Energy: Heat, Nutrients, and Enthalpy Page 13
|
|
- Shawn Summers
- 6 years ago
- Views:
Transcription
1 V. Thermochemistry A. Thermochemistry is concerned with the B. Such reactions and changes are. VI. Chemical Reactions A. Chemical compounds contain B. Chemical potential energy. C. In chemical reactions, D. Exothermic reactions. Example: E. Endothermic reactions. Example: VII. Enthalpy A. Enthalpy ( ) is defined as the. B. The in enthalpy (not the actual enthalpy) is measured and represents The ( ) is the change in enthalpy for a reaction. C. Hrxn = C. THE SIGN OF Hrxn 1. Endothermic: Reactants heat; therefore, Hproducts Hreactants, and Hrxn is. 2. Exothermic: Reactants heat; therefore, Hproducts Hreactants, and Hrxn is. E. Hrxn = (at constant pressure) VIII. Thermochemical Equations A. Express the amount of during reactions. B. Balanced thermochemical equations include and, expressed as the. Energy: Heat, Nutrients, and Enthalpy Page 13
2 IX. Endothermic Processes 1. Energy is. Certain chemical reactions and phase changes require energy. 2. Activation energy is the. Energy must be. 3. Reactants have energy than products. 4. Example: A cold pack can be used to ice down a knee injury. When the pack is opened and squeezed, an inner membrane releases ammonium nitrate into water. Heat is the knee and is by the cold pack. X. Exothermic Processes A. Energy is. According to the Law of Conservation of Energy, B. Once sufficient activation energy is added, the reaction. C. Reactants have energy than products. D. Example: A heat pack can warm your hands on a cold day. When the pack is opened, oxygen from the air reacts with iron in the pack. Energy is. Energy: Heat, Nutrients, and Enthalpy Page 14
3 XI. Changes of Phase A. Phase changes are. B. Phase changes always occur with and can be. XII. Molar Enthalphies Phase Changes for Water H2O(g) Hvap = kj Enthalpy Hcond = 40.7 kj H2O(l) Hfusion = kj Hsolid = 6.01 kj H2O(s) The energy of the system increases as ice melts and then vaporizes, as illustrated by the upward arrows. The downward arrows indicate that the energy of the system decreases as water vapor condenses and then solidifies. A. Molar enthalpy (heat) of vaporization: = 1. Vaporization or ( ): H 2 O ( ) H 2 O ( ) 2. process 3. Hvap is. Energy: Heat, Nutrients, and Enthalpy Page 15
4 B. Molar enthalpy (heat) of fusion: = 1. Fusion or ( ): H 2 O ( ) H 2 O ( ) 2. process 3. Hfus is. C. Molar enthalpy (heat) of condensation: = 1. Condensation ( ): H 2 O ( ) H 2 O ( ) 2. process 3. Same numerical value but opposite sign of Hvap. Hcond is. D. Molar enthalpy (heat) of solidification: = 1. Solidification or ( ): H 2 O ( ) H 2 O ( ) 2. process 3. Same numerical value but opposite sign of Hfus. Hsolid is. E. Sublimation ( ) and deposition ( ) encompass two phase changes. XIII. Heating Curve for Water 140 C 120 C T E M P E R A T U R E ( C) 100 C 80 C 60 C 40 C 20 C 0 C -20 C -40 C ENERGY Kinetic Energy: Potential Energy: Energy: Heat, Nutrients, and Enthalpy Page 16
5 Phase Change State Change IMF Energy Endo/Exo Sign on q or ΔH To calculate heat released or absorbed during phase changes, use the equation. Example: How much energy is required to melt 36.0 grams of water? The heat capacity for water varies for different phases. Specific heat (c) for liquid water = Specific heat (c) for solid water (ice) = Specific heat (c) for gaseous water (steam) = Example: How much heat is required to heat 5 grams of ice from 10 C to 70 C? Water is going through three processes: Heat (q) must be calculated for each process, and the three values must be added together to determine the total amount of heat required. XIV. Phase Diagram A. Defined: Energy: Heat, Nutrients, and Enthalpy Page 17
6 B. Diagram differs for different substances because of different and points. 1. Freezing point: 2. Boiling point: C. Triple point: D. Critical point: XV. Combustion A. Combustion is the. 1. For biological systems, are used as fuel. 2. also undergo combustion reactions and provide warmth and fuel for transportation. B. Combustion is. D. STANDARD ENTHALPIES OF COMBUSTION:. When symbolized by, the changes were determined with all reactants and products at standard conditions ( ). Substance Formula H 0 comb Sucrose C 12 H 22 O 12 (s) 5644 kj/mol Octane C 8 H 18 (l) 5471 kj/mol Glucose C 6 H 12 O 6 (s) 2808 kj/mol Propane C 3 H 8 (g) 2219 kj/mol Methane CH 4 (g) 891 kj/mol Hydrogen H 2 (g) 286 kj/mol Combustion Calculation Practice 1. How much heat is evolved when 54.0 grams of glucose (C6H12O6) is burned? C6H12O6 (s) + 6O2(g) 6CO2 (g) + 6H2O (l) Hcomb = 2808 kj/mol 2. How much thermal energy is produced by burning 12 g of octane? Energy: Heat, Nutrients, and Enthalpy Page 18
