CHEMISTRY. Unit 4, Area of Study 1: Industrial Chemistry. Energy Profile Diagrams & the use of Delta H
|
|
- Agnes Rosanna Robbins
- 6 years ago
- Views:
Transcription
1 Watch this lesson online: CHEMISTRY Unit 4, Area of Study 1: Industrial Chemistry Energy Profile Diagrams & the use of Delta H 1
2 Key Knowledge energy pro-ile diagrams and the use of ΔH notation including: activation energy; alternative reaction pathways for catalysed reactions; and deduction of ΔH for an overall reaction given energy pro-iles or ΔH of two related reactions 2
3 Chemical energy The chemical energy of a substance is made up of its potential energy and kinetic energy. Potential energy attraction between nuclei and electrons Repulsion between electrons Repulsion between nuclei 3
4 Kinetic energy - movement of particles Movement of electrons Vibrations of and rotations around bonds. Actual movement in the substance (gases vs liquids and solids) 4
5 Enthalpy The chemical energy of a substance cannot be directly measured, but it can be determined theoretically. It is known as enthalpy or heat content and has the symbol H. However, a change in enthalpy, ΔH, for a chemical reaction can be determined. 5
6 Measuring enthalpy The change in temperature, ΔT, gives an indication of change in enthalpy. If temperature increases during the course of a reaction, then heat energy is being released to the surroundings by the reaction So enthalpy of the products is less than enthalpy of reactants. 6
7 Energy pro-ile diagram Exothermic reaction We can visualise this change using an energy pro-ile diagram: 7
8 If temperature decreases during the course of a reaction, then heat energy is being absorbed from the surroundings by the reaction So enthalpy of the products is greater than enthalpy of reactants. 8
9 Energy pro-ile diagram endothermic reaction To visualise the decrease in enthalpy when a temperature decrease occurs we can also use an energy pro-ile diagram: 9
10 De-inition of ΔH ΔH = H(products) H(reactants) So if the temp increases, H(products) < H(reactants), So ΔH is negative This is an exothermic reaction If the temp decreases H(products) > H(reactants), So ΔH is positive This is an endothermic reaction 10
11 We can recognise an exothermic reaction by the increase in temperature of the surroundings eg Combustion reactions, neutralization reactions Endothermic reactions are much less common. The temperature of the surroundings decreases eg chemical cold packs 11
12 Activation energy The activation energy is the amount of energy required to break the bonds of the reactants. It is the amount of energy needed to start a reaction. eg a spark to start a -ire, or to burn fuel in an engine. 12
13 Reversing the reaction If we were to turn products back into reactants, then the activation energy could still be determined from the energy pro-ile diagram: 13
14 Catalysts and activation energy A catalyst increases the rate of a reaction. It does this by creating an alternative energy pathway for the reaction. This pathway has a lower activation energy than the original reaction. 14
15 Sample exam question energy pro-ile diagrams The reaction A + B C involves a two step process. A + B X: ΔH positive and X C; ΔH negative Which one of the diagrams below best represents the energy changes during the course of the reaction? VCAA June 2007 Q19 15
Energetics. Topic
Energetics Topic 5.1 5.2 Topic 5.1 Exothermic and Endothermic Reactions?? total energy of the universe is a constant if a system loses energy, it must be gained by the surroundings, and vice versa Enthalpy
More informationBond Enthalpy and Activation Energy
Bond Enthalpy and Activation Energy Energy of a Chemical Reaction ΔH = ΔH (bonds broken) - ΔH (bonds formed) Add up all the energies of the broken bonds Add up all the energies of the bonds that are reformed
More information3. A forward reaction has an activation energy of 50 kj and a H of 100 kj. The PE. diagram, which describes this reaction, is
Kinetics Quiz 4 Potential Energy Diagrams 1. A catalyst increases the rate of a reaction by A. Increasing the concentration of the reactant(s) B. Decreasing the concentration of the reactant(s) C. Increasing
More informationNote: 1 calorie = 4.2 Joules
Enthalpy Changes All substances contain chemical energy, called enthalpy. Like any kind of energy it is measured in Joules (previously energy was measured in Calories). When reactions happen, energy is
More information5.1 Exothermic and endothermic reactions
Topic 5: Energetics 5.1 Exothermic and endothermic reactions Chemical reactions involve the breaking and making of bonds. Breaking bonds requires energy,whereas energy is given out when new bonds are formed.
