Unit cells describe the repeating arrangements of atoms or molecules in crystalline solids. A unit cell contains the smallest group of particles that can be repeated to form the entire crystal structure. Common unit cell types include cubic, hexagonal, and body-centered cubic, with the specific arrangement depending on the bonding and packing of particles within the solid material.
The document discusses key concepts about gases from the kinetic molecular theory and gas laws. It introduces gases in the atmosphere and how they were studied historically. It then covers gas pressure, units of pressure, Boyle's law, Charles' law, Avogadro's law, the ideal gas law, gas stoichiometry, Dalton's law of partial pressures, and the kinetic molecular theory of gases. Examples are provided to demonstrate calculations using these gas laws and concepts.
1. The document describes properties of gases and gas laws, including Boyle's law, Charles' law, the combined gas law, Gay-Lussac's law, Avogadro's law, and Dalton's law of partial pressures.
2. It defines key terms like pressure, temperature, volume, moles, and ideal gas equation.
3. The three main gas laws - Boyle's law, Charles' law, and Avogadro's law - are combined into the ideal gas equation: PV=nRT.
Gases have no definite volume and assume the volume of any vessel. The behavior of gases is described by gas laws including Boyle's law, Charles' law, Avogadro's law, and the ideal gas law. Real gases deviate from ideal behavior at high pressures and low temperatures and are better described by equations like van der Waals. Key gas properties include gas formation volume factor, gas compressibility factor, gas viscosity, and gas solubility in oil. Gas formation volume factor relates the volume of gas at reservoir conditions to standard surface conditions.
Here are the densities of the gases at STP:
Hydrogen: 0.0899 g/L or 0.0899 g/m3
Oxygen: 1.429 g/L or 1.429 g/m3
Chlorine: 3.214 g/L or 3.214 g/m3
Radon: 9.73 g/L or 9.73 g/m3
The van der Waals gas model takes into account intermolecular interactions that the ideal gas model neglects. It explains the liquid-gas phase transition through a critical point, where the vapor and liquid phases become indistinguishable. The model approximates molecules as rigid spheres that experience short-range repulsion and long-range attraction. It derives an equation of state relating pressure, volume, and temperature. This equation reduces to the ideal gas law under conditions of high temperature or low density.
Gas is one of the three forms of matter. Every known substance is either a solid, liquid or a gas. These forms differ in the way they fill space and change shape. A gas, such as air has neither a fixed shape nor a fixed volume and has weight.
The document discusses the characteristics and properties of gases. It defines the gaseous state as the state where intermolecular forces are at a minimum. Some key characteristics of gases include having low density, high compressibility, diffusibility, and filling their container uniformly. The document also discusses various gas laws including Boyle's law, Charles' law, Gay-Lussac's law, Avogadro's law, and the ideal gas equation. It provides the mathematical relationships and graphical representations for each gas law.
The document discusses key concepts about gases from the kinetic molecular theory and gas laws. It introduces gases in the atmosphere and how they were studied historically. It then covers gas pressure, units of pressure, Boyle's law, Charles' law, Avogadro's law, the ideal gas law, gas stoichiometry, Dalton's law of partial pressures, and the kinetic molecular theory of gases. Examples are provided to demonstrate calculations using these gas laws and concepts.
1. The document describes properties of gases and gas laws, including Boyle's law, Charles' law, the combined gas law, Gay-Lussac's law, Avogadro's law, and Dalton's law of partial pressures.
2. It defines key terms like pressure, temperature, volume, moles, and ideal gas equation.
3. The three main gas laws - Boyle's law, Charles' law, and Avogadro's law - are combined into the ideal gas equation: PV=nRT.
Gases have no definite volume and assume the volume of any vessel. The behavior of gases is described by gas laws including Boyle's law, Charles' law, Avogadro's law, and the ideal gas law. Real gases deviate from ideal behavior at high pressures and low temperatures and are better described by equations like van der Waals. Key gas properties include gas formation volume factor, gas compressibility factor, gas viscosity, and gas solubility in oil. Gas formation volume factor relates the volume of gas at reservoir conditions to standard surface conditions.
Here are the densities of the gases at STP:
Hydrogen: 0.0899 g/L or 0.0899 g/m3
Oxygen: 1.429 g/L or 1.429 g/m3
Chlorine: 3.214 g/L or 3.214 g/m3
Radon: 9.73 g/L or 9.73 g/m3
The van der Waals gas model takes into account intermolecular interactions that the ideal gas model neglects. It explains the liquid-gas phase transition through a critical point, where the vapor and liquid phases become indistinguishable. The model approximates molecules as rigid spheres that experience short-range repulsion and long-range attraction. It derives an equation of state relating pressure, volume, and temperature. This equation reduces to the ideal gas law under conditions of high temperature or low density.
Gas is one of the three forms of matter. Every known substance is either a solid, liquid or a gas. These forms differ in the way they fill space and change shape. A gas, such as air has neither a fixed shape nor a fixed volume and has weight.
The document discusses the characteristics and properties of gases. It defines the gaseous state as the state where intermolecular forces are at a minimum. Some key characteristics of gases include having low density, high compressibility, diffusibility, and filling their container uniformly. The document also discusses various gas laws including Boyle's law, Charles' law, Gay-Lussac's law, Avogadro's law, and the ideal gas equation. It provides the mathematical relationships and graphical representations for each gas law.
Properties of gases: gas laws, ideal gas equation, dalton’s law of partial pressure, diffusion of gases, kinetic theory of gases, mean free path, deviation from ideal gas behavior, vander wails equation, critical constants, liquefaction of gases, determination of molecular weights, law of corresponding states and heat capacity
The statistical mechanical derivation of the van der waals equation of stateUNICAMP
The document provides a statistical mechanical derivation of the van der Waals equation of state and its associated thermodynamic properties. Some key points:
- It accounts for finite molecular size and intermolecular attractive forces in the van der Waals fluid model.
- Expressions are derived for various thermodynamic properties like pressure, internal energy, heat capacities in terms of temperature and molar volume.
- Conditions for vapor-liquid equilibrium are obtained by setting the Gibbs free energy of vaporization to zero and equating chemical potentials.
1) Pressure is defined as force per unit area. The greater the force on a given area, the greater the pressure.
