Gaslaws
•Download as PPTX, PDF•
0 likes•195 views
- Boyle's law states that the volume of a fixed mass of gas is inversely proportional to its pressure at constant temperature. PV = k. - Charles' law describes how the volume of a gas is directly proportional to its absolute temperature if pressure remains constant. V/T = k. - According to Gay-Lussac's law, the pressure of a fixed mass of gas is directly proportional to its absolute temperature when volume is kept constant. P/T = k. - The general gas law combines Boyle's, Charles', and Gay-Lussac's laws to relate pressure, volume, temperature, and amount of gas: PV/T = k.
Report
Share
Report
Share
Recommended
Gaslawsprep
The document summarizes several gas laws:
1) Boyle's law states that the volume of a fixed mass of gas is inversely proportional to its pressure at constant temperature.
2) Charles' law states that the volume of a fixed mass of gas is directly proportional to its absolute temperature if pressure remains constant.
3) Gay-Lussac's law states that the pressure of a fixed mass of gas is directly proportional to its absolute temperature if volume remains constant.
4) The general gas law combines Boyle's, Charles', and Gay-Lussac's laws to relate the pressure, volume, temperature, and amount of gas in a system.
Combined gas law
PCO2
Ptotal = PN2 + PO2 + PCO2
2.50 atm = 0.90 atm + 0.60 atm + PCO2
PCO2 = 2.50 atm - 0.90 atm - 0.60 atm
PCO2 = 1 atm
So the partial pressure of CO2 is 1 atm.
3 d presentation
This document explains the combined gas law formula and provides an example of how to use it to solve problems involving gas pressure, volume, and temperature.
The combined gas law states that the pressure-volume product of a gas divided by its temperature remains constant. The formula combines Boyle's law, Charles' law, and Gay-Lussac's law.
An example problem applies the formula to calculate the volume of a gas at a new pressure and temperature, given the initial pressure, volume, and temperature. The formula is used and the calculation is shown step-by-step to arrive at the answer.
Charle's law
Charle's law states that at a constant pressure, the volume of a gas increases or decreases by 1/273 of its original volume for each 1 degree Celsius increase or decrease in temperature. Specifically, the volume is directly proportional to the absolute temperature. This relationship has been verified experimentally by plotting graphs of volume versus temperature, which produce straight lines passing through the origin, indicating a direct proportionality. The law allows for calculations of gas volume changes with temperature changes and has applications like filling hot air balloons due to air's decreasing density when heated.
Boyles Law
Boyle's Law states that the pressure and volume of a gas are inversely proportional at a constant temperature. It can be expressed as a formula: Pressure x Volume = Constant. An experiment was conducted where the pressure of a gas was increased while the volume decreased, keeping the pressure x volume constant. When the results were graphed with volume on the y-axis and the reciprocal of pressure on the x-axis, the points lay along a straight line, illustrating that volume is inversely proportional to pressure according to Boyle's Law.
Lecture 4 Charles' law
This lesson talks about another gas law, the Charles' Law. This is a simplify lesson for intended for the level of my students understanding. Hope it helps you too!
Chapter 4.4(charles' law)
Charles' Law states that the volume of a gas is directly proportional to its absolute temperature when pressure is held constant. As temperature increases, the molecules move faster and push outward, increasing the volume. This relationship is expressed mathematically as V1/V2 = T1/T2, where V is volume and T is temperature measured on the Kelvin scale. Absolute zero is defined as 0K or -273°C, the lowest possible temperature.
Gas laws
This document discusses the key gas laws and their relationships. It begins by introducing the four main properties that determine gas behavior: pressure, volume, amount of gas, and temperature. It then explains each gas law in more detail: Boyle's Law describes the inverse relationship between pressure and volume; Charles' Law specifies the direct relationship between volume and temperature; Gay-Lussac's Law shows the direct link between pressure and temperature; and the Combined Gas Law incorporates all three. The document also presents sample problems demonstrating applications of the gas laws.
Recommended
Gaslawsprep
The document summarizes several gas laws:
1) Boyle's law states that the volume of a fixed mass of gas is inversely proportional to its pressure at constant temperature.
2) Charles' law states that the volume of a fixed mass of gas is directly proportional to its absolute temperature if pressure remains constant.
3) Gay-Lussac's law states that the pressure of a fixed mass of gas is directly proportional to its absolute temperature if volume remains constant.
4) The general gas law combines Boyle's, Charles', and Gay-Lussac's laws to relate the pressure, volume, temperature, and amount of gas in a system.
Combined gas law
PCO2
Ptotal = PN2 + PO2 + PCO2
2.50 atm = 0.90 atm + 0.60 atm + PCO2
PCO2 = 2.50 atm - 0.90 atm - 0.60 atm
PCO2 = 1 atm
So the partial pressure of CO2 is 1 atm.
3 d presentation
This document explains the combined gas law formula and provides an example of how to use it to solve problems involving gas pressure, volume, and temperature.
The combined gas law states that the pressure-volume product of a gas divided by its temperature remains constant. The formula combines Boyle's law, Charles' law, and Gay-Lussac's law.
An example problem applies the formula to calculate the volume of a gas at a new pressure and temperature, given the initial pressure, volume, and temperature. The formula is used and the calculation is shown step-by-step to arrive at the answer.
Charle's law
Charle's law states that at a constant pressure, the volume of a gas increases or decreases by 1/273 of its original volume for each 1 degree Celsius increase or decrease in temperature. Specifically, the volume is directly proportional to the absolute temperature. This relationship has been verified experimentally by plotting graphs of volume versus temperature, which produce straight lines passing through the origin, indicating a direct proportionality. The law allows for calculations of gas volume changes with temperature changes and has applications like filling hot air balloons due to air's decreasing density when heated.
Boyles Law
Boyle's Law states that the pressure and volume of a gas are inversely proportional at a constant temperature. It can be expressed as a formula: Pressure x Volume = Constant. An experiment was conducted where the pressure of a gas was increased while the volume decreased, keeping the pressure x volume constant. When the results were graphed with volume on the y-axis and the reciprocal of pressure on the x-axis, the points lay along a straight line, illustrating that volume is inversely proportional to pressure according to Boyle's Law.
Lecture 4 Charles' law
This lesson talks about another gas law, the Charles' Law. This is a simplify lesson for intended for the level of my students understanding. Hope it helps you too!
Chapter 4.4(charles' law)
Charles' Law states that the volume of a gas is directly proportional to its absolute temperature when pressure is held constant. As temperature increases, the molecules move faster and push outward, increasing the volume. This relationship is expressed mathematically as V1/V2 = T1/T2, where V is volume and T is temperature measured on the Kelvin scale. Absolute zero is defined as 0K or -273°C, the lowest possible temperature.
Gas laws
This document discusses the key gas laws and their relationships. It begins by introducing the four main properties that determine gas behavior: pressure, volume, amount of gas, and temperature. It then explains each gas law in more detail: Boyle's Law describes the inverse relationship between pressure and volume; Charles' Law specifies the direct relationship between volume and temperature; Gay-Lussac's Law shows the direct link between pressure and temperature; and the Combined Gas Law incorporates all three. The document also presents sample problems demonstrating applications of the gas laws.
2 22 What Is The Combined Gas Law
The document contains instructions and objectives for a chemistry class. It provides the date of February 22nd and instructs students to take their seats, get out their binders and yesterday's practice questions. It then shares the results from an exit slip on Friday, ranging from 88% to 97%. The objective for the day is to apply the combined gas law to relationships between temperature, pressure and volume.