More 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 informationWorksheet 5.2. Chapter 5: Energetics fast facts
Worksheet 52 Chapter 5: Energetics fast facts 51 Exothermic and endothermic reactions Energetics deals with heat changes in chemical reactions Enthalpy is the amount of heat energy contained in a substance
More informationUnit 13: Rates and Equilibrium- Guided Notes
Name: Period: What is a Chemical Reaction and how do they occur? Unit 13: Rates and Equilibrium- Guided Notes A chemical reaction is a process that involves of atoms Law of Conservation of : Mass is neither
More informationEnergetics. These processes involve energy exchanges between the reacting system and its surroundings.
Energetics Chemical reactions involve: the breaking of bonds between atoms the making of new bonds between atoms These processes involve energy exchanges between the reacting system and its surroundings.
More information3.2 Calorimetry and Enthalpy
3.2 Calorimetry and Enthalpy Heat Capacity Specific heat capacity (c) is the quantity of thermal energy required to raise the temperature of 1 g of a substance by 1 C. The SI units for specific heat capacity
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 informationCHEM3.4 Demonstrate understanding of thermochemical principles and the properties of particles and substances
CHEM3.4 Demonstrate understanding of thermochemical principles and the properties of particles and substances We have covered the underlined part so far. This is: Electron configurations with s, p, d orbitals
More informationDescribe how the inter-conversion of solids, liquids and gases are achieved and recall names used for these inter-conversions
Understand the arrangements, movements and energy of the particle in each of the 3 states of matter : solid, liquid and gas Describe how the inter-conversion of solids, liquids and gases are achieved and
More informationHEAT, TEMPERATURE, & THERMAL ENERGY. Work - is done when an object is moved through a distance by a force acting on the object.
HEAT, TEMPERATURE, & THERMAL ENERGY Energy A property of matter describing the ability to do work. Work - is done when an object is moved through a distance by a force acting on the object. Kinetic Energy
More informationNotes: Unit 10 Kinetics and Equilibrium
Name: Regents Chemistry: Mr. Palermo Notes: Unit 10 Kinetics and Equilibrium Name: KEY IDEAS Collision theory states that a reaction is most likely to occur if reactant particles collide with the proper
More informationChapter Introduction Lesson 1 Understanding Chemical Reactions Lesson 2 Types of Chemical Reactions Lesson 3 Energy Changes and Chemical Reactions
Chapter Introduction Lesson 1 Understanding Chemical Reactions Lesson 2 Types of Chemical Reactions Lesson 3 Energy Changes and Chemical Reactions Chapter Wrap-Up Changes in Matter A physical change does
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 informationEnergy: Heat, Nutrients, and Enthalpy Page 13
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,
More informationUnit 2: Chemical Kinetics Chemistry 30
Practice Questions Section 3.2 Factors Influencing Reaction Rate - Activation Energy 1. Answer the following questions based on the potential energy diagram shown here: a. Does the graph represent an endothermic
More informationUnit 3, Lesson 02: Enthalpy Changes in Chemical Reactions
Unit 3, Lesson 02: Enthalpy Changes in Chemical Reactions Chemical Potential Energy refers to the energy that is stored within an atom or molecule because of electrostatic attraction and repulsion between
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 informationCollision Theory. and I 2
Collision Theory To explain why chemical reactions occur, chemists have proposed a model, known as collision theory, which states that molecules must collide in order to react. These collisions can involve
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 informationChanges & Chemical Reactions. Unit 5
Changes & Chemical Reactions Unit 5 5 Types of Chemical Reactions Double Decomposition Replacement 1 2 3 4 5 Synthesis Single Replacement Combustion Continue Synthesis 2H 2 + O 2 2H 2 O Menu Decomposition
More informationPropose a method for measuring your results.