2) Gas pressure is caused by collisions of gas molecules with each other and surfaces. The pressure exerted by a gas depends on its volume, temperature, and number of molecules.
3) Boyle's law, Charles' law, and Gay-Lussac's law describe the relationships between pressure, volume, and temperature for an ideal gas. Boyle's law states that pressure and volume are inversely proportional at constant temperature. Charles' law states that volume and temperature are directly proportional at constant pressure. Gay-Lussac's law states that pressure and temperature are directly proportional at constant
This document provides an overview of key concepts relating to gases, including:
- Characteristics of gases such as expanding to fill their container and being highly compressible.
- Definitions and units used to measure gas pressure, such as pascals, bars, mmHg, and atmospheres.
- Laws describing the behavior of gases, including Boyle's law, Charles's law, Avogadro's law, Dalton's law of partial pressures, and the ideal gas equation.
- The kinetic molecular theory which models the behavior of gas particles at the molecular level.
1. The document summarizes key concepts from chemistry chapter 12 on gas laws, including Boyle's law relating pressure and volume at constant temperature, Charles' law relating temperature and volume at constant pressure, and Dalton's law of partial pressures.
2. Boyle's law states that the volume of a gas is inversely proportional to its pressure when temperature is kept constant. Charles' law specifies that the volume of a gas is directly proportional to its temperature when pressure remains constant.
3. Dalton's law of partial pressures states that in a mixture of gases, the total pressure is equal to the sum of the partial pressures of the individual gases.
Deviation of real gas from ideal behaviourvidyakvr
Real gases deviate from ideal gas behavior at high pressures and low temperatures due to the assumptions of negligible molecular volume and no intermolecular forces being incorrect in those conditions. Van der Waals proposed an equation to account for these deviations that includes pressure and volume correction terms related to intermolecular attractive forces and molecular size. The compressibility factor Z, which is the ratio of PV to nRT, can quantify this deviation from ideal behavior for real gases as it equals 1 for ideal gases but varies from 1 for real gases.
This document provides an overview of the kinetic theory of gases. It outlines the assumptions of the kinetic theory, including that gas molecules move randomly and collide elastically. It also describes how kinetic theory can be used to derive the pressure exerted by an ideal gas. Specifically, it shows that the average force on the walls of a container is proportional to the average kinetic energy of the gas molecules colliding with the walls. Additionally, it defines key terms like root mean square speed and relates these concepts to the equation of state for an ideal gas.
The document discusses the three states of matter - solid, liquid, and gas. It focuses on the gaseous state and properties of gases. Some key points:
- Gases have molecules that are separated by large distances and move freely and independently of each other.
- Many substances can exist as gases under normal conditions, including elements like hydrogen, nitrogen, oxygen as well as compounds like carbon dioxide and ammonia.
- Gases exert pressure uniformly on all surfaces. Gas pressure is measured using instruments like barometers and manometers.
- The behavior of gases is described by gas laws including Boyle's law, Charles' law, Avogadro's law, and the ideal gas equation.
Gases are highly compressible and expand to fill their containers, with pressure inversely proportional to volume according to Boyle's Law. The properties and behavior of gases can be explained by the kinetic molecular theory, which models gases as large numbers of molecules in random motion. Real gases deviate from ideal gas behavior at high pressures and low temperatures due to intermolecular forces and molecular volumes.
The document discusses real gases and how they deviate from ideal gas behavior. It introduces the virial equation as a way to model real gases over a wider range of pressures and temperatures compared to the ideal gas law. The virial equation treats the deviation of real gases from ideality as a power series in terms of the molar volume. It also discusses how the second virial coefficient, which accounts for intermolecular forces, varies with temperature and exhibits a minimum value at the Boyle temperature for some gases like hydrogen and helium. Finally, it introduces the van der Waals equation as a simplified model compared to the virial equation that treats real gas behavior using just two constants related to molecular size and attraction.
The document discusses the properties and characteristics of gases. It describes gases as being fluids that have low density due to large distances between particles, allowing them to flow freely and expand to fill their containers. The document also defines pressure as force per unit area and discusses different units used to measure pressure, including pascals, atmospheres, torr, mmHg, and psi. It notes that average air pressure at sea level is 760 mmHg or 1 atmosphere.
I. Gases assume the shape and volume of their container, are highly compressible, and mix evenly when confined together. They have lower densities than liquids or solids.
II. Gases were the first state of matter studied in detail. Their behavior can be described by simple mathematical equations that generally apply over certain temperature and pressure ranges. The study of gases provided evidence that matter is composed of particles rather than being continuous.
III. The measurable properties of gases are mass (moles), pressure, volume, and temperature (which must be in Kelvin). Various gas laws describe the relationships between these properties, and the ideal gas law combines these individual laws into one equation.
1. The document discusses the kinetic theory of gases and the gas laws. It explains that gas pressure is due to particle collisions with the container walls and increases with temperature as the particle speed and collision rate increases.
2. The gas laws of Boyle, Charles, and Gay-Lussac are summarized. Boyle's law states that at constant temperature, pressure and volume are inversely related. Charles' law specifies that at constant pressure, volume and temperature are directly related. Gay-Lussac's law indicates that at constant volume, pressure and temperature are directly related.
3. Experiments are described that verify each gas law through varying one property while holding the others constant. Graphs illustrate the mathematical relationships between pressure
The document discusses concepts from the kinetic theory of gases including:
1. The assumptions of the kinetic theory and that gas pressure arises from molecular collisions with container walls.
2. Equations are derived relating pressure, temperature, volume, number of moles and the gas constant for ideal gases.
3. The gas laws of Boyle, Charles and Avogadro are proven from kinetic theory assumptions.
4. Dalton's law of partial pressures is proven, stating that the total pressure of a gas mixture equals the sum of the partial pressures of its components.
5. The mean free path is defined as the average distance traveled between molecular collisions.
Dalton's law of partial pressure states that total pressure of the mixture of inert gases is equal to the sum of partial pressures of each gas present in the mixture.
1. Boyle's law states that the volume of a gas is inversely proportional to its pressure when temperature is kept constant.
