Name: Regents Chemistry: Mr. Palermo. Notes: Unit 7 Heat.
|
|
|
- Gilbert Clarke
- 6 years ago
- Views:
Transcription
1 Name: Regents Chemistry: Mr. Palermo Notes: Unit 7 Heat 1
2 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 energy is the energy associated with the random motion of atoms and molecules. (4.2a) Temperature is a measurement of the average kinetic energy of the particles in a sample of material. Temperature is not a form of energy. (4.2b) The concepts of potential and kinetic energy can be used to explain physical processes that include: fusion (melting), solidification (freezing), vaporization (boiling, evaporation), condensation, sublimation, and deposition. (4.2c) VOCABULARY For each word, provide a short but specific definition from YOUR OWN BRAIN! No boring textbook definitions. Write something to help you remember the word. Explain the word as if you were explaining it to an elementary school student. Give an example if you can. Don t use the words given in your definition! Potential Energy: Kinetic Energy: Heat: Specific Heat: Heat of Fusion: Heat of Vaporization: Endothermic: Exothermic: 2
3 Lesson 1: What is Heat? Objective: Determine the direction of heat flow Determine the change in heat of a reaction POTENTIAL ENERGY: Stored energy KINETIC ENERGY: Energy of motion TYPES OF ENERGY: WHAT IS HEAT? Energy of random motion of atoms/molecules in a sample of matter Heat moves from HOT objects to cold Measured in Joules (table D) In terms of heat flow what happens when an ice pack is placed on your skin? PRACTICE: In a laboratory, a student makes a solution by completely dissolving 80.0 grams of KNO3(s) in grams of hot water. The resulting solution has a temperature of 60. C. The room temperature in the laboratory is 22 C. What is the direction of heat flow? 1
4 Lesson 1: What is Heat? TEMPERATURE: Measure of the of the particles in matter PRACTICE: In which sample of water do the molecules have the highest average kinetic energy? a) 20. ml at 100. C b) 40. ml at 80. C c) 60. ml at 60. C d) 80. ml at 40. C ENERGY CHANGES DURING REACTIONS reactions release heat (energy on right) Ex. A + B C + Energy reactions absorb heat (energy on left) Ex. A + B + energy C TABLE I: SHOWS ENERGY CHANGES FOR SPECIFIC REACTIONS ΔH change in heat of reaction +ΔH (heat is exothermic) - ΔH (heat is endothermic) 2
5 Lesson 1: What is Heat? EXAMPLE TABLE I: When C2H4 is formed, is heat released or absorbed? EXAMPLE TABLE I (reverse reaction): When C2H4 is broken down, is heat released or absorbed? PRACTICE: When C(s) + O2 (g) CO2 (g) is heat absorbed or released? CHECK YOUR UNDERSTANDING: When 2NO2 (g) N2 + 2O2 (g) is heat absorbed or released? 3
6 Lesson 2: Calculating Heat Objective: Calculate heat, specific heat mass and change in temperature of a reaction q is the symbol for heat (equal to ΔH) o Measured in joules or kilojoules o if q is positive, the heat is endo. o if q is negative, the heat is exo. CALCULATING HEAT OF REACTIONS The heat of a reaction is based on: o the mass of the substance o the temperature change it undergoes o specific heat. SPECIFIC HEAT: The heat needed to raise the temperature of one gram of a substance one degree Celsius. Specific heat of water: located on table B Formula on Table T: q = heat m = mass c = specific heat of substance ΔT = final temp initial temp CALCULATING HEAT 1
7 Lesson 2: Calculating Heat EXAMPLE: Solving for heat (q) How much heat is needed to raise the temperature of 500. g of water by 15 C? Step1: List the known variables m = 500. g C = 4.18 J /g C (from Table B) ΔT = 15 C Step 2: Determine the product q = mcδt q = (500. g)(4.18 J /g C)(15 C) q = 31,500 J = 32,000 J EXAMPLE: Solving for specific heat (c) The temperature of 95.4g of copper increases from 25 to 48 C and absorbed 849J. Calculate copper s specific heat. PRACTICE: How many joules of heat are absorbed when 50.0g of water are heated from 30.2 C to 58.6 C? 2
