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Chem Sem 2 > Assignment 6 > Flashcards

Assignment 6 Flashcards

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1
Q

properties of a gas

A

volume

density

mass/amount/moles

pressure

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2
Q

IMFs (what do they determine)

A

determine physical properties

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3
Q

Particle Theory/Kinetic Molecular Theory

A

particles…

are meaured in moles (6.02 x 1023)

have mass

are the smallest representative unit of a substance that contain the properties of the larger substance

travel randomly in a straight line

speed indicate its heat

have no IMFs (ideal gas assumption)

collide with each other and the walls of the container (measured by vol and pressure)

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4
Q

particles

A

the smallest representative unit of a substance that contains the properties of the larger substance

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5
Q

ideal gas assumption

A

no IMFs

PV = nRT

theoretical

no freezing/boiling point

no energy (heat) lost

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6
Q

Relationship of Pressure to Volume

A

Inverse

same # particles + more volume/space = less bumping of particles = less pressure

same # particles + less volume/space = more bumping = more pressure

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7
Q

Relationship of Pressure to Temperature

A

Direct (if you start at absolute zero)

more temp = more movement of particles = more bumping = more pressure

less temp = less movement of particles = less bumping = less pressure

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8
Q

Relationship of Temperature to Volume

A

Direct (if you start at absolute zero)

more temp = more motion = more collision = more push on conainer = more volume

less temp = less motion = less collision = less push on conainer = less volume

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9
Q

Relationship of Number of Moles (n) to Pressure/Temperature/Volume

A

Direct

more moles = more mass = more vol

more moles = more particles in same space = more bumping = more pressure

more moles = more particles bumping = more KE/heat = more temp

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10
Q

Proportionality Constant R =

A
  1. 0821 (for atm)
  2. 314 (for kPa)
  3. 396 (for mmHg/torr)
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11
Q

what happens as a system is cooled

A

density increases

kinetic energy (temp) decreases

pressure decreases

volume decreases

particles squish together (IMFs became important, no ideal gas assumptions no equations)

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12
Q

solid

A

low KE

IMFs > KE of particles

incompressable

maintains shape and vol

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13
Q

liquid

A

medium KE

IMFs ≈ KE of particles

incompressable

constant vol, variable shape

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14
Q

gas

A

high KE

IMFs (essentially zero) < KE

compressable

no set vol or shape

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15
Q

boyle’s law

A

P1V1 = P2V2

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16
Q

charles’ law

A

V1/T1 = V2/T2

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17
Q

Gay-Lussac’s Law

A

P1/T1 = P2/T2

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18
Q

gas law equation for descriptive and changing moles

A

PV = nRT

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19
Q

gas law equation for changing conditions, constant moles

A

P1V1 P2V2

———— = nR = ———-

T1 T2

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20
Q

mole fraction equation

A

Px nx

—————— = —————–

PTOTAL nTOTAL

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21
Q

PV = nRT

A

gas law equation for descriptive and changing moles

22
Q

P1V1 P2V2

———— = nR = ———-

T1 T2

A

gas law equation for changing conditions, constant moles

23
Q

density (at STP) =

A

gfm

22.4

24
Q

density (not at STP) =

A

P(gfm)

RT

25
Q

Dalton’s Law of Partial Pressures

A

sum of the pressures in a vessel for a mixture of gases depend only on the pressures of the individual gases

PTOTAL = P1 + P2 + … + Pn

26
Q

Graham’s Law (of Diffusion and Effusion)

A

smaller things diffuse faster

27
Q

diffusion

A

particles move from high concentration to low concentrations until they are equal

28
Q

effusion

A

particles will move from a pressurized space to a non-pressurized space (vaccum)

29
Q

temperature

A

measure of avg kinetic energy

30
Q

STP

A

standard temp (0ºC/273K) and pressure (1atm/101.3kPa/760mmHg/760torr)

31
Q

vapor

A

small airborne particles of liquid (not molecules like gas)

intermediary between gas and liquid

gas where liquid phase is present

32
Q

dynamic equilibrium

A

evaporation rate = condensation rate

33
Q

evaporation

A

no external energy added

automatically occurs with any liquid

34
Q

vapor pressure

A

partial pressure of vapor above any liquid

temp dependent: higher temp = higher avg KE = more particles have ability to leave = higher vapor pressure

35
Q

boiling

A

PTOTAL = PVAPOR

atmospheric pressure = vapor pressure

36
Q

freezing

A

phase change from liquid to solid

37
Q

melting

A

phase change from solid to liquid

38
Q

condensation

A

phase change from gas to liquid

39
Q

vaporization

A

phase change from liquid to gas

40
Q

sublimation

A

phase change from solid to gas without passing through liquid

41
Q

desposition

A

phase change from gas to solid without passing through liquid

42
Q

triple point

A

temp and pressure where all phases (solid, liquid, gas) occur simultaneously

43
Q

equilibrium

A

the temp and pressure where two phases exist simultaneously

44
Q

critical point

A

temp above which the substance is always a gas

45
Q

when do ideal gases behave like actual gases

A

at high temp/volume or low pressure

46
Q

1 atm =

A

101.3 kPa = 760 mmHg = 760 torr

47
Q

2 bonds + electron pairs

A

linear

sp

48
Q

3 bonds + electron pairs

A

trigonal planar

sp2

49
Q

4 bonds + electron pairs

A

tetrahedral

sp3

50
Q

5 bonds + electron pairs

A

bipyramidal

sp3d

51
Q

6 bonds + electron pairs

A

octahedral symmtery

sp3d2

Chem Sem 2 (6 decks)

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