1-To know how to calculate Equivalent Weight (eq. wt)
2- To know how to express concentrations in Normality (N)
3- To know how to convert between ppm, ppb and M.
To determine rate exponents experimentally, concentrations of reactants must be changed one at a time to observe how the reaction rate changes. Rate exponents represent the order of the reaction with respect to each reactant and can be determined by running experiments where one concentration is doubled, tripled, or quadrupled and observing the corresponding change in reaction rate. The rate law and rate constant can then be used to predict reaction rates under different conditions.
1. The document outlines the general procedure for solving equilibrium problems which includes: tabulating initial and equilibrium concentrations, calculating concentration changes, using stoichiometry to determine other concentration changes, calculating equilibrium concentrations, and computing the equilibrium constant Keq.
2. It then provides 5 example equilibrium problems to solve using this procedure, involving reactions of ammonia dissolving in water, sulfur trioxide decomposing, calcium chromate dissolving, the Haber process of nitrogen and hydrogen reacting to form ammonia, and a general reaction of reactants A and B forming products C and D.
The document contains a chemistry exam with multiple choice questions about reaction rates and stoichiometry. Question 1 asks about the relationship between the rates of disappearance of H2 and appearance of HF in the reaction H2 + F2 → 2HF. Question 2 asks about the relationship between the average rate of appearance of product B and disappearance of reactant A in the reaction 3A → 2B. Question 3 asks about the order of reactants and overall order of the reaction for the hydrolysis of t-butyliodide.
This document discusses chemical reaction rates. It defines reaction rate as the change in concentration of reactants over time. Reaction rate can be expressed as the decrease in molar concentration of reactants or increase in molar concentration of products over a set period of time. Reaction rate equations are provided for both reactants and products, and the relationships between their rates are shown based on stoichiometric coefficients. Order of reaction and rate constants are also discussed, along with example calculations.
This document contains a practice test for General Chemistry II with 15 multiple choice questions and 5 true/false questions testing concepts related to gases, gas laws, and intermolecular forces. It also includes a bonus section matching chemical names and formulas. The key indicates the correct answers to all questions.
1. Chemical kinetics is the study of time vs. the rate of chemical change. The three factors that affect chemical reactions are concentration, temperature, and catalysts.
2. Instantaneous rate is the slope of a line drawn tangent to the concentration-time curve at a specific time. Beer's Law states that absorption of electromagnetic radiation by a substance is directly proportional to its concentration.
3. A first-order reaction has a rate proportional to the concentration of a single reactant raised to the first power. The rate is equal to k[A] and a plot of ln[A] versus time gives a straight line with a slope of -k.
This document contains 7 questions regarding chemical equilibrium calculations. The questions involve writing equilibrium constants, calculating equilibrium constants based on given partial pressures or concentrations at equilibrium, and determining unknown values at equilibrium given some known values. Specifically, it asks the student to:
1) Write the equilibrium constant expression for a dissolution reaction.
2) Write the equilibrium constant expression for a complex ion formation reaction.
3) Calculate the equilibrium constant for a decomposition reaction given partial pressures at equilibrium.
4) Calculate the equilibrium constant for a decomposition reaction given partial pressures at equilibrium.
5) Calculate the equilibrium constant for a reaction given partial pressures in a container at equilibrium.
6) Calculate unknown concentrations and the equilibrium constant for a reaction given initial
This document provides 13 multiple choice and calculation questions about key concepts in general chemistry including the ideal gas law, density, molar mass, reaction stoichiometry involving gases, and gas behavior. It tests understanding of gas laws, calculations using the ideal gas equation, and properties that affect how real gases deviate from ideal behavior. The final question indicates that an ideal gas is distinguished from real gases by the fact that ideal gas molecules have no attraction for one another.
To determine rate exponents experimentally, concentrations of reactants must be changed one at a time to observe how the reaction rate changes. Rate exponents represent the order of the reaction with respect to each reactant and can be determined by running experiments where one concentration is doubled, tripled, or quadrupled and observing the corresponding change in reaction rate. The rate law and rate constant can then be used to predict reaction rates under different conditions.
1. The document outlines the general procedure for solving equilibrium problems which includes: tabulating initial and equilibrium concentrations, calculating concentration changes, using stoichiometry to determine other concentration changes, calculating equilibrium concentrations, and computing the equilibrium constant Keq.
2. It then provides 5 example equilibrium problems to solve using this procedure, involving reactions of ammonia dissolving in water, sulfur trioxide decomposing, calcium chromate dissolving, the Haber process of nitrogen and hydrogen reacting to form ammonia, and a general reaction of reactants A and B forming products C and D.
The document contains a chemistry exam with multiple choice questions about reaction rates and stoichiometry. Question 1 asks about the relationship between the rates of disappearance of H2 and appearance of HF in the reaction H2 + F2 → 2HF. Question 2 asks about the relationship between the average rate of appearance of product B and disappearance of reactant A in the reaction 3A → 2B. Question 3 asks about the order of reactants and overall order of the reaction for the hydrolysis of t-butyliodide.
