CHEMISTRY 3310 PROBLEM SHEET #4
|
|
- Louise O’Connor’
- 1 years ago
- Views:
Transcription
1 CHEMISTRY 3310 PROBLEM SHEET #4 1. The specific heats of a number of materials are listed below. Calculate the molar heat capacity for each. (a) gold, (b) rust (Fe 2 O 3 ) (c) sodium chloride 2. Calculate the final temperature that results from each of the following processes. (a) A 8.82 g sample of water at 20.3 C absorbs 112 calories of heat. (b) A 6.25 kg sample of solid sulfur at 45.3 C gives off 165 kcal of heat. 3. What is the quantity of work performed in the expansion of the gas that is confined in a pistoncylinder configuration if the mass of the piston is 500. g and a height of 16.8 cm is lifted? 4. Derive the expressions for the pressure volume work involved in the following processes: (a) any process which occurs with no change in volume, (b) expansion of an ideal gas into a vacuum, (c) any process occurring with a constant external pressure, (d) expansion of an ideal case during which the temperature is held constant and the external pressure is constantly adjusted to match the pressure while the gas itself exerts. 5. The combustion of benzoic acid is often used to establish the heat capacity of a bomb calorimeter. If the combustion of a g sample of benzoic acid (HC 7 H 5 O 2 ) causes a temperature increase to 4.96 C, what is the heat capacity of the bomb calorimeter assembly? 6. Calculate q, w, ΔH, and ΔE for the heating of 10 moles of carbon dioxide gas from 0 C to 100 C at constant pressure. Assume that the C p of carbon dioxide for this temperature range is constant. 7. In a particular change in state, a system absorbed 200 cal of heat. When the system was returned to its initial state by a different process, 100 cal of heat were emitted and the system did the equivalent of 400 cal of work on the surroundings. How much work was involved in the first process? 8. A glass containing 200 g of tap water is at 15 C. How many ice cubes weighing 10 g each at 5 C are required to bring the water temperature to 0 C? Assume specific heat of ice to be the same as that of water. 9. When food is heated in a metal pot on a stove, heat must be added to warm the pot as well as the food. Calculate the average specific heat of a pot which weighs 0.50 kg if 2.54 kilowatt are needed to heat the pot from 25 C to 100 C in 1 minute when it contains 375 ml of water. Assume 100% heat transfer from the unit to the pot. What material is the pot made of?
2 10. Suppose a weighed specimen of excised fatty tissue is sealed in a vessel filled with oxygen. The vessel is then immersed in 1000 ml of water in a calorimeter. The combustion reaction is initiated by an electric current. The completed reaction was observed to raise the water temperature from 25.0 to 38.8 C. A previous calibration has shown that the heat capacity of those calorimeter parts undergoing temperature rise may be expressed as a "water equivalent" of 210 ml. What is the heat given off or absorbed in this process? 11. A man who weighs 68.0 kg produces about 3000 kcal of heat every day as a result of his normal metabolism processes. If we assume that his heat capacity to be the same as that of water, how hot would he get if his body retained all the heat produced in a day? 12. A 1.50 g sample of NH 4 NO 3 is added to 35 g of H 2 O in a Dewar flask and stirred until it dissolves. The temperature of the solution drops from 22.7 to 19.4 C. (a) Is the process endothermic or exothermic? (b) What is the enthalpy change of NH 4 NO 3 in kj/mole. Assume that the specific heat of the solution is 4.18 J/g C. 13. Consider a system consisting of 1 mole of a monatomic gas contained in a piston. What is the temperature change of the gas if q = 50 joules and w = 100 joules? 14. How much heat is evolved from 50.0 g of hydrogen gas is burned to water in a rocket engine? H 2 (g) + ½O 2 (g) H 2 O (l) ΔH = 68.3 kcal 15. Calculate the heat evolved when 50.0 g of H 2 gas is mixed with equal amount of N 2 gas. The 3 H 2 (g) + N 2 (g) 2 NH 3 (g) ΔH = kcal reaction is carried out at constant pressure condition. 16. Predict ΔH for the following reaction from N (g) + O (g) NO (g) ½ N 2 (g) + ½ O 2 (g) NO (g) N (g) ½ N 2 (g) O (g) ½ O 2 (g) ΔH = 21.6 kcal ΔH = kcal ΔH = 59.6 kcal 17. Give the thermal equations C (graphite) C (diamond) C (diamond) + O 2 (g) CO 2 (g) ΔH = kcal ΔH = kcal Write the thermochemical equation for the combustion of C (graphite).
