Kinetic theory
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1. The kinetic theory states that all matter is composed of small particles that are in constant motion and that particle collisions are perfectly elastic. 2. Pressure is caused by particle collisions with container walls, and can be directly or inversely proportional to temperature and volume. Standard atmospheric pressure is 101.325 kPa. 3. Particle speed depends on temperature and mass, with lighter particles moving faster at the same temperature. Temperature is measured in Kelvin and relates to molecular motion and gas pressure.
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This document provides an introduction to elements of mechanical engineering. It defines key concepts related to prime movers, sources of energy, types of prime movers, and basic definitions of force, mass, pressure, work, power, energy, heat, temperature, and the laws of thermodynamics. It also describes properties of gases according to the kinetic molecular theory and outlines the gas laws of Boyle, Charles, Gay-Lussac, the combined gas law, and the ideal gas law. Finally, it discusses non-flow processes, the relationship between specific heats, and properties of steam.
Basics of Thermodynamics-1.pptx
Thermodynamics deals with stability of systems and tells us what should happen. It concerns heat, work, temperature, pressure, volume and equilibrium. The laws of thermodynamics relate these macroscopic properties and describe spontaneous processes and the behavior of systems as they approach absolute zero. Thermodynamics considers systems as either open, closed, or isolated and can undergo various processes like isothermal, isobaric, or adiabatic processes between different equilibrium states.
B.tech i eme u 1 intoduction
This document provides an overview of key concepts in elements of mechanical engineering related to prime movers and thermodynamics. It defines prime movers as engines that convert fuel to useful work and lists various energy sources and types of prime movers. The document also defines fundamental concepts such as force, mass, pressure, work, power, energy, heat, temperature and thermodynamic laws. It describes gas properties and the gas laws including Boyle's law, Charles' law, Gay-Lussac's law, the combined gas law and the ideal gas law.
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
Chapter 3(heat and properties)
Temperature can be measured using a thermometer and is expressed in different scales like Celsius, Fahrenheit and Kelvin. Heat is the transfer of energy between objects due to a temperature difference and is measured in Joules. The specific heat of a substance is the amount of heat required to raise its temperature by 1°C or 1K. Phase changes like melting, freezing, vaporization and condensation involve heat and are characterized by heat of fusion and heat of vaporization values. Solids have a definite shape and volume while liquids and gases have indefinite shapes but definite and indefinite volumes respectively. Density is a property that relates the mass and volume of a substance.
Spontaneity-Entropy-and-Free-Energy.ppt
The document discusses key concepts in chemical thermodynamics including:
1) The first law of thermodynamics states that energy cannot be created or destroyed, only converted from one form to another.
2) Spontaneous processes are those that can proceed without outside intervention. Processes that are spontaneous in one direction are nonspontaneous in the reverse direction.
3) Entropy is a measure of the randomness or disorder of a system. It increases for spontaneous processes according to the second law of thermodynamics.
4) The Gibbs free energy, ΔG, can be used to determine whether a process is spontaneous, with a negative ΔG corresponding to a spontaneous process.
Thermodynamics
Thermodynamics is the study of heat and its relationship to other physical phenomena such as work, temperature and energy. It examines the macroscopic behavior of materials using variables like pressure, volume and temperature rather than their microscopic constitution. Thermodynamics establishes that heat is a form of energy transfer between systems due to a temperature difference, and explores the behavior of gases, liquids and solids through concepts like the ideal gas law, thermal expansion, and heat transfer via specific heat capacity.
Ideal gas law
The document discusses the ideal gas law and its relationship between the pressure, volume, temperature, and amount of gas. It defines Boyle's law, Charles' law, Gay-Lussac's law, and how they combine to form the ideal gas law (PV=nRT). It provides the definitions and units for pressure, volume, temperature, moles, and the gas constant in the ideal gas law. Examples are given for converting between pressure units and using the ideal gas law to calculate moles or temperature given the other variables.
Principal of gases, gas law flow of
This document discusses gas laws and the behavior of gases. It covers topics like gas pressure, temperature, Boyle's law, Charles' law, the three states of matter, diffusion and effusion of gases, Dalton's law of partial pressures, Henry's law, the ideal gas law, laminar and turbulent gas flow, and the clinical implications of gas behavior. Key points include that gas pressure is caused by molecular collisions, Boyle's law states that pressure and volume are inversely proportional at constant temperature, and Charles' law relates volume and temperature changes at constant pressure.
GAS LAWS Boyle's Charles law ideal gas law
The document discusses the kinetic molecular theory and properties of gases. It explains that gas particles are in constant, random motion with no attraction between particles. It also describes gas pressure, temperature, volume, and the relationships between these properties as defined by Boyle's law, Charles' law, Gay-Lussac's law, and the combined gas law. Examples are provided for using these gas laws to calculate changes in gas properties like volume under different conditions.
GAS LAWS Gas is one of four natural states of matter, along with liquid, soli...
The term gas is also used in reference to the state itself when applied to matter that has the properties of a gaseous substance.
UNIT 08 HEAT AND THERMODYNAMICS PART 1.pptx
Thermodynamics is the same thing as a new one doubt the same way that has been done in the past and I will not have to be the same way that you can get to the developing society and the same way you could have to go to a 3coincidence and hip 3hop or the one mark you ok you ok baby and I think you 6th grade girls are you mad at jiosaavn and 5th 6th class la school name 5PM but I don't know how to check a value for 6a and I have to do it in a month or so on a bit 6th 6th grade but I don't want a bit more of a 6th grade teacher sex drive I 5am a lot more attractive to me than daNa point of a year and two of my 6relationship classes leave the same way of being in tamil or Asian and I have a good idea for a given time of engineering coi or a bit more than a few years of experience in the universe that has the ability
Properties of Gases
The document discusses the gas laws and properties of gases. It begins by describing the composition of Earth's atmosphere, which is primarily nitrogen and oxygen. It then discusses that gases have mass and low densities compared to liquids and solids. The document outlines four variables that describe gases - pressure, volume, temperature, and amount. It explains concepts such as gas compressibility, units of measurement for gases, and the kinetic molecular theory which describes gas particles as being in constant random motion.
