This report contains the theory behind the algorithm to find the composition of air at temperatures 200-9000 K. A C++ program for the same is hosted at my profile on GitHub.com/kcavatar.
This document summarizes a study that measured the thermodynamic properties of Al1-xGaxN solid solutions at high temperatures using a solid-state electrochemical cell. The cell was used to determine the activity of GaN in Al1-xGaxN at 1100 K. Excess Gibbs free energy of mixing was then calculated. Results showed a mild tendency for ordering at specific compositions, along with predominantly positive deviation from ideal mixing behavior. Thermodynamic calculations also indicated instability below 410 K for compositions between 0.26≤x≤0.5.
The document discusses equilibrium constants (Kc) and how to calculate them using concentrations of reactants and products at equilibrium. It provides examples of calculating Kc values for reactions, including determining initial and change in concentrations. It also discusses using Kc to predict the direction a reaction will proceed based on comparing the reaction quotient (Q) to Kc.
The document discusses several gas laws:
- Boyle's law states that at constant temperature, the volume of a gas is inversely proportional to its pressure.
- Charles' law states that at constant pressure, the volume of a gas is directly proportional to its kelvin temperature.
- Combined gas law allows calculation of gas properties when temperature and/or pressure change.
It also discusses concepts like the kinetic molecular theory of gases and how real gases deviate from ideal gas behavior due to intermolecular forces and molecular size. Sample calculations demonstrate use of the gas laws and kinetic theory.
Chemical equations are used to represent chemical changes. They show the reactants and products of a reaction. A balanced chemical equation has the same number and type of atoms of each element on both sides. To balance an equation, the coefficients of the molecules are adjusted without changing subscripts so that atomic balance is achieved. Balanced equations indicate the mole ratios in which substances react, allowing for calculations relating amounts in moles of reactants and products.
This document provides an overview of chapter 5 from the textbook, which covers gases and the kinetic molecular theory. It begins with learning objectives and concepts to understand from sections 5.5 through 5.12. There is then an explanation of applications of the gas laws, including Dalton's law of partial pressures and collecting gases over water. The document continues with explanations of gas density, the ideal gas law, Graham's law of effusion, and the kinetic molecular theory. It includes sample problems and exercises related to these topics.
Entropy is a measure of disorder or randomness in a system. It increases as a reaction progresses from reactants to products. Nuclear reactions like fission and fusion release large amounts of energy and can be spontaneous or non-spontaneous depending on whether the products have lower or higher energy than the reactants. Nuclear reactions involve the emission of particles like alpha, beta, or gamma rays and must balance atomic and mass numbers.
This document provides an overview of gas laws and the behavior of gases. It begins by defining the three states of matter and distinguishing properties of gases. Gas pressure and its measurement are then discussed, including common pressure units. The document outlines the major gas laws - Boyle's Law relating pressure and volume at constant temperature, Charles' Law relating volume and temperature at constant pressure, and the Combined Gas Law combining these relationships. Examples are provided to demonstrate applications of the gas laws. The ideal gas law is defined as relating pressure, volume, temperature, and moles of gas. The behavior of gases at standard temperature and pressure is also covered.
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.
This document summarizes a study that measured the thermodynamic properties of Al1-xGaxN solid solutions at high temperatures using a solid-state electrochemical cell. The cell was used to determine the activity of GaN in Al1-xGaxN at 1100 K. Excess Gibbs free energy of mixing was then calculated. Results showed a mild tendency for ordering at specific compositions, along with predominantly positive deviation from ideal mixing behavior. Thermodynamic calculations also indicated instability below 410 K for compositions between 0.26≤x≤0.5.
The document discusses equilibrium constants (Kc) and how to calculate them using concentrations of reactants and products at equilibrium. It provides examples of calculating Kc values for reactions, including determining initial and change in concentrations. It also discusses using Kc to predict the direction a reaction will proceed based on comparing the reaction quotient (Q) to Kc.
The document discusses several gas laws:
- Boyle's law states that at constant temperature, the volume of a gas is inversely proportional to its pressure.
- Charles' law states that at constant pressure, the volume of a gas is directly proportional to its kelvin temperature.
- Combined gas law allows calculation of gas properties when temperature and/or pressure change.
It also discusses concepts like the kinetic molecular theory of gases and how real gases deviate from ideal gas behavior due to intermolecular forces and molecular size. Sample calculations demonstrate use of the gas laws and kinetic theory.
Chemical equations are used to represent chemical changes. They show the reactants and products of a reaction. A balanced chemical equation has the same number and type of atoms of each element on both sides. To balance an equation, the coefficients of the molecules are adjusted without changing subscripts so that atomic balance is achieved. Balanced equations indicate the mole ratios in which substances react, allowing for calculations relating amounts in moles of reactants and products.
This document provides an overview of chapter 5 from the textbook, which covers gases and the kinetic molecular theory. It begins with learning objectives and concepts to understand from sections 5.5 through 5.12. There is then an explanation of applications of the gas laws, including Dalton's law of partial pressures and collecting gases over water. The document continues with explanations of gas density, the ideal gas law, Graham's law of effusion, and the kinetic molecular theory. It includes sample problems and exercises related to these topics.
Entropy is a measure of disorder or randomness in a system. It increases as a reaction progresses from reactants to products. Nuclear reactions like fission and fusion release large amounts of energy and can be spontaneous or non-spontaneous depending on whether the products have lower or higher energy than the reactants. Nuclear reactions involve the emission of particles like alpha, beta, or gamma rays and must balance atomic and mass numbers.