3 18. Predict ΔH for the following reaction from C 6 H 4 (OH) 2 (aq) + H 2 O 2 (aq) C 6 H 4 O 2 (aq) + 2 H 2 O (l) C 6 H 4 (OH) 2 (aq) C 6 H 4 O 2 (aq) + H 2 (g) ΔH = 42.2 kcal ½ O 2 (g)+ H 2 O (l) H 2 O 2 (aq) ΔH = 22.6 kcal H 2 (g) + ½ O 2 (g) H 2 O (l) ΔH = 68.3 kcal 19. Calculate the heat of reaction for 2 SO 2 (g) + O 2 (g) 2SO 3 (g) 20. From the following data, calculate the molar heat of formation of solid PCl 5 (s). P 4 (s) + 6 Cl 2 (g) 4 PCl 3 (l) PCl 3 (l) + Cl 2 (g) PCl 5 (s) ΔH = kcal ΔH = 32.8 kcal 21. Calculate the molar heat of formation of methyl alcohol from the following equations: CH 3 OH (l) + 3 / 2 O 2 (g) CO 2 (g) + 2 H 2 O (l) C (s) + O 2 (g) CO 2 (aq) H 2 (g) + 1 / 2 O 2 (g) H 2 O (l) ΔH = kcal ΔH = 94.0 kcal ΔH = 68.3 kcal 22. Use the values of bond energies to calculate ΔH for each of the following reactions: (a) H 2 (g) + Cl 2 (g) 2 HCl (g) (b) CH 4 (g) + 4 F 2 (g) CF 4 (g) + 4 HF (g) (c) C 2 H 4 (g) + Cl 2 (g) C 2 H 4 Cl 2 (g) (d) cyclopentane (g) 1 pentene (g) 23. From the following equations, determine the molar heat of formation of HNO 2 (aq): NH 4 NO 2 (aq) N 2 (g) + 2 H 2 O (l) ΔH = 76.5 kcal NH 3 (aq) + HNO 2 (aq) NH 4 NO 2 (aq) ΔH = 9.00 kcal 2 NH 3 (aq) N 2 (g) + 3 H 2 (g) ΔH = 40.6 kcal 2 H 2 (g) + O 2 (g) 2 H 2 O (l) ΔH = kcal 24. Calculate the heat of vaporization of 1 gram of water at body temperature (37 C). The heat capacity of liquid water may be taken as constant 18.0 cal mole 1 deg 1 ; the heat capacity of water vapor varies with temperature: C p (H 2 O, g) = x 10 3 T x 10 7 T 2 (in cal mole 1 deg 1 ) H 2 O (l) H 2 O (g) ΔH 373 = 9.70 kcal
4 25. Predict the enthalpy of reaction for the oxidation of CH 3 OH (l) CH 3 OH (l) + 3 / 2 O 2 (g) CO 2 (g) + 2 H 2 O (l) using the given table of mean bond energies. The enthalpy of vaporization at 25 C is kj/mole for CH 3 OH and kj/mole for H 2 O. 26. For the constant pressure process, C 2 H 6 (g) + 7 / 2 O 2 (g) 2 CO 2 (g) + 3 H 2 O (l) ΔH at 298 K for the above reaction is kcal/mole. (a) Find w, q, and ΔE for the process. (b) Using Table I to help you, find ΔH 298 for the process C 2 H 6 (g) + 7 / 2 O 2 (g) 2 CO 2 (g) + 3 H 2 O (g) 27. (a) Calculate the enthalpy of formation, per mole, of ZnS (s) by using the following information, and Table I. 2 ZnS (s) + 3 O 2 (g) 2 ZnO (s) + 2 SO 2 (g) ΔH = kj (b) What reaction and conditions are implied when the enthalpy of formation of ZnS (s) in (a) is calculated.
