This document contains a summary of a course on the design of natural gas measurement and regulation bridges. It discusses the properties and characteristics of natural gas, including its composition, physical properties, thermodynamic properties, and quality standards. It also covers topics like the value chain of natural gas, processing methods like sweetening, dehydration, and liquefaction. Finally, it discusses Supreme Decree 1996 which establishes the regulations for natural gas distribution networks in Peru. The document contains detailed information on modeling and calculating the key parameters of natural gas.
This document outlines various laws and equations relating to gas mixtures, including:
1) Dalton's Law which states that the total pressure of a gas mixture is equal to the sum of the partial pressures of the individual components.
2) Amagat's Law which describes how the total volume of a gas mixture is equal to the sum of the volumes the components would occupy individually at the same temperature and pressure.
3) Equations for determining the molecular weight, gas constant, and specific heat of a gas mixture based on the properties of its individual components.
Dasar Keteknikan (Dastek) Pengolahan Pangan FTP UB 150529064527-lva1-app6891Muhammad Luthfan
The document discusses food process engineering which includes converting raw materials into ready or processed foods through various unit operations like heat transfer, drying, evaporation, and mechanical separations. It explains that food processes can be broken down into a small number of basic unit operations and outlines the aims of the food industry as extending shelf life, increasing variety, providing nutrients, and generating income. Food processes are usually represented through flow charts that show the flow of materials and energy.
This document provides additional notes and solutions for Thermodynamics by Enrico Fermi. It includes:
1) Clarifications and derivations of concepts from the textbook such as constraints on motion in the p-V plane, equivalence of work formulations, and change in heat in terms of variables T and p.
2) Worked examples such as adiabatic transformations of an ideal gas and comparison of isothermal and adiabatic transformations.
3) An example application to adiabatic expansion in the atmosphere.
4) Postulates regarding reversible thermodynamic engines.
This document compares different methods for predicting the density of liquid refrigerants, including correlations by ISH, Rackett, Yamada & Gunn, Spencer & Danner, Hankinson & Thomson, Reidel, and NM. It finds that the NM correlation best predicts densities for R22, R32, R134a, R152a, R600, and R12, while the Hankinson & Thomson method works best for R290, R600a, and R1270. The Reidel correlation accurately models R143a and R125, and the Yamada & Gunn and Spencer & Danner modifications are suitable for R123 and R718, respectively. Overall, the document evaluates methods for various refriger
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 summarizes key concepts in advanced thermodynamics including:
- Pressure-temperature and pressure-volume diagrams for pure fluids and the phase change curves and points they depict.
- Equations of state relating pressure, volume, and temperature for homogeneous fluids in equilibrium.
- Properties and examples of ideal gas behavior and the virial equation of state for real gases.
- Calculation of work, heat, internal energy, and enthalpy changes for various thermodynamic processes involving ideal gases including isothermal, adiabatic, constant pressure, and throttling processes.
This document discusses thermodynamic properties of fluids, including:
1) Derivations of equations relating the primary thermodynamic properties of pressure, volume, temperature, internal energy, and entropy for homogeneous phases and fluids.
2) Calculations of changes in enthalpy, entropy, and internal energy based on changes in pressure and temperature.
3) The thermodynamic properties of Gibbs energy and residual properties.
4) An example problem calculating the enthalpy and entropy of saturated isobutane vapor at a specified temperature and pressure using compressibility factor and ideal gas heat capacity data.
This document contains the work of Steven Brandon in answering 6 calculation questions regarding the flow properties of a non-Newtonian fluid flowing through a pipe. Brandon calculates the velocity profile, volumetric flow rate, average velocity, Reynolds number, friction factor, and viscosity at 5°C. He determines that the flow is laminar based on the Reynolds number. The velocity profile is flattened compared to Newtonian flow. The volumetric flow rate is 1.71 L/s. The average velocity is 1.78 m/s. The Reynolds number is 288.6. The friction factor is 0.222. The viscosity at 5°C is calculated to be 1100 mPa·s.
This document outlines various laws and equations relating to gas mixtures, including:
1) Dalton's Law which states that the total pressure of a gas mixture is equal to the sum of the partial pressures of the individual components.
2) Amagat's Law which describes how the total volume of a gas mixture is equal to the sum of the volumes the components would occupy individually at the same temperature and pressure.
3) Equations for determining the molecular weight, gas constant, and specific heat of a gas mixture based on the properties of its individual components.
Dasar Keteknikan (Dastek) Pengolahan Pangan FTP UB 150529064527-lva1-app6891Muhammad Luthfan
The document discusses food process engineering which includes converting raw materials into ready or processed foods through various unit operations like heat transfer, drying, evaporation, and mechanical separations. It explains that food processes can be broken down into a small number of basic unit operations and outlines the aims of the food industry as extending shelf life, increasing variety, providing nutrients, and generating income. Food processes are usually represented through flow charts that show the flow of materials and energy.
This document provides additional notes and solutions for Thermodynamics by Enrico Fermi. It includes:
1) Clarifications and derivations of concepts from the textbook such as constraints on motion in the p-V plane, equivalence of work formulations, and change in heat in terms of variables T and p.
2) Worked examples such as adiabatic transformations of an ideal gas and comparison of isothermal and adiabatic transformations.
3) An example application to adiabatic expansion in the atmosphere.
4) Postulates regarding reversible thermodynamic engines.
This document compares different methods for predicting the density of liquid refrigerants, including correlations by ISH, Rackett, Yamada & Gunn, Spencer & Danner, Hankinson & Thomson, Reidel, and NM. It finds that the NM correlation best predicts densities for R22, R32, R134a, R152a, R600, and R12, while the Hankinson & Thomson method works best for R290, R600a, and R1270. The Reidel correlation accurately models R143a and R125, and the Yamada & Gunn and Spencer & Danner modifications are suitable for R123 and R718, respectively. Overall, the document evaluates methods for various refriger
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 summarizes key concepts in advanced thermodynamics including:
- Pressure-temperature and pressure-volume diagrams for pure fluids and the phase change curves and points they depict.
- Equations of state relating pressure, volume, and temperature for homogeneous fluids in equilibrium.
- Properties and examples of ideal gas behavior and the virial equation of state for real gases.
- Calculation of work, heat, internal energy, and enthalpy changes for various thermodynamic processes involving ideal gases including isothermal, adiabatic, constant pressure, and throttling processes.