8 Lesson 2: Calculating Heat PRACTICE: How much heat is needed to raise the temperature of 25 g of water from 27 C to 47 C? CHECK YOUR UNDERSTANDING 1: How much heat is needed to raise the temperature of 100g of water 50 C? CHECK YOUR UNDERSTANDING 2: The temperature of aluminum increases from 30 to 38 C and absorbed 900J. Calculate the mass of aluminum used if the specific heat is j/g K. 3
9 Lesson 3: Phase Changes and Heat Objective: Differentiate between endo and exothermic Identify a phase change as either endo or exothermic REVIEW OF SOLIDS, LIQUID, GASES SOLIDS: LIQUIDS: GASES: 1
10 Lesson 3: Phase Changes and Heat Solid STRONGEST force of attraction between particles Liquids MODERATE force of attraction between particles Gases WEAKEST force of attraction between particles PHASE CHANGES: Phase changes: ENDOthermic (s) + heat (l) + heat (s) + heat (l) (g) (l) Phase changes: EXOthermic (l) (g) (g) (s) + heat (l) + heat (s) + heat 2
11 Lesson 3: Phase Changes and Heat THERMOCHEMSITRY The study of energy changes that occur in chemical reactions. Kinetic energy refers to energy of motion. (Temperature) Potential Energy refers to stored energy PHASE CHANGE DIAGRAM 3
12 Lesson 4: Calculating Heat of Phase Changes Objective: Calculate heat of phase changes using q=mhf and q=mhv HEAT OF FUSION: Located on Table B Heat needed to Formula located table T: V HEAT OF VAPORIZATION: Located on Table B Heat needed to Formula located table T: V 1
13 Lesson 4: Calculating Heat of Phase Changes EFFECTS OF IMF S ON Hv & Hf If the IMF is strong, the heats of vaporization and fusion is high (high melting/boiling pt) EXAMPLE: (Heat of fusion) How many joules does it take to melt a 16 gram sample of water at 0 C? EXAMPLE: (Heat of vaporization) How many joules does it take to boil a 250. gram sample of water at 100 C? PRACTICE: How much heat is needed to melt ice at 0C if the sample weighs 255g? PRACTICE: Calculate the number of joules needed to vaporize 423g of H2O 2
14 Lesson 4: Calculating Heat of Phase Changes CHECK YOUR UNDERSTANDING 1: How many joules of energy are required to vaporize 423g of water at 100 C? CHECK YOUR UNDERSTANDING 2: What is the total number of joules of heat needed to change 30.0g of ice to water at 0 C? HEATING CURVE (HEAT ADDED OVER TIME) Vertical Parts: Temp inc Avg. Kinetic energy inc Potential energy remains the same Horizontal Parts (Plateaus): Temp remains the same Avg. Kinetic energy remains the same Potential increases COOLING CURVE (HEAT REMOVED OVER TIME) Vertical Parts: Temp dec Avg. Kinetic energy dec Potential energy remains the same Horizontal Parts (Plateaus): Temp remains the same Avg. Kinetic energy remains the same Potential decreases REMEMBER THE 3 P S Plateau Phase change Potential energy change **diagonal Parts: Temperature is changing.therefore kinetic energy is changing 3
Name: Regents Chemistry: Mr. Palermo. Student Version. Notes: Unit 6A Heat
Name: Regents Chemistry: Mr. Palermo Student Version Notes: Unit 6A Heat Name: KEY IDEAS Heat is a transfer of energy (usually thermal energy) from a body of higher temperature to a body of lower temperature.
Name: 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
solid 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
Practice 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
Practice Packet Unit 7: Heat
Regents Chemistry: Mr. Palermo Practice Packet Unit 7: Heat Review (Things you need to know in order to understand the new stuff ) Particle Diagrams Draw a particle diagram of a compound of CaCl2, using
Thermochemistry. 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
Chemistry 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
Matter and Energy Review Packet
Name Date Matter and Energy Review Packet 1. A compound differs from a mixture in that a compound always has a (1) homogeneous composition (2) maximum of two components (3) minimum of three components
Unit 6: Energy. Aim: What is Energy? Energy: Energy is required to bring about changes in matter (atoms, ions, or molecules).
Name: Date: Unit 6: Energy Aim: What is Energy? Energy: Energy is required to bring about changes in matter (atoms, ions, or molecules). Physical Changes Chemical Changes Example: Example: Energy is measured
What are the states of Matter?