5 Some useful data: Specific heats (cal g 1 deg 1 ): water gold Fe 2 O 3 NaCl sulfur aluminum steel copper Heat of fusion (joules/g): ice 320 Density (g/cc): water steel Heat of combustion (kj/g): benzoic acid C p (cal/mole deg): CO Acceleration due to gravity 9.81 m s 2 Normal body temperature 37 C 1 calorie = joules 1 Joule = 1 watt sec = 1 kg m 2 s 2 Table 1 ΔH f for selected substances ΔH f (kj/mole) ΔH f (kj/mole) Al 2 O 3 (s) 1676 CuO (s) BaCO 3 (s) 1216 HBr (g) Br (g) HCl (g) Br 2 (g) HF (g) C (diamond) 1.90 HI (g) CCl 4 (g) H 2 O (g) CO (g) H 2 O (l) CO 2 (g) H 2 S (g) CH 4 (g) Hg (g) C 2 H 4 (g) KCl (s) C 2 H 6 (g) MnO 2 (s) C 3 H 8 (g) NH 3 (g) C 6 H 6 (g) N 2 O (g) C 6 H 6 (l) NO 2 (g) CH 3 OH (g) N 2 O 4 (g) 9.16 CH 3 OH (l) O 3 (g) C 2 H 5 OH (g) SO 2 (g) C 2 H 5 OH (l) SO 3 (g) Ca(OH) 2 (s) ZnO (s) 348.3
6 Table 2 Mean bond energies
Practice Test Questions:
Practice Test Questions: There are a lot of questions. Please feel free to do a problem, skip around and make sure you are doing all types of problems heat exchange, Hess Law problems, specific heat problems,
CHEM 1411, chapter 6. Thermochemistry Exercises
CHEM 1411, chapter 6. Thermochemistry Exercises 1. The heat capacity of 20.0 g of water is 83.7 J/ C. A) True B) False 2. Find the heat absorbed from the surroundings when 15 g of O 2 reacts according
CHEMISTRY Practice exam #4 answer key October 16, 2007
CHEMISTRY 123-01 Practice exam #4 answer key October 16, 2007 1. An endothermic reaction causes the surroundings to a. warm up. b. become acidic. c. condense. 2. Which of the following is an example of
3. Of energy, work, enthalpy, and heat, how many are state functions? a) 0 b) 1 c) 2 d) 3 e) 4 ANS: c) 2 PAGE: 6.1, 6.2
1. A gas absorbs 0.0 J of heat and then performs 15.2 J of work. The change in internal energy of the gas is a) 24.8 J b) 14.8 J c) 55.2 J d) 15.2 J ANS: d) 15.2 J PAGE: 6.1 2. Calculate the work for the
Chemistry Guide
551534 - Chemistry Guide 1- Contents Question Item Objective Type Skill 1 0102 M03.02.04 Multiple-choice answer Mastery of Problem Solving 2 0099 M03.03.02 Multiple-choice answer Mastery of Concepts 3
Name: Thermochemistry. Practice Test B. General Chemistry Honors Chemistry
Name: Thermochemistry B Practice Test B 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
THERMOCHEMISTRY & 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
Name: Thermochemistry. Practice Test A. General Chemistry Honors Chemistry
Name: Thermochemistry Practice Test A 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
ENERGY. Thermochemistry. Heat. Temperature & Heat. Thermometers & Temperature. Temperature & Heat. Energy is the capacity to do work.
ENERGY Thermochemistry Energy is the capacity to do work. Chapter 6 Kinetic Energy thermal, mechanical, electrical, sound Potential Energy chemical, gravitational, electrostatic Heat Heat, or thermal energy,
Bomb Calorimetry. Example 4. Energy and Enthalpy
Bomb Calorimetry constant volume often used for combustion reactions heat released by reaction is absorbed by calorimeter contents need heat capacity of calorimeter q cal = q rxn = q bomb + q water Example
Chapter 5 Thermochemistry
Chapter 5 Thermochemistry I. Nature of Energy Energy units SI unit is joule, J From E = 1/2 mv 2, 1J = 1kg. m 2 /s 2 Traditionally, we use the calorie as a unit of energy. 1 cal = 4.184J (exactly) The
Thermochemistry. Thermochemistry 1/25/2010. Reading: Chapter 5 (omit 5.8) As you read ask yourself
Thermochemistry Reading: Chapter 5 (omit 5.8) As you read ask yourself What is meant by the terms system and surroundings? How are they related to each other? How does energy get transferred between them?
UNIT 1 THERMOCHEMISTRY
UNIT 1 THERMOCHEMISTRY THERMOCHEMISTRY LEARNING OUTCOMES Students will be expected to: THERMOCHEMISTRY STSE analyse why scientific and technological activities take place in a variety individual and group
STOICHIOMETRY. - the study of the quantitative aspects of chemical
STOICHIOMETRY - the study of the quantitative aspects of chemical GENERAL PLAN FOR STOICHIOMETRY Mass reactant Mass product Moles reactant Stoichiometric factor Moles product STOICHIOMETRY It rests on
CHAPTER 6 THERMOCHEMISTRY
Chapter 6 Thermochemistry Page 1 CHAPTER 6 THERMOCHEMISTRY 6-1. The standard state of an element or compound is determined at a pressure of and a temperature of. (a) 760 atm, 0 o C (b) 1 mmhg, 273 o C
6.1 Some basic principles
Ch 6 Thermochemistry: Energy Flow and Chemical Change 6.1 Forms of Energy and Their Interconversion 6.2 Enthalpy: Heats of Reaction and Chemical Change 6.3 Calorimetry: Laboratory Measurement of Heats
Calorimeter: A device in which the heat associated with a specific process is measured.