This document discusses thermodynamic properties of fluids, including:
1) Derivations of equations relating the primary thermodynamic properties of pressure, volume, temperature, internal energy, and entropy for homogeneous phases and fluids.
2) Calculations of changes in enthalpy, entropy, and internal energy based on changes in pressure and temperature.
3) The thermodynamic properties of Gibbs energy and residual properties.
4) An example problem calculating the enthalpy and entropy of saturated isobutane vapor at a specified temperature and pressure using compressibility factor and ideal gas heat capacity data.
This document contains the work of Steven Brandon in answering 6 calculation questions regarding the flow properties of a non-Newtonian fluid flowing through a pipe. Brandon calculates the velocity profile, volumetric flow rate, average velocity, Reynolds number, friction factor, and viscosity at 5°C. He determines that the flow is laminar based on the Reynolds number. The velocity profile is flattened compared to Newtonian flow. The volumetric flow rate is 1.71 L/s. The average velocity is 1.78 m/s. The Reynolds number is 288.6. The friction factor is 0.222. The viscosity at 5°C is calculated to be 1100 mPa·s.
This document discusses determining the Reid Vapor Pressure (RVP) and deriving the True Vapor Pressure (TVP) of various hydrocarbons through experimentation. The experiment involves using an RVP apparatus to measure the vapor pressure of diesel, benzene, and gasoline at 37.8°C. The RVP values are then used to calculate the TVP through established equations and graphs. The results show the RVP is slightly lower than the TVP due to other volatile components not measured. Measuring vapor pressure is important for safety during storage and transportation of hydrocarbons as well as understanding the hydrocarbon composition.
The document discusses chemical kinetics and reaction rates. It begins by defining chemical kinetics as the study of the rate at which a chemical reaction occurs. It notes that kinetics provides information about both reaction speed and reaction mechanism. The document then discusses several factors that affect reaction rates, including physical state of reactants, concentration of reactants, temperature, and presence of a catalyst. It explains that reaction rates can be determined by monitoring changes in concentration over time. The document provides examples of calculating average and instantaneous reaction rates. It also discusses how reaction rates relate to stoichiometry and explains rate laws.
This document provides an overview of methods for calculating key gas properties including:
1. The z-factor, which can be calculated using correlations like Hall-Yarborough or Dranchuk-Abu-Kassem that were developed based on the Standing-Katz chart.
2. Isothermal gas compressibility (Cg), which can be determined from the z-factor or using models that relate it to reduced gas density.
3. Gas formation volume factor (Bg) and gas expansion factor (Eg), which relate the volume of gas at reservoir conditions to standard conditions.
4. Gas viscosity, which can be estimated using correlations like Carr-Kobayashi-Burrows that are functions of
The document discusses gases and their behavior. It covers Dalton's law of partial pressures, which states that the total pressure of a gas mixture is equal to the sum of the partial pressures of the individual gases. It also discusses Graham's law, which relates the rates of gas diffusion and effusion to the molar masses of the gases, with lower molar mass gases diffusing and effusing faster. Specific examples are provided to demonstrate applications of these laws to calculating partial pressures and effusion rate ratios.
This document discusses the gas laws of Boyle's law, Charles's law, Gay-Lussac's law, and the combined gas law. It provides explanations and examples of how each law describes the relationships between the pressure, volume, and temperature of a gas. Sample problems demonstrate how to use the gas laws to calculate unknown pressure, volume, or temperature values. The combined gas law incorporates all three variables and can be used to derive the other individual gas laws by holding one variable constant.
1. The document defines key concepts related to ideal gases including the ideal gas law, gas constant, Boyle's law, Charles' law, Avogadro's law, specific heat, ratio of specific heats, entropy change, gas mixtures, and processes involving gases.
2. It provides equations of state for ideal gases, gas mixtures, and non-ideal gases. Equations are given for properties of gas mixtures including volume, pressure, molecular weight, and specific heat.
3. Key thermodynamic processes involving gases are summarized including isobaric and isometric processes for both closed and open systems, with equations provided for heat, work, internal energy, and entropy changes.
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.
This document discusses drug stability calculations and kinetics. It defines drug stability as a drug remaining within established specifications over time. The purpose of stability studies is to determine a drug product's quality and shelf life under recommended storage conditions. Drug kinetics examines how drug concentration changes over time and helps predict stability and shelf life. The document explains how to calculate half-life and shelf life based on zero-order, first-order, and second-order rate reactions using rate equations and graphs. Examples are provided for each reaction order.
There are four main factors that affect the rates of chemical reactions: reactant concentration, temperature, catalysts, and surface area. The rate of a reaction is determined by measuring how the concentration of reactants or products changes over time. Reaction rates can be calculated based on either the disappearance of reactants or the appearance of products.
1. The document describes various thermodynamic processes including isobaric, isometric, isothermal, isentropic, and polytropic processes.
2. For isobaric processes in closed systems, work done is equal to pressure times change in volume. For open systems at constant pressure, work done is zero and heat absorbed is equal to enthalpy change.
3. For isentropic processes in closed systems, work done is equal to the negative change in internal energy, and for open systems work done is equal to the negative enthalpy change.
Thermodynamics (2013 new edition) copyYuri Melliza
Thermodynamics deals with energy transformation between different forms. Some key concepts covered in the document include:
- The first law of thermodynamics states that energy cannot be created or destroyed, only converted from one form to another.
- For a closed system, the heat transfer (Q) equals the change in internal energy (U) plus the work (W) done by the system.
- For an open system, the heat (Q) equals the change in enthalpy (H) of the system plus the sum of kinetic energy (KE), potential energy (PE), and work (W).
- Other concepts defined include systems, surroundings, properties of fluids, phases of substances, forms of energy
Mechanical engineer's manual(by. engr. yuri g. melliza)Yuri Melliza
1. This document defines common mechanical engineering terms such as mass, velocity, acceleration, force, pressure, and temperature scales. Conversion factors are provided.
2. Properties of fluids such as density, specific volume, specific gravity, and equations of state for gases are defined. Characteristics including viscosity, elasticity, and surface tension are also explained.
3. Ten sample problems are worked through as examples of applying the definitions and concepts to calculations involving forces, densities, pressures, temperatures, and manometers.
Kinetics is the study of reaction rates and mechanisms. There are four main factors that affect reaction rates: the nature of reactants, temperature, catalysts, and concentration. The rate of a reaction is measured based on how quickly the concentration of reactants decreases or products increases over time. As reactions proceed, the rate generally decreases as reactant concentrations decrease until the reaction reaches equilibrium or the reactants are used up.
