1.8. ΔG = ΔH - TΔS ΔG = ΔG + RT ln Q ΔG = - RT ln K eq. ΔX rxn = Σn ΔX prod - Σn ΔX react. ΔE = q + w ΔH = ΔE + P ΔV ΔH = q p = m Cs ΔT
|
|
- Ashlynn Atkins
- 6 years ago
- Views:
Transcription
1 ThermoDynamics Practice Exam Thermodynamics Name (last) (First) Read all questions before you start. Show all work and explain your answers to receive full credit. Report all numerical answers to the proper number of significant figures. By signing your signature above you agree that you have worked alone and neither give nor received help from any source. Keep your eyes on your own paper at all times System LENGTH: VOLUME MASS Temperature English: 1 ft = 12 in 1 gal = 4 qt 1 lb = 16 oz T F = 1.8T C mile = 5280 ft 1 qt = in 3 1 ton = 2000 lb 1 yd = 3 ft SI- English: 1 in = 2.54 cm 1 mi = km 1 L = qt 1 qt = L 1 lb = g 1 oz = g T C = (T F 32) 1.8 Misc. info 1 mole = R = J/ mol K or L atm/mol K Thermodynamics Universe = surroundings + system State Function (X) where X = E, H, S or G ΔX rxn = Σn ΔX prod - Σn ΔX react w = -P ΔV ΔE = q + w ΔH = ΔE + P ΔV ΔH = q p = m Cs ΔT ΔS univ = ΔS surr + ΔS sys ΔS surr = - ΔH sys / T Thermodynamics ΔG = ΔH - TΔS ΔG = ΔG + RT ln Q ΔG = - RT ln K eq K eq = exp {-ΔG /RT} ln K eq = (ΔS / R) - (ΔH / RT) Temperature Conversion C = 5/9 ( F - 32) F = ( 9/5 _ C ) + 32)
2 Multiple -choice. Show work for partial credit. 1 Consider the room temperature condensation of steam: H 2 O (g) H 2 O (l). Which parameter is positive? a) ΔH b) ΔS c) ΔG d) none 2 Which law of thermodynamics states that energy in, equals energy out: Energy in = Energy out. a) First Law of Thermodynamics b) Second Law of T Thermodynamics c) Third Law of Thermodynamics d) This statement violates all Laws of Thermodynamics 3 If the heat of reaction is endothermic, which of the following is always true? a) the reaction is fast b) the energy of the reactants is greater than the products c) the reaction is slow d) the energy of the reactants is lower than the products 4 Which among the following has the lowest entropy? a) H 2 O (g) b) H 2 O (l) c) H 2(l) d) All the same 5 Which gas law states that at zero Kelvin, matter ceases to have volume? a) Boyle b) Gay-Lussac c) Charles d) Avogadro 6 What will happen to a reaction if H sys < 0 and S sys < 0? a) will never proceed spontaneously to the right. b) proceed spontaneously to the right only at low temperatures. c) proceed spontaneously to the right only at high temperatures. d) proceed spontaneously to the right at all temperatures. 7 Consider the formation of ammonia: N 2(g) + 3 H 2(g) 2 NH 3(g) Assuming that H and S are constant with temperature, find the temperature at which K p = a) 695 K b) 233 K c) 466 K d) 348 K ΔH = 2(-46.19) - [0 + 0] = kj ΔG = 2(-16.66) - [0 + 0] = kj ΔS = 2(192.5) - [ ( )] = J T = ΔH ΔS = = 466 K 8 When water freezes at 0 C, which of the following is always true? a) Keq = 0 b) ΔG = 0 c) Q = 0 e) ΔS = 0 9 Which thermodynamic parameter is equal to the difference between the energy of the product and the energy of the reactant at constant pressure? a) ΔG Sys b) E cell c) ΔS sys d) ΔH sys 10 The super zero, ( ) in the state functions S, E, H and G stands for: a) Standard state. b) raising the state function to the zeroth power. c) Temperature at absolute zero. d) an oxidation state of zero for the system.
