This 1-hour presentation discusses the differences and similarities between solids and gases as they move to equilibrium through the combustion process.
This document discusses chemical equilibrium and related concepts from a chapter of an introductory chemistry textbook. It covers dynamic equilibrium, factors that affect reaction rates, collision theory, the definition of a chemical equilibrium constant Keq and how it relates to the amounts of reactants and products, Le Châtelier's principle of chemical equilibrium, and how various disturbances like concentration changes, temperature changes and volume changes affect systems at equilibrium. It also provides examples of how equilibrium concepts apply to biochemistry like oxygen transport from the mother's blood to a fetus.
Lecture 2 By MUHAMMAD FAHAD ANSARI 12 IEEM 14fahadansari131
This document summarizes the key points about types of chemical reactions and factors that affect reaction rates. It discusses the 5 main types of chemical reactions: synthesis, decomposition, single-replacement, double-replacement, and oxidation-reduction. It also outlines characteristics of each type and provides examples. Additionally, the document covers concepts like activation energy, catalysts, temperature effects, and concentration effects on reaction rates. Finally, it briefly discusses chemical equilibrium and kinetic molecular theory of gases.
This document discusses reaction rates and chemical equilibrium. It begins by defining reaction rates and factors that influence reaction rates such as temperature, concentration, surface area, and catalysts. It then explains collision theory and the role of activation energy in reactions. The document also covers Le Chatelier's principle, how stresses such as concentration, temperature, and pressure affect chemical equilibrium. It defines equilibrium constants and discusses solubility equilibrium, including solubility product constants and the common ion effect. Finally, it introduces entropy, the role of entropy in spontaneous reactions, and free energy.
The document discusses the basic concept of matter according to the kinetic theory. It states that:
1) Matter can exist in three physical states - solid, liquid, and gas - depending on the arrangement and movement of its particles.
2) In solids, particles are closely packed and arranged orderly, while in liquids they are farther apart but not in an orderly arrangement. In gases, particles are very far apart and move freely at high speeds.
3) Changes in temperature can cause changes in a substance's state as it absorbs or releases heat, altering the kinetic energy and motion of its particles. For example, melting occurs when a solid absorbs enough heat energy to allow its particles to vibrate vigorously
This document discusses the three states of matter - solid, liquid, and gas. It explains that the state of a substance depends on temperature and pressure, and describes several phase changes between the different states (melting, freezing, boiling, evaporation, condensation, sublimation) and the energy exchanges that occur. It also compares the properties of the three states in terms of particle arrangement, movement, and interactions. In addition, the document discusses other topics including diffusion, osmosis, and the particle theory of matter.
This document discusses the three states of matter - solid, liquid, and gas. It explains that the state of a substance depends on temperature and pressure, and describes several phase changes between the different states (melting, freezing, boiling, evaporation, condensation, sublimation) and the energy changes involved. It also compares the properties of solids, liquids, and gases in terms of particle arrangement and movement. In addition, the document discusses diffusion, osmosis, and the particle theory of matter.
The document discusses the three states of matter - solid, liquid, and gas. It explains the properties of gases and how gas particles are in constant random motion. The gas laws including Boyle's law, Charles' law, Avogadro's law, and the ideal gas equation are described. It also covers gas pressure, measurement of pressure using barometers and manometers, gas density calculations, and sample problems involving the gas laws.
1. There are 12 known states of matter including solid, liquid, gas, plasma, and more exotic states like Bose-Einstein condensate and string-net liquid.
2. Solids have a fixed shape and volume while liquids have a fixed volume but not shape. Gases have neither a fixed shape nor volume.
3. Phase changes between solid, liquid, and gas can occur when temperature or pressure changes. Melting, freezing, vaporization, condensation, and sublimation involve changes in state with associated latent heat effects.
This document discusses chemical equilibrium and related concepts from a chapter of an introductory chemistry textbook. It covers dynamic equilibrium, factors that affect reaction rates, collision theory, the definition of a chemical equilibrium constant Keq and how it relates to the amounts of reactants and products, Le Châtelier's principle of chemical equilibrium, and how various disturbances like concentration changes, temperature changes and volume changes affect systems at equilibrium. It also provides examples of how equilibrium concepts apply to biochemistry like oxygen transport from the mother's blood to a fetus.
Lecture 2 By MUHAMMAD FAHAD ANSARI 12 IEEM 14fahadansari131
This document summarizes the key points about types of chemical reactions and factors that affect reaction rates. It discusses the 5 main types of chemical reactions: synthesis, decomposition, single-replacement, double-replacement, and oxidation-reduction. It also outlines characteristics of each type and provides examples. Additionally, the document covers concepts like activation energy, catalysts, temperature effects, and concentration effects on reaction rates. Finally, it briefly discusses chemical equilibrium and kinetic molecular theory of gases.
This document discusses reaction rates and chemical equilibrium. It begins by defining reaction rates and factors that influence reaction rates such as temperature, concentration, surface area, and catalysts. It then explains collision theory and the role of activation energy in reactions. The document also covers Le Chatelier's principle, how stresses such as concentration, temperature, and pressure affect chemical equilibrium. It defines equilibrium constants and discusses solubility equilibrium, including solubility product constants and the common ion effect. Finally, it introduces entropy, the role of entropy in spontaneous reactions, and free energy.
