WORKSHEET #1. Dougherty Valley HS AP Chemistry Hess s Law Problems
|
|
- Emory Dennis
- 6 years ago
- Views:
Transcription
1 Dougherty Valley HS AP Chemistry Hess s Law Problems WORKSHEET #1 1. Calculate the standard enthalpy change, ΔH o, for the formation of 1 mol of strontium carbonate (the material that gives the red color in fireworks) from its elements. ( 10 KJ) Sr (s) Theinformation available is (1) () () Sr (s) SrO (s) C(graphite) 1 C(graphite) O O O SrO (s) Sr (s) Sr (s) H H H - 59 kj - kj - 9 kj. The combination of coke and steam produces a mixture called coal gas, which can be used as a fuel or as a starting material for other reactions. If we assume coke can be represented by graphite, the equation for the production of coal gas is (+ 15. kj) C (s) Determine thestandard enthalpy change for this reaction from the following standard enthalpies of reaction : (1) () () C(s) CH The next one is challenging! H O H O HO H O CH H H H. One reaction involved in the conversion of iron ore to the metal is ( 11 kj) FeO (s) (1) Fe O (s) () Fe O (s) of iron oxides with : Fe(s) Fe O Fe(s) FeO (s) (s) H H H 11. kj - 1. kj 06.1 kj Calculate thestandard enthalpy change for this reaction from these reactions () Fe O (s) H H H - 7 kj - 5 kj 19 kj
2 [] Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values: PCl 5 PCl + Cl P (s) + 6Cl PCl PCl 5 P (s) + 10Cl Answer = 9.8 kj ΔH = 9 kj ΔH = 8 kj [5] Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values: + H O C H + O C H + H C H 6 H O H + O C H 6 + O + H O Answer = 5 kj ΔH = 9.5 kj ΔH = 71. kj ΔH = 8 kj [6] Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values: N H (l) + H NH N H (l) + CH O(l) CH O + N + H N + H NH CH O(l) CH O + H Answer = 18 kj ΔH = 7 kj ΔH = 6 kj ΔH = 65 kj [7] Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values: H SO (l) SO + H O H S + O H SO (l) H S + O SO + H O(l) H O(l) H O Answer = 7 kj ΔH = 5.5 kj ΔH = 07 kj ΔH = kj [8] Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values: C H O(l) + H O(l) C H 6 O(l) + O C H 6 O(l) + O + H O(l) C H O(l) + O + H O(l) Answer = 0.0 kj ΔH = kj ΔH = 58.5 kj [9] Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values: N + O NO N + H NH NH + H O(l) NO + 7H H O(l) H + O Answer = 8 kj ΔH = 115 kj ΔH = 1.5 kj ΔH =.7 kj [10] Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values: C(s) + O H O(l) H + O C H 6 C(s) + H + H O(l) C H 6 + O Answer = 886 kj ΔH = 6 kj ΔH = kj ΔH = kj
3 [11] Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values: N H (l) + CH O(l) CH O + N + H NH N H (l) + H NH N + H CH O + H CH O(l) Answer = 6. kj ΔH =.5 kj ΔH = 57.5 kj ΔH = 81. kj [1] Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values: H + Cl HCl Cl + H O(l) CH Cl (l) + O HCl + O H O(l) + Cl CH Cl (l) + H + O Cl + H O(l) Answer = 0 kj ΔH = 7.5 kj ΔH = 105 kj ΔH = 0.5 kj [1] Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values: C H + O + H O C H 6 C H + H H + O H O + H O C H 6 + O Answer = 705 kj ΔH = 8.5 kj ΔH = 1.7 kj ΔH = 89 kj [1] Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values: HCl + NaNO (s) HNO (l) + NaCl(s) NaCl(s) + H O(l) HCl + Na O(s) NO + NO + Na O(s) NaNO (s) NO + NO N O + O HNO (l) N O + O + H O(l) Answer = 78 kj ΔH = 507 kj ΔH = 7 kj ΔH = kj ΔH = kj [15] Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values: