Lec 02 15042013
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This document provides definitions and concepts related to thermodynamics. It discusses how thermodynamics deals with the conversion of energy from one form to another. Key points include: - Thermodynamics analyzes energy processes and relationships between heat, work, and systems. It is governed by the conservation of energy principle. - Temperature indicates heat flow direction. Heat is the form of energy transferred between systems due to a temperature difference. - Systems can be open, closed, or isolated depending on if mass and/or energy cross the boundary. Properties can be intensive or extensive. - Thermodynamic equilibrium occurs when there are no unbalanced potentials within a system, such as when temperature is uniform throughout (thermal
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Lec 03 18042013.pptx
This document discusses properties of systems and concepts in thermodynamics including:
- Intensive properties are independent of system size while extensive properties depend on system size. Temperature is intensive while mass and volume are extensive.
- A system is in equilibrium when there are no unbalanced potentials within the system. Thermal, mechanical, and phase equilibriums are discussed.
- The zeroth law of thermodynamics states that two bodies in thermal equilibrium with a third are in equilibrium with each other, establishing temperature. Temperature scales like Kelvin and Rankine are then introduced.
Laws of thermodynamics
The four laws of thermodynamics define fundamental physical quantities like temperature, energy, and entropy that characterize systems in thermal equilibrium, and describe how these quantities behave under different conditions, prohibiting certain phenomena like perpetual motion. The laws were established after Count Rumford showed in 1797 that mechanical action can generate unlimited heat from a fixed amount of material, challenging earlier theories of heat. The first law was then formulated by Sadi Carnot in 1824.
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This document provides an overview of basic thermodynamic concepts including:
1. It defines thermodynamic systems as specified collections of matter that can be open, closed, isolated, or adiabatic depending on whether mass and energy are exchanged.
2. It explains that thermodynamics describes how changes in a system's state like temperature and pressure affect equilibrium using mathematical models.
3. It lists some key thermodynamic variables like extensive and intensive properties, entropy, phases, components, and solutions.
4. The master equation shows how changes in Gibbs free energy depend on changes in chemical potential, molar volume, pressure, entropy, temperature, and mole fractions of phases in a system.
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This document discusses concepts related to energy and heat. It defines temperature and explains that temperature is related to the kinetic energy of atoms and molecules. It explores the relationship between energy, work, and heat, noting that heat refers to the transfer of energy between systems with a temperature difference. The document also discusses historical theories of heat and caloric and introduces the modern idea that heat is related to the motion of particles and internal energy of a system.
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Lec 03 18042013.pptx
This document discusses properties of systems and concepts in thermodynamics including:
- Intensive properties are independent of system size while extensive properties depend on system size. Temperature is intensive while mass and volume are extensive.
- A system is in equilibrium when there are no unbalanced potentials within the system. Thermal, mechanical, and phase equilibriums are discussed.
- The zeroth law of thermodynamics states that two bodies in thermal equilibrium with a third are in equilibrium with each other, establishing temperature. Temperature scales like Kelvin and Rankine are then introduced.
Laws of thermodynamics
The four laws of thermodynamics define fundamental physical quantities like temperature, energy, and entropy that characterize systems in thermal equilibrium, and describe how these quantities behave under different conditions, prohibiting certain phenomena like perpetual motion. The laws were established after Count Rumford showed in 1797 that mechanical action can generate unlimited heat from a fixed amount of material, challenging earlier theories of heat. The first law was then formulated by Sadi Carnot in 1824.
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This document provides an overview of basic thermodynamic concepts including:
1. It defines thermodynamic systems as specified collections of matter that can be open, closed, isolated, or adiabatic depending on whether mass and energy are exchanged.
2. It explains that thermodynamics describes how changes in a system's state like temperature and pressure affect equilibrium using mathematical models.
3. It lists some key thermodynamic variables like extensive and intensive properties, entropy, phases, components, and solutions.
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This document discusses the difference between temperature and heat. It defines temperature as a physical property that underlies perceptions of hot and cold, with higher temperature meaning greater molecular kinetic energy. Heat is defined as energy transferred between bodies or systems due to a temperature difference. The document also discusses different temperature scales like Fahrenheit, Celsius, and Kelvin and the types of molecular motion and energy, including translational, vibrational, and rotational energy of molecules. It aims to distinguish temperature and heat which are often confused but related concepts regarding thermal energy.