The document discusses the basic concept of matter according to the kinetic theory. It states that:
1) Matter can exist in three physical states - solid, liquid, and gas - depending on the arrangement and movement of its particles.
2) In solids, particles are closely packed and arranged orderly, while in liquids they are farther apart but not in an orderly arrangement. In gases, particles are very far apart and move freely at high speeds.
3) Changes in temperature can cause changes in a substance's state as it absorbs or releases heat, altering the kinetic energy and motion of its particles. For example, melting occurs when a solid absorbs enough heat energy to allow its particles to vibrate vigorously
This document discusses the three states of matter - solid, liquid, and gas. It explains that the state of a substance depends on temperature and pressure, and describes several phase changes between the different states (melting, freezing, boiling, evaporation, condensation, sublimation) and the energy exchanges that occur. It also compares the properties of the three states in terms of particle arrangement, movement, and interactions. In addition, the document discusses other topics including diffusion, osmosis, and the particle theory of matter.
This document discusses the three states of matter - solid, liquid, and gas. It explains that the state of a substance depends on temperature and pressure, and describes several phase changes between the different states (melting, freezing, boiling, evaporation, condensation, sublimation) and the energy changes involved. It also compares the properties of solids, liquids, and gases in terms of particle arrangement and movement. In addition, the document discusses diffusion, osmosis, and the particle theory of matter.
The document discusses the three states of matter - solid, liquid, and gas. It explains the properties of gases and how gas particles are in constant random motion. The gas laws including Boyle's law, Charles' law, Avogadro's law, and the ideal gas equation are described. It also covers gas pressure, measurement of pressure using barometers and manometers, gas density calculations, and sample problems involving the gas laws.
1. There are 12 known states of matter including solid, liquid, gas, plasma, and more exotic states like Bose-Einstein condensate and string-net liquid.
2. Solids have a fixed shape and volume while liquids have a fixed volume but not shape. Gases have neither a fixed shape nor volume.
3. Phase changes between solid, liquid, and gas can occur when temperature or pressure changes. Melting, freezing, vaporization, condensation, and sublimation involve changes in state with associated latent heat effects.
This document provides a summary of sections from a chemistry textbook chapter on properties and changes in matter. It summarizes key concepts from sections on properties of matter, changes in matter, mixtures of matter, and elements and compounds. The sections define states of matter, physical and chemical properties, physical and chemical changes, mixtures, elements, compounds, and laws of chemistry such as definite and multiple proportions.
This document provides an overview of key concepts relating to matter and energy from a chemistry textbook. It defines the three common states of matter as solid, liquid, and gas. Matter is composed of atoms and molecules and can be classified as elements, compounds, or mixtures based on its composition. A physical property is one that does not change the composition of a substance, while a chemical property involves a change in composition. Energy and mass are conserved in physical and chemical changes. The document also discusses heat, temperature, and heat capacity, and provides formulas for calculating energy changes associated with temperature variations.
The document discusses different types of matter including elements, compounds, homogeneous and heterogeneous materials, and mixtures. It defines key terms like phase, interface, and molarity. It also covers physical and chemical properties and changes, energy transfer during chemical reactions, and using calorimetry to measure energy changes.
The document is from an honors chemistry textbook and discusses thermochemistry, specifically:
1) The molar heat of fusion and solidification, and how the heat absorbed during melting equals the heat released during solidification.
2) The molar heat of vaporization and condensation, and how the heat required for vaporization equals the heat released during condensation.
3) Hess's law, which states that the enthalpy change of a reaction is the same whether it occurs in one step or multiple steps.
Pharmaceutical chemistry of inorganic medicinalsEnter Exit
This document provides an introduction to chemical kinetics and equilibrium. It defines chemical kinetics as the study of reaction rates and mechanisms. It describes factors that influence reaction rates, such as the nature of reactants, physical state, concentration, temperature, catalysts and pressure. It then discusses collision theory and activation energy. The document also explains chemical equilibrium, including the law of mass action and Le Chatelier's principle. Finally, it covers pH, pOH, pKa and pKb calculations and their relationships to acid/base ionization constants.
This document provides an overview of matter and its properties according to the ICSE curriculum for upper primary classes. It defines matter as anything that occupies space, has mass and volume, and can be sensed. All matter is composed of molecules, which are made up of atoms. Matter can exist in three states - solid, liquid, and gas - depending on the strength of intermolecular forces and the distance between molecules. Changes in state, such as melting, boiling, and sublimation, occur when matter gains or loses heat. Heating matter can also cause chemical changes in addition to physical changes like expansion and changes in state.
General Chemistry and Inorganic Pharmaceutical Chemistry Module 1 Pharmacist ...Senyora Ouf'ra
This document provides an overview of Module 1 of the pharmacist licensure exam, which covers various topics in pharmaceutical chemistry. It will be the first module administered on the first day of the exam from 8-10 AM. The module will include questions from general chemistry, inorganic and organic medicinal chemistry, analytical chemistry, and other related chemical topics. The document emphasizes that Module 1 will be the most difficult and important module to study for. It then provides examples of key topics covered, such as atomic structure, types of chemical bonds, gas laws, and thermodynamics.