Zn(s) + S 8 (s) + O ZnSO (s) Zn(s) + S 8 (s) ZnS(s) ZnS(s) + O ZnO(s) + SO SO + O SO ZnO(s) + SO ZnSO (s) Answer = kj ΔH = 18.9 kj ΔH = 97.5 kj ΔH = kj ΔH = 0. kj These problems involve using heat of formation values that are found in the appendix of your textbook. [16] What is the enthalpy of the following reactions? Use equation from Equation Sheet [Products minus reactants] (a) SiF Si(s) + F (b) SiF Si + F (c) SO + H O H SO (aq) (d) K O (s) + H O(l) 6KOH(aq) + O (e) Fe O (s) + 8HCl FeCl (s) + FeCl (s) + H O SiF - H f = KJ/mol FeCl - H f = 1.8 KJ/mol FeCl - H f = 99.5 KJ/mol Fe O - H f = KJ/mol SO - H f = 5.5 KJ/mol Si - H f = 50 KJ/mol
4 Dougherty Valley HS AP Chemistry Enthalpies of Formation Practice WORKSHEET # Directions: use your textbooks appendix to calculate the standard enthalpy change for each of the following reactions using heats of formation. Must show all work to receive credit. These are from another textbook, H f values may be a bit different. (5.71) [1] SO + O SO (196.6 kj) [] Mg(OH) (s) MgO(s) + H O(l) (7.1 kj) [] N O + H N + H O (976.9 kj) [] SiCl (l) + H O(l) SiO (s) + HCl (68. kj) (5.7) [5] HBr + O H O(l) + Br (l) (6.7 kj) [6] NaOH(s) + SO Na SO (s) + H O (8.5 kj) [7] CH + Cl CCl (l) + HCl (.7 kj) [8] Fe O (s) + HCl FeCl (s) + H O (150 kj)
5 PRACTICE TEST/THERMOCHEMISTRY/AP CHEMISTRY 1. a) Calculate the amount of heat transferred when g of NO is formed by the following reaction: N + O NO ΔHrxn = +16. kj b) Draw an energy diagram for this process.. Predict the value for ΔH f for the following scenarios: a) Br b) Br(l) c) I d) I(s). Calculate the ΔHrxn for the following reaction: CH + O + HO(l) ΔH f CH = 6.6 kj/mol ΔH f = -9.5 kj/mol ΔH f HO(l) = kj/mol. A 5.00 g sample of liquid water at 5.0 C is heated by the addition of 8.0 J of energy. The final temperature of the water is C. The specific heat capacity of the liquid is.18 J/g C. a) -1 b).0 c) 5. d) 95. e) This problem was taken directly from the 1995 AP chem. exam. Propane is a hydrocarbon that is commonly used as a fuel for cooking. Propane s formula is CH8. a) Write a balanced equation for the complete combustion of propane gas. b) Calculate the volume of air at 0 C and 1.00 atm that is needed to burn completely 10.0 g of propane. Assume that air is 1.0% O by volume. c) The heat of combustion (ΔH combustion ) is -,0.1 kj/mol. Calculate the heat of formation, ΔH f, of propane given that ΔH f of HO(l) is -85. kj/mol and ΔH f of is -9.5 kj/mol. d) Assuming that all of the heat evolved burning 10.0 g propane is transferred to 8.00 kg of water (specific heat =.18 J/g C), calculate the increase in temperature of the water.
6 AP Chemistry Thermochem FRQs 00 00B. 006
7 005B Skip part (d) for now.
AP Chapter 6: Thermochemistry Name
AP Chapter 6: Thermochemistry Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. AP Chapter 6: Thermochemistry 2 Warm-Ups (Show your work for credit)
More informationCHEM 1105 S10 March 11 & 14, 2014
CHEM 1105 S10 March 11 & 14, 2014 Today s topics: Thermochemistry (Chapter 6) Basic definitions Calorimetry Enthalpy Thermochemical equations Calculating heats of reaction Hess s Law Energy and Heat Some
More informationLearning Check. How much heat, q, is required to raise the temperature of 1000 kg of iron and 1000 kg of water from 25 C to 75 C?