2. Charles's law describes the direct relationship between volume and temperature in a gas at constant pressure.
3. According to Gay-Lussac's law, the pressure of a gas rises directly with temperature if volume remains fixed.
4. Avogadro's law explains that equal volumes of gases under identical conditions of temperature and pressure contain equal numbers of molecules.
Chemistry - Chp 14 - The Behavior of Gases - Study GuideMr. Walajtys
This document provides a study guide for a test on gas laws and behavior of gases. It lists key concepts to know about gas properties and equations, including how changing temperature, pressure, or volume affects gas pressure. It also provides example problems applying gas laws and concepts like the combined gas law, ideal gas laws, Dalton's law of partial pressures, and Graham's law for gas diffusion rates. Students are expected to know gas laws, how to convert between Celsius and Kelvin, and how to set up and solve problems related to gas behavior.
An ideal gas is a theoretical gas that follows Boyle's, Charles's, and the ideal gas laws. It is made of particles with negligible volume that exhibit random motion and no intermolecular forces. Real gases deviate from ideal behavior at low temperatures or high pressures due to intermolecular forces or particle volume. The ideal gas law relates pressure, volume, amount of gas, and temperature as PV=nRT.
Cuándo ocurrirá el rapto de la iglesiaZaida Flores
Este documento discute tres posiciones diferentes sobre el Rapto de la Iglesia. La primera es que el Rapto ocurrirá después de la Gran Tribulación y los cristianos sufrirán. La segunda es que no habrá ni Rapto ni Gran Tribulación. La tercera posición, defendida por el autor, es que el Rapto ocurrirá antes de la Gran Tribulación para evitar que los cristianos sufran la ira de Dios destinada a los impíos.
Dokumen tersebut membahas tentang perilaku berbelanja berlebihan (gila berbelanja) dan cara-cara mengatasinya. Dokumen tersebut menyajikan grafik tentang kecenderungan berbelanja setiap kenaikan pendapatan di beberapa negara, diikuti definisi gila berbelanja, sebab-sebab, faktor penyumbang, kesan-kesannya, dan cara mengatasinya seperti mengubah tingkah laku, berjimat cermat, dan melakuk
Properties of gases: gas laws, ideal gas equation, dalton’s law of partial pressure, diffusion of gases, kinetic theory of gases, mean free path, deviation from ideal gas behavior, vander wails equation, critical constants, liquefaction of gases, determination of molecular weights, law of corresponding states and heat capacity
The statistical mechanical derivation of the van der waals equation of stateUNICAMP
The document provides a statistical mechanical derivation of the van der Waals equation of state and its associated thermodynamic properties. Some key points:
- It accounts for finite molecular size and intermolecular attractive forces in the van der Waals fluid model.
- Expressions are derived for various thermodynamic properties like pressure, internal energy, heat capacities in terms of temperature and molar volume.
- Conditions for vapor-liquid equilibrium are obtained by setting the Gibbs free energy of vaporization to zero and equating chemical potentials.
1) Pressure is defined as force per unit area. The greater the force on a given area, the greater the pressure.
2) Gas pressure is caused by collisions of gas molecules with each other and surfaces. The pressure exerted by a gas depends on its volume, temperature, and number of molecules.
3) Boyle's law, Charles' law, and Gay-Lussac's law describe the relationships between pressure, volume, and temperature for an ideal gas. Boyle's law states that pressure and volume are inversely proportional at constant temperature. Charles' law states that volume and temperature are directly proportional at constant pressure. Gay-Lussac's law states that pressure and temperature are directly proportional at constant
This document provides an overview of key concepts relating to gases, including:
- Characteristics of gases such as expanding to fill their container and being highly compressible.
- Definitions and units used to measure gas pressure, such as pascals, bars, mmHg, and atmospheres.
- Laws describing the behavior of gases, including Boyle's law, Charles's law, Avogadro's law, Dalton's law of partial pressures, and the ideal gas equation.
- The kinetic molecular theory which models the behavior of gas particles at the molecular level.
1. The document summarizes key concepts from chemistry chapter 12 on gas laws, including Boyle's law relating pressure and volume at constant temperature, Charles' law relating temperature and volume at constant pressure, and Dalton's law of partial pressures.
2. Boyle's law states that the volume of a gas is inversely proportional to its pressure when temperature is kept constant. Charles' law specifies that the volume of a gas is directly proportional to its temperature when pressure remains constant.
3. Dalton's law of partial pressures states that in a mixture of gases, the total pressure is equal to the sum of the partial pressures of the individual gases.
Deviation of real gas from ideal behaviourvidyakvr
Real gases deviate from ideal gas behavior at high pressures and low temperatures due to the assumptions of negligible molecular volume and no intermolecular forces being incorrect in those conditions. Van der Waals proposed an equation to account for these deviations that includes pressure and volume correction terms related to intermolecular attractive forces and molecular size. The compressibility factor Z, which is the ratio of PV to nRT, can quantify this deviation from ideal behavior for real gases as it equals 1 for ideal gases but varies from 1 for real gases.
This document provides an overview of the kinetic theory of gases. It outlines the assumptions of the kinetic theory, including that gas molecules move randomly and collide elastically. It also describes how kinetic theory can be used to derive the pressure exerted by an ideal gas. Specifically, it shows that the average force on the walls of a container is proportional to the average kinetic energy of the gas molecules colliding with the walls. Additionally, it defines key terms like root mean square speed and relates these concepts to the equation of state for an ideal gas.
The document discusses the three states of matter - solid, liquid, and gas. It focuses on the gaseous state and properties of gases. Some key points:
- Gases have molecules that are separated by large distances and move freely and independently of each other.
- Many substances can exist as gases under normal conditions, including elements like hydrogen, nitrogen, oxygen as well as compounds like carbon dioxide and ammonia.
- Gases exert pressure uniformly on all surfaces. Gas pressure is measured using instruments like barometers and manometers.
- The behavior of gases is described by gas laws including Boyle's law, Charles' law, Avogadro's law, and the ideal gas equation.
Gases are highly compressible and expand to fill their containers, with pressure inversely proportional to volume according to Boyle's Law. The properties and behavior of gases can be explained by the kinetic molecular theory, which models gases as large numbers of molecules in random motion. Real gases deviate from ideal gas behavior at high pressures and low temperatures due to intermolecular forces and molecular volumes.
