Name: General Chemistry Chapter 11 Thermochemistry- Heat and Chemical Change
|
|
- Shanon Gallagher
- 6 years ago
- Views:
Transcription
1 Name: General Chemistry Chapter 11 Thermochemistry- Heat and Chemical Change Notepack 1
2 Section 11.1: The Flow of Energy Heat (Pages ) 1. Define the following terms: a. Thermochemistry b. Energy c. Chemical Potential Energy d. Heat (q) e. System f. Surroundings g. Universe h. Law of conservation of energy i. Endothermic process j. Exothermic process k. Calorie l. Joule m. Heat Capacity n. Specific heat capacity (specific heat) i. What is the specific heat of water in units of Calories/g-C? ii. What is the specific heat of water in units of Joules/g-c? 2. Calculating heat (q) a. We use this equation: 2
3 Example problems: 1. The temperature of a piece of copper with a mass of 95.4 grams increases from 25 C to 48 C when the metal absorbs 849 Joules of heat. What is the specific heat of copper? 2. When 435 J of heat is added to 3.4 grams of olive oil at 21 C, the temperature increases to 85 C. What is the specific heat of olive oil? 3. A piece of stainless steel weighing 1.55 grams absorbs 141 Joules of heat when its temperature increases by 178 C. What is the specific heat of the stainless steel? 4. How much heat is required to raise the temperature of 250 grams of mercury 52 C? The specific heat for mercury is 0.14 J/g-C. 5. Will the specific heat of 50 grams of a substance be the same as, or greater than, the specific heat of 10 grams of the same substance? Explain. 6. On a sunny day, why does the concrete deck around an outdoor swimming pool become hot, while the water stays cool? 7. Using calories, calculate how much heat 32.0 grams of water absorbs when it is heated from 25 C to 80 C. How many Joules is this? 8. A chunk of silver has a heat capacity of 42.8 J/C. If the silver has a mass of 181 grams, calculate the specific heat of silver. 9. How many kilojoules of heat are absorbed when 1.0 Liter of water is heated from 18 C to 85 C? 3
4 11.2 Calorimetry: Measuring and Expressing Heat Changes CONSTANT PRESSURE CALORIMETER (coffee cup calorimeter) 1. What is calorimetry? 2. What is Enthalpy a. What is the sign of H for exothermic reactions? b. What is the sign of H for endothermic reactions? Example Problems for Constant Pressure Calorimetry 1. To study the amount of heat released during a neutralization reaction, 25.0 ml of moles of HCl is added to 25.0 ml of moles of NaOH in a foam cup calorimeter. At the start, the solutions and the calorimeter are all at 25 C. During the reaction, the highest temperature observed is 32 C. Calculate the heat (in kj) released during this reaction. Assume the densities of the solutions are 1.00 g/ml. 4
5 2. A student mixed 50 ml of water containing 0.5 mol HCl at 22.5 C with 50 ml of water containing 0.50 mol MaOH at 22.5 C in a foam cup calorimeter. The temperature of the resulting solution increased to 26 C. How much heat in kilojoules (kj) was released by this reaction? 3. A small pebble is heated and placed in a foam cup calorimeter containing 25.0 ml of water at 25 C. The water reaches a maximum temperature of 26.4 C. How many joules of heat were released by the pebble? Thermochemical Equations Show the thermochemical equation for calcium oxide reacting with water and releasing 65.2 kj of heat energy. o You can treat heat change in a chemical reaction like any other reactant or product in a chemical equation. Draw the Enthalpy diagram for this process: o Write the thermochemical equation for sodium hydrogen carbonate decomposing into sodium carbonate, water and carbon dioxide. It absorbs 129 kj of heat energy. o Draw the enthalpy diagram for this process. 5
6 To solve problems involving thermochemical equations, treat the enthalpy value as any other stoichiometric value. Examples: 1. Using the equation from above, calculate the kilojoules of heat required to decompose 2.24 mole of sodium hydrogen carbonate. 2. When carbon disulfide is formed from its elements, 89.3 kj of heat is absorbed. Calculate the amount of heat (in kj) absorbed when 5.66 grams of carbon disulfide is formed. 3. The production of iron and carbon dioxide from iron III oxide and carbon monoxide is an exothermic reaction, releasing 26.3 kj of heat energy. How many kilojoules of heat are produced when 100 grams of iron III oxide reacts with excess of CO? 4. Combusting one mole of methane, CH 4, releases 890 kj of heat energy. How many grams of methane are needed to release 1250 kj of heat energy? 11.3 Heat in Changes of State Phase diagrams display the state of a substance at various pressures and temperatures and the places where equilibria exist between phases. 6