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Law's of thermodynamics
The document summarizes the main laws of thermodynamics:
The First Law states that energy can neither be created nor destroyed, only changed in form. The Second Law states that heat spontaneously flows from hotter to colder bodies until they reach the same temperature. Entropy, a measure of disorder, always increases over time as energy spreads out. The Third Law establishes that entropy approaches a minimum, constant value as temperature approaches absolute zero. The Zeroth Law defines temperature as a physical property of a system, such that systems in thermal equilibrium have the same temperature.
Worksheet first law
The First Law of Thermodynamics states that energy cannot be created or destroyed, only transferred or changed in form. For any process, the change in internal energy of a system is equal to the heat added to the system minus the work done by the system. Heat is the transfer of energy between systems due to a temperature difference, while work is the transfer of energy by a force acting through a distance. Endothermic processes absorb heat from the surroundings, while exothermic processes release heat.
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Thermal energy transfer notes
Thermal energy is the kinetic energy of particles in a substance that are constantly in motion. The amount of thermal energy determines the temperature, and it can be transferred from warmer objects to cooler ones through three main processes: conduction, convection, and radiation. Conduction involves the direct transfer of thermal energy between objects or particles that are touching. Convection occurs through the circulation of fluids, where warmer material rises and cooler material sinks. Radiation allows thermal energy to be transferred through empty space by electromagnetic waves like light.
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The document discusses key concepts in temperature physics including:
1) It defines temperature as a variable that measures "hot" and "cold" and is related to the internal kinetic energy of an object or substance.
2) It provides formulas for converting between Celsius and Fahrenheit temperature scales.
3) It explains that thermal energy is the total kinetic and potential energy of all particles in a substance, and increases with higher temperature as the particles' kinetic energy increases.
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Thermal energy can be transferred between objects in three ways: conduction, convection, and radiation. Conduction occurs when particles in materials collide with neighboring particles. Convection is the transfer of thermal energy by the movement of molecules within a material. Radiation occurs through electromagnetic waves and can transfer energy through empty space. Some materials are better conductors or insulators of thermal energy depending on their composition and molecular structure. The transfer of excess warm water into bodies of water can cause thermal pollution, raising the temperature and reducing oxygen levels, harming aquatic life. Cooling towers can help reduce thermal pollution by lowering the temperature of warm water before release.
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The document provides an overview of statistical thermodynamics including:
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- The key difference between classical thermodynamics and statistical thermodynamics is that the latter links microscopic properties to macroscopic behaviors.
- Statistical thermodynamics is needed to explain thermodynamic parameters in terms of molecular properties and interactions since classical thermodynamics does not address this microscopic level.
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This document provides an introduction to a thermodynamics course. It defines thermodynamics as the study of heat and work transfer on a specified system. A system is any part of the universe being studied, separated from its surroundings by a real or imaginary boundary. The document outlines different types of systems (isolated, closed, open) and phases of matter (solid, liquid, gas). It also defines important thermodynamic concepts like state, equilibrium, properties, processes, the laws of thermodynamics, and heat transfer including latent heat and phase changes.
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The scientific method is used to make observations, form hypotheses and laws, and conduct experiments to test hypotheses. Scientific theories are hypotheses that have been supported through many experiments. Scientific laws provide mathematical relationships that describe observable phenomena without explaining them. Accuracy refers to how close a measurement is to the true value, while precision refers to the reproducibility of measurements. Significant figures are used to indicate the precision of measurements in calculations.
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Thermal energy is the kinetic energy of particles in a substance that are constantly in motion. The amount of thermal energy determines the temperature, and it can be transferred from warmer objects to cooler ones through three main processes: conduction, convection, and radiation. Conduction involves the direct transfer of thermal energy between objects or particles that are touching. Convection occurs through the circulation of fluids, where warmer material rises and cooler material sinks. Radiation allows thermal energy to be transferred through empty space by electromagnetic waves like light.
