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| The energy of an object because it has motion. |
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| All matter consists of tiny particles that are in constant motion. |
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| Assumptions from the Kinetic Molecular Theory for Gases |
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Definition
| *Key Concept: The particles in a gas are considered to be small, hard spheres with insignificant volume.* *Key Concept: The motions of particles in a gas is rapid, constant and rapid.* *Key Concept: All collisions between particles of gas are perfectly elastic.* |
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| A result from the force exerted by the gas per units of surface area on an object. *Key Concept: Gas pressure is the result of simultaneous collisions of billions of rapidly moving particles in a gas with an object.* |
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Definition
| An empty sace with no particles and no pressure. |
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| The result of collisions of gas molecules in the air with objects. |
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Definition
| A device used to measure atmospheric pressure. |
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Definition
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| Standard Atmosphere (atm) |
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Definition
| the pressure required to support 760 mm of mercury in a barometer at 25*C |
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| Average Kinetic Energy and Kelvin Temperature |
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Definition
| *Key Concept: The Kelvin Temperature of a substance is directly proportional to the average kinetic energy of the particles of the substance. |
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Definition
| *Key Concept: The interplay between the disruptive motions of particles in a liquid and the attractions among particles determine the physical properties of a liquid.* |
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Definition
| The conversion of a liquid to a gas. |
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| When vaporization occurs to a liquid below its boiling point. *Key Concept: During evaporation, only those molecules with a certain minimum kinetic energy will evaporate.* |
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Definition
| *key Concept: In a system at constant vapor pressure, a dynamic equilibrium exists between the vapor and liquid. The system is in equilibrium because the rate of evaporation equals the rate of consdensaation of a gas.* |
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Definition
| The temperature at which the vapor pressure of the liquid is just equal to the external pressure of the liquid. *Key Concept: When a liquid is heated to a temperature at which particles throughout the liquid have enough kinetic energy to vaporize, the liquid begins to boil.* |
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Definition
| The boiling point of a liquid at 101.3 kPa.(See table 13.2 page 395) |
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Definition
| *key Concept: The general properties of a solid reflect the orderly arrangement of their particles and the fixed locations of their particles.* |
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Definition
| The temperature at which a solid changes to a liquid. |
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Definition
| *Key concept: The shape of a crystal reflects the arrangement of the particles within the solid.* |
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Term
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Definition
| two or more differant molecuar forms of the same element in the same physical state. |
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Definition
| Lacks order in the internal structure. |
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Definition
| A rigid set of inorganic molecules that have been heated and cooled without crystallizing. |
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Definition
| The change of a solid to a gas without becoming a liquid. *Key Concept: Aublimation occurs in solids when the vapor pressures exceed atmospheric pressure near or at room temperature.* |
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Definition
| The graph which shows the relationshp among the solids liquids and gasses of a substance in a sealed container. *Key Concept: The conditions of pressure and temperature at which two phases exist in equilibrium are represented by a line or curve on the graph.* |
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Definition
| The point on a phase diagram at which all three phases exist in equilibrium. |
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