This document presents a new two-parameter model for predicting the thermal conductivity of liquids. The model is derived based on theories of molecular dynamics, liquid free volume, and the authors' previous model for estimating heat of vaporization. Thermal conductivity data for 68 liquids over a wide range of temperatures are fitted using the model and compared to other existing models, showing good agreement. Key parameters A and B are determined for different liquids to allow calculation of thermal conductivity based on fundamental physical property data.
This document provides an overview of Chapter 6 from a general chemistry textbook. The chapter covers the key topics of gases, including gas laws, kinetic molecular theory, gas properties and behavior, gas mixtures, and real gases. It includes definitions of terms like pressure, the gas laws of Boyle, Charles, Avogadro, Dalton's law of partial pressures, effusion and diffusion. Equations like the ideal gas law, van der Waals equation and Graham's law are presented. Examples are provided to demonstrate applications of concepts to stoichiometry and determining molar mass.
This document discusses chemical kinetics and reaction rates. It explains that kinetics studies how fast chemical reactions occur. The rate of a reaction depends on factors like the concentrations of reactants, temperature, and presence of catalysts. Reaction rates can be determined by measuring changes in concentration over time. The order of a reaction indicates how the rate depends on reactant concentrations. First-order and second-order reactions follow distinct rate laws that allow calculation of rate constants from experimental data. Reaction mechanisms involve elementary steps that may be fast or slow, with the overall rate determined by the slowest step.
1. A liter of gasoline contains 8000 calories of energy. A person uses an average of 2000 calories per day. Excess calories are stored as fat.
2. Calorimetry is used to determine the energy content of substances by measuring heat changes. Specific heat and heat capacity allow calculation of heat from temperature changes.
3. Enthalpy (H) quantifies heat flow during chemical reactions. Standard enthalpies of formation provide a reference scale for enthalpy values.
Thermochemistry deals with the heat involved in chemical and physical changes. It is a branch of thermodynamics that studies energy and its transformations. Enthalpy (H) is a measure of the total energy of a system at constant pressure and can be used to determine the heat of a reaction. Calorimetry experiments allow measurement of heat changes through determination of temperature changes of a system and surroundings using equations such as q = cmΔT. Bomb calorimetry and coffee cup calorimetry are two common techniques used to directly measure the heat of chemical reactions.
The document discusses chemical equilibrium, including:
- When equilibrium is reached, concentrations of reactants and products remain constant, with the forward and reverse reaction rates being equal.
- Le Chatelier's principle states that applying stress (changing temperature, concentration, volume, or pressure) causes a system at equilibrium to shift in a way that reduces the stress.
- For example, increasing temperature shifts exothermic reactions toward reactants and endothermic reactions toward products.
This document summarizes key concepts in thermochemistry, including:
1) Energy can be transferred as heat or work. The SI unit of energy is the joule. Internal energy is the sum of kinetic and potential energies within a system.
2) Enthalpy is a measure of the total energy of a system at constant pressure. It can be used to determine whether chemical reactions are endothermic or exothermic.
3) Calorimetry allows the measurement of heat and enthalpy changes through experiments on chemical reactions. Hess's law states that the enthalpy change of an overall reaction is the sum of enthalpy changes for individual steps.
The document discusses various thermodynamic concepts including:
1) Reversible and irreversible processes, with reversible processes proceeding in both directions and irreversible only proceeding in one direction.
2) Extensive and intensive properties, with extensive depending on amount and intensive independent of amount.
3) Types of processes like isothermal, isobaric, isochoric, cyclic, and adiabatic classified based on constant temperature, pressure, volume, state functions, and no heat transfer.
4) First law of thermodynamics stating energy is conserved and can be converted between forms.
5) Free energy and how it relates to available work for a system.
This document provides an overview of Chapter 6 from a general chemistry textbook. The chapter covers the key topics of gases, including gas laws, kinetic molecular theory, gas properties and behavior, gas mixtures, and real gases. It includes definitions of terms like pressure, the gas laws of Boyle, Charles, Avogadro, Dalton's law of partial pressures, effusion and diffusion. Equations like the ideal gas law, van der Waals equation and Graham's law are presented. Examples are provided to demonstrate applications of concepts to stoichiometry and determining molar mass.
This document discusses chemical kinetics and reaction rates. It explains that kinetics studies how fast chemical reactions occur. The rate of a reaction depends on factors like the concentrations of reactants, temperature, and presence of catalysts. Reaction rates can be determined by measuring changes in concentration over time. The order of a reaction indicates how the rate depends on reactant concentrations. First-order and second-order reactions follow distinct rate laws that allow calculation of rate constants from experimental data. Reaction mechanisms involve elementary steps that may be fast or slow, with the overall rate determined by the slowest step.
1. A liter of gasoline contains 8000 calories of energy. A person uses an average of 2000 calories per day. Excess calories are stored as fat.
2. Calorimetry is used to determine the energy content of substances by measuring heat changes. Specific heat and heat capacity allow calculation of heat from temperature changes.