1. Chemical kinetics deals with the rates of chemical reactions and factors that affect reaction rates. It examines how fast reactions occur and the mechanisms of reactions.
2. Reaction rates can vary significantly, from fractions of seconds to years. Third-order reactions involve three molecules and are also called termolecular reactions.
3. The rate of a reaction is affected by temperature - higher temperatures provide more energy and increase reaction rates by producing more effective collisions between reactant molecules.
The document discusses key concepts related to gas-vapor mixtures and air conditioning including:
- Dry and atmospheric air, specific and relative humidity.
- Dew-point, adiabatic saturation, and wet-bulb temperatures.
It provides examples and explanations of these terms. Several problems are also included and solved relating to determining properties of air-vapor mixtures under various conditions.
Chapter 4 (propertiesof pure substance)Yuri Melliza
This document discusses the properties of pure substances during phase changes. It defines key terms like saturation temperature, saturation pressure, sub-cooled liquid, saturated liquid, saturated vapor, and superheated vapor. The document explains that 100°C is the saturation temperature corresponding to a pressure of 101.325 kPa. It also provides diagrams to illustrate the different regions on a T-S and h-S chart during phase changes and defines concepts like quality.
This document describes an experimental study that measured ignition delay times for fuel-air mixtures behind reflected shock waves under conditions relevant to homogeneous charge compression ignition (HCCI) engines. Ignition delay times were measured for n-heptane, gasoline, and a gasoline surrogate mixture (iso-octane/toluene/n-heptane) over a range of pressures, temperatures, equivalence ratios, and exhaust gas recirculation levels using pressure history and chemiluminescence diagnostics in shock tubes. The results provide benchmark data for validating detailed chemical kinetic models under HCCI combustion conditions.
The first law of thermodynamics states that the change in internal energy of a system is equal to the heat supplied to the system minus the work done by the system. For a closed system undergoing a process, this can be expressed as ΔU=Q-W. The first law applies to both closed systems undergoing non-flow processes as well as open systems undergoing steady flow processes. For non-flow processes such as constant volume, constant pressure, isothermal, and adiabatic processes, the first law allows determining the relationships between heat, work and changes in internal energy or enthalpy. For steady flow processes, the general energy equation accounts for changes in kinetic and potential energy of the fluid in addition to heat
The document discusses thermodynamic property relations for ideal gases. It provides examples of calculating changes in pressure (dP) given changes in temperature (dT) or specific volume (dv) using the ideal gas law. The examples show that for air and helium, a 1% increase in both T and v results in no net change in pressure (dP=0). The document also examines using partial derivatives to determine slopes of lines on temperature-volume and temperature-pressure diagrams for ideal gases and the van der Waals equation of state.
This document describes a chemistry laboratory experiment to measure the density, specific gravity (SG), and API gravity of fluids. Two methods are used: a hydrometer method and a pycnometer method. The pycnometer method is found to be more accurate due to factors like temperature that can affect hydrometer readings. Calculations are shown to determine the SG and API gravity of a crude oil sample. The API gravity is found to be 47.84, indicating a paraffinic crude oil. Higher API gravity values correspond to crude oils that contain more gasoline and less sulfur.
This document discusses methods for determining the compressibility factor (Z) in gas mixtures. It defines different types of natural gas and describes using pseudocritical properties and reduced conditions to calculate Z based on corresponding states theory. The Standing-Katz method is commonly used to determine Z for sweet gases graphically using reduced pressure and temperature. This method can be modified to account for sour gases containing H2S and CO2 by adjusting the pseudocritical properties. An example calculation demonstrates determining the volume of a gas sample at different conditions using both the unmodified and modified Standing-Katz methods.
This document discusses determining the Reid Vapor Pressure (RVP) and deriving the True Vapor Pressure (TVP) of various hydrocarbons through experimentation. The experiment involves using an RVP apparatus to measure the vapor pressure of diesel, benzene, and gasoline at 37.8°C. The RVP values are then used to calculate the TVP through established equations and graphs. The results show the RVP is slightly lower than the TVP due to other volatile components not measured. Measuring vapor pressure is important for safety during storage and transportation of hydrocarbons as well as understanding the hydrocarbon composition.
The document discusses chemical kinetics and reaction rates. It begins by defining chemical kinetics as the study of the rate at which a chemical reaction occurs. It notes that kinetics provides information about both reaction speed and reaction mechanism. The document then discusses several factors that affect reaction rates, including physical state of reactants, concentration of reactants, temperature, and presence of a catalyst. It explains that reaction rates can be determined by monitoring changes in concentration over time. The document provides examples of calculating average and instantaneous reaction rates. It also discusses how reaction rates relate to stoichiometry and explains rate laws.
This document provides an overview of methods for calculating key gas properties including:
1. The z-factor, which can be calculated using correlations like Hall-Yarborough or Dranchuk-Abu-Kassem that were developed based on the Standing-Katz chart.
2. Isothermal gas compressibility (Cg), which can be determined from the z-factor or using models that relate it to reduced gas density.
3. Gas formation volume factor (Bg) and gas expansion factor (Eg), which relate the volume of gas at reservoir conditions to standard conditions.
4. Gas viscosity, which can be estimated using correlations like Carr-Kobayashi-Burrows that are functions of
The document discusses gases and their behavior. It covers Dalton's law of partial pressures, which states that the total pressure of a gas mixture is equal to the sum of the partial pressures of the individual gases. It also discusses Graham's law, which relates the rates of gas diffusion and effusion to the molar masses of the gases, with lower molar mass gases diffusing and effusing faster. Specific examples are provided to demonstrate applications of these laws to calculating partial pressures and effusion rate ratios.
This document discusses the gas laws of Boyle's law, Charles's law, Gay-Lussac's law, and the combined gas law. It provides explanations and examples of how each law describes the relationships between the pressure, volume, and temperature of a gas. Sample problems demonstrate how to use the gas laws to calculate unknown pressure, volume, or temperature values. The combined gas law incorporates all three variables and can be used to derive the other individual gas laws by holding one variable constant.
1. The document defines key concepts related to ideal gases including the ideal gas law, gas constant, Boyle's law, Charles' law, Avogadro's law, specific heat, ratio of specific heats, entropy change, gas mixtures, and processes involving gases.