Dalton partial-pressure
This document discusses gas laws and properties related to gas pressure. It begins with questions about gas pressure in balloons and containers filled with pure oxygen. It then summarizes Dalton's law of partial pressures, which states that the total pressure of a gas mixture is equal to the sum of the individual gas partial pressures. The document provides examples of calculating total and partial pressures. It continues discussing vapor pressure and how to measure and correct for vapor pressure when collecting gases over water. It concludes with sample calculations for determining the volume of dry gas collected at standard temperature and pressure.
Lec5 a
Here are the key steps to solve this problem using Charles' Law:
1) Convert temperatures to Kelvin:
T1 = 297.0 K
T2 = 216.5 K
2) Use the Charles' Law equation:
V1/T1 = V2/T2
3) Solve for V2:
V2 = V1 * T2/T1
= 20.0 L * 216.5 K/297.0 K
= 14.6 L
So the volume outside at -70°F would be 14.6 L.
06 dalton’s law of partial pressures
Dalton's Law of Partial Pressures states that the total pressure of a gas mixture is equal to the sum of the partial pressures of the individual gases in the mixture. The partial pressure of a gas is the pressure that gas would exert if it alone occupied the total volume. For example, in a mixture of O2, N2, and CO2 gases with pressures of 37 kPa, 41 kPa and 57 kPa respectively, the total pressure is equal to the sum of the partial pressures, which is 37 + 41 + 57 = 135 kPa. This law can be used to calculate the pressure of a gas collected by water displacement, where the total pressure equals the pressure of the collected gas plus the vapor pressure of
Unit 10 daltons law fl14 final
Mostly conceptual explanation of Dalton's Law of Partial Pressures plus a few examples. General Chemistry
Dalton's law tutorial 5.1
Dalton's law states that the total pressure of a gas mixture is equal to the sum of the partial pressures of the individual gases in the mixture. The document provides an explanation of Dalton's law, including definitions of key terms like partial pressure. It also provides several examples and practice problems that apply Dalton's law to calculate total pressure, partial pressures, or missing values in gas mixtures.
3 charles law
1) This document discusses Charles' Law and how it relates the volume of an ideal gas to its temperature when pressure is held constant. Charles' Law states that the volume of a gas is directly proportional to its absolute temperature.
2) An example problem demonstrates how to use the Charles' Law equation to calculate the volume of a gas at a different temperature given its initial volume and temperature.
3) Learning checks are included to test understanding of Charles' Law and how the volume and temperature of a gas are related at constant pressure.
Charles law
An introduction to Charles' Law: The relationship between the volume of a trapped gas and its temperature at constant pressure and amount of gas.
Dalton's Law of Partial Pressures
John Dalton was an English chemist, physicist and meteorologist born in 1776. He formulated the Law of Partial Pressures in 1801, which states that the total pressure of a mixture of gases in a container is equal to the sum of the pressures of each gas if they occupied the container alone at the same temperature. Dalton's law is useful for calculating the pressure of individual gases in a mixture based on their partial pressures and the total pressure. It can be applied, for example, to find the air pressure inside a bottle by subtracting the pressure of water vapor from the total pressure.
Gases law (2014) al-faruq
The document discusses the kinetic theory of gases and summarizes several gas laws including Boyle's law, Charles' law, and the pressure law. It explains that Boyle's law relates the inverse relationship between pressure and volume of a gas at constant temperature. Charles' law describes the direct relationship between volume and temperature of a gas at constant pressure. The pressure law states pressure is directly proportional to temperature for a gas at constant volume. Examples are provided to demonstrate how to use these laws to calculate gas properties under different conditions. The gas equation is derived by combining the gas laws.
Chapter 4.4(pressure law)
The document discusses pressure law and how pressure relates to temperature for a gas at constant volume and mass. It states that pressure is directly proportional to absolute temperature, explains how to solve problems involving pressure and temperature using the equation P1/T1 = P2/T2, and defines absolute zero as the lowest possible temperature of -273°C or 0K. It also provides an example of converting between Celsius and Kelvin temperatures.
Chapter 10.3 : The Gas Laws
The document summarizes several gas laws including Boyle's law, Charles' law, Gay-Lussac's law, Dalton's law of partial pressures, and the combined gas law. It defines each law using the kinetic molecular theory and provides sample problems and equations to demonstrate how to use each law to calculate changes in gas properties like volume, pressure and temperature. Sample problems are worked through step-by-step to show how the gas laws can be applied to different scenarios involving gases.
Application gas laws pt
The document discusses gas laws and their applications. It outlines several gas laws including Boyle's law, Charles' law, Gay-Lussac's law, Dalton's law of partial pressures, and Avogadro's law. These laws describe the relationships between various gas properties including pressure, volume, temperature, and number of moles. The document also provides examples of how gas laws are applied in areas like bicycles, cars, and medical equipment. Students will demonstrate their understanding of gas behavior and laws through various performance tasks.
Joule thomson effect
This document summarizes a laboratory experiment on the Joule-Thomson effect. The experiment measured the temperature change of carbon dioxide gas as it underwent adiabatic expansion from high to low pressures. The measured experimental Joule-Thomson coefficient for CO2 was 0.0074 K/kPa, with a 7.76% error compared to the theoretical coefficient calculated from gas properties. The results confirmed that temperature decreases with decreasing pressure during Joule-Thomson expansion of real gases.
1 a. pneumatic introduction, gas laws
This document discusses pneumatic and electro-pneumatic systems. It covers the properties of air and gases, including the ideal gas laws of Boyle's law, Charles' law, Avogadro's law, and Dalton's law of partial pressures. It also discusses key components of pneumatic systems like compressors, filters, regulators, valves and actuators. The document introduces electro-pneumatic systems and their elements, as well as pneumatic logic circuits.
Dalton's Law of Partial Pressure
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.
3 behavior of gases
This document discusses key concepts relating to the behavior of gases, including the definitions of pressure and how it relates to force and area. It describes how pressure decreases with increasing altitude due to lower atmospheric pressure. Boyle's Law and Charles' Law are also summarized, with Boyle's Law stating that gas pressure increases as volume decreases if temperature remains constant, while Charles' Law indicates that gas temperature increases as volume increases if pressure remains constant. Charles' Law is used to calculate the temperature at which gas volume would reach absolute zero.
Ch 12 gas laws
The document discusses the physical properties and behavior of gases. It covers several topics:
(1) The kinetic molecular theory describes how gas particles behave with constant, random motion and no attraction between particles. Real gases deviate from this ideal behavior at low temperatures and pressures.
(2) Gases expand to fill their containers due to their random motion. Their densities are very low due to empty space between particles. Temperature is described using Kelvin, and various instruments are used to measure gas pressure.
(3) The gas laws - Boyle's, Charles', Gay-Lussac's and combined gas law - quantitatively describe the relationships between pressure, volume, temperature and amount of gas. Examples show how
Gas law and partial pressures
The document summarizes key concepts of gas laws and gas behavior:
1. Gases assume the volume and shape of their container, are highly compressible, and mix completely. The ideal gas law relates the pressure, volume, amount, and temperature of a gas.
2. Boyle's, Charles', and Avogadro's laws describe how gas properties change with pressure, temperature, and amount at constant conditions. Dalton's law explains partial pressures in gas mixtures.