System vs. Surroundings In thermodynamics, a system is defined as that part of the universe that is under consideration (the part of the universe that you are studying). A hypothetical boundary separates
More information2013, 2011, 2009, 2008 AP
Lecture 15 Thermodynamics I Heat vs. Temperature Enthalpy and Work Endothermic and Exothermic Reactions Average Bond Enthalpy Thermodynamics The relationship between chemical reactions and heat. What causes
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 16.3 Phase Changes
Section 16.3 Phase Changes Solid Liquid Gas 3 Phases of Matter Density of Matter How packed matter is (The amount of matter in a given space) Solid: Liquid: Gas: High Density Medium Density Low Density
More informationName Chemistry / / Understanding Phase Changes
Name Chemistry / / Understanding Phase Changes As a piece of ice is exposed to a warmer environment, it begins to absorb heat. The heat causes the solid molecules to vibrate faster. Eventually, the ice
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 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 informationWhy do cold packs get cold?
Assignment #5 Temperature in Reactions LO: To determine which solute dissolves most endothermically and exothermically in water. EQ: What makes an endothermic reaction feel cold? (explain using bonds and
More informationName: Regents Chemistry: Mr. Palermo. Notes: Unit 7 Heat.
Name: Regents Chemistry: Mr. Palermo Notes: Unit 7 Heat 1 Name: KEY IDEAS Heat is a transfer of energy (usually thermal energy) from a body of higher temperature to a body of lower temperature. Thermal
More informationQuiz I: Thermodynamics
Quiz I: Thermodynamics SCH4U_2018-2019_V2 NAME: (Total Score: / 30) Multiple Choice (12) 1. What can be deduced from the following reaction profile? A. The reactants are less stable than the products and
More informationOCR Chemistry A H432
All the energy changes we have considered so far have been in terms of enthalpy, and we have been able to predict whether a reaction is likely to occur on the basis of the enthalpy change associated with
More information3.1 Metabolism and Energy
3.1 Metabolism and Energy Metabolism All of the chemical reactions in a cell To transform matter and energy Step-by-step sequences metabolic pathways Metabolic Pathways Anabolic reactions Build large molecules
More informationStudy Guide Chapter 5
Directions: Answer the following 1. When writing a complete ionic equation, a. what types of substances should be shown as dissociated/ionized? soluble ionic compounds, acids, bases b. What types of substances
More 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 informationThermodynamics: Entropy
Name: Band: Date: Thermodynamics: Entropy Big Idea: Entropy When we were studying enthalpy, we made a generalization: most spontaneous processes are exothermic. This is a decent assumption to make because
More informationChemical Equilibrium
Chemical Equilibrium Forward Rxn: A + B C + D Reverse Rxn: A + B C + D Written as: A + B C + D OR A + B C + D A reversible reaction has both an endothermic rxn and an exothermic rxn Reactants Exothermic
More informationFACTFILE: GCE CHEMISTRY
FACTFILE: GCE CHEMISTRY 2.9 KINETICS Learning Outcomes Students should be able to: 2.9.1 recall how factors, including concentration, pressure, temperature and catalyst, affect the rate of a chemical reaction;
More informationIn order for two molecules to react, they must with each other. When they collide they transfer among themselves.