3 11 Supply the missing information (question marks) in each row of the following table: ΔSrnx ΔHrxn ΔGrxn Comment i Spontaneous ii Spontaneous iii Not Spontaneous iv Spontaneous v non-spontaneous vi TΔS > ΔH non-spontaneous 12 For each of the following group, arrange each system in order of increasing standard entropy, S, and explain your choice. ( lowest (1) medium (2) - highest (3) ) i) K, Li, Rb: Li (1) < K (2) < Rb (3) Complexity, atomic mass ii) HF, HBr, HCl: HF (1) < HCl (2) < HBr (3) Complexity, Molar mass iii) hot water, steam, ice water: iv) diamond, charcoal, graphite: Ice water (1) < Hot water (2) < Steam (3) Phase and Temperature graphite (1) < diamond (2) < charcoal (3) Complexity, organization of carbon 13 i) The Entropy in the universe is always a) increasing b) decreasing c) zero d) constant ii) Which law of thermodynamics states the condition of spilled water. a) first law b) second law c) third law d) outlaw iii) Which of the following is not a state function? a) work b) q (constant pressure) c) Entropy d) Free Energy
4 14 You must follow the directions for this question. Arrange each of the following groups in order of increasing state function, X, and explain your choice. The order should be smallest or most negative (1) to medium (2) to largest or most positive (3). Place numerical value for each choice, 1, 2 or 3 after placing them in order and justify your answer. i) Enthalpy: (a) 2.0 gram of NH3 (g), (b) 1.0 gram of CH4 (g), (c) 2.0 grams of HCl(g) ii) Entropy: (a) Na (s) + C (s) + 3/2 O 2(g), (b) NaCO 3(s), (c) NaO (s) + CO 2(g) iii) Free energy under standard conditions: (a) Cr +3 /Cr, (b) Ag + /Ag, (c) Ga +3 /Ga 15 The excessive production of ozone (O3) gas in the lower atmosphere causes rubber to deteriorate, green plants to turn brown, and persons with respiratory disease to have difficulty breathing. i) Is the formation of O3 from O2 favor at all temperature, at no temperature, at high temperature, or low temperature? ii) Calculate ΔG for this reaction at 298 K and 1 atm. iii) Calculate ΔG, at 298 K for this reaction urban smog where [O2] = 0.21 M and [O3] = M The reaction is: 3 O2 (g) 2 O3 (g) kj/mol
5 16 Check mark if you agree or disagree with the following statement, then write a short convincing explanation to support or refute the statement. No credit will be given without justification. i) Agree Disagree: All reactions with equilibrium constant greater than one (Keq > 1) are spontaneous. ΔG = -RT lnkeq for Keq >1, ΔG becomes negative. ii) Agree Disagree: All spontaneous reactions occur quickly. Kinetics and Thermodynamics occur independently from each other. iii) Agree Disagree: The electrolysis of salt water will result in the oxidation of Na + at the anode. The oxidation and reduction of water occurs at a lower potential of ~ 2.1 V iv) Agree Disagree: The following line-notation represents a voltaic cell. Ag(s) Ag + (aq) Cd +2 (aq) Cd(s) v) _+_ Agree Disagree: A typical car batter can carry a voltage greater than 12 Volts. If the concentration of reactant is higher than 1M, then the Nernst equation will show a potential of greater than 12 V for a car battery. vi) Agree _+_ Disagree: Positive electromotive force corresponds to positive free energy and positive ΔS(Universe). False, positive EMF, according to ΔG = - nfe, yields a negative free energy (and postive ΔSUniverse). 17 K w at 25 = , and K w at 50 = What is ΔH, ΔS and ΔG for the auto-ionization of water at 25? ΔG = 79.8 kj/mol, ΔH = 55.8 kj/mol, ΔS = J/mol 18 In photosynthesis, CO2 (g) and H2O(g) is converted to glucose C6H12O6 (s) and oxygen (O2) (g). at 298 K. 6 CO2 (g) + 6 H2O(g) C6H12O6 (s) + 6 O 2 (g) [C6H12O6 (s) : ΔHf = KJ/mol, ΔSf = J/mol K ] a) Is this an exothermic or endothermic process? Calculated ΔH rxn. b) What is ΔS sys, ΔS surr? c) Calculate K eq for this reaction.
6 19 Consider the formation of methyl alcohol from carbon monoxide and hydrogen: 2 CO (g) + 4 H 2 (g) 2 CH 3 OH (g) a) What are ΔH and ΔS for the reaction (T= 298 K)? In what direction will this reaction proceed spontaneously? b) Calculate ΔG rxn (T = 298 K and P = 1 atm for all species) c) At what temperature will the spontaneity of the reaction reverse itself? 20 During a hot summer day, your friend suggests opening the door of your refrigerator to cool your kitchen. Will his strategy work? Discuss your answer in terms of thermodynamics. 21 During a hot summer day, your friend suggests opening the door of your refrigerator to cool your kitchen. Will his strategy work? Discuss your answer in terms of thermodynamics.