3. Real gases deviate from ideal behavior due to intermolecular forces, following the same trends but requiring correction factors at high pressures or low temperatures.
Notes gas laws
The document discusses various gas laws including Boyle's law, Charles' law, Gay-Lussac's law, the combined gas law, and the ideal gas law. It explains how changing variables like pressure, volume, temperature, and moles of gas affects the behavior of gases based on these laws. Examples are provided to demonstrate how to use the gas laws to calculate unknown variable values.
9th Grade Chapter 7 Lesson 3
The document provides an overview of biochemistry and the key components of cells. It discusses the four main compounds that make up cells - carbohydrates, lipids, proteins, and nucleic acids. Carbohydrates like glucose are used for energy, lipids include fats and oils, proteins perform important functions and are made of amino acids, and nucleic acids DNA and RNA control cell activities and inheritance. The document also describes important cell structures like mitochondria and the nucleus, as well as metabolic processes like cellular respiration.
Shapes And Bond Angles Of Simple Organic Compounds
The document discusses the structures and bonding in several simple organic compounds and solid materials. It describes:
1) The hybridization of atomic orbitals that gives rise to the tetrahedral structure of methane (CH4) with sp3 hybrid orbitals on carbon and single C-H sigma bonds.
2) The sp2 hybridization in ethene (C2H4) which forms three sp2 hybrid orbitals for C-H and C-C sigma bonds and a perpendicular p orbital for a pi bond between the carbons in the double bond.
3) The delocalized pi bonding and resonance structures in the hexagonal ring structure of benzene.
More Related Content
What's hot
2 22 What Is The Combined Gas Law
The document contains instructions and objectives for a chemistry class. It provides the date of February 22nd and instructs students to take their seats, get out their binders and yesterday's practice questions. It then shares the results from an exit slip on Friday, ranging from 88% to 97%. The objective for the day is to apply the combined gas law to relationships between temperature, pressure and volume.
Dalton partial-pressure
This document discusses gas laws and properties related to gas pressure. It begins with questions about gas pressure in balloons and containers filled with pure oxygen. It then summarizes Dalton's law of partial pressures, which states that the total pressure of a gas mixture is equal to the sum of the individual gas partial pressures. The document provides examples of calculating total and partial pressures. It continues discussing vapor pressure and how to measure and correct for vapor pressure when collecting gases over water. It concludes with sample calculations for determining the volume of dry gas collected at standard temperature and pressure.
Lec5 a
Here are the key steps to solve this problem using Charles' Law:
1) Convert temperatures to Kelvin:
T1 = 297.0 K
T2 = 216.5 K
2) Use the Charles' Law equation:
V1/T1 = V2/T2
3) Solve for V2:
V2 = V1 * T2/T1
= 20.0 L * 216.5 K/297.0 K
= 14.6 L
So the volume outside at -70°F would be 14.6 L.
06 dalton’s law of partial pressures
Dalton's Law of Partial Pressures states that the total pressure of a gas mixture is equal to the sum of the partial pressures of the individual gases in the mixture. The partial pressure of a gas is the pressure that gas would exert if it alone occupied the total volume. For example, in a mixture of O2, N2, and CO2 gases with pressures of 37 kPa, 41 kPa and 57 kPa respectively, the total pressure is equal to the sum of the partial pressures, which is 37 + 41 + 57 = 135 kPa. This law can be used to calculate the pressure of a gas collected by water displacement, where the total pressure equals the pressure of the collected gas plus the vapor pressure of
Unit 10 daltons law fl14 final
Mostly conceptual explanation of Dalton's Law of Partial Pressures plus a few examples. General Chemistry
Dalton's law tutorial 5.1
Dalton's law states that the total pressure of a gas mixture is equal to the sum of the partial pressures of the individual gases in the mixture. The document provides an explanation of Dalton's law, including definitions of key terms like partial pressure. It also provides several examples and practice problems that apply Dalton's law to calculate total pressure, partial pressures, or missing values in gas mixtures.
3 charles law
1) This document discusses Charles' Law and how it relates the volume of an ideal gas to its temperature when pressure is held constant. Charles' Law states that the volume of a gas is directly proportional to its absolute temperature.
2) An example problem demonstrates how to use the Charles' Law equation to calculate the volume of a gas at a different temperature given its initial volume and temperature.
3) Learning checks are included to test understanding of Charles' Law and how the volume and temperature of a gas are related at constant pressure.
Charles law
An introduction to Charles' Law: The relationship between the volume of a trapped gas and its temperature at constant pressure and amount of gas.
Dalton's Law of Partial Pressures
John Dalton was an English chemist, physicist and meteorologist born in 1776. He formulated the Law of Partial Pressures in 1801, which states that the total pressure of a mixture of gases in a container is equal to the sum of the pressures of each gas if they occupied the container alone at the same temperature. Dalton's law is useful for calculating the pressure of individual gases in a mixture based on their partial pressures and the total pressure. It can be applied, for example, to find the air pressure inside a bottle by subtracting the pressure of water vapor from the total pressure.
Gases law (2014) al-faruq
The document discusses the kinetic theory of gases and summarizes several gas laws including Boyle's law, Charles' law, and the pressure law. It explains that Boyle's law relates the inverse relationship between pressure and volume of a gas at constant temperature. Charles' law describes the direct relationship between volume and temperature of a gas at constant pressure. The pressure law states pressure is directly proportional to temperature for a gas at constant volume. Examples are provided to demonstrate how to use these laws to calculate gas properties under different conditions. The gas equation is derived by combining the gas laws.
Chapter 4.4(pressure law)
The document discusses pressure law and how pressure relates to temperature for a gas at constant volume and mass. It states that pressure is directly proportional to absolute temperature, explains how to solve problems involving pressure and temperature using the equation P1/T1 = P2/T2, and defines absolute zero as the lowest possible temperature of -273°C or 0K. It also provides an example of converting between Celsius and Kelvin temperatures.
Chapter 10.3 : The Gas Laws
The document summarizes several gas laws including Boyle's law, Charles' law, Gay-Lussac's law, Dalton's law of partial pressures, and the combined gas law. It defines each law using the kinetic molecular theory and provides sample problems and equations to demonstrate how to use each law to calculate changes in gas properties like volume, pressure and temperature. Sample problems are worked through step-by-step to show how the gas laws can be applied to different scenarios involving gases.
Application gas laws pt
The document discusses gas laws and their applications. It outlines several gas laws including Boyle's law, Charles' law, Gay-Lussac's law, Dalton's law of partial pressures, and Avogadro's law. These laws describe the relationships between various gas properties including pressure, volume, temperature, and number of moles. The document also provides examples of how gas laws are applied in areas like bicycles, cars, and medical equipment. Students will demonstrate their understanding of gas behavior and laws through various performance tasks.
Joule thomson effect
This document summarizes a laboratory experiment on the Joule-Thomson effect. The experiment measured the temperature change of carbon dioxide gas as it underwent adiabatic expansion from high to low pressures. The measured experimental Joule-Thomson coefficient for CO2 was 0.0074 K/kPa, with a 7.76% error compared to the theoretical coefficient calculated from gas properties. The results confirmed that temperature decreases with decreasing pressure during Joule-Thomson expansion of real gases.