Learning Check q = c * m * ΔT How much heat, q, is required to raise the temperature of 1000 kg of iron and 1000 kg of water from 25 C to 75 C? (c water =4.184 J/ C g, c iron =0.450 J/ C g) q Fe = 0.450
More informationChemistry 30: Thermochemistry. Practice Problems
Name: Period: Chemistry 30: Thermochemistry Practice Problems Date: Heat and Temperature 1. Pretend you are doing a scientific study on the planet Earth. a. Name three things in the system you are studying.
More informationCHEM J-11 June /01(a)
CHEM1001 2014-J-11 June 2014 22/01(a) Combustion of 15.0 g of coal provided sufficient heat to increase the temperature of 7.5 kg of water from 286 K to 298 K. Calculate the amount of heat (in kj) absorbed
More informationGENERAL CHEMISTRY I CHEM SYSTEM FINAL EXAM VERSION A Fall 2016
GENERAL CHEMISTRY I CHEM 1411 SYSTEM FINAL EXAM VERSION A Fall 2016 Departmental Final Exam General Chemistry I, CHEM 1411 Fall 2016 VERSION A Part I: 35 Multiple Choice (2 pts each). Directions: Select
More informationName. Practice Test 2 Chemistry 111
Name Practice Test 2 Chemistry 111 1) In the aqueous reaction of K 2 SO 4 (aq) + Ba(NO 3 ) 2 (aq) BaSO 4 (s) + 2KNO 3 (aq), which ions are the spectator ions? A) Ba 2+ 2- and SO 4 B) Ba 2+ and K + C) Ba
More informationCH 221 Sample Exam Exam II Name: Lab Section:
Exam II Name: Lab Section: Part I: Multiple Choice Questions (100 Points) Use a scantron sheet for Part I. There is only one best answer for each question. 1. When methanol undergoes complete combustion,
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 informationChapter 19 Chemical Thermodynamics
Chapter 19. Chemical Thermodynamics Sample Exercise 19.2 (p. 819) Elemental mercury is a silver liquid at room temperature. Its normal freezing point is -38.9 o C, and its molar enthalpy of fusion is H
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 informationMUNISH KAKAR's INSTITUE OF CHEMISTRY
ENTHALPY CHANGE & HESS's LAW ( WS #4 ) Q1. H and E for the reaction, S(s) + 3 O(g) SO3(g) are related as: (a) H = E 0.5 RT (b) H = E 1.5RT (c) H = E + RT (d) H = E + 1.5 RT Q. The enthalpy of solution
More informationEnergy Relationships in Chemical Reactions
Energy Relationships in Chemical Reactions What is heat? What is a state function? What is enthalpy? Is enthalpy a state function? What does this mean? How can we calculate this? How are the methods the
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 informationThermodynamics I. Prep Session
Thermodynamics I Prep Session Dr. John I. Gelder Department of Chemistry Oklahoma State University Stillwater, OK 74078 john.gelder@okstate.edu http://intro.chem.okstate.edu 12/5/09 1 Thermo I Prep Session
More informationEnthalpy and Internal Energy
Enthalpy and Internal Energy H or ΔH is used to symbolize enthalpy. The mathematical expression of the First Law of Thermodynamics is: ΔE = q + w, where ΔE is the change in internal energy, q is heat and
More information(E) half as fast as methane.
Name AP Chem / / AP Chem Practice Exam #2 Part I: 40 Questions, 40 minutes, Multiple Choice, No Calculator Allowed Bubble the correct answer on the BLUE SIDE of your scantron for each of the following.