What are the states of Matter? Solid Lowest energy/heat Molecules barely moving Definite, uniform shape Example: ice States of Matter Liquid Medium energy/heat Molecules slowly moving Shape of container
q = m x C x ΔT or, think of it as unit cancellation: = ( ) (
Chemistry Ms. Ye Name Date Block Heat, Kinetic Energy, and Changes in State of Matter *Kinetic Energy=the energy associated with *Temperature=measure of the of a sample. *Heat=is measured as the that is
Unit 6. Unit Vocabulary: Distinguish between the three phases of matter by identifying their different
*STUDENT* Unit Objectives: Absolute Zero Avogadro s Law Normal Boiling Point Compound Cooling Curve Deposition Energy Element Evaporation Heat Heat of Fusion Heat of Vaporization Unit 6 Unit Vocabulary:
Practice Packet: Energy. Regents Chemistry: Dr. Shanzer. Practice Packet. Chapter 4: Energy.
Regents Chemistry: Dr. Shanzer Practice Packet Chapter 4: Energy http:/drshanzerchemistry.weebly.com Energy Objectives Define energy. Demonstrate the difference between endothermic and exothermic reactions
Chemistry Review Unit 5 Physical Behavior of Matter
Chemistry Review Phases of Matter, Changes of Phase, Substances, Mixtures, Solutions, Effect of Solute on Solution, Energy, Kinetics of Solids, Liquids and Gases Matter, Phases and Gas Laws 1. Matter is
Ch. 11 States of matter
Ch. 11 States of matter States of Matter Solid Definite volume Definite shape Liquid Definite volume Indefinite shape (conforms to container) Gas Indefinite volume (fills any container) Indefinite shape
The 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
Name 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
Heat. 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
CHAPTER 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
q = m. C p. T q = heat (Joules) m = mass (g) C p = specific heat (J/g.o C) T = change in temp. ( o C) UNIT 11 - SOLIDS, LIQUIDS, & PHASE CHANGES
HEAT ENERGY NOTES UNIT 11 - SOLIDS, LIQUIDS, & PHASE CHANGES SECTION (A): same temp or change? SECTION (B): same temp or change? temp is called the energy difference at same temp = SECTION (C): same temp
Name 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
Phase Change Diagram. Rank Solids, liquids and gases from weakest attractive forces to strongest:
Unit 11 Kinetic molecular theory packet Page 1 of 13 Chemistry Unit 11 Kinetic Theory Unit Quiz: Test Objectives Be able to define pressure and memorize the basic pressure units. Be able to convert to/from:
Kinetic Theory of Matter
1 Temperature and Thermal Energy Kinetic Theory of Matter The motion of the particles in matter is described by kinetic theory of matter. Matter is composed of particles that are atoms, molecules, or ions
Name 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
Duncan. Q = m. C p. T. Q = heat (Joules) m = mass (g) C p = specific heat capacity (J/g.o C) T = change in temp. ( o C)
HEAT ENERGY NOTES SECTION (A): phase(s) of matter = SECTION (B): phase(s) of matter = energy difference at same temp = temp is called the SECTION (C): phase(s) of matter = SECTION (D): phase(s) of matter
Chapter 3: Matter and Energy
Chapter 3: Matter and Energy Convert between Fahrenheit, Celsius, and Kelvin temperature scales. Relate energy, temperature change, and heat capacity. The atoms and molecules that compose matter are in
ENTHALPY 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
Thermochemistry: 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
Energy 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:
Types 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
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 - ]?
![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 - ]?](/thumbs/78/77877522.jpg "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 - ]?")
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
Name: Class: Date: Figure 3-1
Name: Class: Date: Chapter 3 test Multiple Choice Identify the choice that best completes the statement or answers the question. 1. A gas has a. a definite volume but no definite shape. b. a definite shape
Energy 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
Energy 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:
Pagel. Energy Review. 1. Which phase change results in the release of energy? (1) H20(s)_>H20(4 (3) H20«)->H20(g) (2) H20(s)-»H20(g) (4) H20(g)-*H20«
Energy Review 1. Which phase change results in the release of energy? (1) H20(s)_>H20(4 (3) H20«)->H20(g) (2) H20(s)-»H20(g) (4) H20(g)-*H20«2. The burning of magnesium involves a conversion of (1) chemical
3. 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
The graph represents the uniform cooling of water at 1 atmosphere, starting with water as a gas above its boiling point.