Chemistry 12 Reaction Kinetics II Name: Date: Block: 1. Collision Theory 2. Activation Energy 3. Potential Energy Diagrams Collision Theory (Kinetic Molecular Theory) In order for two molecules to react,
More informationChemical reactions. C2- Topic 5
Chemical reactions C2- Topic 5 What is a chemical reaction? A chemical reaction is a change that takes place when one or more substances (called reactants) form one or more new substances (called products)
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 informationChapter 17. Preview. Lesson Starter Objectives Reaction Mechanisms Collision Theory Activation Energy The Activated Complex Sample Problem A
Preview Lesson Starter Objectives Reaction Mechanisms Collision Theory Activation Energy The Activated Complex Sample Problem A Section 1 The Reaction Process Lesson Starter The reaction H 2 + I 2 2HI
More informationChapter 17: Energy and Kinetics
Pages 510-547 S K K Chapter 17: Energy and Kinetics Thermochemistry: Causes of change in systems Kinetics: Rate of reaction progress (speed) Heat, Energy, and Temperature changes S J J Heat vs Temperature
More information10 Enthalpy changes Answers to Activity and Practice questions
Page 150 151 Activity: Measuring the enthalpy change for the reaction of zinc with copper sulfate solution 1 The graph should have: axes with scales and labels points plotted accurately a clean, smooth
More informationLesson 01 and 02: Introduction to Chemical Reaction Equations. 01 Chemical Reactions
Chemistry 11, Chemical Reactions, Unit 05 1 Lesson 01 and 02: Introduction to Chemical Reaction Equations 01 Chemical Reactions A chemical reaction is a process by which one or more substances may be transformed
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 information2.3.1 Enthalpy Changes Exam Questions
2.3.1 Enthalpy Changes Exam Questions 1. The standard enthalpy change of formation of hexane is 199 kj mol 1. Using the axes below, show the enthalpy profile diagram for the formation of hexane. On your
More informationChapter 6 CONSERVATION OF ENERGY AND MATTER
Chapter 6 CONSERVATION OF ENERGY AND MATTER Identifying Chemical Change (6.1) Chemical reactions: Process in which the physical and chemical properties of the original substance change as new substances
More informationEnthalpy Changes. Note: 1 calorie = 4.2 Joules
Enthalpy Changes All substances contain chemical energy, called enthalpy. Like any energy it is measured in Joules (previously energy was measured in Calories). When reactions happen, energy is given out
More information[4] Answer all the questions. Look at the energy profile for a reaction. What can you deduce about this reaction?
Answer all the questions. 1(a). Look at the energy profile for a reaction. What can you deduce about this reaction? Include the quantities A and B and a full explanation. [4] (b). Look at the equation.
More informationActivation Energy is the minimum amount of energy needed to start a chemical reaction.
5.3 Controlling Chemical Reactions Vocabulary: Activation energy Concentration Catalyst Enzyme Inhibitor - How do reactions get started? Chemical reactions won t begin until the reactants have enough energy.
More informationThermodynamics - Energy Relationships in Chemical Reactions:
Thermodynamics - Energy Relationships in Chemical Reactions: energy - The capacity to do work. Types of Energy: radiant-energy from the sun. potential-energy due to an objects position. chemical-energy
More informationEquilibrium Lesson Plan and Handout for Chemistry I. High Tech High. Jay A. Haron, Ph.D. April 24, 2007
Chemical Equilibrium Lesson Plan 1.. Equilibrium Lesson Plan and Handout for Chemistry I High Tech High Jay A. Haron, Ph.D. April 24, 2007. Chemical Equilibrium Lesson Plan 2 Equilibrium Lesson Plan and
More informationStudent Worksheet for Thermochemistry
Student Worksheet for Attempt to work the following practice problems after working through the sample problems in the videos. Answers are given on the last page(s). Relevant Equations/Information Specific
More informationI. Chemical Reactions that Involve Heat
Unit 12 Energy I. Chemical Reactions that Involve Heat Thermochemistry: study of changes in heat in chemical reactions. Endothermic: absorbs heat; temp. goes down Exothermic: releases heat; temp. goes
More informationName: Section: Score: /10 PRE LABORATORY ASSIGNMENT EXPERIMENT 7
Name: Section: Score: /10 PRE LABORATORY ASSIGNMENT EXPERIMENT 7 1. Is the sign of Δ r H for an exothermic reaction positive or negative? Why? 2. When 4.21 grams of potassium hydroxide are added to 250.