This document discusses different types of changes in matter, including physical changes which do not alter the substance's composition, changes in state from solid to liquid to gas or vice versa depending on temperature, and chemical changes which produce new substances through irreversible reactions. It also defines pure substances, mixtures, heterogeneous and homogeneous mixtures, and other key chemistry terms.
The document discusses the science of fire behavior as it relates to energy, ignition, and combustion. It explains that there are two types of changes - physical and chemical - that firefighters need to understand. There are also different forms of energy, states of fuel, factors that affect fire development, and stages of fire development that firefighters must be familiar with to safely and effectively combat fires. The key concepts covered include the fire triangle and tetrahedron, different types of heat transfer, how oxygen relates to life safety, and the products of combustion.
The document discusses states of matter and changes between different states. It provides information on:
- The three main states of matter - solid, liquid, gas - and how a change of state involves a change in physical form but not chemical identity.
- Energy must be gained or lost for a substance to change states, altering temperature or motion of particles.
- Specific changes include melting (solid to liquid), freezing (liquid to solid), evaporation/boiling (liquid to gas), condensation (gas to liquid), and sublimation (solid to gas).
- Phase diagrams illustrate conditions where states coexist and phase boundaries. Eutectic mixtures have a lower melting point than their components.
This document provides an overview of organic chemistry and organic medicinal chemistry. It discusses general chemistry topics including the definition of chemistry, classification of matter, physical and chemical properties, and acid-base properties. It also covers organic chemistry topics such as the difference between inorganic and organic chemistry, functional groups, isomerism, and reactions. The document is intended to serve as a refresher course on these fundamental concepts.
This document provides an overview of three sections (13.1, 13.2, 13.3) from a chemistry textbook chapter on gases. Section 13.1 describes gas laws including Boyle's law, Charles' law, Gay-Lussac's law, and the combined gas law. Section 13.2 introduces the ideal gas law, Avogadro's principle, and compares real and ideal gases. Section 13.3 explains how to use gas laws and stoichiometry to solve problems involving gaseous reactants and products in chemical equations.
The document defines the four phases of matter as solid, liquid, gas, and plasma. It provides examples of each phase and explains their properties. Specifically, it states that in a solid, molecules are close together and cannot move around, in a liquid molecules are close and move slowly, in a gas molecules are far apart and move freely at high speeds, and in a plasma the matter is ionized. It then discusses the processes by which matter changes between phases, such as melting, boiling, subliming, freezing, condensation, and deposition.
Some basic concepts of chemistry
chapter 1 of class 11.
N.B : This is for reference only. Students are advised not to copy, but to take ideas and do the work in their own style-it builds your imagination.
Chapter 1 some basic concepts of chemistry class 11 UPDATED PPTritik
The document summarizes several important concepts and laws in chemistry:
1) The law of conservation of mass states that matter is neither created nor destroyed in chemical reactions.
2) The law of definite proportions states that a chemical compound always contains the same elements in the same proportions by mass.
3) Gay-Lussac's law of gaseous volumes describes how gases combine or are produced in simple volume ratios in chemical reactions at the same temperature and pressure.
4) Avogadro's law states that equal volumes of gases under the same conditions contain an equal number of molecules.
Matter exists in four states - solid, liquid, gas, and plasma - depending on temperature. In solids, particles vibrate in place and maintain a definite shape and volume. In liquids, particles can move around each other while maintaining a definite volume. In gases, particles separate and move freely in all directions without definite shape or volume. Plasma is an ionized gas state not found naturally on Earth. Phase changes between states require or release energy.
The document defines over 100 key terms used in quantitative chemistry, including:
- Amount refers to the number of moles of a substance.
- Aqueous solution is a solution with water as the solvent.
- Atmospheric pressure is the pressure exerted by the atmosphere on Earth's surface.
- Avogadro's constant is the number of particles in exactly 12 grams of carbon-12.
Ch - 1 some basic concepts of chemistryVimlesh Gupta
Chemistry deals with the composition, structure, and properties of matter. This document outlines key concepts in chemistry including the three states of matter, classification of substances, physical and chemical properties, the mole concept, laws of chemical combination, stoichiometry, and concentration terms. It provides definitions and examples of important terminology and calculations in chemistry.
This document defines key terms related to fire chemistry and behavior. It explains that the three necessary elements for a fire are heat, fuel, and an oxidizing agent (usually oxygen from air). Fires start when these elements come together in the proper proportions. Fuels must be in gaseous form to burn, requiring solids and liquids to undergo pyrolysis or vaporization first when heated. Heat is then transferred between objects via conduction, convection or radiation to allow the fire to spread.
This document provides an introduction to general chemistry. It defines chemistry as the study of matter and its transformations. Matter is anything that has mass and occupies space, and can exist in different states such as solid, liquid, gas, and plasma. The document discusses physical and chemical properties of matter, as well as physical and chemical changes. It classifies matter as either pure substances like elements and compounds, or mixtures that are either homogeneous or heterogeneous. The key concepts covered include the states of matter, phase changes, and the classification of matter.
III STUDY GUIDEChemistry and Physics of Fire and FireProtecti.docxMARRY7
III STUDY GUIDE
Chemistry and Physics of Fire and Fire
Protection Systems and Equipment
Reading
Assignment
Chapter 4:
Chemistry and Physics of
Fire
Chapter 12:
Fire Protection Systems and Equipment
Additional Required
Reading
See information below.