01 part1-ideal-gas
This document discusses ideal gases and their properties. It defines an ideal gas as a theoretical gas composed of point-like particles that obey gas laws perfectly. Some key properties of ideal gases are that they have negligible volume and mass and undergo perfectly elastic collisions. The document also covers gas laws such as Boyle's, Charles', and Gay-Lussac's laws. It provides the ideal gas equation of state and defines terms like molar mass, gas constant, pressure units and heat capacities. Several example problems applying the ideal gas law are also included.
Chapter10.pdf
This document provides an overview of key concepts related to gases, including:
- Characteristics of gases and units of pressure like atmospheres and torr
- Gas laws like Boyle's, Charles', and Avogadro's laws and how they relate to the ideal gas equation
- How to calculate variables like pressure, volume, moles, and temperature using the ideal gas equation
- Kinetic molecular theory and how it explains gas behavior and properties
- Deviations from ideal gas behavior at high pressures or low temperatures
- The van der Waals equation for correcting for non-ideal behavior
Thermodynamic, part 1
Thermodynamics is the study of heat, work, and energy. It describes macroscopic properties of systems in thermal equilibrium. A system is defined along with its surroundings and properties. Systems can be open, closed, or isolated. Thermodynamic properties include extensive properties that depend on system size and intensive properties that do not. The four laws of thermodynamics relate temperature, heat, work, and energy within a system. Heat transfer and phase changes involve latent heat in addition to specific heat.
Basic concept and first law of thermodynamics
This document provides an introduction to engineering thermodynamics. It defines key terms like heat, power, temperature, and the science of thermodynamics. It describes different types of thermodynamic systems like closed, open, isolated, homogeneous, and heterogeneous systems. The document outlines thermodynamic properties, processes, cycles, and the first law of thermodynamics. It also reviews the laws of perfect gases and examples of thermodynamic processes like isothermal, isobaric, isochoric, reversible, and adiabatic processes.
Unit 7 Presentation.ppt
The document provides an overview of kinetic theory and the states of matter. It discusses the following key points:
- Kinetic theory states that all matter is made of tiny particles in constant motion. The behavior of solids, liquids, and gases can be understood through this model.
- There are five states of matter: solid, liquid, gas, plasma, and Bose-Einstein condensate. Solids have tightly packed particles that don't move much. Liquids have spread particles that move slowly. Gases have very far apart particles that move very fast.
- Phase changes between states, such as melting, boiling, and condensation, occur when sufficient thermal energy is added to or
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Kinetic theory
- 1. 1 The 3 Basic Assumptions of the Kinetic Theory 1. All matter is composed of small particles (atoms ions or molecules)particles (atoms, ions, or molecules) 2. These small particles are in constant motion 3. All collisions between particles are perfectly elasticperfectly elastic. - there is no change in total Kinetic Energy of two particles before and after their collision Pressure • Caused by the force of collision and the # of collisions with the walls of athe # of collisions with the walls of a container • Standard Pressure (avg. air pressure at sea level) = 101.325 kPa • Pressure can be directly or inverselyPressure can be directly or inversely related or proportional to other characteristics of gases (temp, volume)
- 2. 2 Standard Atmospheric Pressure 101.325 kPa101.325 kPa 760 mmHg 760 torr 14.7 psi All of these represent the same pressure – Standard Atmospheric Pressure – just inp 1 atm 29.92 inHg different pressure units Converting Pressure Units 1. Write down what you’re given 2. Conversion factor: units)(originalPressureStandard units)(desiredPressureStandard 3. Cancel units and solve units)(originalPressureStandard
- 3. 3 Example Convert: 477 kPa = ___________ torr What would the pressure 26.5 psi be if it × kPa477 = kPa101.325 torr760 torr 101.325 362520 torr5803= p p were expressed in units of in Hg? × psi6.52 = psi14.7 inHg92.29 inHg 14.7 88.792 inHg9.53= Factors Affecting Molecular Motion • Speed of gas particles depends on: –Temperature –Mass of the particle • Lighter gases travel faster thang g heavier gases (at the same temperature)
- 4. 4 Effects of Temperature on Molecular Motion • Temperature of a substance is the avg• Temperature of a substance is the avg. KE of its particles • A decrease in temperature causes decrease in speed Sl d f lli i• Slower speed = fewer collisions lower pressure Temperature (cont.) • Standard unit of temperature = Kelvin (K) • Absolute zero – temperature at which all molecular motion ceases –(0 K = -273.15°C) –Round to –273 °C • Conversion between K and °C: K = °C + 273
- 5. 5 Temperature Conversion Equations • Celsius Fahrenheit • Fahrenheit Celsius • Celsius Kelvin 32)8.1T(T CF +×= 8.1 )32T( T F C − = 273TT + • Kelvin Celsius • Fahrenheit Kelvin? Combine equations! 273TT KC −= 273TT CK += States of Matter Gases • Independent, straight-line motion • Change direction only following collisions • Gas molecules travel in a random manner • Gases assume the shape and volume of their container. G
- 6. 6 States of Matter Liquid • Restricted particle motion • Particles vibrate and slip past one another • Liquids have a definite volume but• Liquids have a definite volume, but assume the shape of their container L States of Matter Solids • Highly restricted particle motiong y p • Particles vibrate around a fixed point • Particles arranged in a definite pattern • Solids have a definite volume and a definite shapedefinite shape S