chemistry 101 - section h solids, liquids, and especially gases this presentation was created by...
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![Page 1: Chemistry 101 - Section H Solids, Liquids, and Especially Gases This presentation was created by Professor Carl H. Snyder Chemistry Department University](https://reader036.vdocuments.mx/reader036/viewer/2022062518/56649e2e5503460f94b1f0a9/html5/thumbnails/1.jpg)
Chemistry 101 - Section HSolids, Liquids, and Especially
Gases• This presentation was created by
Professor Carl H. SnyderChemistry DepartmentUniversity of MiamiCoral Gables, FL [email protected]
• Copyright 2003 by Carl H. Snyder, University of Miami. All rights reserved.
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Chapter 12 - Solids, Liquids, and Especially Gases
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Solids, Liquids, and Gases
• Solids - maintain their own volumes and shapes
• Liquids - maintain their own volumes but take the shapes of their containers
• Gases - maintain neither their own volumes nor shapes, but take both the volumes and shapes of their containers.
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Why Solids Melt, Liquids Boil• When we heat a substance, we add energy to
its chemical particles.• This energy makes their particles move,
vibrate, rotate, etc., faster … in every way.
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Melting Point
• Melting - Solid to liquid
• Freezing - Liquid to solid
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Boiling Point
• Boiling - Liquid to gas throughout the entire mass of the liquid.
• Evaporation - Liquid to gas only at the surface• Condensation - Gas to liquid
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Evaporation
• Evaporation occurs when molecules with high translational energies escape from the surface of the liquid.
• Evaporation can occur at temperatures far below the boiling point
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Sublimation
• The disappearance of snow at temperatures too cold for melting to occur takes place through sublimation.
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The Gas We Live In
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The Composition of Dry Air
• Dry air is roughly 80% N2, 20% O2, and traces of other gases.
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Atmospheric Pressure• The total mass of all the
atmosphere above any give point on or above the earth’s surface produces the atmospheric pressure at that point.
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Measuring Atmospheric Pressure
• The barometer, an instrument for measuring atmospheric pressure
• Invented by Evangelista Torricelli
• 1643
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The Kinetic-Molecular Theory
• What happens when you pump up a tire -- and much more -- is explained by the kinetic-molecular theory of gases.
• Kinetic (moving) molecular (molecules) = moving molecules.
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The Basis of The Kinetic-Molecular Theory
• All gases are composed of atoms or molecules that are in constant motion, richocheting off each other and off walls like billiard balls.
• The higher the temperature, the faster the atoms or moleucles move.
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The Cast of Characters
• Each of these scientists contributed to our understanding of the behavior of gases.
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Robert Boyle
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A Statement of Boyle’s Law
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Illustrations of Boyle’s Law
• Double the pressure on a fixed quantity of gas held at constant temperature, and its volume decreases to half.
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Boyle’s Law and The Kinetic-Molecular Theory of Gases
• As we decrease the volume of a constant quantity of gas molecules (kept at constant temperature), the moving molecules hit the sides of their container more often.
• This results in a higher pressure.
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Jacques Alexandre Cesar Charles
• Q: But . . . what value of temperature shall we use?
• A: The Kelvin temperature.
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William Thomson, Lord Kelvin• William Thomson,
Lord Kelvin, gave us the Kelvin temperature scale.
• The Kelvin temperature scale begins at absolute zero and move upward in degrees the same size as those of the Celsius scale.
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Charles’ Law and The Kinetic-Molecular Theory of Gases
• As we decrease the temperature, the gas molecules move with less energy.
• If we keep the pressure constant, the volume of the gas decreases.
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Can the Volume of a Gas Drop to Zero?
• No, because the gas laws apply strictly only to ideal gases.
• A real gas will condense to a liquid before it reaches absolute zero.
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Combining Boyle’s Law and and Charles’ Law
• Combining Boyle’s Law and Charles’ Law, we get the combined gas law equation.
• P1 V1 and T1 apply to one set of condition, P2 V2 and T2 apply to a second set of conditions.
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Joseph Louis Gay-Lussac
• Gay-Lussac’s Law can be restated to: When gases react with each other, the ratio of their reacting volumes is the same as the ratio of their reacting molecules.
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Amedeo Avogadro
• At a constant pressure and temperature, the volume a gas occupies is directly proportional to the number of molecules (or number of moles) of the gas that’s present.
• This is the same Avogadro who gave us Avogadro’s number
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Demonstrating Avogadro’s Law
• Blow into a balloon (increase the value of n) and
the balloon gets larger (the value of V increases).
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John Dalton
• The total pressure of all the gases in a mixture of several gases is the sum of the pressures exerted by each of the individual gases -- the sum of their individual partial pressures.
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The Partial Pressures of the Air We Breathe
• Notice that the sum of these partial pressures is 760 mm-Hg, which is our standard atmospheric pressure.
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William Henry
• If the partial pressure of a gas above a liquid is low, very little of the gas dissolves in the liquid.
• If the partial pressure of a gas above a liquid is high, plenty of the gas dissolves in the liquid.
• We can describe the concentration of the dissolved gas in the liquid by using the partial pressue of the gas above the liquid.
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The Laws of a Bottle of SodaPart I
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The Laws of a Bottle of SodaPart II
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The Art and Science of Breathing
• We metabolize glucose (and other nutrients) for energy.
• Body cells require O2 as a reactant.
• Body cells produce CO2 as a product.
• Our blood must supply oxygen and remove carbon dioxide.
• The gas laws come into play in the process.
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The Physiology of the Lungs
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Blood Transports O2 and CO2 Between the Alveolae and the
Cells
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Partial Pressures of Blood Gases
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End - Chapter 12