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School > Chemistry - Chapter 13 > Flashcards

Chemistry - Chapter 13 Flashcards

1
Q

kinetic energy

A

the energy an object has because of its motion

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2
Q

kinetic theory

A

all matter consists of tiny particles that are in constant motion

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3
Q

what are the three assumptions of the kinetic theory as it applies to gases? (3)

A
  1. the particles in a gas are considered to be small, hard spheres with an insignificant volume
  2. the motion of the particles in a gas is rapid, constant, and random
  3. all collisions between particles in a gas are perfectly elastic
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4
Q

How does kinetic theory explain gas pressure?

A

gas pressure is the result of billions of rapidly moving particles in a gas simultaneously colliding with an object

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5
Q

gas pressure

A

results from the force exerted by a gas per unit surface area of an object

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6
Q

vacuum

A

an empty space with no particles and no pressure

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7
Q

atmospheric pressure

A

the collisions of atoms and molecules in air with objects

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8
Q

what happens to the atmospheric pressure if elevation went up? down? (2)

A

up = atmospheric pressure decreases b/c the density of Earth’s atmosphere decreases as the elevation increases

down = atmospheric pressure increases b/c the density of Earth’s atmosphere increases as the elevation decreases

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9
Q

barometer

A

device used to measure atmospheric pressure

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10
Q

what does atmospheric pressure depend on?

A

weather and altitude

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11
Q

pascal (Pa)

what does it represent?

A

SI unit of pressure

represents a very small amount of pressure

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12
Q

what are the 3 mathematical conversions?

A

1 atm = 760mm Hg = 101.3kPa

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13
Q

standard atmosphere (atm)

A

the pressure required to support 760mm of mercury in a mercury barometer at 25 degrees Celcius

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14
Q

what is the standard temperature and pressure (STp) are defined as…?

A

a temp. of 0 degrees Celcius and a pressure of 101.3kPa, or 1 atm

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15
Q

what is the relationship between the temperature in kelvins and the average kinetic energy of particles?

A

the Kelvin temperature of a substance is directly proportional to the average kinetic energy of the particles of the substance

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16
Q

Relationship between the average kinetic energy of the particles and the substance’s temperature?

A

they are directly related to each other

  • increase in average kinetic energy of the particles cause the temp. of a substance to rise
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17
Q

what is absolute zero? (3)

A

(0 K, or -273.15 degrees Celsius)

the temp at which the motion of particles theoretically ceases

no temp. can be lower than absolute zero

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18
Q

what states of matter are known as condensed states of matter? (2)

why?

A

liquids and solids

b/c increasing pressure on either of them will have little to no effect on them

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19
Q

what is the relationship between evaporation and kinetic energy?

A

during evaporation, only those molecules with a certain minimum kinetic energy can escape from the surface of the liquid

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20
Q

vaporization

A

the conversion of a liquid to a gas or vapor

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21
Q

evaporation

A

vaporization that occurs at the surface of a liquid that is not boiling

22
Q

vapor pressure

A

a measure of the force exerted by a gas above a liquid

23
Q

when can a dynamic equilibrium exist between a liquid and its vapor?

A

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

24
Q

what happens to the particles in equilibrium?

A

the particles in the system continue to evaporate and condense, but no net charge occurs in the number of particles in the liquid or vapor.

25
Q

what will happen when there is a rise in the temperature of a contained liquid?

A

an increase in vapor pressure, b/c the particles in the warmed liquid have increased kinetic energy

26
Q

volatile

A

how easy it will melt

27
Q

what liquid is the most / least volatile?

A

most = diethyl

least = water

28
Q

what is used to measure vapor pressure?

A

manometer

29
Q

under what conditions does boiling occur?

A

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

30
Q

boiling point

A

the temp. at which the vapor pressure of the liquid is just equal to the external pressure on the liquid

31
Q

what happens to a liquid in an open container? (3)

A

the rate of evaporation increased as heat is applied

heating allows a greater number of particles to overcome the attractive forces that keep them in the liquid state

average kinetic energy increases and the temp. rises

32
Q

b/c atmospheric pressure is lower at high altitudes…?

A

boiling points decrease at higher altitudes

33
Q

at a lower external pressure…?

A

the boiling point decreases

34
Q

at a higher external pressure…?

A

the boiling point increases

35
Q

what kind of a process is boiling?

A

a cooling process

36
Q

normal boiling point

A

the boiling point of a liquid at a pressure of 101.3kPa

37
Q

Difference b/t crystalline structure of diamond and graphite? (2)

A

Diamond = each carbon atom in the interior of the diamond is strongly bonded to 4 others and the array is rigid and compact

Graphite = has carbon atoms that are linked in widely spaced layers of hexagonal arrays

38
Q

melting point

A

the temp. at which a solid changes into a liquid

39
Q

freezing point

A

the temp. at which a liquid changes into a solid

40
Q

the melting and freezing points of a substance are… (2)

A

at the same room temp. At that temp., the liquid and solid phases are in equilibrium

41
Q

crystal

A

the particles are arranged in an orderly, repeating, 3-D pattern called a lattice

42
Q

unit cell

A

the smallest group of particles within a crystal that retains the geometric shape of the crystal

43
Q

allotropes (3)

A

two or more molecular forms of the same element in the same physical state

composed of atoms of the same element but we have different properties b/c of diff. structures

44
Q

amorphous solid

A

lacks an ordered internal structure

atoms are randomly arranged

45
Q

glass

A

a transparent fusion product of inorganic substances that have cooled to a rigid state without crystallizing

  • doesn’t melt, it gradually heats up and softens.
46
Q

when can sublimation occur?

A

in solids with vapor pressures that exceed atmospheric pressure at or near room temperature

47
Q

sublimation

A

the change of a substance from a solid to a vapor without passing through the liquid state

48
Q

which type of solid is likely to have the lowest melting point – an ionic solid or a molecular solid? Explain.

A

a molecular solid b/c the attractive forces holding them together are weak

49
Q

how are the conditions at which phases are in equilibrium represented on a phase diagram?

A

the conditions of pressure and temperature at which two phases exist in equilibrium are indicated on a phase diagram by a line separating the two regions representing the phases

50
Q

phase diagram

A

gives the conditions of temperature and pressure at which a substances exists as a solid, liquid, or gas (vapor)

51
Q

triple point

A

describes the only set of conditions at which all of the three phases can exist in equilibrium with one another

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