Introduction to gases
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The document discusses the properties of gases and how various factors can affect gas pressure. It explains that gases are easy to compress because the particles can be squeezed closer together, and that gas pressure is determined by four variables - pressure, volume, temperature, and amount of gas. It also outlines how changing any of these variables, such as decreasing the volume or increasing the temperature, will affect the pressure of an enclosed gas.
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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 ...
Chemistry - Chp 14 - The Behavior of Gases - Notes
The document describes factors that affect gas pressure, including the amount of gas, volume of the container, and temperature. It explains that gases are easily compressed and expand to fill their container, unlike solids or liquids. The document also provides the key variables used to describe gases and discusses several gas laws relating pressure, volume, temperature, and amount of gas.
2-7 Gas Laws
The document discusses the gas laws and how temperature, pressure, and volume of a gas are related. It defines key terms like pressure, temperature, and volume. It explains Boyle's law, Charles' law, and the combined gas law. Boyle's law states that if temperature and amount of gas are kept constant, pressure and volume are inversely related. Charles' law states that if pressure and amount of gas are kept constant, volume and temperature are directly related. The combined gas law incorporates all factors - if temperature increases while amount and volume remain constant, pressure will also increase.
Chapter 12.3 : Changes of State
This document discusses changes of state and phase equilibria. It defines equilibrium as a dynamic condition where opposing changes occur at equal rates in a closed system. Equilibrium is established between phases, such as liquid and vapor, when the rate of evaporation equals the rate of condensation. Le Chatelier's principle states that if a system at equilibrium is disturbed, it will shift to a new equilibrium that minimizes the stress. Phase diagrams graphically depict the conditions under which different phases exist in equilibrium.
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Introduction to gases
- 1. Reference text: 14.1 page 413-417
- 2. Solid Liquid Gas Which has a specific volume? Which has a specific shape?
- 3. Compressibility – how much the volume of matter decreases under pressure A gas can be squeezed into a small space See the all the space between the gas particles? The particles can be squeezed closer together under pressure
- 4. Pressure is the force the gas molecules exert on the container as they collide with it Four variables to describe a gas: Pressure (P): measured in kilopascals (kPa) Volume (V): measured in liters (L) Temperature (T): measured in kelvins (K) Amount (n): measured in number of moles
- 5. When you pump air into a container, you increase the amount of gas inside the tire, which increases the number of collisions between gas particles, which increases the pressure Relationship is direct: If you double the amount of gas, the pressure will double
- 6. Fewer gas particles, lower pressure More gas particles, higher pressure
- 7. In a sealed container, gases move from an area of high pressure to low pressure
- 8. If the volume of a container is reduced, the pressure will increase
- 9. If the volume of a container is increased, the pressure will decrease Relationship is inverse If the volume is doubled, the pressure will decrease by half
- 10. If the temperature is increased, the particles will move faster, Which causes more collisions between particles Which increases the pressure
- 11. Increasing the temperature causes the pressure to increase
- 12. Decreasing the temperature will cause the pressure to decrease Relationship is direct As the temperature is doubled, the pressure is doubled As the temperature is decreased by half, the pressure will decrease by half
- 13. 1. Why is a gas easy to compress? 2. List three factors that can affect gas pressure. 3. Why does a collision with an air bag cause less damage than a collision with a steering wheel? (extra help) 4. How does a decrease in temperature affect the pressure of a contained gas? 5. If the temperature is constant, what change in volume would cause the pressure of an enclosed gas to be reduced to one quarter of its original volume? 6. What happens to particle motion as the temperature increases? What if it decreases? 7. Write a paragraph explaining how the compressed gas in an aerosol can force paint out of the can. Describe how the gas pressure inside the can changes as the paint is sprayed, and identify the variable that causes this change. Refer to figure 14.5 in the text.