3. Enthalpy (H) quantifies heat flow during chemical reactions. Standard enthalpies of formation provide a reference scale for enthalpy values.
Thermochemistry deals with the heat involved in chemical and physical changes. It is a branch of thermodynamics that studies energy and its transformations. Enthalpy (H) is a measure of the total energy of a system at constant pressure and can be used to determine the heat of a reaction. Calorimetry experiments allow measurement of heat changes through determination of temperature changes of a system and surroundings using equations such as q = cmΔT. Bomb calorimetry and coffee cup calorimetry are two common techniques used to directly measure the heat of chemical reactions.
The document discusses chemical equilibrium, including:
- When equilibrium is reached, concentrations of reactants and products remain constant, with the forward and reverse reaction rates being equal.
- Le Chatelier's principle states that applying stress (changing temperature, concentration, volume, or pressure) causes a system at equilibrium to shift in a way that reduces the stress.
- For example, increasing temperature shifts exothermic reactions toward reactants and endothermic reactions toward products.
This document summarizes key concepts in thermochemistry, including:
1) Energy can be transferred as heat or work. The SI unit of energy is the joule. Internal energy is the sum of kinetic and potential energies within a system.
2) Enthalpy is a measure of the total energy of a system at constant pressure. It can be used to determine whether chemical reactions are endothermic or exothermic.
3) Calorimetry allows the measurement of heat and enthalpy changes through experiments on chemical reactions. Hess's law states that the enthalpy change of an overall reaction is the sum of enthalpy changes for individual steps.
The document discusses various thermodynamic concepts including:
1) Reversible and irreversible processes, with reversible processes proceeding in both directions and irreversible only proceeding in one direction.
2) Extensive and intensive properties, with extensive depending on amount and intensive independent of amount.
3) Types of processes like isothermal, isobaric, isochoric, cyclic, and adiabatic classified based on constant temperature, pressure, volume, state functions, and no heat transfer.
4) First law of thermodynamics stating energy is conserved and can be converted between forms.
5) Free energy and how it relates to available work for a system.
Combustion reactions involve the release or absorption of energy as heat during chemical reactions where products form from reactants. A combustion reaction between fuel and oxygen releases heat. Stoichiometric coefficients in chemical equations represent equal amounts of each chemical element on both sides of the equation. The air-fuel ratio refers to the ratio of air to fuel, either by mass or moles. The theoretical air is the minimum amount of air needed for complete combustion of carbon, hydrogen, and sulfur in the fuel. Analysis of exhaust and flue gases can be done through wet analysis including steam or using an Orsat apparatus. Enthalpy of formation is the change in enthalpy when a compound forms from its elements in their standard states.
This chapter discusses thermochemistry and the concepts of heat, work, internal energy, enthalpy, and the first law of thermodynamics. It introduces terminology like system, surroundings, heat capacity, and heat of reaction. Methods for determining heats of reaction through calorimetry are presented, including bomb calorimetry and coffee cup calorimetry. The relationship between internal energy, enthalpy, and heat of reaction is explored. Standard states and standard enthalpy changes are defined. Hess's law for determining heats of reaction indirectly is introduced.
The fundamentals of chemical equilibrium including Le Chatier's Principle and solved problems for heterogeneous and homogeneous equilibrium.
**More good stuff available at:
www.wsautter.com
and
http://www.youtube.com/results?search_query=wnsautter&aq=f
This document discusses chemical equilibrium, including:
- Reactions reach equilibrium when concentrations of reactants and products remain constant over time.
- The equilibrium constant, K, quantifies the position of equilibrium and can be used to calculate concentrations at equilibrium.
- Equilibrium expressions can involve gas concentrations or pressures, and heterogeneous equilibria only include gases and dissolved substances in expressions.
- Knowing K allows prediction of whether a reaction will occur and the direction a system will shift to reach equilibrium.
The document discusses factors that affect the rate of chemical reactions, including concentration, temperature, surface area, and catalysts. It explains collision theory and activation energy. Exothermic reactions release heat while endothermic reactions absorb heat. Le Chatelier's principle states that chemical equilibriums shift to counteract changes in concentration, temperature, pressure or addition of reactants/products.
This document presents a new correlation for predicting the thermal conductivity of liquids based on their molar polarization. The correlation relates two parameters (A and b) from an existing thermal conductivity equation to molar polarization. Molar polarization takes into account molecular structure, polarity, and temperature effects. Experimental thermal conductivity data for various substances was used to develop a correlation between the parameters and molar polarization. The new correlation was found to predict thermal conductivity with average errors less than 5% for most substances tested, outperforming some existing methods.
The document presents a new two-constant equation of state that modifies the attractive pressure term of the van der Waals equation. Examples show the new equation provides improved predictions of liquid densities and phase behavior for single- and multi-component systems compared to the Soave-Redlich-Kwong equation. The development outlines determining parameters from critical properties and vapor pressure data, and using mixing and interaction rules to extend the equation to mixtures. Comparisons demonstrate the new equation performs as well or better than the Soave-Redlich-Kwong equation in all cases tested, with its greatest advantage in predicting liquid phase densities.