1.8. ΔG = ΔH - TΔS ΔG = ΔG + RT ln Q ΔG = - RT ln K eq. ΔX rxn = Σn ΔX prod - Σn ΔX react. ΔE = q + w ΔH = ΔE + P ΔV ΔH = q p = m Cs ΔT
ThermoDynamics Practice Exam Thermodynamics Name (last) (First) Read all questions before you start. Show all work and explain your answers to receive full credit. Report all numerical answers to the proper
More informationChemical Kinetics. System LENGTH: VOLUME MASS Temperature. 1 gal = 4 qt. 1 qt = in 3. 1 L = qt. 1 qt = L
Chemical Kinetics Practice Exam Chemical Kinetics Name (last) (First) Read all questions before you start. Show all work and explain your answers to receive full credit. Report all numerical answers to
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 informationSecond Law of Thermodynamics
Second Law of Thermodynamics First Law: the total energy of the universe is a constant Second Law: The entropy of the universe increases in a spontaneous process, and remains unchanged in a process at
More informationThermochemistry Chapter 8
Thermochemistry Chapter 8 Thermochemistry First law of thermochemistry: Internal energy of an isolated system is constant; energy cannot be created or destroyed; however, energy can be converted to different
More informationQuadratic Equation: ax 2 + bx + c = 0
Exam # Key (last) (First-Name) Signature Exam 2 General Chemistry 201. May 12, 2009 No credit will be given for correct numerical answers without a clear indication of how they were obtained. Show all
More informationDisorder and Entropy. Disorder and Entropy
Disorder and Entropy Suppose I have 10 particles that can be in one of two states either the blue state or the red state. How many different ways can we arrange those particles among the states? All particles
More informationUnit 5: Spontaneity of Reaction. You need to bring your textbooks everyday of this unit.
Unit 5: Spontaneity of Reaction You need to bring your textbooks everyday of this unit. THE LAWS OF THERMODYNAMICS 1 st Law of Thermodynamics Energy is conserved ΔE = q + w 2 nd Law of Thermodynamics A
More informationLecture #13. Chapter 17 Enthalpy and Entropy
Lecture #13 Chapter 17 Enthalpy and Entropy First Law of Thermodynamics Energy cannot be created or destroyed The total energy of the universe cannot change Energy can be transferred from one place to
More informationChemical Thermodynamics
Page III-16-1 / Chapter Sixteen Lecture Notes Chemical Thermodynamics Thermodynamics and Kinetics Chapter 16 Chemistry 223 Professor Michael Russell How to predict if a reaction can occur, given enough
More informationEntropy, Free Energy, and Equilibrium
Entropy, Free Energy, and Equilibrium Chapter 17 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Spontaneous Physical and Chemical Processes A waterfall runs
More informationChapter 19 Chemical Thermodynamics
Chapter 19 Chemical Thermodynamics Spontaneous Processes Entropy and the Second Law of Thermodynamics The Molecular Interpretation of Entropy Entropy Changes in Chemical Reactions Gibbs Free Energy Free
More informationThermochemistry. Chapter 6. Dec 19 8:52 AM. Thermochemistry. Energy: The capacity to do work or to produce heat
Chapter 6 Dec 19 8:52 AM Intro vocabulary Energy: The capacity to do work or to produce heat Potential Energy: Energy due to position or composition (distance and strength of bonds) Kinetic Energy: Energy
More informationThermodynamics: Free Energy and Entropy. Suggested Reading: Chapter 19
Thermodynamics: Free Energy and Entropy Suggested Reading: Chapter 19 System and Surroundings System: An object or collection of objects being studied. Surroundings: Everything outside of the system. the
More informationCHM 112 Chapter 16 Thermodynamics Study Guide
CHM 112 Chapter 16 Thermodynamics Study Guide Remember from Chapter 5: Thermodynamics deals with energy relationships in chemical reactions Know the definitions of system, surroundings, exothermic process,
More informationSpontaneity, Entropy, and Free Energy
Spontaneity, Entropy, and Free Energy A ball rolls spontaneously down a hill but not up. Spontaneous Processes A reaction that will occur without outside intervention; product favored Most reactants are
More informationChapter 16. Thermodynamics. Thermochemistry Review. Calculating H o rxn. Predicting sign for H o rxn. Creative Commons License
Chapter 16 Thermodynamics GCC CHM152 Creative Commons License Images and tables in this file have been used from the following sources: OpenStax: Creative Commons Attribution License 4.0. ChemWiki (CC
More informationFind this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site.
Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site. Still having trouble understanding the material? Check
More informationChemistry 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
More informationBCIT Fall Chem Exam #2
BCIT Fall 2017 Chem 3310 Exam #2 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 informationChapter Eighteen. Thermodynamics
Chapter Eighteen Thermodynamics 1 Thermodynamics Study of energy changes during observed processes Purpose: To predict spontaneity of a process Spontaneity: Will process go without assistance? Depends
More information1. III only 2. II, III. 3. II only. 4. I only 5. I, III. 6. I, II, III correct
Version 001 EXAM 8 PRACTICE PROBLEMS chemistry (78712) 1 This print-out should have 20 questions. Multiple-choice questions may continue on the next column or page find all choices before answering. 001
More informationBonus Final Exam 3. 1 Calculate the heat of reaction,δh 0 rxn, for the following reaction as written at 298 K: g 2H 2 CH 4. g CF 4.