This document provides an overview of gas laws and the behavior of gases. It begins by defining the three states of matter and distinguishing properties of gases. Gas pressure and its measurement are then discussed, including common pressure units. The document outlines the major gas laws - Boyle's Law relating pressure and volume at constant temperature, Charles' Law relating volume and temperature at constant pressure, and the Combined Gas Law combining these relationships. Examples are provided to demonstrate applications of the gas laws. The ideal gas law is defined as relating pressure, volume, temperature, and moles of gas. The behavior of gases at standard temperature and pressure is also covered.
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.
1) The document describes the ideal gas law and how to use it to solve problems involving gases. It defines the ideal gas law equation and explains how to rearrange it to solve for unknown pressure, volume, moles, or temperature.
2) Sample problems demonstrate using the ideal gas law to calculate pressure given moles, volume and temperature, and to determine molar mass given mass, pressure, volume and temperature.
3) Additional applications include using the gas law to calculate density from pressure, molar mass and temperature, or to determine temperature given density, pressure and molar mass.
This document provides an overview of three sections (13.1, 13.2, 13.3) from a chemistry textbook chapter on gases. Section 13.1 describes gas laws including Boyle's law, Charles' law, Gay-Lussac's law, and the combined gas law. Section 13.2 introduces the ideal gas law, Avogadro's principle, and compares real and ideal gases. Section 13.3 explains how to use gas laws and stoichiometry to solve problems involving gaseous reactants and products in chemical equations.
1. The document discusses irreversible and reversible reactions. Irreversible reactions proceed in only the forward direction, while reversible reactions can proceed in both directions.
2. It defines chemical equilibrium as the state where the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. At equilibrium, the reaction is dynamic rather than stopped.
3. It explains the law of mass action, which states that the rate of a reaction is directly proportional to the active masses or concentrations of reactants. The equilibrium constant K is derived from the law of mass action.
This document contains the solutions to homework problems assigned in a thermodynamics course. It provides instructions for submitting homework solutions, including showing all work. It then lists 7 problems and provides the numerical solutions. The problems cover various thermodynamic concepts like the ideal gas law, polytropic processes, work calculations, property tables and definitions.
The document discusses chemical equilibrium. It begins by defining chemical equilibrium as a state where the forward and reverse reaction rates are equal, but the reactions are still occurring dynamically. It also notes that at equilibrium, the concentrations or pressures of all species remain constant over time. The document then provides the definitions and expressions for equilibrium constants Kc and Kp, which relate the concentrations or pressures of reactants and products at equilibrium. It also discusses how equilibrium positions can be manipulated by changing conditions based on Le Chatelier's principle.
The document provides information about chemical reactions, including defining reactants and products, describing types of chemical reactions like synthesis, decomposition, double displacement, displacement and combustion reactions. It also discusses how to write and balance chemical equations.
The document discusses reaction rates and factors that affect them. It defines reaction rate as how quickly reactants disappear to form products. Five main factors that affect reaction rates are outlined: (1) chemical nature of reactants, (2) surface area, (3) reactant concentration, (4) temperature, and (5) presence of a catalyst. Reaction rates can be quantified using rate laws and rate constants. The order of a reaction is determined experimentally and indicated by the exponents in the rate law equation.
F.Sc. Part 1 Chemistry.Ch.03.Test (Malik Xufyan)Malik Xufyan
The document lists chemistry test series books for various classes from 9th to F.Sc published by Malik Xufyan of JIAS Academy. It provides information about chapter-wise and board paper-wise test series for different topics in chemistry. Contact details are given at the end for the publisher Jhang Institute for Advanced Studies.
The document discusses kinetic theory of gases and related concepts. It contains 60 multiple choice questions related to:
1) Gas laws such as Boyle's law, Charles' law and their relationships to kinetic theory
2) Concepts such as pressure, volume, temperature, gas constant and their relationships defined by the kinetic theory
3) Properties of ideal gases such as root mean square speed, average kinetic energy and their dependence on temperature and molecular mass.
The document discusses equilibrium and contains 20 questions with answers regarding concepts like how changing the volume of a container affects vapor pressure, how to calculate equilibrium constants (Kc and Kp) for different chemical reactions, and how to determine equilibrium concentrations. It provides examples of calculating equilibrium concentrations and equilibrium constants from initial concentrations and reaction quotients or partial pressures. The questions cover a range of equilibrium concepts and chemical reactions.
States of matter can exist as solids, liquids, or gases. Gases have no definite shape or volume, are highly compressible, and their molecules are far apart with weak intermolecular forces. Liquids have a definite volume but no definite shape, while solids have both a definite shape and volume. The behavior of gases is explained by gas laws such as Boyle's law, Charles's law, Avogadro's law, Dalton's law of partial pressures, Graham's law of diffusion, and the ideal gas law. Gases can be liquefied under high pressure and low temperature due to intermolecular attractions that cause real gases to deviate from ideal behavior.
The document contains multiple choice questions about gas laws, kinetic molecular theory, and properties of gases.
1) Questions ask about calculating properties like density and pressure given temperature, volume, amount of gas, and other variables.
2) Other questions relate to concepts like effusion rates, van der Waals constants, and the relationship between temperature, pressure, volume, and number of gas molecules.