More informationUnit 13: Rates and Equilibrium- Funsheets
Name: Period: Unit 13: Rates and Equilibrium- Funsheets Part A: Reaction Diagrams 1) Answer the following questions based on the potential energy diagram shown here: a. Does the graph represent an endothermic
More informationLesmahagow High School
Lesmahagow High School Higher Chemistry Enthalpy - Tutorial Questions Energy Changes Tutorial Questions 1 1. A pupil found the enthalpy of combustion of propan-1-ol using the following apparatus: a. In
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 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 101 Fall 08 Exam III(a)
CHEM 101 Fall 08 Exam III(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 information8. Relax and do well.
CHEM 1314.05 Exam II John II. Gelder October 18, 1994 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 9 different pages. The last three pages include a periodic table,
More information47 people in recitation yesterday. Expect quizzes there and in class.
Announcements 47 people in recitation yesterday. Expect quizzes there and in class. Chapter 6 Problems: 6.9, 6.11, 6.13(except c), 6.19, 6.23, 6.34, 6.38, 6.42, 6.51, 6.53, 6.54, 6.57, 6.64, 6.66, 6.69,
More informationWorkbook 5. Chem 1A Dr. White 1
Chem 1A Dr. White 1 Workbook 5 5-1: Dalton s Law, KMT, Effusion/Diffusion/Real Gases 1. What is the total pressure and the partial pressure of each gas (in atm) in a mixture of 3.2 g of O 2, 1.6 g of CH
More information33. a. Heat is absorbed from the water (it gets colder) as KBr dissolves, so this is an endothermic process.
31. This is an endothermic reaction so heat must be absorbed in order to convert reactants into products. The high temperature environment of internal combustion engines provides the heat. 33. a. Heat
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 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 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 informationThermochemistry HW. PSI Chemistry
Thermochemistry HW PSI Chemistry Name Energy 1) Objects can possess energy as: (a) endothermic energy (b) potential energy A) a only B) b only C) c only D) a and c E) b and c (c) kinetic energy 2) The
More informationKwantlen Polytechnic University Chemistry 1105 S10 Spring Term Test No. 3 Thursday, April 4, 2013
Kwantlen Polytechnic University Chemistry 1105 S10 Spring Term Test No. 3 Thursday, April 4, 2013 Name: Student Number Instructions: Ensure that this exam contains all eight pages including this page.
More information1. How many protons, electrons, and neutrons are in one atom of the following isotopes (6 points)?
Chemistry 11 Department of Physical Sciences Kingsborough Community College City University of New York NAME Exam 1: Chapters 1-3 50 points 1. How many protons, electrons, and neutrons are in one atom
More informationChemical Reactions Unit
Name: Hour: Teacher: ROZEMA / Chemistry Chemical Reactions Unit 1 P a g e 2 P a g e 3 P a g e 4 P a g e 5 P a g e 6 P a g e Chemistry Balancing Equations Balance the following equations by inserting the
More informationTHERMOCHEMISTRY & DEFINITIONS
THERMOCHEMISTRY & DEFINITIONS Thermochemistry is the study of the study of relationships between chemistry and energy. All chemical changes and many physical changes involve exchange of energy with the
More information10/23/10. Thermodynamics and Kinetics. Chemical Hand Warmers
10/23/10 CHAPTER 6 Thermochemistry 6-1 Chemical Hand Warmers Most hand warmers work by using the heat released from the slow oxidation of iron 4 Fe(s) + 3 O2(g) 2 Fe2O3(s) The amount your hand temperature
More informationCHEM3.4 Demonstrate understanding of thermochemical principles and the properties of particles and substances
CHEM3.4 Demonstrate understanding of thermochemical principles and the properties of particles and substances We have covered the underlined part so far. This is: Electron configurations with s, p, d orbitals
More informationCHAPTER SIX THERMOCHEMISTRY. Questions
CHAPTER SIX Questions 9. A coee-cup calorimeter is at constant (atmospheric) pressure. The heat released or gained at constant pressure is H. A bomb calorimeter is at constant volume. The heat released
More informationEnthalpy changes practice qs
Enthalpy changes practice qs Q1. The combustion of hydrocarbons is an important source of energy. Define the term standard enthalpy of combustion. (i) Write an equation for the complete combustion of ethane,
More informationChapter 6 Review. Part 1: Change in Internal Energy
Chapter 6 Review This is my own personal review, this should not be the only thing used to study. You should also study using notes, PowerPoint, homework, ect. I have not seen the exam, so I cannot say
More information8. Relax and do well.