This document discusses chemical reaction rates. It defines reaction rate as the change in concentration of reactants over time. Reaction rate can be expressed as the decrease in molar concentration of reactants or increase in molar concentration of products over a set period of time. Reaction rate equations are provided for both reactants and products, and the relationships between their rates are shown based on stoichiometric coefficients. Order of reaction and rate constants are also discussed, along with example calculations.
This document contains a practice test for General Chemistry II with 15 multiple choice questions and 5 true/false questions testing concepts related to gases, gas laws, and intermolecular forces. It also includes a bonus section matching chemical names and formulas. The key indicates the correct answers to all questions.
1. Chemical kinetics is the study of time vs. the rate of chemical change. The three factors that affect chemical reactions are concentration, temperature, and catalysts.
2. Instantaneous rate is the slope of a line drawn tangent to the concentration-time curve at a specific time. Beer's Law states that absorption of electromagnetic radiation by a substance is directly proportional to its concentration.
3. A first-order reaction has a rate proportional to the concentration of a single reactant raised to the first power. The rate is equal to k[A] and a plot of ln[A] versus time gives a straight line with a slope of -k.
This document contains 7 questions regarding chemical equilibrium calculations. The questions involve writing equilibrium constants, calculating equilibrium constants based on given partial pressures or concentrations at equilibrium, and determining unknown values at equilibrium given some known values. Specifically, it asks the student to:
1) Write the equilibrium constant expression for a dissolution reaction.
2) Write the equilibrium constant expression for a complex ion formation reaction.
3) Calculate the equilibrium constant for a decomposition reaction given partial pressures at equilibrium.
4) Calculate the equilibrium constant for a decomposition reaction given partial pressures at equilibrium.
5) Calculate the equilibrium constant for a reaction given partial pressures in a container at equilibrium.
6) Calculate unknown concentrations and the equilibrium constant for a reaction given initial
This document provides 13 multiple choice and calculation questions about key concepts in general chemistry including the ideal gas law, density, molar mass, reaction stoichiometry involving gases, and gas behavior. It tests understanding of gas laws, calculations using the ideal gas equation, and properties that affect how real gases deviate from ideal behavior. The final question indicates that an ideal gas is distinguished from real gases by the fact that ideal gas molecules have no attraction for one another.
The document provides information about key concepts in general chemistry including the definitions of matter, homogeneous mixtures, and pressure. It also summarizes several gas laws including Boyle's law that pressure and volume are inversely proportional at constant temperature and amount, Charles' law that volume is directly proportional to temperature at constant pressure and amount, and Avogadro's law relating volume and amount of gas particles. Sample problems are provided to demonstrate how to use the gas laws and equations of state to calculate pressure, volume, temperature and amount in gas systems.
To determine the rate exponent of a reaction, experiments are conducted where the concentration of one reactant is varied while keeping other concentrations constant. This allows observation of how the reaction rate changes and determines the order of the reaction with respect to that reactant. For a second order reaction, doubling the concentration of a reactant will quadruple the reaction rate.
The document defines standard enthalpy of formation (ΔHf°) as the amount of heat absorbed or released when one mole of a substance is formed from its elements in their standard states at 25°C and 100kPa. ΔHf° values are used to calculate the enthalpy change (ΔH°) of a chemical reaction. Examples are provided to demonstrate how to determine the ΔHf° of a compound from combustion reactions and how to calculate ΔH° from the ΔHf° values of reactants and products.
This document discusses acids, bases, and pH. It defines acids as substances that produce hydrogen ions in water and bases as substances that produce hydroxide ions. pH is defined as the negative base-10 logarithm of the hydronium ion concentration and is a measure of acidity, with values below 7 indicating acidic solutions and above 7 indicating basic solutions. The autoionization of water is described by the ion product constant Kw, which relates the concentrations of hydronium and hydroxide ions in solution.
This document discusses solubility equilibria and the formation of precipitates. It defines key terms like solubility product constant (Ksp), explains how to calculate Ksp values from molar solubility and vice versa, and shows examples of using Ksp to determine whether precipitates will form when solutions are mixed. The key points are that solubility is dependent on equilibrium, saturated solutions have concentrations where Ksp = Q, and precipitates form when mixing produces Q > Ksp (supersaturation).
Composite Carbonic Acid and Carbonate Kineticsaqion
There are two types of carbonic acid: true carbonic acid (H2CO3) and composite carbonic acid (H2CO3*). True carbonic acid involves the direct reaction of CO2 and H2O, while composite carbonic acid treats CO2(aq) and H2CO3 as a single entity. Each acid has its own equilibrium constant (Ktrue and K1). K1 is around 500 times smaller than Ktrue due to the inclusion of dissolved CO2 in the composite definition. The reaction kinetics between the three species (CO2(aq), H2CO3, HCO3-) were also described, noting that the direct reaction between CO2 and H2O is much slower than
This document contains examples of chemical kinetics problems involving determination of rate laws, rate constants, orders of reactions, and activation energies from experimental data. Several questions ask the reader to identify reaction intermediates and rate-determining steps based on given reaction mechanisms and rate laws. The document demonstrates how kinetic concepts can be applied to analyze reaction rates and mechanisms.
1) The document discusses open and closed carbon dioxide (CO2) systems and how they differ in their behavior under acid/base titration.