2. It provides equations of state for ideal gases, gas mixtures, and non-ideal gases. Equations are given for properties of gas mixtures including volume, pressure, molecular weight, and specific heat.
3. Key thermodynamic processes involving gases are summarized including isobaric and isometric processes for both closed and open systems, with equations provided for heat, work, internal energy, and entropy changes.
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.
This document discusses drug stability calculations and kinetics. It defines drug stability as a drug remaining within established specifications over time. The purpose of stability studies is to determine a drug product's quality and shelf life under recommended storage conditions. Drug kinetics examines how drug concentration changes over time and helps predict stability and shelf life. The document explains how to calculate half-life and shelf life based on zero-order, first-order, and second-order rate reactions using rate equations and graphs. Examples are provided for each reaction order.
There are four main factors that affect the rates of chemical reactions: reactant concentration, temperature, catalysts, and surface area. The rate of a reaction is determined by measuring how the concentration of reactants or products changes over time. Reaction rates can be calculated based on either the disappearance of reactants or the appearance of products.
1. The document describes various thermodynamic processes including isobaric, isometric, isothermal, isentropic, and polytropic processes.
2. For isobaric processes in closed systems, work done is equal to pressure times change in volume. For open systems at constant pressure, work done is zero and heat absorbed is equal to enthalpy change.
3. For isentropic processes in closed systems, work done is equal to the negative change in internal energy, and for open systems work done is equal to the negative enthalpy change.
Thermodynamics (2013 new edition) copyYuri Melliza
Thermodynamics deals with energy transformation between different forms. Some key concepts covered in the document include:
- The first law of thermodynamics states that energy cannot be created or destroyed, only converted from one form to another.
- For a closed system, the heat transfer (Q) equals the change in internal energy (U) plus the work (W) done by the system.
- For an open system, the heat (Q) equals the change in enthalpy (H) of the system plus the sum of kinetic energy (KE), potential energy (PE), and work (W).
- Other concepts defined include systems, surroundings, properties of fluids, phases of substances, forms of energy
Mechanical engineer's manual(by. engr. yuri g. melliza)Yuri Melliza
1. This document defines common mechanical engineering terms such as mass, velocity, acceleration, force, pressure, and temperature scales. Conversion factors are provided.
2. Properties of fluids such as density, specific volume, specific gravity, and equations of state for gases are defined. Characteristics including viscosity, elasticity, and surface tension are also explained.
3. Ten sample problems are worked through as examples of applying the definitions and concepts to calculations involving forces, densities, pressures, temperatures, and manometers.
Kinetics is the study of reaction rates and mechanisms. There are four main factors that affect reaction rates: the nature of reactants, temperature, catalysts, and concentration. The rate of a reaction is measured based on how quickly the concentration of reactants decreases or products increases over time. As reactions proceed, the rate generally decreases as reactant concentrations decrease until the reaction reaches equilibrium or the reactants are used up.
1. Chemical kinetics deals with the rates of chemical reactions and factors that affect reaction rates. It examines how fast reactions occur and the mechanisms of reactions.
2. Reaction rates can vary significantly, from fractions of seconds to years. Third-order reactions involve three molecules and are also called termolecular reactions.
3. The rate of a reaction is affected by temperature - higher temperatures provide more energy and increase reaction rates by producing more effective collisions between reactant molecules.
The document discusses key concepts related to gas-vapor mixtures and air conditioning including:
- Dry and atmospheric air, specific and relative humidity.
- Dew-point, adiabatic saturation, and wet-bulb temperatures.
It provides examples and explanations of these terms. Several problems are also included and solved relating to determining properties of air-vapor mixtures under various conditions.
Chapter 4 (propertiesof pure substance)Yuri Melliza
This document discusses the properties of pure substances during phase changes. It defines key terms like saturation temperature, saturation pressure, sub-cooled liquid, saturated liquid, saturated vapor, and superheated vapor. The document explains that 100°C is the saturation temperature corresponding to a pressure of 101.325 kPa. It also provides diagrams to illustrate the different regions on a T-S and h-S chart during phase changes and defines concepts like quality.
This document describes an experimental study that measured ignition delay times for fuel-air mixtures behind reflected shock waves under conditions relevant to homogeneous charge compression ignition (HCCI) engines. Ignition delay times were measured for n-heptane, gasoline, and a gasoline surrogate mixture (iso-octane/toluene/n-heptane) over a range of pressures, temperatures, equivalence ratios, and exhaust gas recirculation levels using pressure history and chemiluminescence diagnostics in shock tubes. The results provide benchmark data for validating detailed chemical kinetic models under HCCI combustion conditions.
The first law of thermodynamics states that the change in internal energy of a system is equal to the heat supplied to the system minus the work done by the system. For a closed system undergoing a process, this can be expressed as ΔU=Q-W. The first law applies to both closed systems undergoing non-flow processes as well as open systems undergoing steady flow processes. For non-flow processes such as constant volume, constant pressure, isothermal, and adiabatic processes, the first law allows determining the relationships between heat, work and changes in internal energy or enthalpy. For steady flow processes, the general energy equation accounts for changes in kinetic and potential energy of the fluid in addition to heat
The document discusses thermodynamic property relations for ideal gases. It provides examples of calculating changes in pressure (dP) given changes in temperature (dT) or specific volume (dv) using the ideal gas law. The examples show that for air and helium, a 1% increase in both T and v results in no net change in pressure (dP=0). The document also examines using partial derivatives to determine slopes of lines on temperature-volume and temperature-pressure diagrams for ideal gases and the van der Waals equation of state.
This document describes a chemistry laboratory experiment to measure the density, specific gravity (SG), and API gravity of fluids. Two methods are used: a hydrometer method and a pycnometer method. The pycnometer method is found to be more accurate due to factors like temperature that can affect hydrometer readings. Calculations are shown to determine the SG and API gravity of a crude oil sample. The API gravity is found to be 47.84, indicating a paraffinic crude oil. Higher API gravity values correspond to crude oils that contain more gasoline and less sulfur.
This document discusses methods for determining the compressibility factor (Z) in gas mixtures. It defines different types of natural gas and describes using pseudocritical properties and reduced conditions to calculate Z based on corresponding states theory. The Standing-Katz method is commonly used to determine Z for sweet gases graphically using reduced pressure and temperature. This method can be modified to account for sour gases containing H2S and CO2 by adjusting the pseudocritical properties. An example calculation demonstrates determining the volume of a gas sample at different conditions using both the unmodified and modified Standing-Katz methods.