7 3. The heat of combustion of carbon to carbon dioxide is kj/mol. Calculate the heat released upon formation of 35.2 g CO2 from carbon and oxygen gas. C (s) + O2 (g) CO2 (g) Hcomb = kj/mol 4. How much heat is released by the combustion of 206 g of hydrogen gas? [ Hcomb = 286 kj/mol]. 5. How many kilojoules of heat would be provided by the combustion of 10.0 g of butane? [ Hcomb = 2878 kj/mol]. 6. What mass of propane (C3H8) must be burned in a barbecue grill to release 4560 kj of heat? The Hcomb of propane is 2219 kj/mol. X. Entropy and Spontaneous Processes A. Entropy ( ) is a measure of. It is also referred to as a measure of the or of a system. Entropy as the number of possible arrangements of particles. Entropy of Solid Entropy of Liquid Entropy of Gas B. Processes that result in greater entropy are, like ice melting. For example, messing up your bedroom is not hard to do! C. Processes that result in less entropy are ; energy must be supplied. For example, cleaning up your messy bedroom takes energy; it doesn t happen automatically! D. The states that processes always proceed in such a way that the entropy of the universe. E. ( ) is similar to change in enthalpy. S system = If entropy increases, S products S reactants and S system is. If entropy decreases, S products S reactants and S system is. Energy: Heat, Nutrients, and Enthalpy Page 19
8 F. Spontaneity can sometimes be. Increases entropy ( Ssystem > 0) Decreases entropy ( Ssystem < 0) Prediction Practice Indicate whether the Ssystem is greater than (>) or less than (<) zero, and predict the sign of Ssystem (+ or ) for each of the following. 1. ClF (g) + F2 (g) ClF3 (g) 2. NH3 (g) NH3 (aq) 3. CH3OH (l) CH3OH (aq) 4. C10H8 (l) C10H8 (s) 5. Fe (s) + Zn 2 + (aq) Fe 2 + (aq) + Zn (s) 6. CaCl 2 (s) Ca+ (aq) + 2Cl (aq) 7. H 2 O (l) H 2 O (g) 8. 2H2 (g) + O2 (g) 2H2O (l) 9. N2H4 (l) + 2H2O2 (l) N2 (g) + 4H2O (g) 10. HgS (s) + O2 (g) Hg (l) + SO2 (g) Energy: Heat, Nutrients, and Enthalpy Page 20
All 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 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. 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 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 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 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 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 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 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 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 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 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 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 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 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 informationChapter 5 Practice Multiple Choice & Free
Name Response 1. A system has an increase in internal energy, E, of 40 kj. If 20 kj of work, w, is done on the system, what is the heat change, q? a) +60 kj d) -20 kj b) +40 kj e) -60 kj c) +20 kj 2. Which
More informationName: Thermochemistry. Practice Test C. General Chemistry Honors Chemistry
Name: Thermochemistry C Practice Test C General Chemistry Honors Chemistry 1 Objective 1: Use the relationship between mass, specific heat, and temperature change to calculate the heat flow during a chemical
More informationChemistry Heat Review. Heat: Temperature: Enthalpy: Calorimetry: Activation energy:
Chemistry Heat Review Name Date Vocabulary Heat: Temperature: Enthalpy: Calorimetry: Activation energy: Formulas Heat of phase change Heat for temperature increase Heat of reaction Endothermic/Exothermic
More 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 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 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 informationKinetic energy is the energy of motion (of particles). Potential energy involves stored energy (energy locked up in chemical bonds)
Enthalpy (H) Enthalpy (H) is the total energy amount (Epotential + Ekinetic) of a system during a chemical reaction under constant temperature and pressure conditions. Kinetic energy is the energy of motion
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 informationChapter 15 Energy and Chemical Change
Chapter 15 Energy and Chemical Change Chemical reactions usually absorb or release energy. Section 1: Energy Section 2: Heat Section 3: Thermochemical Equations Section 4: Calculating Enthalpy Change Section