2) In a closed CO2 system, the total dissolved inorganic carbon (DIC) remains constant during titration. But in an open CO2 system, the CO2 partial pressure remains constant and DIC increases exponentially with increasing pH.
3) Graphs of speciation versus pH show that in a closed system, carbonate species shift between each other to conserve DIC, while in an open system each species increases independently without conservation of DIC.
1. The document discusses key concepts from general chemistry including:
- The van der Waals equation accounting for non-zero particle volumes and interparticle interactions.
- Using the ideal gas law to calculate changes in volume with temperature changes.
- The value of the gas constant R at standard temperature and pressure.
- Conversions between various pressure and volume units.
- Calculating moles, pressure, volume, and number of molecules using the ideal gas law.
Derivation of mathematical closed-from equations for multiprotic acids, which allow the calculation of titration curves and buffer intensities (with Excel). Examples are given for acetic acid, carbonic acid, phosphoric acid, and citric acid.
The reaction of A + B will proceed faster than the reaction of A + B + C because:
- Reactions requiring more particles to collide simultaneously have lower probabilities of a successful reaction occurring.
- The overall rate of a reaction is determined by the slowest elementary step. So if one step is slower than the others, it will be the rate determining step and limit the overall reaction rate.
- Catalysts increase the rate of reactions by reducing the activation energy of steps, but are not used up in the reaction. They can also change the reaction mechanism.
Mathematical description of an acid-base system using the tableaux method (including proton balance and mole balance). Equivalence points for carbonic acid are calculated.
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.
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.
This document discusses chemical equilibrium, including:
- The concept of equilibrium and how it applies to both physical and chemical processes.
- How to write expressions for the equilibrium constant (K) and what K represents in terms of reactant and product concentrations/pressures.
- Factors that can influence chemical equilibrium according to Le Chatelier's principle, including changes in concentration, pressure/volume, temperature, and adding a catalyst.
- Examples of using K expressions to calculate equilibrium concentrations and predict the direction reactions will shift to reestablish equilibrium when conditions change.
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.
The concept of equivalence points (EP) runs like a golden thread through acid-base theory and applications. There are different types of equivalence points. This article provides a classification of EPs and semi-EPs. This is done for the general case of N-protic acids (based on simple mathematical equations).
This document discusses measurement units including the SI units, mass and weight, volume, and temperature scales. It provides information on the seven SI basic units, converting between units, derived units, common volume units like liters and milliliters, and temperature scales like Celsius, Kelvin and Fahrenheit. Examples are given for converting between units of length, mass, volume, density and temperature. The goal is for the reader to understand fundamental measurement units and conversions between unit systems.
This document contains calculations of the standard enthalpy change (ΔH°rxn) for several chemical reactions. For each reaction, ΔH°rxn is calculated using the formula ΔH°rxn = ΔH°products - ΔH°reactants. The standard enthalpy of formation values (ΔH°f) of the reactants and products are used to determine if the reaction is exothermic or endothermic. It is found that all the reactions presented are exothermic, with negative ΔH°rxn values ranging from -65.2 kJ/mol to -1124.0 kJ/mol.
Irrazábal instó a implementar Mercado Consignatario de Yerba MateEconomis
El senador Juan Manuel Irrazábal (Frente para la Victoria, Misiones) reclamó la puesta en funcionamiento del Mercado Consignatario de la Yerba Mate y la sanción del Fondo Especial Yerbatero.
The document provides information about key concepts in general chemistry including the definitions of matter, homogeneous mixtures, and pressure. It also summarizes several gas laws including Boyle's law that pressure and volume are inversely proportional at constant temperature and amount, Charles' law that volume is directly proportional to temperature at constant pressure and amount, and Avogadro's law relating volume and amount of gas particles. Sample problems are provided to demonstrate how to use the gas laws and equations of state to calculate pressure, volume, temperature and amount in gas systems.
To determine the rate exponent of a reaction, experiments are conducted where the concentration of one reactant is varied while keeping other concentrations constant. This allows observation of how the reaction rate changes and determines the order of the reaction with respect to that reactant. For a second order reaction, doubling the concentration of a reactant will quadruple the reaction rate.
The document defines standard enthalpy of formation (ΔHf°) as the amount of heat absorbed or released when one mole of a substance is formed from its elements in their standard states at 25°C and 100kPa. ΔHf° values are used to calculate the enthalpy change (ΔH°) of a chemical reaction. Examples are provided to demonstrate how to determine the ΔHf° of a compound from combustion reactions and how to calculate ΔH° from the ΔHf° values of reactants and products.
This document discusses acids, bases, and pH. It defines acids as substances that produce hydrogen ions in water and bases as substances that produce hydroxide ions. pH is defined as the negative base-10 logarithm of the hydronium ion concentration and is a measure of acidity, with values below 7 indicating acidic solutions and above 7 indicating basic solutions. The autoionization of water is described by the ion product constant Kw, which relates the concentrations of hydronium and hydroxide ions in solution.
This document discusses solubility equilibria and the formation of precipitates. It defines key terms like solubility product constant (Ksp), explains how to calculate Ksp values from molar solubility and vice versa, and shows examples of using Ksp to determine whether precipitates will form when solutions are mixed. The key points are that solubility is dependent on equilibrium, saturated solutions have concentrations where Ksp = Q, and precipitates form when mixing produces Q > Ksp (supersaturation).