3) Graphs and diagrams are included that must be interpreted in the context of gas behavior and equations of state.
Heat transfer ies gate ias 20 years question and answers by s k mondalbinny 004
This document contains 20 chapters on heat transfer topics including modes of heat transfer, conduction, extended surfaces, unsteady conduction, convection, boiling and condensation, heat exchangers, and radiation. It also contains objective questions from previous GATE and IES exams on these topics along with explanations of the answers. The author, S.K. Mondal, is an engineering professional with over 12 years of teaching experience in heat transfer topics relevant to the GATE, IES, and IAS exams.
This document provides an overview of the key concepts covered in 5 sections of a chapter on energy and chemical change:
Section 15.1 defines energy and distinguishes between potential and kinetic energy. It relates chemical potential energy to heat released or absorbed in chemical reactions.
Section 15.2 describes how calorimetry is used to measure energy changes and defines enthalpy and enthalpy changes.
Section 15.3 explains how to write thermochemical equations and describes energy changes during state changes.
Section 15.4 discusses calculating enthalpy changes using Hess's law and standard enthalpies of formation.
Section 15.5 differentiates between spontaneous and nonspontaneous processes and explains how entropy
The document summarizes 12 gas laws including Boyle's law, Charles' law, Avogadro's law, and the ideal gas law. It provides examples of calculations using these laws to determine moles of gas, volumes at different temperatures and pressures, and identities of gases based on density. Key formulas covered are PV=nRT, relationships between volume, pressure and temperature, and stoichiometric calculations using gas volumes.
This document contains a chapter menu and outline for a chapter on reaction rates. The chapter is divided into 4 main sections:
1) A Model for Reaction Rates - discusses calculating reaction rates from data and relating rates to collisions between particles.
2) Factors Affecting Reaction Rates - identifies factors like concentration, temperature, surface area, and catalysts that affect reaction rates.
3) Reaction Rate Laws - expresses the relationship between reaction rate and concentration, and how to determine reaction orders.
4) Instantaneous Reaction Rates and Reaction Mechanisms - discusses calculating instantaneous rates, complex reactions having multiple steps, and relating rates to reaction mechanisms.
This chapter discusses the key concepts and gas laws relating to gases:
1) Boyle's law describes the inverse relationship between pressure and volume at constant temperature.
2) Charles' law explains that gas volume increases with temperature at constant pressure.
3) Avogadro's law states that equal volumes of gases under the same conditions contain equal numbers of molecules.
4) The ideal gas law combines these relationships to quantitatively relate the pressure, volume, temperature, and amount of an ideal gas.
11.a new mechanism of sodium zirconate formationAlexander Decker
This document presents a new mechanism for forming sodium zirconate (Na2ZrO3) through the thermal decomposition of sodium acetate (CH3COONa) and zirconium(IV) acetylacetonate (Zr(C5H7O2)4). Thermogravimetric analysis showed the reaction occurs in three significant weight losses. Fourier transform infrared spectroscopy identified gases like CO2 and CO released during the reaction. X-ray diffraction confirmed the product was sodium zirconate. A kinetic study determined the activation energy, pre-exponential factor, and reaction order for each weight loss region using the Arrhenius equation. The proposed mechanism involves three reactions corresponding to the decomposition
5-Determining Equilibrium Constant General Chemistry 2OliricFabiolas
1. The document discusses calculating equilibrium constants and determining which species are dominant at equilibrium for different chemical reactions.
2. It provides rules for writing equilibrium constant expressions and examples of calculating KC and KP values using concentration or pressure data.
3. The key steps shown are converting between KC and KP using the Van't Hoff equation, and using the calculated equilibrium constant values to determine whether the equilibrium lies towards the reactants or products.
Regression Modelling of Thermal Degradation Kinetics, of Concentrated, Aqueou...Shaukat Mazari
The document presents the results of regression analysis performed on experimental thermal degradation kinetics data of concentrated aqueous piperazine (PZ) solvent loaded with carbon dioxide. Six expressions based on first-order and second-order rate laws were used to model the data using linear and non-linear regression. The analysis revealed that the data followed both first-order and second-order kinetics. Expressions 3 and 5 provided the best fits with R2 values over 0.99, indicating the thermal degradation of PZ is best described by a second-order rate law. The rate constants k1 and k2 could be predicted using the developed models.
This document contains 116 multiple choice questions from an AIEEE exam covering topics in chemistry and physics. The questions test knowledge of quantum numbers, atomic structure, chemical bonding, thermodynamics, equilibrium, electrochemistry, and other core concepts. Sample questions include identifying the correct set of quantum numbers for an electron in the 4f orbital and determining the standard reduction potential of a cell involving a one electron change reaction.
1) The document describes the ideal gas law and how to use it to solve problems involving gases. It defines the ideal gas law equation and explains how to rearrange it to solve for unknown pressure, volume, moles, or temperature.
2) Sample problems demonstrate using the ideal gas law to calculate pressure given moles, volume and temperature, and to determine molar mass given mass, pressure, volume and temperature.
3) Additional applications include using the gas law to calculate density from pressure, molar mass and temperature, or to determine temperature given density, pressure and molar mass.
This document provides an overview of three sections (13.1, 13.2, 13.3) from a chemistry textbook chapter on gases. Section 13.1 describes gas laws including Boyle's law, Charles' law, Gay-Lussac's law, and the combined gas law. Section 13.2 introduces the ideal gas law, Avogadro's principle, and compares real and ideal gases. Section 13.3 explains how to use gas laws and stoichiometry to solve problems involving gaseous reactants and products in chemical equations.