Stoichiometry is the study of quantitative relationships between reactants and products in chemical reactions based on mole ratios from balanced equations. Key concepts include:
1) Balanced equations show mole, mass, and particle relationships between reactants and products
2) Limiting reactants determine the maximum amount of product that can be formed
3) Excess reactants remain after the limiting reactant is used up in the reaction
I Hope You all like it very much. I wish it is beneficial for all of you and you can get enough knowledge from it. Clear and appropriate objectives, in terms of what the audience ought to feel, think, and do as a result of seeing the presentation. Objectives are realistic – and may be intermediate parts of a wider plan.
Equilibrium is a state in which there are no observable changes over time in a chemical system. At equilibrium, the concentrations of reactants and products remain constant. An equilibrium constant (K) can be defined based on the concentrations or pressures of reactants and products at equilibrium. The value of K is independent of initial concentrations and depends only on temperature. A change in concentration, pressure, volume, or temperature will shift the equilibrium in the direction that counteracts the applied stress according to Le Chatelier's principle.
Here is a one page paper relating chemistry and gases:
Chemistry and gases are intimately related. Many of the most important discoveries and applications in chemistry involve gases. Historically, scientists like Robert Boyle, Jacques Charles, and Joseph Gay-Lussac made seminal discoveries about gas behavior through careful experimentation. Their gas laws laid the foundation for understanding the properties and interactions of gases.
One area where gases play a huge role is in industry and energy. The Haber process converts nitrogen gas and hydrogen gas into ammonia, a key component of fertilizers that have enabled the growth of the global population. Natural gas, composed primarily of methane, heats homes and fuels power plants around the world. Greenhouse gases like carbon dioxide
This document discusses the topic of chemical equilibrium. It provides an introduction to key concepts such as reversible reactions occurring at the same rate and the equilibrium constant. It also discusses factors that affect chemical equilibrium such as concentration, pressure, temperature and catalysts. Le Chatelier's principle is explained, which states that applying stress to a system at equilibrium causes it to counteract the change. Specific examples are provided to illustrate how changing concentration, pressure and temperature impacts the position of equilibrium.
This document discusses energy transfer and heat, defining key concepts like temperature, heat capacity, enthalpy, and calorimetry. It explains that enthalpy is a measure of the total energy of a system and can be used to calculate the energy change of chemical reactions using Hess's law by adding the enthalpy changes of individual steps. Calorimetry is used to experimentally measure enthalpy changes.
This document provides instructions for an experiment to determine the heat of neutralization (ΔH) for acid-base reactions using calorimetry. It discusses key concepts like enthalpy, Hess' Law, and heat capacity. The procedure involves first calibrating thermometers and determining the heat capacity of the calorimeter. Then neutralization reactions between acids and bases are carried out in the calorimeter, and the temperature change is used to calculate the heat of reaction (ΔH) based on the calorimeter's heat capacity.
The document discusses chemical equilibrium and reversible reactions. It defines chemical equilibrium as a state where the forward and reverse reactions are proceeding at the same rate, such that the concentrations of reactants and products remain constant. It describes characteristics of equilibrium such as it being dynamic, having equal forward and reverse reaction rates, and requiring a closed system. It also introduces Le Châtelier's principle, which states that disturbances to a system at equilibrium cause the equilibrium to shift in a direction that counteracts the applied stress.
This document provides an overview of key concepts in thermochemistry, including:
1) Kinetic and potential energy, and how temperature relates to the average kinetic energy of molecules. Heat is energy transferred between objects of different temperature.
2) The first law of thermodynamics states that the change in energy of a system equals the heat added plus work done. Enthalpy (H) accounts for heat and pressure-volume work.
3) Hess's law allows determining the enthalpy change of a reaction by summing the enthalpy changes of intermediate steps. Standard enthalpies of formation (ΔH°f) quantify energy released when compounds form from elements.
The document discusses chemical equilibrium. It defines equilibrium as a state where the rates of the forward and reverse reactions of a chemical process are equal, resulting in no net change in the concentrations or properties of the system. It provides examples of physical and chemical equilibrium processes. It describes key characteristics of equilibrium like dynamic nature, constant concentrations and temperatures, and the relationship between reaction rates and equilibrium constants.
Современный мир ускоряется, и от тестирования требуется быстрые и стабильные тесты. В этом мастер-классе предлагается уйти от UI автоматизации и перейти на уровень ниже "пирамиды тестирования", на уровень WEB API. Не обещаю теорию, но будет много практических кейсов. В качестве примера я возьму популярный веб сайт с открытым API и покажу как за относительно небольшое время можно создавать хорошие тесты! Причем тесты мы будем создавать совместно, и особых навыков программирования от участников здесь не потребуется, достаточно включить логику и желание освоить что-то новое.
El documento describe la importancia de tener productos de primeros auxilios disponibles para tratar cortes, heridas y lesiones oculares. Ofrece una variedad de soluciones lavaojos y productos para primeros auxilios que pueden colocarse en lugares visibles y de fácil acceso para tratar accidentes de manera rápida, segura e higiénica. Resalta la necesidad de tener estos productos siempre a mano para poder asistir a alguien de manera inmediata en caso de un accidente.