The document discusses real gases and how they deviate from ideal gas behavior. It introduces the virial equation as a way to model real gases over a wider range of pressures and temperatures compared to the ideal gas law. The virial equation treats the deviation of real gases from ideality as a power series in terms of the molar volume. It also discusses how the second virial coefficient, which accounts for intermolecular forces, varies with temperature and exhibits a minimum value at the Boyle temperature for some gases like hydrogen and helium. Finally, it introduces the van der Waals equation as a simplified model compared to the virial equation that treats real gas behavior using just two constants related to molecular size and attraction.
The document discusses the properties and characteristics of gases. It describes gases as being fluids that have low density due to large distances between particles, allowing them to flow freely and expand to fill their containers. The document also defines pressure as force per unit area and discusses different units used to measure pressure, including pascals, atmospheres, torr, mmHg, and psi. It notes that average air pressure at sea level is 760 mmHg or 1 atmosphere.
I. Gases assume the shape and volume of their container, are highly compressible, and mix evenly when confined together. They have lower densities than liquids or solids.
II. Gases were the first state of matter studied in detail. Their behavior can be described by simple mathematical equations that generally apply over certain temperature and pressure ranges. The study of gases provided evidence that matter is composed of particles rather than being continuous.
III. The measurable properties of gases are mass (moles), pressure, volume, and temperature (which must be in Kelvin). Various gas laws describe the relationships between these properties, and the ideal gas law combines these individual laws into one equation.
1. The document discusses the kinetic theory of gases and the gas laws. It explains that gas pressure is due to particle collisions with the container walls and increases with temperature as the particle speed and collision rate increases.
2. The gas laws of Boyle, Charles, and Gay-Lussac are summarized. Boyle's law states that at constant temperature, pressure and volume are inversely related. Charles' law specifies that at constant pressure, volume and temperature are directly related. Gay-Lussac's law indicates that at constant volume, pressure and temperature are directly related.
3. Experiments are described that verify each gas law through varying one property while holding the others constant. Graphs illustrate the mathematical relationships between pressure
The document discusses concepts from the kinetic theory of gases including:
1. The assumptions of the kinetic theory and that gas pressure arises from molecular collisions with container walls.
2. Equations are derived relating pressure, temperature, volume, number of moles and the gas constant for ideal gases.
3. The gas laws of Boyle, Charles and Avogadro are proven from kinetic theory assumptions.
4. Dalton's law of partial pressures is proven, stating that the total pressure of a gas mixture equals the sum of the partial pressures of its components.
5. The mean free path is defined as the average distance traveled between molecular collisions.
Dalton's law of partial pressure states that total pressure of the mixture of inert gases is equal to the sum of partial pressures of each gas present in the mixture.
1. Boyle's law states that the volume of a gas is inversely proportional to its pressure when temperature is kept constant.
2. Charles's law describes the direct relationship between volume and temperature in a gas at constant pressure.
3. According to Gay-Lussac's law, the pressure of a gas rises directly with temperature if volume remains fixed.
4. Avogadro's law explains that equal volumes of gases under identical conditions of temperature and pressure contain equal numbers of molecules.
Chemistry - Chp 14 - The Behavior of Gases - Study GuideMr. Walajtys
This document provides a study guide for a test on gas laws and behavior of gases. It lists key concepts to know about gas properties and equations, including how changing temperature, pressure, or volume affects gas pressure. It also provides example problems applying gas laws and concepts like the combined gas law, ideal gas laws, Dalton's law of partial pressures, and Graham's law for gas diffusion rates. Students are expected to know gas laws, how to convert between Celsius and Kelvin, and how to set up and solve problems related to gas behavior.
An ideal gas is a theoretical gas that follows Boyle's, Charles's, and the ideal gas laws. It is made of particles with negligible volume that exhibit random motion and no intermolecular forces. Real gases deviate from ideal behavior at low temperatures or high pressures due to intermolecular forces or particle volume. The ideal gas law relates pressure, volume, amount of gas, and temperature as PV=nRT.
Cuándo ocurrirá el rapto de la iglesiaZaida Flores
Este documento discute tres posiciones diferentes sobre el Rapto de la Iglesia. La primera es que el Rapto ocurrirá después de la Gran Tribulación y los cristianos sufrirán. La segunda es que no habrá ni Rapto ni Gran Tribulación. La tercera posición, defendida por el autor, es que el Rapto ocurrirá antes de la Gran Tribulación para evitar que los cristianos sufran la ira de Dios destinada a los impíos.
Dokumen tersebut membahas tentang perilaku berbelanja berlebihan (gila berbelanja) dan cara-cara mengatasinya. Dokumen tersebut menyajikan grafik tentang kecenderungan berbelanja setiap kenaikan pendapatan di beberapa negara, diikuti definisi gila berbelanja, sebab-sebab, faktor penyumbang, kesan-kesannya, dan cara mengatasinya seperti mengubah tingkah laku, berjimat cermat, dan melakuk
The document discusses making an independent British film called "Tortured" that would challenge stereotypes by having a young black female lead. An independent production company like the fictional Clockwork Productions would be better than a large multi-national company for this film, as it would allow full creative freedom and breaking conventions, whereas a major company may be hesitant to greenlight a film that does not feature a "normal" lead according to societal standards.
The document discusses editing the process of a new poster. It likely outlines the steps involved in editing and finalizing the design of the poster before it is printed and distributed. The editing process is being done to ensure the poster clearly and effectively conveys its intended message or information to viewers.
This document provides information on various aspects of Spanish grammar including:
1) The future tense and how it is used to express future actions. Verb endings in the future tense are the same for both regular and irregular verbs.
2) The conditional tense and how it is used to express hypothetical or possible actions. Common irregular verbs in the conditional are also listed.
3) The present perfect tense and how it is formed using the present tense of haber and a past participle. Examples of irregular past participles are provided.
4) Relative pronouns such as que, el/la que, and quienes and how they are used to connect sentences.
The document discusses how to effectively design advertisements to promote music albums and artists. Through research, the author found that ads need to catch audience attention by relating to the artist's style and showcasing the album in a recognizable way. Ads also aim to create brand recognition for the artist using matching fonts, colors, and making the artist's name stand out, all with the goal of selling more albums and increasing the artist's popularity.