7 The AB line is the interface. It starts at the (A), the point at which all three states are in equilibrium. It ends at the (B); above this critical temperature and critical pressure the liquid and vapor are indistinguishable from each other. Each point along this line is the of the substance at that pressure. The AD line is the interface between. The at each pressure can be found along this line. Below A the substance cannot exist in the. Along the AC line the phases are in equilibrium; the point at each pressure is along this line. 7
8 Energy Changes Associated with Changes of State Phase Changes Intermolecular Forces : Energy required to change a solid at its melting point to a liquid. Hfus : Energy required to change a liquid at its boiling point to a gas. Hvap Notice that the heat of vaporization is always larger than its heat of fusion. The heat of fusion, or enthalpy of fusion, for ice is 6.01 kj/mol. The heat of vaporization, or enthalpy of vaporization, for water is 40.7 kj/mol. The heat of sublimation is the sum of heats of vaporization and fusion. For water = approx 47 kj/mol 8
9 The heat added to the system at the melting and boiling points goes into pulling the molecules farther apart from each other. The temperature of the substance does not rise during the phase change SAMPLE PROBLEM #1: Calculate the enthalpy change upon converting 1 mol of ice at -25 o C to water vapor (steam) at 125 o C under a constant pressure of 1 atm. The specific heats of ice, water, and steam are 2.09 J/g-K, 4.18 J/g-K, and 1.84 J/g-K respectively. For H 2 O, Hfus = 6.01 kj/mol and Hvap = kj/mol. SAMPLE PROBLEM #2: What is the enthalpy change during the process in which 100 g of water at 50.0 o C is cooled to ice at -30 o C? 9
10 Heat of Solution 1. Heat changes can also occur when a solute dissolves in a solvent. The heat change caused by dissolution of one mole of substance is the. ( Hsoln) 2. When one mole of sodium hydroxide dissolves in water, sodium ions and hydroxide ions separate and interact with the water. The temperature of the solution increases, releasing kj of heat. Write the thermochemical equation. 3. The heat of solution for the dissolving process of calcium chloride is kj/mol. Write this thermochemical equation. 4. The heat of solution for the dissolving process of ammonium nitrate is kj/mol. Write this thermochemical equation. Sample Problems: 1. How much heat (in kj) is released when 2.5 mol of NaOH is dissolved in water? (Use the thermochemical equation from above) 2. How much heat (in kj) is released when 100 grams of sodium hydroxide are dissolved in water? 3. How many grams of ammonium nitrate must be dissolved in water so that 88 kj of heat is absorbed? 10
11 Section 11.4: Hess s Law Enthalpy is a state function. It is independent of the path. We can add equations to come up with the desired final product, and add the H Two rules o o Sample Problem #1: If the reaction is reversed the sign of H is changed If the reaction is multiplied or divided, so is H The following information is known: o C(s) + O 2 (g) CO 2 (g) H 1 = kj o CO(g) + ½ O 2 (g) CO 2 (g) H 2 = kj Using these data, calculate the enthalpy for: C(s) + ½ O 2 (g) CO(g) Sample Problem #2 Calculate H for the reaction 2C(s) + H 2 (g) C 2 H 2 (g) Given the following chemical equations and their respective H. C 2 H 2 (g) + 5/2O 2 2CO 2 (g) + H 2 C(s) + O 2 (g) CO 2 (g) H 2 (g) + ½ O 2 (g) H 2 O(l) H = kj H = kj H = kj 11
12 Sample Problem #3 Calculate H for the reaction NO(g) + O(g) NO 2 (g) Given the following information: NO(g) + O 3 (g) NO 2 (g) + O 2 (g) O 3 (g) 3/2 O 2 (g) O 2 (g) 2 O (g) H = kj H = kj H = kj 12
Name: Thermochemistry. Practice Test C. General Chemistry Honors Chemistry
Name: Thermochemistry C Practice Test C General Chemistry Honors Chemistry 1 Objective 1: Use the relationship between mass, specific heat, and temperature change to calculate the heat flow during a chemical
More informationChapter 11 Thermochemistry Heat and Chemical Change
Chemistry/ PEP Name: Date: Chapter 11 Thermochemistry Heat and Chemical Change Chapter 11:1 35, 57, 60, 61, 71 Section 11.1 The Flow of Energy - Heat 1. When 435 of heat is added to 3.4 g of olive oil
More informationChapter 11. Thermochemistry. 1. Let s begin by previewing the chapter (Page 292). 2. We will partner read Pages
Chapter 11 Thermochemistry 1. Let s begin by previewing the chapter (Page 292). 2. We will partner read Pages 293-94 The Flow of energy - heat Thermochemistry concerned with the heat changes that occur
More informationCh. 17 Thermochemistry
Ch. 17 Thermochemistry 17.1 The Flow of Energy Energy Transformations Thermochemistry: study of energy changes in chemical reactions and changes in state Chemical potential energy: energy stored in bonds
More informationName Class Date. As you read Lesson 17.1, use the cause and effect chart below. Complete the chart with the terms system and surroundings.