Composite Carbonic Acid and Carbonate Kineticsaqion
There are two types of carbonic acid: true carbonic acid (H2CO3) and composite carbonic acid (H2CO3*). True carbonic acid involves the direct reaction of CO2 and H2O, while composite carbonic acid treats CO2(aq) and H2CO3 as a single entity. Each acid has its own equilibrium constant (Ktrue and K1). K1 is around 500 times smaller than Ktrue due to the inclusion of dissolved CO2 in the composite definition. The reaction kinetics between the three species (CO2(aq), H2CO3, HCO3-) were also described, noting that the direct reaction between CO2 and H2O is much slower than
This document contains examples of chemical kinetics problems involving determination of rate laws, rate constants, orders of reactions, and activation energies from experimental data. Several questions ask the reader to identify reaction intermediates and rate-determining steps based on given reaction mechanisms and rate laws. The document demonstrates how kinetic concepts can be applied to analyze reaction rates and mechanisms.
1) The document discusses open and closed carbon dioxide (CO2) systems and how they differ in their behavior under acid/base titration.
2) In a closed CO2 system, the total dissolved inorganic carbon (DIC) remains constant during titration. But in an open CO2 system, the CO2 partial pressure remains constant and DIC increases exponentially with increasing pH.
3) Graphs of speciation versus pH show that in a closed system, carbonate species shift between each other to conserve DIC, while in an open system each species increases independently without conservation of DIC.
1. The document discusses key concepts from general chemistry including:
- The van der Waals equation accounting for non-zero particle volumes and interparticle interactions.
- Using the ideal gas law to calculate changes in volume with temperature changes.
- The value of the gas constant R at standard temperature and pressure.
- Conversions between various pressure and volume units.
- Calculating moles, pressure, volume, and number of molecules using the ideal gas law.
Derivation of mathematical closed-from equations for multiprotic acids, which allow the calculation of titration curves and buffer intensities (with Excel). Examples are given for acetic acid, carbonic acid, phosphoric acid, and citric acid.
The reaction of A + B will proceed faster than the reaction of A + B + C because:
- Reactions requiring more particles to collide simultaneously have lower probabilities of a successful reaction occurring.
- The overall rate of a reaction is determined by the slowest elementary step. So if one step is slower than the others, it will be the rate determining step and limit the overall reaction rate.
- Catalysts increase the rate of reactions by reducing the activation energy of steps, but are not used up in the reaction. They can also change the reaction mechanism.
Mathematical description of an acid-base system using the tableaux method (including proton balance and mole balance). Equivalence points for carbonic acid are calculated.
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.
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.
This document discusses chemical equilibrium, including:
- The concept of equilibrium and how it applies to both physical and chemical processes.
- How to write expressions for the equilibrium constant (K) and what K represents in terms of reactant and product concentrations/pressures.
- Factors that can influence chemical equilibrium according to Le Chatelier's principle, including changes in concentration, pressure/volume, temperature, and adding a catalyst.
- Examples of using K expressions to calculate equilibrium concentrations and predict the direction reactions will shift to reestablish equilibrium when conditions change.
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.
The concept of equivalence points (EP) runs like a golden thread through acid-base theory and applications. There are different types of equivalence points. This article provides a classification of EPs and semi-EPs. This is done for the general case of N-protic acids (based on simple mathematical equations).
This document discusses measurement units including the SI units, mass and weight, volume, and temperature scales. It provides information on the seven SI basic units, converting between units, derived units, common volume units like liters and milliliters, and temperature scales like Celsius, Kelvin and Fahrenheit. Examples are given for converting between units of length, mass, volume, density and temperature. The goal is for the reader to understand fundamental measurement units and conversions between unit systems.
This document contains calculations of the standard enthalpy change (ΔH°rxn) for several chemical reactions. For each reaction, ΔH°rxn is calculated using the formula ΔH°rxn = ΔH°products - ΔH°reactants. The standard enthalpy of formation values (ΔH°f) of the reactants and products are used to determine if the reaction is exothermic or endothermic. It is found that all the reactions presented are exothermic, with negative ΔH°rxn values ranging from -65.2 kJ/mol to -1124.0 kJ/mol.
Irrazábal instó a implementar Mercado Consignatario de Yerba MateEconomis
El senador Juan Manuel Irrazábal (Frente para la Victoria, Misiones) reclamó la puesta en funcionamiento del Mercado Consignatario de la Yerba Mate y la sanción del Fondo Especial Yerbatero.
This document discusses using high ionicity ionic liquids (HIILs) based on 1-ethyl-3-methylimidazolium ethyl sulphate for separating ethanol from n-heptane mixtures. Three HIILs were prepared with different amounts of ammonium thiocyanate added to increase ionicity. Liquid-liquid equilibria experiments were conducted on ternary mixtures of n-heptane, ethanol, and each HIIL. The HIILs were able to break the azeotrope and their selectivity and distribution coefficients were correlated to ionicity. Compared to the neat ionic liquid, the HIILs showed improved extraction performance due to their higher ion
Shamira, de 15 años, se va a casar pronto con un hombre que no conoce. Ella quiere ser profesora pero en su sociedad las mujeres no deciden su futuro. Su padre Saïd ve su sufrimiento y decide salvarla de un matrimonio forzado dándole la dote para que elija su propio camino y ayude a otras mujeres.