1 CALORIMETRY p. 661-667 (simple), 673-675 (bomb) Calorimeter: A device in which the heat associated with a specific process is measured. There are two basic types of calorimeters: 1. Constant-pressure
Unit 14 Thermochemistry
Unit 14 Thermochemistry Name May 5 6 Unit 13 Acids and Bases Test Intro to Thermochemistry Videos (p.2-3) HW: p. 4-5 9 10 11 12 13 Thermochemistry Interpret graphs Heat of reaction & Specific Heat Heat
Example: orange juice from frozen concentrate.
Dilution: a process in which the concentration (molarity) of a solution is lowered. The amount of solute (atoms, moles, grams, etc.) remains the same, but the volume is increased by adding more solvent.
Chapter 5 Thermochemistry
Chapter 5 Thermochemistry 1. The ΔE of a system that releases 14.4 J of heat and does 4.8 J of work on the surroundings is J. (a). 19.2 J (b). 14.4 J (c). 4.8 J (d). - 19.2 J Explanation: The ΔE can be
Name Date Class THERMOCHEMISTRY. SECTION 17.1 THE FLOW OF ENERGY HEAT AND WORK (pages 505 510)
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 and specific heat.
Energy Changes in Chemical Reactions. System loses heat (negative); gains heat (positive) Describe the difference between the two.
Energy Changes in Chemical Reactions Most reactions give off or absorb energy Energy is the capacity to do work or supply heat. Heat: transfer of thermal (kinetic) energy between two systems at different
System. System, Boundary and surroundings: Nature of heat and work: Sign convention of heat: Unit-7 Thermodynamics
Unit-7 Thermodynamics Introduction: The term Thermo means heat and dynamics means flow or movement.. So thermodynamics is concerned with the flow of heat. The different forms of the energy are interconvertible
Chapter 5 Chemical Quantities and Reactions
Chapter 5 Chemical Quantities and Reactions 1 Avogadro's Number Small particles such as atoms, molecules, and ions are counted using the mole. 1 mole = 6.02 x 10 23 items Avogadro s number 602 000 000
Chapter 6: Thermochemistry (Chemical Energy) (Ch6 in Chang, Ch6 in Jespersen)
Chapter 6: Thermochemistry (Chemical Energy) (Ch6 in Chang, Ch6 in Jespersen) Energy is defined as the capacity to do work, or transfer heat. Work (w) - force (F) applied through a distance. Force - any
As long as the relative ratios are constant the amounts are correct. Using these ratios to determine quantities is called Stoichiometry.
The Meaning of the Balanced Equation Tuesday, October 11, 2011 2:05 PM The Balanced Equation is a measure of the relative amounts of a compounds that participate in or are produced by a reaction. Since
Chemistry Thermochemistry Lesson 10 Lesson Plan David V. Fansler
Chemistry Thermochemistry Lesson 10 Lesson Plan David V. Fansler The Flow of Energy-Heat Objectives: Explain the relationship between energy and heat; Distinguish between heat capacity and specific heat.
Calorimetry and Enthalpy. Chapter 5.2
Calorimetry and Enthalpy Chapter 5.2 Heat Capacity Specific heat capacity (c) is the quantity of thermal energy required to raise the temperature of 1g of a substance by 1⁰C The units for specific heat
EXPERIMENT 9. Thermochemistry: Hess Law and the Heat of Formation of MgO
Outcomes EXPERIMENT 9 Thermochemistry: Hess Law and the Heat of Formation of MgO After completing this experiment, the student should be able to: 1. Differentiate between exothermic and endothermic reactions.
Enthalpy changes and calorimetry. Enthalpy changes in reactions Calorimetry and heat measurement Hess s Law Heats of formation
Enthalpy changes and calorimetry Enthalpy changes in reactions Calorimetry and heat measurement Hess s Law Heats of formation Learning objectives Describe the standard state for thermodynamic functions
Thermochemical equations allow stoichiometric calculations.
CHEM 1105 THERMOCHEMISTRY 1. Change in Enthalpy ( H) Heat is evolved or absorbed in all chemical reactions. Exothermic reaction: heat evolved - heat flows from reaction mixture to surroundings; products
CHEMISTRY 110 Assignment #3 - answers 2011.