The document discusses ideal gases and the ideal gas law. It explains that the ideal gas law (PV=nRT) allows one to calculate the number of moles of a gas given its pressure, volume, and temperature. Real gases behave most ideally at higher temperatures and lower pressures, as the particles have volume and are attracted to each other. The characteristics of an ideal gas are that its particles have no volume and no attraction between particles.
This document provides an overview of a reservoir fluid properties course covering reservoir hydrocarbons including natural gas and crude oil. The course discusses sampling and analysis of reservoir fluids, properties of natural gases such as density and compressibility, properties of crude oils like density and gas solubility, and how reservoir fluids change from reservoir conditions to downstream production and processing facilities as pressure and temperature decrease. Key concepts covered include gas formation volume factor, gas expansion factor, gas solubility and its relationship to pressure and temperature, and methods for determining fluid properties.
This document summarizes a study evaluating correlations for calculating the compressibility factor of natural gases containing non-hydrocarbon components. It discusses how the compressibility factor is used to calculate important gas properties and outlines standard methods like correlations, equations of state, and laboratory measurements. The document focuses on evaluating correlations that account for components like nitrogen, carbon dioxide, and hydrogen sulfide which make predicting the compressibility factor more difficult compared to sweet gases containing only hydrocarbons. It also discusses how these non-hydrocarbon components can affect pseudo-critical temperature and pressure values used in correlations.
This document discusses the basic physics principles relevant to anesthesiology. It explains how anesthesiologists can calculate the amount of gas in a nitrous oxide cylinder using Avogadro's principle and the cylinder's weight. It also describes how pressure regulators work by balancing the pressure and surface area of two diaphragms. Additionally, it covers partial pressure gradients, diffusion of gases, the Joule-Thomson effect, ventilation principles, and how pulmonary surfactant prevents alveolar collapse.
PHYSICAL CHEMISTRY - Gases
Is the branch of chemistry which deals with measurable quantities.
PARTS OF PHYSICAL CHEMISTRY
The physical chemistry is studied under the following sub topics. These are
1. States of matter
2. Chemical equilibrium
3. Thermochemistry/ Energetics
4. Electrochemistry
5. Chemical kinetics
This document contains information about a gaseous state test or assignment, including:
- The table of contents lists 5 exercises and an answer key.
- The document provides definitions and equations for key concepts in the gaseous state including pressure, temperature, the ideal gas law, Boyle's law, Charles' law, Gay-Lussac's law, Avogadro's hypothesis, and the kinetic molecular theory of gases.
- Real gas behavior is discussed along with the van der Waals equation.
Research Internship Thesis - Final Report - Ankit KukrejaANKIT KUKREJA
This document is a project report that measures the vapor pressures and gaseous diffusion coefficients of some selected organic and metalorganic compounds. It begins with an introduction to vapor pressure and its importance in chemical vapor deposition processes. It then describes three common techniques to measure vapor pressure: the Langmuir effusion method, transpiration method, and Knudsen effusion method. The document discusses how vapor pressure depends on temperature based on the Clausius-Clapeyron equation and heat of sublimation. It also covers the measurement of gaseous diffusion coefficients using a quartz crystal microbalance. The experimental section provides details of the Knudsen method setup used and diffusion coefficient measurements. Results are then presented and discussed for
DETERMINING NATURAL GAS PARAMETERS EXPRESSED IN VOLUMEJessol Salvo
This document discusses how to determine natural gas quality parameters expressed in volume (m3) to comply with ISO standards, which traditionally express parameters in mass. It derives density and molecular weight equations to relate mass and volume units. Using composition data, it computes parameters like heating value, density, and Wobbe Index for Nigerian gas. Key parameters and their significance are summarized.
The document discusses several key properties of gases, including mass, volume, temperature, and pressure. It defines these properties and provides examples of how they relate to gases. The document also summarizes several gas laws, including Boyle's Law, Charles' Law, Gay-Lussac's Law, Dalton's Law, and Graham's Law. It provides examples of using these laws to calculate gas properties under different conditions.
1) The document describes an experiment to determine the specific gravity (SG) and API gravity of kerosene and gasoline samples using two methods: hydrometer and pycnometer.
2) The pycnometer method was found to be more accurate than the hydrometer method as the hydrometer is affected by temperature, carbon dioxide, and alcohol content whereas the pycnometer is not.
3) The API gravity value is useful because it provides information on the quality and composition of petroleum products, with higher API gravity indicating more valuable gasoline and less toxic sulfur content.
Specific Gravity, and API Gravity for petroleum productsMuhammad Akram
1) The document describes an experiment to determine the specific gravity and API gravity of kerosene and gasoline using two methods: the hydrometer method and pycnometer method.
2) The pycnometer method was found to be more accurate than the hydrometer method for measuring API and specific gravity, as the hydrometer can be affected by temperature, carbon dioxide, and alcohol content.
3) The API gravity value provides information about the quality and composition of petroleum products, with higher API gravity indicating a product contains more desirable and valuable components like gasoline.
PyTeCK: A Python-based automatic testing package for chemical kinetic modelsOregon State University
Combustion simulations require detailed chemical kinetic models to predict fuel oxidation, heat release, and pollutant emissions. These models are typically validated using qualitative rather than quantitative comparisons with limited sets of experimental data. This work introduces PyTeCK, an open-source Python-based package for automatic testing of chemical kinetic models. Given a model of interest, PyTeCK automatically parses experimental datasets encoded in a YAML format, validates the self-consistency of each dataset, and performs simulations for each experimental datapoint. It then reports a quantitative metric of the model's performance, based on the discrepancy between experimental and simulated values and weighted by experimental variance. The initial version of PyTeCK supports shock tube and rapid compression machine experiments that measure autoignition delay. PyTeCK relies on several packages in the SciPy stack and greater scientific Python ecosystem. In addition to providing an easy-to-use, automated tool for evaluating chemical kinetic model performance, a secondary objective of PyTeCK is to encourage greater openness and reproducibility in combustion research.
This document provides an overview of gas laws and the kinetic molecular theory. It begins with learning objectives and a concept map showing how gas properties are related by the gas laws. It then discusses the kinetic molecular theory and its assumptions that gases are made of particles in constant, rapid, random motion. This theory can explain gas behavior such as how pressure, volume, temperature, and number of moles are related. The document provides definitions and examples of these gas properties and laws including Boyle's law, Charles' law, Avogadro's law, and the combined gas law. It emphasizes that the combined gas law can be used to solve all gas law problems by transforming it based on what variables are held or changed.