Teacher: Mr. gerraputa Print Close Name: 1. Which graph best represents a change of phase from a gas to a solid? 1. 3. 2. 4. 2. The graph represents the uniform cooling of water at 1 atmosphere, starting
Thermodynamics 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:
2 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
Section 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
SPECIFIC HEAT OF WATER LAB 11-2
CONCEPT Heat of Fusion Changes of state (phase changes) involve the conversion or transition of matter from one of the common states (solid, liquid or gas) to another. Examples include fusion or melting
ENTROPY
ENTROPY 6.2.8 6.2.11 ENTHALPY VS. ENTROPY ENTROPY (S) the disorder of a system - solid liquid gas = entropy - gas liquid solid = entropy - mixing substances always = entropy SPONTANEOUS VS. NONSPONTANEOUS
Ch. 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
Exam Accelerated Chemistry Study Sheet Chap12 Solids/Liquids/Intermolecular Forces
Exam Accelerated Chemistry Study Sheet Chap12 Solids/Liquids/Intermolecular Forces Name /66 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Intermolecular
2. State the direction of heat transfer between the surroundings and the water in the bottle from 7 a.m. to 3 p.m.
Base your answers to questions 1 through 3 on the information below. A student investigated heat transfer using a bottle of water. The student placed the bottle in a room at 20.5 C. The student measured
Chapter 5 Energy and States of Matter. Changes of State. Melting and Freezing. Calculations Using Heat of Fusion
Chapter 5 Energy and States of Matter Changes of State 5.6 Melting and Freezing 5.7 Boiling and Condensation 1 2 Melting and Freezing A substance is melting while it changes from a solid to a liquid. A
Notes: 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
This activity has been used in an introductory chemistry course (prep chemistry or GOB course) Learning Goals: Prerequisite knowledge
This activity has been used in an introductory chemistry course (prep chemistry or GOB course) Learning Goals: Name phase changes Identify phase changes at molecular (particulate) level Name intermolecular
Chapter 12 Intermolecular Forces of Attraction
Chapter 12 Intermolecular Forces of Attraction Intermolecular Forces Attractive or Repulsive Forces between molecules. Molecule - - - - - - Molecule Intramolecular Forces bonding forces within the molecule.
Vocabulary. Pressure Absolute zero Charles Law Boyle s Law (take a moment to look up and record definitions in your notes)
The Gas Laws Vocabulary Pressure Absolute zero Charles Law Boyle s Law (take a moment to look up and record definitions in your notes) Key Concepts What causes gas pressure in a closed container? What
AlCl3(aq) + 3 NaOH(aq) Al(OH)3(s) + 3 NaCl(aq)
1. Under which conditions does a real gas behave most like an ideal gas? A) at low temperatures and high pressures B) at low temperatures and low pressures C) at high temperatures and high pressures D)
Ch 100: Fundamentals for Chemistry
Ch 100: Fundamentals for Chemistry Chapter 4: Properties of Matter Lecture Notes Physical & Chemical Properties Physical Properties are the characteristics of matter that can be changed without changing
Chemistry Topic 4. Physical Behavior of Matter
Chemistry Topic 4 Physical Behavior of Matter 11/30 Chemistry Unit 4 Physical Behavior of Matter Aim: What are the 3 states of matter? Obj: SWBAT compare and contrast the states of matter Do now: 2H 2
Liquids and Solids Chapter 10
Liquids and Solids Chapter 10 Nov 15 9:56 AM Types of Solids Crystalline solids: Solids with highly regular arrangement of their components Amorphous solids: Solids with considerable disorder in their
Unit 14. States of Matter & Thermochemistry
Unit 14 Flashback: States of Matter & Thermochemistry Characteristic Solids Liquids Gases Shape Volume Density Fluidity Compressibility Picture Phase Diagram Shows the relationship between solid, liquid,
1. Thermo = the that happen in a chemical reaction. 4. You must ADD energy to melt solids into liquids example:
ThermoChem Notes 1. Thermo = the that happen in a chemical reaction. 2. When heat is given off it is an reaction. 3. Sometimes energy is absorbed in order for the reaction happen; this is called an reaction.
