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chem > unit 3 vocab > Flashcards

unit 3 vocab Flashcards

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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
Q

viscosity

A

a measure of the resistance of a liquid to flow. increases with molar mass

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26
Q

poise (P)

A

unit used to measure viscosity, 1g/cm*s

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27
Q

capillary action

A

the ability of a liquid to flow against gravity up a narrow tube due to adhesive and cohesive forces

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28
Q

cohesive forces

A

attraction between molecules in a liquid. wants to hold together

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29
Q

adhesive forces

A

attraction between molecules and the surface of the tube. wants to spread out

30
Q

volatile

A

vaporizes easily

31
Q

sublimation

A

solid -> gas

32
Q

vaporization

A

liquid-> gas

33
Q

melting/fusion

A

solid-> liquid

34
Q

deposition

A

gas -> solid

35
Q

condensation

A

gas -> liquid

36
Q

freezing

A

liquid -> solid

37
Q

supercooling

A

when a liquid is cooled below the freezing point but remains liquid

38
Q

boiling point

A

temperature where the vapor pressure of a liquid exceeds external pressure

39
Q

normal boiling point

A

temperature when the vapor pressure equals 1atm

40
Q

critical temperature (Tc)

A

temperature where a liquid can’t exist, regardless of pressure

41
Q

critical pressure (Pc)

A

pressure required to bring about a transition to a liquid at Tc

42
Q

heat of fusion

A

the amount of heat required to melt 1 mol of a solid

43
Q

heat of sublimation

A

amount of heat required to sublime 1 mol of a solid to gas. sum of heat of fusion + heat of vaporization

44
Q

phase diagram

A

a map of the state or phase of a substance as a function of pressure (y axis) and temp (x axis)

45
Q

triple point

A

unique set of conditions where all three phases of a substance are equally stable and in equilibrium

46
Q

solution

A

homogeneous mixture of two substances

47
Q

solvent

A

majority component of a solution

48
Q

solubility

A

amount of a substance that will dissolve in a given amount of solvent

49
Q

entropy

A

a measure of the energy randomization or energy dispersal in a system

50
Q

miscible

A

the ability of two or more substances to be soluble in each other in all proportions

51
Q

enthalpy of solution

A

the enthalpy change associated with the formation of a solution

52
Q

heat of hydration

A

the energy change that occurs when 1 mol of gaseous solute ions is dissolved in water

53
Q

semipermeable membrane

A

membrane that selectively allows some things to permeate but not others

54
Q

osmotic pressure

A

pressure required to stop osmotic flow

55
Q

dynamic equilibrium

A

the point at which the rate of the reverse reaction or process equals the rate of the forward reaction or process

56
Q

saturated solution

A

solution in which the dissolved solute is in dynamic equilibrium with any undissolved solute

57
Q

unsaturated solution

A

solution with less than the equilibrium amount of solute

58
Q

supersaturated solution

A

unstable solution with more than the equilibrium amount of solute dissolved

59
Q

recrystallization

A

common way to purify a solid

60
Q

dilute solution

A

contains a very small amount of solute vs. solvent

61
Q

molarity (M)

A

moles of solute per L of solution

62
Q

molality (m)

A

moles of solute per kg of solvent

63
Q

colligative property

A

a property that depends on the amount of solute but not the type

64
Q

vapor pressure lowering

A

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
Q

ideal solution

A

solute and solvent follow Raoult’s Law at all concentrations

66
Q

freezing point depression

A

effect of a solute that causes a solution to have a lower melting point than the pure solvent

67
Q

boiling point elevation

A

effect of a solute that causes a solution to have a higher boiling point than the pure solvent

68
Q

osmosis

A

flow of a solvent of of lower solute concentration to a solution of higher solute concentration

69
Q

van’t hoff factor

A

ratio of moles of particles in a solution to moles of formula units dissolved

70
Q

colloidal dispersion (colloid)

A

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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