1. The document discusses irreversible and reversible reactions. Irreversible reactions proceed in only the forward direction, while reversible reactions can proceed in both directions.
2. It defines chemical equilibrium as the state where the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. At equilibrium, the reaction is dynamic rather than stopped.
3. It explains the law of mass action, which states that the rate of a reaction is directly proportional to the active masses or concentrations of reactants. The equilibrium constant K is derived from the law of mass action.
This document contains the solutions to homework problems assigned in a thermodynamics course. It provides instructions for submitting homework solutions, including showing all work. It then lists 7 problems and provides the numerical solutions. The problems cover various thermodynamic concepts like the ideal gas law, polytropic processes, work calculations, property tables and definitions.
The document discusses chemical equilibrium. It begins by defining chemical equilibrium as a state where the forward and reverse reaction rates are equal, but the reactions are still occurring dynamically. It also notes that at equilibrium, the concentrations or pressures of all species remain constant over time. The document then provides the definitions and expressions for equilibrium constants Kc and Kp, which relate the concentrations or pressures of reactants and products at equilibrium. It also discusses how equilibrium positions can be manipulated by changing conditions based on Le Chatelier's principle.
The document provides information about chemical reactions, including defining reactants and products, describing types of chemical reactions like synthesis, decomposition, double displacement, displacement and combustion reactions. It also discusses how to write and balance chemical equations.
The document discusses reaction rates and factors that affect them. It defines reaction rate as how quickly reactants disappear to form products. Five main factors that affect reaction rates are outlined: (1) chemical nature of reactants, (2) surface area, (3) reactant concentration, (4) temperature, and (5) presence of a catalyst. Reaction rates can be quantified using rate laws and rate constants. The order of a reaction is determined experimentally and indicated by the exponents in the rate law equation.
F.Sc. Part 1 Chemistry.Ch.03.Test (Malik Xufyan)Malik Xufyan
The document lists chemistry test series books for various classes from 9th to F.Sc published by Malik Xufyan of JIAS Academy. It provides information about chapter-wise and board paper-wise test series for different topics in chemistry. Contact details are given at the end for the publisher Jhang Institute for Advanced Studies.
The document discusses kinetic theory of gases and related concepts. It contains 60 multiple choice questions related to:
1) Gas laws such as Boyle's law, Charles' law and their relationships to kinetic theory
2) Concepts such as pressure, volume, temperature, gas constant and their relationships defined by the kinetic theory
3) Properties of ideal gases such as root mean square speed, average kinetic energy and their dependence on temperature and molecular mass.
The document discusses equilibrium and contains 20 questions with answers regarding concepts like how changing the volume of a container affects vapor pressure, how to calculate equilibrium constants (Kc and Kp) for different chemical reactions, and how to determine equilibrium concentrations. It provides examples of calculating equilibrium concentrations and equilibrium constants from initial concentrations and reaction quotients or partial pressures. The questions cover a range of equilibrium concepts and chemical reactions.
States of matter can exist as solids, liquids, or gases. Gases have no definite shape or volume, are highly compressible, and their molecules are far apart with weak intermolecular forces. Liquids have a definite volume but no definite shape, while solids have both a definite shape and volume. The behavior of gases is explained by gas laws such as Boyle's law, Charles's law, Avogadro's law, Dalton's law of partial pressures, Graham's law of diffusion, and the ideal gas law. Gases can be liquefied under high pressure and low temperature due to intermolecular attractions that cause real gases to deviate from ideal behavior.
The document contains multiple choice questions about gas laws, kinetic molecular theory, and properties of gases.
1) Questions ask about calculating properties like density and pressure given temperature, volume, amount of gas, and other variables.
2) Other questions relate to concepts like effusion rates, van der Waals constants, and the relationship between temperature, pressure, volume, and number of gas molecules.
3) Graphs and diagrams are included that must be interpreted in the context of gas behavior and equations of state.
Heat transfer ies gate ias 20 years question and answers by s k mondalbinny 004
This document contains 20 chapters on heat transfer topics including modes of heat transfer, conduction, extended surfaces, unsteady conduction, convection, boiling and condensation, heat exchangers, and radiation. It also contains objective questions from previous GATE and IES exams on these topics along with explanations of the answers. The author, S.K. Mondal, is an engineering professional with over 12 years of teaching experience in heat transfer topics relevant to the GATE, IES, and IAS exams.
This document provides an overview of the key concepts covered in 5 sections of a chapter on energy and chemical change:
Section 15.1 defines energy and distinguishes between potential and kinetic energy. It relates chemical potential energy to heat released or absorbed in chemical reactions.
Section 15.2 describes how calorimetry is used to measure energy changes and defines enthalpy and enthalpy changes.
Section 15.3 explains how to write thermochemical equations and describes energy changes during state changes.
Section 15.4 discusses calculating enthalpy changes using Hess's law and standard enthalpies of formation.
Section 15.5 differentiates between spontaneous and nonspontaneous processes and explains how entropy
The document summarizes 12 gas laws including Boyle's law, Charles' law, Avogadro's law, and the ideal gas law. It provides examples of calculations using these laws to determine moles of gas, volumes at different temperatures and pressures, and identities of gases based on density. Key formulas covered are PV=nRT, relationships between volume, pressure and temperature, and stoichiometric calculations using gas volumes.