CHEM 34.02 and 34.03 Name Exam III John III. Gelder TA's Name November 5, 2000 Lab Section INSTRUCTIONS:. This examination consists of a total of 9 different pages. The last three pages include a periodic
More informationQuestions 1 13 cover material from Exam 1
Questions 1 13 cover material from Exam 1 1. Which intermolecular forces are present in H Te(l)? A. dispersion only C. dispersion, dipole-dipole, and hydrogen bonding B. dispersion and dipole-dipole D.
More information10 Enthalpy changes Answers to Activity and Practice questions
Page 150 151 Activity: Measuring the enthalpy change for the reaction of zinc with copper sulfate solution 1 The graph should have: axes with scales and labels points plotted accurately a clean, smooth
More information8. Relax and do well.
CHEM 1314 Name Exam IV TA Name John IV. Gelder December 14, 1992 Lab Section INSTRUCTIONS: 1. This examination consists of a total of 9 different pages. The last three pages includes a periodic table and
More information8. Relax and do well.
CHEM 1314.03 Exam II John II. Gelder October 23, 1997 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 9 different pages. The last four pages include a periodic table,
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 informationName Date Class CHEMICAL REACTIONS. SECTION 11.1 DESCRIBING CHEMICAL REACTIONS (pages )
Name Date Class 11 CHEMICAL REACTIONS SECTION 11.1 DESCRIBING CHEMICAL REACTIONS (pages 321 329) This section explains how to write equations describing chemical reactions using appropriate symbols. It
More information5/14/14. How can you measure the amount of heat released when a match burns?
CHEMISTRY & YOU Chapter 7 Thermochemistry How can you measure the amount of heat released when a match burns? 7. The Flow of Energy 7.3 Heat in Changes of State 7.4 Calculating Heats of Reaction Remember:
More informationName: Date: M O L A R M A S S & P E R C E N T C O M P O S I T I O N
Name: Date: M O L A R M A S S & P E R C E N T C O M P O S I T I O N I. Molar Masses Given a periodic table, you should be able to calculate the molecular mass (in amu s) or the molar mass (in grams) for
More informationDo now: Write equations for the following expressions:
Do now: Write equations for the following expressions: ½ N 2(g) + 1 ½ H 2(g) NH 3(g) Δ f H (NH 3(g) ) = -46 kj.mol -1 ½ H 2(g) + ½ Cl 2(g) HCl (g) Δ f H (HCl (g) ) = -92 kj.mol -1 ½ N 2(g) + 2 H 2(g) +
More information(for tutoring, homework help, or help with online classes) 1.
www.tutor-homework.com (for tutoring, homework help, or help with online classes) 1. 2. Consider the following processes used to produce energy. Which does not predominantly use potential energy? 1. Fossil
More informationStoichiometric Calculations
Slide 1 / 109 Slide 2 / 109 Stoichiometric Calculations Slide 3 / 109 Slide 4 / 109 Table of Contents Stoichiometry Calculations with Moles Click on the topic to go to that section Stoichiometry Calculations
More informationUnit 5: Chemical Equations and Reactions & Stoichiometry
pg. 10 Unit 5: Chemical Equations and Reactions & Stoichiometry Chapter 8: Chemical Equations and Reactions 8.1: Describing Chemical Reactions Selected Chemistry Assignment Answers (Section Review on pg.