Name Class Date Thermochemistry 17.1 The Flow of Energy As you read Lesson 17.1, use the cause and effect chart below. Complete the chart with the terms system and surroundings. Process Cause Effect endothermic
More 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 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 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 informationName Date Class THERMOCHEMISTRY
Name Date Class 17 THERMOCHEMISTRY SECTION 17.1 THE FLOW OF ENERGY HEAT AND WORK (pages 505 510) This section explains the relationship between energy and heat, and distinguishes between heat capacity
More 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 informationCHAPTER 17 Thermochemistry
CHAPTER 17 Thermochemistry Thermochemistry The study of the heat changes that occur during chemical reactions and physical changes of state. Chemical Change: new substances created during chemical reaction
More information17.4 Calculating Heats Essential Understanding Heats of reaction can be calculated when it is difficult or
17.4 Calculating Heats of Reaction Essential Understanding Heats of reaction can be calculated when it is difficult or impossible to measure them directly. Lesson Summary Hess s Law Hess s law provides
More information17.2 Thermochemical Equations
17.2. Thermochemical Equations www.ck12.org 17.2 Thermochemical Equations Lesson Objectives Define enthalpy, and know the conditions under which the enthalpy change in a reaction is equal to the heat absorbed
More informationName Date Class THE FLOW OF ENERGY HEAT AND WORK
17.1 THE FLOW OF ENERGY HEAT AND WORK Section Review Objectives Explain the relationship between energy, heat, and work Distinguish between exothermic and endothermic processes Distinguish between heat
More informationI. The Nature of Energy A. Energy
I. The Nature of Energy A. Energy is the ability to do work or produce heat. It exists in 2 forms: 1. Potential energy is energy due to the composition or position of an object. 2. Kinetic energy is energy
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 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 informationName: Class: Date: ID: A
Name: Class: _ Date: _ ID: A Chpter 17 review Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which of these phase changes is an endothermic process? a.
More 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 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 informationChapter 8. Thermochemistry 강의개요. 8.1 Principles of Heat Flow. 2) Magnitude of Heat Flow. 1) State Properties. Basic concepts : study of heat flow
강의개요 Basic concepts : study of heat flow Chapter 8 Thermochemistry Calorimetry : experimental measurement of the magnitude and direction of heat flow Thermochemical Equations Copyright 2005 연세대학교이학계열일반화학및실험
More 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 informationChemistry Chapter 16. Reaction Energy
Chemistry Reaction Energy Section 16.1.I Thermochemistry Objectives Define temperature and state the units in which it is measured. Define heat and state its units. Perform specific-heat calculations.