Este documento resume las diferencias entre la psicología clínica y otras profesiones relacionadas con la salud mental. Explica que la psicología clínica se enfoca en evaluar y tratar diversos problemas mentales a través de la evaluación psicológica y la psicoterapia. Aunque trabaja de forma multidisciplinaria con otros profesionales como psiquiatras, trabajadores sociales y enfermeras, se delinean las diferencias en sus enfoques y áreas de trabajo. El documento concluye que la psicología clínica of
El documento describe las herramientas tecnológicas y sus efectos en los estudiantes. Define las herramientas tecnológicas como programas y aplicaciones que facilitan el trabajo y el intercambio de información. Explica que estas herramientas ayudan a los estudiantes a estructurar conocimientos, mejorar exposiciones y fomentar cambios metodológicos. También motivan a los estudiantes, desarrollan su iniciativa y permiten aprendizajes significativos. Finalmente, destaca ventajas como la involuc
Este documento trata sobre los orígenes y evolución de los conceptos de autoritarismo y totalitarismo. Explica que el término "autoridad" proviene del latín "auctoritas" y se refería originalmente a la cualidad de alguien que se hacía merecedor de respeto a través de la experiencia y las virtudes. Luego define autoritarismo como los regímenes que privilegian el mando sobre el consenso e ideológicamente niegan la igualdad y enfatizan la jerarquía. Finalmente, explica el origen del término
Este estudo de caso avaliou o impacto da realização de desejos em crianças com cancro, dividindo-as em grupos de intervenção e controle. A avaliação mostrou que o grupo de intervenção experimentou mais emoções positivas e esperança devido à distração proporcionada pela realização do desejo.
Software Relacionado con la Contratacion AdministrativaFERNANDA CAMPO
El Portal Único de Contratación en Colombia concentra información sobre licitaciones del sector público, ofreciendo datos básicos de todas las entidades estatales. Los usuarios pueden acceder a detalles de los procesos a través de enlaces a los portales de cada entidad. Los bancos de datos jurídicos son bases de datos en línea u offline que contienen normas, jurisprudencia y doctrina con herramientas de búsqueda para encontrar información de forma rápida. Los bancos de datos ofrecen información de calidad actualizada y permit
Erwin Schrödinger was an Austrian physicist who formulated the wave equation and developed quantum theory. He is known for proposing Schrödinger's cat, a thought experiment where a cat is placed in a box with a radioactive particle that has a 50% chance of decaying within an hour, meaning the cat is both alive and dead simultaneously until the box is opened.
O documento discute os seguintes tópicos sobre democracia: 1) democracia formal teórica; 2) democracia real prática; 3) democracia ao avesso na América Latina e Brasil; 4) democracia do futuro como um processo em constante transformação e abertura.
Calculo y graficas de las fuerzas de la competencia (oferta y demanda).Abraham Barbosa
Este documento explica los conceptos básicos de oferta, demanda y precio de equilibrio. Muestra cómo calcular la curva de oferta y demanda a partir de datos de precios y cantidades, y cómo determinar el punto de equilibrio donde ambas curvas se interceptan. También explica cómo calcular la elasticidad de la oferta y la demanda usando fórmulas que comparan los cambios porcentuales en precios y cantidades, y lo que esto indica sobre la elasticidad del mercado.
Este documento presenta el código de ética de la Clínica Chía S.A., el cual establece que el respeto debe ser la base fundamental de las acciones de la institución y su personal hacia los pacientes, sus familias y la comunidad, y enfatiza la importancia de la coherencia entre los pensamientos, palabras y acciones para lograr ser una IPS amiga de sus usuarios.
Leancamp is an unconference, an open space on topic of lean product development, lean startup, lean UX. Leancamp Brussels was the first edition of Leancamp in Belgium.
1) El documento discute las controversias en el tratamiento de la fiebre y el choque séptico, incluyendo si el control de la temperatura con antipiréticos o medios físicos es beneficioso o perjudicial.
2) La fiebre puede ser provocada por numerosos estímulos e implica la producción de citocinas pirógenas, aunque también tiene efectos metabólicos dañinos.
3) Si bien la fiebre puede mejorar la respuesta inmune y suprimir el crecimiento bacteriano, en pacientes cardiópat
1. The document provides a chemistry practice problems document (DPP) containing multiple choice questions.
2. The DPP covers topics such as chemical equilibrium, equilibrium constants, reaction stoichiometry, and thermochemistry.
3. The document includes the answer key for the 10 questions in DPP No. 15 and the 10 questions in DPP No. 14, providing the correct option for each multiple choice question.
This document provides an overview of some basic concepts in chemistry. It defines matter as anything that has mass and occupies space, and describes the three common states of matter as solids, liquids, and gases. It then discusses the characteristics of these different states, and introduces concepts like homogeneous and heterogeneous mixtures, pure substances, and the international system of units used in chemistry. Finally, it summarizes some important laws of chemical combination like the law of conservation of mass and Dalton's atomic theory.