More informationExothermic process is any process that gives off heat transfers thermal energy from the system to the surroundings. H 2 O (l) + energy
Exothermic process is any process that gives off heat transfers thermal energy from the system to the surroundings. H 2 O (g) H 2 O (l) + energy Endothermic process is any process in which heat has to
More informationChapter 6 Thermochemistry
Chapter 6 Thermochemistry Contents and Concepts Understanding Heats of Reaction The first part of the chapter lays the groundwork for understanding what we mean by heats of reaction. 1. Energy and Its
More information5.1 Exothermic and endothermic reactions
Topic 5: Energetics 5.1 Exothermic and endothermic reactions Chemical reactions involve the breaking and making of bonds. Breaking bonds requires energy,whereas energy is given out when new bonds are formed.
More informationStoichiometric Calculations
Slide 1 / 109 Slide 2 / 109 Stoichiometric Calculations Slide 3 / 109 Table of Contents Click on the topic to go to that section Stoichiometry Calculations with Moles Stoichiometry Calculations with Particles
More informationThermochemistry: Energy Flow and Chemical Reactions
Thermochemistry: Energy Flow and Chemical Reactions Outline thermodynamics internal energy definition, first law enthalpy definition, energy diagrams, calorimetry, theoretical calculation (heats of formation
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 informationAP Questions: Thermodynamics
AP Questions: Thermodynamics 1970 Consider the first ionization of sulfurous acid: H2SO3(aq) H + (aq) + HSO3 - (aq) Certain related thermodynamic data are provided below: H2SO3(aq) H + (aq) HSO3 - (aq)
More informationProblem Set III Stoichiometry - Solutions
Chem 121 Problem set III Solutions - 1 Problem Set III Stoichiometry - Solutions 1. 2. 3. molecular mass of ethane = 2(12.011) + 6(1.008) = 30.07 g 4. molecular mass of aniline = 6(12.011) + 7(1.008) +
More informationSection 7.2: Equilibrium Law and the Equilibrium Constant Tutorial 1 Practice, page (a) 2 CO 2 (g) #!!"
Section 7.: Equilibrium Law and the Equilibrium Constant Tutorial Practice, page 4. (a) CO (g) #!!"! CO(g) + O (g) Products: CO(g); O (g) Reactant: CO (g) [CO [O Equilibrium law equation: [CO (b) Cl (g)
More informationStudy Guide Chapter 5
Directions: Answer the following 1. When writing a complete ionic equation, a. what types of substances should be shown as dissociated/ionized? soluble ionic compounds, acids, bases b. What types of substances
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 information26. N 2 + H 2 NH N 2 + O 2 N 2 O 28. CO 2 + H 2 O C 6 H 12 O 6 + O SiCl 4 + H 2 O H 4 SiO 4 + HCl 30. H 3 PO 4 H 4 P 2 O 7 + H 2 O
Balance the following chemical equations: (Some may already be balanced.) 1. H 2 + O 2 H 2 O 2. S 8 + O 2 SO 3 3. HgO Hg + O 2 4. Zn + HCl ZnCl 2 + H 2 5. Na + H 2 O NaOH + H 2 6. C 10 H 16 + Cl 2 C +
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 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 informationThermodynamics. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Thermodynamics Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Thermodynamics is the scientific study of the interconversion of heat and other kinds of energy.
