Section A-Gases 1A. Circle the correct answer (18 pts total) (2 points each)
|
|
- Suzanna Henry
- 5 years ago
- Views:
Transcription
1 Section A-Gases 1A. Circle the correct answer (18 pts total) (2 points each) (b) If a sample of gas is warmed in a rigid container (i.e., with fixed volume), which is true? i) the density of the gas remains the same ii) the pressure of the gas increases iii) the average distance between the gas particles remains the same iv) all of the above 2A. Write T (True) or F (False) for the following statements. If the statement is false correct it by changing, dropping, or adding a few words (6 points) c) For a fixed number of moles of an ideal gas at a constant temperature, when the pressure increases the volume will decrease and the molecular speed will increase. stay the same d) Gases are easier to compress than liquids because there is much more space between particles in a gas than in a liquid. T Free Response Questions--A 7A. (8 pts) A box of fixed volume contains two gases inside, A and B, at 35 C. Assuming the data in the plots are corrrect, state whether each statement below is true (T) or false (F). You do NOT need to correct it if it is false here!! _ F_(a) The particles of A have a greater average speed than those of B. _ T_(b) The partial pressure of A is greater than the partial pressure of B. _ T_(c) The molar mass of A is greater than the molar mass of B. _ F_(d) The particles of A have a greater average kinetic energy than the particles of B. speed 10A. (11 pts) (a) (7 pts) One industrial process for the removal of hydrogen sulfide from natural gas is its reaction with sulfur dioxide: 2 H 2 S(g) + SO 2 (g) 3 S(s) + 2 H 2 O(g) What volume of SO 2 at 5.0 atm and 252C will be used up in the production of 21 mol of S(s)? 1 mol SO 2 used 21 mol S 7.0 mol SO 2(g) used up. Assuming ideal gas behavior, 3 mol S produced this many moles of gas at 5.0 atm and 252 C will occupy a volume given by the ideal gas equation: # p a r t i c l e s A B T = 35C
2 V 7.0 mol L atm mol K ( ) K nrt L = 6.0 x 10 L P 5.0 atm (b) (4 pts) (not related to part (a) at all) A sample of a gas has a volume of 27.3 L at 134 K and 1.0 atm pressure. What will be the volume if the temperature becomes 222 K and the pressure becomes 2.5 atm? P T 1.0 atm 222 K V V P T (27.3 L) atm 134 K PV You could use T PV T L as well (equivalent mathematical statement
3 Section B- Thermochemistry 1B. (b) ii (c) ii It TAKES energy to break bonds; energy is RELEASED when bonds are made. If more energy is used up breaking bonds than the energy released making bonds, then the process overall will require energy (energy must flow IN for it to occur) and it will be endothermic. Since the number of bonds made in this case is two, and the number of bonds broken is also two, if the bonds in the reactants are stronger than the bonds in the products (i.e. bond energies of reactants are larger), it WILL take more energy to break the bonds in the reactants than the energy released upon making the bonds in the products, so the process will be endothermic. (e) v (2(90) 2(33) = 114); (f) ii 4B
4 6B. 10B. (a) (333 J/g)(9.2 g) = 3064 J needed (b) Answer: 60. C Energy flows out of the coffee in order to do TWO things: 1) melt the ice cube and 2) raise the T of the melted water at 0 C up to the final temperature. (It is the 2 nd one that I suspect many students would not think about, but if you did not include that part, I d certainly give you partial credit if you did the rest of the problem correctly.) The deltat of the coffee is related to the amount of energy that flows out of it. So, mathematically: q coffee = -(q flowing into ice to melt it + q flowing into the melted ice to raise its temperature to the final T ) (4.184 J/g C)(238g)(T f 65 C) = - [ (4.184 J/g C)(9.2g)(T f 0 C)] 996T f = T f 1034T f = T f = 60. C (which is reasonable (1 ice cube didn t cool down the coffee by that much)). NOTE: If you ignored the extra energy required to raise the T of the water from the melted ice [i.e., just assumed that the ice cube melted, and that was the only heat flow from the coffee], you d have gotten: (4.184 J/g C)(238g)(T f 65 C) = - [3064] (only approximately correct) 996T f = T f = = T f = 61.9 = 62 C
