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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
Q

usually insoluble

A
  • Ag+
  • Pb2+
  • Pb4+
  • Hg2 2+
  • Hg2+
  • Co3 2-
  • PO4 3-
  • S2-
26
Q

strength of IMFs

A
  • solids > liquids > gases > ideal gases
27
Q

liquid to gas

A
  • vaporization (boiling)
28
Q

gas to liquid

A
  • condensation
29
Q

solid to liquid

A
  • fusion (melting)
30
Q

liquid to solid

A
  • crystallization (freezing)
31
Q

solid to gas

high imf to low imf

A
  • sublimination
  • heat absorbed
  • internal KE increases
  • entropy increases
  • dec IMF
32
Q

gas to solid

low imf to high imf

A
  • deposition
  • heat released
  • Internal KE decreases
  • entropy decreases
  • inc IMF
33
Q

boundary line between two phases

A
  • all the T/P points at which the two phases exist in equilibrium
34
Q

triple point

A
  • the one T&P when all three phases coexist in equilibrium
35
Q

critical point

A
  • the T&P above which the different between liquid and gas is no longer distinct
  • properties of both liquid and gas
36
Q

phase diagram of water

A
  • 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
Q

density

A
  • measure of how condensed a substance is

- p=m/V

38
Q

density affected by

A
  • external pressure directly proportional to density
  • external temperature indirectly proportional to density
  • IMF directly proportional to density
39
Q

formulas for heat

A

q=mcΔT (for temperature change)
q=nΔH_phase change (for phase change)

CANNOT HAPPEN AT THE SAME TIME!

40
Q

inverse of slope on heating curve

A
  • equals c

- smaller slope = higher heat capacity

41
Q

potential energy and IMF

A
  • PE increases as IMFs break
42
Q

ideal gas

A
  • 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
Q

ideal gas law

A

PV=nRT

R=0.08
V=22.4L at or near 1 atm, 273K

44
Q

units for pressure

A
  • 1 atm = 101 kPa = 760 torr = 760 mm Hg
45
Q

units for volume

A
  • 1L = 1000 mL = 1000 cm^3 = 0.001 m^3
46
Q

units for temperature

A
  • must be absolute temperature scale or kelvin

- C + 273=K

47
Q

Avagadro’s law

A
  • 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
Q

Boyle’s law

A
  • P = 1/V
  • P1V1=P2V2

BAT - Boyle at T and n

49
Q

Charle’s law

A
  • T = V
  • V1/T1=V2/T2
  • CAP - Charles at Pressure and n
50
Q

Gay-Lussac’s Law

A
  • P = T

- P1/T1=P2/T2

51
Q

combined gas law

A
  • P1V1/T1 = P2V2/T2
  • number of moles are still constant
  • temp must be in K
52
Q

non- ideality

A
  • 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
Q

Real Gas Law

A

(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
Q

Dalton’s law

A
  • P_total = Pa+Pb+Pc……Pn

- the total pressure of a mixture of gases is equal to the sum of their partial pressures

55
Q

mole fraction

A
  • Pa=XaP_total where Xa=na/n_total
56
Q

grahams law of diffusion/effusion

A

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
Q

formula for density

A

p=m/v

58
Q

STP

A
  • 0 degrees Celsius

- 1 ATM

59
Q

standard state

A
  • 25 degrees Celsius

- 1 ATM.

60
Q

mantra for ideal versus real

A
  • ideal world is always greater than the real world.

Princeton Chemistry (6 decks)

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