This document contains a chapter menu and outline for a chapter on reaction rates. The chapter is divided into 4 main sections:
1) A Model for Reaction Rates - discusses calculating reaction rates from data and relating rates to collisions between particles.
2) Factors Affecting Reaction Rates - identifies factors like concentration, temperature, surface area, and catalysts that affect reaction rates.
3) Reaction Rate Laws - expresses the relationship between reaction rate and concentration, and how to determine reaction orders.
4) Instantaneous Reaction Rates and Reaction Mechanisms - discusses calculating instantaneous rates, complex reactions having multiple steps, and relating rates to reaction mechanisms.
This chapter discusses the key concepts and gas laws relating to gases:
1) Boyle's law describes the inverse relationship between pressure and volume at constant temperature.
2) Charles' law explains that gas volume increases with temperature at constant pressure.
3) Avogadro's law states that equal volumes of gases under the same conditions contain equal numbers of molecules.
4) The ideal gas law combines these relationships to quantitatively relate the pressure, volume, temperature, and amount of an ideal gas.
11.a new mechanism of sodium zirconate formationAlexander Decker
This document presents a new mechanism for forming sodium zirconate (Na2ZrO3) through the thermal decomposition of sodium acetate (CH3COONa) and zirconium(IV) acetylacetonate (Zr(C5H7O2)4). Thermogravimetric analysis showed the reaction occurs in three significant weight losses. Fourier transform infrared spectroscopy identified gases like CO2 and CO released during the reaction. X-ray diffraction confirmed the product was sodium zirconate. A kinetic study determined the activation energy, pre-exponential factor, and reaction order for each weight loss region using the Arrhenius equation. The proposed mechanism involves three reactions corresponding to the decomposition
5-Determining Equilibrium Constant General Chemistry 2OliricFabiolas
1. The document discusses calculating equilibrium constants and determining which species are dominant at equilibrium for different chemical reactions.
2. It provides rules for writing equilibrium constant expressions and examples of calculating KC and KP values using concentration or pressure data.
3. The key steps shown are converting between KC and KP using the Van't Hoff equation, and using the calculated equilibrium constant values to determine whether the equilibrium lies towards the reactants or products.
Regression Modelling of Thermal Degradation Kinetics, of Concentrated, Aqueou...Shaukat Mazari
The document presents the results of regression analysis performed on experimental thermal degradation kinetics data of concentrated aqueous piperazine (PZ) solvent loaded with carbon dioxide. Six expressions based on first-order and second-order rate laws were used to model the data using linear and non-linear regression. The analysis revealed that the data followed both first-order and second-order kinetics. Expressions 3 and 5 provided the best fits with R2 values over 0.99, indicating the thermal degradation of PZ is best described by a second-order rate law. The rate constants k1 and k2 could be predicted using the developed models.
This document contains 116 multiple choice questions from an AIEEE exam covering topics in chemistry and physics. The questions test knowledge of quantum numbers, atomic structure, chemical bonding, thermodynamics, equilibrium, electrochemistry, and other core concepts. Sample questions include identifying the correct set of quantum numbers for an electron in the 4f orbital and determining the standard reduction potential of a cell involving a one electron change reaction.
The document provides 13 numerical problems related to chemical thermodynamics and energetics. The problems cover topics like work done during gas expansion/compression, standard enthalpy of reaction calculations using bond energies and standard state data, spontaneity of reactions using standard Gibbs free energy and entropy values, heat and enthalpy changes during phase transitions, and calculations involving standard enthalpies of formation.
ch13_part1 (Reacting mixtures and combustion, Heating values, Gibbs function)...Mehran Bashir
This chapter discusses combustion reactions and concepts related to modeling combustion processes. It introduces key topics like complete combustion, theoretical air, enthalpy of formation, and adiabatic flame temperature. The chapter explains how to determine balanced reaction equations for combustion and apply concepts like mass, energy, and entropy balances to systems undergoing chemical reactions. It also discusses dry product analysis and modeling combustion air as an ideal gas mixture.
The document contains 13 problems related to thermodynamics concepts like heat, work, internal energy, enthalpy, free energy, and chemical equilibrium. The problems involve calculations using these concepts for systems involving gases, reactions, and phase changes. Thermodynamic properties like heat capacities, enthalpies, and free energies are provided to calculate unknown values like temperature changes, energies, and equilibrium constants.
This document provides instructions for determining the molar volume of carbon dioxide gas through experiment. Students will measure the mass and volume of a CO2 gas sample under laboratory conditions. By calculating the mass of CO2 using the mass difference between an empty flask and one filled with CO2, and knowing the volume and temperature/pressure, students can use the ideal gas law to calculate the molar volume of CO2. The percentage error between the calculated and theoretical molar volume will also be determined to evaluate the accuracy of the experiment.
This document contains a 30 question chemistry sample exam with multiple choice and long answer questions. It provides instructions for the exam, including question types and point values. The questions cover topics such as chemical formulas, hybrid orbitals, equilibrium reactions, acid-base chemistry, and organic chemistry reactions. Sample solutions are provided for some questions as examples. The exam is designed to test understanding of essential chemistry concepts and principles.