5 13B. Zero. The standard enthalpy of formation of any substance is the enthalpy change associated with forming ONE MOLE of a substance from its ELEMENTS (in their standard states and most stable forms). Since N 2 (g) is already an element (in its standard state and most stable form), then forming one mole of it from N 2 (g) is doing absolutely nothing (i.e., nothing changed), so there can be no change in enthalpy (H = 0) 13B (added) For each of the following substances, predict whether its standard enthalpy of formation is positive, negative, zero, or state that there not enough information to tell, and provide your reasoning. Strategy: In order to answer this, you need to write (or at least imagine ) what elements the substance is being formed from in the formation equation. So although it was not formally asked for in this problem, I have written those out in each case. If bonds are only broken in forming the substance from its elements (in their standard states and stable form), the enthalpy change is positive; if bonds are only made in forming the substance from its elements, the enthalpy change is negative. If both are involved, you cannot say without quantitative data. And if the substance is an element in its standard state, there is no process (no change at all physically) and thus the enthalpy change is obviously zero (see 13B above). Answers: (a) NO(g): ½ N 2 (g) + ½ O 2 (g) NO(g) Can t tell the sign b/c some bond making and some bond breaking. (b) Cl(g): ½ Cl 2 (g) Cl(g) Positive, b/c only thing happening is the breaking of a bond (c) Fe(s): Fe(s) Fe(s) (d) H 2 (l): H 2 (g) H 2 (l) Zero, b/c there is no change at all here; Fe(s) is the most stable form of iron in its standard state. Negative, b/c although H 2 (l) is an element, it is not in its standard state (at reasonable temperatures). This phase change (condensation) involves the bringing together of H 2 molecules (which attract one another), and so the process is energylowering/exothermic. (e) Mg(NO 3 ) 2 (s): Mg(s) + N 2 (g) + 3 O 2 (g) Mg(NO 3 ) 2 (s) Can t technically tell the sign (without some additional insight/knowledge) since there is both bond making and bond making occurring Section C-QM Model of the Atom (through electron configurations) 1C(a) iv (d) iii (photons of red light have lower energy than photons of green light, so the transition leading to the red emission must correspond to a smaller E between levels. The difference
6 between the 3 rd and 2 nd levels must be less than the difference between the 4 th and 2 nd levels since the higher the n value, the higher the (potential) energy. 2C(a) T The third ionization energy refers to removing the third electron out which would make Mg 3+. Many students don t think this through and think that changing third to second is correct. That is not true, so if you were thinking that, take some time to write out each ionization step and see if you can see why this is statement is true as stated. (b) F diamagnetic (c) T Blue light has photons with higher energy than yellow light. 5C. 7C. 8C. (a) (I ll give verbal descriptions here since I can t easily make boxes. (i) O: 2 electrons in the 1s; 2 electrons in the 2s; 2 electrons in one 2p; 1 electron in each of the other two 2p orbitals. (ii) O 2- : 2 electrons in the 1s; 2 electrons in the 2s; 2 electrons in all three 2p orbitals. (filled shell) (iii) Mg: 2 electrons in the 1s; 2 electrons in the 2s; 2 electrons in all three 2p orbitals. 2 electrons in the 3s. (iv) Mg 2+ : same as (b) (v) excited state of O: One of an infinite number is: 2 electrons in the 1s; 2 electrons in the 2s; 1 electron in each of the three 2p orbitals; 1 electron in the 3s (b) Ne
7 11C. 9C.(a) Small wavelength is associated with higher frequency and thus higher energy-per-photon light (E photon = h = hc/. What dictates the ability of light to eject electrons is its energy per photon (since it takes a certain minimum amount of energy to eject an electron from a surface).
ENTHALPY, INTERNAL ENERGY, AND CHEMICAL REACTIONS: AN OUTLINE FOR CHEM 101A
ENTHALPY, INTERNAL ENERGY, AND CHEMICAL REACTIONS: AN OUTLINE FOR CHEM 101A PART 1: KEY TERMS AND SYMBOLS IN THERMOCHEMISTRY System and surroundings When we talk about any kind of change, such as a chemical
More informationThermochemistry. Energy. 1st Law of Thermodynamics. Enthalpy / Calorimetry. Enthalpy of Formation
THERMOCHEMISTRY Thermochemistry Energy 1st Law of Thermodynamics Enthalpy / Calorimetry Hess' Law Enthalpy of Formation The Nature of Energy Kinetic Energy and Potential Energy Kinetic energy is the energy
More informationGeneral Chemistry 1 CHM201 Unit 3 Practice Test
General Chemistry 1 CHM201 Unit 3 Practice Test 1. Heat is best defined as a. a substance that increases the temperature and causes water to boil. b. a form of potential energy. c. a form of work. d. the
More informationGeneral Chemistry I Final Exam 100 pts Fall 2010
General Chemistry I Final Exam 100 pts Fall 2010 Name This is a closed-book exam: the only reference materials you may use are a periodic table of the elements, a table of enthalpies of formation, and
More informationChemistry Chapter 16. Reaction Energy
Chemistry Reaction Energy Section 16.1.I Thermochemistry Objectives Define temperature and state the units in which it is measured. Define heat and state its units. Perform specific-heat calculations.
