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43 Cards in this Set
- Front
- Back
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Kinetic Energy |
The energy an object has because of its motion |
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Kinetic Theory |
All matter consists of tiny particles that are in constant motion |
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Shape of gas particles |
Small, hard spheres with an insignificant volume |
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Motion of gas |
Rapid, constant, random |
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Collisions between gas particles |
No energy gained or lost, total kinetic energy remains constant |
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Gas pressure |
The force exerted by a gas per unit surface area of an object |
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Cause of gas pressure |
Simultaneous collisions of billions of rapidly moving particles in gas with an object |
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Vacuum |
An empty space with no particles and no pressure |
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Atmospheric pressure |
Results from the collisions of atoms and molecules in air with objects |
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Barometer |
A device used to measure atmospheric pressure |
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Pascal (Pa) |
The SI unit of pressure |
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Standard atmosphere (atm) |
The pressure required to support 760 mm of mercury in a Mercury barometer at 25 degrees Celsius |
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Atm=mm Hg=kPa |
1 atm = 760 mm Hg = 101.3 kPa |
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Kelvin temperature of a substance to average kinetic energy of its particles |
Directly proportional |
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What determines the physical properties of liquids |
The interplay between the disruptive motions of particles in a liquid and the attractions among the particles |
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Vaporization |
The conversion of a liquid to a gas or vapor |
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Evaporation |
When a liquid turns to a gas or vapor without the surface of a liquid boiling |
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What happens during evaporation |
During evaporation, only those molecules with a certain minimum kinetic energy can escape from the surface of a liquid |
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Vapor Pressure |
A measure of the force exerted by a gas above a liquid |
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Liquid to a vapor (gas) |
Evaporation |
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Vapor (gas) to a liquid |
Condensation |
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Dynamic Equilibrium |
Occurs in a system at constant vapor pressure between the vapor and the liquid because the rate of evaporation of liquid equals the rate of condensation of a vapor |
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Boiling |
When a liquid is heated to a temperature at which particles throughout the liquid have enough kinetic energy to vaporize |
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Boiling point |
The temperature at which the vapor pressure of the liquid is just equal to the external pressure on the liquid |
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Boiling point |
The temperature at which the vapor pressure of the liquid is just equal to the external pressure on the liquid |
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Normal boiling point |
The boiling point of a liquid at a pressure of 101.3 kPa |
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Boiling point |
The temperature at which the vapor pressure of the liquid is just equal to the external pressure on the liquid |
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Normal boiling point |
The boiling point of a liquid at a pressure of 101.3 kPa |
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General properties of solids |
Orderly arrangement of their particles and the fixed locations of their particles |
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Melting point |
The temperature at which a solid changed into a liquid |
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Solid to liquid |
Melting |
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Solid to liquid |
Melting |
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Liquid to solid |
Freezing |
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Crystal |
The particles are arranged in an orderly, repeating, three dimensional pattern called a crystal lattice |
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Shape of a crystal to the structure of a crystal |
The shape of a crystal reflects the arrangement of the particles within the solid |
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Unit cell |
The smallest group of particles within a crystal that retains the geometric shape of the crystal |
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Allotropes |
Two or more different molecular forms of the same element in the same physical state |
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Amorphous solid |
Lacks an ordered internal structure (rubber, plastic, asphalt) |
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Glass |
A transparent fusion product of inorganic substances that have cooled to a rigid state without crystallizing |
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Sublimation |
The change of a substance from a solid to a vapor without passing through the liquid state |
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When sublimation occurs |
Sublimation occurs in solids with vapor pressures that exceed atmospheric pressure at or near room temperature |
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Phase Diagram |
A diagram that shows the relationships among the solid liquid, and vapor states (or phases) of a substance in a sealed container on a single graph |
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Triple point |
The point on the diagram at which all three curves meet |