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 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 informationChemistry Grade : 11 Term-3/Final Exam Revision Sheet
Chemistry Grade : 11 Term-3/Final Exam Revision Sheet Exam Date: Tuesday 12/6/2018 CCS:Chem.6a,6b,6c,6d,6e,6f,7a,7b,7d,7c,7e,7f,1g Chapter(12):Solutions Sections:1,2,3 Textbook pages 378 to 408 Chapter(16):Reaction
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 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 informationName Energy Test period Date
Name Energy Test period Date 1. The temperature 30. K expressed in degrees Celsius is 1) 243ºC 2) 243ºC 3) 303ºC 4) 303ºC 2. The potential energy diagram for a chemical reaction is shown below. 4. A sample
More informationName: General Chemistry Chapter 11 Thermochemistry- Heat and Chemical Change
Name: General Chemistry Chapter 11 Thermochemistry- Heat and Chemical Change Notepack 1 Section 11.1: The Flow of Energy Heat (Pages 293 299) 1. Define the following terms: a. Thermochemistry b. Energy
More informationChapter 8 Thermochemistry
William L Masterton Cecile N. Hurley http://academic.cengage.com/chemistry/masterton Chapter 8 Thermochemistry Edward J. Neth University of Connecticut Outline 1. Principles of heat flow 2. Measurement
More informationName: REGENTS CHEMISTRY
Name: REGENTS CHEMISTRY 1 Key Ideas Matter is classified as a pure substance or as a mixture of substances. (3.1q) Mixtures are composed of two or more different substances that can be separated by physical
More informationMr Chiasson Advanced Chemistry 12 / Chemistry 12 1 Unit B: Thermochemical Changes
Mr Chiasson Advanced Chemistry 12 / Chemistry 12 1 Unit B: Thermochemical Changes Students will be expected to: Compare the molar enthalpies of several combustion reactions involving organic compounds.
More informationThermochemistry. Chapter 6. Concept Check 6.1. Concept Check 6.2. Solution
Chapter 6 Thermochemistry Concept Check 6.1 A solar-powered water pump has photovoltaic cells on protruding top panels. These cells collect energy from sunlight, storing it momentarily in a battery, which
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 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 informationsolid IMF>liquid IMF>gas IMF Draw a diagram to represent the 3 common states of matter of a given substance: solid liquid gas
Thermochemistry Part 1 Notes States of Matter and Intermolecular Forces (IMF) Chemistry HP At the end of this unit, students should be able to: Describe the various states of matter in terms of kinetic
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 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 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 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 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 informationThermochemistry. Using Heats of Reaction - Hess s Law - Standard Enthalpies of Formation - Fuels Foods, Commercial Fuels, and Rocket Fuels
Thermochemistry Understanding Heats of Reaction - Energy and Its Units - Heat of Reaction - Enthalpy and Enthalpy Change - Thermochemical Equations - Applying Stoichiometry to Heats of Reaction - Measuring
More informationChemical Thermodynamics
Chemical Thermodynamics 1 Thermodynamics Thermodynamics is a Greek term which means, heat power. Thermodynamics is the study of energy and its transformations. 2 Thermodynamics Thermochemistry how we observe,
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 informationChapter 16 Theories of Energy Changes
{Read p. 624 and 626 to understand concepts} Class discussion for chapter 17.3 Chapter 16 Theories of Energy Changes Section 16.1A Temperature change and Heat THERMODYNAMICS - the study of energy and energy
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 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 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 informationUnit 7 Thermochemistry Chemistry 020, R. R. Martin
Unit 7 Thermochemistry Chemistry 020, R. R. Martin 1. Thermochemistry Heat is a form of energy - which may take many forms: - Kinetic energy due to motion, ½ mv 2 - Potential energy due to position - Electrical
More informationEnergy Changes in Reactions p
Energy Changes in Reactions p.126 210 Heat vs. temperature: Heat is a form of energy, it is transferred from one system to another Temperature is an indication of the intensity of heat, it measures the
More informationCHEMISTRY - CLUTCH CH CHEMICAL THERMODYNAMICS.