1. Titanium metal is used as a structural material in many high tech applications such as in jet engines. What is the specific heat of titanium in J/() if it takes 89.7 J to raise the temperature of a
CHEM 101 WINTER EXAM II
CHEM 101 WINTER 09-10 EXAM II 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
Specific Heat Capacity
Specific Heat Capacity Specific Heat Capacity The amount of energy it takes to heat up 1 gram of a substance by 1 C What heats up faster, metal or water? Calorie Energy changes can also be measured in
CHM1045 Practice Test 3 v.1 - Answers Name Fall 2013 & 2011 (Ch. 5, 6, 7, & part 11) Revised April 10, 2014
CHM1045 Practice Test 3 v.1 - Answers Name Fall 013 & 011 (Ch. 5, 6, 7, & part 11) Revised April 10, 014 Given: Speed of light in a vacuum = 3.00 x 10 8 m/s Planck s constant = 6.66 x 10 34 J s E (-.18x10
( )( L L)
Chemistry 360 Dr. Jean M. Standard Problem Set 5 Solutions 1. Determine the amount of pressure-volume work performed by 1 mole of water freezing to ice at 0 C and 1 atm pressure. The density of liquid
Chapter 6 Quantities in Chemical Reactions
Chapter 6 Quantities in Chemical Reactions The Meaning of a Balanced Chemical Equation Mole-Mole Conversions Mass-Mass Conversions Limiting Reactants Percent Yield Energy Changes Copyright The McGraw-Hill
Thermodynamics- Chapter 19 Schedule and Notes
Thermodynamics- Chapter 19 Schedule and Notes Date Topics Video cast DUE Assignment during class time One Review of thermodynamics 1_thermo_review AND Review of thermo Wksheet 2.1ch19_intro Optional: 1sc_thermo
Unit 5 Practice Test. Name: Class: Date: Multiple Choice Identify the choice that best completes the statement or answers the question.
Name: Class: Date: Unit 5 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1) The internal energy of a system is always increased by. A) adding
The Relationships Between. Internal Energy, Heat, Enthalpy, and Calorimetry
The Relationships Between Internal Energy, Heat, Enthalpy, and Calorimetry Recap of Last Class Last class, we began our discussion about energy changes that accompany chemical reactions Chapter 5 discusses:
Chapter 5 Energy Relationships in Chemistry: Thermochemistry
Chapter 5 Energy Relationships in Chemistry: Thermochemistry In order to study thermochemical changes, we first have to define (a) system that specify part of the universe of interest to us. (b) surrounding
Chapter 16 Review Packet
Chapter 16 Review Packet AP Chemistry Chapter 16 Practice Multiple Choice Portion 1. For which process is ΔS negative? Note: ΔS = S final S initial therefore, if ΔS is positive, S final > S initial if
Procedure. Day 1 - Calibration of the Calorimeter. (Part I) The Heat Capacity of the Calorimeter.
Thermochemistry Experiment 10 Thermochemistry is the study of the heat energy involved in chemical reactions and changes of physical state. Heat energy is always spontaneously transferred from hotter to
Calorimetry and Thermochemistry
CHEM 121L General Chemistry Laboratory Revision 1.3 Calorimetry and Thermochemistry Learn how to measure Heat flow. Learn about the Specific Heat of substances. Learn about Exothermic and Endothermic chemical
Thermodynamics Review
Thermodynamics Review 1. According to Reference Table I, the dissolving of NH 4Cl(s) in water is 1) exothermic and the heat of reaction is negative 2) exothermic and the heat of reaction is positive 3)
Chapter 7 Energy and Chemical Change: Breaking and Making Bonds
Multiple Choice Chapter 7 Energy and Chemical Change: Breaking and Making Bonds Section 7.1 1. Which one of the following is a unit of energy, but not an SI unit of energy? a. joule b. newton c. pascal
Stoichiometry. 1. The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 0.1; (4) 0.2.