The document discusses chemical reactions involving combustion. It provides information on:
1) Common fuels like gasoline, diesel, and natural gas and their chemical formulas.
2) How nitrogen and moisture are generally not reactive but affect combustion by absorbing heat and changing dew points.
3) The concepts of air-fuel ratio, stoichiometric combustion, theoretical combustion, and causes of incomplete combustion.
4) Examples of combustion calculations involving finding products and their masses and mole fractions.
The document discusses nuclear magnetic resonance (NMR) spectroscopy, specifically proton (1H) and carbon-13 (13C) NMR. It provides information on why NMR is used, the types of information it can provide about compounds, and the physical properties of 1H and 13C nuclei that influence their NMR spectra. It also discusses factors that affect chemical shifts, common chemical shift ranges, coupling behaviors, and how to determine the number of signals expected for given compounds from their carbon environments. The document aims to explain the fundamentals and applications of 1H and 13C NMR spectroscopy.
The document discusses reaction kinetics and reaction rates. It defines reaction rate as the change in concentration of a reactant or product with time. Reaction rates can be determined from graphs of concentration versus time or from differential rate equations. Differential rate equations relate the rates of changes of concentrations of reactants and products. Several examples show how to write differential rate equations for reactions and calculate reaction rates from given information. Common student mistakes in working with differential rate equations are also discussed.
Incremento de capacidad de biorreactores convencionales por la implementación de un anillos con superficie para formación de biofilm con microorganismos.
This Presentation Clarifying about potable Water analysis and their methods which i gave training on operation and maintenance team for Oman Al Ghubrah Independence Water Project (SWRO Desalination 42 MIGD)
Laws of Chemical Combination and Balancing Chemical Equation.pptxAdikpe2
The verification of each of the following chemical laws was well established with examples to simplify it.
THE LAW OF CONSERVATION OF MASS
This Law was established by Lavoisier, a French Chemist. This law states that matter is neither created nor destroyed during chemical reaction but changes from one form to another. This means that in a chemical reaction, the total mass of all reacting substances (i.e. the reactants) is equal to the total mass of the products.
THE LAW OF DEFINITE PROPORTIONS OR CONSTANT COMPOSITION
This Law was proposed by Proust (1755-1826). The Law of Definite Proportions states that all pure samples of a particular chemical compound contain similar elements combined in the same proportion by mass.
THE LAW OF MULTIPLE PROPORTIONS
The law of Multiple Proportions states that if two elements, A and B, combine to form more than one chemical compound, the various masses of one element, A which combine separately with a fixed mass of the other element, B, are in simple multiple ratios.
BALANCING CHEMICAL EQUATION WITH CALCULATION
A chemical equation is a shorthand expression for a chemical change or reaction. It shows among other things the arrangement of atoms that are involved in the reaction.
When balancing an equation, you must remember the following:
Know the reacting substances and the products formed.
Know the chemical formulae for all the substances.
Write, in front of the formulae, coefficients that will balance the equation.
Common gases, such as oxygen, hydrogen, chlorine and nitrogen, in the free state, are diatomic, e.g. O2, H2, Cl2 and N2
Other elements in the free state, such as sodium, potassium, copper and iron, are represented by their atomic symbols, e.g. Na, K, Cu and Fe.
This document contains information about a physical chemistry course for petroleum engineering students. It includes the course contents which cover topics like stoichiometry, gases, kinetics, spontaneity criteria, and phase diagrams. It describes the assessments and passing requirements. Additionally, it provides examples of stoichiometry calculations and explains concepts like limiting reagents and percent yields in chemical reactions.
1. Calculate the enthalpy change for the reaction P4O6 (s) + 2 O2 (g) → P4O10 (s) using given enthalpy values for related reactions.
2. Calculate the standard enthalpy of reaction (ΔH°) for several reactions using standard enthalpies of formation from appendix C.
3. Calculate the standard enthalpy of formation of gaseous diborane (B2H6) using thermochemical cycles and given reaction enthalpies.
4. Explain the meaning of "fuel value" and determine whether 5 g of fat or 9 g of carbohydrates provides more energy as food using their fuel
The document describes a scientific study that compares two different chemical oxygen demand (COD) test kits. Standard COD solutions and wastewater samples were tested using a COD kit containing mercury and a mercury-free kit. The results from both kits were analyzed statistically by examining the mean and standard deviation of the data. The study aimed to cross-validate the two kits by comparing the analyzed data. The results showed that the kits produce the same measurements for COD standard solutions, but do not overlap well when measuring wastewater samples.
The document discusses chemical reactions and stoichiometry. It defines chemical reactions as processes where substances are changed into new substances. Reactants are the original substances, and products are the new substances formed. The document covers types of chemical reactions like combustion and replacement reactions. It also discusses balancing chemical equations, mole ratios, and using mole-mole calculations to solve stoichiometry problems involving masses of reactants and products. An example uses a balanced equation to determine the mass of CO2 produced given the mass of CH4 consumed.
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How to Add Chatter in the odoo 17 ERP ModuleCeline George
In Odoo, the chatter is like a chat tool that helps you work together on records. You can leave notes and track things, making it easier to talk with your team and partners. Inside chatter, all communication history, activity, and changes will be displayed.