What have you learned from target audience feedbackcaityduggan
The document summarizes feedback received from various target audiences on a music video project. Focus groups provided feedback on portrayals of gender, themes, and locations. Older audiences advised against explicit content and felt a cover song was appealing. Flickr comments helped select photos for packaging. Polls on Twitter and Facebook guided advertising strategies and logo design. A final questionnaire evaluated the video's stars, narrative, editing, costumes, and ability to encourage music purchases. Minor changes were identified to better establish themes and the artist duo. Overall, the feedback helped strengthen audience appeals.
Erikson's theory of psychosocial development describes 8 stages from infancy to late adulthood. The adolescent stage from 12-18 years involves resolving identity vs. role confusion. Successfully developing an identity leads to fidelity while failure can result in fanaticism or repudiation. Erikson's theory is applied in classrooms by providing role models and activities for identity exploration. Outside class, adolescents work to understand their identity and role in life. The theory has limitations but provides a framework for understanding social and emotional development.
Combustion reactions involve the release or absorption of energy as heat during chemical reactions where products form from reactants. A combustion reaction between fuel and oxygen releases heat. Stoichiometric coefficients in chemical equations represent equal amounts of each chemical element on both sides of the equation. The air-fuel ratio refers to the ratio of air to fuel, either by mass or moles. The theoretical air is the minimum amount of air needed for complete combustion of carbon, hydrogen, and sulfur in the fuel. Analysis of exhaust and flue gases can be done through wet analysis including steam or using an Orsat apparatus. Enthalpy of formation is the change in enthalpy when a compound forms from its elements in their standard states.
This chapter discusses thermochemistry and the concepts of heat, work, internal energy, enthalpy, and the first law of thermodynamics. It introduces terminology like system, surroundings, heat capacity, and heat of reaction. Methods for determining heats of reaction through calorimetry are presented, including bomb calorimetry and coffee cup calorimetry. The relationship between internal energy, enthalpy, and heat of reaction is explored. Standard states and standard enthalpy changes are defined. Hess's law for determining heats of reaction indirectly is introduced.
The fundamentals of chemical equilibrium including Le Chatier's Principle and solved problems for heterogeneous and homogeneous equilibrium.
**More good stuff available at:
www.wsautter.com
and
http://www.youtube.com/results?search_query=wnsautter&aq=f
This document discusses chemical equilibrium, including:
- Reactions reach equilibrium when concentrations of reactants and products remain constant over time.
- The equilibrium constant, K, quantifies the position of equilibrium and can be used to calculate concentrations at equilibrium.
- Equilibrium expressions can involve gas concentrations or pressures, and heterogeneous equilibria only include gases and dissolved substances in expressions.
- Knowing K allows prediction of whether a reaction will occur and the direction a system will shift to reach equilibrium.
The document discusses factors that affect the rate of chemical reactions, including concentration, temperature, surface area, and catalysts. It explains collision theory and activation energy. Exothermic reactions release heat while endothermic reactions absorb heat. Le Chatelier's principle states that chemical equilibriums shift to counteract changes in concentration, temperature, pressure or addition of reactants/products.
This document presents a new correlation for predicting the thermal conductivity of liquids based on their molar polarization. The correlation relates two parameters (A and b) from an existing thermal conductivity equation to molar polarization. Molar polarization takes into account molecular structure, polarity, and temperature effects. Experimental thermal conductivity data for various substances was used to develop a correlation between the parameters and molar polarization. The new correlation was found to predict thermal conductivity with average errors less than 5% for most substances tested, outperforming some existing methods.
The document presents a new two-constant equation of state that modifies the attractive pressure term of the van der Waals equation. Examples show the new equation provides improved predictions of liquid densities and phase behavior for single- and multi-component systems compared to the Soave-Redlich-Kwong equation. The development outlines determining parameters from critical properties and vapor pressure data, and using mixing and interaction rules to extend the equation to mixtures. Comparisons demonstrate the new equation performs as well or better than the Soave-Redlich-Kwong equation in all cases tested, with its greatest advantage in predicting liquid phase densities.
Stoichiometry is the study of quantitative relationships between reactants and products in chemical reactions based on mole ratios from balanced equations. Key concepts include:
1) Balanced equations show mole, mass, and particle relationships between reactants and products
2) Limiting reactants determine the maximum amount of product that can be formed
3) Excess reactants remain after the limiting reactant is used up in the reaction
I Hope You all like it very much. I wish it is beneficial for all of you and you can get enough knowledge from it. Clear and appropriate objectives, in terms of what the audience ought to feel, think, and do as a result of seeing the presentation. Objectives are realistic – and may be intermediate parts of a wider plan.
Equilibrium is a state in which there are no observable changes over time in a chemical system. At equilibrium, the concentrations of reactants and products remain constant. An equilibrium constant (K) can be defined based on the concentrations or pressures of reactants and products at equilibrium. The value of K is independent of initial concentrations and depends only on temperature. A change in concentration, pressure, volume, or temperature will shift the equilibrium in the direction that counteracts the applied stress according to Le Chatelier's principle.
