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CHEM 119 > Unit 8: Gases > Flashcards

Unit 8: Gases Flashcards

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1
Q

describe the volume and shape of gases

A

indefinite volume and shape

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2
Q

do gases tend to have low or high densities

A

low densities

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3
Q

are gases easily able to mix with other gases

A

yes, mix with one another readily

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4
Q

what condition causes a dramatic change in the volume of a gas

A

changing temperature

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5
Q

what are common units of pressure

A
  • mmHg
  • torr
  • atm
  • Pa
  • kPa
  • psi
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6
Q

what are the conversions for units of pressure

A
  • 1 mmHg = 1 torr
  • 1 atm = 760 mmHg / torr
  • 1 atm = 101.3 kPa
  • 1 atm = 14.7 psi
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7
Q

how is the pressure exerted by a gas measured

A
  • the frequency of collisions between gas molecules and the container walls
  • more collisions = higher pressure
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8
Q

what happens to pressure when volume decreases

A

pressure increases

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9
Q

describe boyle’s law

A

pressure and volume are inversely proportional

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10
Q

what is the equation for the relation between pressure and volume

A

P1V1 = P2V2

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11
Q

what happens to volume when temperature decreases

A

volume decreases

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12
Q

describe charles’s law

A

volume and temperature are directly proportional

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13
Q

what is the equation for the relation between volume and temperature

A

V1/T1 = V2/T2

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14
Q

what unit of temperature must be used in all gas law calculations

A

kelvin

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15
Q

how do you convert celsius to kelvin

A

273.15 + C

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16
Q

what happens to volume when moles increase

A

volume increases

17
Q

describe avogadro’s law

A

moles and volume are directly proportional

18
Q

what is the equation for the relation between moles and volume

A

V1/n1 = V2/n2

19
Q

what formula can be used to combine all the individual gas laws

A

P1V1/n1T1 = P2V2/n2T2

20
Q

what happens to pressure when moles decrease

A

pressure decreases

21
Q

are moles and pressure directly or inversely proportional

A

directly proportional

22
Q

define the ideal gas law

A

implies that all gases behave the same way under the same conditions

23
Q

what is the equation for the ideal gas law

A

PV=nRT

24
Q

what does R equal

A
  • PV/nT
  • 0.0821 Latm/molK
25
Q

what is the equation for density of gases

A

d=P(MW)/RT

26
Q

are density and temperature inversely or directly proportional

A

inversely proportional

27
Q

which gases are more dense: higher or lower molecular weights

A

higher molecular weights = more dense gas

28
Q

describe dalton’s law of partial pressures

A
  • Ptotal = P1 + P2 + P3 …
  • the pressures of the different types of gases in a sample will add to be the total pressure of the entire sample
  • each gases pressure can be determined by multiplying the total pressure by the mole fraction of a gas (mols of one type of gas / total mols)
29
Q

what are the steps to determining the mass of a gas through stoichiometry

A
  1. use ideal gas law (PV=nRT) to determine moles of gas
  2. perform stoichiometric conversion to get to grams
30
Q

what are the steps to determining the volume, pressure, or temperature of a gas through stoichiometry

A
  1. perform stoichiometry conversions to determine the moles of a gas
  2. use ideal gas law (PV=nRT) to determine the volume, pressure, or temperature
31
Q

what are the 5 pillars of kinetic molecular theory

A
  • gases consist of large number of molecules that move continuously and randomly
  • the combined volume of the gas molecules is negligible compared to the total volume in which the gas is contained
  • attractive and repulsive forces between gas molecules are negligible because they are moving so fast past each other
  • the average kinetic energy of the molecules is proportional to the absolute temperature (K)
  • all collisions are elastic; no energy lost
32
Q

is the kinetic energy of gas molecules directly or inversely proportional to temperature (in K)

A
  • directly proportional
  • as temperature increases, the kinetic energy increases
33
Q

are molecular weight and average molecular speed directly or inversely proportional

A
  • inversely proportional
  • as molecular weight decreases, speed increases (smaller molecules are faster)
34
Q

are gases more ideal at low or high pressures and why

A
  • low pressures (0-20 atm)
  • low pressure = higher volume = size of molecules is more negligible
35
Q

are gases more ideal at low or high temperatures and why

A
  • high temperatures
  • high temp = high speed = less time molecules spend near each other = less attractive/repulsive forces

CHEM 119 (8 decks)

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