This document summarizes an investigation into the behavior of gases at different temperatures, pressures, and volumes. Three experiments were conducted: 1) Boyle's law experiment showing an inverse relationship between pressure and volume at constant temperature, 2) Charles' law experiment showing a direct relationship between volume and temperature at constant pressure, and 3) Gay-Lussac's law experiment showing a direct relationship between pressure and temperature at constant volume. The results of the experiments validated the theoretical gas laws and supported the conclusion that the volume, pressure, and temperature of gases are mutually related as described by the general gas equation.
This document provides an overview of gas laws and the kinetic molecular theory. It begins with learning objectives about the gas laws, pressure, volume, temperature, moles, density, and molar mass. It then discusses the kinetic molecular theory and its assumptions that gases are made of particles in constant random motion. Temperature is proportional to particle kinetic energy. Gas behavior can be explained by kinetic molecular theory, with pressure being due to particle collisions with containers. Several gas laws are introduced relating pressure, volume, temperature, and moles of a gas sample before and after a change. These include Boyle's law, Charles' law, Avogadro's law, and the combined gas law. Problem-solving strategies for using the gas laws
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KuberTENes Birthday Bash Guadalajara - K8sGPT first impressionsVictor Morales
K8sGPT is a tool that analyzes and diagnoses Kubernetes clusters. This presentation was used to share the requirements and dependencies to deploy K8sGPT in a local environment.
Literature Review Basics and Understanding Reference Management.pptxDr Ramhari Poudyal
Three-day training on academic research focuses on analytical tools at United Technical College, supported by the University Grant Commission, Nepal. 24-26 May 2024
HEAP SORT ILLUSTRATED WITH HEAPIFY, BUILD HEAP FOR DYNAMIC ARRAYS.
Heap sort is a comparison-based sorting technique based on Binary Heap data structure. It is similar to the selection sort where we first find the minimum element and place the minimum element at the beginning. Repeat the same process for the remaining elements.
We have compiled the most important slides from each speaker's presentation. This year’s compilation, available for free, captures the key insights and contributions shared during the DfMAy 2024 conference.
CHINA’S GEO-ECONOMIC OUTREACH IN CENTRAL ASIAN COUNTRIES AND FUTURE PROSPECTjpsjournal1
The rivalry between prominent international actors for dominance over Central Asia's hydrocarbon
reserves and the ancient silk trade route, along with China's diplomatic endeavours in the area, has been
referred to as the "New Great Game." This research centres on the power struggle, considering
geopolitical, geostrategic, and geoeconomic variables. Topics including trade, political hegemony, oil
politics, and conventional and nontraditional security are all explored and explained by the researcher.
Using Mackinder's Heartland, Spykman Rimland, and Hegemonic Stability theories, examines China's role
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china’s geo economic outreach in central Asian countries and its future prospect. China is thriving in trade,
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Low power architecture of logic gates using adiabatic techniquesnooriasukmaningtyas
The growing significance of portable systems to limit power consumption in ultra-large-scale-integration chips of very high density, has recently led to rapid and inventive progresses in low-power design. The most effective technique is adiabatic logic circuit design in energy-efficient hardware. This paper presents two adiabatic approaches for the design of low power circuits, modified positive feedback adiabatic logic (modified PFAL) and the other is direct current diode based positive feedback adiabatic logic (DC-DB PFAL). Logic gates are the preliminary components in any digital circuit design. By improving the performance of basic gates, one can improvise the whole system performance. In this paper proposed circuit design of the low power architecture of OR/NOR, AND/NAND, and XOR/XNOR gates are presented using the said approaches and their results are analyzed for powerdissipation, delay, power-delay-product and rise time and compared with the other adiabatic techniques along with the conventional complementary metal oxide semiconductor (CMOS) designs reported in the literature. It has been found that the designs with DC-DB PFAL technique outperform with the percentage improvement of 65% for NOR gate and 7% for NAND gate and 34% for XNOR gate over the modified PFAL techniques at 10 MHz respectively.
1. DISEÑO DE PUENTES DE
MEDICIÓN Y REGULACIÓN DE
GAS NATURAL
Docente: Ing. David Romero Garcia M.Sc.
Módulo 1: Generalidades del Gas Natural y el
D.S. 1996
2. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Generalidades del Gas Natural
Generalidades del
Gas Natural
3. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Generalidades del Gas Natural
EL GAS NATURAL
4. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Generalidades del Gas Natural
Composición Típica
5. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Propiedades Físicas del Gas Natural
Ecuación de Estado de Gas Ideal:
Se denomina comportamiento de gas ideal cuando el gas esta sometido condiciones
estándar, incluso a presiones hasta de 150 psia.
𝑃 𝑉 = 𝑛 𝑅 𝑇
Ecuación de Estado de Gas Real:
Se denomina comportamiento de gas real cuando el gas No esta sometido condiciones
estándar.
𝑃 𝑉 = 𝑍 𝑛 𝑅 𝑇
6. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Propiedades Físicas del Gas Natural
Peso Molecular del Gas (MWa):
El peso molecular aparente de una mezcla de gases (gas natural) puede ser determinado por
la siguiente expresión:
𝑀𝑊𝑎 =
𝑖=1
𝑁
𝑌𝑖 𝑀𝑊𝑖
Donde:
MWa: Peso molecular aparente de la mezcla de Gas, [lb/lbmol].
Yi : Fracción Molar del componente “i”
MWi: Peso molecular del componente “i”, [lb/lbmol].
7. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Propiedades Físicas del Gas Natural
Propiedades Pseudocríticas del Gas:
Las propiedades o condiciones pseudocríticas de una mezcla de gases (gas natural) puede
ser determinado por la siguiente expresión:
Donde:
Psc: Presión pseudocrítica de la mezcla de gas, [psia].
Tsc: Temperatura pseudocrítica de la mezcla de gas, [°R].
Yi : Fracción Molar del componente “i”
Pci: Presión critica del componente “i”, [psia].
Tci: Temperatura critica del componente “i”, [°R].