The document discusses the benefits of exercise for mental health. Regular physical activity can help reduce anxiety and depression and improve mood and cognitive function. Exercise causes chemical changes in the brain that may help protect against mental illness and improve symptoms.
The document discusses the benefits of exercise for mental health. Regular physical activity can help reduce anxiety and depression and improve mood and cognitive functioning. Exercise causes chemical changes in the brain that may help protect against mental illness and improve symptoms.
Dokumen tersebut membahas tentang kebutuhan sistem, use case model, actor, use case, relasi antar use case, dan use case diagram. Secara ringkas, dokumen tersebut menjelaskan bahwa use case diagram digunakan untuk menggambarkan fungsionalitas sistem berdasarkan interaksi antara actor dengan use case, serta hubungan antar komponen yang ada dalam diagram tersebut.
Life is full of wonders that can be captured through cinematography. Filmmakers are able to showcase the beauty in the world and tell impactful stories through the art of cinematography. Movies allow audiences to experience life's wonders from new perspectives.
1. Sistem operasi mengelola perangkat fisik dan menyajikan abstraksi mesin virtual untuk aplikasi.
2. Untuk hardisk, sistem operasi menyediakan dua abstraksi: perangkat raw dan sistem berkas.
3. Sistem operasi menangani removable media seperti hardisk tetapi tape ditampilkan sebagai perangkat penyimpanan mentah.
The document discusses gas laws and the ideal gas law. It defines an ideal gas as having perfectly elastic collisions between molecules with no intermolecular forces. The ideal gas law relates pressure, volume, amount of gas, and temperature. It also discusses:
- Constant volume heat capacity (CV) which is the heat required to change temperature with constant volume
- Constant pressure heat capacity (CP) which is the heat required to change temperature with constant pressure
- Derivations of Boyle's law (inverse relationship between pressure and volume at constant temperature) and Charles' law (direct relationship between volume and temperature at constant pressure) from the ideal gas law
- Heat capacities of monoatomic and diatomic ideal gases depend only on
The document discusses the key characteristics and behaviors of gases. It introduces several gas laws including Boyle's law relating pressure and volume, Charles's law relating temperature and volume, Avogadro's law relating amount and volume, and Dalton's law of partial pressures. It derives the ideal gas equation and shows how it can be used to calculate gas properties like density from variables like molar mass, pressure, temperature.
1. Gases have no definite shape or volume but take the shape of their container. Gas particles are in constant random motion and collide with each other and the container walls.
2. The kinetic molecular theory provides an explanation for gas behavior at the molecular level. It states that gas particles are in constant random motion and exert pressure due to collisions with container walls.
3. The gas laws describe the macroscopic behavior of gases through relationships between pressure, volume, temperature, and amount of gas. The kinetic molecular theory qualitatively explains the gas laws based on gas particle motion and interactions.
1. Gases have certain physical properties according to the kinetic molecular theory including occupying the shape and volume of their container, being highly compressible, and mixing evenly.
2. The gas laws describe the relationships between pressure, volume, temperature, and amount of gas including Boyle's law, Charles' law, Avogadro's law, and the combined ideal gas law.
3. Real gases deviate from ideal behavior at high pressures as described by the van der Waals equation.
The document discusses the three states of matter - solid, liquid, and gas. It explains the properties of gases and how gas particles are in constant random motion. The gas laws including Boyle's law, Charles' law, Avogadro's law, and the ideal gas equation are described. It also covers gas pressure, measurement of pressure using barometers and manometers, gas density calculations, and sample problems involving the gas laws.
The document summarizes several gas laws:
- Boyle's law relates the inverse relationship between gas volume and pressure at constant temperature
- Charles' law describes how gas volume increases with temperature at constant pressure
- Gay-Lussac's law explains how gas pressure rises with increasing temperature at constant volume
- Combined gas law incorporates changes in pressure, volume, and temperature for a fixed amount of gas
- Dalton's law of partial pressures states that the total pressure of a gas mixture equals the sum of the individual gas pressures
1. The document discusses gas laws, including Boyle's law relating volume and pressure at constant temperature, and Charles' law relating volume and temperature at constant pressure.
2. It provides examples of using the gas laws to calculate volume or pressure changes given initial and final conditions.
3. The kinetic molecular theory is described as explaining the gas laws based on the random motion and elastic collisions of gas molecules.
Charles' law describes how gas volume changes with temperature. It states that the volume of a gas is directly proportional to its temperature when pressure is kept constant. The document provides the formula for Charles' law and shows examples of using it to calculate unknown volumes or temperatures given other variables like initial and final volumes and temperatures. It also discusses the limitations of Charles' law and provides sample problems and solutions demonstrating how to apply the law to calculate unknown values.
This document discusses the behavior of gases through summarizing the kinetic molecular theory and gas laws. It describes five assumptions of the kinetic theory, including that gas particles are in constant random motion and collisions are perfectly elastic. It then discusses how temperature, pressure, volume, and number of moles are related for a gas based on the gas laws of Boyle, Charles, Gay-Lussac, combined, and ideal gases. It provides examples of using the gas laws to solve problems involving changes in pressure, volume, temperature, or number of moles of a gas.
The document summarizes the kinetic molecular theory and gas laws. It explains that kinetic molecular theory models gases as particles in constant, random motion that exert pressure during collisions. It describes the gas laws of Boyle's law, Charles' law, Gay-Lussac's law, Avogadro's hypothesis, and Dalton's law of partial pressures which relate the variables of pressure, volume, temperature, and moles of gas. Examples are provided to illustrate applications of the gas laws.
This chapter discusses the key concepts and gas laws relating to gases:
1) Boyle's law states that at a constant temperature, the pressure and volume of a gas are inversely proportional.
2) Charles' law describes the direct relationship between volume and temperature of a gas at constant pressure.
3) Avogadro's law relates the volume and amount of gas present at constant pressure and temperature.
4) The ideal gas law combines these relationships between pressure, volume, temperature, and amount of gas.
5) Dalton's law of partial pressures describes how the total pressure of a gas mixture is equal to the sum of the individual gas partial pressures.
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.