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 informationChapter 5 Thermochemistry
Chapter 5 Thermochemistry Learning Outcomes: Interconvert energy units Distinguish between the system and the surroundings in thermodynamics Calculate internal energy from heat and work and state sign
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 informationCHAPTER 17: THERMOCHEMISTRY. Mrs. Brayfield
CHAPTER 17: THERMOCHEMISTRY Mrs. Brayfield REVIEW What is the law of conservation of energy? It states that energy cannot be created or destroyed So the energy of any process is the same THERMOCHEMISTRY
More informationQ=mcDt. Chemistry 30 notes review of specific heat capacity. Thermodynamics the movement of thermal energy
Chemistry 30 notes review of specific heat capacity Thermodynamics the movement of thermal energy o Open system: both matter and energy are allowed to enter or leave the system. o Closed system: energy
More informationPractice Test: Energy and Rates of Reactions
Practice Test: Energy and Rates of Reactions NAME: /65 Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. (20 marks) 1. What is the symbol for
More informationScience 10. Unit 2: Chemistry. Book 6: energy changes in chemical reactions. Block: Name: Zukowski
Science 10 Unit 2: Chemistry Book 6: energy changes in chemical reactions Name: Zukowski Block: 1 How is energy involved in chemical processes? and energy are continually interacting in the world around
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 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 informationUNIT 9 IB MATERIAL KINETICS & THERMODYNAMICS
UNIT 9 IB MATERIAL KINETICS & THERMODYNAMICS Name: ESSENTIALS: Know, Understand, and Be Able To State that combustion and neutralization are exothermic processes. Calculate the heat energy change when
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 Ch. 8
Definitions I. Energy (E): capacity to do work. II. Heat (q): transfer of energy from a body at a high temp. to a body at a low temp. III. Reaction perspectives: A. System: the focus. B. Surroundings:
More information(g) 2NH 3. (g) ΔH = 92 kj mol 1
1 The uses of catalysts have great economic and environmental importance For example, catalysts are used in ammonia production and in catalytic converters (a) Nitrogen and hydrogen react together in the
More informationChemical Reactions and Energy
Topic 9 Chemical Reactions and Energy Unit 34 Energy changes in chemical reactions Unit 35 Hess s Law and its applications Key C o ncepts Energy changes in chemical reactions Nature of energy and internal
More informationChemistry (separate) for November PPE
1.1 Elements and 1.2 Atoms, formulae and Chapter 1 Atomic Structure and Periodic Table Identify symbols of elements from the periodic table Recognise the properties of elements and. Identify the elements
More informationBasics of Thermodynamics: Easy learning by Dr. Anjana Sen
Basics of Thermodynamics: Easy learning by Dr. Anjana Sen Part 1: Theory and concept Part 2: Definitions and equations Part 3: Laws of Thermodynamics Part 1: theory and concept Thermodynamics means conversion
More information[Thermochemistry] April Mr. Dvorsky
Energy and Rates [Thermochemistry] April 11 2011 SCH 4U1 Mr. Dvorsky Chemistry = the study of matter and its transformations Thermochemistry h = the study of energy changes that accompany these transformations
More informationChapter 6: Thermochemistry
Chapter 6: Thermochemistry 1. Light the Furnace: The Nature of Energy and Its Transformations a. Thermochemistry is the study of the relationships between chemistry and energy i. This means that we will
More informationEnergy Changes, Reaction Rates and Equilibrium. Thermodynamics: study of energy, work and heat. Kinetic energy: energy of motion
Energy Changes, Reaction Rates and Equilibrium Thermodynamics: study of energy, work and heat Kinetic energy: energy of motion Potential energy: energy of position, stored energy Chemical reactions involve
More informationChemistry 101 Chapter 10 Energy
Chemistry 101 Chapter 10 Energy Energy: the ability to do work or produce heat. Kinetic energy (KE): is the energy of motion. Any object that is moving has kinetic energy. Several forms of kinetic 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 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 informationCHAPTER 6: Chemical Energetics
CHAPTER 6: Chemical Energetics 6.1 Enthalpy Changes 6.2 Standard Enthalpy Changes 6.3 Hess' Law 6.4 Bond Energy Learning outcomes: (a) explain that some chemical reactions are accompanied by energy changes,
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 information1. Reactions can be followed by measuring changes in concentration, mass and volume of reactants and products.