More informationAP 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 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 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 informationChapter 5 Thermochemistry
Chapter 5 Thermochemistry Section 17.1 The Flow of Energy Heat and Work OBJECTIVES: Explain how energy, heat, and work are related. 2 Section 17.1 The Flow of Energy Heat and Work OBJECTIVES: Classify
More informationEnergy Transformations
Thermochemistry Energy Transformations Thermochemistry - concerned with heat changes that occur during chemical reactions Energy - capacity for doing work or supplying heat weightless, odorless, tasteless
More informationSection 9: Thermodynamics and Energy
Section 9: Thermodynamics and Energy The following maps the videos in this section to the Texas Essential Knowledge and Skills for Science TAC 112.35(c). 9.01 Law of Conservation of Energy Chemistry (11)(A)
More informationEnthalpies of Reaction
Enthalpies of Reaction Enthalpy is an extensive property Magnitude of H is directly related to the amount of reactant used up in a process. CH 4 (g) + 2O 2 (g) CO 2 (g) + 2H 2 O(l) H = 890 kj 2CH 4 (g)
More informationThermochemistry. Questions to ponder. Because 4/20/14. an ice-cube? an ice-cube? Part 2: Calorimetry. But I KNOW. Q=mc T, but T=0
Thermochemistry Part 2: Calorimetry p p If you leave your keys and your chemistry book sitting in the sun on a hot summer day, which one is hotter? Why is there a difference in temperature between the
More informationCh 9 Practice Problems
Ch 9 Practice Problems 1. One mole of an ideal gas is expanded from a volume of 1.50 L to a volume of 10.18 L against a constant external pressure of 1.03 atm. Calculate the work. (1 L atm = 101.3 J) A)
More information8.6 The Thermodynamic Standard State
8.6 The Thermodynamic Standard State The value of H reported for a reaction depends on the number of moles of reactants...or how much matter is contained in the system C 3 H 8 (g) + 5O 2 (g) > 3CO 2 (g)
More informationChemistry Heat Review. Heat: Temperature: Enthalpy: Calorimetry: Activation energy:
Chemistry Heat Review Name Date Vocabulary Heat: Temperature: Enthalpy: Calorimetry: Activation energy: Formulas Heat of phase change Heat for temperature increase Heat of reaction Endothermic/Exothermic
More informationTopic 05 Energetics : Heat Change. IB Chemistry T05D01
Topic 05 Energetics 5.1-5.2: Heat Change IB Chemistry T05D01 5.1 Exothermic and endothermic reactions - 1 hour 5.1.1 Define the terms exothermic reaction, endothermic reaction and standard enthalpy change
More informationThermochemistry. Section The flow of energy
Thermochemistry Section 17.1 - The flow of energy What is Energy? Energy is the capacity for doing work or supplying heat Energy does not have mass or volume, and it can only be detected because of its
More informationTHE ENERGY OF THE UNIVERSE IS CONSTANT.
Chapter 6 Thermochemistry.notebook Chapter 6: Thermochemistry Jan 29 1:37 PM 6.1 The Nature of Energy Thermodynamics: The study of energy and its interconversions Energy: the capacity to do work or to
More informationChapter 17 Thermochemistry
Chapter 17 Thermochemistry Section 17.1 The Flow of Energy Heat and Work OBJECTIVES: Explain how energy, heat, and work are related. 2 Section 17.1 The Flow of Energy Heat and Work OBJECTIVES: Classify
More informationAP CHEMISTRY NOTES 4-1 THERMOCHEMISTRY: ENTHALPY AND ENTROPY
AP CHEMISTRY NOTES 4-1 THERMOCHEMISTRY: ENTHALPY AND ENTROPY Reaction Rate how fast a chemical reaction occurs Collision Theory In order for a chemical reaction to occur, the following conditions must
More informationThermochemistry. Energy and Chemical Change
Thermochemistry Energy and Chemical Change Energy Energy can change for and flow, but it is always conserved. The Nature of Energy Energy the ability to do work or produce heat Potential energy Kinetic
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 informationCP Chapter 17 Thermochemistry
CP Chapter 17 Thermochemistry Thermochemistry Thermochemistry is the study of energy that occur during chemical reactions and phase changes (changes of state) The Nature of Energy Energy is the ability
More informationTHERMOCHEMISTRY CHAPTER 11
THERMOCHEMISTRY CHAPTER 11 ENERGY AND HEAT nthermochemistry: The study of the energy changes that accompany chemical reactions and changes in the physical states of matter. ENERGY AND HEAT nwork: Energy
More informationChapter 5 Practice Multiple Choice & Free
Name Response 1. A system has an increase in internal energy, E, of 40 kj. If 20 kj of work, w, is done on the system, what is the heat change, q? a) +60 kj d) -20 kj b) +40 kj e) -60 kj c) +20 kj 2. Which
More informationTypes of Energy Calorimetry q = mc T Thermochemical Equations Hess s Law Spontaneity, Entropy, Gibb s Free energy
Unit 7: Energy Outline Types of Energy Calorimetry q = mc T Thermochemical Equations Hess s Law Spontaneity, Entropy, Gibb s Free energy Energy Energy is the ability to do work or produce heat. The energy
More informationChapter 8. Thermochemistry
Chapter 8 Thermochemistry Copyright 2001 by Harcourt, Inc. All rights reserved. Requests for permission to make copies of any part of the work should be mailed to the following address: Permissions Department,
More 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 informationAdditional Calculations: 10. How many joules are required to change the temperature of 80.0 g of water from 23.3 C to 38.8 C?
