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chem > unit 3 vocab > Flashcards

unit 3 vocab Flashcards

(70 cards)

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1
Q

pressure

A

the amount of force per unit area. F/A

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2
Q

barometer

A

an evacuated glass tube, the tip of which is submerged in a pool of mercury. used to measure pressure

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3
Q

torr

A

a millimeter of mercury (Hg)

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4
Q

manometer

A

u-shaped tube containing a dense liquid, usually mercury. used to measure the pressure of a sample relative to atmospheric pressure

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5
Q

boyle’s law

A

volume is proportional to 1 divided by pressure

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6
Q

charles’ law

A

volume is proportional to temperature

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7
Q

avogadro’s law

A

volume is proportional to number of moles

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8
Q

ideal gas law

A

PV=nRT

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9
Q

ideal gas

A

hypothetical gas that exactly follows the ideal gas law

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10
Q

molar volume of an ideal gas at STP

A

22.4 L

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11
Q

STP

A

standard temperature and pressure

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12
Q

partial pressure

A

the pressure due to any individual component in a gas mixture (Pn)

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13
Q

mole fraction

A

the number of moles of a component in a mixture divided by the total number of moles in the mixture

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14
Q

vapor pressure

A

the partial pressure of water vapor in a gas from the gas collection process after a chemical reaction

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15
Q

dalton’s law

A

the total pressure of a gas mixture is the sum of the partial pressures of its components

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16
Q

kinetic molecular theory

A
  1. particles are negligibly small in volume but have mass
  2. the average kinetic energy of a particle is proportional to the temperature in kelvins, atom’s motion is due to thermal energy
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17
Q

kinetic molecular theory

A
  1. particles are negligibly small in volume but have mass
  2. the average kinetic energy of a particle is proportional to the temperature in kelvins, atom’s motion is due to thermal energy
  3. when particles collide, there’s no loss of energy
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18
Q

mean free path

A

the average distance that a molecule travels in between collisions. increases as pressure decreases

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19
Q

diffusion

A

the process by which gas molecules spread out in response to a concentration gradient. influenced by the root mean square velocity

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20
Q

effusion

A

the process by which a gas escapes from a container into a vacuum through a small hole

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21
Q

graham’s law of effusion

A

rate A/rate B = square root of MB/MA

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22
Q

amorphous

A

a solid in which the atoms don’t have an sort of long-range order

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23
Q

miscibility

A

a liquid’s ability to mix without separating into two states

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24
Q

surface tension

A

the energy required to increase the surface area of a liquid by a unit amount. decreases as intermolecular forces decrease

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25
viscosity
a measure of the resistance of a liquid to flow. increases with molar mass
26
poise (P)
unit used to measure viscosity, 1g/cm*s
27
capillary action
the ability of a liquid to flow against gravity up a narrow tube due to adhesive and cohesive forces
28
cohesive forces
attraction between molecules in a liquid. wants to hold together
29
adhesive forces
attraction between molecules and the surface of the tube. wants to spread out
30
volatile
vaporizes easily
31
sublimation
solid -> gas
32
vaporization
liquid-> gas
33
melting/fusion
solid-> liquid
34
deposition
gas -> solid
35
condensation
gas -> liquid
36
freezing
liquid -> solid
37
supercooling
when a liquid is cooled below the freezing point but remains liquid
38
boiling point
temperature where the vapor pressure of a liquid exceeds external pressure
39
normal boiling point
temperature when the vapor pressure equals 1atm
40
critical temperature (Tc)
temperature where a liquid can't exist, regardless of pressure
41
critical pressure (Pc)
pressure required to bring about a transition to a liquid at Tc
42
heat of fusion
the amount of heat required to melt 1 mol of a solid
43
heat of sublimation
amount of heat required to sublime 1 mol of a solid to gas. sum of heat of fusion + heat of vaporization
44
phase diagram
a map of the state or phase of a substance as a function of pressure (y axis) and temp (x axis)
45
triple point
unique set of conditions where all three phases of a substance are equally stable and in equilibrium
46
solution
homogeneous mixture of two substances
47
solvent
majority component of a solution
48
solubility
amount of a substance that will dissolve in a given amount of solvent
49
entropy
a measure of the energy randomization or energy dispersal in a system
50
miscible
the ability of two or more substances to be soluble in each other in all proportions
51
enthalpy of solution
the enthalpy change associated with the formation of a solution
52
heat of hydration
the energy change that occurs when 1 mol of gaseous solute ions is dissolved in water
53
semipermeable membrane
membrane that selectively allows some things to permeate but not others
54
osmotic pressure
pressure required to stop osmotic flow
55
dynamic equilibrium
the point at which the rate of the reverse reaction or process equals the rate of the forward reaction or process
56
saturated solution
solution in which the dissolved solute is in dynamic equilibrium with any undissolved solute
57
unsaturated solution
solution with less than the equilibrium amount of solute
58
supersaturated solution
unstable solution with more than the equilibrium amount of solute dissolved
59
recrystallization
common way to purify a solid
60
dilute solution
contains a very small amount of solute vs. solvent
61
molarity (M)
moles of solute per L of solution
62
molality (m)
moles of solute per kg of solvent
63
colligative property
a property that depends on the amount of solute but not the type
64
vapor pressure lowering
the change in vapor pressure that occurs in pure substances upon addition of a solute. directly proportional to the mole fraction of the solute
65
ideal solution
solute and solvent follow Raoult's Law at all concentrations
66
freezing point depression
effect of a solute that causes a solution to have a lower melting point than the pure solvent
67
boiling point elevation
effect of a solute that causes a solution to have a higher boiling point than the pure solvent
68
osmosis
flow of a solvent of of lower solute concentration to a solution of higher solute concentration
69
van't hoff factor
ratio of moles of particles in a solution to moles of formula units dissolved
70
colloidal dispersion (colloid)
a mixture in which a dispersed substance is finely dived but not truly dissolved in a dispersing medium. ex. fog, smoke, milk

chem (15 decks)

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