamics (Energies of Reactions) a reaction will occur b) Kinetics (Rates of Reactions)
Steward Fall 08. Moles of atoms/ions in a substance. Number of atoms/ions in a substance. MgCl 2(aq) + 2 AgNO 3(aq) 2 AgCl (s) + Mg(NO 3 ) 2(aq)
Dealing with chemical stoichiometry Steward Fall 08 of Not including volumetric stoichiometry of Chapter 6.0x10 A 6.0x10 Mol/mol ratio from balanced equation B 6.0x10 6.0x10 s, Equations, and Moles: II
Accelerated Chemistry Semester 2 Review Sheet
Accelerated Chemistry Semester 2 Review Sheet The semester test will be given in two parts. The first part is a performance assessment and will be given the day before the semester test. This will include
Exam 3 Concepts! CH110 FA10 SAS 33
Exam 3 Concepts! CH110 FA10 SAS 33 Properties of Gases What sorts of elements and compounds tend to be found as gasses at room temperature? What are the physical properties of gases? What is pressure?
Chapter 5. Chemistry for Changing Times, Chemical Accounting. Lecture Outlines. John Singer, Jackson Community College. Thirteenth Edition
Chemistry for Changing Times, Thirteenth Edition Lecture Outlines Chemical Accounting John Singer, Jackson Community College Chemical Sentences: Equations Chemical equations represent the sentences in
let: rate constant at sea level be ks and that on mountain be km ks/km = 100 ( 3mins as opposed to 300 mins)
homework solution : "egg question" let: rate constant at sea level be ks and that on mountain be km ks/km = 100 ( 3mins as opposed to 300 mins) ln ks/km = Ea x 10 / 373 x 363 x 8.314 x 10-3 4.605 = 10Ea/1125.7
VAPOR PRESSURE LOWERING - Described by RAOULT'S LAW
73 VAPOR PRESSURE LOWERING - Described by RAOULT'S LAW partial pressure of the VAPOR of solvent molecules. mole fraction of component A vapor pressure of pure component A (depends on temperature) partial
CHEM 235 Physical Chemistry II NJIT Spring Semester, 2016
CHEM 235 Physical Chemistry II NJIT Spring Semester, 2016 Prerequisites: Textbook: Chem 231 or equivalent, Math 211 or 213, Phys 111 P. W. Atkins and J. de Paula Physical Chemistry 10th Edition, Freeman
CSTR 1 CSTR 2 X A =?
hemical Engineering HE 33 F Applied Reaction Kinetics Fall 014 Problem Set 3 Due at the dropbox located in the hallway outside of WB 5 by Monday, Nov 3 rd, 014 at 5 pm Problem 1. onsider the following
Stoichiometry: Chemical Calculations. Chemistry is concerned with the properties and the interchange of matter by reaction i.e. structure and change.
Chemistry is concerned with the properties and the interchange of matter by reaction i.e. structure and change. In order to do this, we need to be able to talk about numbers of atoms. The key concept is
Chapter 13. This ratio is the concentration of the solution.
Concentration Calculation Concentration In a solution, the solute is distributed evenly throughout the solvent. This means that any part of a solution has the same ratio of solute to solvent as any other
KINETICS CHEMICAL CHEMIC. Unit. I. Multiple Choice Questions (Type-I)
Unit 4 CHEMICAL CHEMIC KINETICS I. Multiple Choice Questions (Type-I) 1. The role of a catalyst is to change. gibbs energy of reaction. enthalpy of reaction. activation energy of reaction. equilibrium
15.1 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
Name: Score: /100. Part I. Multiple choice. Write the letter of the correct answer for each problem. 3 points each
Name: Score: /100 Part I. Multiple choice. Write the letter of the correct answer for each problem. 3 points each 1. Which of the following contains the greatest number of moles of O? A) 2.3 mol H 2 O
REACTION RATES AND EQUILIBRIUM
Name Date Class 18 REACTION RATES AND EQUILIBRIUM SECTION 18.1 RATES OF REACTION (pages 541 547) This section explains what is meant by the rate of a chemical reaction. It also uses collision theory to
Since the coefficients are only determined up to a multiplicative constant, set c 1 1 and solve for the coefficients: c 1 1 c c 3 1
In[1]:= dipole moment of S4 Input interpretation: sulfur tetrafluoride dipole moment Result:.632 D (debyes) Unit conversions: 2.18 1-18 pc m (picocoulomb meters) 2.18 1-21 nc m (nanocoulomb meters) 2.18
**continued on next page**
Chapter 9 Stoichiometry Section 9.1 Introduction to Stoichiometry Standard.e.: Students know how to calculate the masses of reactant and products in a chemical reaction from the mass of one of the reactants
CH 221 Chapter Four Part II Concept Guide
CH 221 Chapter Four Part II Concept Guide 1. Solubility Why are some compounds soluble and others insoluble? In solid potassium permanganate, KMnO 4, the potassium ions, which have a charge of +1, are
Brown 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
Department of Mechanical Engineering BM 7103 FUELS AND COMBUSTION QUESTION BANK UNIT-1-FUELS
Department of Mechanical Engineering BM 7103 FUELS AND COMBUSTION QUESTION BANK UNIT-1-FUELS 1. Define the term fuels. 2. What are fossil fuels? Give examples. 3. Define primary fuels. Give examples. 4.
