Thermal expansion
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Most matter expands when heated and contracts when cooled. The volume of a material generally increases as its temperature increases, with the fractional change in length or volume defined as the coefficient of linear expansion. Charles' Law states that for a given temperature change, all gases expand by the same amount of volume, while Boyle's Law says the volume of a gas varies inversely with pressure if temperature is held constant. The General Gas Law combines these, relating the pressure, volume, and temperature of a gas.
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Heat and temperature are related but distinct concepts. Temperature is a measure of the average kinetic energy of molecules, while heat is the transfer of energy between objects due to a temperature difference. Heat is measured in joules, while temperature has several scales including Celsius, Fahrenheit and Kelvin. When objects at different temperatures are brought into contact, heat flows spontaneously from the warmer to the cooler object until thermal equilibrium is reached and they have the same temperature, as stated by the zeroth law of thermodynamics. Materials expand and contract with changes in temperature. The amount of expansion depends on properties of the material such as its coefficient of linear, area or volume expansion. Phase changes between solid, liquid and gas involve latent heat, which
GAS BEHAVIOUR & GAS LAWS
This document discusses several gas laws including Boyle's law, Charles' law, Gay-Lussac's law, and Avogadro's law. Boyle's law states that at constant temperature, the volume of a gas is inversely proportional to its pressure. Charles' law specifies that at constant pressure, the volume of a gas is directly proportional to its temperature. Gay-Lussac's law describes how pressure and temperature are directly proportional at constant volume. Finally, Avogadro's law concerns the relationship between volume and number of moles of gas at constant temperature and pressure.
Lecture on thermodynamics
This document provides an overview of thermodynamics concepts. It defines thermodynamics as dealing with energies of gases and vapors in terms of heat and work. It describes three types of thermodynamic systems - closed, open, and isolated. It also defines extensive and intensive properties. The document then explains the zeroth, first, and second laws of thermodynamics. It concludes by describing various thermodynamic processes like isobaric, isothermal, adiabatic, and throttling processes.
Gas Laws
Kinetic Gas Theory including Ideal Gas Equation. Temperature, Volume, Applications
Boyle's Law, Charles' Law and Avogadro's Law. Ideal Gas Theory, Dalton's Partial Pressure
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Physicochemical properties of drug molecules: Refractive index, optical rotation, dielectric constant, dipole moment, dissociation constant, determinations and applications
Unit 2 states of matter
States of Matter and properties of matter: State of matter, changes in the state of matter, latent heats, vapour pressure, sublimation critical point, eutectic mixtures, gases, aerosols – inhalers, relative humidity, liquid complexes, liquid crystals, glassy states, solid- crystalline, amorphous & polymorphism.
Physicochemical properties of drug molecules: Refractive index, optical rotation, dielectric constant, dipole moment, dissociation constant, determinations and applications
Boyle report
1) The document summarizes an experiment on Boyle's law and Gay-Lussac's law.
2) Boyle's law states that for a fixed amount of gas at constant temperature, the product of pressure and volume is constant. Gay-Lussac's law states that for a fixed amount of gas at constant volume, pressure and temperature are directly proportional.
3) The experiment aims to demonstrate these gas laws experimentally by measuring how the pressure of air changes with volume at constant temperature for Boyle's law and how pressure changes with temperature at constant volume for Gay-Lussac's law.
1 a. pneumatic introduction, gas laws
This document discusses pneumatic and electro-pneumatic systems. It covers the properties of air and gases, including the ideal gas laws of Boyle's law, Charles' law, Avogadro's law, and Dalton's law of partial pressures. It also discusses key components of pneumatic systems like compressors, filters, regulators, valves and actuators. The document introduces electro-pneumatic systems and their elements, as well as pneumatic logic circuits.
GAS LAWS AND THEIR APPLICATION.ppt
This document discusses the laws governing the behavior of gases and their applications in anesthesia. It introduces Boyle's law, Charles' law, Gay-Lussac's law, Avogadro's law, Henry's law, and Dalton's law. It then discusses applications of these laws to oxygen, nitrous oxide, Entonox, Heliox, and volatile anesthetic agents. Specifically, it explains how the gas laws can be used to calculate oxygen volumes and nitrous oxide amounts in cylinders. It also discusses how Henry's law relates anesthetic vapor pressures to their blood concentrations.
Gas laws
The document discusses several gas laws including Boyle's law, Charles' law, Avogadro's law, and Gay-Lussac's law. It provides the formulas for each law and graphs demonstrating the relationships between pressure, volume, temperature, and number of moles for ideal gases. It also discusses how real gases deviate from ideal gas behavior and provides the combined gas law formula.
gas laws in anesthesia
This document discusses the gas laws and their clinical applications. It covers the key gas laws including Boyle's law, Charles' law, Gay-Lussac's law, Dalton's law of partial pressures, Henry's law, and the combined gas law. Some clinical applications mentioned are spirometry, effects of altitude on oxygen levels, use of cryoprobes, and properties of gases like nitrous oxide that are relevant to anesthesia. The document also defines important gas properties and concepts such as the ideal gas, STP, critical temperature, and pseudocritical temperature.
Cmcchapter13 100613153048-phpapp02
The document outlines key concepts about the gas laws from three sections:
Section 13.1 discusses Boyle's law, Charles's law, and Gay-Lussac's law which describe the relationships between pressure, volume, and temperature for gases. It also introduces the combined gas law.
Section 13.2 introduces the ideal gas law and how it relates the number of gas particles to pressure, volume, and temperature using the ideal gas constant. It compares properties of real and ideal gases.
Section 13.3 explains how to use gas stoichiometry and the mole concept with chemical equations involving gases to determine volume and amount relationships between reactants and products.
Gaseous state
Gases are composed of tiny particles that are in constant, random motion. Three properties of gases are pressure, volume, and temperature. The kinetic molecular theory and gas laws describe the relationships between these properties. The ideal gas law combines earlier gas laws relating pressure, volume, amount of gas, and temperature into a single equation.
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State of matter and properties of matter (Part-4) (Gases, Ideal gas law)
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- 1. In Solids, Liquids and Gases
- 2. Most matter expands when heated and contracts when cooled General increase in the volume of a material is its temperature is increased Fractional change in length or volume per unit temperature change
- 3. ∆𝐿 = 𝛼𝐿𝑜∆𝑇Change in Length Coefficient of Linear Expansion Change in Temperature Original Length
- 4. Charles Law (constant pressure) -For a given temperature change, all gases expanded by the same amount of volume. - 𝑉1 𝑉2 = 𝑇1 𝑇2
- 5. Boyle’s Law -If temperature held constant, the volume of the gas varies inversely with its pressure. - 𝑃1 𝑉1 = 𝑃2 𝑉2
- 6. General Gas Law -Combination of Charles Law and Boyle’s Law - 𝑃1 𝑉1 𝑇1 = 𝑃2 𝑉2 𝑇2
- 7. With the pressure held constant, the volume of a gas will be doubled if its temperature is increased from 120°C to what final temperature?