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Ideal gas

AP Chemistry Zumdahl 7E Chapter 5 Notes

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Gas laws
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Ideal gas
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Boyle's law
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Temperature

AP Chemistry A. Allan Chapter 5 - Gases 5.1 Pressure A. Properties of gases 1. Gases uniformly fill any container 2. Gases are easily compressed 3. Gases mix completely with any other gas 4. Gases exert pressure on their surroundings a. Pressure = force/area B. Measuring barometric pressure 1. The barometer a. Inventor - Evangelista Torricelli (1643) 2. Units a. mm Hg (torr) (1) 760 torr = Standard pressure b. newtons/meter2 = pascal (Pa) (1) 101,325 Pa = Standard pressure c. atmospheres (1) 1 atmosphere = Standard pressure 5.2 The Gas Laws of Boyle, Charles, and Avogadro A. Boyle's Law (Robert Boyle, 1627 - 1691) 1. the product of pressure times volume is a constant, provided the temperature remains the same kPV = a. P is inversely related to V

inorganic chemistry lab report Al-Zn alloy

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Water vapor
ideal gas law
Air–fuel ratio
Gas
Hydrogen
Mass fraction

1 Experiment 7: Analysis of Aluminum ?Zinc Alloy Objective: The objective of this experiment is to determine the percent composition of Aluminum in an Aluminum-Zinc Alloy. In addition, we use Excel get the trendline equation of H2 gas and %Al. Method:

inorganic chemistry lab report Al-Zn alloy

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Atmospheric thermodynamics
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Water vapor
ideal gas law
Air–fuel ratio
Gas
Hydrogen
Mass fraction

5 Chemistry 181 Yeting Liu Fall 2014 Thu 7:30 Experiment 7: Analysis of Aluminum ?Zinc Alloy Objective: The objective of this experiment is to determine the percent composition of Aluminum in an Aluminum-Zinc Alloy. In addition, we use Excel get the trendline equation of H2 gas and %Al. Method:

Principles of Chemistry Chapter 5

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Pressure
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Atmospheric pressure
Volume
Ideal gas

Chapter 5: Gases Section 5.2: Pressure Sunday, October 19, 2014 12:43 PM Pressure = Force / Area ? **note: atmospheric pressure is caused by the weight of air molecules as they are attracted by gravity (hence why pressure decreases as altitude decreases) ? Measuring Pressure ? Barometer - device that measures atmospheric pressure Long tube filled with mercury, essentially you pour the mercury out of the tube until it stops because the mercury creates a seal and a vacuum in the closed end of the tube -pressure decreases cause the mercury seal to fall lower -pressure increases cause the mercury seal to fall higher ? Units of Pressure ? Pascal - (Pa) unit for pressure, equal to one Newton / meter squared --> Force / area

Gas Stoich Notes

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thermodynamics
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Ideal gas
Standard conditions for temperature and pressure
Volume
Monatomic gas

preAP Chemistry 2013-2014 1 Name ___________________________ Period ______ I. Avogadro?s Law ? Avogadro?s Law states that ____________ volumes of gases at the __________ temperature and pressure contain equal numbers of particles. - At STP, _________________ particles (1 mol) will have a volume of ___________ Using Avogadro?s Law EX 1: Determine the volume (in L) occupied by 212 g of oxygen at STP. EX 2: Determine the density of nitrogen at STP. II. Ideal Gas Law ? Up to now we have always kept the ______________ of gas constant. Recognize that as the amount of gas changes, its corresponding _________________ changes. (Avogadro?s Law)

Chapter 11

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ideal gas law
Ideal gas
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Van der Waals equation
Environment
behavior
Human development
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Love
Psychoanalysis
Human behavior
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Kinetic Theory Of Gases Postulates of the Kinetic Theory of Gases: A gas consists of a large number of tiny particles that are in constant, random motion The gas particles occupy a net volume so small in relation to the volume of their container that their contribution to the total volume can be ignored The collisions between particles and the walls of the container are perfectly elastic (no energy transfer) Kinetic Theory of Gases relates temperature to average kinetic energy Kinetic Theory of Gases (aka Kinetic Molecular Theory) can be used to explain the Gas Laws: Pressure-Volume Relationship (Boyle?s Law) P? 1/V or V ? 1/P (at constant n, T) Pressure-Temperature Relationship (Guy-Lussac?s Law) ?T, ?v ?v, ?P Volume-Temperature Relationship (Charles?s Law)

Chapter 11

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Chemistry 1210: Introduction to General Chemistry Dr. Gina M. Florio 06 Dec. 2012 Brady, Jespersen, & Hyslop Chapter 11 Properties of Gases Properties of Gases Compressible Low Density Exert Pressure (temperature dependence) Expand Mixable Some common properties of gases: While bulk properties, these intimate a molecular level foundation. Properties of Gases Recall that our understanding of kinetic energy in molecular systems relies on a molecular-level picture of gases. Kinetic Theory of Gases (CH 7) Example: Pressure Units of Pressure Standard atmosphere (atm): the pressure needed to support a column of mercury 760 mm high measures at 0 ?C The SI unit of pressure is the pascal (Pa): Pressure Measurements Open-ended Mercury Manometer:

Gas laws

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A Gas Uniformly fills any container. Mixes completely with any other gas Exerts pressure on its surroundings. A Gas It might help to define a gas based on the other phases as well. -Movie Clip- Kinetic Molecular Theory 1. Volume of individual particles is ? zero. 2. Collisions of particles with container walls cause pressure exerted by gas. 3. Particles exert no forces on each other. 4. Average kinetic energy ? Kelvin temperature of a gas. The Meaning of Temperature Kelvin temperature is an index of the random motions of gas particles (higher T means greater motion.) -Kinetic Energy Video- Pressure is equal to force/unit area SI units = Newton/meter2 = 1 Pascal (Pa) 1 standard atmosphere = 101,325 Pa 1 standard atmosphere = 1 atm = 760 mm Hg = 760 torr atm mmHg torr
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