13.2 Up Up And Away
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The document discusses the behavior of gases and how their volume and pressure change with temperature. It explains that Charles' Law states that for a fixed amount of gas, volume is proportional to temperature. The Pressure Law similarly states that for a fixed amount of gas, pressure is proportional to temperature. The document indicates that experiments will be conducted to observe how the volume and pressure of a gas change when temperature is increased and the results are recorded.
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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:
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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.
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This document provides an overview of several gas laws:
- Boyle's Law states that the pressure and volume of a gas are inversely proportional at constant temperature.
- Charles' Law explains that the volume of a gas is proportional to the Kelvin temperature if pressure remains constant.
- The Combined Gas Law combines Boyle's, Charles', and Gay-Lussac's Laws to relate the pressure, volume, temperature, and amount of gas.
- According to Avogadro's Law, equal volumes of gas at the same temperature and pressure contain the same number of particles.
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The document discusses the gas laws of Boyle's law, Charles' law, and Gay-Lussac's law. Boyle's law states that the pressure and volume of a gas are inversely proportional at constant temperature. Charles' law describes the direct proportionality of volume and temperature at constant pressure. Gay-Lussac's law found the direct relationship between pressure and temperature when volume is kept constant. The document also defines ideal gases as having no particle volume or intermolecular forces, while real gases do have particle volume and intermolecular attractive forces.
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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.
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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.
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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.
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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.
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- Charles' Law explains that the volume of a gas is proportional to the Kelvin temperature if pressure remains constant.
- The Combined Gas Law combines Boyle's, Charles', and Gay-Lussac's Laws to relate the pressure, volume, temperature, and amount of gas.
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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.
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3) Gay-Lussac's law relates temperature and pressure at constant volume - as temperature increases, pressure increases.
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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.
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This document discusses quantum numbers which describe the location of electrons within an atom. There are four quantum numbers: 1) the principal quantum number (n) indicates the energy level, 2) the azimuthal quantum number (l) indicates the orbital type, 3) the magnetic quantum number (ml) represents a specific orbital based on the l value, and 4) the spin quantum number (s or ms) indicates the spin direction of the electron as either up or down. Examples are provided to demonstrate writing the full set of quantum numbers for various atoms.
Crayfish classroom slides
Crayfish have identifiable structures that serve different functions for survival. These include eyes, antennae, walking legs, a tail, and a carapace. Males and females can be differentiated based on structures like swimmerets and pincers.
To thrive, crayfish require a habitat that provides food, clean water, shelter, and space. In the classroom, crayfish were kept in tubs with elodea plants, cat food, and plastic cups for shelter.
Through observations, students learned crayfish behaviors like hiding in shelters. Crayfish were found to be territorial and would defend their preferred hiding places and locations in the habitat.
Tang 09 intermolecular forces and solubility
This document discusses intermolecular and intramolecular forces. It describes that intramolecular forces are the forces within a molecule that form covalent bonds. Intermolecular forces are the weaker forces between molecules and include London dispersion forces, dipole-dipole forces, and hydrogen bonding. London dispersion forces exist between all molecules and depend on the number of electrons. Dipole-dipole forces exist between polar molecules. Hydrogen bonding is the strongest intermolecular force and occurs when hydrogen is bonded to fluorine, oxygen, or nitrogen. Intermolecular forces influence properties such as melting point, boiling point, solubility, and surface tension.
Independent gas laws investigation
This document provides instructions and assessment criteria for students to design an experiment investigating the relationships between temperature, volume, and pressure in gases. Students will spend 5 lessons developing their experiment, which includes generating a question and hypothesis, designing a method, collecting and analyzing data, and evaluating their results. The document includes detailed rubrics to guide students in earning high marks by thoroughly explaining their question, hypothesis, method, data analysis, and evaluation.
Tang 04 periodic trends
1) Atomic radius generally increases down a group and decreases across a period due to shielding effects of additional electron shells and increasing nuclear charge, respectively.
2) Ionization energy generally increases down a group and across a period as it becomes increasingly difficult to remove an electron due to greater nuclear attraction from less shielding and more protons. Exceptions occur when removing an electron would destabilize a full shell.
3) Electronegativity generally increases across a period as the effective nuclear charge felt by valence electrons increases with fewer shielding shells and more protons.
Tang 06 bond energy
- Chemical reactions involve breaking old bonds and forming new ones. Bond breaking requires energy and is endothermic, while bond formation releases energy and is exothermic.
- The bond energies table lists the average energy required to break common types of bonds. However, bond energies can vary depending on neighboring bonds.
- Reaction enthalpy change (ΔH) can be calculated by adding the bond energies of reactants and subtracting the bond energies of products. This was demonstrated for combustion reactions of ethanol and methoxymethane.