Here is a one page paper relating chemistry and gases:
Chemistry and gases are intimately related. Many of the most important discoveries and applications in chemistry involve gases. Historically, scientists like Robert Boyle, Jacques Charles, and Joseph Gay-Lussac made seminal discoveries about gas behavior through careful experimentation. Their gas laws laid the foundation for understanding the properties and interactions of gases.
One area where gases play a huge role is in industry and energy. The Haber process converts nitrogen gas and hydrogen gas into ammonia, a key component of fertilizers that have enabled the growth of the global population. Natural gas, composed primarily of methane, heats homes and fuels power plants around the world. Greenhouse gases like carbon dioxide
This document discusses the topic of chemical equilibrium. It provides an introduction to key concepts such as reversible reactions occurring at the same rate and the equilibrium constant. It also discusses factors that affect chemical equilibrium such as concentration, pressure, temperature and catalysts. Le Chatelier's principle is explained, which states that applying stress to a system at equilibrium causes it to counteract the change. Specific examples are provided to illustrate how changing concentration, pressure and temperature impacts the position of equilibrium.
This document discusses energy transfer and heat, defining key concepts like temperature, heat capacity, enthalpy, and calorimetry. It explains that enthalpy is a measure of the total energy of a system and can be used to calculate the energy change of chemical reactions using Hess's law by adding the enthalpy changes of individual steps. Calorimetry is used to experimentally measure enthalpy changes.
This document provides instructions for an experiment to determine the heat of neutralization (ΔH) for acid-base reactions using calorimetry. It discusses key concepts like enthalpy, Hess' Law, and heat capacity. The procedure involves first calibrating thermometers and determining the heat capacity of the calorimeter. Then neutralization reactions between acids and bases are carried out in the calorimeter, and the temperature change is used to calculate the heat of reaction (ΔH) based on the calorimeter's heat capacity.
The document discusses chemical equilibrium and reversible reactions. It defines chemical equilibrium as a state where the forward and reverse reactions are proceeding at the same rate, such that the concentrations of reactants and products remain constant. It describes characteristics of equilibrium such as it being dynamic, having equal forward and reverse reaction rates, and requiring a closed system. It also introduces Le Châtelier's principle, which states that disturbances to a system at equilibrium cause the equilibrium to shift in a direction that counteracts the applied stress.
This document provides an overview of key concepts in thermochemistry, including:
1) Kinetic and potential energy, and how temperature relates to the average kinetic energy of molecules. Heat is energy transferred between objects of different temperature.
2) The first law of thermodynamics states that the change in energy of a system equals the heat added plus work done. Enthalpy (H) accounts for heat and pressure-volume work.
3) Hess's law allows determining the enthalpy change of a reaction by summing the enthalpy changes of intermediate steps. Standard enthalpies of formation (ΔH°f) quantify energy released when compounds form from elements.
The document discusses chemical equilibrium. It defines equilibrium as a state where the rates of the forward and reverse reactions of a chemical process are equal, resulting in no net change in the concentrations or properties of the system. It provides examples of physical and chemical equilibrium processes. It describes key characteristics of equilibrium like dynamic nature, constant concentrations and temperatures, and the relationship between reaction rates and equilibrium constants.
Современный мир ускоряется, и от тестирования требуется быстрые и стабильные тесты. В этом мастер-классе предлагается уйти от UI автоматизации и перейти на уровень ниже "пирамиды тестирования", на уровень WEB API. Не обещаю теорию, но будет много практических кейсов. В качестве примера я возьму популярный веб сайт с открытым API и покажу как за относительно небольшое время можно создавать хорошие тесты! Причем тесты мы будем создавать совместно, и особых навыков программирования от участников здесь не потребуется, достаточно включить логику и желание освоить что-то новое.
El documento describe la importancia de tener productos de primeros auxilios disponibles para tratar cortes, heridas y lesiones oculares. Ofrece una variedad de soluciones lavaojos y productos para primeros auxilios que pueden colocarse en lugares visibles y de fácil acceso para tratar accidentes de manera rápida, segura e higiénica. Resalta la necesidad de tener estos productos siempre a mano para poder asistir a alguien de manera inmediata en caso de un accidente.
What have you learned from target audience feedbackcaityduggan
The document summarizes feedback received from various target audiences on a music video project. Focus groups provided feedback on portrayals of gender, themes, and locations. Older audiences advised against explicit content and felt a cover song was appealing. Flickr comments helped select photos for packaging. Polls on Twitter and Facebook guided advertising strategies and logo design. A final questionnaire evaluated the video's stars, narrative, editing, costumes, and ability to encourage music purchases. Minor changes were identified to better establish themes and the artist duo. Overall, the feedback helped strengthen audience appeals.