More informationAP Chemistry Chapter 16 Assignment. Part I Multiple Choice
Page 1 of 7 AP Chemistry Chapter 16 Assignment Part I Multiple Choice 1984 47. CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 O(l) H = 889.1 kj H f H 2 O(l) = 285.8 kj mol 1 H f CO 2 (g) = 393.3 kj mol 1 What is
More informationTypes of Energy Calorimetry q = mc T Thermochemical Equations Hess s Law Spontaneity, Entropy, Gibb s Free energy
Unit 7: Energy Outline Types of Energy Calorimetry q = mc T Thermochemical Equations Hess s Law Spontaneity, Entropy, Gibb s Free energy Energy Energy is the ability to do work or produce heat. The energy
More informationChapter 5 Practice Multiple Choice & Free
Name Response 1. A system has an increase in internal energy, E, of 40 kj. If 20 kj of work, w, is done on the system, what is the heat change, q? a) +60 kj d) -20 kj b) +40 kj e) -60 kj c) +20 kj 2. Which
More informationName: Thermochemistry. Practice Test C. General Chemistry Honors Chemistry
Name: Thermochemistry C Practice Test C General Chemistry Honors Chemistry 1 Objective 1: Use the relationship between mass, specific heat, and temperature change to calculate the heat flow during a chemical
More informationChemistry Heat Review. Heat: Temperature: Enthalpy: Calorimetry: Activation energy:
Chemistry Heat Review Name Date Vocabulary Heat: Temperature: Enthalpy: Calorimetry: Activation energy: Formulas Heat of phase change Heat for temperature increase Heat of reaction Endothermic/Exothermic
More informationStates of Matter 1 of 21 Boardworks Ltd 2016
States of Matter 1 of 21 Boardworks Ltd 2016 States of Matter 2 of 21 Boardworks Ltd 2016 What are the three states of matter? 3 of 21 Boardworks Ltd 2016 At any given temperature, all substances exist
More informationChapter 8. Thermochemistry
Chapter 8 Thermochemistry Copyright 2001 by Harcourt, Inc. All rights reserved. Requests for permission to make copies of any part of the work should be mailed to the following address: Permissions Department,
More information2. If the volume of a container holding a gas is reduced, what will happen to the presure within the container?
1. Which gas law states that the volume of a fixed mass of a gas is directly proportional to its Kelvin temperature if the pressure is kept constant? A. Boyle s law B. Charles law C. Dalton s law D. Gay-Lussac
More informationChapter 8. Thermochemistry 강의개요. 8.1 Principles of Heat Flow. 2) Magnitude of Heat Flow. 1) State Properties. Basic concepts : study of heat flow
강의개요 Basic concepts : study of heat flow Chapter 8 Thermochemistry Calorimetry : experimental measurement of the magnitude and direction of heat flow Thermochemical Equations Copyright 2005 연세대학교이학계열일반화학및실험
More informationChemistry 4A Midterm Exam 2 Version B October 17, 2008 Professor Pines Closed Book, 50 minutes, 125 points 5 pages total (including cover)
Chemistry 4A Midterm Exam 2 Version B October 17, 2008 Professor Pines Closed Book, 50 minutes, 125 points 5 pages total (including cover) Student Name: KEY Student ID#: GSI Name: Lab Section Day/Time:
More informationIntroduction to Thermochemistry. Thermochemistry Unit. Definition. Terminology. Terminology. Terminology 07/04/2016. Chemistry 30
Thermochemistry Unit Introduction to Thermochemistry Chemistry 30 Definition Thermochemistry is the branch of chemistry concerned with the heat produced and used in chemical reactions. Most of thermochemistry
More informationCHEM 101 Fall 08 Exam II(a)
CHEM 101 Fall 08 Exam II(a) On the answer sheet (scantron) write you name, student ID number, and recitation section number. Choose the best (most correct) answer for each question and enter it on your
More informationThermodynamics: Entropy
Name: Band: Date: Thermodynamics: Entropy Big Idea: Entropy When we were studying enthalpy, we made a generalization: most spontaneous processes are exothermic. This is a decent assumption to make because
More informationCHAPTER 17 Thermochemistry
CHAPTER 17 Thermochemistry Thermochemistry The study of the heat changes that occur during chemical reactions and physical changes of state. Chemical Change: new substances created during chemical reaction
More informationChapter 14. Liquids and Solids
Chapter 14 Liquids and Solids Review Solid - Has a definite (fixed) shape and volume (cannot flow). Liquid - Definite volume but takes the shape of its container (flows). Gas Has neither fixed shape nor
More informationWater SECTION The properties of water in all phases are determined by its structure.