Combustion 1st question Erdi Karaçal Mechanical EngineerErdi Karaçal
The document discusses calculating the gas composition from burning methane at different temperatures. It provides the equations and kinetics approach used, including equilibrium constants, to determine the molar coefficients and resulting mole fractions of CO2, CO, H2O, and H2. The calculations were performed using software and show that the gas composition does not change significantly when the temperature is increased from 1500K to 2500K, as requested in the questions. The document concludes by providing a table of the exhaust gas compositions at various temperatures.
The document contains 76 multiple choice questions from a chemistry exam. It covers topics like quantum numbers, light wavelength and energy, gas laws, chemical bonding, acid-base reactions, and organic chemistry reactions. For each question, the possible multiple choice answers are provided along with the correct answer identified. Brief explanations or solutions are given for each question to justify the right answer.
Thermal Simulation of Biogas Plants Using Mat LabIJERA Editor
The major prerequisite for the optimum production of methane from a biogas plant is the sustenance of digester temperature within the narrow limits (300C-350C). It is experimentally investigated that, the MIT biogas plant is not maintaining optimum temperature, this decreases the efficiency and increases the detention time for charge. To maintain the plant in optimum temperature, it is necessary to find out the heat losses from the biogas plant and the external energy inputs need to operate the plant. Rate of gas yield, and the detention time (time necessary to anaerobically digest organic wastes) in a biogas reactor, are favorable functions of the temperature in the digester. A thermal simulation for MIT biogas plant has developed using matlab in order to understand the heat transfer from the slurry and the gas holder to the surrounding earth and air respectively. The computation has been performed when the slurry is maintained at 200C and 300C, optimum temperature of anaerobic fermentation. If the slurry is considered to be at 350C, the optimum temperature of anaerobic fermentation, the total heat loss from the plant is higher than the heat loss when the slurry is maintained at 200C. The heat calculations provide an appraisal for the heat which has to be supplied by external means to compensate for the net heat losses which occur if the slurry is to be maintained at 350C. A solar system with auxiliary electric heater is designed for maintaining the slurry at 350C.In conclusion; the results of thermal analysis are used to define a strategy for operating biogas plant at optimum temperatures.
Thermoelectric Power Studies Cu-Cd Nano FerritesIJERA Editor
Thermoelectric Power Studies of Cadmium Substituted Copper nano Ferrites of various compositions were investigated from room temperature to well beyond the curie temperature by differential method. The Seebeck coefficient is negative for all compositions showing that these ferrites behave as n-type semi conductors. Plots of Seebeck coefficient verses temperature shows maximum at Curie temperature. On the basis of these results an explanation for the conduction mechanism in Cu-Cd mixed ferrites is suggested
Thermoelectric Power Studies Cu-Cd Nano FerritesIJERA Editor
Thermoelectric Power Studies of Cadmium Substituted Copper nano Ferrites of various compositions were investigated from room temperature to well beyond the curie temperature by differential method. The Seebeck coefficient is negative for all compositions showing that these ferrites behave as n-type semi conductors. Plots of Seebeck coefficient verses temperature shows maximum at Curie temperature. On the basis of these results an explanation for the conduction mechanism in Cu-Cd mixed ferrites is suggested
This document provides an overview of chemical equilibria, including:
- Equilibrium is the state where concentrations of reactants and products remain constant over time. Reactions at equilibrium are reversible.
- The equilibrium position depends on initial concentrations, relative energies of reactants/products, and degree of organization.
- The equilibrium constant K relates concentrations of products over reactants at equilibrium. K values indicate whether a reaction favors products or reactants.
- The reaction quotient Q is similar to K but used when a system is not at equilibrium to predict the direction of the shift to reach equilibrium.
Several examples are provided to demonstrate calculating equilibrium concentrations and values of K using balanced reactions, initial concentrations, and equilibrium expressions.
Chemical equilibrium is a state where the rates of the forward and reverse reactions are equal and the concentrations of reactants and products remain constant. Equilibrium is achieved when these conditions are met. The equilibrium constant, K, provides a quantitative measure of the position of equilibrium and can be expressed in terms of concentrations or pressures depending on whether the reaction involves gases or solutions. Factors such as concentration, pressure, temperature, and catalysis can influence the position of equilibrium based on Le Chatelier's principle.
This document provides an outline for 8 lessons on chemical kinetics for an IB Chemistry class. It includes objectives, content, and activities for each lesson. Lesson 1 reviews topic 6. Lessons 2-4 cover rate equations, determining rate experimentally, and evaluating reaction mechanisms. Lesson 5 discusses the rate-determining step. Lessons 6-7 focus on the Arrhenius equation and determining activation energy experimentally. Lesson 8 reviews the topic with exam questions. The lessons provide definitions, examples, and practice problems to help students understand reaction rates, orders, rate laws, mechanisms, and the temperature dependence of reaction rates.
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Algorithm to find the composition of air at temperatures 200-9000 K
1. A C++ algorithm for computing
equilibrium chemical composition of air at
temperatures 200-9000 K
A REPORT
by
G R Krishna Chand Avatar
BE (Aerospace Engineering)
Punjab Engineering College, Chandigarh
July 5, 2016
3. Abstract
The chemical composition of air drastically changes at high tempera-
tures, which is triggered mainly due to molecular dissociation of diatomic
nitrogen (N2) and diatomic oxygen (O2). The algorithm presented here at-
tempts to compute the composition of air for the temperature range 200 –
9000 K. The constituents of air are assumed to be primarily N2, O2, O, N
and NO as they are present in substantial amounts for the selected range of
study.