Supplemental
Reading
See information below.
Key Terms
1. Ambient temperature
2. Bonnet
3. Fire department connection
4. Free radicals
5. Halogenated agents
6. Latent heat of vaporization
7. Miscible
8. Molecule
9. Nonmiscible
10. Open screw and yoke valve (OS&Y)
11. Oxidation
12. Oxidizer
13. Polar solvents
14. Post indicator valve
(PI)
15. Pyrolysis
16. Retard chamber
17. Thrust block
Learning Objectives
Upon completion of this unit, students should be able to:
1. Describe the differences between fire triangle and fire tetrahedron.
2. Illustrate the comparison between chemistry of fire and physics of fire.
3. Differentiate the principles of flame spread of solid, liquid, and gas/vapor fuels.
4. Describe classes of fire, stages of fire, and heat transfer during a fire.
5. Differentiate public and private water supply systems.
6. Illustrate the design and components of a water supply system.
7. Describe various extinguishing agents.
8. Illustrate the design and components of various types of extinguishing systems.
Written Lecture
Introduction
In this unit we will explore the world of the chemistry and physics of fire found in Chapter 4. We will also explore Chapter 12 where we will consider fire protection systems and the equipment associated with fire protection systems.
Chapter 4: Chemistry and Physics of Fire
Definition of fire: Fire is a rapid and self-sustaining oxidation process that is assisted by the generation of heat and light in various degrees of intensity. As stated in your textbook, fire is the process of oxidation and is associated with the term combustion, which is the chemical chain reaction that releases both light and heat. For all intents and purposes, fire is both friend and foe. We use fire for heating, cooking, manufacturing, and controlling other fire sources.
Fire triangle and fire tetrahedron: Perhaps as a child you were taught that fire was represented by a triangle with each side denoting one of the three components required to sustain fire: air, fuel, and heat. Classically known as the Fire Triangle we learned that by removing any one of the three components fire would be extinguished.
1
Over time, the scientific community has added another dimension called the chemical reaction found during the combustion process. With the addition of this fourth side we now have the new symbol of fire called the fire tetrahedron.
Chemistry of fire: Fire needs two basic elements in order to sustain its existence, and without the two in union, fire cannot occur. These two elements are oxidizer and fuel.
Oxidizer: An oxidizer is any substance that generates oxygen. The most common and abundant oxidizer ...
Fire requires four key elements - fuel, oxygen, heat, and a chemical chain reaction. These four elements form a tetrahedron shape to represent what is needed for fire. Each element must be present for combustion to occur and removing any one will extinguish the fire. Heat is transferred during fires through conduction, convection, and radiation. A fire goes through distinct stages from ignition to fully developed. Understanding how fires start and progress is important for fire investigation and arson detection.
This document provides a summary of sections from a chemistry textbook chapter on properties and changes in matter. It summarizes key concepts from sections on properties of matter, changes in matter, mixtures of matter, and elements and compounds. The sections define states of matter, physical and chemical properties, physical and chemical changes, mixtures, elements, compounds, and laws of chemistry such as definite and multiple proportions.
This document provides an overview of key concepts relating to matter and energy from a chemistry textbook. It defines the three common states of matter as solid, liquid, and gas. Matter is composed of atoms and molecules and can be classified as elements, compounds, or mixtures based on its composition. A physical property is one that does not change the composition of a substance, while a chemical property involves a change in composition. Energy and mass are conserved in physical and chemical changes. The document also discusses heat, temperature, and heat capacity, and provides formulas for calculating energy changes associated with temperature variations.
The document discusses different types of matter including elements, compounds, homogeneous and heterogeneous materials, and mixtures. It defines key terms like phase, interface, and molarity. It also covers physical and chemical properties and changes, energy transfer during chemical reactions, and using calorimetry to measure energy changes.
The document is from an honors chemistry textbook and discusses thermochemistry, specifically:
1) The molar heat of fusion and solidification, and how the heat absorbed during melting equals the heat released during solidification.
2) The molar heat of vaporization and condensation, and how the heat required for vaporization equals the heat released during condensation.
3) Hess's law, which states that the enthalpy change of a reaction is the same whether it occurs in one step or multiple steps.
Pharmaceutical chemistry of inorganic medicinalsEnter Exit
This document provides an introduction to chemical kinetics and equilibrium. It defines chemical kinetics as the study of reaction rates and mechanisms. It describes factors that influence reaction rates, such as the nature of reactants, physical state, concentration, temperature, catalysts and pressure. It then discusses collision theory and activation energy. The document also explains chemical equilibrium, including the law of mass action and Le Chatelier's principle. Finally, it covers pH, pOH, pKa and pKb calculations and their relationships to acid/base ionization constants.
This document provides an overview of matter and its properties according to the ICSE curriculum for upper primary classes. It defines matter as anything that occupies space, has mass and volume, and can be sensed. All matter is composed of molecules, which are made up of atoms. Matter can exist in three states - solid, liquid, and gas - depending on the strength of intermolecular forces and the distance between molecules. Changes in state, such as melting, boiling, and sublimation, occur when matter gains or loses heat. Heating matter can also cause chemical changes in addition to physical changes like expansion and changes in state.