Additional Calculations: 10. How many joules are required to change the temperature of 80.0 g of water from 23.3 C to 38.8 C? q = m C T 80 g (4.18 J/gC)(38.8-23.3C) = 5183 J 11. A piece of metal weighing
More informationAP* Chemistry THERMOCHEMISTRY
AP* Chemistry THERMOCHEMISTRY Let s begin with terms for you to master: Heat (q) Two systems with different temperatures that are in thermal contact will exchange thermal energy, the quantity of which
More information2 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
CHEMISTRY & YOU Chapter 17 Thermochemistry 17.1 The Flow of Energy 17. Measuring and Expressing Enthalpy Changes 17.3 Heat in Changes of State 17.4 Calculating Heats of Reaction Why does sweating help
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 informationIntroduction to Thermochemistry. Thermochemistry Unit. Definition. Terminology. Terminology. Terminology 07/04/2016. Chemistry 30
Thermochemistry Unit Introduction to Thermochemistry Chemistry 30 Definition Thermochemistry is the branch of chemistry concerned with the heat produced and used in chemical reactions. Most of thermochemistry
More informationChapter 5 Thermochemistry
Chapter 5 Thermochemistry Energy -Very much a chemistry topic Every chemical change has an accompanying change of. Combustion of fossil fuels The discharging a battery Metabolism of foods If we are to
More informationGilbert Kirss Foster. Chapter 9. Thermochemistry. Energy Changes in Chemical Reactions
Gilbert Kirss Foster Chapter 9 Thermochemistry Energy Changes in Chemical Reactions Chapter Outline 9.1 Energy as a Reactant or Product 9.2 Transferring Heat and Doing Work 9.3 Enthalpy and Enthalpy Changes
More informationCRHS Academic Chemistry Unit 15 Thermochemistry HOMEWORK. Due Date Assignment On-Time (100) Late (70)
Name Period CRHS Academic Chemistry Unit 15 Thermochemistry HOMEWORK Due Date Assignment On-Time (100) Late (70) 15.1 15.2 15.3 15.4 Warm Ups Extra Credit Notes, Homework, Exam Reviews and Their KEYS located
More informationHeat. Heat Terminology 04/12/2017. System Definitions. System Definitions
System Definitions Heat Physical Science 20 Ms. Hayduk Heat Terminology System: the part of the universe being studied (big Earth, or small one atom) Surroundings: the part of the universe outside the
More informationChapter 8 Thermochemistry: Chemical Energy. Chemical Thermodynamics
Chapter 8 Thermochemistry: Chemical Energy Chapter 8 1 Chemical Thermodynamics Chemical Thermodynamics is the study of the energetics of a chemical reaction. Thermodynamics deals with the absorption or
More informationChapter 5 Principles of Chemical Reactivity: Energy and Chemical Reactions
Chapter 5 Principles of Chemical Reactivity: Energy and Chemical Reactions Jeffrey Mack California State University, Sacramento Energy & Chemistry Questions that need to be addressed: How do we measure
More information_ + Units of Energy. Energy in Thermochemistry. Thermochemistry. Energy flow between system and surroundings. 100º C heat 50º C
Units of Energy Like we saw with pressure, many different units are used throughout the world for energy. SI unit for energy 1kg m 1J = 2 s 2 Joule (J) calorie (cal) erg (erg) electron volts (ev) British
More informationThermochemistry. Chapter 6. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Thermochemistry Chapter 6 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Energy is the capacity to do work. Radiant energy comes from the sun and is earth s
More informationJune Which is a closed system? (A) burning candle (B) halogen lightbulb (C) hot water in a sink (D) ripening banana
June 2005 28. Which is a closed system? burning candle halogen lightbulb hot water in a sink ripening banana 29. Which involves the greatest energy change? chemical reaction nuclear reaction phase change
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 informationAll chemical reactions involve changes in energy. Typically this energy comes in the form of heat.