SECTION 10.5 Water Water commonly exists in all three physical states on Earth, where it is by far the most abundant liquid. It covers nearly three-quarters of Earth s surface. Water is an essential component
More informationSemester 2 Final Exam Review. Semester 2 Final Exam Review. South Pasadena Chemistry. Period Date / /
South Pasadena Chemistry Name Period Date / / S T A T I O N 1 H E A T For water, Cp,ice = 2.10 J/ g C, Cp,water = 4.18 J/ g C, Cp,steam = 2.08 J/g C, Hfus = 333 J/g, Hvap = 2260 J/g 50.0 g of water at
More informationChemical Thermodynamics
Chemical Thermodynamics Overview Everything in the world is a balance of energy, in various forms from biological processes to the rusting of a nail. Two of the most important questions chemists ask are:
More informationUseful Information to be provided on the exam: 1 atm = 760 mm Hg = 760 torr = lb/in 2 = 101,325 Pa = kpa. q = m C T. w = -P V.
Chem 101A Study Questions, Chapters 5 & 6 Name: Review Tues 10/25/16 Due 10/27/16 (Exam 3 date) This is a homework assignment. Please show your work for full credit. If you do work on separate paper, attach
More informationPlease pass in only this completed answer sheet on the day of the test. LATE SUBMISSIONS WILL NOT BE ACCEPTED
CHM-201 General Chemistry and Laboratory I Unit #3 Take Home Test Due April 8, 2019 Please pass in only this completed answer sheet on the day of the test. LATE SUBMISSIONS WILL NOT BE ACCEPTED CHM-201
More informationThermochemistry Chapter 4
Thermochemistry Chapter 4 Thermochemistry is the study of energy changes that occur during chemical reactions Focus is on heat and matter transfer between the system and the surroundings Energy The ability
More informationCHEM 200/202 Exam 2 October 18, Lab Section #:
Name: Lab Section #: Please mark your answers on the scantron sheet using a #2 pencil and also mark your answers on the exam itself. Mark Test From A on your scantron. 1. A 4.25 L container is filled with
More informationHeat. Heat Terminology 04/12/2017. System Definitions. System Definitions
System Definitions Heat Physical Science 20 Ms. Hayduk Heat Terminology System: the part of the universe being studied (big Earth, or small one atom) Surroundings: the part of the universe outside the
More informationCHEMISTRY 102B Hour Exam II. Dr. D. DeCoste T.A.
CHEMISTRY 10B Hour Exam II March 19, 015 Dr. D. DeCoste Name Signature T.A. This exam contains questions on 9 numbered pages. Check now to make sure you have a complete exam. You have one hour and thirty
More information= (25.0 g)(0.137 J/g C)[61.2 C - (-31.4 C)] = 317 J (= kj)
CHEM 101A ARMSTRONG SOLUTIONS TO TOPIC D PROBLEMS 1) For all problems involving energy, you may give your answer in either joules or kilojoules, unless the problem specifies a unit. (In general, though,
More informationCHEMISTRY Practice Exam #3 - SPRING 2013
CHEMISTRY 1710 - Practice Exam #3 - SPRING 2013 Section 1 - This section of the exam is multiple choice. Choose the BEST answer from the choices which are given and write the letter for your choice in
More informationCHEM 1211K Test IV. 3) The phase diagram of a substance is given above. This substance is a at 25 o C and 1.0 atm.
CEM 1211K Test IV A MULTIPLE COICE. ( points) 1) A sample of a gas (5.0 mol) at 1.0 atm is expanded at constant temperature from 10 L to 15 L. The final pressure is atm. A). B) 1.5 C) 15 D) 7.5 E) 0.67
More informationThermochemistry-Part 1
Brad Collins Thermochemistry-Part 1 Chapter 7 Thermochemistry Thermodynamics: The study of energy Thermochemistry: The study of energy in chemical reactions Energy: The capacity to do work Work = force
More information(3 pts) 2. In which gas sample do the molecules have a lower average kinetic energy? (A) Gas A (B) Gas B (C) Neither
Consider two samples of gas, A and B, as shown in the figure below. Both containers are at the same temperature and pressure. Gas A 1.0 L 0.32 g Gas B 1.0 L 0.48 g (3 pts) 1. Which gas sample contains
More informationThermochemistry is the study of the relationships between chemical reactions and energy changes involving heat.