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How to Make a Field Mandatory in Odoo 17Celine George
In Odoo, making a field required can be done through both Python code and XML views. When you set the required attribute to True in Python code, it makes the field required across all views where it's used. Conversely, when you set the required attribute in XML views, it makes the field required only in the context of that particular view.
Reimagining Your Library Space: How to Increase the Vibes in Your Library No ...Diana Rendina
Librarians are leading the way in creating future-ready citizens – now we need to update our spaces to match. In this session, attendees will get inspiration for transforming their library spaces. You’ll learn how to survey students and patrons, create a focus group, and use design thinking to brainstorm ideas for your space. We’ll discuss budget friendly ways to change your space as well as how to find funding. No matter where you’re at, you’ll find ideas for reimagining your space in this session.
LAND USE LAND COVER AND NDVI OF MIRZAPUR DISTRICT, UPRAHUL
This Dissertation explores the particular circumstances of Mirzapur, a region located in the
core of India. Mirzapur, with its varied terrains and abundant biodiversity, offers an optimal
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advanced technologies such as GIS (Geographic Information Systems) and Remote sensing to
analyze the transformations that have taken place over the course of a decade.
The complex relationship between human activities and the environment has been the focus
of extensive research and worry. As the global community grapples with swift urbanization,
population expansion, and economic progress, the effects on natural ecosystems are becoming
more evident. A crucial element of this impact is the alteration of vegetation cover, which plays a
significant role in maintaining the ecological equilibrium of our planet.Land serves as the foundation for all human activities and provides the necessary materials for
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land.
The utilization of land is impacted by human needs and environmental factors. In countries
like India, rapid population growth and the emphasis on extensive resource exploitation can lead
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Therefore, human intervention has significantly influenced land use patterns over many
centuries, evolving its structure over time and space. In the present era, these changes have
accelerated due to factors such as agriculture and urbanization. Information regarding land use and
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Accurate understanding of land use and cover is imperative for the development planning
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changes, conversion trends, and other related patterns. The spatial dimensions of land use and
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Remote Sensing and Geographic Information Systems
9
Changes in vegetation cover refer to variations in the distribution, composition, and overall
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How to Manage Your Lost Opportunities in Odoo 17 CRMCeline George
Odoo 17 CRM allows us to track why we lose sales opportunities with "Lost Reasons." This helps analyze our sales process and identify areas for improvement. Here's how to configure lost reasons in Odoo 17 CRM
Leveraging Generative AI to Drive Nonprofit InnovationTechSoup
In this webinar, participants learned how to utilize Generative AI to streamline operations and elevate member engagement. Amazon Web Service experts provided a customer specific use cases and dived into low/no-code tools that are quick and easy to deploy through Amazon Web Service (AWS.)
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This slide is special for master students (MIBS & MIFB) in UUM. Also useful for readers who are interested in the topic of contemporary Islamic banking.
Chapter wise All Notes of First year Basic Civil Engineering.pptxDenish Jangid
Chapter wise All Notes of First year Basic Civil Engineering
Syllabus
Chapter-1
Introduction to objective, scope and outcome the subject
Chapter 2
Introduction: Scope and Specialization of Civil Engineering, Role of civil Engineer in Society, Impact of infrastructural development on economy of country.
Chapter 3
Surveying: Object Principles & Types of Surveying; Site Plans, Plans & Maps; Scales & Unit of different Measurements.
Linear Measurements: Instruments used. Linear Measurement by Tape, Ranging out Survey Lines and overcoming Obstructions; Measurements on sloping ground; Tape corrections, conventional symbols. Angular Measurements: Instruments used; Introduction to Compass Surveying, Bearings and Longitude & Latitude of a Line, Introduction to total station.
Levelling: Instrument used Object of levelling, Methods of levelling in brief, and Contour maps.
Chapter 4
Buildings: Selection of site for Buildings, Layout of Building Plan, Types of buildings, Plinth area, carpet area, floor space index, Introduction to building byelaws, concept of sun light & ventilation. Components of Buildings & their functions, Basic concept of R.C.C., Introduction to types of foundation
Chapter 5
Transportation: Introduction to Transportation Engineering; Traffic and Road Safety: Types and Characteristics of Various Modes of Transportation; Various Road Traffic Signs, Causes of Accidents and Road Safety Measures.
Chapter 6
Environmental Engineering: Environmental Pollution, Environmental Acts and Regulations, Functional Concepts of Ecology, Basics of Species, Biodiversity, Ecosystem, Hydrological Cycle; Chemical Cycles: Carbon, Nitrogen & Phosphorus; Energy Flow in Ecosystems.