𝑃𝑠𝑐 =
𝑖=1
𝑁
𝑌𝑖 𝑃𝑐𝑖 𝑇𝑠𝑐 =
𝑖=1
𝑁
𝑌𝑖 𝑇𝑐𝑖
8. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Propiedades Físicas del Gas Natural
Propiedades Pseudorreducidas del Gas:
Las propiedades o condiciones pseudorreducidas de una mezcla de gases (gas natural)
puede ser determinado por la siguiente expresión:
Donde:
Psr: Presión pseudorreducida de la mezcla de gas.
Tsr: Temperatura pseudorreducida de la mezcla de gas.
P: Presión del sistema, [psia].
T: Temperatura del sistema, [°R].
Psc: Presión pseudocrítica de la mezcla de gas, [psia].
Tsc: Temperatura pseudocrítica de la mezcla de gas, [°R].
𝑃𝑠𝑟 =
𝑃
𝑃𝑠𝑐
𝑇𝑠𝑟 =
𝑇
𝑇𝑠𝑐
9. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Propiedades Físicas del Gas Natural
Factor de Compresibilidad del Gas:
Existen varias correlaciones y ábacos para el calculo del factor de compresibilidad del gas,
una de las correlaciones mas exactas es la ecuación de Brill & Beggs:
𝑍 = 𝐴 +
1 − 𝐴
exp(𝐵)
+ 𝐶 𝑃𝑠𝑟
𝐷
𝐴 = 1,39 𝑇𝑠𝑟 − 0,92 0,5
− 0,36𝑇𝑠𝑟 − 0,10
𝐵 = 0,62 − 0,23 𝑇𝑠𝑟 𝑃𝑠𝑟 +
0,066
𝑇𝑠𝑟 − 0,86
− 0,037 𝑃𝑠𝑟
2 +
0,32
109(𝑇𝑠𝑟−1)
𝑃𝑠𝑟6
𝐶 = 0,132 − 0,32 log 𝑇𝑠𝑟
𝐷 = 𝑎𝑛𝑡𝑖𝑙𝑜𝑔 ( 0,3106 − 0,49 𝑇𝑠𝑟 + 0,1824 𝑇𝑠𝑟
2)
10. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Propiedades Físicas del Gas Natural
Densidad del Gas (ρ𝒈):
La densidad de un gas real, puede ser determinado a partir de la siguiente ecuación de
estado:
𝑃 𝑉 = 𝑍 𝑛 𝑅 𝑇
ρ𝑔 =
𝑃 𝑀𝑊
𝑎
𝑍 𝑅 𝑇
Donde:
ρ𝒈: Densidad del gas, [lb/ft3].
P: Presión. [psia].
MWa: Peso molecular aparente de la mezcla de Gas, [lb/lbmol].
Z: Factor de compresibilidad.
R: Constante universal de los gases (10,73),
T: Temperatura, [°R].
11. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Propiedades Físicas del Gas Natural
Viscosidad del Gas (µ𝒈):
La viscosidad de un gas, puede ser determinado a partir de las correlaciones de Lee,
Gonzales y Eakin que se muestran a continuación:
µ𝑔 =
𝐾 exp(𝑋 ρ𝑔
𝑌
)
104
𝐾 =
9,4 + 0,02 𝑀𝑊𝑎 𝑇1,5
209 + 19 𝑀𝑊𝑎 + 𝑇
𝑋 = 3,5 +
986
𝑇
+ 0,01 𝑀𝑊𝑎
𝑌 = 2,4 − 0,2 𝑋
ρ𝑔 = 1,4935 ∗ 10−3
𝑃 𝑀𝑊𝑎
𝑍 𝑇
Donde:
µg: Viscosidad del gas a P y T, [cP].
ρg: Densidad del gas, [gr/cc].
MWa: Peso molecular del Gas,
[lb/lbmol].
Z: Factor de compresibilidad del gas.
P: Presión del sistema, [psia].
T: Temperatura del sistema, [°R].
12. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Propiedades Termodinámicas del G. N.
Entalpía del Gas Natural (H):
La entalpía es una magnitud termodinámica simbolizada con la letra H, la variación de
entalpía expresa una medida de la cantidad de energía absorbida o cedida por un sistema
termodinámico, es decir, la cantidad de energía que un sistema puede intercambiar con su
entorno.
La entalpia puede ser descrita con la siguiente ecuación:
𝐻 = 𝐸 + 𝑃 𝑉
H: entalpía total del sistema.
E: energía interna.
P: presión.
V: volumen.
13. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Propiedades Termodinámicas del G. N.
Entalpía del Gas Natural (Continuación):
Existen métodos analíticos que combinados con ábacos nos ayudan a determinar la entalpía
del gas natural a diferentes condiciones de presión y temperatura, también existen métodos
netamente gráficos (ábacos).
Para propósitos del curso se desarrollarán solamente los métodos gráficos, para lo cual
emplearemos las graficas del capitulo 24 del GPSA.
14. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Propiedades Termodinámicas del G. N.
Entropía del Gas Natural (S):
La entropía es una propiedad termodinámica extensiva la cual se define en términos de un
proceso reversible por la relación:
−𝑑𝑆 =
𝑑𝑄
𝑇
Donde, Q es la cantidad de calor que ingresa o deja un sistema a una temperatura absoluta.
La entropía es una propiedad que tiene importantes aplicaciones, entre las que se destaca la
interpretación del comportamiento de gases y líquidos en procesos de expansión y
compresión.
Las entropías tanto para mezclas de gases o componentes puros puede ser determinado a
partir de las graficas presentadas en la capítulo 24 del GPSA.
15. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Cadena de Valor del Gas Natural
16. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Cadena de Valor del Gas Natural
17. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Endulzamiento del Gas Natural
18. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Deshidratación del Gas Natural
19. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Procesamiento del Gas Natural
Ajuste de Punto de Rocío del Gas Natural y
Estabilización de Condensados
20. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Procesamiento del Gas Natural
Extracción de Líquidos con Turbo Expander
21. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Licuefacción del Gas Natural (GNL)
22. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Decreto Supremo N°1996
Descripción General
del Decreto Supremo
N°1996
23. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Decreto Supremo N°1996
Decreto Supremo 1996 (14 DE MAYO DE 2014):
El D.S. aprueba los siguientes Reglamentos:
• Reglamento de Distribución de Gas Natural por Redes en sus ochenta y tres (83) Artículos
y tres (3) Disposiciones Transitorias,
• Reglamento de Diseño, Construcción, Operación de Redes de Gas Natural e Instalaciones
Internas en sus veintiocho (28) Artículos y una (1) Disposición Transitoria.