Tang 06 vsepr
VSEPR (Valence Shell Electron Pair Repulsion) theory describes the shapes of individual molecules based on the number of electron pairs around a central atom. It predicts 13 different geometries including linear, bent, trigonal planar, tetrahedral and octahedral. The theory states that electron pairs around an atom will repel each other and adopt a shape that minimizes repulsions between these pairs.
Introduction to Simple Machines
This document discusses simple machines and how they help humans do work. It defines simple machines as tools with few or no moving parts that change the amount or direction of force. The document lists and describes six simple machines: the lever, inclined plane, wedge, screw, wheel and axle, and pulley. It provides examples of each machine and explains how compound machines combine two or more simple machines to help with work.
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23 gases
- Gases have negligible volume and molecules are far apart with mostly empty space between them. Gas molecules move randomly in straight lines and collide elastically.
- The kinetic molecular theory describes gas properties including high translational energy of gas molecules that move randomly in all directions.
- Pressure, volume, temperature of gases are directly or inversely related as described by Boyle's, Charles', and Gay-Lussac's laws and the combined gas law.
fluid.docx
The document summarizes an experiment to examine the relationship between pressure and temperature as described by Gay-Lussac's law. The experiment was simulated using an online simulation program. The simulation showed that as temperature increased from 50K to 400K at a constant volume of 270 cubic meters, the pressure also increased in a linear fashion from 13513 pascals to 108080 pascals, validating the direct proportionality predicted by Gay-Lussac's law. However, the document notes that a real-world experiment may yield different results than a simulation due to gases not being truly perfect.
Gas Laws
Kinetic Gas Theory including Ideal Gas Equation. Temperature, Volume, Applications
Boyle's Law, Charles' Law and Avogadro's Law. Ideal Gas Theory, Dalton's Partial Pressure
Kinetic theory of gases C-1 PHYSICAL CHEMISTRY (1) .pdf
This document discusses the key principles of the kinetic theory of gases and gas laws. It begins by defining gases and their properties, then covers the kinetic theory which explains gas behavior at the molecular level. The document then thoroughly explains the four main gas laws: Boyle's law relating pressure and volume, Charles' law relating volume and temperature, the combined gas law, and Avogadro's law relating volume and amount of gas. Examples are provided for each law to demonstrate how to apply the mathematical relationships.
3.2 gas laws
The document discusses several gas laws:
- Boyle's law states that at constant temperature, the volume of a gas is inversely proportional to its pressure.
- Charles' law states that at constant pressure, the volume of a gas is directly proportional to its kelvin temperature.
- Combined gas law allows calculation of gas properties when temperature and/or pressure change.
It also discusses concepts like the kinetic molecular theory of gases and how real gases deviate from ideal gas behavior due to intermolecular forces and molecular size. Sample calculations demonstrate use of the gas laws and kinetic theory.
ιδανικα αερια και μεταβολες
The document provides an overview of key concepts in thermodynamics including:
- The four laws of thermodynamics, which relate to heat transfer, energy conservation, entropy, and the impossibility of reaching absolute zero temperature
- Ideal gas behavior and the ideal gas law, which relates pressure, volume, temperature and moles of gas
- Thermodynamic processes like isobaric, isochoric, isothermal and adiabatic that involve constant properties
- Using pressure-volume diagrams to visualize gas behavior and calculate work
Chemistry notes ideal gas laws
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.
Unit 4: Behavior of Gases
Gas laws
Boyle's Law
Charles' Law
Guy Lussac's Law
Combined Gas Law
Avogadro's Law
The Ideal Gas Law
Grade 10
2-7 Gas Laws
The document discusses the gas laws and how temperature, pressure, and volume of a gas are related. It defines key terms like pressure, temperature, and volume. It explains Boyle's law, Charles' law, and the combined gas law. Boyle's law states that if temperature and amount of gas are kept constant, pressure and volume are inversely related. Charles' law states that if pressure and amount of gas are kept constant, volume and temperature are directly related. The combined gas law incorporates all factors - if temperature increases while amount and volume remain constant, pressure will also increase.
Liyue.pptx
This document discusses gas laws and the behavior of gases. It introduces Boyle's law, which states that the pressure and volume of a gas are inversely proportional at constant temperature. Charles' law is described as stating the volume and absolute temperature of a gas are directly proportional at constant pressure. Gay-Lussac's law holds that pressure and absolute temperature of a gas are directly proportional at constant volume. Sample problems demonstrate using these gas laws and the ideal gas law to calculate unknown values like pressure, volume, temperature. The learning goals are to describe and apply the gas laws and ideal gas law to calculations.