!! www.clutchprep.com CONCEPT: THERMOCHEMICAL PROCESSES is the branch of physical science concerned with heat and its transformations to and from other forms of energy. In terms of a chemical reaction,
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 informationNo Brain Too Small CHEMISTRY Energy changes ( ) & Expired ( ) QUESTIONS QUESTION 1 (2016:3)
QUESTION 1 (2016:3) QUESTIONS (iii) Pentane combustion: C5H12(l) + 8O2(g) 5CO2(g) + 6H2O(l) Δr H o = 3509 kj mol 1 Hexane, C6H14, like pentane, will combust (burn) in sufficient oxygen to produce carbon
More informationPractice Packet Unit 3: Phase Changes & Heat
Regents Chemistry: Practice Packet Unit 3: Phase Changes & Heat Name: Assess Yourself: Lesson 1: Lesson 2: Lesson 3: Lesson 4: Vocab: 1 Review (Things you need to know in order to understand the new stuff
More 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 informationUnit 7 Kinetics and Thermodynamics
17.1 The Flow of Energy Heat and Work Unit 7 Kinetics and Thermodynamics I. Energy Transformations A. Temperature 1. A measure of the average kinetic energy of the particles in a sample of matter B. Heat
More informationCHM 111 Dr. Kevin Moore
CHM 111 Dr. Kevin Moore Kinetic Energy Energy of motion E k 1 2 mv 2 Potential Energy Energy of position (stored) Law of Conservation of Energy Energy cannot be created or destroyed; it can only be converted
More informationUnit 10 Thermodynamics, Kinetics and Equilibrium Notes
Unit 10 Thermodynamics, Kinetics and Equilibrium Notes What is Thermodynamics? Almost all chemical reactions involve a between the and its. Thermo = Dynamics = What is energy? What is heat? Thermochemistry
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 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 informationWarm up. 1) What is the conjugate acid of NH 3? 2) What is the conjugate base of HNO 2? 3) If the ph is 9.2, what is the [H 3 O + ], poh, and [OH - ]?
Warm up 1) What is the conjugate acid of NH 3? 2) What is the conjugate base of HNO 2? 3) If the ph is 9.2, what is the [H 3 O + ], poh, and [OH - ]? 4) What is the concentration of H 2 SO 4 if 30.1 ml
More informationUnit 5: Spontaneity of Reaction. You need to bring your textbooks everyday of this unit.
Unit 5: Spontaneity of Reaction You need to bring your textbooks everyday of this unit. THE LAWS OF THERMODYNAMICS 1 st Law of Thermodynamics Energy is conserved ΔE = q + w 2 nd Law of Thermodynamics A
More 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 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 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 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 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 informationGeneral Chemistry 1 CHM201 Unit 3 Practice Test
General Chemistry 1 CHM201 Unit 3 Practice Test 1. Heat is best defined as a. a substance that increases the temperature and causes water to boil. b. a form of potential energy. c. a form of work. d. the
More informationENTHALPY CHANGE CHAPTER 4
ENTHALPY CHANGE CHAPTER 4 ENTHALPY Is the total energy of a system. E k = Kinetic energy. Vibrational Rotational Translational E due to motion H = E k + E p E P = Potential energy Attractive force b/w
More informationReaction Energy. Thermochemistry
Reaction Energy Thermochemistry Thermochemistry The study of the transfers of energy as heat that accompany chemical reactions & physical changes Thermochemistry -In studying heat changes, think of defining
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
Chapter 6 Thermochemistry Section 5.6 The Kinetic Molecular Theory of Gases http://www.scuc.txed.net/webpages/dmackey/files /chap06notes.pdf ..\..\..\..\..\..\Videos\AP Videos\Thermochemistry\AP
More informationUnit 5 A3: Energy changes in industry
1. ENTHALPY CHANGES Unit 5 A3: Energy changes in industry 1.1 Introduction to enthalpy and enthalpy changes 2 1.2 Enthalpy profile diagrams 2 1.3 Activation energy 3 1.4 Standard conditions 5 1.5 Standard
More informationGravity is a force which keeps us stuck to the earth. The Electrostatic force attracts electrons to protons in an atom.