CHEM134- F18 Dr. Al- Qaisi Chapter 06: Thermodynamics Thermochemistry is the study of the relationships between chemical reactions and energy changes involving heat. Energy is anything that has the capacity
More informationCHEMISTRY 110 EXAM 3 April 2, 2012 FORM A 1. Which plot depicts the correct relationship between the volume and number of moles of an ideal gas at constant pressure and temperature? 2. The height of the
More informationCHEMISTRY 202 Hour Exam I. Dr. D. DeCoste T.A.
CHEMISTRY 202 Hour Exam I September 22, 2016 Dr. D. DeCoste Name Signature T.A. This exam contains 23 questions on 11 numbered pages. Check now to make sure you have a complete exam. You have two hours
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 informationS = k log W 11/8/2016 CHEM Thermodynamics. Change in Entropy, S. Entropy, S. Entropy, S S = S 2 -S 1. Entropy is the measure of dispersal.
Entropy is the measure of dispersal. The natural spontaneous direction of any process is toward greater dispersal of matter and of energy. Dispersal of matter: Thermodynamics We analyze the constraints
More informationSection 1 - Thermochemistry
Reaction Energy Section 1 - Thermochemistry Virtually every chemical reaction is accompanied by a change in energy. Chemical reactions usually absorb or release energy as heat. You learned in Chapter 12
More informationName Date Class THERMOCHEMISTRY
Name Date Class 17 THERMOCHEMISTRY SECTION 17.1 THE FLOW OF ENERGY HEAT AND WORK (pages 505 510) This section explains the relationship between energy and heat, and distinguishes between heat capacity
More informationThermochemistry: Heat and Chemical Change
Thermochemistry: Heat and Chemical Change 1 Heat or Thermal Energy (q) Heat is a form of energy Is heat the same as temperature? Heat flows between two objects at different temperatures. Hot Cold 2 Chemical
More informationAccelerated Chemistry Study Guide Chapter 12, sections 1 and 2: Heat in Chemical Reactions
Accelerated Chemistry Study Guide Chapter 12, sections 1 and 2: Heat in Chemical Reactions Terms, definitions, topics Joule, calorie (Re-read p 57-58) Thermochemistry Exothermic reaction Endothermic reaction
More information1. State in your own terms what is the first law of thermodynamics, a closed system, an isolated system, surroundings, heat, work, and energy.
Worksheet 1 1. State in your own terms what is the first law of thermodynamics, a closed system, an isolated system, surroundings, heat, work, and energy. The first law of thermodynamics is the conservation
More informationCHEMISTRY 109 #25 - REVIEW
CHEMISTRY 109 Help Sheet #25 - REVIEW Chapter 4 (Part I); Sections 4.1-4.6; Ch. 9, Section 9.4a-9.4c (pg 387) ** Review the appropriate topics for your lecture section ** Prepared by Dr. Tony Jacob http://www.chem.wisc.edu/areas/clc
More informationChapter 5 Thermochemistry
Chapter 5 Thermochemistry Energy -Very much a chemistry topic Every chemical change has an accompanying change of. Combustion of fossil fuels The discharging a battery Metabolism of foods If we are to
More informationPUT YOUR NAME ON THE THIRD PAGE, AND ALL FOLLOWING PAGES
PUT YOUR NAME ON THE THIRD PAGE, AND ALL FOLLOWING PAGES REFERENCE SHEET FOR CHEM 1 MIDTERM EXAMINATION (Not all data on this sheet will be necessary for any given exam) 1 THIS EXAM HAS 8 PAGES (INCLUDING
More informationCST Review Part 2. Liquid. Gas. 2. How many protons and electrons do the following atoms have?
CST Review Part 2 1. In the phase diagram, correctly label the x-axis and the triple point write the names of all six phases transitions in the arrows provided. Liquid Pressure (ATM) Solid Gas 2. How many
More informationPractice Test F.1 (pg 1 of 7) Unit F - General Equilibrium Kp and Kc Name Per
Practice Test F. (pg of 7) Unit F - General Equilibrium Kp and Kc Name Per This is practice - Do NOT cheat yourself of finding out what you are capable of doing. Be sure you follow the testing conditions
More informationOUTLINE. States of Matter, Forces of Attraction Phase Changes Gases The Ideal Gas Law Gas Stoichiometry
UNIT 6 GASES OUTLINE States of Matter, Forces of Attraction Phase Changes Gases The Ideal Gas Law Gas Stoichiometry STATES OF MATTER Remember that all matter exists in three physical states: Solid Liquid
More information2nd Semester Exam Review. C. K eq = [N 2][H 2 ]
Name: ate: 1. Which pair of formulas represents the empirical formula and the molecular formula of a compound?. H 2 O, 4 H 6 O 4. HO, 6 H 12 O 6 8. Given the reaction at equilibrium: N 2 (g) + 3H 2 (g)
More informationMelting. Freezing. Triple Point. Sublimation. Deposition. Temperature. 2. How many protons and electrons do the following atoms have?