This document summarizes several gas laws including Boyle's law, Charles' law, Avogadro's law, the combined gas law, and the ideal gas law. Boyle's law states that for a fixed amount of gas at constant temperature, the volume is inversely proportional to the pressure. Charles' law states that for a fixed amount of gas at constant pressure, the volume is directly proportional to the temperature. Avogadro's law states that equal volumes of gases at the same temperature and pressure contain equal numbers of molecules. The combined gas law incorporates Boyle's, Charles's and Avogadro's laws. The ideal gas law relates the pressure, volume, quantity, and temperature of an ideal gas using the formula
Gases are highly compressible and expand to fill their containers, with pressure inversely proportional to volume according to Boyle's Law. The properties and behavior of gases can be explained by the kinetic molecular theory, which models gases as large numbers of molecules in random motion. Real gases deviate from ideal gas behavior at high pressures and low temperatures due to intermolecular forces and molecular volumes.
This document provides an overview of key concepts related to gases, including:
- Characteristics of gases and units of pressure like atmospheres and torr
- Gas laws like Boyle's, Charles', and Avogadro's laws and how they relate to the ideal gas equation
- How to calculate variables like pressure, volume, moles, and temperature using the ideal gas equation
- Kinetic molecular theory and how it explains gas behavior and properties
- Deviations from ideal gas behavior at high pressures or low temperatures
- The van der Waals equation for correcting for non-ideal behavior
The document discusses properties of gases and gas laws. It begins by explaining the importance of gases in airbags and sodium azide. It then covers the three states of matter and general gas properties including having free space, expanding infinitely, filling containers uniformly, and diffusing rapidly. Key gas laws are also summarized, including Boyle's law relating pressure and volume inversely, Charles' law relating volume and temperature directly, and Gay-Lussac's law relating pressure and temperature directly. The combined gas law and ideal gas law PV=nRT are also presented.
The document discusses the kinetic molecular theory of gases and properties of gases. Some key points:
1) Gases are composed of molecules that are in constant random motion and interact through perfectly elastic collisions. The average kinetic energy is proportional to temperature.
2) Gas pressure is caused by molecular collisions with container walls. Pressure increases with higher temperature or lower volume based on the gas laws.
3) The kinetic molecular theory explains gas properties and laws such as Boyle's, Charles', Avogadro's, and Dalton's through consideration of molecular motion and collisions.
4) Gas density, pressure, volume, temperature, and amount relationships can be described using the ideal gas law. Real gases deviate from
1) Gases expand to fill their containers, are highly compressible, and have low densities due to the large distances between molecules. Their physical properties are similar regardless of chemical properties.
2) Pressure is caused by molecular collisions with surfaces. It increases with more frequent or forceful collisions. Temperature increases collision frequency and force. Pressure also rises with increased amount or decreased volume of gas.
3) Kinetic molecular theory explains gas behavior by modeling gases as particles in random motion, where temperature corresponds to average kinetic energy. This enables understanding of gas laws and pressure in terms of molecular collisions.
Chemistry - Chp 14 - The Behavior of Gases - PowerPointMel Anthony Pepito
Gases are easily compressed and expanded to fill their container due to the large spaces between their particles. The three main factors that affect gas pressure are the amount of gas, the volume of the container, and the temperature. The relationships between these factors are described by Boyle's law, Charles's law, Gay-Lussac's law, and the combined gas law. Real gases approximate ideal gas behavior at high temperatures or low pressures when intermolecular forces and molecular volume can be ignored.
Chemistry - Chp 14 - The Behavior of Gases - PowerPoint
States of matter
1.
2.
3.
4. Review
What’s matter?
What are the three common
states of matter?
1) Solids
2) Liquids
3) Gases
What can the states also be called? Phases
So, a phase describes a physical state of matter.
5.
6. Comparison of States
gas liquid solid
Do not have Take the shape Definite shape
SHAPE
definite shape of the container
in which it is
poured
lots of free little free space little free space
DENSITY space between between between
particles particles particles
FLOW particles can particles can rigid - particles
move past one move/slide past cannot
another one another move/slide past
one another
7. THREE GAS LAWS
BOYLE’SLAW :
RELATE PRESSURE WITH VOLUME
CHARLES’ LAW
RELATE VOLUME WITH TEMPERATURE
GAY LUSSAC’S LAW
RELATE PRESSURE WITH TEMPERATURE
8. Robert Boyle (1627-1691)
• Boyle had the good fortune to have Robert Hooke as
an assistant and together they made an air pump.
In 1662, Boyle published what is
now known as Boyle's law:
At constant temperature the volume of a gas is
inversely proportional to the pressure
9. Boyle’s Law :
The volume of definite quantity of gas is inversely
proportional to it’s pressure at constant temperature.
Mathematically expressed as V ∝ 1 (Constant temp.)
P
∴ V = K/P where K = constant
∴ PV = K
Thus it can also be stated as
“At constant temperature the product of volume and
pressure of definite quantity of gas is constant.
If P1 and V1 is initial pressure and volume of gas at
constant temp and P2, V2 at final state then above equation
can be written as :
P1V1 = P2V2
13. Jacques Charles
In the century
following Boyle, a
French physicist,
Jacques Charles
(1746-1823), was
the first person
to fill a balloon
with hydrogen
gas and who
made the first
solo balloon
14. Volume vs. Temperature:
Charles’ Law
• Notice the linear
relationship. This
relationship between
temperature and
volume describes a
“direct relationship”.
This means when
temperature
increases, so does
the volume.
15. Charles' Law :
• ‘The volume of definite quantity of gas is directly
proportional to its absolute temperature at
constant pressure.’
• Mathematically expressed as
V ∝ T (constant pressure)
V = KT (K = constant)
V/T = K
• If V1 and T1 are the volume and temperature of gas
in initial state and V2, T2 at final state then above
equation can be written as :
V1 = V2 or V1 = T1
16. GAY LUSACC LAW
“At constant volume the pressure of the given
quantity 0f the gas is directly proportional to
it’s absolute temperature”.