Bonus Final Exam 3 1 Calculate the heat of reaction,δh rxn, for the following reaction as written at 298 K: CH 4 2F 2 CF 4 2H 2 substance CH 4 CF 4 ΔH f kj/mol 75 68 (A) ΔH rxn 23 kj (B) ΔH rxn 914 kj
More informationEntropy and Free Energy
Page 1 Entropy and Free Energy How to predict if a reaction can occur at a reasonable rate? KINEICS Chapter 17 How to predict if a reaction can occur, given enough time? HERMODYNAMICS 1 Objectives Spontaneity
More informationconcentrations (molarity) rate constant, (k), depends on size, speed, kind of molecule, temperature, etc.
#80 Notes Ch. 12, 13, 16, 17 Rates, Equilibriums, Energies Ch. 12 I. Reaction Rates NO 2(g) + CO (g) NO (g) + CO 2(g) Rate is defined in terms of the rate of disappearance of one of the reactants, but
More informationChemical Thermodynamics. Chapter 18
Chemical Thermodynamics Chapter 18 Thermodynamics Spontaneous Processes Entropy and Second Law of Thermodynamics Entropy Changes Gibbs Free Energy Free Energy and Temperature Free Energy and Equilibrium
More informationChapter 19. Chemical Thermodynamics. Chemical Thermodynamics
Chapter 19 Enthalpy A thermodynamic quantity that equal to the internal energy of a system plus the product of its volume and pressure exerted on it by its surroundings; Enthalpy is the amount of energy
More informationCHEMpossible. Final Exam Review
CHEMpossible Final Exam Review 1. Given the following pair of reactions and their equilibrium constants: 2NO 2 (g) 2NO (g) + O 2 (g) K c = 15.5 2NO (g) + Cl 2 (g) 2 NOCl (g) K c = 3.20 10-3 Calculate a
More informationSecond law of thermodynamics
Second law of thermodynamics It is known from everyday life that nature does the most probable thing when nothing prevents that For example it rains at cool weather because the liquid phase has less energy
More informationChapter 16 - Spontaneity, Entropy, and Free Energy
Chapter 16 - Spontaneity, Entropy, and Free Energy 1 st Law of Thermodynamics - energy can be neither created nor destroyed. Although total energy is constant, the various forms of energy can be interchanged
More information(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
More informationClass XI Chapter 6 Thermodynamics Chemistry
Class XI Chapter 6 Chemistry Question 6.1: Choose the correct answer. A thermodynamic state function is a quantity (i) used to determine heat changes (ii) whose value is independent of path (iii) used
More information0. Graphite is thermodynamically less stable that diamond under standard conditions. 1. True 2. False
0. Graphite is thermodynamically less stable that diamond under standard conditions. 1. True 2. False 1. Which statement would be the best interpretation of the First Law of Thermodynamics? 1. The total
More informationChem. 1B Final Practice Test 2 Solutions
First letter of last name Chem. 1B Final Practice Test 2 Solutions Name Print Neatly. You will lose 1 point if I cannot read your name or perm number. Student Number If you are sitting next to someone
More informationCHEMICAL THERMODYNAMICS. Nature of Energy. ΔE = q + w. w = PΔV
CHEMICAL HERMODYNAMICS Nature of Energy hermodynamics hermochemistry Energy (E) Work (w) Heat (q) Some Definitions Study the transformation of energy from one form to another during physical and chemical
More informationA proposed mechanism for the decomposition of hydrogen peroxide by iodide ion is: slow fast (D) H 2 O
Chemistry 112, Spring 2007 Prof. Metz Exam 2 Practice Use the following information to answer questions 1 through 3 A proposed mechanism for the decomposition of hydrogen peroxide by iodide ion is: H 2
More informationChem 1B Dr. White 1 Chapter 17: Thermodynamics. Review From Chem 1A (Chapter 6, section 1) A. The First Law of Thermodynamics
Chem 1B Dr. White 1 Chapter 17: Thermodynamics Review From Chem 1A (Chapter 6, section 1) A. The First Law of Thermodynamics 17.1 Spontaneous Processes and Entropy A. Spontaneous Change Chem 1B Dr. White
More informationClass work on Calorimetry. January 11 and 12, 2011
Class work on Calorimetry January 11 and 12, 2011 Name 1. The number of calories needed to raise the temperature of 100 grams of water 10 degrees Celsius is the same as the number of calories needed to
More informationAP* 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,
More informationChemistry 112, Fall 2006, Section 1 (Garman and Heuck) Final Exam A (100 points) 19 Dec 2006
Chemistry 112, Fall 2006, Section 1 (Garman and Heuck) (100 points) 19 Dec 2006 Name: YOU MUST: Put your name and student ID on the bubble sheet correctly. Put the exam version on the bubble sheet on the
More informationSaturday Study Session 1 3 rd Class Student Handout Thermochemistry
Saturday Study Session 1 3 rd Class Student Handout Thermochemistry Multiple Choice Identify the choice that best completes the statement or answers the question. 1. C 2 H 4 (g) + 3 O 2 (g) 2 CO 2 (g)
More informationB 2 Fe(s) O 2(g) Fe 2 O 3 (s) H f = -824 kj mol 1 Iron reacts with oxygen to produce iron(iii) oxide as represented above. A 75.