Stoichiometry 1 The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 01; (4) 02 2 A 44 gram sample of a hydrate was heated until the water of hydration was driven
Chemistry Final Exam Review
Name: Date: Block: Chemistry Final Exam Review 2012-2013 Unit 1: Measurement, Numbers, Scientific Notation, Conversions, Dimensional Analysis 1. Write 0.000008732 in scientific notation 8.732x10-6 2. Write
Enthalpy of Neutralization. Introduction
Enthalpy of Neutralization Introduction Energy changes always accompany chemical reactions. If energy, in the form of heat, is liberated the reaction is exothermic and if energy is absorbed the reaction
Energy and Chemical Reactions. Characterizing Energy:
Energy and Chemical Reactions Energy: Critical for virtually all aspects of chemistry Defined as: We focus on energy transfer. We observe energy changes in: Heat Transfer: How much energy can a material
Chapter 3 Mass Relationships in Chemical Reactions
Chapter 3 Mass Relationships in Chemical Reactions Student: 1. An atom of bromine has a mass about four times greater than that of an atom of neon. Which choice makes the correct comparison of the relative
PREPARATION FOR CHEMISTRY LAB: COMBUSTION
1 Name: Lab Instructor: PREPARATION FOR CHEMISTRY LAB: COMBUSTION 1. What is a hydrocarbon? 2. What products form in the complete combustion of a hydrocarbon? 3. Combustion is an exothermic reaction. What
Chemistry Distributed Practice Assessment
Name Hour Chemistry Distributed Practice Assessment Practice 2011 Practice Exam A **This END OF COURSE Practice Exam is a qualifier for all Exam Takers 1 Objective 1 Answer questions relating to atomic
87 16 70 20 58 24 44 32 35 40 29 48 (a) graph Y versus X (b) graph Y versus 1/X
HOMEWORK 5A Barometer; Boyle s Law 1. The pressure of the first two gases below is determined with a manometer that is filled with mercury (density = 13.6 g/ml). The pressure of the last two gases below
SUGGESTION ANSWER SCHEME CHAPTER 8: THERMOCHEMISTRY. 1 (a) Use the data in the table below to answer the following questions:
SUGGESTION ANSWER SCHEME CHAPTER 8: THERMOCHEMISTRY ANSWER SCHEME UPS 2004/2005 SK027 1 (a) Use the data in the table below to answer the following questions: Enthalpy change ΔH (kj/mol) Atomization energy
Heats of Transition, Heats of Reaction, Specific Heats, and Hess s Law
Heats of Transition, Heats of Reaction, Specific Heats, and Hess s Law GOAL AND OVERVIEW A simple calorimeter will be made and calibrated. It will be used to determine the heat of fusion of ice, the specific
Thermodynamics. S (reactants) S S (products) AP Chemistry. Period Date / / R e v i e w. 1. Consider the first ionization of sulfurous acid:
AP Chemistry Thermodynamics 1. Consider the first ionization of sulfurous acid: H 2SO 3(aq) H + (aq) + HSO 3 - (aq) Certain related thermodynamic data are provided below: H 2SO 3(aq) H + (aq) HSO 3 - (aq)
4. Aluminum chloride is 20.2% aluminum by mass. Calculate the mass of aluminum in a 35.0 gram sample of aluminum chloride.
1. Calculate the molecular mass of table sugar sucrose (C 12 H 22 O 11 ). A. 342.30 amu C. 320.05 amu B. 160.03 amu D. 171.15 amu 2. How many oxygen atoms are in 34.5 g of NaNO 3? A. 2.34 10 23 atoms C.
Chem 1A Exam 2 Review Problems
Chem 1A Exam 2 Review Problems 1. At 0.967 atm, the height of mercury in a barometer is 0.735 m. If the mercury were replaced with water, what height of water (in meters) would be supported at this pressure?
CHEM 105 HOUR EXAM III 28-OCT-99. = -163 kj/mole determine H f 0 for Ni(CO) 4 (g) = -260 kj/mole determine H f 0 for Cr(CO) 6 (g)
CHEM 15 HOUR EXAM III 28-OCT-99 NAME (please print) 1. a. given: Ni (s) + 4 CO (g) = Ni(CO) 4 (g) H Rxn = -163 k/mole determine H f for Ni(CO) 4 (g) b. given: Cr (s) + 6 CO (g) = Cr(CO) 6 (g) H Rxn = -26
AP* Chemistry THERMOCHEMISTRY
AP* Chemistry THERMOCHEMISTRY Terms for you to learn that will make this unit understandable: Energy (E) the ability to do work or produce heat ; the sum of all potential and kinetic energy in a system
Example. c. Calculate the amount of heat (in kj) required to heat 1.00 kg (~1 L) of water at 25 C to its boiling point.
Example When consuming an ice-cold drink, one must raise the temperature of the beverage to 37.0 C (normal body temperature). Can one lose weight by drinking ice-cold beverages if the body uses up about
PREPARATION FOR CHEMISTRY LAB: COMBUSTION
1 1. What is a hydrocarbon? PREPARATION FOR CHEMISTRY LAB: COMBUSTION 2. Give an example of a combustion reaction? 3. What products form in the complete combustion of a hydrocarbon? Are these products
ENTHALPY CHANGES FOR A CHEMICAL REACTION scaling a rxn up or down (proportionality) quantity 1 from rxn heat 1 from Δ r H. = 32.
CHEMISTRY 103 Help Sheet #10 Chapter 4 (Part II); Sections 4.6-4.10 Do the topics appropriate for your lecture Prepared by Dr. Tony Jacob http://www.chem.wisc.edu/areas/clc (Resource page) Nuggets: Enthalpy
Enthalpy of Reaction and Calorimetry worksheet
Enthalpy of Reaction and Calorimetry worksheet 1. Calcium carbonate decomposes at high temperature to form carbon dioxide and calcium oxide, calculate the enthalpy of reaction. CaCO 3 CO 2 + CaO 2. Carbon
Stoichiometry. 1. The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 0.1; (4) 0.2.
