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HS Chemistry > UNIT FIVE > Flashcards

UNIT FIVE Flashcards

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1
Q

kinetic-molecular theory of gases

A

particles of matter are always in motion

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2
Q

ideal gas

A

imaginary gas that perfectly fits all assumptions of kinetic-molecular theory

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3
Q

assumptions of kinetic-molecular theory

A

1) gases consist of many tiny particles that are far apart
2) collisions between gas particles, particles, container walls are elastic (no net loss of kinetic energy)
3) in constant, rapid motion
4) no forces of attraction/repulsion between particles
5) average kinetic energy of gas particles depends on temperature (KE=1/2 mass x speed)

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4
Q

expansion

A

fills container

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5
Q

fluidity

A

gas particles slide easily due to few attractive forces

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6
Q

low density

A

particles very far apart

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7
Q

compressibility

A

initially far apart can be pushed together

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8
Q

diffusion

A

spontaneous mixing of particles of 2 substances caused by random motion and depends on particle speed, diameter, attractive forces

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9
Q

effusion

A

process where gas particles under pressure pass through tiny openings and is directly proportional to particle velocity

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10
Q

barometer

A

measures atmospheric pressure

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11
Q

Boyle’s Law

A

P1V1 = P2V2

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12
Q

Charles’ Law

A

V1/T1 = V2/T2

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13
Q

Gay-Lussac’s Law

A

P1/T1 = P2/T2

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14
Q

Combined Law

A

(P1V1)/T1 = (P2V2)/T2

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15
Q

Ideal Gas Law

A

PV = nRT

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16
Q

Avogadro’s Law

A

equal volume of gases at the same temperature and pressure has the same number of molecules

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17
Q

gas standard molar volume

A

volume occupied by 1 mole of gas at standard temperature and pressure

18
Q

Graham’s Law of Effusion

A

rate of effusion of gases at same temperature and pressure are inversely proportional to their square root molar masses

19
Q

liquid

A

form of matter that has definite volume and takes shape of container

20
Q

fluid

A

substance that can flow and take the shape of its container

21
Q

properties of liquids

A
  • relatively high density
  • relative incompressibility
  • ability to diffuse
  • surface tension
  • evaporation
  • boiling
22
Q

crystalline solids

A

consists of many crystal (most solids) and particles are pattered orderly, geometric and repeating

23
Q

amorphous solids

A

particles arranged randomly such as plastic and gas

24
Q

equilibrium

A

dynamic condition where two opposite charges occur at closed rates in equal rates

25
Q

Le-Chatelier’s Principle

A

when equilibrium system is disturbed y application of stress, it attains new equilibrium that minimizes stress

26
Q

volatile liquids

A

liquids that evaporate easily

27
Q

molar heat of vaporaization

A

energy required to vaporize one mole of liquid at boiling point, high when intermolecular forces are strong

28
Q

molar heat of fusion

A

energy required to melt one mole of solid at melting point

29
Q

phase diagrams

A

graph of pressure versus temperature, shows conditions under which phases exist

30
Q

triple point of a substance

A

indicates temperature and pressure conditions when solid, liquid, and vapour coexist at equilibrium

31
Q

solution

A

uniform mixture of two or more substances

32
Q

solvent

A

component of a solution present in largest amount

33
Q

solute

A

components of solution present in smaller amounts than solvent

34
Q

solute

A

components of solution present in smaller amounts than solvent

35
Q

electrolyte

A

substance that dissolves in water and creates conductive solution, includes all soluble ionic compounds and highly polar molecular compounds

36
Q

nonelectrolyte

A

dissolves but does not create conductivity, eg sugar

37
Q

solution equilibrium

A

physical state in which opposing process of dissolution and crystallization occur at equal rates

38
Q

saturated solution

A

contains maximum amount of dissolved solute

39
Q

supersaturated solution

A

contains more dissolved solute in same conditions

40
Q

Henry’s Law

A

solubility of gas in a liquid is directly proportional to partial pressure of that gas on surface of liquid

41
Q

molality

A

amount of solute (moles, n) divided by mass (m) of solvent in kg

m=n/m

42
Q

molarity

A

amount of solute divided by volume

M=n/V

HS Chemistry (6 decks)

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