Higher Chemistry - Traffic Lights Unit 1 CHEMICAL CHANGES AND STRUCTURE I know: Controlling the rate Collision theory and relative rates 1. Reactions can be followed by measuring changes in concentration,
More informationSUPPLEMENTARY TOPIC 3 ENERGY AND CHEMICAL REACTIONS
SUPPLEMENTARY TOPIC 3 ENERGY AND CHEMICAL REACTIONS Rearranging atoms. In a chemical reaction, bonds between atoms in one or more molecules (reactants) break and new bonds are formed with other atoms to
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 informationUnit 4, Lesson 03: Collision Theory and the Rates of Chemical Reactions Homework
Unit 4, Lesson 03: Collision Theory and the Rates of Chemical Reactions Homework Page 294, Q 13 16 13. Reaction: 2 ClO (g) Cl 2 (g) + O 2 (g) Potential Energy Diagram for Decomposition of ClO (g) activated
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 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 informations Traditionally, we use the calorie as a unit of energy. The nutritional Calorie, Cal = 1000 cal. Kinetic Energy and Potential Energy
AP Chemistry: Thermochemistry Lecture Outline 5.1 The Nature of Energy Thermodynamics is the study of energy and its transformations. Thermochemistry is the study of the relationships between chemical
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 informationS8P1C. STATES OF MATTER E.Q. WHAT ARE THE STATES OF MATTER? WHAT ARE THE CHARACTERISTICS OF EACH STATE OF MATTER?
S8P1C. STATES OF MATTER E.Q. WHAT ARE THE STATES OF MATTER? WHAT ARE THE CHARACTERISTICS OF EACH STATE OF MATTER? ATOMIC MODEL PROJECT BE CREATIVE!!! MIXTURES VS. SUBSTANCES TASK DUE BY FRIDAY, NOVEMBER
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 informationI.1 REACTION KINETICS
I.1 REACTION KINETICS KEY QUESTION: Why do reactions occur and how do you control them? REACTION KINETICS is the study of the REACTION RATES Express REACTION RATE as Example 1: The rate of a reaction is
More informationThermochemistry. The study of energy changes that occur during chemical reactions and changes in state.
Energy Thermochemistry The study of energy changes that occur during chemical reactions and changes in state. The Nature of Energy Energy - the ability to do work or produce heat Energy is stored in the
More informationAP* 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
More informationHeat energy change revision questions
Name: Heat energy change revision questions Date: Time: Total marks available: 63 Total marks achieved: Q1. A student uses this apparatus to find the increase in temperature of water when methanol, CH
More information7.4 Potential Energy Diagrams
Name: Date: Chemistry ~ Ms. Hart Class: Anions or Cations Remember: 7.4 Potential Energy Diagrams Chemical reactions can react in both the and directions All chemical reactions need Reactions can either
More informationUNIT 9: KINETICS & EQUILIBRIUM. Essential Question: What mechanisms affect the rates of reactions and equilibrium?
UNIT 9: KINETICS & EQUILIBRIUM Essential Question: What mechanisms affect the rates of reactions and equilibrium? What is Kinetics? Kinetics is the branch of chemistry that explains the rates of chemical
More informationChapter 8: Reaction Rates and Equilibrium
Chapter 8: Reaction Rates and Equilibrium ACTIVATION ENERGY In some reaction mixtures, the average total energy of the molecules is too low at the prevailing temperature for a reaction to take place at
More information