1 2004 B 2 Fe(s) + 3 2 O 2(g) Fe 2 O 3 (s) H f = -824 kj mol 1 Iron reacts with oxygen to produce iron(iii) oxide as represented above. A 75.0 g sample of Fe(s) is mixed with 11.5 L of O 2 (g) at 2.66
More informationThis test is closed note/book. One 8.5 x 11 handwritten crib sheet (one sided) is permitted.
Exam3 TestFormA Chem1310 Fall2008 11/24/2008 Dr.Williams PrintName Signature This test is closed note/book. One 8.5 x 11 handwritten crib sheet (one sided) is permitted. Use a #2 pencil. Calculators are
More informationCHAPTER 12: Thermodynamics Why Chemical Reactions Happen
CHAPTER 12: Thermodynamics Why Chemical Reactions Happen Useful energy is being "degraded" in the form of unusable heat, light, etc. A tiny fraction of the sun's energy is used to produce complicated,
More informationEnergy Ability to produce change or do work. First Law of Thermodynamics. Heat (q) Quantity of thermal energy
THERMOCHEMISTRY Thermodynamics Study of energy and its interconversions Energy is TRANSFORMED in a chemical reaction (POTENTIAL to KINETIC) HEAT (energy transfer) is also usually produced or absorbed -SYSTEM:
More informationEnergy is the capacity to do work
1 of 10 After completing this chapter, you should, at a minimum, be able to do the following. This information can be found in my lecture notes for this and other chapters and also in your text. Correctly
More informationCHEMISTRY 202 Practice Hour Exam II. Dr. D. DeCoste T.A (60 pts.) 21 (40 pts.) 22 (20 pts.)
CHEMISTRY 202 Practice Hour Exam II Fall 2016 Dr. D. DeCoste Name Signature T.A. This exam contains 22 questions on 7 numbered pages. Check now to make sure you have a complete exam. You have two hours
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 informationEnergy Ability to produce change or do work. First Law of Thermodynamics. Heat (q) Quantity of thermal energy
THERMOCHEMISTRY Thermodynamics Study of energy and its interconversions Energy is TRANSFORMED in a chemical reaction (POTENTIAL to KINETIC) HEAT (energy transfer) is also usually produced or absorbed -SYSTEM:
More informationENTROPY HEAT HEAT FLOW. Enthalpy 3/24/16. Chemical Thermodynamics. Thermodynamics vs. Kinetics
Chemical Thermodynamics The chemistry that deals with energy exchange, entropy, and the spontaneity of a chemical process. HEAT The energy that flows into or out of system because of a difference in temperature
More informationThermodynamics. Thermodynamically favored reactions ( spontaneous ) Enthalpy Entropy Free energy
Thermodynamics Thermodynamically favored reactions ( spontaneous ) Enthalpy Entropy Free energy 1 Thermodynamically Favored Processes Water flows downhill. Sugar dissolves in coffee. Heat flows from hot
More informationCHE 107 Spring 2018 Exam 2
CHE 107 Spring 2018 Exam 2 Your Name: Your ID: Question #: 1 Which substance has the smallest standard molar entropy ( S)? A He(g) B H2O(g) C CH4(g) D F2(g) Question #: 2 Phosgene, a chemical weapon used
More informationThermodynamics. Thermodynamics of Chemical Reactions. Enthalpy change
Thermodynamics 1 st law (Cons of Energy) Deals with changes in energy Energy in chemical systems Total energy of an isolated system is constant Total energy = Potential energy + kinetic energy E p mgh
More informationFor more info visit
Basic Terminology: Terms System Open System Closed System Isolated system Surroundings Boundary State variables State Functions Intensive properties Extensive properties Process Isothermal process Isobaric
More informationThermodynamics II. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Thermodynamics II Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Spontaneous Physical and Chemical Processes A waterfall runs downhill A lump of sugar dissolves
More informationThermochemistry: the study of energy (in the from of heat) changes that accompany physical & chemical changes