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Thermal energy is related to the kinetic energy and potential energy of molecules. The temperature of an object is a measure of the average kinetic energy of its molecules - the higher the temperature, the faster molecules move and the more kinetic energy they have. When temperature increases, molecules speed up and objects expand; when temperature decreases, molecules slow down and objects contract. Thermometers measure temperature by using the expansion and contraction of liquid in a tube in response to temperature changes. Common temperature scales are Celsius, Fahrenheit, and Kelvin.
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Heat transfer deals with the amount of heat transferred between systems or objects at different temperatures. There are three main modes of heat transfer: conduction, convection, and thermal radiation. Conduction involves the transfer of heat through direct contact of objects, convection involves the transfer of heat by a moving fluid, and thermal radiation involves the emission and transmission of electromagnetic waves. Heat transfer is important in engineering applications where the rate and distribution of heat transferred over time, such as in heaters, refrigerators, and other appliances, can impact efficiency.
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The document discusses key concepts in temperature physics including:
1) It defines temperature as a variable that measures "hot" and "cold" and is related to the internal kinetic energy of an object or substance.
2) It provides formulas for converting between Celsius and Fahrenheit temperature scales.
3) It explains that thermal energy is the total kinetic and potential energy of all particles in a substance, and increases with higher temperature as the particles' kinetic energy increases.
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Thermal energy can be transferred between objects in three ways: conduction, convection, and radiation. Conduction occurs when particles in materials collide with neighboring particles. Convection is the transfer of thermal energy by the movement of molecules within a material. Radiation occurs through electromagnetic waves and can transfer energy through empty space. Some materials are better conductors or insulators of thermal energy depending on their composition and molecular structure. The transfer of excess warm water into bodies of water can cause thermal pollution, raising the temperature and reducing oxygen levels, harming aquatic life. Cooling towers can help reduce thermal pollution by lowering the temperature of warm water before release.
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- The first law of thermodynamics concerns the conservation of energy as work and heat are applied to a system. The second law concerns entropy.
- Systems must be in thermal, mechanical, and chemical equilibrium for their properties to be well-defined and for reversible processes to occur. Temperature is a measure of thermal equilibrium.
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The document provides an overview of thermodynamics from both macroscopic and microscopic perspectives. It discusses the basic concepts, laws, and principles of thermodynamics including:
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Thermodynamics deals with the relationships between heat and other forms of energy in a system. A system is a quantity of matter that has defined boundaries that distinguish it from its surroundings. Thermodynamic properties can be extensive, meaning they depend on the amount of matter in the system, or intensive, meaning they do not depend on amount. The thermodynamic state of a system is defined by its macroscopic properties like temperature, pressure, and volume. State functions depend only on the initial and final states, while path functions depend on the process between states. Thermodynamic equilibrium occurs when a system's properties no longer change over time during interactions with its surroundings.
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This document provides an introduction to thermodynamics concepts. It defines thermodynamics as the branch of science dealing with energy, energy transformations, and properties of matter. It discusses microscopic and macroscopic approaches, distinguishing between analyzing individual particle behavior and averaged bulk properties. Key concepts defined include systems, surroundings, boundaries, states, paths, processes, cycles, equilibrium, intensive/extensive properties, and the various forms of energy including work, heat, and power. The document lays out the foundation for further exploring thermodynamic principles.
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Thermodynamics deals with energy and its transformation between different forms. The first law of thermodynamics states that energy cannot be created or destroyed, only transformed from one form to another. A thermodynamic system exchanges energy in the form of heat or work with its surroundings. Closed systems exchange only energy, while open systems can exchange both energy and matter. Thermodynamic properties like pressure, temperature, and volume are used to describe different thermodynamic processes that occur at either constant values (isobaric, isochoric, isothermal) or with varying values.
Thermodynamics.PPT
Thermodynamics deals with concepts of heat, temperature, and energy conversion. Thermal equilibrium occurs between substances when there is no further heat transfer between them. Internal energy is the total energy of all atoms and molecules in a substance due to their random motion. Thermodynamic systems are classified as open, closed, or isolated based on heat and matter transfer ability. The first law of thermodynamics relates heat and work through a mathematical equation. Entropy is a measure of disorder or randomness that increases for energy received by a system and decreases for energy given out. The second law of thermodynamics prohibits heat from spontaneously flowing from cold to hot without work.