1 a. pneumatic introduction, gas laws
This document discusses pneumatic and electro-pneumatic systems. It covers the properties of air and gases, including the ideal gas laws of Boyle's law, Charles' law, Avogadro's law, and Dalton's law of partial pressures. It also discusses key components of pneumatic systems like compressors, filters, regulators, valves and actuators. The document introduces electro-pneumatic systems and their elements, as well as pneumatic logic circuits.
Dalton's Law of Partial Pressure
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.
3 behavior of gases
This document discusses key concepts relating to the behavior of gases, including the definitions of pressure and how it relates to force and area. It describes how pressure decreases with increasing altitude due to lower atmospheric pressure. Boyle's Law and Charles' Law are also summarized, with Boyle's Law stating that gas pressure increases as volume decreases if temperature remains constant, while Charles' Law indicates that gas temperature increases as volume increases if pressure remains constant. Charles' Law is used to calculate the temperature at which gas volume would reach absolute zero.
Ch 12 gas laws
The document discusses the physical properties and behavior of gases. It covers several topics:
(1) The kinetic molecular theory describes how gas particles behave with constant, random motion and no attraction between particles. Real gases deviate from this ideal behavior at low temperatures and pressures.
(2) Gases expand to fill their containers due to their random motion. Their densities are very low due to empty space between particles. Temperature is described using Kelvin, and various instruments are used to measure gas pressure.
(3) The gas laws - Boyle's, Charles', Gay-Lussac's and combined gas law - quantitatively describe the relationships between pressure, volume, temperature and amount of gas. Examples show how
Gas law and partial pressures
The document summarizes key concepts of gas laws and gas behavior:
1. Gases assume the volume and shape of their container, are highly compressible, and mix completely. The ideal gas law relates the pressure, volume, amount, and temperature of a gas.
2. Boyle's, Charles', and Avogadro's laws describe how gas properties change with pressure, temperature, and amount at constant conditions. Dalton's law explains partial pressures in gas mixtures.
3. Real gases deviate from ideal behavior due to intermolecular forces, following the same trends but requiring correction factors at high pressures or low temperatures.
Notes gas laws
The document discusses various gas laws including Boyle's law, Charles' law, Gay-Lussac's law, the combined gas law, and the ideal gas law. It explains how changing variables like pressure, volume, temperature, and moles of gas affects the behavior of gases based on these laws. Examples are provided to demonstrate how to use the gas laws to calculate unknown variable values.
What's hot (20)
Viewers also liked
9th Grade Chapter 7 Lesson 3
The document provides an overview of biochemistry and the key components of cells. It discusses the four main compounds that make up cells - carbohydrates, lipids, proteins, and nucleic acids. Carbohydrates like glucose are used for energy, lipids include fats and oils, proteins perform important functions and are made of amino acids, and nucleic acids DNA and RNA control cell activities and inheritance. The document also describes important cell structures like mitochondria and the nucleus, as well as metabolic processes like cellular respiration.
Shapes And Bond Angles Of Simple Organic Compounds
The document discusses the structures and bonding in several simple organic compounds and solid materials. It describes:
1) The hybridization of atomic orbitals that gives rise to the tetrahedral structure of methane (CH4) with sp3 hybrid orbitals on carbon and single C-H sigma bonds.
2) The sp2 hybridization in ethene (C2H4) which forms three sp2 hybrid orbitals for C-H and C-C sigma bonds and a perpendicular p orbital for a pi bond between the carbons in the double bond.
3) The delocalized pi bonding and resonance structures in the hexagonal ring structure of benzene.
general chemistry ch1
The document is a slide presentation on chapter 1 of a general chemistry textbook. Chapter 1 covers fundamental topics like the properties and states of matter, measurement units, and dimensional analysis. It defines physical and chemical properties, classifies matter as elements, compounds, and mixtures, and discusses techniques for separating mixtures. Key concepts explained include significant figures, temperature scales, volume, density, and unit conversions. The presentation concludes with sample end-of-chapter questions.
Chapter 12 Stoichiometry
This document discusses stoichiometry, which is the calculation of quantities in chemical reactions using balanced chemical equations. It explains that balanced equations show the mole ratios of reactants and products, which can be used to determine the amounts of substances involved. Examples are given of how to calculate quantities in moles, masses, and volumes using mole-mole, mass-mole, mole-mass, and mass-mass methods based on the mole ratios from balanced equations. The concept of a limiting reagent is also introduced, which determines the maximum amount of product that can be formed.
Electrochemistry
The document outlines learning outcomes for a chapter on electrochemistry. It will describe investigations into classifying substances as conductors or non-conductors, distinguish between metallic and electrolytic conduction, define key terms like electrolysis, electrodes, and ions. It will also cover predicting reactions and products of electrolysis, calculating quantities produced using Faraday's constant, and discussing industrial applications of electrolysis.
Acids And Alkali
This document discusses acids and alkalis. It defines acids as substances that produce hydrogen ions in water, and provides examples like hydrochloric acid. Acids have properties like a sour taste, turning litmus red, and reacting with metals and carbonates. Alkalis are defined as metal oxides or hydroxides soluble in water, with examples like sodium hydroxide. Alkalis have properties like a bitter taste, turning litmus blue, and reacting with acids. The document also describes how acids and alkalis neutralize each other to form salts and water.
Esters, all properties
A general view of all chemical and physical properties of esters. Ass well as their daily use and structure ;)
Stoichiometry
This document discusses stoichiometry, which uses balanced chemical equations to determine amounts of reactants and products in chemical reactions. It provides examples of using mole ratios from chemical equations to solve stoichiometry problems involving moles of substances or conversions between moles and grams. The key aspects are that chemical equations provide mole ratios that can be used as conversion factors, and problems must be worked in moles since equations relate substances in moles.
Electrochemistry class 12 ( a continuation of redox reaction of grade 11)
Electrochemistry involves the study of chemical reactions that produce electricity and chemical reactions produced by electricity. A galvanic (voltaic) cell converts the chemical energy of a spontaneous redox reaction into electrical energy. Daniell's cell uses the redox reaction of zinc oxidizing copper ions to produce a cell potential of 1.1 V. An electrolytic cell uses an applied voltage to drive a nonspontaneous redox reaction in the opposite direction of the natural reaction in a galvanic cell. Standard reduction potentials allow prediction of the tendency of half-reactions to occur and their oxidizing or reducing power.
Biochemistry lecture 1
1. The document provides an introduction to biochemistry including defining it as the science concerned with chemical basis of life and chemical constituents of living cells.
2. It describes the key components of living matter including water, inorganic substances, and organic biomolecules.
3. The key cellular organelles such as nucleus, mitochondria, endoplasmic reticulum, Golgi complex, lysosomes, and their functions are outlined.
Chapter 15 Lecture- Chemical Equilibrium
1. The document discusses chemical equilibrium, including the concepts of equilibrium, depicting equilibrium reactions with equations, the equilibrium constant K, and how the value of K relates to whether a reaction favors reactants or products.
2. It also covers heterogeneous equilibria involving solids or liquids, how the concentrations of solids and liquids do not appear in equilibrium expressions, and examples of heterogeneous equilibrium reactions like the decomposition of calcium carbonate.
3. The key aspects covered are the definition of chemical equilibrium as when forward and reverse reactions proceed at the same rate, the use of concentration ratios and partial pressures to define equilibrium constants Kc and Kp, and how heterogeneous reactions involve gases in equilibrium with solids or liquids.