Mathematically expressed as
P ∝ T (constant pressure)
P = KT (K = constant)
P/T = K
If P1 and T1 are the volume and temperature
of gas in initial state and P2, T2 at final state
then above equation can be written as :
P1 = P2 or P1 = T1
T1 T2 P2 T2
17. Mechanics of
Breathing
Timberlake, Chemistry 7th Edition, page 254
18. Simple gas equation P1 VI T I P2 V 2 T 2
P2 V X T 2
HereV T step –volume isVx T instep – 2 stepsP V T
P1 change in 1 P2 done two
1 1 1 2 2 2
In first step, according to Boyle’s Law
P1V1 = P2Vx (constant temp)
∴Vx = P1V1
P2
In second step, according to Charle’s Law
Vx = V2 ∴ Vx = V2T1
T1 T2 T2
On combining both above steps,
P1V1 = V2T1 ∴P1V1 = P2V2
19. COMBINED GAS EQUATION
P1V1 = P2 V2 .
T1 T2
In simple form combined gas equation can be written as
PV = K (constant)
T
∴ PV = KT
Value of constant K depends on quantity of gas
Here putting K = nR KαV;Vα
where n = quantity of gas in mole n
R = gas constant (does not depend on quantity of
Kαn
gas)
∴ PV = nRT
Above equation is called simple gas equation
20. Derive the value of R
According to Ideal gas equation : PV =
nRT
∴ R = PV = pressure x volume
nT no. of moles x temp.
force x volume
=
area
______________
no. of moles x temp.
force x (length)3
=
(length)2
___________
no. of moles x temp.
= force x length__________
21. • But, force x length = work energy
∴R = work energy________
no. of moles x temp.
• Thus unit of R is work energy/Kelvin mole.
• It is proved by experiment that volume of one mole
of any gas at 0°C and 1 atm pressure is 22.4 litre.
22. It is proved by experiment that volume of one mole of
any gas at 0°C and 1 atm pressure is 22.4 litre
According to simple gas equation
R = PV/nT
where P = 1 atm n = 1 mole
V = 22.4 litre T = 0°C = 273 Kelvin
∴ R = 1 atm x 22.4 litre
1 mole x 273 Kelvin
R = 0.082 litre atm/Kelvin mole
23. Value of gas constant R in
different unit
Value Unit
0.082 litre – atm / Kelvin mole } work
1.987 calorie/Kelvin mole in heat
1.987 x 10-3 Kcal / Kelvin mole energy
8.314 x 107 erg / Kelvin mole (CGS)
8.314 joule / Kelvin mole (MKS)
24. Standard temperature and pressure :
• The temperature of 0°C or 273
Kelvin and pressure of 1 atmosphere
or 760 mm is called standard temp.
and pressure.
25. Dalton’s Law of Partial Pressure :
The pressure of gaseous mixture is sum of partial
pressure of each component gas’.
Suppose A and B are the gases filled in two
different vessel of same size and kept at same
temperature.
Let PA = partial pressure of a gm of gas A
PB = partial pressure of b gm of gas B
If both this gas are filled in the third container of
same volume and kept at same temperature then
total pressure of gases, according to Dalton law of
partial pressure would be.
PTotal = PA + PB.
Here gas A and gas B donot react with each other.
27. Application :
• For the gases collected over water, the total
pressure of the gas is equal to partial pressure of
dry gas as well as partial pressure of water
vapour.
• Eg : For oxygen gas collected over water, acc. to
Dalton’s law
• PTotal = Pgas + PH2O Here Pgas = PO2
∀ ∴PO2 = PTotal – PH2O
where PTotal = pressure of gases
PH2O = vapour pressure of water at 25°C
• When volume percentage composition is given,
then
partial pressure of gas P,
•
= Percentage of volume x total pressure
100
28. Graham’s law of gaseous difusion
Graham in 1928 presented a relation between diffusion
rate of gas and its density in the name of Graham’s law
of diffusion of gases.
‘The rate of diffusion of various gases at same conditions
of temperature and pressure is inversely proportional to
the square root of their densities.’
Suppose the density of any gas is (d) and its rate of
diffusion is (r) then,
r α 1/ d
The diffusion rate of two gases are compared after
carrying out the experiment at same temperature and
pressure.
29. • Suppose r1 and r2 are the diffusion rate of
gas-1 and gas-2 respectively.
• The densities of these two gases at the
same temperature and pressure are d1
and d2 respectively.
• Acc. to Graham’s law of diffusion of
gases.
r1/r2 = dαM
=
• The ratio of densities of any two gases is
equal to the ratio of the molecular weight
of those two gases.
30. • The diffusion rate of a gas means the
volume of the diffused gas in one second.
• diffusion rate (r) = Volume of gas diffused (V)
Time required for diffusion (t)
r= v/t
• For two gases at the same temperature and
pressure,
r1 = V1/t1 and r2 = V2/t2
• During the experiment, for convenience,
the times required for diffusion of same
volumes of two gases diffusing in the same
time are measured.
31.
Hence the above equation can be written as follows :
r1/r2 = V1/t1 =
M2 OR V1•t2 = =
d1 M2
V2/t2 M1 V 2•t1 d2 M1
V1 =
V2
Now if t1 = t2
M2
M1
then
t2
t1
=
But if V1 = V2 then
M2
M1
32. Importance of Graham’s law of gaseous
diffusion
Uranium metal has two isotopes : U235 and U238.
U235 is very important in production of atomic energy.
The proportion of U235 in uranium metal is only 0.7%.
As uranium hexafluoride (UF₆) is a volatile compound
uranium hexafluoride is prepared from uranium metal.
The difference of molecular weight between 235UF₆ and
238
UF₆ is much less. Hence, the ratio of rate of diffusion
of these gases will be 1.0047.
Now, if uranium hexafluoride gas is filled in a porous
vessel allowed to have the diffusion, the amount of
235
UF₆ of less density will diffused somewhat more.
Because of the small difference in diffusion rate, a
series of a number of experiments is constructed.
33. This type of work is carried out in a laboratory
extended to kilometer at oak-Ridge in tenessy
state of america.
The experiment of diffusion of this gas through
porous membranes distributed (extended) to
about a kilometer.
After a long time pure 235UF₆ is obtained which is
decomposed to get pure 235U.
In short, the isotopes of uranium 235U and 238U
can be separated.
The importance of this law is in finding the
molecular weights of gases and the densities.
The components gases can also be separated
from the mixture of gases.
34. Avogadro’s Hypothesis
Avogadro gave a principle in 1811 A.D.