More informationName Date Class SECTION 16.1 PROPERTIES OF SOLUTIONS
SOLUTIONS Practice Problems In your notebook, solve the following problems. SECTION 16.1 PROPERTIES OF SOLUTIONS 1. The solubility of CO 2 in water at 1.22 atm is 0.54 g/l. What is the solubility of carbon
More informationChapter 6: Thermochemistry
Chem 1045 General Chemistry by Ebbing and Gammon, 8th Edition George W.J. Kenney, Jr Last Update: 24-Oct-2008 Chapter 6: Thermochemistry These Notes are to SUPPLIMENT the Text, They do NOT Replace reading
More informationSolution: 1) Energy lost by the hot water: q = m C p ΔT. q = (72.55 g) (4.184 J/g 1 C 1 ) (24.3 C) q = J. 2) Energy gained by the cold water:
A calorimeter is to be calibrated: 72.55 g of water at 71.6 C added to a calorimeter containing 58.85 g of water at 22.4 C. After stirring and waiting for the system to equilibrate, the final temperature
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 informationGeneral Chemistry Study Guide
General Chemistry 1311 Study Guide Name : Louise K number: Date: Oct 02006 Instructor: Jingbo Louise Liu kfjll00@tamuk.edu 1 Chapter 04 & 05 (10 questions required and 5 questions for extra credit) Credited
More informationName Chem 161, Section: Group Number: ALE 27. Hess s Law. (Reference: Chapter 6 - Silberberg 5 th edition)
Name Chem 161, Section: Group Number: ALE 27. Hess s Law (Reference: Chapter 6 - Silberberg 5 th edition) Important!! For answers that involve a calculation you must show your work neatly using dimensional
More informationThe chemical potential energy of a substance is known as its ENTHALPY and has the symbol H.
Enthalpy Changes The chemical potential energy of a substance is known as its ENTHALPY and has the symbol H. During chemical reactions, the enthalpy can increase or decrease. The change in enthalpy during
More informationEquation (4) has 2 mol of water on the reactant side, while the desired equation has 6 mol. Multiply equation (4) and its ΔH by the factor 3:
Section 5.4: Hess s Law Tutorial 1 Practice, page 317 1. (a) Solution: The desired equation is: 2 N 2 (g) + 6 H 2 O(g) 3 O 2 (g) + 4 NH 3 (g) (1) NH 3 (g) 1 2 N 2(g) + 3 2 H 2(g) H = 46 kj (2) 2 H 2 (g)
More informationCHAPTER 16 REVIEW. Reaction Energy. SHORT ANSWER Answer the following questions in the space provided.
CHAPTER 16 REVIEW Reaction Energy SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. For elements in their standard state, the value of H 0 f is 0. 2. The formation and decomposition
More information6. Place the following elements in order of increasing atomic radii: Mg, Na, Rb, Cl.
CH141 Practice Problems/Practice Final Exam Page 1 of 12 Name: 1. What is the SO 4 2- concentration of a solution prepared by dissolving 3.00 g of Na 2 SO 4 in 1.00 L of water? 2. What is the hybridization
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 informationChapter 8 Thermochemistry: Chemical Energy
Chapter 8 Thermochemistry: Chemical Energy 國防醫學院生化學科王明芳老師 2011-11-8 & 2011-11-15 Chapter 8/1 Energy and Its Conservation Conservation of Energy Law: Energy cannot be created or destroyed; it can only be
More informationCHEM1901/ J-8 June 2013
CHEM1901/3 2013-J-8 June 2013 The atmosphere of Venus contains 96.5 % CO 2 at 95 atm of pressure, leading to an average global surface temperature of 462 C. The energy density of solar radiation striking
More informationThermochemistry Notes
Name: Thermochemistry Notes I. Thermochemistry deals with the changes in energy that accompany a chemical reaction. Energy is measured in a quantity called enthalpy, represented as H. The change in energy
More information(02) WMP/Jun10/CHEM2
Energetics 2 Section A Answer all the questions in the spaces provided. 1 An equation for the equilibrium reaction between hydrogen, iodine and hydrogen iodide is shown below. H 2 (g) + I 2 (g) 2HI(g)
More informationChemistry 1A Fall Midterm Exam 3
Chemistry 1A Fall 2017 Name Student ID Midterm Exam 3 You will have 120 minutes to complete this exam. Please fill in the bubble that corresponds to the correct answer on the answer sheet. Only your answer
More informationThermodynamics- Chapter 19 Schedule and Notes
Thermodynamics- Chapter 19 Schedule and Notes Date Topics Video cast DUE Assignment during class time One Review of thermodynamics ONE and TWO Review of thermo Wksheet Two 19.1-4; state function THREE
More informationChem 115 POGIL Worksheet - Week 8 - Answers Thermochemistry (Continued), Electromagnetic Radiation, and Line Spectra. ΔH o = 285.