Biochemistry PowerPoint
This document summarizes key chemistry concepts related to the building blocks of life. It covers the elements, atoms, and molecules that make up living organisms. It also describes the four main types of organic compounds - carbohydrates, lipids, proteins, and nucleic acids - and provides examples of each. Water is highlighted for its importance as a solvent and in biological processes and reactions.
Chemical kinetics presentation
Kinetics – Background
Rate Of Reaction
Factors Affecting the Rate
Concentration & Rate – Rate Laws, Order
Reaction Mechanism – Molecularity
Temperature & Rate – Arrhenius equation
Pseudo Order Reactions - Brief Overview
Adsorption Kinetic Models – Types
Adsorption Reaction Models
Adsorption Diffusion Models
Kinetic Best Fit Model Interpretation
Ch11
This document summarizes Chapter 11 of a General Chemistry textbook. Chapter 11 discusses chemical bonding, including Lewis theory, ionic and covalent bonds, molecular geometry, bond order, bond energies, and exceptions to the octet rule. It also introduces polymers as macromolecular substances. The chapter contains examples of writing Lewis structures and determining formal charges and molecular geometry using VSEPR theory. Key questions at the end review these concepts.
Thermodynamics
M.THIRUNAVUKKARASU
Sr. LECTURER
Bharathiyar college of Engineering and Technology at karaikal
Tamil Nadu
Thermodynamic Chapter 3 First Law Of Thermodynamics
This document provides an overview of the first law of thermodynamics for closed systems. It defines key terms like internal energy, kinetic energy, and potential energy. It presents the general energy balance equation for closed systems undergoing various processes like constant volume, constant pressure, or adiabatic. Example problems demonstrate applying the first law to calculate changes in internal energy or heat transfer. The document also discusses thermodynamic cycles and how the first law applies to systems that return to their initial state.
Shelf ready packaging changing the face of the retail experience
Hoxton Changing the face of the Retail Packaging Solutions Experience
What Changes does this mean?
1. Items can be easily placed on a shelf by store persons.
2. Gives suppliers the opportunity to develop packaging.
3. Rapid introduction and expansion of international low-cost retailers.
4. Provides replenishment efficiencies
Young Marketers Elite 3 - Assignment 4.1 - Nhóm 6 - Vỹ, Lâm, Vân
Marketers need marketing research to help make informed business decisions. The document outlines the key reasons why marketers conduct marketing research and how different types of research help address different needs. Marketing research helps marketers understand markets and consumers, develop new product or campaign ideas, evaluate concepts and initiatives, and monitor performance after launch. Well-designed marketing research provides reliable insights to support strategic planning, innovation, and decision-making.
Social media
This document discusses the history and power of hashtags in social media marketing. It highlights quotes from entrepreneurs discussing their difficulties sharing ideas and building an audience. The document advises businesses to engage with customers on social media as it is not a passing trend. It provides tips to create and share content and maximize posts to connect with others on social media.
Viewers also liked (20)
Shapes And Bond Angles Of Simple Organic Compounds
Shapes And Bond Angles Of Simple Organic Compounds
Electrochemistry class 12 ( a continuation of redox reaction of grade 11)
Electrochemistry class 12 ( a continuation of redox reaction of grade 11)
Thermodynamic Chapter 3 First Law Of Thermodynamics
Thermodynamic Chapter 3 First Law Of Thermodynamics
Shelf ready packaging changing the face of the retail experience
Shelf ready packaging changing the face of the retail experience
Young Marketers Elite 3 - Assignment 4.1 - Nhóm 6 - Vỹ, Lâm, Vân
Young Marketers Elite 3 - Assignment 4.1 - Nhóm 6 - Vỹ, Lâm, Vân
Similar to Gaslaws
ppt-chem-gas-laws.pptx
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.
Lecture 14.2b- Gas Law Equations
The document discusses four key gas laws:
1) Boyle's law relates pressure and volume at constant temperature - as pressure increases, volume decreases and vice versa.
2) Charles's law relates temperature and volume at constant pressure - as temperature increases, volume increases.
3) Gay-Lussac's law relates temperature and pressure at constant volume - as temperature increases, pressure increases.
4) The combined gas law allows calculations involving changes in pressure, volume, and temperature for a constant amount of gas.
combined-gas-law-1.pptjsjsisujshsjsjjsjsjs
jajaiishshs sjisishshs jsoaoajshs ksoajshshis isisjshsj ksishshsh ksosjshs kosshhs akaisihwhwhe jsishshshjs ksishshs jsishshs kshsbs jsisbsbsjs jsisbsbs sksjnsjsis sisisjjs ksishs jsbsjsj jsbjsjs ksbsb sjsisjsujs sjsjjsjsjs isisjsjsj jsjsjsjsjsh jsisjsiejshs kajsjshsb disjsndbbdjs sksjnsjsid sjieishd isjsbdjsksie ksksjsjjsje sisksjjdjd sisisjjsisjsjsj siksisjsjsjdjjs sksjsjjdjdisis jsisjsjsjshshsje isodjsjsjgsbd kdidhbeksidhhe sjudbdjsosihsjeb skisbsbskosjdjeb oshsbs ksishshbdnwnsidb dnsjdb sjsjdbdn
GAS LAWS AND GENERAL GAS EQUATION (CHARLES, BOYLES AND AVOGADRO)
related to gas laws. charles law, boyles , avogadros law and the ideal gas law. inclusive is the general gas equation with worked examples.
Ch5 Gases
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.
Chapter 10 Lecture- Gases
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.
Properties of Gas Manik
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
Gas Laws
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 law (2014) faruq
The document discusses the kinetic theory of gases and summarizes several gas laws including Boyle's law, Charles' law, and the pressure law. It explains that Boyle's law relates the inverse relationship between pressure and volume of a gas at constant temperature. Charles' law describes the direct relationship between volume and temperature of a gas at constant pressure. The pressure law states pressure is directly proportional to temperature for a gas at constant volume. Examples are provided to demonstrate how to use these laws to calculate gas properties under different conditions.
Apchemunit5 gasespresentation-110901062845-phpapp01
This document provides an overview of gases and the gas laws. It begins with an introduction to the composition of Earth's atmosphere and how gases shield us and keep the planet warm. It then discusses gas pressure and how Torricelli invented the barometer to measure atmospheric pressure in 1643. Other sections cover the gas laws of Boyle, Charles, Avogadro, and the ideal gas law. The document provides examples of using these laws to solve gas stoichiometry problems. It concludes with an introduction to Dalton's law of partial pressures and the kinetic molecular theory of gases.
Gas laws Diagrams
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
Equations of State
1) An equation of state relates macroscopic variables like pressure, volume, temperature, and number of moles that describe a substance. The ideal gas law is the equation of state for gases.
2) Standard temperature and pressure (STP) are defined as 0°C (273.15 K) and 1 atmosphere (101.3 kPa). At STP, 1 mole of any gas occupies 22.4 L of volume.
3) Experiments on gas behavior led to Boyle's, Charles', and Gay-Lussac's laws, which combined form the ideal gas law: PV=nRT, relating pressure, volume, moles, and temperature.
GAS-LAWS -Properties of gases, relationships of temperature , volume and pres...