According to it, “Equal volume of the gases
contain equal number of molecules at standard
temperature and pressure .
Simple gas equation is one of the methods to
presents the Avogadro’s principle.
One important dimension resulting from
Avogadro’s principle is molar volume.
Molar volume means the volume occupied by
molecular weight expressed in gram of gas. The
volume of 1 mole at 273 kelvin and 1
atmosphere pressure can be found out by
general gas equation.
35.
36. • PV = nRT where P = 1 atmosphere
V = ? litre
V = nRT n = 1 mole gas
P R = 0.082 lit.a tm./k.mol.
T = 273 K.
V = 1 mole x 0.082 lit.atm./k.mol. 273 גkelvin
1 atmosphere
V = 22.4 litre
Thus molar volume is also called gram molar
37. Thus molar volume is also called gram molar volume.
The presentation of Avogadro’s principle on the basis
of molar volume can be done as follows :
“In 22.4 litre of any gas at 273 kelvin 1 atmosphere
contains 1 mole molecules.”
This statement can be given alternatively as, “The
weight of 22.4 litre of any gas at 273 kelvin
temperature and 1 atmosphere pressure, is its
molecular weight.”
According to Avogadro’s principle, “ the number of
molecules in 1 molar volume of any gas is 6.022 10 23.”
The weight of one mole of any substance is its
molecular weight.”
39. Kinetic molecular theory
All the gases are composed of innumerable microscopic particles (atoms or
molecules).
The volume of molecules is negligible in comparison with the volume
(volume of the vessel) occupied by the gas. All the molecules in each have
same volume and weight.
The molecules of the gas are in continuous motion.
The molecules of the gas created (develops) pressure on the wall by striking
with the walls of the vessel.
The molecules in the gas have no attraction or repulsion for each other.
When the continuously moving molecules strike with one another, they
exchange the kinetic energy
As this process is continuously going on, the molecules in the gas do not
move with uniform velocity. At any time and any temperature, the velocity of
certain molecules will be very less, some will have moderate and will have very
high. Really the average velocity of each molecule
40. What are the different types of solids?
There are four types of crystalline solids --
Ionic solids-- These substances have a definite melting point
and contain ionic bonds. An example would be sodium
chloride (NaCl). View the 3-D structure of a salt crystal.
Covalent solids -- These substance appear as a single giant
molecule made up of an almost endless number of covalent bonds.
An example would be graphite. View the 3-D structure of graphite).
Molecular solids are represented as repeating units made up
of molecules. An example would be ice. View the 3-D
structure of ice.
Metallic solids are repeating units made up of metal atoms. The
valence electrons in metals are able to jump from atom to atom.
41. CRYSTAL LATTICE
• The definate arrangement of constituent
particle (atoms,ions or molecules) shown
by dots in three dimension in crystal is
known as crystal lattice.
UNIT CELL :
• A tiny or smallest part of the crystal lattice
lattice which bears all the characteristics
of the crystal and when repeated in three
dimension forms complete crystal structure
43. Unit cell of NaCl
It is be observed that each Na+ is surrounded octahedrally by
six chloride icons and similarly each chloride icon by six Na+
ion.
Here the ionic size of Na+ ions is similar and cannot be
arranged in a manner that each ions touches its neighbour
ion.
In this configuration Na+ and Cl- ions are arranged in such a
way that they remain as near as possible with each other.
In this construction Na+ - Na+ ion is maximum. Because of a
such a arrangement, the distance between Cl- ions increased
automatically.
The co-ordination number of Na+ in NaCl crystal is six and the
ratio of Na+ /Cl- radii is 0.53.
45. Unit cell of CsCl
If we examine the configuration of unit cell of CsCl,
it will be found that each Cs+ is surrounded by eight
Cl- and similarly each Cl- ions is surrounded by eight
Cs+ ions.
If the co-ordination number of metal ion is more in an
ionic crystal, the stability is also more.
Hence the stability of CsCl is more than that of
NaCl .
The co-ordination number of Cs+ in CsCl crystal is
eight and the ratio of Cs+ in CsCl crystal is eight and
the ratio of Cs+ / Cl- radii is 0.92.
It has body centered cubic arrangement.
47. Unit cell of LiI
In LiI, negative charge possessing I- is much larger in
size as compared to the positive charge possessing
Li+ ion. Hence the negatively charged ions can be
arranged very near to each other.
The positively charged ion can be arranged very
near to each other.
The positively charged ions can be easily placed in
the vacant space formed between these ions. This
type situation arises in the crystal of LiI.
The cross section of layer containing ions is shown
in figure. In this four I- ions are arranged almost
touching each other. I- ions are also above and below
of this central void of this configuration.
48. UNIT CELL OF LiI
• Due to eight I- ions arranged in a manner touching
each other, the shape that evolves is octahedral.
• As I- ion is big, the size of octahedral configuration is
comparatively big.
• Li+ ion being smaller in size can be arranged easily
in the central void (space). In this configuration,
similarly charged I- ions are arranged near each
other in such a manner that the attraction between
them is less and repulsion is more.
• Thus this configuration possesses relatively less
stability. Because of this, the melting point of LiI is
less than that of NaCl.
49. Information about different co-ordination
numbers and ratio of radii
Radii Ratio Co-ordination Arrangement of Examples
(r+/r-) number of positive-negative
positive ions ions
Upto 0.155 2 Linear
0.155 to 0225 3 Planer triangle
0.225 to 0.414 4 Tetrahedral ZnS
0.414 to 0.73 4 Square planer
0.414 to 0.73 6 FCC NaCl
0.73 to 1.0 8 Octahedral-BCC CsCl
Above 1.0 12 HCP
51. Clearity of the term
Diffusion :
The property of the liquid to spread
in another liquid.
Evaporation :
The property of liquids to get
converted of its own into gaseous
state at normal temperature
52. Vapour pressure :
The vapour exert pressure on the
surface of the liquid at equillibrium.
Surface tension :
The force exerted by the molecules
on the hypothetical line of unit
length parellel to the surface of the
liquid and perpendicular to the
molecules on the other side of the
molecules.
Editor's Notes
MECHANICS OF BREATHING Gas travels from high pressure to low pressure. This is also responsible for all weather patterns.