Stoichiometry 1 The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 01; (4) 02 2 A 44 gram sample of a hydrate was heated until the water of hydration was driven
I. CALORIMETRY CALORIMETRY
CALORIMETRY I. CALORIMETRY If the process (e.g. chemical reaction, phase conversion) requires heat to proceed, it is said to be endothermic. For endothermic process, q > 0. If the process (e.g. chemical
Chemistry 102 Chapter 17 THERMODYNAMICS
THERMODYNAMICS Thermodynamics is concerned with the energy changes that accompany chemical and physical processes. Two conditions must be fulfilled in order to observe a chemical or physical change: The
STOICHIOMETRY II UNIT
STOICHIOMETRY II UNIT Assignment #1 (Conversions with compounds) 1. Convert 1.806 x 10 23 molecules of Cl2 to moles. 2. Convert 1000 molecules of P4O10 to moles. 3. Convert 360 grams of NH3 (ammonia gas)
Lab Session 9, Experiment 8: Calorimetry, Heat of Reaction
Lab Session 9, Experiment 8: Calorimetry, Heat of Reaction Specific heat is an intensive property of a single phase (solid, liquid or gas) sample that describes how the temperature of the sample changes
(3) AgCl(s) Ag + (aq) + Cl (aq) (4) 2 HgO(s) 2 Hg( ) + O 2. A(g) + B(g) AB(g) 2 SO 2 (g) + O 2 (g) 2 SO 3 (g)
1. Given the reaction at equilibrium: H 2 + Cl 2 2 HCl As the pressure s at constant temperature, the number of moles of HCl (1) s (3) remains the same (2) s 2. The Haber process is represented by the
1. Balance the following equation. What is the sum of the coefficients of the reactants and products?
1. Balance the following equation. What is the sum of the coefficients of the reactants and products? 1 Fe 2 O 3 (s) + _3 C(s) 2 Fe(s) + _3 CO(g) a) 5 b) 6 c) 7 d) 8 e) 9 2. Which of the following equations
Calorimetry Experiments
Calorimetry Experiments Pre-Lab: Today s laboratory period will include a variety of activities designed to re-familiarize you with safe practices for chemistry laboratory, the space and equipment you
Chemistry: Chemical Equations
Chemistry: Chemical Equations Write a balanced chemical equation for each word equation. Include the phase of each substance in the equation. Classify the reaction as synthesis, decomposition, single replacement,
7. 2. KOH (you need an acid or a base, this is a base) 8. 1. 76. All gold atoms have 79 protons and electrons, this is a +3 cation.
IB/SL Chemistry Name ANSWERS Test; Past Chemistry Regents Exams Most Frequently Missed Questions 1. 1. A HIGH PROBABLITY OF FINDING AN ELECTRON 2. 3. +8 (every atom of oxygen in the universe) 3. 2. LOW
Chemical Equations C5.6b Predict single replacement reactions.
Chemistry 2SEM Chemical Equations C5.6b Predict single replacement reactions. Common Assessment Review Predict the following single replacement reactions: a. Zn + Pb(C2H3O2)2 ----> Pb + Zn(C2H3O2)2_ b.
Standard States. Standard Enthalpy of formation
Standard States In any thermochemical equation, the states of all reactants and products must be specified; otherwise it becomes difficult for scientists to understand the experimental results of other
2 NO + O 2 2 NO 2 3/18/2014. iclicker Participation Question: A B C
Today: Stoichiometric Analysis: Gram to Gram Conversions: Use MOLAR MASS to get to moles Limiting Reagents: Method 1 Method 2 Actual Yield & Percent Yield Combustion Analysis Titrations Next Meeting Reading
Heat Practice Test Name: Date: Period:
Name: Date: Period: 1. Base your answer to the following question on the information below. The temperature of a sample of a substance is increased from 20. C to 160. C as the sample absorbs heat at a
Chapter 5 Principles of Chemical Reactivity: Energy and Chemical Reactions
PRACTICING SKILLS Energy Chapter 5 Principles of Chemical Reactivity: 1. To move the lever, one uses mechanical energy. The energy resulting is manifest in electrical energy (which produces light); thermal
Chapter 7: Chemical Equations. Name: Date: Period:
Chapter 7: Chemical Equations Name: Date: Period: 7-1 What is a chemical reaction? Read pages 232-237 a) Explain what a chemical reaction is. b) Distinguish between evidence that suggests a chemical reaction
DETERMINING THE ENTHALPY OF FORMATION OF CaCO 3
DETERMINING THE ENTHALPY OF FORMATION OF CaCO 3 Standard Enthalpy Change Standard Enthalpy Change for a reaction, symbolized as H 0 298, is defined as The enthalpy change when the molar quantities of reactants
Thermochemistry: Enthalpy of Reaction Hess s Law
Thermochemistry: Enthalpy of Reaction Hess s Law Objective Demonstrate Hess s Law for determining the enthalpy of formation for MgO by measuring temperature change for several reactions. Introduction The