The document discusses three gas laws: Boyle's law, Charles' law, and the combined gas law. Boyle's law states that for a fixed amount of gas at constant temperature, the pressure and volume are inversely proportional. Charles' law states that for a fixed amount of gas at constant pressure, the volume and temperature are directly proportional. The combined gas law allows calculation of pressure, volume, or temperature given two sets of conditions for gas amount, pressure, volume, and temperature. Examples are provided to demonstrate application of the gas laws.
States of matter
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.
Advchemchapt5 101015113821-phpapp01
The document discusses gases and gas laws. It provides an overview of the composition and importance of Earth's atmosphere. Key topics covered include gas pressure, how it is measured using devices like the barometer, and how pressure varies with weather and altitude. The document then explains Boyle's, Charles', and Avogadro's laws regarding the behavior of gases. It introduces the ideal gas law and provides examples of using it to solve gas problems involving changes in pressure, volume, temperature, and moles of gas. It also covers gas stoichiometry, partial pressures of gases in mixtures, and the kinetic molecular theory of gases.
Ch5 Gases
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.
GAS LAWS.pptx
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.
PHYSICS WEEK 1 and 2.ppt
The document discusses several gas laws:
- Boyle's law states that for a fixed amount of gas at constant temperature, the volume is inversely proportional to the pressure.
- Charles's law describes the direct relationship between volume and temperature for a fixed amount of gas at constant pressure.
- Gay-Lussac's law explains that pressure and temperature are directly proportional for a fixed volume of gas.
- The combined gas law incorporates all three by relating pressure, volume, and temperature for a fixed amount of gas. It can be used to derive the other gas laws by holding one variable constant. Sample problems demonstrate applying the gas laws to calculate unknown properties.
the gas laws
The document discusses several gas laws including Boyle's law, Charles' law, Gay-Lussac's law, Avogadro's law, the combined gas law, and the ideal gas law. It provides definitions of these laws and examples of calculations using each one. The key relationships covered are: the inverse relationship between pressure and volume at constant temperature (Boyle's law), the direct relationship between volume and temperature at constant pressure (Charles' law), the direct relationship between pressure and temperature at constant volume (Gay-Lussac's law), the relationship between volume and amount of gas at constant pressure and temperature (Avogadro's law), and the ideal gas law which relates pressure, volume, temperature,
Similar to Gaslaws (20)
GAS LAWS AND GENERAL GAS EQUATION (CHARLES, BOYLES AND AVOGADRO)
GAS LAWS AND GENERAL GAS EQUATION (CHARLES, BOYLES AND AVOGADRO)
Apchemunit5 gasespresentation-110901062845-phpapp01
Apchemunit5 gasespresentation-110901062845-phpapp01
GAS-LAWS -Properties of gases, relationships of temperature , volume and pres...
GAS-LAWS -Properties of gases, relationships of temperature , volume and pres...
More from Conferat Conferat
Cellbiologybiolog
This document summarizes the key organelles and their functions in eukaryotic cells. It discusses three main jobs cells must perform: 1) make energy using mitochondria through cellular respiration or chloroplasts through photosynthesis, 2) make proteins using the nucleus, ribosomes, endoplasmic reticulum and Golgi apparatus, and 3) make more cells using the nucleus and centrioles during cell division. Each organelle, including the cell membrane, vacuoles, lysosomes and others, plays an important role in allowing the cell to carry out these essential functions needed for life.
Salts
A salt is formed when all or part of the hydrogen in an acid is replaced by metal or ammonium ions. There are different types of salts including normal salts, acid salts, basic salts, double salts, and complex salts. Salts can be prepared through reactions such as mixing a dilute acid with a metal to form a soluble salt, reacting an alkali with an acid, and mixing solutions containing ions that form an insoluble salt to produce precipitation. Insoluble salts can also be prepared through double decomposition reactions or by directly combining element constituents.
Acids,basesandsalts acids
This document discusses acids and bases. It defines acids as substances that produce hydrogen ions in water and describes strong acids as completely ionizing and weak acids as partially ionizing. It discusses the basicity of acids based on the number of replaceable hydrogen ions. Acids have sour taste, turn litmus red, and are corrosive when concentrated. Acids react with metals and bases. Bases are substances that neutralize acids to form salts and water. The document also discusses alkalis, neutralization, properties of bases, pH scale, calculations involving concentrations and ions, and buffer solutions.
Atomic sructureandbonding
This document discusses atomic structure and bonding. It begins by explaining electron states using notation like 1s, 2p, 3d. The energy of an electron depends on its state and interactions with other electrons. Valence electrons in the outer shell are important for chemical reactivity. Atoms gain, lose, or share electrons to achieve stable noble gas configurations through ionic bonding between metals and nonmetals or covalent bonding between less electronegative elements. The two main types of chemical bonding are ionic, involving transfer of electrons, and covalent, involving sharing of electron pairs.
Calculationsofwaterofcrystallisation
This document provides examples of calculating the percentage of water in hydrated salts and the percentage of water of crystallization. It also shows how to determine the formula of a salt based on the water of crystallization. Specifically, it demonstrates that the percentage of water in MgSO4.5H2O is 42.86% and the percentage of water of crystallization in CuSO4.xH2O is 36%. It further determines that the formula for CuSO4.xH2O is CuSO4.5H2O based on the mole ratio of CuSO4 to H2O being 1:5.
Chemicalcombinationsmoles,molecularandempirical
1) The document discusses concepts related to chemistry including relative atomic mass, relative molecular mass, moles, and empirical and molecular formulae.
2) It provides examples of calculating relative atomic mass, relative molecular mass, moles, percentage composition by mass, and determining empirical and molecular formulae.
3) Key formulas and concepts covered include using the atomic masses of elements to determine relative atomic mass and molecular mass, the definition of a mole in relation to Avogadro's number, and methods for calculating the number of moles and atoms in a sample.
Chemicalcombinationsbalancingchemeqns
The document discusses several laws of chemical combinations and balancing chemical equations. It introduces the law of conservation of mass, law of definite proportions, law of multiple proportions, and law of reciprocal proportions. It also defines valency as the combining power of an element and discusses balancing chemical equations by ensuring the left and right sides match based on atom counts. An example calculation is provided to determine the mass of O2 needed to burn a given mass of sodium.
Separationof mixtures andpurification of chemicalsubstances
This document discusses various techniques for separating mixtures and purifying chemical substances, including sieving, magnetic separation, sublimation, decantation, filtration, centrifugation, evaporation, crystallization, fractional crystallization, precipitation, distillation, fractional distillation, separating funnel, and chromatography. It provides examples of using sublimation to purify iodine and ammonium chloride, centrifugation to separate suspensions by spinning, and crystallization to separate salts that decompose on heating, such as iron(II) tetraoxosulphate(VI)-heptahydrate. Distillation and fractional distillation techniques are also outlined for recovering solvents from solutions and separating miscible liquids like in petroleum industries.
Work,energyandpower
Work is done when a force moves an object through a distance in the direction of the force. Work (W) is equal to the product of the force (F) and distance (s) moved, or W=Fxs. Energy is the capacity to do work and is also measured in joules. The principle of conservation of energy states that in a closed system, the total amount of energy remains constant. Power is the time rate of doing work and is measured in watts. Power is equal to work done divided by the time taken, or W/t.