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Lec 02 15042013
- 1. LECTURE NO: 02 (15th April, 2013) Engr.Abdur Rafai abdurrafai29@gmail.com 0333-8171950 Jan 14, 2016 1
- 2. Introduction Thermodynamics is derived from two words: ‘Thermo’ which means ‘Heat energy’ and ‘Dynamics’ which means ‘conversion’ or ‘transformation’ Concisely, thermodynamics is a division of science that deals with conversion of energy from one form to another Jan 14, 2016 2
- 3. Definitions Thermodynamics is the science of the relationship between heat, work, and systems that analyze energy processes. Conservation of energy principle. It simply states that during an interaction, energy can change from one form to another but the total amount of energy remains constant. That is, energy cannot be created or destroyed. Jan 14, 2016 3
- 4. Definitions Temperature is indicator of direction for heat flow. It doesn't refer to the internal thermal energy of a system. Temperature describes the tendency of an object to give up energy to it's surroundings. Heat is defined as the form of energy that is transferred between two systems by virtue of a temperature difference. Jan 14, 2016 4
- 5. Definitions The change in the energy content of a body or any other system is equal to the difference between the energy input and the energy output, and the energy balance is expressed as Ein - Eout = E. Macroscopic approach to the study of thermodynamics that does not require a knowledge of the behavior of individual particles is called classical thermodynamics. Average behavior of large groups of individual particles, is called statistical thermodynamics. Jan 14, 2016 5
- 6. Applications Of Thermodynamics I.C Engines Power Plants Heat Transfer Refrigeration Energy Efficient Buildings Jan 14, 2016 6
- 7. Systems and Control Volume A system is defined as a quantity of matter or a region in space chosen for study. . The mass or region outside the system is called the surroundings. The real or imaginary surface that separates the system from its surroundings is called the boundary. The boundary of a system can be fixed or movable. A boundary is a closed surface surrounding a system through which energy and mass may enter or leave the system. Jan 14, 2016 7
- 8. Systems and Control Volume A closed system (also known as a control mass) consists of a fixed amount of mass, and no mass can cross its boundary. But it permits transfer of energy in the form of heat or work across the boundary. If neither mass or energy allowed to cross the boundary, that system is called an isolated system. An isolated system is one with rigid walls that has no communication (i.e., no heat, mass, or work transfer) with its surroundings. Jan 14, 2016 8
- 9. Systems and Control Volume A Open system (also known as a control volume) is one in which both mass and energy cross the boundary. Jan 14, 2016 9
- 10. PROPERTIES OF A SYSTEM Any characteristic of a system is called a property. Intensive properties are those that are independent of the mass of a system. Extensive properties are those whose values depend on the size or extent of the system such as proportional to mass of system. Extensive properties per unit mass are called specific properties. A continuous, homogeneous matter with no holes, that is, a continuum. Jan 14, 2016 10
- 11. Density and specific gravity Density is defined as mass per unit volume. The reciprocal of density is the specific volume v, which is defined as volume per unit mass. Specific gravity or relative density is ratio of the density of a substance to the density of some standard substance at a specified temperature. The weight of a unit volume of a substance is called specific weight. Jan 14, 2016 11
- 12. State and Equilibrium Each unique condition of system is called state. In an equilibrium state there are no unbalanced potentials (or driving forces) within the system. The system will be in thermal equilibrium if its temperature is same throughout the system. Jan 14, 2016 12
- 13. Figure1: A closed system reaching thermal equilibrium Jan 14, 2016 13
- 14. State and Equilibrium Mechanical equilibrium is related to pressure, and a system is in mechanical equilibrium if there is no change in pressure at any point of the system with time. If a system involves two phases, it is in phase equilibrium when the mass of each phase reaches an equilibrium level and stays there. Jan 14, 2016 14
- 15. State and Equilibrium A system is in chemical equilibrium if its chemical composition does not change with time, Jan 14, 2016 15