5.2. Determining Enthalpy of Reaction by Experiment. Specific Heat Capacity. 234 MHR Unit 3 Energy Changes and Rates of Reaction
In this section, you will 5.2 Section Preview/ Specific Expectations determine the heat that is produced by a reaction using a calorimeter, and use the data obtained to calculate the enthalpy change for
Chemistry Sample Questions
Chemistry Sample Questions Name: 1) Which phase change represents deposition? A) liquid gas B) gas solid C) solid liquid D) gas liquid 2) Which pair has identical electron configurations? A) K 0 and Na
Prelab attached (p 8-9) (g)! MgO (s) + heat (1)
CHEM 151 ENTHALPY OF FORMATION OF MgO FALL 2008 Fill-in Prelab attached (p 8-9) Stamp Here Name Partner Lecture instructor Date INTRODUCTION Chemical reactions either produce heat as they proceed (exothermic)
Gen Chem I Exam 1 Review (Chapters 1 & 2)
Gen Chem I Exam 1 Review (Chapters 1 & 2) 1 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. All of the following are properties of antimony. Which one
Chemical Equations & Stoichiometry
Chemical Equations & Stoichiometry Chapter Goals Balance equations for simple chemical reactions. Perform stoichiometry calculations using balanced chemical equations. Understand the meaning of the term
Chapter 5. Name: Class: Date: Multiple Choice Identify the choice that best completes the statement or answers the question.
Class: Date: Chapter 5 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. What is the pressure of the sample of gas trapped in the open-tube mercury manometer
Chemistry 1 Final Exam Study Guide Spring 2009
Chemistry 1 Final Exam Study Guide Spring 2009 1. If a substance has a mass of 36.4 g and a volume of 8.500 ml, what is its density? 2. Which involves a chemical change? a. powdering sugar b. condensing
STOICHIOMETRY ANALOGY
STOICHIOMETRY ANALOGY Stoichiometry is the quantitative relationship between the reactants and products in a balanced chemical equation. Stoichiometry allows chemists to predict how much of a reactant
3A Energy. What is chemical energy?
3A Energy What is chemical energy? Chemical energy is a form of potential energy which is stored in chemical bonds. Chemical bonds are the attractive forces that bind atoms together. As a reaction takes
Stoichiometry. Stoichiometry Which of the following forms a compound having the formula KXO 4? (A) F (B) S (C) Mg (D) Ar (E) Mn
The Advanced Placement Examination in Chemistry Part I Multiple Choice Questions Part II - Free Response Questions Selected Questions from 1970 to 2010 Stoichiometry Part I 1984 2. Which of the following
IB Chemistry. DP Chemistry Review
DP Chemistry Review Topic 1: Quantitative chemistry 1.1 The mole concept and Avogadro s constant Assessment statement Apply the mole concept to substances. Determine the number of particles and the amount
STOICHOMETRY UNIT Determine the mass of carbon present in a sample of glucose weighing 5.4 g.
PERCENTAGE COMPOSITION STOICHOMETRY UNIT 3 1. A sample of magnesium weighing 2.246 g burns in oxygen to form 3.724 g of magnesium oxide. What are the percentages of magnesium and oxygen in magnesium oxide?
CHM2045 Study Union Final Review Fall 2015
CHM2045 Study Union Final Review Fall 2015 Chapter One 1. Classify each substance as a pure substance or a mixture. If it is a pure substance, classify it as an element or a compound. If it is a mixture,
CHEMICAL REACTIONS. Chemistry 51 Chapter 6
CHEMICAL REACTIONS A chemical reaction is a rearrangement of atoms in which some of the original bonds are broken and new bonds are formed to give different chemical structures. In a chemical reaction,
Answers and Solutions to Text Problems
Chapter 6 Answers and Solutions 6 Answers and Solutions to Text Problems 6.1 A chemical change occurs when the atoms of the initial substances rearrange to form new substances. Chemical change is indicated
Thermodynamics. Energy can be used * to provide heat * for mechanical work * to produce electric work * to sustain life
Thermodynamics Energy can be used * to provide heat * for mechanical work * to produce electric work * to sustain life Thermodynamics is the study of the transformation of energy into heat and for doing
Determination of the enthalpy of combustion using a bomb calorimeter TEC
Determination of the enthalpy of TEC Related concepts First law of thermodynamics, Hess s law of constant heat summation, enthalpy of combustion, enthalpy of formation, heat capacity. Principle The bomb