Thermochemistry Thermochemistry: the study of energy (in the from of heat) changes that accompany physical & chemical changes heat flows from high to low (hot cool) endothermic reactions: absorb energy
More informationCHM 111 Dr. Kevin Moore
CHM 111 Dr. Kevin Moore Kinetic Energy Energy of motion E k 1 2 mv 2 Potential Energy Energy of position (stored) Law of Conservation of Energy Energy cannot be created or destroyed; it can only be converted
More informationEntropy. Spontaneity. Entropy. Entropy mol of N 2 at 1 atm or 1 mol of N 2 at atm. process a process that occurs without intervention
Entropy Spontaneity process a process that occurs without intervention can be fast or slow Entropy (s) the measure of molecular randomness or disorder Think of entropy as the amount of chaos Entropy Predict
More information(03) WMP/Jun10/CHEM4
Thermodynamics 3 Section A Answer all questions in the spaces provided. 1 A reaction mechanism is a series of steps by which an overall reaction may proceed. The reactions occurring in these steps may
More informationChem 1310 A/B 2005, Professor Williams Practice Exam 3 (chapters 10, 11 and 12) Chapter 10 Thermochemistry
Chem 1310 A/B 2005, Professor Williams Practice Exam 3 (chapters 10, 11 and 12) Chapter 10 Thermochemistry 1. The heat capacity (C P ) is related to the heat absorbed at constant pressure (q P ) and the
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 informationChapter 19 Chemical Thermodynamics Entropy and free energy
Chapter 19 Chemical Thermodynamics Entropy and free energy Learning goals and key skills: Explain and apply the terms spontaneous process, reversible process, irreversible process, and isothermal process.
More information3/30/2017. Section 17.1 Spontaneous Processes and Entropy Thermodynamics vs. Kinetics. Chapter 17. Spontaneity, Entropy, and Free Energy
Chapter 17 Spontaneity, Entropy, and Thermodynamics vs. Kinetics Domain of Kinetics Rate of a reaction depends on the pathway from reactants to products. Thermodynamics tells us whether a reaction is spontaneous
More informationBCIT Fall Chem Exam #2
BCI Fall 2016 Chem 3310 Exam #2 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 informationCHM 152 Exam 4 Review Ch KEY
CHM 152 Exam 4 Review Ch. 18 19 KEY 1. Predict whether the entropy change will be positive or negative for the following: a. H 2 O (g) H 2 O (l) S - b. C 6 H 12 O 6 (s) 2C 2 H 5 OH(l) + 2CO 2 (g) S +_
More information7. a. A spontaneous process is one that occurs without any outside intervention.
CHAPTER SIXTEEN SPONTANEITY, ENTROPY, AND FREE ENERGY Questions 7. a. A spontaneous process is one that occurs without any outside intervention. b. Entropy is a measure of disorder or randomness. c. The
More informationCHEMISTRY 202 Hour Exam II. Dr. D. DeCoste T.A (60 pts.) 31 (20 pts.) 32 (40 pts.)
CHEMISTRY 202 Hour Exam II October 27, 2015 Dr. D. DeCoste Name Signature T.A. This exam contains 32 questions on 11 numbered pages. Check now to make sure you have a complete exam. You have two hours
More informationMcCord CH301 Exam 5 Dec 5, 2017
425 version last name first name signature McCord CH301 Exam 5 Dec 5, 2017 50070 BUR 106 Tuesday TTh 9:30 am - 11 pm Remember to refer to the Periodic Table handout that is separate from this exam copy.
More informationAP* Chemistry Spontaneity: Entropy and Free Energy
WHAT DRIVES A REACTION TO BE SPONTANEOUS? AP* Chemistry Spontaneity: Entropy and Free Energy Dr. Valverde s AP Chemistry Class Chapter 17 Review: Spontaneity, Entropy, and Free Energy (1) ENTHALPY ( H)
More informationENTHALPY, ENTROPY AND FREE ENERGY CHANGES
ENTHALPY, ENTROPY AND FREE ENERGY CHANGES Refer to the following figures for Exercises 1-6. The lines on the vertical axis represent the allowed energies. Assume constant spacing between levels to determine
More information1 A reaction that is spontaneous.