Topic: Thermochemistry Essential Question: How does energy flow in chemical reactions? Name: Class: Date: / / Period: All chemical reactions involve changes in energy. Typically this energy comes in the
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 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 informationChapter 5 THERMO. THERMO chemistry. 5.4 Enthalpy of Reactions 5.5 Calorimetry 5.6 Hess s Law 5.7 Enthalpies of Formation
Chapter 5 THERMO THERMO chemistry 5.4 Enthalpy of Reactions 5.5 Calorimetry 5.6 Hess s Law 5.7 Enthalpies of Formation Chemical Equations 1 st WRITE the Chemical Equation 2 nd BALANCE the Chemical Equation
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 information2 nd Semester Study Guide 2016
Chemistry 2 nd Semester Study Guide 2016 Name: Unit 6: Chemical Reactions and Balancing 1. Draw the remaining product 2. Write a balanced equation for the following reaction: The reaction between sodium
More informationThermochemistry. Energy and Chemical Change
Thermochemistry Energy and Chemical Change Energy Energy can change for and flow, but it is always conserved. The Nature of Energy Energy the ability to do work or produce heat Potential energy Kinetic
More information2 nd Semester Study Guide 2017
Chemistry 2 nd Semester Study Guide 2017 Name: KEY Unit 6: Chemical Reactions and Balancing 1. Draw the remaining product 2. Write a balanced equation for the following reaction: The reaction between sodium
More information2. Calculate the heat change in joules when 45.2 g of steam at C condenses to water at the same temperature.!
Chem L3 Worksheet:Thermochemistry: Chapter 11 Page 1 Water Heating Cooling curve Problems ( Stairstep ): pp. 292-325, 549-556 1. How much heat is released when 65.0 g of steam cools from 150.0 C to 130.0
More information(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
More informationCRHS Academic Chemistry Unit 15 Thermochemistry HOMEWORK. Due Date Assignment On-Time (100) Late (70)
Name KEY Period CRHS Academic Chemistry Unit 15 Thermochemistry HOMEWORK Due Date Assignment On-Time (100) Late (70) 15.1 15.2 15.3 15.4 Warm Ups Extra Credit Notes, Homework, Exam Reviews and Their KEYS
More informationEnergy and Chemical Change
Energy and Chemical Change Section 16.1 Energy In your textbook, read about the nature of energy. In the space at the left, write true if the statement is true; if the statement is false, change the italicized
More information11B, 11E Temperature and heat are related but not identical.
Thermochemistry Key Terms thermochemistry heat thermochemical equation calorimeter specific heat molar enthalpy of formation temperature enthalpy change enthalpy of combustion joule enthalpy of reaction
More information2. What is a measure of the average kinetic energy of particles? (A) heat capacity (B) molar enthalpy (C) specific heat (D) temperature
Thermochemistry #1 Chemistry 3202 Name: 1. Classify the following systems as open or closed a) glass of cold water b) a gel filled freezer pack c) a burning candle d) a fluorescent lightbulb e) hot water
More informationThe following gas laws describes an ideal gas, where
Alief ISD Chemistry STAAR Review Reporting Category 4: Gases and Thermochemistry C.9.A Describe and calculate the relations between volume, pressure, number of moles, and temperature for an ideal gas as
More information3. When the external pressure is kpa torr, water will boil at what temperature? a C b C c. 100 C d. 18 C
Chemistry EOC Review 5: Physical Behavior of Matter 1. Which gas is monatomic at STP? a. chlorine b. fluorine c. neon d. nitrogen 2. What Kelvin temperature is equal to 25 C? a. 248 K b. 298 K c. 100 K
More informationThermodynamics Test Clio Invitational January 26, 2013
Thermodynamics Test Clio Invitational January 26, 2013 School Name: Team Number: Variables specified: s = specific heat C = heat capacity H f = heat of fusion H v = heat of vaporization Given information:
More informationFirst Law of Thermodynamics: energy cannot be created or destroyed.