4. Nomenclature
i, j : Indices
ai,j : Interpolating polynomials
bn : Polynomial coefficients
R : Ideal gas constant (8.314 J/mol/K)
ρ : Density of air (kg/m3)
∆G : Gibbs energy function (J/mol)
P0 : Reference pressure (101325 Pa)
T0 : Reference temperature (0 K)
T : Temperature (K)
Go
i : Molar Gibbs energy for ith species (J/mol)
Ho
i : Molar enthalpy for ith species (J/mol)
So
i : Molar entropy for ith species (J/mol/K)
σN : Mole number of nitrogen atoms
σO : Mole number of oxygen atoms
σi : Mole number of ith species
σ : Sum of mole numbers of all species
ν : Stoichiometric coefficients of any species in a chemical reaction
Ki : Equilibrium constant based on mole numbers
Kpi : Equilibrium constant based on partial pressures
tol : Tolerance value
1
5. Chapter 1
Introduction
1.1 Air
Air is a mixture of gases, which at low temperatures are primarily
Nitrogen, Oxygen and small amounts of argon, carbon dioxide and other
gases. Since nitrogen and oxygen form almost all of the air, it is considered
that the former has a presence with 79% and the latter with 21% by moles
at low temperatures. Five chemically reacting species are assumed to be
present in air, viz., N2, N, O, O2 and NO and designed respectively as :
σ1, σ2, σ3, σ4 and σ5.
Three independent chemical reactions are considered involving all the
5 reacting species which are enumerated as :
O2 → 2O (1.1)
N2 + O2 → 2NO (1.2)
N2 → 2N (1.3)
1.2 Equilibrium fundamentals
To determine whether a reaction has reached its state of equilibrium or
not, a parameter known as equilibrium coefficient is defined. This equilib-
rium coefficient, when expressed in terms of partial pressures of the partici-
pating gaseous entities, Kp is more easily computed once the Gibbs standard
energy change for the particular reaction (∆G) is calculated. Both these
terms are related via the expression :
Kpj = e−∆Go
j /RT
for any jth
reaction.
∆Go for any reaction is calculated using the following expression:
∆Go
=
products
νiGi −
reactants
νiGi
2
6. For the reactions in the previous section, ∆Go
j (j = 1,2,3) is given as under;
∆Go
1 = 2Go
3 − Go
4
∆Go
2 = 2Go
5 − Go
1 − Go
4
∆Go
3 = 2Go
2 − Go
1
In order to detemine ∆G, Gibbs free energy with reference to a temperature
0 K has to be computed for each of the five species that have been considered
using a Gibbs energy function, Go(T). Many research organisations, notably
NASA, have curve-fitted the data, using least-squares method, obtained af-
ter performing rigorous experiments using a set of interpolating polynomials
valid for continual temperature ranges. These values for the interpolating
coefficients could be obtained from any reliable source. For our purpose, we
have used the data from "A Rapid Method for the Computation of Equilib-
rium Chemical Composition of Air to 15000 K" - Ramadas K. Prabhu and
Wayne D. Erickson, NASA Technical Paper 2792 published in March 1988.
Gibbs energy function is expressed as:
Go
i
RT
=
Ho
i
RT
−
So
i
R
Ho
i
RT
=
5
j=1
ai,jTj−1
j
+
ai,6
T
So
i
R
= ai,1 log T +
5
j=2
ai,jTj−1
j − 1
+ ai,7
The coefficients ai,6 and ai,7 are the itegration constants. The
values of ai,6 were determined from the enthalpy of formation (taken from
the JANAF Thermochemical Tables published by The Dow Chemical Co.)
for all the species at the reference temperature (T0 = 0 K). The values of
ai,7 were determined from the values of entropy at T = 298.15 K.
3
7. Chapter 2
Governing Equations
2.1 Equilibrium equations
There are three reactions which govern the equilibrium chemical compo-
sition of air at various temperatures. At these temperatures, corresponding
equilibrium constants in terms of the mole numbers, Ki (i=1,2,3) of the
participating species for the three reactions are obtained.
The reactions with their Ki’s are enumerated as:
O2 → 2O; K1 =
σ3
2
σ4
(2.1)
N2 + O2 → 2NO; K2 =
σ5
2
σ1 · σ4
(2.2)
N2 → 2N; K3 =
σ2
2
σ1
(2.3)
As the equilibrium constants are based on mole numbers Ki of the
species, they have to be expressed in terms of equilibrium constants based on
partial pressures of the participating species, Kpi (i=1,2,3). This is because
the latter can be easily expressed as a function of the Gibbs’ free energy
change for each of the reactions as discussed in the introduction.
The two types of equibrium constants are related through an expression as:
Ki = Kpi · (P0/ρRT)∆N
∆N = Nmole numbers of products − Nmole numbers of reactants
2.2 Conservation equations
All the species that are considered here are made of two fundamental
elements, Oxygen and Nitrogen which allows for the formulation of two con-
4
8. servation equations, one each for Oxygen and Nitrogen, as:
2σ4 + σ3 + σ5 = σO (2.4)
2σ1 + σ2 + σ5 = σN (2.5)
One mole of diatomic species, N2 (σ1) and O2 (σ4) contributes two
moles of atoms of their constituent element species. Similarly one mole of
species NO (σ5) contributes one mole of Oxygen atoms and another mole of
Nitrogen atoms.