Slide 1 / 55 1 A reaction that is spontaneous. A B C D E is very rapid will proceed without outside intervention is also spontaneous in the reverse direction has an equilibrium position that lies far to
More informationOAT General Chemistry Problem Drill 15: Thermochemistry & Thermodynamics
OAT General Chemistry Problem Drill 15: Thermochemistry & Thermodynamics Question No. 1 of 10 1. A metal with a high heat capacity is put on a hot plate. What will happen? Question #01 (A) The temperature
More informationAdvanced Chemistry Practice Problems
Thermodynamics: Review of Thermochemistry 1. Question: What is the sign of DH for an exothermic reaction? An endothermic reaction? Answer: ΔH is negative for an exothermic reaction and positive for an
More informationMCAT General Chemistry Discrete Question Set 19: Thermochemistry & Thermodynamics
MCAT General Chemistry Discrete Question Set 19: Thermochemistry & Thermodynamics Question No. 1 of 10 1: A metal with a high heat capacity is put on a hot plate. What will happen? Question #01 A. The
More informationChemistry 112, Spring 2007 Prof. Metz Exam 2 Solutions April 5, 2007 Each question is worth 5 points, unless otherwise indicated
Chemistry 11, Spring 007 Prof. Metz Exam Solutions April 5, 007 Each question is worth 5 points, unless otherwise indicated 1. A proposed mechanism for the reaction of NO with Br to give BrNO is NO + NO
More informationHomework 11 - Second Law & Free Energy
HW11 - Second Law & Free Energy Started: Nov 1 at 9:0am Quiz Instructions Homework 11 - Second Law & Free Energy Question 1 In order for an endothermic reaction to be spontaneous, endothermic reactions
More informationExam 3, Ch 7, 19, 14 November 9, Points
Chem 30 Name Exam 3, Ch 7, 9, 4 November 9, 206 00 Points Please follow the instructions for each section of the exam. Show your work on all mathematical problems. Provide answers with the correct units
More informationChapter 15 Equilibrium
Chapter 15. Chemical Equilibrium Sample Exercise 15.1 (p. 632) Write the equilibrium expression for K eq for these three reactions: a) 2 O 3(g) 3 O 2(g) b) 2 NO (g) + Cl 2(g) 2 NOCl (g) c) Ag + (aq) +
More informationCHEMISTRY 102 FALL 2009 EXAM 2 FORM B SECTION 501 DR. KEENEY-KENNICUTT PART 1
NAME CHEMISTRY 102 FALL 2009 EXAM 2 FORM B SECTION 501 DR. KEENEY-KENNICUTT Directions: (1) Put your name on PART 1 and your name and signature on PART 2 of the exam where indicated. (2) Sign the Aggie
More informationThermodynamics C Test
Northern Regional: January 19 th, 2019 Thermodynamics C Test Name(s): Team Name: School Name: Team Number: Rank: Score: Science Olympiad North Florida Regional at the University of Florida Thermodynamics
More informationSlide 1 / Objects can possess energy as: (a) endothermic energy (b) potential energy (c) kinetic energy. a only b only c only a and c b and c
Slide 1 / 84 1 Objects can possess energy as: (a) endothermic energy (b) potential energy (c) kinetic energy A B C D E a only b only c only a and c b and c Slide 2 / 84 2 The internal energy of a system
More informationChem 1A, Fall 2015, Midterm Exam 3. Version A November 17, 2015 (Prof. Head-Gordon) 2. Student ID: TA:
Chem 1A, Fall 2015, Midterm Exam 3. Version A November 17, 2015 (Prof. Head-Gordon) 2 Name: Student ID: TA: Contents: 6 pages A. Multiple choice (10 points) B. Thermochemistry and Equilibria (12 points)
More information2/18/2013. Spontaneity, Entropy & Free Energy Chapter 16. The Dependence of Free Energy on Pressure Sample Exercises
Spontaneity, Entropy & Free Energy Chapter 16 16.7 The Dependence of Free Energy on Pressure Why is free energy dependent on pressure? Isn t H, enthalpy independent of pressure at constant pressure? No
More informationThermodynamics part 2
Thermodynamics part 2 The thermodynamic standard state of a substance is its most stable pure form under standard pressure (one atmosphere) and at some specific temperature (25 C or 298 K unless otherwise
More informationChapter 17: Spontaneity, Entropy, and Free Energy
Chapter 17: Spontaneity, Entropy, and Free Energy Review of Chemical Thermodynamics System: the matter of interest Surroundings: everything in the universe which is not part of the system Closed System:
More information1. Read all questions thoroughly and answer each question completely. ALL WORK MUST BE SHOWN IN ORDER TO RECEIVE ANY CREDIT.
