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Princeton Chemistry > Phases and Gases > Flashcards

Phases and Gases Flashcards

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1
Q

vapor pressure

A
  • the force exerted by the gas particles that vaporize from a solid or liquid sample
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2
Q

vapor pressure depends on

A
  • the substance itself only
  • not external pressure
  • proportional to temperature and KE
  • indirectly proportional to IMF
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3
Q

boiling point

A
  • the temperature at which the condensation/vaporization phase transitions occur
  • when Pvap=Patm
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4
Q

boiling point depends on

A
  • external pressure directly proportional

- intermolecular forces directly proportional

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5
Q

boiling point elevation

A
  • dissolve a solute in a solvent, the additional IMF add more bonds that must be broken to achieve boiling
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6
Q

factors affecting boiling point

A
  • IMF (inc IMF inc BP dec Pvap)
  • Molecular weight (inc MW inc BP)
  • branching (dec branching inc BP)
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7
Q

melting/freezing point

A
  • the temperature at which the fusion/crystallization phase transitions occur
  • same rules as melting point
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8
Q

FP depression

A
  • dissolve a salt in water, the ions act like a road block to water arranging in a regular crystal lattice
  • so, it must get even colder before things will freeze with ions in the way
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9
Q

solute

A
  • present in a small quantity
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10
Q

solvent

A
  • present in a larger quantity

- usually water on the MCAT

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11
Q

strong electrolyte

A
  • complete dissociation
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12
Q

weak electrolyte

A
  • partial dissociation
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13
Q

non-electrolyte

A
  • no dissociation
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14
Q

van’t hoff factor

A
  • the number of particles produced in solution per mole of substance
  • number of particles it breaks down into when it dissolves
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15
Q

electrolytes dissolve in water

A
  • agitation (endothermic) - breaking bonds
  • dissociation (endothermic) - breaking bonds
  • solvation (exothermic) - forming bonds IMF
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16
Q

polar non-electrolytes dissolve in water

A
  • agitation (endothermic)

- solvation (exothermic)

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17
Q

nonpolar non-electrolytes do not dissolve in water

A
  • agitation (endothermic)

- won’t dissolve.

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18
Q

solubility

A
  • the amount of a substance that can dissolve in a specific solvent AT A SPECIFIC TEMPERATURE
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19
Q

unsaturated solution

A
  • concentration of solute < solubility

- additional solute can still dissolve

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20
Q

saturation solution

A
  • concentration of solute = solubility

- no additional solute will dissolve

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21
Q

supersaturated solution

A
  • concentration of solute > solubility

- additional solute causes excess to precipitate

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22
Q

solids and liquids in water

A
  • solubility directly proportional to temperature

- not affected by pressure

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23
Q

gaseous solutes in water

A
  • solubility indirectly proportional to temperature

- directly proportional to pressure

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24
Q

always soluble

A
  • group 1 ions
  • H+
  • NH4+
  • NO3-
  • CH3COO- (acetate)
  • ClO4-
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25
usually insoluble
- Ag+ - Pb2+ - Pb4+ - Hg2 2+ - Hg2+ - Co3 2- - PO4 3- - S2-
26
strength of IMFs
- solids > liquids > gases > ideal gases
27
liquid to gas
- vaporization (boiling)
28
gas to liquid
- condensation
29
solid to liquid
- fusion (melting)
30
liquid to solid
- crystallization (freezing)
31
solid to gas high imf to low imf
- sublimination - heat absorbed - internal KE increases - entropy increases - dec IMF
32
gas to solid low imf to high imf
- deposition - heat released - Internal KE decreases - entropy decreases - inc IMF
33
boundary line between two phases
- all the T/P points at which the two phases exist in equilibrium
34
triple point
- the one T&P when all three phases coexist in equilibrium
35
critical point
- the T&P above which the different between liquid and gas is no longer distinct - properties of both liquid and gas
36
phase diagram of water
- same general trend of other phase diagrams except negative slope at solid-liquid boundary - freezing point/melting point of ice decreases under increasing pressure (how we are able to ice skate)
37
density
- measure of how condensed a substance is | - p=m/V
38
density affected by
- external pressure directly proportional to density - external temperature indirectly proportional to density - IMF directly proportional to density
39
formulas for heat
q=mcΔT (for temperature change) q=nΔH_phase change (for phase change) CANNOT HAPPEN AT THE SAME TIME!
40
inverse of slope on heating curve
- equals c | - smaller slope = higher heat capacity
41
potential energy and IMF
- PE increases as IMFs break
42
ideal gas
- has no IMFs - particles with negligible volume compared to their container size - an average KE proportional to its temperature - elastic collisions between particles and container walls (creates pressure) - favored with high temperature and low pressure since interactions of the particles are minimized
43
ideal gas law
PV=nRT R=0.08 V=22.4L at or near 1 atm, 273K
44
units for pressure
- 1 atm = 101 kPa = 760 torr = 760 mm Hg
45
units for volume
- 1L = 1000 mL = 1000 cm^3 = 0.001 m^3
46
units for temperature
- must be absolute temperature scale or kelvin | - C + 273=K
47
Avagadro's law
- V=n - V is proportional to n at a given P and T regardless of the identity of the gas PlATe - Avo at P and T
48
Boyle's law
- P = 1/V - P1V1=P2V2 BAT - Boyle at T and n
49
Charle's law
- T = V - V1/T1=V2/T2 - CAP - Charles at Pressure and n
50
Gay-Lussac's Law
- P = T | - P1/T1=P2/T2
51
combined gas law
- P1V1/T1 = P2V2/T2 - number of moles are still constant - temp must be in K
52
non- ideality
- P_ideal > P_real - V_ideal > V_real - because the particles of a real gas DO experience IMF, their paths are deviated and thus the frequency of collisions on the container wall will result in a lower pressure - because particles of a real gas DO have physical size, they take up space in the container and thus the free space in the container is smaller
53
Real Gas Law
(P + an^2/V^2)(V-nb) = nRT - a increases as IMFs of a gas get stronger - b increases as the size of a gas particle increases
54
Dalton's law
- P_total = Pa+Pb+Pc......Pn | - the total pressure of a mixture of gases is equal to the sum of their partial pressures
55
mole fraction
- Pa=XaP_total where Xa=na/n_total
56
grahams law of diffusion/effusion
rate of gas 1 = sqrt (molar mass of gas 1) _________________________________ rate of gas 2 (molar mass of gas 2) - heavy particles move slowly - light particles move quickly
57
formula for density
p=m/v
58
STP
- 0 degrees Celsius | - 1 ATM
59
standard state
- 25 degrees Celsius | - 1 ATM.
60
mantra for ideal versus real
- ideal world is always greater than the real world.

Princeton Chemistry (6 decks)

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