WavesPREPWALK
A wave is a disturbance that transfers energy through a medium without displacing the medium. There are two types of waves: transverse waves, where the direction of vibration is perpendicular to the direction of travel, and longitudinal waves, where the direction of vibration is parallel. The amplitude of a wave is its maximum displacement from the mean position. Important wave properties include speed, frequency, wavelength, and the equation that describes a traveling wave using variables like amplitude, angular velocity, time, and position. Waves can be progressive, traveling in one direction, or stationary, formed by the combination of two progressive waves traveling in opposite directions. Key wave properties include reflection, refraction, diffraction, polarization, and interference.
Unitsandmeasurements
This document discusses the International System of Units (SI) used to measure physical quantities. It defines fundamental units like length, time and temperature, and derived units obtained by combining fundamental units, like volume. Multiples and submultiples are used to modify units. Dimensional analysis determines if equations are dimensionally correct by examining the dimensions of each term. Various instruments are described for measuring length, time, mass and weight at different scales, including vernier calipers, micrometer screws, stopwatches, balances and more. The key difference between mass and weight is also noted.
Thermalexpansion
Thermal expansion describes how the size of materials changes with increasing temperature. There are three main types of thermal expansion:
1. Linear expansion is the increase in length per unit length for each degree rise in temperature.
2. Area expansion can be calculated from linear expansion.
3. Volume expansion also relates to linear expansion, with volume expansion being three times the linear expansion rate.
Water is an anomaly as it contracts in volume from 0 to 4 degrees C before expanding normally at higher temperatures.
Temperatureanditsmeasurement
This document discusses temperature and its measurement. It defines temperature as a measure of hotness or coldness, while heat is a form of energy that can transfer between bodies with different temperatures. There are several types of thermometers discussed for measuring temperature, including mercury-in-glass, gas, thermoelectric, and resistance thermometers. Gas and resistance thermometers provide the widest measurement ranges, from -270°C to 1500°C and -180°C to 1520°C respectively. The document also provides examples of converting between Celsius, Fahrenheit and Kelvin temperature scales.
Soundwaves
This document summarizes key concepts about sound waves, including:
- The speed of sound varies in different mediums, such as 332 m/s in air, 1500 m/s in water, and up to 500 m/s in steel.
- The Doppler effect describes the change in frequency or pitch of a sound wave emitted by a moving source as it approaches or moves away from an observer.
- For vibrations in closed and open pipes, the fundamental frequency and harmonic frequencies are determined by the length of the pipe based on quarter, half, and three-quarter wave patterns.
- The velocity of a wave propagated along a fixed medium like a string or wire depends on the square root of
Simpleharmonicmotion
This document discusses simple harmonic motion and provides useful formulas. It explains that the period of a simple pendulum is calculated as T = 2π√l/g, where T is the period, l is the length of the pendulum, and g is the acceleration due to gravity. For an elastic spring undergoing simple harmonic motion, the total energy is calculated as the kinetic energy (1/2mv^2) plus the potential energy (1/2kx^2), where k is the spring constant. The document also states that the total energy is equal to the maximum potential energy when the kinetic energy is zero, and equal to the maximum kinetic energy when the potential energy is zero.
Refractionoflight onplanesurfacescurved
This document discusses refraction of light through plane and curved surfaces as well as glass prisms. It defines refractive index as the ratio of the speed of light in one medium to the speed in another. Snell's law states that the ratio of the sine of the angle of incidence to the sine of the angle of refraction is a constant, known as the refractive index, depending on the optical densities of the two media. Total internal reflection occurs when light passes from a denser to a less dense medium and the incident angle exceeds the critical angle.
Reflection of light at plane or curved surfaces
This document discusses the reflection of light at plane and curved surfaces. It covers the laws of reflection, the formation of images in plane mirrors, reflection using inclined and curved mirrors, and mirror formulas. The two laws of reflection are that the incident ray, reflected ray, and normal all lie in the same plane, and that the angle of incidence equals the angle of reflection. Images in plane mirrors are virtual, upright, and laterally inverted with the same size and distance behind the mirror as the object is in front. Reflection by curved mirrors depends on whether the mirror is convex or concave, with concave mirrors forming real images and convex mirrors forming virtual images.
Projectiles
This document defines a projectile as an object launched into the air under the influence of gravity and air resistance. It describes useful parameters for projectiles like time of flight, maximum height, and range. Formulas are provided for calculating time to maximum height, maximum height, range, and maximum range based on the initial velocity, angle of projection, and gravitational acceleration. The document also explains how to resolve projectile motion into horizontal and vertical components.
Pressure
Pressure is defined as force per unit area. Pressure in liquids is determined by the density of the liquid, height of the liquid column, and acceleration due to gravity. According to Pascal's principle, pressure applied to a confined fluid is transmitted undiminished throughout the fluid and to the walls of its container. Atmospheric pressure is caused by the weight of the air above the earth's surface and decreases with increasing altitude. Simple devices like mercury barometers and aneroid barometers can be used to measure atmospheric pressure.
Newton’s laws of motion
This document summarizes Newton's laws of motion, including:
1) Newton's first law states that an object at rest stays at rest and an object in motion stays in motion with the same speed and in the same direction unless acted upon by an unbalanced force.
2) Newton's second law states that the acceleration of an object as produced by a net force is directly proportional to the magnitude of the net force, in the same direction as the net force, and inversely proportional to the mass of the object.
3) Newton's third law states that for every action, there is an equal and opposite reaction.
More from Conferat Conferat (20)
Separationof mixtures andpurification of chemicalsubstances
Separationof mixtures andpurification of chemicalsubstances
Recently uploaded
Executive Directors Chat Leveraging AI for Diversity, Equity, and Inclusion
Let’s explore the intersection of technology and equity in the final session of our DEI series. Discover how AI tools, like ChatGPT, can be used to support and enhance your nonprofit's DEI initiatives. Participants will gain insights into practical AI applications and get tips for leveraging technology to advance their DEI goals.
ANATOMY AND BIOMECHANICS OF HIP JOINT.pdf
it describes the bony anatomy including the femoral head , acetabulum, labrum . also discusses the capsule , ligaments . muscle that act on the hip joint and the range of motion are outlined. factors affecting hip joint stability and weight transmission through the joint are summarized.
A Strategic Approach: GenAI in Education
Artificial Intelligence (AI) technologies such as Generative AI, Image Generators and Large Language Models have had a dramatic impact on teaching, learning and assessment over the past 18 months. The most immediate threat AI posed was to Academic Integrity with Higher Education Institutes (HEIs) focusing their efforts on combating the use of GenAI in assessment. Guidelines were developed for staff and students, policies put in place too. Innovative educators have forged paths in the use of Generative AI for teaching, learning and assessments leading to pockets of transformation springing up across HEIs, often with little or no top-down guidance, support or direction.
This Gasta posits a strategic approach to integrating AI into HEIs to prepare staff, students and the curriculum for an evolving world and workplace. We will highlight the advantages of working with these technologies beyond the realm of teaching, learning and assessment by considering prompt engineering skills, industry impact, curriculum changes, and the need for staff upskilling. In contrast, not engaging strategically with Generative AI poses risks, including falling behind peers, missed opportunities and failing to ensure our graduates remain employable. The rapid evolution of AI technologies necessitates a proactive and strategic approach if we are to remain relevant.