Gases and Kinetic Molecular Theory
1 Gases and Kinetic Molecular Theory 1 CHAPTER GOALS 1. Comparison of Solids, Liquids, and Gases. Composition of the Atmosphere and Some Common Properties of Gases 3. Pressure 4. Boyle s Law: The Volume-Pressure
EECE 507 Take Home Exam 1
Spring 27 EECE 57 Take ome Exam This homework tests your ability to integrate the concepts learned so far in quantitatively addressing an important problem in atmospheric chemistry -that of acid rain.
CHEMICAL 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,
Chapter 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
Be able to Define/Understand:
NAME: CLASS PERIOD: REVIEW FOR HONORS CHEMISTRY SEMESTER 2 EXAM: PART 1 Be able to Define/Understand: Know how to: Chapter 8 Chapter 9 Chapter 10 Law of conservation of mass Characteristics of a chemical/physical
Section 3 Environmental Chemistry
Section 3 Environmental Chemistry 1 Environmental Chemistry Definitions Chemical Reactions Stoichiometry Photolytic Reactions Enthalpy and Heat of Reaction Chemical Equilibria ph Solubility Carbonate Systems
Dr. 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
Enthalpy Chapter 5.3-4,7
Enthalpy Chapter 5.3-4,7 heat transfer in (endothermic), +q heat transfer out (exothermic), -q SYSTEM E = q + w w transfer in (+w) w transfer out (-w) Internal Energy at Constant Volume E = E K + E P ΔE
Chemistry: The Central Science Twelfth Edition, AP* Edition 2012
A Correlation of The Central Science Twelfth Edition, AP* Edition 2012 to the AP* Chemistry Topics I. Structure of Matter A. Atomic theory and atomic structure 1. Evidence for the atomic theory SECTIONS:
CFC: chlorofluorocarbons
The rate of reaction is markedly affected by temperature. Chemical Kinetics & k versus T Two theories were developed to explain the temperature effects. 1. 2. 2 UV radiation strikes a CFC molecule causing
Liquids and Solutions Crib Sheet
Liquids and Solutions Crib Sheet Determining the melting point of a substance from its solubility Consider a saturated solution of B in a solvent, A. Since the solution is saturated, pure solid B is in
Reaction Dynamics (2) Can we predict the rate of reactions?
Reaction Dynamics (2) Can we predict the rate of reactions? Reactions in Liquid Solutions Solvent is NOT a reactant Reactive encounters in solution A reaction occurs if 1. The reactant molecules (A, B)
L = 6.02 x mol Determine the number of particles and the amount of substance (in moles)
1.1 The Mole 1.1.1 - Apply the mole concept to substances A mole is the name given to a certain quantity. It represents 6.02 x 10 23 particles. This number is also known as Avogadro's constant, symbolised
Objective: To Evaluate Predictions of Alternative Models
www.optience.com Methanol Synthesis Objective: To Evaluate Predictions of Alternative Models In this example, we propose and evaluate Mass Action and Langmuir Hinshelwood (LHHW) models for methanol synthesis
Solutions and Their Properties
Chapter 11 Solutions and Their Properties Solutions: Definitions A solution is a homogeneous mixture. A solution is composed of a solute dissolved in a solvent. When two compounds make a solution, the
Name: Score: /100. Part I. Multiple choice. Write the letter of the correct answer for each problem. 3 points each
Name: Score: /100 Part I. Multiple choice. Write the letter of the correct answer for each problem. 3 points each 1. Which of the following contains the greatest number of moles of O? A) 2.3 mol H 2 O
AP 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
Learning Outcomes: At the end of this assignment, students will be able to:
Chemical Equilibria & Sample Preparation Purpose: The purpose of this assignment is to predict how solute concentrations are controlled by chemical equilibria, understand the chemistry involved with sample
- Applications: In chemistry, this effect is often used to determine the molecular weight of an unknown molecule.
73 FREEZING POINT DEPRESSION concentration of solute (molality) Freezing point depression constant (for SOLVENT) Freezing point depression: The amount the freezing temperature is LOWERED by the solute.