Energy Relations in Chemistry: Thermochemistry The Nature of Energy Sugar you eat is "combusted" by your body to produce CO 2 and H 2 O. During this process energy is also released. This energy is used
More informationCh. 6 Enthalpy Changes
Ch. 6 Enthalpy Changes Energy: The capacity to do work. In Physics, there are 2 main types of energy Kinetic (energy of motion) = ½ mv 2 Potential (energy of position due to gravity)= mgh In Chemistry,
More informationEnthalpy. Enthalpy. Enthalpy. Enthalpy. E = q + w. Internal Energy at Constant Volume SYSTEM. heat transfer in (endothermic), +q
heat transfer in (endothermic), +q heat transfer out (exothermic), -q SYSTEM E = q + w w transfer in (+w) w transfer out (-w) Internal Energy at Constant Volume E = KE + PE ΔE = q + w Because most systems,
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 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 informationUNIT 15 - Reaction Energy & Reaction Kinetics. I. Thermochemistry: study of heat in chemical reactions and phase changes
I. Thermochemistry: study of heat in chemical reactions and phase changes II. A. Heat equation (change in temperature): Q = m. C. p T 1. Q = heat (unit is Joules) 2. m = mass (unit is grams) 3. C p = specific
More informationAP* Chemistry THERMOCHEMISTRY
AP* Chemistry THERMOCHEMISTRY Let s begin with terms for you to master: Energy (E) the ability to do work or produce heat ; the sum of all potential and kinetic energy in a system is known as the internal
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 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 informationEnergy and Chemical Change
Energy and Chemical Change Section 15.1 Energy Section 15.2 Heat Section 15.3 Thermochemical Equations Section 15.4 Calculating Enthalpy Change Section 15.5 Reaction Spontaneity Click a hyperlink or folder
More informationWork hard. Be nice. 100% EVERYDAY.
Name: Period: Date: UNIT 10: Energy Lesson 1: Entropy vs. Enthalpy By the end of today, you will have an answer to: What conditions are favored during reactions? Definition Enthalpy is another word for
More informationEnergy and Chemical Change
Energy and Chemical Change Reviewing Vocabulary Match the definition in Column A with the term in Column B. h e d p c f a r m t j i s l u k n q g o Column A 1. The ability to do work or produce heat 2.
More informationChapter 6. Thermochemistry
Chapter 6 Thermochemistry This chapter develops for the student the concepts of thermochemistry. Upon completion of Chapter 6, the student should be able to: 1. Define and explain the following terms:
More informationThermodynamics. Thermodynamics1.notebook. December 14, Quality vs Quantity of Energy
Thermodynamics Quality vs Quantity of Energy Your textbook discusses the idea that although energy is conserved we face an energy crisis because the quality of energy we have available to do work like
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 informationSupplemental Activities. Module: Thermodynamics. Section: Second Law of Thermodynamics Key
Supplemental Activities Module: Thermodynamics Section: Second Law of Thermodynamics Key Spontaneity ACTIVITY 1 The purpose of this activity is to practice your understanding of the concept of spontaneous
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 informationENERGY (THERMOCHEMISTRY) Ch 1.5, 6, 9.10, , 13.3
ENERGY (THERMOCHEMISTRY) Ch 1.5, 6, 9.10, 11.5-11.7, 13.3 Thermochemistry Prediction and measurement of energy transfer, in the form of heat, that accompanies chemical and physical processes. Chemical
More informationLECTURE 4 Variation of enthalpy with temperature
LECTURE 4 Variation of enthalpy with temperature So far, we can only work at 25 C. Like c v we define a constant pressure heat capacity, c p, as the amount of heat energy needed to raise the temperature
More informationExam 1A. 4) Calculate the H 0 rxn in kj for this reaction. a) 6339 b) 5106 c) 775 d) 6535 e) 2909
Exam 1A 1) The molar solubility of a salt M 2 X 3 is 1.9 10 3 M. (M is the cation and X is the anion.) What is the value of Ksp for this salt? a) 1.5E-13 b) 2.7E-12 c) 2.5E-14 d) 8.9E-13 e) 3.8E-3 2) What
More informationCHEMISTRY - TRO 4E CH.6 - THERMOCHEMISTRY.
!! www.clutchprep.com CONCEPT: ENERGY CHANGES AND ENERGY CONSERVATION is the branch of physical science concerned with heat and its transformations to and from other forms of energy. is the branch of chemistry
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 informationThermochemistry-Part 1
Brad Collins Thermochemistry-Part 1 Chapter 7 Thermochemistry Thermodynamics: The study of energy Thermochemistry: The study of energy in chemical reactions Energy: The capacity to do work Work = force
More information