General Chemistry and Inorganic Pharmaceutical Chemistry Module 1 Pharmacist ...Senyora Ouf'ra
This document provides an overview of Module 1 of the pharmacist licensure exam, which covers various topics in pharmaceutical chemistry. It will be the first module administered on the first day of the exam from 8-10 AM. The module will include questions from general chemistry, inorganic and organic medicinal chemistry, analytical chemistry, and other related chemical topics. The document emphasizes that Module 1 will be the most difficult and important module to study for. It then provides examples of key topics covered, such as atomic structure, types of chemical bonds, gas laws, and thermodynamics.
This document discusses different types of changes in matter, including physical changes which do not alter the substance's composition, changes in state from solid to liquid to gas or vice versa depending on temperature, and chemical changes which produce new substances through irreversible reactions. It also defines pure substances, mixtures, heterogeneous and homogeneous mixtures, and other key chemistry terms.
The document discusses the science of fire behavior as it relates to energy, ignition, and combustion. It explains that there are two types of changes - physical and chemical - that firefighters need to understand. There are also different forms of energy, states of fuel, factors that affect fire development, and stages of fire development that firefighters must be familiar with to safely and effectively combat fires. The key concepts covered include the fire triangle and tetrahedron, different types of heat transfer, how oxygen relates to life safety, and the products of combustion.
The document discusses states of matter and changes between different states. It provides information on:
- The three main states of matter - solid, liquid, gas - and how a change of state involves a change in physical form but not chemical identity.
- Energy must be gained or lost for a substance to change states, altering temperature or motion of particles.
- Specific changes include melting (solid to liquid), freezing (liquid to solid), evaporation/boiling (liquid to gas), condensation (gas to liquid), and sublimation (solid to gas).
- Phase diagrams illustrate conditions where states coexist and phase boundaries. Eutectic mixtures have a lower melting point than their components.
This document provides an overview of organic chemistry and organic medicinal chemistry. It discusses general chemistry topics including the definition of chemistry, classification of matter, physical and chemical properties, and acid-base properties. It also covers organic chemistry topics such as the difference between inorganic and organic chemistry, functional groups, isomerism, and reactions. The document is intended to serve as a refresher course on these fundamental concepts.
This document provides an overview of three sections (13.1, 13.2, 13.3) from a chemistry textbook chapter on gases. Section 13.1 describes gas laws including Boyle's law, Charles' law, Gay-Lussac's law, and the combined gas law. Section 13.2 introduces the ideal gas law, Avogadro's principle, and compares real and ideal gases. Section 13.3 explains how to use gas laws and stoichiometry to solve problems involving gaseous reactants and products in chemical equations.
The document defines the four phases of matter as solid, liquid, gas, and plasma. It provides examples of each phase and explains their properties. Specifically, it states that in a solid, molecules are close together and cannot move around, in a liquid molecules are close and move slowly, in a gas molecules are far apart and move freely at high speeds, and in a plasma the matter is ionized. It then discusses the processes by which matter changes between phases, such as melting, boiling, subliming, freezing, condensation, and deposition.
Some basic concepts of chemistry
chapter 1 of class 11.
N.B : This is for reference only. Students are advised not to copy, but to take ideas and do the work in their own style-it builds your imagination.
Chapter 1 some basic concepts of chemistry class 11 UPDATED PPTritik
The document summarizes several important concepts and laws in chemistry:
1) The law of conservation of mass states that matter is neither created nor destroyed in chemical reactions.
2) The law of definite proportions states that a chemical compound always contains the same elements in the same proportions by mass.
3) Gay-Lussac's law of gaseous volumes describes how gases combine or are produced in simple volume ratios in chemical reactions at the same temperature and pressure.
4) Avogadro's law states that equal volumes of gases under the same conditions contain an equal number of molecules.
Matter exists in four states - solid, liquid, gas, and plasma - depending on temperature. In solids, particles vibrate in place and maintain a definite shape and volume. In liquids, particles can move around each other while maintaining a definite volume. In gases, particles separate and move freely in all directions without definite shape or volume. Plasma is an ionized gas state not found naturally on Earth. Phase changes between states require or release energy.
The document defines over 100 key terms used in quantitative chemistry, including:
- Amount refers to the number of moles of a substance.
- Aqueous solution is a solution with water as the solvent.
- Atmospheric pressure is the pressure exerted by the atmosphere on Earth's surface.
- Avogadro's constant is the number of particles in exactly 12 grams of carbon-12.
Ch - 1 some basic concepts of chemistryVimlesh Gupta
Chemistry deals with the composition, structure, and properties of matter. This document outlines key concepts in chemistry including the three states of matter, classification of substances, physical and chemical properties, the mole concept, laws of chemical combination, stoichiometry, and concentration terms. It provides definitions and examples of important terminology and calculations in chemistry.
This document defines key terms related to fire chemistry and behavior. It explains that the three necessary elements for a fire are heat, fuel, and an oxidizing agent (usually oxygen from air). Fires start when these elements come together in the proper proportions. Fuels must be in gaseous form to burn, requiring solids and liquids to undergo pyrolysis or vaporization first when heated. Heat is then transferred between objects via conduction, convection or radiation to allow the fire to spread.