Your Skill Boost Masterclass: Strategies for Effective Upskilling
Your Skill Boost Masterclass: Strategies for Effective UpskillingExcellence Foundation for South Sudan
Strategies for Effective Upskilling is a presentation by Chinwendu Peace in a Your Skill Boost Masterclass organisation by the Excellence Foundation for South Sudan on 08th and 09th June 2024 from 1 PM to 3 PM on each day.A Survey of Techniques for Maximizing LLM Performance.pptx
A Survey of Techniques for Maximizing LLM Performance
How to Build a Module in Odoo 17 Using the Scaffold Method
Odoo provides an option for creating a module by using a single line command. By using this command the user can make a whole structure of a module. It is very easy for a beginner to make a module. There is no need to make each file manually. This slide will show how to create a module using the scaffold method.
DRUGS AND ITS classification slide share
Any substance (other than food) that is used to prevent, diagnose, treat, or relieve symptoms of a
disease or abnormal condition
Pollock and Snow "DEIA in the Scholarly Landscape, Session One: Setting Expec...
Pollock and Snow "DEIA in the Scholarly Landscape, Session One: Setting Expec...National Information Standards Organization (NISO)
This presentation was provided by Steph Pollock of The American Psychological Association’s Journals Program, and Damita Snow, of The American Society of Civil Engineers (ASCE), for the initial session of NISO's 2024 Training Series "DEIA in the Scholarly Landscape." Session One: 'Setting Expectations: a DEIA Primer,' was held June 6, 2024.What is the purpose of studying mathematics.pptx
Students often ask about what the purpose is for their learning. This PowerPoint highlights some really important reasons to study Mathematics.
Exploiting Artificial Intelligence for Empowering Researchers and Faculty, In...
Exploiting Artificial Intelligence for Empowering Researchers and Faculty, In...Dr. Vinod Kumar Kanvaria
Exploiting Artificial Intelligence for Empowering Researchers and Faculty,
International FDP on Fundamentals of Research in Social Sciences
at Integral University, Lucknow, 06.06.2024
By Dr. Vinod Kumar KanvariaHow to Manage Your Lost Opportunities in Odoo 17 CRM
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
Natural birth techniques - Mrs.Akanksha Trivedi Rama University
Natural birth techniques - Mrs.Akanksha Trivedi Rama UniversityAkanksha trivedi rama nursing college kanpur.
Natural birth techniques are various type such as/ water birth , alexender method, hypnosis, bradley method, lamaze method etcIntroduction to AI for Nonprofits with Tapp Network
Dive into the world of AI! Experts Jon Hill and Tareq Monaur will guide you through AI's role in enhancing nonprofit websites and basic marketing strategies, making it easy to understand and apply.
CACJapan - GROUP Presentation 1- Wk 4.pdf
Macroeconomics- Movie Location
This will be used as part of your Personal Professional Portfolio once graded.
Objective:
Prepare a presentation or a paper using research, basic comparative analysis, data organization and application of economic information. You will make an informed assessment of an economic climate outside of the United States to accomplish an entertainment industry objective.
South African Journal of Science: Writing with integrity workshop (2024)
South African Journal of Science: Writing with integrity workshop (2024)Academy of Science of South Africa
A workshop hosted by the South African Journal of Science aimed at postgraduate students and early career researchers with little or no experience in writing and publishing journal articles.Recently uploaded (20)
Film vocab for eal 3 students: Australia the movie
Film vocab for eal 3 students: Australia the movie
Executive Directors Chat Leveraging AI for Diversity, Equity, and Inclusion
Executive Directors Chat Leveraging AI for Diversity, Equity, and Inclusion
Your Skill Boost Masterclass: Strategies for Effective Upskilling
Your Skill Boost Masterclass: Strategies for Effective Upskilling
A Survey of Techniques for Maximizing LLM Performance.pptx
A Survey of Techniques for Maximizing LLM Performance.pptx
How to Build a Module in Odoo 17 Using the Scaffold Method
How to Build a Module in Odoo 17 Using the Scaffold Method
Pollock and Snow "DEIA in the Scholarly Landscape, Session One: Setting Expec...
Pollock and Snow "DEIA in the Scholarly Landscape, Session One: Setting Expec...
Exploiting Artificial Intelligence for Empowering Researchers and Faculty, In...
Exploiting Artificial Intelligence for Empowering Researchers and Faculty, In...
How to Manage Your Lost Opportunities in Odoo 17 CRM
How to Manage Your Lost Opportunities in Odoo 17 CRM
Natural birth techniques - Mrs.Akanksha Trivedi Rama University
Natural birth techniques - Mrs.Akanksha Trivedi Rama University
Liberal Approach to the Study of Indian Politics.pdf
Liberal Approach to the Study of Indian Politics.pdf
Introduction to AI for Nonprofits with Tapp Network
Introduction to AI for Nonprofits with Tapp Network
Digital Artefact 1 - Tiny Home Environmental Design
Digital Artefact 1 - Tiny Home Environmental Design
South African Journal of Science: Writing with integrity workshop (2024)
South African Journal of Science: Writing with integrity workshop (2024)
Gaslaws
- 1. PHYSICS GAS LAWS Short revision series
- 2. Boyle’s law The vol of fixed mass of gas is inversely proportional to its pressure provided the temperature is constant P α 1/V P = k 1/V PV = k P1 V1 = P2 V2 Application Use it to determine volume when the pressure is given, and also to determine pressure of a gas when the volume is known at constant temperature
- 3. Charles’ Law The volume of a given mass of gas is directly proportional to its absolute temperature T provided pressure is constant. V α T V = kT V/T = k V1/T1 = V2/T2
- 4. Gay Lussac’s law The pressure of a fixed mass of gas is directly proportional to its absolute temperature provided volume is constant P α T P = Kt k = P/T P1/T1 = P2/T2
- 5. Calculating absolute temperature Pθ = T T=absolute temperature P0 273 Pθ = Pressure at θ0C P0 = Pressure at 00C Eg Pressure of a gas at 00C is 200cmHg and 250cmHg at 600C Calulate the absolute temperature
- 6. solution 250/200 = T/273 T = 273 x 250 = 341.25K 200
- 7. General gas law Gotten by combination of Boyle’s, Charles, and Pressure law(gay lussac’s) PV = k Boyle’s V/T =k Charles P/T =k Gay Lussac’s PV/T = k P1 V1 = P2 V2 T1 T2
- 8. Eg A certain gas with a volume of 100mm3 at 200 C in a container under pressure of 80mmHg. It was heated to a temperature of 1000 C and its volume increased to 150mm3. What is the pressure of the gas at the new temperature?
- 9. solution P1 V1 = P2 V2 T1 T2 P2 = P1 V1 T2 V2 T1 = 80 x 100 x 100 = 267mmHg 150 x 20
- 10. Dalton’s law of partial pressures Ptotal = PA + PB + PC + .... If there is a mixture of gases which do not combine chemically, then the total pressure exerted by the mixture is the sum of the partial pressures of the individual gases that make up the mixture.
- 11. Vapour density = ½ x relative molecular mass of the gas or vapour Eg what is the VD of CO2? (C = 12, O = 16) =molecular mass of CO2 = 12 + 32 = 44g/mol VD = ½ x 44 = 22
- 12. Graham’s law of difussion At constant temperature and pressure, the rate of diffusion of a gas is inversely proportional to the squareroot of its density. R = 1 √ρ Where 2 gases are involved R1 = ρ2 R2 ρ1 R is also inversely proportional to molecular mass R1 = M2 R2 M1 √ √
- 13. End