Water Pollution: Water Quality standards, Introduction to Treatment & Disposal of Waste Water. Reuse and Saving of Water, Rain Water Harvesting. Solid Waste Management: Classification of Solid Waste, Collection, Transportation and Disposal of Solid. Recycling of Solid Waste: Energy Recovery, Sanitary Landfill, On-Site Sanitation. Air & Noise Pollution: Primary and Secondary air pollutants, Harmful effects of Air Pollution, Control of Air Pollution. . Noise Pollution Harmful Effects of noise pollution, control of noise pollution, Global warming & Climate Change, Ozone depletion, Greenhouse effect
Text Books:
1. Palancharmy, Basic Civil Engineering, McGraw Hill publishers.
2. Satheesh Gopi, Basic Civil Engineering, Pearson Publishers.
3. Ketki Rangwala Dalal, Essentials of Civil Engineering, Charotar Publishing House.
4. BCP, Surveying volume 1
1. Lecture (4)
(242 Chem)
College of Sciences
Department of Chemistry
Level: 4th
Semester BSc
Quantitative analysis-1
Dr Brima Monday 01/02//2016---22/4/1437 1
King Khalid University
Dr Eid Ibrahim Brima
2. 1-To know how to calculate Equivalent Weight (eq. wt)
2- To know how to express concentrations in Normality (N)
3- To know how to convert between ppm, ppb and M.
learning objectives
Dr Brima Monday 01/02//2016---22/4/1437 2
3. 3
Expressing concentration in Normality (N)-1
i. Equivalent Weight (eq wt):
Where: R = number of Reactive Units
a. For acids and bases:
R = no of replaceable H+
or OH-
ions
e.g. H2SO4 ; CaOH2
Mw
R
eq wt =
Dr Brima Monday 01/02//2016---22/4/1437
4. 4
i. Equivalent Weight (eq wt):
a. For acids and bases:
● Example:
For HCl R = 1
For H2SO4 R = 2 (Unless otherwise prescribed)
For H3PO4 R = 3 (Unless otherwise prescribed)
For CH3COOHR = 1
Expressing concentration in Normality (N)-2
Dr Brima Monday 01/02//2016---22/4/1437
5. 5
i. Equivalent Weight (eq wt):
a. For acids and bases:
● Example:
For NaOH R = 1
For Cu(OH)2 R = 2
For Al(OH)3 R = 3
Expressing concentration in Normality (N)-3
Dr Brima Monday 01/02//2016---
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6. 6
i. Equivalent Weight (eq wt):
b. In Reduction – Oxidation (Redox)
reactions:
R = no of electrons transferred
(gained or lost)
● Ex.: MnO4
-
+ 8 H+
+ 5 e-
Mn2+
+ 4 H2O
∴ R = 5
Expressing concentration in Normality (N)-4
Dr Brima Monday 01/02//2016---22/4/1437
7. 7
i. Equivalent Weight (eq wt):
c. For Salts:
R = Total no of +ve or -ve charges
on the cation or the anion of the salt
● Example:
For Na+
Cl-
R = 1
For Na2
2+
CO3
2-
R = 2
Expressing concentration in Normality (N)-5
Dr Brima Monday 01/02//2016---22/4/1437
8. 8
ii. Gram equivalent weight (g eq wt):
It is the equivalent weight expressed in
grams
● Example:
eq wt of Na2CO3 = Mw / 2 = 106 / 2 = 53
∴1 g eq wt for Na2CO3 = 53 g
Expressing concentration in Normality (N)-6
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9. 9
iii. Number of g eq wt’s:
● Example: How many g eq wt’s are in 106 g of
Na2CO3 (MW = 106)?
- eq wt of Na2CO3 = MW / 2 = 106 / 2 = 53
∴ No of g eq wt’s = 106 / 53 = 2
No of g eq wt =
wt of substance
its eq wt
Expressing concentration in Normality (N)-7
Dr Brima Monday 01/02//2016---
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10. 10
iv. Normality (N):
It is the number of g eq wt’s per one liter
of solution
∴ N x VL = wt of solute / its eq wt
No of g eq wt’s of solute
sol.n Volume in Liters
=
wt / eq wt
VL
∴ N =
Expressing concentration in Normality (N)-8
Dr Brima Monday 01/02//2016---
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11. Dr Brima Monday 01/02//2016---22/4/1437 11
Normality calculation-1
- *Calculate the normality for 0.212g of Na2CO3
dissolved in 100ml water?
- Answer:
[212mg/(106/2)]/100ml = 0.04N
[0.212g/(106/2)]/0.1L = 0.04N
No of g eq wt’s of solute
sol.n Volume in Liters
=
wt / eq wt
VL
∴ N =
83
12. Dr Brima Monday 01/02//2016---22/4/1437 12
Normality calculation-2
- *Calculate the normality for 0.25g/L of Oxalic
acid (H C O₂ ₂ 4) dissolved in 100ml water?
- Answer:
- N = wt(mg)/[Mwt/R]/Vml
= 250mg/[290.4/2]/1000ml = 0.006N
—84-85
13. 13
Relations between ppm, ppb and M
- To convert M to ppm:
∴ ppm = M x MW x 1000
- To convert ppm to M:
∴ M = ppm / (MW x 1000)
- To convert M to ppb:
∴ ppb = M x MW x 106
- To convert ppb to M:
∴ M = ppb / (MW x 106
)
Dr Brima Monday 01/02//2016---
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14. Lecture Summary
• Eq.Wt. :
• Number of g eq wt’s:
• Normality (N):
Dr Brima Monday 01/02//2016---
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14
Mw
R
eq wt =
No of g eq wt’s of solute
Soln. Volume in Liters
=
wt / eq wt
VL
N =
N x VL = wt of solute / its eq wt
No of g eq wt =
wt of substance
its eq wt