CHAPTER 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
Chapter 3. States of Matter
Chapter 3 States of Matter 1. Solid 2. Liquid 3. Gas States of Matter Two More (discuss later) Plasma Bose-Einstein condensate States of Matter Solid (definite shape and volume) Particles are tightly packed
Unit 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
0 o K is called absolute zero. Water Freezes: 273 o K Water Boils: 373 o K
Part I Notes Temperature and Heat The terms at the right all mean the same thing. The heat energy of a substance is the sum of the kinetic and potential energies of all of the atoms and molecules in the
Thermochemistry: 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
Energy and Energy Calculations Test Provide the correct answer as a word, phrase or sentence. (3 points each) 1) Define Matter.
Provide the correct answer as a word, phrase or sentence. (3 points each) 1) Define Matter. 2) What is ENERGY? 3) Give an example of an endothermic process. 4) Give an example of an exothermic process.
Name... Class... Date... Specific heat capacity and specific latent heat
Specific heat capacity and specific latent heat Specification references: P3.2.2 Temperature changes in a system and specific heat capacity P3.2.3 Changes of heat and specific latent heat Aims This is
Energy. Different types of energy exist (heat, potential, kinetic, chemical, nuclear etc.)
Change in Energy Energy Different types of energy exist (heat, potential, kinetic, chemical, nuclear etc.) Heat - the energy transferred between objects that are at different temperatures. Unit of heat
Solids (cont.) Describe the movement of particles in a solid and the forces between them.
Solids A solid is matter that has a definite shape and a definite volume. The attractive forces between the particles in a solid are strong and pull them close together. Solids (cont.) Describe the movement
Name 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
( Practice(Packet( ( Chapter(4:(Energy((
PracticePacket:Energy Regents Chemistry: Dr. Mintz PracticePacket Chapter4:Energy http://mintzchemistry.weebly.com 116 Energy Objectives Define energy. Demonstrate the difference between endothermic and
Name: Regents Review Quiz #1 2016
Name: Regents Review Quiz #1 2016 1. Which two particle diagrams represent mixtures of diatomic elements? A) A and B B) A and C C) B and C D) B and D 2. At STP, which physical property of aluminum always
Physical Changes can be observed without changing the identity of the substance (often states of matter changes).
Physical Changes can be observed without changing the identity of the substance (often states of matter changes). Remember: States of matter changes are physical changes. The identify of the substance
CP 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
Work 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
Chapter 11. Liquids and Intermolecular Forces
Chapter 11 Liquids and Intermolecular Forces States of Matter The three states of matter are 1) Solid Definite shape Definite volume 2) Liquid Indefinite shape Definite volume 3) Gas Indefinite shape Indefinite
SPECIFIC HEAT CAPACITY AND HEAT OF FUSION
SPECIFIC HEAT CAPACITY AND HEAT OF FUSION Apparatus on each table: Thermometer, metal cube, complete calorimeter, outer calorimeter can (aluminum only), balance, 4 styrofoam cups, graduated container,
Chapter 11 part 2. Properties of Liquids Viscosity Surface Tension Capillary Action. Phase Changes (energy of phase changes)
Chapter 11 part 2 Properties of Liquids Viscosity Surface Tension Capillary Action Phase Changes (energy of phase changes) Dynamic Equilibrium Vapor pressure Phase diagram 1 Structure Affects Function
4 Discuss and evaluate the 5th state of matter. 3 - Differentiate among the four states of matter in terms of energy,
Goal: Differentiate among the four states of matter in terms of energy, particle motion, and phase transitions. 4 States of Mater Sections 3.1, 3.2 4 Discuss and evaluate the 5 th state of matter. 3 -
Thermochemistry. 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
Changes and Properties of Matter
Changes and Properties of Matter Physical Properties of Matter Physical Changes: Changes that change only the appearance of a substance, not its chemical identity. Physical Properties: Properties that
Chapter 22 States of matter. Section 1 matter Section 2 Changes of State
Chapter 22 States of matter Section 1 matter Section 2 Changes of State States of Matter is a physical property ***Matter is made of atoms Atoms form chemical bonds to make matter **** Atoms vibrate constantly
Topic 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
Energy 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
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
Name Chemistry / / SOL Questions Chapter 9 For each of the following, fill in the correct answer on the BLUE side of the scantron.