This document provides an introduction to general chemistry. It defines chemistry as the study of matter and its transformations. Matter is anything that has mass and occupies space, and can exist in different states such as solid, liquid, gas, and plasma. The document discusses physical and chemical properties of matter, as well as physical and chemical changes. It classifies matter as either pure substances like elements and compounds, or mixtures that are either homogeneous or heterogeneous. The key concepts covered include the states of matter, phase changes, and the classification of matter.
III STUDY GUIDEChemistry and Physics of Fire and FireProtecti.docxMARRY7
III STUDY GUIDE
Chemistry and Physics of Fire and Fire
Protection Systems and Equipment
Reading
Assignment
Chapter 4:
Chemistry and Physics of
Fire
Chapter 12:
Fire Protection Systems and Equipment
Additional Required
Reading
See information below.
Supplemental
Reading
See information below.
Key Terms
1. Ambient temperature
2. Bonnet
3. Fire department connection
4. Free radicals
5. Halogenated agents
6. Latent heat of vaporization
7. Miscible
8. Molecule
9. Nonmiscible
10. Open screw and yoke valve (OS&Y)
11. Oxidation
12. Oxidizer
13. Polar solvents
14. Post indicator valve
(PI)
15. Pyrolysis
16. Retard chamber
17. Thrust block
Learning Objectives
Upon completion of this unit, students should be able to:
1. Describe the differences between fire triangle and fire tetrahedron.
2. Illustrate the comparison between chemistry of fire and physics of fire.
3. Differentiate the principles of flame spread of solid, liquid, and gas/vapor fuels.
4. Describe classes of fire, stages of fire, and heat transfer during a fire.
5. Differentiate public and private water supply systems.
6. Illustrate the design and components of a water supply system.
7. Describe various extinguishing agents.
8. Illustrate the design and components of various types of extinguishing systems.
Written Lecture
Introduction
In this unit we will explore the world of the chemistry and physics of fire found in Chapter 4. We will also explore Chapter 12 where we will consider fire protection systems and the equipment associated with fire protection systems.
Chapter 4: Chemistry and Physics of Fire
Definition of fire: Fire is a rapid and self-sustaining oxidation process that is assisted by the generation of heat and light in various degrees of intensity. As stated in your textbook, fire is the process of oxidation and is associated with the term combustion, which is the chemical chain reaction that releases both light and heat. For all intents and purposes, fire is both friend and foe. We use fire for heating, cooking, manufacturing, and controlling other fire sources.
Fire triangle and fire tetrahedron: Perhaps as a child you were taught that fire was represented by a triangle with each side denoting one of the three components required to sustain fire: air, fuel, and heat. Classically known as the Fire Triangle we learned that by removing any one of the three components fire would be extinguished.
1
Over time, the scientific community has added another dimension called the chemical reaction found during the combustion process. With the addition of this fourth side we now have the new symbol of fire called the fire tetrahedron.
Chemistry of fire: Fire needs two basic elements in order to sustain its existence, and without the two in union, fire cannot occur. These two elements are oxidizer and fuel.
Oxidizer: An oxidizer is any substance that generates oxygen. The most common and abundant oxidizer ...
Fire requires four key elements - fuel, oxygen, heat, and a chemical chain reaction. These four elements form a tetrahedron shape to represent what is needed for fire. Each element must be present for combustion to occur and removing any one will extinguish the fire. Heat is transferred during fires through conduction, convection, and radiation. A fire goes through distinct stages from ignition to fully developed. Understanding how fires start and progress is important for fire investigation and arson detection.
Homogeneous catalysis involves substrates and catalysts in the same phase, often liquid, such as simple molecules, ions, and enzymes. Heterogeneous catalysis involves substrates and solid catalysts in different phases. Some key differences are that homogeneous catalysis often depends on pH and has higher heat and mass transfer rates, while heterogeneous catalysis can operate at higher temperatures and more easily separates products. Examples of each include acid-catalyzed reactions for homogeneous and the Haber process for heterogeneous catalysis.
This chapter discusses the chemistry and physics of fire. It defines the fire triangle and fire tetrahedron, and describes the key elements of fire - fuel, heat, and oxygen or oxidizer. It explains the states of matter and process of pyrolysis. Properties that affect different types of solid, liquid, and gas fuels are outlined. Heat and temperature are differentiated, and the methods of heat transfer are illustrated. The five classifications of fire and four stages of fire are described. Understanding the chemical and physical properties of fire allows for better control and prediction of fire behavior and choice of appropriate extinguishing methods.
This document discusses different types of changes in matter. It defines physical changes as changes that alter a substance's properties without changing its composition, giving examples like breaking, cutting, dissolving, and changes in state. Chemical changes are defined as changes involving one or more substances turning into new substances. The five states of matter are identified as solid, liquid, gas, plasma and Bose-Einstein condensate. Phase changes between these states are explained. The law of conservation of mass is also defined as mass being neither created nor destroyed in chemical reactions.
The document discusses various topics related to states of matter including:
- The three common states of matter are solids, liquids, and gases. Particles in each state are arranged differently and have different properties.
- Matter can change between solid, liquid, and gas states through heating and cooling. This involves absorbing or releasing energy in the form of latent heat.
- Other topics covered include vapor pressure, sublimation, critical points, and phase diagrams. The document provides definitions and examples for understanding different states of matter and changes between them.