1 CHEMICAL THERMODYNAMICS ANSWERS energy = anything that has the capacity to do work work = force acting over a distance Energy (E) = Work = Force x Distance First Law of Thermodynamics: energy cannot
More informationDETERMINING AND USING H
DETERMINING AND USING H INTRODUCTION CHANGES IN CHEMISTRY Chemistry is the science that studies matter and the changes it undergoes. Changes are divided into two categories: physical and chemical. During
More informationChapter 6 Problems: 9, 19, 24, 25, 26, 27, 31-33, 37, 39, 43, 45, 47, 48, 53, 55, 57, 59, 65, 67, 73, 78-82, 85, 89, 93
Chapter 6 Problems: 9, 19, 24, 25, 26, 27, 31-33, 37, 39, 43, 45, 47, 48, 53, 55, 57, 59, 65, 67, 73, 78-82, 85, 89, 93 Chapter 6 Thermochemistry The study of chemical reactions and the energy changes
More informationThermochemistry. Energy (and Thermochemistry) World of Chemistry Chapter 10. Energy. Energy
Thermochemistry Thermodynamics is the science of the relationship between heat and other forms of energy. (and Thermochemistry) World of Chemistry Chapter 10 is defined as the ability to do work or produce
More informationChapter 6 Energy and Chemical Change. Brady and Senese 5th Edition
Chapter 6 Energy and Chemical Change Brady and Senese 5th Edition Index 6.1 An object has energy if it is capable of doing work 6.2 Internal energy is the total energy of an object s molecules 6.3 Heat
More informationThe Nature of Energy Energy is the ability to do work or produce Heat, q or Q, is ; flows due to temperature differences (always to )
CP Chapter 17 Thermochemistry 2014-2015 Thermochemistry Thermochemistry is the study of energy that occur during chemical and physical changes (changes of state) The Nature of Energy Energy is the ability
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 informationThermochemistry. Energy. 1st Law of Thermodynamics. Enthalpy / Calorimetry. Enthalpy of Formation
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 of motion:
More informationEnergy and Chemical Change
Energy and Chemical Change Section 15.1 Energy In your textbook, read about the nature of energy. In the space at the left, write true if the statement is true; if the statement is false, change the italicized
More informationPlease print: Provided information: A periodic table and conversion chart are provided for you inside this exam booklet.
Please print: Last name: First name: Chem 1061 Exam 3 Fall 2004 Andy Aspaas, Instructor Tuesday, November 9, 2004 Instructions: Time: You have 85 minutes to complete this exam. Allowed items: This exam
More informationMeasuring and Expressing Enthalpy Changes. Copyright Pearson Prentice Hall. Measuring and Expressing Enthalpy Changes. Calorimetry
Measuring and Expressing Enthalpy Changes A burning match releases heat to its surroundings in all directions. How much heat does this exothermic reaction release? You will learn to measure heat flow in
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 informationGuided Notes and Practice- Topi 5.1: Calorimetry and Enthalpy Calculations
Name: Date: Pd: Guided Notes and Practice- Topi 5.1: Calorimetry and Enthalpy Calculations Endothermic vs. Exothermic 1. Label each ΔH value as being exothermic or endothermic. Thermochemical Equations
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 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 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 informationChapter 11. Thermochemistry: Heat & Chemical Change
Chapter 11 Thermochemistry: Heat & Chemical Change The Flow of Energy Thermochemistry: Study of heat changes that occur during physical processes and chemical reactions Energy Energy is the capacity to
More informationIB Chemistry Solutions Gasses and Energy
Solutions A solution is a homogeneous mixture it looks like one substance. An aqueous solution will be a clear mixture with only one visible phase. Be careful with the definitions of clear and colourless.
More informationTHERMOCHEMISTRY. This section explains the relationship between energy and heat, and distinguishes between heat capacity and specific heat.
I Name _ Date _ Class _ THERMOCHEMISTRY SECTION 17.1 THE FLOW OF ENERGY-HEAT AND WORK (pages 505-510) This section explains the relationship between energy and heat, and distinguishes between heat capacity
More informationTHERMOCHEMISTRY & 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 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 information