Erikson's theory of psychosocial development describes 8 stages from infancy to late adulthood. The adolescent stage from 12-18 years involves resolving identity vs. role confusion. Successfully developing an identity leads to fidelity while failure can result in fanaticism or repudiation. Erikson's theory is applied in classrooms by providing role models and activities for identity exploration. Outside class, adolescents work to understand their identity and role in life. The theory has limitations but provides a framework for understanding social and emotional development.
This document discusses scientific concepts related to Sahajayoga and the brain/nervous system. It covers:
1) The central nervous system (CNS) which includes the brain and spinal cord, and the peripheral nervous system (PNS). The CNS interprets sensory signals and dictates motor responses while the PNS facilitates communication.
2) Differences in brain size across species from mice to humans, with the human cortex being about 1000 times larger than a mouse's.
3) The brain's electrical activity as measured by EEG, which records brain waves, versus MRI and fMRI which provide images of brain tissues and blood flow, respectively.
4) Types of brain waves detected by EEG
Aayush Gagneja has over 5 years of experience as a Systems Engineer and Senior Systems Engineer at Infosys working on contact center implementations. He has extensive experience with Genesys contact center software, including installations, upgrades, and providing level 2 and level 3 support. He is currently working as part of the support team for a US-based bank, focusing on inbound and outbound calls in a development environment. Aayush has a Bachelor's degree in Computer Engineering from Punjabi University and is proficient in Java, SQL, and various Microsoft and Linux tools.
Hadis, sunnah, khabar dan atsar secara harfiah berarti berita atau pesan. Secara istilah, mereka merujuk kepada ucapan, perbuatan, dan ketetapan Nabi Muhammad SAW, baik yang berasal langsung darinya maupun sahabat dan tabi'in-nya. Perbedaannya terletak pada ruang lingkup sumbernya, dengan hadis bersumber langsung dari Nabi SAW sedangkan yang lain bisa juga dari sumber lain. Mereka
Modeling and simulation of temperature profiles in a reactiveAlexander Decker
This document summarizes a study that developed a mathematical model to simulate temperature profiles in a reactive distillation system for the esterification of acetic anhydride and methanol. The model was based on reaction kinetics determined from experimental temperature data. Simulation results showed good agreement with experiments, with deviations less than 4%. An overview of the experimental setup and procedures for thermistor calibration and reactor calibration are also provided.
1 s2.0-s037838121100207 x-main.correlation of thermodynamic modeling and mole...Josemar Pereira da Silva
The document describes a method for correlating thermodynamic modeling and molecular simulations to predict liquid-liquid equilibrium in ternary polymer mixtures. The method uses a modified double lattice theory thermodynamic model combined with molecular simulations to determine interaction energy parameters. Dummy atoms are used to represent polymer segments in the simulations. The method is applied to four real ternary polymer systems, with the energy parameters directly used in the thermodynamic model. The results show good agreement with experimental observations using one or no adjustable parameters.
1 s2.0-s037838121100207 x-main.correlation of thermodynamic modeling and mole...Josemar Pereira da Silva
The document describes a method for correlating thermodynamic modeling and molecular simulations to predict liquid-liquid equilibrium in ternary polymer mixtures. The method uses a modified double lattice theory thermodynamic model combined with molecular simulations to determine interaction energy parameters. Dummy atoms are used to represent polymer segments in the simulations. The method is applied to four real ternary polymer systems, with the energy parameters directly used in the thermodynamic model. The results show good agreement with experimental observations using one or no adjustable parameters.
Heat Transfer Enhancement Using Aluminium Oxide Nanofluid: Effect of the Base...CSCJournals
The flow and heat transfer is an important phenomenon in engineering systems due to its wide application in electronic cooling, heat exchangers, double pane windows etc.. The enhancement of heat transfer in these systems is an essential topic from an energy saving perspective. The lower heat transfer performance when conventional fluids, such as water, engine oil and ethylene glycol are used hinders improvements in performance and a consequent reduction in the size of such systems. The use of solid particles as an additive suspended into the base fluid is a technique for heat transfer enhancement. Therefore, the heat transfer enhancement in a horizontal circular tube that is maintained at a constant temperature under laminar regime has been investigated numerically. A computational code applied to the problem by use of the finite volume method was developed. Nanofluid was made by dispersion of Al2O3 nanoparticles in pur water and ethylene glycol. Results illustrate that the suspended nanoparticles increase the heat transfer with an increase in the nanoparticles volume fraction and for a considered range of Reynolds numbers. And in other hand, the heat transfer is very sensitive to the base fluid.
Photovoltaic (PV) cell from solar energy is one of the most widely adopted renewable energy source and commercially available system that can be used in various applications. More appealing application of PV arrays used in thermoelectric (TE) device was it can convert solar thermal energy from temperature difference into electric energy to act as power generators. In this study, a theoretical model is developed by using conducting steady state energy analysis of a PVT-TE air collector. The matrix inversion method is used to obtain energy balance equation. The effect of various parameters also investigated. The mass flow rate of range 0.01 kg/s to 0.05 kg/s and solar intensity of 400 W/m2, 600 W/m2 and 800 W/m2 was used to obtain outlet temperature, To in the range about 28.9oC to 43.7oC and PV temperature, Tp about 35.3oC to 60oC.
heat capacity of sitric acid0c96051e8eb63eea58000000Tika Ningsih
This document summarizes thermodynamic properties of the citric acid-water binary system determined through various experimental methods. Key findings include:
- The phase diagram exhibits eutectic and peritectic behavior with solid-liquid and vapor-liquid equilibria measured.
