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Chemistry > Unit 2: Gases, Liquids, and Solids > Flashcards

Unit 2: Gases, Liquids, and Solids Flashcards

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1
Q

pressure

A

the force exerted by a gas on a container

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2
Q

what are the four units of pressure? Which two are honors level?

A
  • mmHg
  • torr
  • atm
  • kPa
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3
Q

Name the three characteristics of a gas

A
  • uniformly fills any container
  • mixes completely with any other gas
  • exerts pressure on it’s surroundings
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4
Q

the amount of pressure exerted is dependent on the…

A

kinetic energy of the particles

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5
Q

Name the four parts of the Kinetic Molecular Theory

A
  1. All gases move in random, straight-line motion separated by empty space
  2. Collisions between gas particles will result in a transfer of energy, but the overall energy remains constant. Collisions of particles with container walls cause the pressure exerted by gas.
  3. Volume of an individual particle is approx. 0
  4. Particles exert no forces on each other
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6
Q

real gases have…

A

volume, mass, and have an attraction for other particles.

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7
Q

under what conditions of pressure and temperature do you have to correct for ideal gas behavior?

A

low temperature and high pressure

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8
Q

what is vanderwaal’s equation

A

corrected pressure x corrected volume = nRT

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9
Q

what is the purpose of vanderwaal’s equation?

A

to correct real gases to give the exact pressure and volume of an ideal gas.

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10
Q

what is the universal or ideal gas law?

A

PV = nRT

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11
Q

what is the expression for corrected pressure?

A

observed pressure minus ‘a’ times (‘n’ divided by volume)^2

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12
Q

what is the expression for corrected volume?

A

the observed volume minus ‘n’ times ‘b’

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13
Q

what is the constant ‘a’ from vanderwaal’s equation related to?

A

related to pressure, specific to that gas

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14
Q

what is the constant b related to?

A

related to the attraction between molecules, also specific to the gas.

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15
Q

what does ‘n’ stand for?

A

the number of moles

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16
Q

what does ‘M’ stand for?

A

GFM, i.e. gram formula mass, molar mass… etc.

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17
Q

what is the “formula” for pressure?

A

force/area

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18
Q

when temperature increases, KE increases, and pressure…

A

increases

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19
Q

effective collision

A

a collision that creates a new product (some collisions are not strong/direct enough to break bonds and change the structure of the particles)

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20
Q

What does GFM stand for? What are some other names for it?

A

gram formula mass

  • molecular mass
  • formula weight
  • molar mass
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21
Q

what are the units for GFM?

A

grams per mole (g/mol)

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22
Q

what is the ‘state’ of a gas?

A

the condition of the gas at a given time

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23
Q

what is the universal/ideal gas law and what is it used for?

A

PV = nRT, an equation of state for a gas

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24
Q

are moles applicable to sig figs??

A

NOO

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25
Q

formula for moles?

A

grams of substance / GFM of substance

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26
Q

what is a hydrate?

A

a substance where water is part of the equation, connected with a not-multiplication sign.

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27
Q

anhydrate?

A

version of a hydrate with the water removed.

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28
Q

what unit of pressure MUST be used with the ideal gas law?

A

atm. If it is kPa, CONVERT IT

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29
Q

what is the constant R?

A

0.0821

30
Q

what unit of temperature must be used for PV = nRT and V/T?

A

Kelvin, convert if Celsius

31
Q

ideal gases/ideal gas model

A

where the volume of the gas particles are negligible and there are no attractive forces between ideal gas particles because of the amount of space between them.

32
Q

under what conditions of temp and pressure would a real gas behave like an idea one?

A

high temperature and low pressure

33
Q

under what conditions will an ideal gas behave like a real one?

A

low temperature and high pressure.

34
Q

what is the formula for density in terms of molar mass and the ideal gas law?

A

D = (MP/RT)
remember- PRESSURE MUST BE IN UNITS OF atm
- TEMP MUST BE KELVIN

35
Q

law of partial pressures

A

in a sealed container with a mixture of different gases, each type of gas exerts it’s own pressure. The pressure exerted by each gas is called partial pressure.

