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MCAT chem > phases gases and solutions > Flashcards

phases gases and solutions Flashcards

1
Q

basic phases of matter

A

solid liquids and gases

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2
Q

what forces determine which phase a substance will be in?

A

intermolecular forcers

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3
Q

solid

A

phase with rigid and tighly packed atoms
- fixed volume and noncompressible
- crystalline or amorphous

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4
Q

lattice energy

A

amount of energy required to disrput the crystalline structure of a salt into cations and anions

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5
Q

amorphous solids

A

solids without a crystalline structure (glass and silcone)

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6
Q

liquid

A

phase with fixed volume and are not compressible but do not have a fixed shape

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7
Q

viscocity

A

property of liquids: resistance to flow

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8
Q

gas

A

phase with no fixed volume or shape
- compressible

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9
Q

compressibility

A

lack of fixed volume (only a property of gases)

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10
Q

phase change

A

when substance transitions from one phase to another

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11
Q

melting/fusion

A

solid to liquid

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12
Q

freezing

A

liquid to solid

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13
Q

evaporation/boiling

A

liquid to gas

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14
Q

condensation

A

gas to liquid

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15
Q

sublimation

A

solid to gas

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16
Q

deposition

A

gas to solid

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17
Q

endothermic phase changes

A

melting, evaporating, sublimation
require heat input
breaking bonds

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18
Q

exothermic reactions

A

freezing, condensation, deposition
release heat
forming bonds

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19
Q

is bond formation exothermic or endothermic

A

exothermic

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20
Q

heat of fusion

A

point in phase change where the added heat is no longer increasing the temperature and is focused on breaking the intermolecular forces

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21
Q

heat of vaporization

A

heat required to convert liquid to gas where temperature is no longer rising and heat is focused on breaking intermolecular forces of liquid

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22
Q

specific heat capacity

A

amount of heat required to raise the temperature of one unit mass of a substance by 1 degree

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23
Q

specific heat equation

A

Q = mc ∆T
q is heat, m is mass, c is specific heat capacity

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24
Q

heat at phase changes

A

typically a ratio because temperature remains constant

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25
Q

heat between phase changes

A

q= mc ∆T

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26
Q

how can a gas be converted into solid

A

increase in pressure or decrease in temperature

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27
Q

what phase changes are promoted by a decrease in pressure and an increase in temperature

A

solid to liquid
liquid to gas
solid to gas

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28
Q

triple point

A

point at which solids liquid and gases are at equillibrium

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29
Q

critical point

A

end of the liquid-gas interface
- above this point the substance exsist as a supercritical liquid

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30
Q

high tempertaure and low pressure promotes which phase

A

gas

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31
Q

low temp and high pressure favors which phase

A

solid

32
Q

vapor pressure

A

gas is in equillibrium with liquid

33
Q

gas @ STP

A

volume 22.4L

34
Q

ideal gas

A
  1. average KE of gas molecules is proportional to temperature
  2. gas particle has no volume
  3. gas particles do not exert attractive forces on one another , although they do exert forces on the container they are in –> all collisions are elastic
35
Q

when do gases deviate from ideal gas law?

A

at high pressure and low temperature

36
Q

when do gases behave most ideal?

A

low pressures and high temperatures

37
Q

boyle’s law

A

pressure and volume of a gas are inversely proportional at constant temperature
V1P1=V2P2

38
Q

what happens to the pressure of a gas if the volume increases

A

pressure decreases

39
Q

charles law

A

volume and temperature of a gas are directly proportional under constant pressure
V1/T1 = V2/T2

40
Q

what happens to the volume of a gas if the temperature is increased at constant pressure

A

volume with increase with temperature

41
Q

ideal gas law

A

PV=nRT
n is number of moles of gas
R is gas constant

42
Q

mole fraction

A

Ngas/Ntotal

43
Q

partial pressure

A

pgas/Ptotal

44
Q

Dalton’s Law

A

Pgas = Xgas*Ptotal
partial pressure of gas = total p * moles of gas

45
Q

solution

A

homogenous mixture

46
Q

dissolutions

A

solutes dissolved in solvent

47
Q

supersaturated

A

excess solute not dissolved

48
Q

crystallization

A

supersaturated solute creates nucleation site for solute to parcipitate out and form a cyrstal

49
Q

molarity

A

mols solute/ L solution

50
Q

molality

A

moles of solute/ Kg solvent

51
Q

normality (N)

A

number of equivilent reactive species per liter of solution
N= equivelent solute/ L solution

52
Q

normality for acids

A

N = molarity * (# of H+ in acid)

53
Q

colligative properties

A

vapor pressure reduction
boiling point elevation
freezing pt reduction
osmotic pressure

54
Q

Raoult’s Law

A

P=XaPa
p is vaport pressure of solution
Pa is vapor pressure of pure solvent
Xa is mole fraction of solvent

55
Q

boiling point elevation

A

∆T= iKb*m
- t is change in boiling point elevation
- i is ionization factor
- kb is boiling point constant
- m is molal solute conc

56
Q

reducing vapor pressure does what to boiling point

A

increases

57
Q

what does added solute do to the freezing point

A

decreases

58
Q

freezing point depression eqn

A

∆Tf= iKf*m

59
Q

osmotic pressure

A

Π= iMRT
pressure required to prevent osmosis
M= n solute/ L solution

60
Q

solubility

A

equillibrium process between nondissolved and dissolved forms of substance

61
Q

equillibrium constant (Ksp)

A

solubility product constant [p][p]

62
Q

high ksp

A

substance readily dissolves into solution

63
Q

low ksp

A

largely insoluble

64
Q

common ion effect

A

decrease in solubility of an ionic compound by adding a solute compound with an ion in the precipitate

65
Q

are alkali metals soluble

A

yes

66
Q

are nitrates soluble

A

yes

67
Q

are chlorates soluble

A

yes

68
Q

are halides soluble

A

yes

69
Q

is AgCl soluble

A

no

70
Q

is PbAg soluble

A

no

71
Q

is HgI soluble

A

no

72
Q

are carbonates (CO3 2-) soluble

A

no

73
Q

PO4 2- soluble?

A

no

74
Q

OH- compounds soluble?

A

no

75
Q

is caoh2 soluble?

A

soluble

76
Q

is baoh soluble

A

yes, exception to rule

MCAT chem (11 decks)

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