- Enthalpies of formation for citric acid monohydrate, solution, transition, and vaporization were determined via calorimetry and vapor pressure measurements.
- Specific heat capacity and solubility data were also collected to characterize the phase behavior and thermodynamic functions of citric acid and its monohydrate over a range of temperatures.
This document provides information about an advanced chemical engineering thermodynamics course, including:
1) The course covers basic definitions, concepts, relationships for pure components and mixtures including pvT relationships and thermodynamic property relationships.
2) Relevant textbooks are listed for reference.
3) Methods for determining pvT properties of pure components and mixtures are discussed, including experimental determination, databases, equations of state, and process simulators.
4) The Lydersen and Pitzer methods for corresponding states are summarized, which use critical compressibility factor and acentric factor respectively as third parameters to determine compressibility factor from reduced temperature and pressure.
The Effects of Nanofluids on Forced Convection Heat Transfer Inside Parallel ...AI Publications
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2. 188 F.A. Wang et al. / Chemical Engineering Journal 78 (2000) 187–191
ln λ = −ln(abe) − n ln Vf +
dEc
RT
(5)
Assuming that Eq. (5) is applicable to the vapor phase
of a vapor–liquid equilibrium, and the vapor phase is dilute
gases, then EV
c → 0, V V
f → V [23]. Thus,
ln λV
= −ln(abe) − n ln V (6)
By subtracting Eq. (6) from Eq. (5), the following is ob-
tained:
ln
λ
λV
= −n ln
Vf
V
+
dEc
RT
(7)
According to the theory of chemical engineering ther-
modynamics, chemical potentials are equal at vapor–liquid
equilibrium and can be expressed by configuring partition
function Q as follows [23]:
∂ ln QL
∂N T,V
=
∂ ln QV
∂N T,V
(8)
and
QL
= V N
f exp −
Ec
RT
(9)
QV
=
V N
N!
(10)
Eqs. (9) and (10) are substituted into Eq. (8) and the Stir-
ling approximation is adopted, with Vf=Nvf and Ec=N2f(V,
T) [24]; the following relation is obtained:
ln
Vf
V
=
2Ec
nkT
(11)
Substituting Eq. (11) into Eq. (7), we get
ln
λ
λV
=
BEc
RT
(12)
The liquid lattice energy Ec is approximately equal to the
vaporization energy UV [24] and the latter is related to the
vaporization heat LV as follows [1]:
Ec ≈ UV = LV − RT (13)
According to the theory of molecular dynamics [1,2,4],
the thermal conductivity of dilute gases is [11]
λV
=
C(T/M)1/2
V
2/3
c V
(14)
where the collision integration V is expressed by the
Neufeld–Janzen–Aziz equation [25] as follows:
V = 0.52487 exp(−0.97369Tr) + 2.16178
× exp(−3.07001Tr) + 1.1223T −0.14874
r (15)
By taking the natural logarithm in Eq. (14) and defining
q ≡ VV
2/3
c
T
M
−1/2
(16)
the following is obtained:
ln λV
= ln C − ln q (17)
Introducing Eqs. (13) and (17) into Eq. (12) and arranging
it, we get
ln(λq) = A +
BLV
RT
(18)
We [26,27] have proposed the new equation to estimate
the heat of vaporization for pure liquids based on the statis-
tical thermodynamics theory as follows:
LV =
RTcSW
Pc
Pc ln Pc
θ − 1
− C0
− ωC (19)
where
S = (10 + 3Tr − 2T 2
r )
θ2
10θ2 + 3θ − 2
W =
θ − (T/Tb)
θ − 1
0.38
C0
= 1.097θ1.6
− 0.083
C = 0.8944θ4.2
− 0.139
θ =
Tc
Tb
Tr =
T
Tc
The acentric factor in Eq. (19) is calculated by the
Lee–Kesler equation [28].
Combining Eqs. (18) and (19), the new equation to cal-
culate the thermal conductivity of pure liquids is obtained
as follows:
ln(λq) = A + B
SWT−0.5
r
Pc
Pc ln Pc
θ − 1
− C0
− ωC (20)
3. Results and discussion
By use of the least squares method, the two characteristic
parameters A and B of a liquid in Eq. (20) can be determined
from experimental data over the investigated temperature
range. The values of A and B for some liquids are given in
Table 1.
With the parameters A and B, we can use the most fun-
damental physical property data comprising Tb, Tc, Pc and
Vc to calculate the thermal conductivity of some substances
at any temperature according to Eq. (20). The thermal con-
ductivity of 68 pure liquids including paraffins, olefins,
alkynes, cycloparaffins, aromatics, alcohols, phenol, ethers,
aldehydes, ketones, esters, organic acids, organic halides,
organic nitrogen compounds and inorganic compounds were
calculated from Eq. (20) over wide ranges of temperature,
4. 190 F.A. Wang et al. / Chemical Engineering Journal 78 (2000) 187–191
Table 1 (Continued)
Liquids Temperature
range, Tr
No. of
points
A B×10 ARD (%) Refs.