Name Chemistry / / SOL Questions Chapter 9 For each of the following, fill in the correct answer on the BLUE side of the scantron. 1. Which number on the graph to the right represents the effect of the
Chapter 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
Topic 5: Energetics. Heat & Calorimetry. Thursday, March 22, 2012
Topic 5: Energetics Heat & Calorimetry 1 Heat is energy that is transferred from one object to another due to a difference in temperature Temperature is a measure of the average kinetic energy of a body
Matter and Energy I. Matter Matter is anything that has mass and volume Mass Amount of matter Measured in grams (g) Volume Space matter occupies
Matter and Energy I. Matter Matter is anything that has mass and volume Mass Amount of matter Measured in grams (g) Volume Space matter occupies Measured in milliliters (ml), liters (L) or cubic centimeters
Unit 1 Lesson 6 Changes of State. Copyright Houghton Mifflin Harcourt Publishing Company
The Fact of the Matter What happens when matter changes state? The three most familiar states of matter are solid, liquid, and gas. A change of state is the change of a substance from one physical form
= (25.0 g)(0.137 J/g C)[61.2 C - (-31.4 C)] = 317 J (= kj)
![= (25.0 g)(0.137 J/g C)[61.2 C - (-31.4 C)] = 317 J (= kj)](/thumbs/89/101004910.jpg "= (25.0 g)(0.137 J/g C)[61.2 C - (-31.4 C)] = 317 J (= kj)")
CHEM 101A ARMSTRONG SOLUTIONS TO TOPIC D PROBLEMS 1) For all problems involving energy, you may give your answer in either joules or kilojoules, unless the problem specifies a unit. (In general, though,
17.4 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
CHEMISTRY 109 #25 - REVIEW
CHEMISTRY 109 Help Sheet #25 - REVIEW Chapter 4 (Part I); Sections 4.1-4.6; Ch. 9, Section 9.4a-9.4c (pg 387) ** Review the appropriate topics for your lecture section ** Prepared by Dr. Tony Jacob http://www.chem.wisc.edu/areas/clc
POGIL: Calorimetry DATE:
NAME: DATE: AP Chemistry POGIL: Calorimetry Why? On a hot summer day, you may find that the cement next to a swimming pool is unbearably hot to walk across, but the water in the pool is too chilly for
Thermodynamics and States of Matter
Thermodynamics and States of Matter There are three states (also called phases) ) of matter. The picture to the side represents the same chemical substance, just in different states. There are three states
Mr 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.
Core Chemistry UNIT 1: Matter & Energy Section 1: The Law of Conservation of Mass Section 2: States of Matter & Intro to Thermodynamics
Core Chemistry UNIT 1: Matter & Energy Section 1: The Law of Conservation of Mass Section 2: States of Matter & Intro to Thermodynamics UNIT 1 Synapsis In our first unit we will explore matter & energy
Unit 9 Thermochemistry. Chapter 17
Unit 9 Thermochemistry Chapter 17 This tutorial is designed to help students understand scientific measurements. Objectives for this unit appear on the next slide. Each objective is linked to its description.
1. Base your answer to the following question on the information below and on your knowledge of chemistry.
1. Base your answer to the following question on the information below and on your knowledge of chemistry. A beaker contains a liquid sample of a molecular substance. Both the beaker and the liquid are
Name: 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.
IGCSE Double Award Extended Coordinated Science
IGCSE Double Award Extended Coordinated Science Physics 5 - Thermal Properties of Matter Thermal Expansion You need to know thermal expansions for solids, liquids, and gases, and their applications. Thermal
The Liquid and Solid States
: The Liquid and Solid States 10-1 10.1 Changes of State How do solids, liquids and gases differ? Figure 10.4 10-2 1 10.1 Changes of State : transitions between physical states Vaporization/Condensation
The Can Demonstration
The Can Demonstration With your table, make a prediction as to what will happen to the can. Discuss why you think that the can imploded. What are some reasons? https://www.youtube.com/watch?v=xg5niowf_zw&t=28s
UNIT #8: Low Density: Compression and Expansion: Diffusion:
NAME: UNIT #8: Characteristics of Gases Gas Laws and Calculations Intermolecular Forces Phase Changes Energy Calculations Heating and Cooling Curves Vapor Pressure 1. GENERAL CHARACTERISTICS OF GASES a)