The document provides an overview of a course on fire technology and arson investigation. It discusses key concepts like the fire triangle and tetrahedron, combustion, pyrolysis, oxidation, types of flames, heat transfer, fire behavior, stages of fire, and unique fire events like flashover and backdraft. The document contains lecture content, diagrams, questions, and notes that will be used for the course. It provides foundational knowledge on fire and combustion processes.
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Moving to Equilibrium - Burning Solids and Gases
1. MOVING TO EQUILIBRIUM
BURNING SOLIDS AND GASES: A COMPARISON
Abdur-Raheem As-Siddiq
Fire Behavior and Combustion
SOLID LIQUID LIQUID GAS GAS
2. DEFINITIONS
• Combustion – the process of energy release when one item
reacts completely with oxygen (Gann & Friedman, 2015, p.
79)
• Chemical Thermodynamics – the flow of enthalpy or
energy associated with reactions leading to a state of
chemical equilibrium (Gann & Friedman, 2015, p. 279)
• Chemical Equilibrium – the state in which all chemical
species are present at concentrations that have no further
tendency to change with time. All molecular compounds seek
this state. (Gann & Friedman, 2015, p. 279)
• Gas – A physical state of matter possessing perfect
molecular mobility, has low density, easily compressed, and
the property of indefinite expansion (Dictionary.com &
General Chemistry)
3. DEFINITIONS
Liquid – a physical state of material that is composed of
molecules that move freely amongst themselves with a
constant volume and consistency (Dictionary.com & General
Chemistry)
Molecule – The smallest particle of a substance that retains
all the properties of the substance and is composed of one or
more atoms (Gann & Friedman, 2015, p. 283)
Solid – a relatively dense, rigid state of matter, with a definite
volume and shape. (General Chemistry)
4. PROCESS OF COMBUSTION
Before we discuss the differences between the burning of a
solid versus the burning of a gas, we have to set a foundation
of what happens during combustion.
Anytime something “burns” it is a combustion reaction.
We will use the term “combustion” to describe the process
and “burn” to describe the energy that is released in the form
of heat and light as a result of “combustion.”
5. PROCESS OF COMBUSTION
Combustion is the culmination of four conditions (fuel, heat,
oxygen, chemical reaction) coming together simultaneously to
produce a change in molecular configuration. Commonly
referred to as the Fire Tetrahedron. (Gann & Friedman, 2015)
In simple terms, combustion is just breaking apart of
molecular compounds to form other molecular compounds.
This process is an exothermic reaction therefore it produces
energy. That energy is often experienced as heat and light.
6. PROCESS OF COMBUSTION
THE FIRE TETRAHEDRON
When these
four
conditions
reach their
respective
appropriate
levels, they
begin the
process of
combustion
7. PROCESS OF COMBUSTION
As an easy demonstrative example of combustion, let’s look at the
combustion of methanol (rubbing alcohol):
CH3OH + O2 CO2 + 2H2O + Heat
1. We begin with the molecular compound as methanol (CH3OH)
2. Oxygen is introduced (O2)
3. Heat is generated and a chemical reaction ensues.
4. The result is a breakdown of methane and the formulation of two
different molecular compounds, Carbon Dioxide and Water. (CO2),
(2H2O)
5. The energy generated from the reaction (combustion) is more heat.
Combustion - breaking apart of molecular compounds to form other
molecular compounds
(Combustion Reactions)
8. COMBUSTION OF A SOLID
In the most simplest of terms, the solid itself does not
“burn”.
The solid goes through a physical change process once
a sufficient amount of heat is applied to begin
combustion.
Combustion starts the molecular compound’s journey to
reach chemical equilibrium.
9. COMBUSTION OF A SOLID
Gann & Friedman discuss the physical and
chemical change of solids in their book
Principles of Fire Behavior and Combustion
(2015). They conclude that when a solid
changes state due to combustion, it goes
through five thermochemical steps. Those
steps are (p. 34):
1. The temperature of the solid rises
2. The solid melts, or fuses, becoming a liquid
3. The temperature of the liquid rises
4. The liquid vaporizes, or gasifies
5. The gas temperature rises
11. • The stages of change incorporate both physical and chemical
change depending on what is happening at any given time.
• Whenever heat is being absorbed, this stage is considered purely
a physical change.
• Whenever the matter changes density, is an indication of
chemical change (i.e. the molecular compounds shifted in
configuration). (Gann & Friedman, p. 34)
STAGE TYPE OF CHANGE
The temperature of the solid rises physical change
The solid melts, or fuses, becoming a liquid chemical change
The temperature of the liquid rises physical change
The liquid vaporizes, or gasifies chemical change
The gas temperature Rises physical change
COMBUSTION OF A SOLID
12. COMBUSTION OF A SOLID
• We will use a sugar molecule to demonstrate the combustion
process for a solid
• As we showed in the methanol combustion, the result will be that
sugar will cease to exist.
HYDROGEN
HYDROGEN
HYDROGEN
HYDROGEN
HYDROGEN
HYDROGEN
HYDROGEN
HYDROGEN
HYDROGEN
HYDROGEN
HYDROGEN
HYDROGEN
OXYGEN
OXYGEN
OXYGEN
OXYGEN
OXYGENCARBON
CARBON
CARBON
CARBON
CARBON
CARBON
SUGAR
C6H12O6
OXYGEN
13. C6H12O6 6 O2
6 CO2 6 H2O
COMBUSTION OF A SOLID
SUGAR OXYGEN
CARBON
DIOXIDE
WATER
1. Sugar is exposed to heat
2. The heat causes the molecular compounds in
sugar to destabilize and react with oxygen
3. A chemical reaction ensues
4. The molecular compound of sugar is disrupted
and form new compounds
5. Carbon Dioxide and Water are produced
6. Sugar ceases to exist (Solid ceases to exist)
7. The process continues through physical and
chemical changes until chemical equilibrium is
achieved.
