Term
| What are the three assumptions of the kinetic theory as it applies to gases? |
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Definition
| the particles in a fas are considered to be small, hard spheres with an insignificant volume. The motion of the particles in a fas is rapid, constant, and random. All collisions between particles in a gas are perfectly elastic. |
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Term
| How does kinetic theory explain gas pressure? |
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Definition
| gas pressure is the result of simultaneous collisions of billions of rapidly moving particles in a gas with an object. |
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Term
| What is the relationship between the temperature in kelvins and the average kinetic energy of particles? |
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Definition
| 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
| the energy an object has because of its motion. |
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Term
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Definition
| all matter consists of tiny particles that are in constant motion. |
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Definition
| results from the force exerted by a gas per unit surface area of an object. |
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Term
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Definition
| an empty space with no particles and no pressure. |
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Definition
| results from the collisions of atoms and molecules in air with objects. |
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Definition
| a device that is used to measure atmospheric pressure. |
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Term
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Definition
| the SI unit of pressure. It represents a very small amount of pressure. |
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Term
| Standard atomosphere (atm) |
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Definition
| the pressure required to support 760mm of mercury in a mercury barometer at 25C. |
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Term
| What factors determine the physical properties of a liquid? |
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Definition
| the interplay between the disruptive motions of particles in a liquid and the attractions among the particles determines the physical properties of liquids. |
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Term
| What is the relationship between evaporation and kinetic energy? |
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Definition
| during evaporation, only those molecules with a certain minimum kinetic energy can escape from the surface of the liquid. |
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Term
| When can a dynamic equilibrium exist between a liquid and its vapor? |
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Definition
| in a system at constant vapor pressure, a dynamic equilibrium exists between the vapor and the liquid. The system is in equilibrium because the rate of evaporation of liquid equals the rate of condensation of vapor. |
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Term
| Under what conditions does boiling occur? |
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Definition
| whan 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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Term
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Definition
| the conversion of a liquid to a gas or vapor. |
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Term
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Definition
| when vaporization occurs at the suface of a liquid that is not boiling. |
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Term
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Definition
| a measure of the force exerted by a gas above a liquid. |
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Term
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Definition
| the temperature at which the vapor pressure of the liquid is just equal to the external pressure on the liquid. |
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Term
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Definition
| defined as the boiling point of a liquid at a pressure of 101.3kPa. |
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Term
| How are the structure and properties of solids related? |
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Definition
| the general properties of solids reflect the orderly arrangement of their particles and the fixed locations of their particles. |
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Term
| What determines the shape of a crystal? |
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Definition
| the shape of a crystal reflects the arrangement of the particles within the solid. |
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Term
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Definition
| the temperature at which a solid changes into a liquid. |
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Term
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Definition
| the particles are arranged in an orderly, repeating, three-dimensional pattern called a crystal lattice. |
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Term
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Definition
| the smallest group of particles within a crystal that retains the geometric shape of the crystal. |
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Term
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Definition
| two or more different molecular forms of the same element in the same physical state. |
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Definition
| lacks an ordered internal structure. Ex: rubber, plastic, glass, and asphalt |
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Term
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Definition
| a transparent fusion product of inorganic substances that have cooled to a rigid state without crystallizing. |
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Term
| When can sublimation occur? |
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Definition
| sublimation occurs in solids with vapor pressures that exceed atmospheric pressure at or near room temperature. |
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Term
| How are the conditions at which phases are in equilibrium represented on a phase diagram? |
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Definition
| the conditions of pressure and temperature at which two phases exist in equilibrium are indicated on a phase diagram by a line separating the phases. |
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Term
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Definition
| the change of a substance from a solid to a vapor without passing through the liquid state. |
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Term
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Definition
| a graph showing the conditions at which a substance exists as a solid, liquid, or vapor. |
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Term
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Definition
| describes the only set of conditions at which all three phases can exist in equilibrium with one another. |
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