Final S2 (2011) - Practice Test - Ch 11, 12, 13, 14, 15, 16, 18, 19, 22, 23
Final S2 (2011) - Practice Test - Ch 11, 12, 13, 14, 15, 16, 18, 19, 22, 23 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. If 12.0 g of a gas at 2.5 atm
Thermodynamics IV - Free Energy and Chemical Equilibria Chemical Potential (Partial Molar Gibbs Free Energy)
Thermodynamics IV - Free Energy and Chemical Equilibria Chemical Potential (Partial Molar Gibbs Free Energy) increase in the Gibbs free energy of the system when 1 mole of i is added to a large amount
AP 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
2SO 2(g) + O 2(g) Increasing the temperature. (Total 1 mark) Enthalpy data for the reacting species are given in the table below.
Q1.Which change would alter the value of the equilibrium constant (K p) for this reaction? 2SO 2(g) + O 2(g) 2SO 3(g) A Increasing the total pressure of the system. Increasing the concentration of sulfur
CH302 Spring 2009 Practice Exam 1 (a fairly easy exam to test basic concepts)
CH302 Spring 2009 Practice Exam 1 (a fairly easy exam to test basic concepts) 1) Complete the following statement: We can expect vapor pressure when the molecules of a liquid are held together by intermolecular
Chemical Equilibrium
Chemical Equilibrium Chemical Equilibrium When compounds react, they eventually form a mixture of products and unreacted reactants, in a dynamic equilibrium. A dynamic equilibrium consists of a forward
AP* Thermodynamics Free Response Questions page 1. Essay Questions
AP* Thermodynamics Free Response Questions page 1 Essay Questions 1991 The reaction represented above is a reversible reaction. BCl 3 (g) + NH 3 (g) Cl 3 BNH 3 (s) (a) Predict the sign of the entropy change,
17.2 Thermochemical Equations
17.2. Thermochemical Equations www.ck12.org 17.2 Thermochemical Equations Lesson Objectives Define enthalpy, and know the conditions under which the enthalpy change in a reaction is equal to the heat absorbed
Gas Laws. Bonding. Solutions M= moles solute Mass %= mass solute x 100. Acids and Bases. Thermochemistry q = mc T
Name Period Teacher Practice Test: OTHS Academic Chemistry Spring Semester 2017 The exam will have 100 multiple choice questions (1 point each) Formula sheet (see below) and Periodic table will be provided
Chemical equilibrium. Answers to worked examples
15 Chemical equilibrium Answers to worked examples WE 15.1 Writing expressions for thermodynamic equilibrium constants (on p. 700 in Chemistry 3 ) Write expressions for the thermodynamic equilibrium constants
Chemistry 2 nd Semester Final Exam Review
Chemistry 2 nd Semester Final Exam Review Chemical Bonds 1. Give a physical description of how the atoms and molecules are arranged in solids, liquids, and gases. A: In a liquid, the forces between the
Thermodynamics and Equilibrium. Chemical thermodynamics is concerned with energy relationships in chemical reactions.
1 of 7 Thermodynamics and Equilibrium Chemical thermodynamics is concerned with energy relationships in chemical reactions. In addition to enthalpy (H), we must consider the change in randomness or disorder
Chemistry 1A, Spring 2007 Midterm Exam 3 April 9, 2007 (90 min, closed book)
Chemistry 1A, Spring 2007 Midterm Exam 3 April 9, 2007 (90 min, closed book) Name: KEY SID: TA Name: 1.) Write your name on every page of this exam. 2.) This exam has 34 multiple choice questions. Fill
Name:. Correct Questions = Wrong Questions =.. Unattempt Questions = Marks =
Name:. Correct Questions = Wrong Questions =.. Unattempt Questions = Marks = 1. (12%) Compound X contains 2.239% hydrogen, 26.681% carbon and 71.080 % oxygen by mass. The titration of 0.154 g of this compound
Basic Concepts of Chemistry Notes for Students [Chapter 12, page 1] D J Weinkauff - Nerinx Hall High School. Chapter 12 Properties of Solutions
![Basic Concepts of Chemistry Notes for Students [Chapter 12, page 1] D J Weinkauff - Nerinx Hall High School. Chapter 12 Properties of Solutions](/thumbs/96/127488495.jpg "Basic Concepts of Chemistry Notes for Students [Chapter 12, page 1] D J Weinkauff - Nerinx Hall High School. Chapter 12 Properties of Solutions")
Basic Concepts of Chemistry Notes for Students [Chapter 12, page 1] Chapter 12 Properties of Solutions Section 12 1: The Nature of Aqueous Solutions 1) Sec 12 1.1 Mixtures of Two Liquids When two liquids
Chapter 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
How would we know if equilibrium has been reached? Or if it will be reach?