El D.S. abroga los os siguientes Reglamentos:
• Se abroga el Decreto Supremo N° 28291, de 11 de agosto de 2005, que aprueba el
Reglamento de Distribución de Gas Natural por Redes y Reglamento de Diseño
Construcción, Operación de Redes de Gas Natural e Instalaciones Internas.
24. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Decreto Supremo N°1996
ARTÍCULO 1.- (OBJETO). El presente Reglamento tiene por objeto normar las condiciones
técnicas, legales, económicas, así como los procedimientos administrativos, para realizar
actividades de Distribución de Gas Natural por Redes.
ARTÍCULO 2.- (ÁMBITO DE APLICACIÓN).
I. El presente Reglamento es de cumplimiento obligatorio, para todas aquellas personas
jurídicas, nacionales o extranjeras, públicas o privadas, que realicen directa o indirectamente
la actividad de Distribución de Gas Natural por Redes dentro del territorio nacional.
Asimismo para los usuarios del servicio de Distribución de Gas Natural por Redes
dentro del territorio nacional.
II. Asimismo, están sujetas al presente Reglamento las personas individuales o colectivas,
nacionales o extranjeras, públicas o privadas, cuya actividad esté relacionada con la
Distribución de Gas Natural por Redes.
25. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Decreto Supremo N°1996
ARTÍCULO 3.- (ALCANCE).
I. La actividad de Distribución de Gas Natural por Redes se ejercerá mediante Licencia de
Operación otorgada por el Ente Regulador, de acuerdo a procedimiento administrativo
establecido en el presente Reglamento.
II. La Distribución de Gas Natural por Redes es un servicio público que debe ser prestado de
manera regular y continua, comprende desde el Punto de Entrega del Gas Natural por parte
de la empresa de transporte, hasta la entrega al usuario de las distintas categorías de uso y
consumo.
26. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Decreto Supremo N°1996
ARTÍCULO 22.- (ANEXOS).
I. El diseño, construcción, operación y mantenimiento de las Redes Primarias y Redes
Secundarias se realizarán estrictamente bajo lo establecido en el ANEXO 1: Diseño de Redes;
ANEXO 2: Construcción de Redes de Gas Natural; ANEXO 3: Operación y Mantenimiento de
Redes de Gas Natural; ANEXO 4: Calidad del Gas, del presente Reglamento Técnico.
II. Los parámetros de manejo y calidad del Gas Natural a ser distribuido mediante las Redes
de Distribución deben cumplir con lo expresado en el ANEXO 4: Calidad del Gas Natural, del
presente Reglamento Técnico.
III. La instalación, operación y parámetros de seguridad de las Instalaciones Internas
Domiciliarias y Comerciales deberán ser realizadas cumpliendo lo estipulado en el ANEXO 5:
Instalaciones de Categorías Doméstica y Comercial de Gas Natural.
27. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Decreto Supremo N°1996
ARTÍCULO 22.- (ANEXOS) Cont.
IV. La instalación, operación y parámetros de seguridad de las instalaciones industriales,
deberán ser realizadas cumpliendo lo estipulado en el ANEXO 6: Instalaciones Industriales de
Gas Natural.
V. La instalación, operación y mantenimiento de las Estaciones Distritales de Regulación EDR,
deberán ser realizadas cumpliendo lo estipulado en el ANEXO 7: Estaciones Distritales de
Regulación.
28. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Decreto Supremo N°1996
Anexo 4:
Calidad del Gas Natural
29. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Anexo 4: Calidad del Gas Natural
1. Objeto.
El presente Anexo tiene por objeto establecer las condiciones de composición y odorización
del Gas Natural para asegurar la calidad y seguridad del fluido suministrado.
2. Alcance.
El presente Anexo se aplicará en todo el territorio nacional y consiste en la normativa técnica
de cumplimiento obligatorio para las Distribuidoras.
3. Ámbito de aplicación.
El presente Anexo se aplicará a todos los sistemas de distribución de Gas Natural por
tuberías.
30. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Anexo 4: Calidad del Gas Natural
ODORIZACIÓN DEL GAS NATURAL:
La odorización del gas natural normalmente se realiza en el City Gate.
1. El Gas Natural en un Sistema de Distribución, en su totalidad debe ser odorizado a una
concentración en aire de 1/5 del Límite Inferior de Explosividad.
2. Para casos particulares de Usuarios de Línea, así como Usuarios conectados a la Red
Primaria industriales o GNV, la Distribuidora analizará y presentará al Ente Regulador.
31. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Anexo 4: Calidad del Gas Natural
ODORIZACIÓN DEL GAS NATURAL:
Sistemas de distribución secundaria:
En todo sistema de distribución secundaria, se deberá contar como mínimo con tres puntos
de medición representativos por EDR.
Sistemas de distribución primaria:
Por lo menos deberá contar con un punto de medición en cada sistema de distribución, si
esta no alimenta a una EDR.
* En Redes Primarias el sistema de toma de odorización se podrá realizar en un PRM del
usuario.
32. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Anexo 4: Calidad del Gas Natural
33. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Anexo 4: Calidad del Gas Natural
34. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Anexo 4: Calidad del Gas Natural
35. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Anexo 4: Calidad del Gas Natural
Nota (1): Propiedades cuyas especificaciones deberán ser cumplidas y certificadas
mensualmente por la empresa encargada del proceso de licuefacción del Gas Natural, en
este caso la densidad relativa del Gas Natural será como mínimo de 0,55 y el porcentaje de
N2 no será mayor de 2,5 % vol.
La calidad del Gas Natural suministrado mediante transporte por ductos para el sistema de
distribución y para el sistema de transporte virtual de GNC, debe ser certificada por la
empresa encargada del transporte de Gas Natural por ductos a la Distribuidora en
cumplimiento del Reglamento de Distribución de Gas Natural por Redes y cumpliendo con
las especificaciones de la Tabla 1.
En el caso de suministro de Gas Natural para el sistema de distribución mediante Transporte
Virtual de GNL incluido el sistema mediante transporte de GNC a partir de GNL, la calidad del
Gas Natural debe ser certificada por la empresa encargada de la licuefacción del Gas Natural
para cada uno de los puntos de entrega cumpliendo con las especificaciones
correspondientes de la Tabla 1 Nota (1).
36. Docente: Ing. David Romero Garcia M.Sc.
CURSO: DISEÑO DE P.R.M. DE GAS NATURAL
Módulo I