(The Combustion Reaction)
14. COMBUSTION OF A GAS
• As we used sugar as a demonstrative example for solid
combustion, we will use methane as an example of the combustion
process for gases.
• Methane is a natural gas that is commonly used as fuel and is the
major component of gas used in kitchens and heaters.
• The molecular formula for Methane is CH4 – One (1) Carbon
molecule and 4 Hydrogen atoms.HYDROGEN
HYDROGEN
HYDROGEN
HYDROGEN
CARBON
(The Combustion Reaction)
15. COMBUSTION OF A GAS
METHANE OXYGEN
CARBON DIOXIDE WATER
O2CH4
CO2 H2O
1. Methane is exposed to heat
2. The heat causes the molecular compounds in
methane to destabilize and react with oxygen
3. A chemical reaction ensues
4. The molecular compound of methane is
disrupted and forms new compounds
5. Carbon Dioxide and Water are produced
6. Methane ceases to exist
7. The process continues through physical and
chemical changes until chemical equilibrium is
achieved.
(The Combustion Reaction)
16. SOLIDS AND GASES
The process of combustion is fundamentally the same
whether it is a solid or vapor (gases).
The difference between them is what occurs after
combustion.
Solids are at one end of the matter spectrum while
gases are on the opposite end.
During exothermic combustion, the molecules that
comprise solids continuously move through the chain of
events until they form molecules of gas.
Gases are the last stage before chemical equilibrium is
achieved.
17. SOLIDS AND GASES
HEAT
CHEMICAL
TRANSFORMATION
HEAT
CHEMICAL
TRANSFORMATION
HEAT
SOLID LIQUID LIQUID GAS GAS
• Exothermic combustion always moves in one direction – From Solid – to
Liquid – to Gas – to Equilibrium
• So you can say that in this process, Gas is an evolutionary product of a
solid in terms of combustion
• The reverse order, whereas the gas becomes a solid is a separate subject
that will be discussed in another class
18. SOLIDS AND GASES
Similarities between “burning” of solids and
gases:
• The combustion process (i.e. The Fire tetrahedron)
• The molecular compounds become increasingly unstable when heat
is applied
• The molecular compounds change to form new substances
METHANE
CH4C6H12O6
SUGAR
19. SOLIDS AND GASES
Differences between “burning” of solids and
gases:
• Solids don’t burn whereas gases do
• To reach equilibrium, solids pass through at least two stages of
chemical transformation
• Gases are only one stage away from reaching equilibrium
METHANE
CH4C6H12O6
SUGAR
20. CONCLUSION
Solids are at the beginning of the evolutionary scale
while gases are towards the end of the scale in the
combustion process
Solids don’t “burn” but gases do
In simple terms, “burning” or the process of combustion
is merely a physical and chemical change taking place
by means of energy transfer
Once combustion begins, its goal is to move toward
chemical equilibrium
The “combustion process” is the same between a solid
and a gas.
21. REFERENCES
Gann, R. & Friedman, R. (2015). Principles of fire behavior and
combustion (4th ed.). Burlington, MA: Jones and Bartlett.
Gas. (n.d.). Dictionary.com Unabridged. Retrieved February 28,
2017 from Dictionary.com
website http://www.dictionary.com/browse/gas
Gas. (n.d.). General chemistry online. Retrieved February 28,
2017 from General Chemistry Online! website
http://antoine.frostburg.edu/chem/senese/101/glossary/g.shtml)
Liquid. (n.d.). Dictionary.com Unabridged. Retrieved February
28, 2017 from Dictionary.com
website http://www.dictionary.com/browse/liquid Liquid. (n.d.).
General chemistry online. Retrieved February 28, 2017 from
General Chemistry Online! website
http://antoine.frostburg.edu/chem/senese/101/glossary/l.shtml)
22. REFERENCES
Solid. (n.d.). General chemistry online. Retrieved February 28,
2017 from General Chemistry Online! website
http://antoine.frostburg.edu/chem/senese/101/glossary/s.shtml)
Combustion Reactions. (n.d.) Indiana University Northwest.
Retrieved February 28, 2017 from
http://www.iun.edu/~cpanhd/C101webnotes/chemical%20reactio
ns/combustion.html
The Combustion Reaction. (n.d.). University Federico II of
Naples, Italy, European Chemistry Thematic Network. Retrieved
February 27, 2017 from
http://www.whatischemistry.unina.it/en/burn.html
The Combustion Reaction. (n.d.). University Federico II of
Naples, Italy, European Chemistry Thematic Network. Retrieved
February 27, 2017 from
http://www.whatischemistry.unina.it/en/combust.html
Editor's Notes
University Federico II of Naples, Italy, European Chemistry Thematic Network, The Combustion Reaction (No Date) No Author
http://www.whatischemistry.unina.it/en/burn.html