Physics ib ia
This document summarizes an investigation into the behavior of gases at different temperatures, pressures, and volumes. Three experiments were conducted: 1) Boyle's law experiment showing an inverse relationship between pressure and volume at constant temperature, 2) Charles' law experiment showing a direct relationship between volume and temperature at constant pressure, and 3) Gay-Lussac's law experiment showing a direct relationship between pressure and temperature at constant volume. The results of the experiments validated the theoretical gas laws and supported the conclusion that the volume, pressure, and temperature of gases are mutually related as described by the general gas equation.
Thermal 3.2
1. Pressure of a gas is caused by particle collisions with the container walls. Higher temperature means higher particle kinetic energy, causing more frequent and forceful collisions and higher pressure.
2. Boyle's law states that at constant temperature, pressure and volume of a gas are inversely proportional. Charles' law says volume and temperature are directly proportional at constant pressure. Gay-Lussac's law finds pressure and temperature directly proportional at constant volume.
3. These gas laws can be combined into the ideal gas law: pV = nRT, relating pressure, volume, amount of gas, temperature, and the universal gas constant. This law approximates gas behavior except at low temperatures or high pressures.
Intro-to-Gases-and-Gas-Laws-Gen-Chem-1.pptx
The kinetic molecular theory of gases explains gas behavior using the idea that gases are made of molecules or atoms that are in constant, random motion and have space between them. It describes gases as having no intermolecular forces, occupying no volume, and undergoing elastic collisions. This theory allows for deriving gas laws such as Boyle's law (inverse relationship between pressure and volume at constant temperature), Charles's law (direct relationship between volume and temperature at constant pressure), and Gay-Lussac's law (direct relationship between pressure and temperature at constant volume). The combined gas law incorporates all three simpler gas laws. These gas laws allow for calculations involving pressure, volume, temperature, and amount of gas.
Combined-Avogadros-and-Ideal-Gas-Laws [Autosaved].pptx
The document discusses the Combined Gas Law, which states that the pressure and volume of a gas are inversely proportional to each other and directly proportional to temperature. It provides the mathematical equation relating these variables and explains how to use it to calculate changes in pressure, volume, or temperature when one of the variables is unknown. Sample problems demonstrate how to apply the law to practical situations.
23 gases
Gases are composed of molecules that are far apart from each other and occupy the entire volume of their container. Gas molecules move randomly in straight lines and collide elastically with each other and the container walls. The kinetic molecular theory describes gases as having negligible intermolecular forces and volume. Pressure, volume, temperature of a gas are related by the combined gas law and ideal gas law. Gas calculations involve using stoichiometry, the ideal gas law, and gas laws like Boyle's, Charles', and Gay-Lussac's to determine volume, pressure, amount, or temperature changes.
13.3 Up Up And Away
The document discusses the gas laws and how they relate to buoyancy and the behavior of gases. It introduces the gas laws of Charles, Boyle, pressure and combines them into the ideal gas law of pV=nRT. It then gives examples of using the ideal gas law to calculate volume given pressure, temperature and moles of gas. The key ideas are that gases provide buoyancy by displacing denser gases based on differences in weight, and that the gas laws can be combined into pV=nRT to relate pressure, volume, temperature and amount of gas.
Gas laws
1. The document summarizes several gas laws: Boyle's law describes the inverse relationship between the pressure and volume of a gas at constant temperature. Charles's law describes the direct relationship between volume and temperature of a gas at constant pressure. Gay-Lussac's law describes the direct relationship between pressure and temperature of a gas at constant volume. The combined gas law incorporates all three relationships.
2. Sample problems demonstrate applying the gas laws to calculate unknown pressure, volume, or temperature given values for two variables. Formulas are provided for deriving relationships between the variables under each gas law.
1. Gas Laws.ppt
This document provides an overview of key gas laws:
- Boyle's law relates pressure and volume, stating their product remains constant if temperature and amount of gas stays the same.
- Charles' law describes how volume and temperature directly relate, with their quotient staying constant at constant pressure and gas amount.
- The ideal gas law combines these, relating pressure, volume, temperature, and amount of gas in one equation.
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
Lecture on thermodynamics
This document provides an overview of thermodynamics concepts. It defines thermodynamics as dealing with energies of gases and vapors in terms of heat and work. It describes three types of thermodynamic systems - closed, open, and isolated. It also defines extensive and intensive properties. The document then explains the zeroth, first, and second laws of thermodynamics. It concludes by describing various thermodynamic processes like isobaric, isothermal, adiabatic, and throttling processes.
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13.2 Up Up And Away
- 1. Matter Very Simple Up, Up and Away
- 4. But what happens if we change temperature..?
- 5. Changes in Temperature, Changes in Volume Increase the temperature and record the length of the gas column etc. 40 30 20 Length Temperature
- 7. Changes in Temperature, Changes in Pressure Increase the temperature and record the pressure etc. 40 30 20 Pressure Temperature