Chem 115 POGIL Worksheet - Week 8 - Answers Thermochemistry (Continued), Electromagnetic Radiation, and Line Spectra Key Questions & Exercises 1. Calculate ΔH o for the reaction, Given: C 2 H 2 (g) + H
More informationBrown, LeMay Ch 5 AP Chemistry Monta Vista High School
Brown, LeMay Ch 5 AP Chemistry Monta Vista High School 1 From Greek therme (heat); study of energy changes in chemical reactions Energy: capacity do work or transfer heat Joules (J), kilo joules (kj) or
More informationDISCLAIMER: This review is not meant to replace studying, it should be done for extra practice. Everything on here may or may not be on the final
NAMING COMPOUNDS (COVALENT/IONIC) Covalent: (prefix except Mono-) Name of first element + (prefix)root of Second Element(-ide) Example: CO 2 : Carbon Dioxide CO: Carbon Monoxide C 2F 6: Dicarbon Hexafluoride
More informationCHEMISTRY 15 EXAM II-Version A (White)
CHEMISTRY 15 EXAM II-Version A (White) Dr. M. Richards-Babb June 8, 2001 An optical scoring machine will grade this examination. The machine is not programmed to accept the correct one of two sensed answers
More informationCHEMISTRY Practice Exam #2
CHEMISTRY 1710 - Practice Exam #2 Section 1 - This section of the exam is multiple choice. Choose the BEST answer from the choices which are given. 1. Which of the following solutions will have the highest
More informationb) Na 2 S(aq) + ZnCl 2 (aq) ZnS(s) + 2 NaCl(s)
Chem 111 2010 Name: Vining Exam #2, Version 23 1. Which of the following compounds are soluble in water: K 2 CO 3, CaCO 3, NiCO 3, and Fe 2 (CO 3 ) 3? a) K 2 CO 3 only b) K 2 CO 3 and CaCO 3 c) CaCO 3
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 informationChapter 5. Thermochemistry
Chapter 5 Thermochemistry Dr. A. Al-Saadi 1 Preview Introduction to thermochemistry: Potential energy and kinetic energy. Chemical energy. Internal energy, work and heat. Exothermic vs. endothermic reactions.
More informationmeasure ΔT in water to get q = q surroundings and use q system = q surroundings
example using water: Calculate the amount of energy required to heat 95.0 g of water from 22.5 C to 95.5 C. q = s m ΔT ( C (4.184 J g 1 C 1 ) (95.0 g) (73.0 = = 2.90 x 10 4 J or 29.0 kj Constant Pressure
More informationChem 101 General Chemistry Practice Final Exam
Name h = 6.626 x 10-34 J s (Planck s Constant) c = 3.00 x 10 8 m/s (speed of light) R H = 1.097 x 10-7 m -1 (Rydberg Constant) Chem 101 General Chemistry Practice Final Exam Multiple Choice (5 points each)
More informationChapter 6. Thermochemistry
Chapter 6. Thermochemistry 1 1. Terms to Know: thermodynamics thermochemistry energy kinetic energy potential energy heat heat vs. temperature work work of expanding gases work of expanding gases under
More informationExperiment 2 Heat of Combustion: Magnesium
Experiment 2 Heat of Combustion: Magnesium Purpose Hess s Law states that when are going from a particular set of reactants to a particular set of products, the heat of reaction is the same whether the
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 informationBalancing Equations Notes
. Unit 9 Chemical Equations and Reactions What is a Chemical Equation? A Chemical Equation is a written representation of the process that occurs in a chemical reaction. A chemical equation is written
More information