INSTRUCTIONS: 1. Read all questions thoroughly and answer each question completely. ALL WORK MUST BE SHOWN IN ORDER TO RECEIVE ANY CREDIT. 2. You will be allowed to use only the given sheet of thermodynamic
More informationCollision Theory. Unit 12: Chapter 18. Reaction Rates. Activation Energy. Reversible Reactions. Reversible Reactions. Reaction Rates and Equilibrium
Collision Theory For reactions to occur collisions between particles must have Unit 12: Chapter 18 Reaction Rates and Equilibrium the proper orientation enough kinetic energy See Both In Action 1 2 Activation
More informationFACULTY OF SCIENCE MID-TERM EXAMINATION 2 MARCH 18, :30 TO 8:30 PM CHEMISTRY 120 GENERAL CHEMISTRY
FACULTY OF SCIENCE MID-TERM EXAMINATION 2 MARCH 18, 2011. 6:30 TO 8:30 PM CHEMISTRY 120 GENERAL CHEMISTRY Examiners: Prof. B. Siwick Prof. A. Mittermaier Dr. A. Fenster Name: Associate Examiner: A. Fenster
More informationCh 10 Practice Problems
Ch 10 Practice Problems 1. Which of the following result(s) in an increase in the entropy of the system? I. (See diagram.) II. Br 2(g) Br 2(l) III. NaBr(s) Na + (aq) + Br (aq) IV. O 2(298 K) O 2(373 K)
More informationOCR 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
More informationMCGILL UNIVERSITY FACULTY OF SCIENCE MIDTERM EXAMINATION CHEM 120 MONDAY MARCH 16, :30PM 8:30PM VERSION NUMBER: 1
MCGILL UNIVERSITY FACULTY OF SCIENCE MIDTERM EXAMINATION CHEM 120 MONDAY MARCH 16, 2009 6:30PM 8:30PM VERSION NUMBER: 1 Instructions: BEFORE YOU BEGIN: Enter your student number and name on the computer
More informationCh 17 Free Energy and Thermodynamics - Spontaneity of Reaction
Ch 17 Free Energy and Thermodynamics - Spontaneity of Reaction Modified by Dr. Cheng-Yu Lai spontaneous nonspontaneous Spontaneous Processes Processes that are spontaneous in one direction are nonspontaneous
More informationChapter 17. Free Energy and Thermodynamics. Chapter 17 Lecture Lecture Presentation. Sherril Soman Grand Valley State University
Chapter 17 Lecture Lecture Presentation Chapter 17 Free Energy and Thermodynamics Sherril Soman Grand Valley State University First Law of Thermodynamics You can t win! The first law of thermodynamics
More informationGibbs Free Energy. Evaluating spontaneity
Gibbs Free Energy Evaluating spontaneity Predicting Spontaneity An increase in entropy; Changing from a more structured to less structured physical state: Solid to liquid Liquid to gas Increase in temperature
More informationAP* Chemistry Entropy and Free Energy
AP* Chemistry Entropy and Free Energy WHAT DRIVES A REACTION TO BE THERMODYNAMICALLY FAVORABLE? ENTHALPY ( H) heat exchange (exothermic reactions are generally favored) ENTROPY ( S) dispersal (disorder)
More informationThermodynamics. 1. Which of the following processes causes an entropy decrease?
Thermodynamics 1. Which of the following processes causes an entropy decrease? A. boiling water to form steam B. dissolution of solid KCl in water C. mixing of two gases in one container D. beach erosion
More informationCHEM J-14 June 2014
CHEM1101 2014-J-14 June 2014 An electrochemical cell consists of an Fe 2+ /Fe half cell with unknown [Fe 2+ ] and a Sn 2+ /Sn half-cell with [Sn 2+ ] = 1.10 M. The electromotive force (electrical potential)
More informationThermodynamics- 1) Hess's law states that 1) The standard enthalpy of an overall reaction is the sum of the enthalpy changes in individual reaction. ) Enthalpy of formation of compound is same as the enthalpy
More informationTHERMODYNAMICS I. TERMS AND DEFINITIONS A. Review of Definitions 1. Thermodynamics = Study of the exchange of heat, energy and work between a system
THERMODYNAMICS I. TERMS AND DEFINITIONS A. Review of Definitions 1. Thermodynamics = Study of the exchange of heat, energy and work between a system and its surroundings. a. System = That part of universe
More information4/19/2016. Chapter 17 Free Energy and Thermodynamics. First Law of Thermodynamics. First Law of Thermodynamics. The Energy Tax.
Chemistry: A Molecular Approach, 2nd Ed. Nivaldo Tro First Law of Thermodynamics Chapter 17 Free Energy and Thermodynamics You can t win! First Law of Thermodynamics: Energy cannot be created or destroyed
More information