CST Review Part 2 1. In the phase diagram, correctly label the x-axis and the triple point write the names of all six phases transitions in the arrows provided. Melting Liquid Freezing Pressure (ATM) Solid
More informationName Chemistry / / SOL Questions Chapter 9 For each of the following, fill in the correct answer on the BLUE side of the scantron.
Name Chemistry / / SOL Questions Chapter 9 For each of the following, fill in the correct answer on the BLUE side of the scantron. 1. Which number on the graph to the right represents the effect of the
More informationThermochemistry. Energy (and Thermochemistry) World of Chemistry Chapter 10. Energy. Energy
Thermochemistry Thermodynamics is the science of the relationship between heat and other forms of energy. (and Thermochemistry) World of Chemistry Chapter 10 is defined as the ability to do work or produce
More informationENTHALPY CHANGE CHAPTER 4
ENTHALPY CHANGE CHAPTER 4 ENTHALPY Is the total energy of a system. E k = Kinetic energy. Vibrational Rotational Translational E due to motion H = E k + E p E P = Potential energy Attractive force b/w
More informationChemistry 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
More informationChapter 6: Thermochemistry
Chapter 6: Thermochemistry Section 6.1: Introduction to Thermochemistry Thermochemistry refers to the study of heat flow or heat energy in a chemical reaction. In a study of Thermochemistry the chemical
More informationLecture 20. Phase Transitions. Phase diagrams. Latent heats. Phase-transition fun. Reading for this Lecture: Elements Ch 13.
Lecture 20 Phase ransitions Phase diagrams Latent heats Phase-transition fun Reading for this Lecture: Elements Ch 13 Lecture 20, p 1 Solid-gas equilibrium: vapor pressure Consider solid-gas equilibrium
More informationChapter 11. Thermochemistry. 1. Let s begin by previewing the chapter (Page 292). 2. We will partner read Pages
Chapter 11 Thermochemistry 1. Let s begin by previewing the chapter (Page 292). 2. We will partner read Pages 293-94 The Flow of energy - heat Thermochemistry concerned with the heat changes that occur
More informationThe Equilibrium State. Chapter 13 - Chemical Equilibrium. The Equilibrium State. Equilibrium is Dynamic! 5/29/2012
Chapter 13 - Chemical Equilibrium The Equilibrium State Not all chemical reactions go to completion; instead they attain a state of equilibrium. When you hear equilibrium, what do you think of? Example:
More informationChapter 5 Thermochemistry
Chapter 5 Thermochemistry Learning Outcomes: Interconvert energy units Distinguish between the system and the surroundings in thermodynamics Calculate internal energy from heat and work and state sign
More informationCHAPTER 17: THERMOCHEMISTRY. Mrs. Brayfield
CHAPTER 17: THERMOCHEMISTRY Mrs. Brayfield REVIEW What is the law of conservation of energy? It states that energy cannot be created or destroyed So the energy of any process is the same THERMOCHEMISTRY
More informationCHEM 101 Fall 09 Final Exam (a)
CHEM 101 Fall 09 Final Exam (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
More informationPractice Packet Unit 3: Phase Changes & Heat
Regents Chemistry: Practice Packet Unit 3: Phase Changes & Heat Name: Assess Yourself: Lesson 1: Lesson 2: Lesson 3: Lesson 4: Vocab: 1 Review (Things you need to know in order to understand the new stuff
More informationDepartment of Chemistry Memorial University Chemistry 1050
Department of Chemistry Memorial University Chemistry 1050 Fall 2013 Deferred Examination Time 3 hours NAME: MUN Student Number: Circle your professor s name: Dr. R. Davis Dr. T. Fridgen Dr. C. Kozak Read
More informationSummary of Gas Laws V T. Boyle s Law (T and n constant) Charles Law (p and n constant) Combined Gas Law (n constant) 1 =
Summary of Gas Laws Boyle s Law (T and n constant) p 1 V 1 = p 2 V 2 Charles Law (p and n constant) V 1 = T 1 V T 2 2 Combined Gas Law (n constant) pv 1 T 1 1 = pv 2 T 2 2 1 Ideal Gas Equation pv = nrt
More informationThermodynamics I - Enthalpy
Thermodynamics I - Enthalpy Tinoco Chapter 2 Secondary Reference: J.B. Fenn, Engines, Energy and Entropy, Global View Publishing, Pittsburgh, 2003. 1 Thermodynamics CHEM 2880 - Kinetics An essential foundation
More informationS = k log W CHEM Thermodynamics. Change in Entropy, S. Entropy, S. Entropy, S S = S 2 -S 1. Entropy is the measure of dispersal.