5
9. Chapter 3
Computational models
For computation of equilibrium chemical composition of air for the tem-
perature range 200–9000 K, three models are adopted for three overlapping
temperature ranges. Every model includes two sets of constituent species,
viz,
1. Major species : Comprises of those species which are predominant
for the temperature range under study
2. Minor species : Enumerates those species whose presence is rela-
tively very low
The regions of applicability of the models,as presented above, strictly
depends upon the value of log ρ alongwith temperature, T. The graph show-
ing the same is presented on the last page of this report. The applicability
(in terms of temperature ranges) of each of the models, as mentioned in its
description, is particularly for the case when ρ = 0.01kg/m3.
3.1 Model 1
This model computes the composition of air in the low temperature range :
200-1600 K (or based on the value of log ρ)
Here the major species are N2 (σ1) and O2 (σ4) and the minor
ones are O (σ3), NO (σ5) and N (σ2).
Procedure:
1. Assume initial values for mole numbers for O2 and N2 as:
σ4 = σO
2 and σ1 = σN
2
2. Compute minor species as:
σ3 = K1σ4 σ2 = K3σ1 σ5 = Keσ2σ3; Ke = K2
K1K3
3. Update the major species as:
σ4 = (σO−σ3−σ5)
2 σ1 = (σN −σ2−σ5)
2
6
10. 4. Iterate the preceding steps until convergence is achieved,i.e.,until
|σ4 − σ4| ≤ tol and |σ1 − σ1| ≤ tol
3.2 Model 2
This model computes the composition of air in the median temperature
range : 1600-6000 K (or based on the value of log ρ)
The major species are N2 (σ1), N (σ2), O (σ3), O2 (σ4) and NO
(σ5).
Procedure:
1. Calculate the initial guess for σ3 using the equations as under:
2σ4 + σ3 + σ5 = σO σ4 =
σ2
3
K1
σ5 = σ3
σN K2
2K1
taking σ1 = σN /2
such that : σ3 =
−
K1
2
(1+
σN K2
2K1
)+
K2
1
4
(1+
σN K2
2K1
)2+2σOK1
2
2. Determine values of bn : n=0,1,2,3,4 as:
b0 = 2K1σ2
O
b1 = (−4 + K3Ke)K1σO
b2 = −8σO + 2K1 + (σO − σN )K2 − K1K3Ke
b3 = 8 − K2 − 2K3Ke
b4 = (8−2K2)
K1
3. Compute ∆σ3 = − F
F
as: F = 4
n=0 bnσn
3 F = 4
n=1 nbnσn−1
3
4. Update σ3 and compute the major species as :
σ3 = σ3 + ∆σ3 σ2 =
σO−2
σ2
3
K1
−σ3
Keσ3
σ5 = Keσ2σ3
σ1 = (σN −σ2−σ5)
2
σ4 = (σO−σ3−σ5)
2
5. Iterate steps 3-4 till convergence for σ3 is achieved,i.e.,
|∆σ3| ≤ tol
3.3 Model 3
This model computes the composition of air in the relatively high tempera-
ture range : 3500-9000 K (or based on the value of log ρ)
The major species are N2 (σ1), N (σ2) and O (σ3); the minor ones
are O2 (σ4) and NO (σ5).
Procedure:
1. Assume σ4 = σ5 = 0. Take σ3 = σO.
7
11. 2. σN = σN − σ5 and solving quadratically for σ2 as :
σ2 =
−K3
2 + (K3
2 )2 + 2K3σN
2
3. Compute major and minor species:
σ1 =
(σN −σ2)
2 σ4 =
σ3
2
K1
σ5 = Keσ3σ2
σ3 = σO − 2σ4 − σ5
4. Take σ3 = σ3
5. Keep on iterating steps 2-4 till the following criterion is met:
|σ3 − σ3| ≤ tol
8
12. Chapter 4
Results
The results are discussed when ρ = 1 ∗ 10−2kg/m3. The level of molec-
ular dissociation for the two species N2 and O2 remains substantially very
low at temperatures in the range of 200–2900 K. Thereafter the molecular
dissociation of O2 gets accelerated with increase in temperature beyond 2900
K. And for the range of 2900–6300 K, N2 and O are predominant. Beyond
6300 K, N2 also starts getting dissociated rapidly and so the predominant
species are N and O. A graph for the same is provided on the the next page.
References
"A Rapid Method for the Computation of Equilibrium Chemical Composition
of Air to 15000 K" - Ramadas K. Prabhu and Wayne D. Erickson, NASA
Technical Paper 2792 published in March 1988.
9
13. Chapter 5
Algorithm Description
The algorithm for the entire computation process is listed as:
1. Input temperature (T) and density of air ρ.
2. Gather curve-fitting coefficients, aij corresponding to the input T.
3. Using the values of aij and T, compute values for Ho
i and So
i and
thereby Go
i for i = 1, 2, 3, 4, 5 or simply all the species.
4. Calculate ∆Go
j ∀ j = 1, 2, 3
5. Compute Kpj using the exponential relation and then Kj ∀ j = 1, 2, 3.
6. Invoke the requisite models as per the value of input temperature, (T).
7. Obtain the values of mole fractions of all the species.
10
16. Figure 5.2: Regions of Applicability of Various models
Reproduced with modification from "A Rapid Method for the Computation
of Equilibrium Chemical Composition of Air to 15000 K" - Ramadas K.
Prabhu and Wayne D. Erickson, NASA Technical Paper 2792
13