36
Q

how to find total pressure

A

add up all the partial pressures

37
Q

the partial pressure of each gas in a mixture (when you have the total pressure) is dependent on the…

A

number of moles

38
Q

how to find the partial pressure

A
  • multiply the total pressure by the number of moles of the gas you want the pressure of divided by the total number of moles
  • OR plug into original equation and subtract their totals to find it
39
Q

how many torr and mmHg are in 1 atm?

A

760

40
Q

Avogadro’s Hypothesis

A

Equal volume of different gases at the same temperature and pressure have an equal # of molecules

41
Q

how many particles are in one mole of gas?

A

6.02 x 10^23

42
Q

how many Liters are in one mole of gas at STP?

A

22.4 L

43
Q

STP

A

Standard temperature and pressure (273 K and 1 atm/ 101.3 kPa

44
Q

how would you find the GFM of one element

A

it is just the number of atoms present x the atomic mass. BE CAREFUL - TAKE NOTE OF THE DIATOMIC ELEMENTS

45
Q

EQUAL VOLUME =

A

EQUAL PRESSURE

46
Q

What is the combined gas law formula?

A

P1V1/T1 = P2V2/T2

47
Q

what temperature unit must you use with the combined gas law?

A

kelvin

48
Q

do units for pressure and volume matter when using the combined gas law?

A

NOPE

49
Q

what is boyle’s law?

A

P1V1 = P2V2, where T is constant

50
Q

why does boyle’s law hold precisely only at very low pressures?

A

because the gas would behave more ideal

51
Q

what equipment did they use to find Boyle’s law?

A

a J-tube

52
Q

charles’s law

A

the volume of a gas is directly proportional to temperature and extrapolates to 0 at 0 kelvin

53
Q

what is formula for charles’s law?

A

V1/T1 = V2/T2

54
Q

what is Avogadro’s law?

A

for a gas at constant temperature and pressure, the volume is directly proportional to the number of moles of gas.

55
Q

what is the formula for Avogadro’s law, derived from PV = nRT

A

V = an

56
Q

diffusion

A

describes the mixing of gases. the rate of diffusion is the rate of gas mixing.

57
Q

effusion

A

the passage of gas into an evacuated chamber.

58
Q

what factors effect diffusion and effusion rates?

A

particle size and density.

59
Q

what is Graham’s Law of Diffusion/Effusion

A

sqrt(M2)/sqrt(M1) (for the THEORETICAL) rate

60
Q

properties of liquids

A
  • stronger intermolecular forces of attraction that gases
  • indefinite shape
  • definite volume
  • all liquids EVAPORATE at their surface
  • if T increases there is a KE increase and evaporation increases
61
Q

boiling point

A

when the atmospheric pressure is equal to the vapor pressure (Table H)

62
Q

normal boiling point

A

the boiling point of a liquid at STP

63
Q

surface tension

A

the resistance of a liquid to increase in its surface area

64
Q

why does surface tension exist/why don’t the molecules of the liquid spread out?

A

because the intermolecular forces of attraction between the molecules are stronger than the object that it is attached to.

65
Q

what is the strongest kind of intermolecular bond?

A

hydrogen bond

66
Q

capillary action

A

the spontaneous rising of a liquid in a narrow tube

67
Q

viscosity

A

the resistance of a liquid to flow

68
Q

what causes viscosity?

A

intermolecular forces of attraction (the stronger the attraction, the more viscous the liquid

69
Q

properties of solids

A
  • definite shape and volume
  • strongest intermolecular forces of attraction
  • particle is located in a fixed position, vibrating
  • have a crystalline structure with geometric patterns when viewed with a microscope
70
Q

what are two kinds of odd solids?

A

amorphous and super cooled Liquids

71
Q

amorphous

A

solids that lack ordered structure, like rubber and plastics

72
Q

super cooled liquids

A

cooled to a rigid state without crystallizing

Chemistry (17 decks)

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