New model Jamieson Riedel Klaas et al. Lei et al.
Sulfur dioxide 0.46425–0.92851 15 2.2273 1.8890 0.22 1.85 1.56 3.16 2.82 [16,17,36]
Hydrogen fluoride 0.63470–1.0000 9 1.7282 1.9170 1.23 3.79 1.62 3.62 3.29 [17]
Hydrogen chloride 0.53342–0.93962 10 2.001 2.5376 2.30 4.09 4.34 4.19 4.17 [17]
Hydrogen sulfide 0.57028–0.91116 9 1.0464 3.3193 2.07 3.94 2.67 5.52 4.92 [17]
Ammonia 0.59117–0.96166 38 1.9562 2.2783 1.40 3.86 1.95 3.59 2.69 [16,17,34]
Dowtherm J 0.34009–0.94491 9 3.4327 0.8740 1.17 1.54 0.33 0.25 0.55 [17]
Mercury 0.3574–0.59550 10 1.9630 1.3871 0.53 0.30 0.80 0.43 0.45 [17]
Water (0.1 MPa) 0.42198–0.57647 44 3.3653 0.4102 0.68 0.54 0.79 0.66 0.70 [29,33,35]
Water (5 MPa) 0.42198–0.57647 11 2.5115 0.4940 0.84 0.67 0.97 0.82 0.76 [33]
Water (20 MPa) 0.42198–0.57647 11 2.5063 0.5147 0.84 0.68 0.99 0.82 0.76 [33]
Total 68 1217 1.70 3.43 2.04 5.21 4.09
even up to the critical temperature. The results are shown in
Table 1. The reference data of thermal conductivity come
from Vargaftik [16], Beaton [17], Jamieson [29], Lei et al.
[12], Rohsenow [30], Digullio et al. [31] and Cai and others
[32–36]. Table 1 also shows the comparison between the
new model and other good models, such as the Jamieson
equation [4–6], the modified Reidel equation [7] and the
recent models proposed by Klaas et al. [10] and Lei et al.
[11]. Comparing the calculated data and reference data of
68 pure liquids at 1217 temperature points, the overall aver-
age relative deviations of five models are, respectively, 1.70,
3.43, 2.04, 5.21, and 4.09%. The overall average relative
deviation is calculated as follows:
ARD =
100
Np
|λp − λe|
λe
(21)
Obviously, the new model is the best over the investigated
temperature as well as substance range, and the modified
Reidel equation takes the second place. The Jamieson equa-
tion is applicable to common liquids, but has notable errors
when applied to lower paraffin hydrocarbons, some refrig-
erants, liquefied inert gas, diatomic gas and inorganic gas,
especially when temperatures are close to the critical tem-
perature. The model proposed by Klaas et al. can give good
results when the temperature range is very limited. How-
ever, the calculated error rises sharply when the temperature
range is extended, especially up to the critical temperature.
Klaas et al., however, pointed out [10] that their model gives
good results for the temperature range between the normal
melting point and the normal boiling point of a substance.
The method of Lei et al. has the same limitation as the model
by Klaas et al.
4. Conclusions
Using our previous estimation equation of the heat of
vaporization for liquids with the residual function method,
and with the liquid free volume model as well as the the-
ory of molecular dynamics, a new two-parameter model of
thermal conductivity for liquids has been derived. With this
new model, the thermal conductivity data for 68 kinds of
liquids at 1217 temperature sets were tested. The results are
compared with the recent models proposed by Lei et al.,
Klaas et al., and with the Jamieson equation and the mod-
ified Riedel equation. The comparison shows that the new
model, which has a theoretical basis, is applicable to paraf-
fins, olefins, alkynes, cycloparaffins, aromatics, alcohols,
phenol, ethers, aldehydes, ketones, esters, organic acids,
organic halides, organic nitrogen compounds, refrigerants,
liquefied inert gas, inorganic compounds, and so on. The
new model can give good results over a wide temperature
range, even up to the critical temperature.
5. Nomenclature
a, b, d, e constants
A, B, C characteristic parameters of pure liquids
Ea activation energy
Ec lattice energy
k Boltzmann constant
Lv heat of vaporization
M molecular weight
n model parameter
N molecular number
Np testing data sets
P pressure
PE, PV probability
Q configuration partition function
R gas constant
T temperature
UV vaporization energy
V volume
vf monomolecular free volume
Vf mole free volume
Greek symbols
λ thermal conductivity
V collision integral
ω acentric factor
5. F.A. Wang et al. / Chemical Engineering Journal 78 (2000) 187–191 191
Superscripts
L saturated liquid phase
V saturated vapor phase
Subscripts
b normal boiling point
c critical point
e experimental data
P calculated data
r reduced property
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