, S is the measure of dispersal. The natural spontaneous direction of any process is toward greater dispersal of matter and of energy. Dispersal of matter: Thermodynamics We analyze the constraints on
More informationChem. 1B Final Practice
Chem. 1B Final Practice Name Student Number All work must be shown on the exam for partial credit. Points will be taken off for incorrect or no units and for the incorrect number of significant figures.
More informationChapter 5. Thermochemistry
Chapter 5 Thermochemistry Energy Thermodynamics Study of the relationship between heat, work, and other forms of energy Thermochemistry A branch of thermodynamics Focuses on the study of heat given off
More informationChapter 11. Intermolecular Forces, Liquids, and Solids
Sample Exercise 11.1 (p. 450) In which of the following substances is hydrogen bonding likely to play an important role in determining physical properties: methane (CH 4 ), hydrazine (H 2 NNH 2 ), methyl
More informationName: Class: Date: SHORT ANSWER Answer the following questions in the space provided.
CHAPTER 10 REVIEW States of Matter SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. Identify whether the descriptions below describe an ideal gas or a real gas. a. The gas
More informationCHEM 60 Spring 2016 Exam 3 Ch 9-12, 100 points total.
Name Exam No. F CHEM 60 Spring 2016 Exam 3 Ch 9-12, 100 points total. Multiple Choice. (25 questions, 3 points each = 75 points total) Mark the letter on the scantron form corresponding to the one best
More informationVersion 001 Practice Final Exam 1
Version 001 Practice Final Exam 1 This print-out should have 50 questions. Multiple-choice questions may continue on the next column or page find all choices before answering. 001 2.0 points ow many moles
More informationStates of Matter Chapter 10 Assignment & Problem Set
States of Matter Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. States of Matter 2 Study Guide: Things You Must Know Vocabulary (know the definition
More informationName AP CHEM / / Collected AP Exam Essay Answers for Chapter 16
Name AP CHEM / / Collected AP Exam Essay Answers for Chapter 16 1980 - #7 (a) State the physical significance of entropy. Entropy (S) is a measure of randomness or disorder in a system. (b) From each of
More informationChapter Practice Test Grosser
Class: Date: Chapter 10-11 Practice Test Grosser Multiple Choice Identify the choice that best completes the statement or answers the question. 1. According to the kinetic-molecular theory, particles of
More informationName Class Date. As you read Lesson 17.1, use the cause and effect chart below. Complete the chart with the terms system and surroundings.
Name Class Date Thermochemistry 17.1 The Flow of Energy As you read Lesson 17.1, use the cause and effect chart below. Complete the chart with the terms system and surroundings. Process Cause Effect endothermic
More informationChapter 7. Gases, liquids, and solids. Water coexisting in three states H 2 O (g) in air H 2 O (l) ocean H 2 O (s) iceberg
Chapter 7 Gases, liquids, and solids Water coexisting in three states H 2 O (g) in air H 2 O (l) ocean H 2 O (s) iceberg What s crack a lackin? Kinetic-molecular theory of gases Physical states and the
More informationSection 16.3 Phase Changes
Section 16.3 Phase Changes Solid Liquid Gas 3 Phases of Matter Density of Matter How packed matter is (The amount of matter in a given space) Solid: Liquid: Gas: High Density Medium Density Low Density
More informationSelected Questions on Chapter 5 Thermochemistry
Selected Questions on Chapter 5 Thermochemistry Circle the correct answer: 1) At what velocity (m/s) must a 20.0 g object be moving in order to possess a kinetic energy of 1.00 J? A) 1.00 B) 100 10 2 C)
More informationChemical Equilibrium Practice Problems #2
Chemical Equilibrium Practice Problems #2 2-20-2015 1. A CPHS student does an equilibrium experiment with the general chemical equation and derives the 2 graphs below: A = B: a. When at equilibrium is
More informationLiquids & Solids: Section 12.3
Liquids & Solids: Section 12.3 MAIN IDEA: The particles in and have a range of motion and are not easily. Why is it more difficult to pour syrup that is stored in the refrigerator than in the cabinet?
