Gases

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Freezing-point depression

Colligative properties

Boiling-point elevation

1 BA A A nn nxcomponentAoffractionMole +== Chapter 11 ? Properties of Solutions 11.1 Solution Composition A. Molarity 1. solutionofliters solutemolesMMolarity =)( B. Mass Percent 1. 100? ?? ? ? ? ?? ? ? ? = solutionofmass soluteofmasspercentMass C. Mole Fraction 1. D. Molality 1. solventoframki soluteofmolesMolality log = E. Normality 1. solutionofliter sequivalentNormality = 2. Equivalents of acids and bases a. Mass that donates or accepts a mole of protons 3. Equivalents of oxidizing and reducing agents a. Mass that provides or accepts a mole of electrons 11.2 The Energies of Solution Formation A. ?Like Dissolves Like? 1. Polar molecules and ionic compounds tend to dissolve in polar solvents 2. Nonpolar molecules dissolve in nonpolar compounds

AP Chemistry Zumdahl 7E Chapter 10 Notes

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Chemical bonding

Materials science

intermolecular forces

Enthalpy of vaporization

Boiling point

1 Chapter 10 - Liquids and Solids 10.1 Intermolecular Forces A. Dipole-Dipole Forces 1. Attraction between molecules with dipole moments a. Maximizes (+) ----- ( - ) interactions b. Minimizes (+) ----- ( + ) and (-) ----- ( - ) interactions 2. About 1% of strength of ionic bonds a. Unimportant in gas phase due to distance between molecules B. Hydrogen Bonding 1. Special dipole-dipole attraction a. Hydrogen covalently bonded to highly electronegative elements (N, O, F) has a higher than normal d+ charge 2. Bond strength is higher than other dipole-dipole attractions 3. Important in the bonding of molecules such as water and DNA C. London Dispersion Forces 1. Instantaneous dipoles a. Random movement of electrons can create a momentary

AP Chemistry Zumdahl 7E Chapter 5 Notes

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Gas

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

Principles of Chemistry Chapter 5

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Physical chemistry

Gas laws

Gas

Volume

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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Standard conditions for temperature and pressure

Gas

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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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:

Bob Jones PPT Notes -- Chapter 10a

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Physics

thermodynamics

Fluid dynamics

Vacuum

Properties of Gases Kinetic Theory of Gases Many independent particles Random motion at high speed Separated by great distances Kinetic Theory of Gases Interact only when they collide 5. Elastic collisions Physical Properties of Gases Diffusion Effusion Permeability Compressibility Expansibility Diffusion spontaneous mixing due to particle motion Effusion gas particles passing through a tiny opening into an evacuated area Both diffusion and effusion are directly related to the speed of the gas molecules. rate of effusion for gas 1 Graham?s Law of Effusion rate of effusion for gas 2 = molar mass2 molar mass1 molar massN = 28.02 g/mol Sample Problem 1 Calculate the ratio of effusion rates between nitrogen (N2) and Argon (Ar). molar massAr = 39.95 g/mol rate of effusion for gas 1

Gas laws

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Physics

Gas laws

Ideal gas

Gas

Volume

Partial pressure

Environment

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

States of Matter

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Physics