1 How would we know if equilibrium has been reached? Or if it will be reach? The reaction quotient, Q, or trial KC, enables us to determine this information. The reaction quotient is determined by using
c. K 2 CO 3 d. (NH 4 ) 2 SO 4 Answer c
Chem 130 Name Exam 2, Ch 4-6 July 7, 2016 100 Points Please follow the instructions for each section of the exam. Show your work on all mathematical problems. Provide answers with the correct units and
SSLC CHEMISTRY UNIT 2 MOLE CONCEPT - WORK SHEETS WORK SHEET 1
1 SSLC CHEMISTRY UNIT 2 MOLE CONCEPT - WORK SHEETS WORK SHEET 1 1 GAM atoms Mass in grams equal to its Atomic mass Element and GAM Number of Atoms Mass in grams 1 GAM Hydrogen atoms 1 g 1 GAM Helium atoms
Thermodynamics is the study of the relationship between heat and other forms of energy that are involved in a chemical reaction.
Ch 18 Thermodynamics and Equilibrium Thermodynamics is the study of the relationship between heat and other forms of energy that are involved in a chemical reaction. Internal Energy (U) Internal energy
FIRST PUBLIC EXAMINATION. Trinity Term Preliminary Examination in Chemistry SUBJECT 3: PHYSICAL CHEMISTRY. Time allowed: 2 ½ hours
FIRST PUBLIC EXAMINATION Trinity Term 004 Preliminary Examination in Chemistry SUBJECT 3: PHYSICAL CHEMISTRY Wednesday, June 9 th 004, 9.30 a.m. to 1 noon Time allowed: ½ hours Candidates should answer
aa + 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
Chemistry 431 Problem Set 8 Fall 2018 Solutions
Chemistry 43 Problem Set 8 Fall 208 Solutions. Use able 4. of the text to calculate the equilibrium constant of the reaction NO g + 2 O 2g NO 2g at 25. C and 35. C. r,m G f,m G NO 2g f,m G NO g At 25 C
Enthalpy, Entropy, and Free Energy Calculations
Adapted from PLTL The energies of our system will decay, the glory of the sun will be dimmed, and the earth, tideless and inert, will no longer tolerate the race which has for a moment disturbed its solitude.
TABLE OF CONTENT. Chapter 4 Multiple Reaction Systems 61 Parallel Reactions 61 Quantitative Treatment of Product Distribution 63 Series Reactions 65
TABLE OF CONTENT Chapter 1 Introduction 1 Chemical Reaction 2 Classification of Chemical Reaction 2 Chemical Equation 4 Rate of Chemical Reaction 5 Kinetic Models For Non Elementary Reaction 6 Molecularity
2 Reaction kinetics in gases
2 Reaction kinetics in gases October 8, 2014 In a reaction between two species, for example a fuel and an oxidizer, bonds are broken up and new are established in the collision between the species. In
Thermodynamics of Reactive Systems The Equilibrium Constant
Lecture 27 Thermodynamics of Reactive Systems The Equilibrium Constant A. K. M. B. Rashid rofessor, Department of MME BUET, Dhaka Today s Topics The Equilibrium Constant Free Energy and Equilibrium Constant
Chemical 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
Ch 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
CHEM 116 Colligative Properties and Intro to Rates of Reaction
CHEM 116 Colligative Properties and Intro to Rates of Reaction Note: Some of the slides here were in Lecture 10 but we didn t get to them, so we will begin with those. They are repeated here, but if you
CHEM Chemical Kinetics. & Transition State Theory
Chemical Kinetics Collision Theory Collision Theory & Transition State Theory The rate of reaction is markedly affected by temperature. k versus T Ae E a k RT Two theories were developed to explain the
Equilibrium Unit. Terminology. Terminology 11/04/2018. Chemistry 30 Ms. Hayduk
Equilibrium Unit Chemistry 30 Ms. Hayduk Terminology System: the part of the universe being studied can be tiny (one atom) or big (the Earth) Surroundings: the part of the universe outside of the system
Chapter 11 Properties of Solutions
Chapter 11 Properties of Solutions Solutions Homogeneous mixtures of two or more substances Composition is uniform throughout the sample No chemical reaction between the components of the mixture Solvents
1 A. That the reaction is endothermic when proceeding in the left to right direction as written.
1 Q. If Δ r H is positive, what can you say about the reaction? 1 A. That the reaction is endothermic when proceeding in the left to right direction as written. 2 Q If Δ r H is negative, what can you say
Foundations of Chemical Kinetics. Lecture 12: Transition-state theory: The thermodynamic formalism
Foundations of Chemical Kinetics Lecture 12: Transition-state theory: The thermodynamic formalism Marc R. Roussel Department of Chemistry and Biochemistry Breaking it down We can break down an elementary