More information5. Solve the following a) What energy is required to heat 55.5 g of carbon from -10 C to 47 C (Ccarbon = 0.71 J/g C)
Ch.10 - Energy 1. How is the concept of energy defined? Name: Period: 2. What does temperature measure? 3. Explain what is meant by the terms exothermic and endothermic. 4. What is meant by the specific
More informationCHE 105 EXAMINATION III April 4, 2013
CHE 105 EXAMINATION III April 4, 2013 University of Kentucky Department of Chemistry READ THESE DIRECTIONS CAREFULLY BEFORE STARTING THE EXAMINATION! It is extremely important that you fill in the answer
More information3.3 Phase Changes 88 A NATURAL APPROACH TO CHEMISTRY. Section 3.3 Phase Changes
Section 3.3 Phase Changes 3.3 Phase Changes Solid, liquid and gas During a phase change, a substance rearranges the order of its particles (atoms or molecules). Examples of phase change include melting
More informationUnit 6. Unit Vocabulary: Distinguish between the three phases of matter by identifying their different
*STUDENT* Unit Objectives: Absolute Zero Avogadro s Law Normal Boiling Point Compound Cooling Curve Deposition Energy Element Evaporation Heat Heat of Fusion Heat of Vaporization Unit 6 Unit Vocabulary:
More informationChapter 15 Chemical Equilibrium
Chapter 15 Chemical Chemical 15.1 The Concept of 15.2 The Constant (K) 15.3 Understanding and Working with Constants 15.4 Heterogeneous Equilibria 15.5 Calculating Constants 15.6 Applications of Constants
More informationChemistry 104 Final Exam Content Evaluation and Preparation for General Chemistry I Material
Chemistry 104 Final Exam Content Evaluation and Preparation for General Chemistry I Material What is 25 mph in mm s 1? Unit conversions What is 1025 K in o F? Which is larger 1 ft 3 or 0.1 m 3? What is
More informationCHEMISTRY REVIEW FOR AP BIOLOGY Answer Key
CHEMISTRY REVIEW FOR AP BIOLOGY Answer Key Complete the following and be knowledgeable of the concepts on the first day of school. A. KINETICS = involves factors that affect the rate of a chemical reaction.
More informationChapter 15: Chemical Equilibrium. Chem 102 Dr. Eloranta
Chapter 15: Chemical Equilibrium Chem 102 Dr. Eloranta Equilibrium State in which competing processes are balanced so that no observable change takes place as time passes. Lift Gravity Sometimes called
More informationName: Regents Review Quiz #1 2016
Name: Regents Review Quiz #1 2016 1. Which two particle diagrams represent mixtures of diatomic elements? A) A and B B) A and C C) B and C D) B and D 2. At STP, which physical property of aluminum always
More informationVersion 001 Practice Final Exam 1
Version 001 Practice Final Exam 1 This print-out should have 50 questions. Multiple-choice questions may continue on the next column or page find all choices before answering. 001 2.0 points Thesecond
More informationName: Class: Date: ID: A
Name: Class: _ Date: _ ID: A Chpter 17 review Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which of these phase changes is an endothermic process? a.
More informationChem Hughbanks Final Exam, May 11, 2011
Chem 107 - Hughbanks Final Exam, May 11, 2011 Name (Print) UIN # Section 503 Exam 3, Version # A On the last page of this exam, you ve been given a periodic table and some physical constants. You ll probably
More informationCHEM Thermodynamics. Entropy, S
hermodynamics Change in Change in Entropy, S Entropy, S Entropy is the measure of dispersal. he natural spontaneous direction of any process is toward greater dispersal of matter and of energy. Dispersal
More informationChapter 11. Liquids and Intermolecular Forces
Chapter 11 Liquids and Intermolecular Forces States of Matter The three states of matter are 1) Solid Definite shape Definite volume 2) Liquid Indefinite shape Definite volume 3) Gas Indefinite shape Indefinite
More informationGas 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
More informationSample Exercise 11.1 Identifying Substances That Can Form Hydrogen Bonds
Sample Exercise 11.1 Identifying Substances That Can Form Hydrogen Bonds In which of these substances is hydrogen bonding likely to play an important role in determining physical properties: methane (CH
More informationChemistry 212 Fall 2017 Exam III - A
Chemistry 212 Fall 2017 Exam III - A Name MULTIPLE CHOICE. (1 point each) Choose the one alternative that best completes the statement or answers the question. 1) An important step in the synthesis of
More information