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chemistry > unit 5 - Gas Laws > Flashcards

unit 5 - Gas Laws Flashcards

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1
Q

Kinetic Molecular Theory (ideal gas laws)

A

(KMT) is a theory used to explain the usual behavior of gases

  • describes the relationship among:
    pressure, volume, temperature, velocity, frequency of collisions
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2
Q

(KMT) ideal gas laws are

A
  • gases contain particles that are in constant, random, straight-line motion
  • gas particles collide with each other and with the walls of the container
    - results in a transfer of energy
  • gas particles are separated by great distances
    - no definite shape, no definite volume
  • gas particles DO NOT attract each other
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3
Q

ideal gases (vs context)

A
  • particles spread out
  • gases are most ideal at low pressure, high temperature
  • Hydrogen and Helium are always ideal gases (low density)
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4
Q

real gases (vs context)

A
  • particles are closer together
  • gas particles DO attract each other
  • gas particles DO occupy volume
  • gases are most Real at high pressure and low temperature
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5
Q

avogadro’s hypothesis

A

if two gases are at the same exact temperature and pressure… AND the volumes that the gases occupy are the same
- the # moles (# molecules) are also the same

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6
Q

STP

A

standard temperature and pressure
- 273K = 0°C
- 1 atm = 101.3 Kpa

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7
Q

at STP, 1 mole of any gas will always occupy

A

22.4 L

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8
Q

pressure

A

the amount of force over a certain area

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9
Q

volume

A

the amount of space something takes up

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10
Q

robert boyle

A

discovered the relationship between pressure and volume of a gas

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11
Q

what is the only element that is liquid at room temp

A

mercury

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12
Q

standard pressure

A

760 mmHg = 760 Torr
1 atm
101.3 Kpa

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13
Q

boyle’s law

A

relationship between pressure and volume
- at constant temperature, as pressure is added to a gas (increases), the volume will decrease
- pressure and volume are inversely proportional
- P1V1 = P2V2

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14
Q

boyle’s law equation

A

P1V1 = P2V2
- 1 = initial state
- 2 = final state

  • volume units - measured in mL or L
  • pressure units - measured in Kpa, atm, mmHg, or torr
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15
Q

boyle’s law: if the pressure doubles, what happens to the volume

A

goes down by half

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16
Q

boyle’s law: if the volume doubles, what happens to the pressure

A

goes down by half

17
Q

boyle’s law: if the pressure is halved, what happens to the volume

A

doubled

18
Q

boyle’s law: if the volume is halved, what happens to the pressure

A

doubled

19
Q

charles’s law

A

the relationship between temperature and volume of a gas when pressure is constant

  • at constant pressure of a given gas, its new volume is DIRECTLY proportional to it’s change in temperature
20
Q

jacques charles

A

discovered the relationship between temperature and volume of a gas

21
Q

charles’s law equation

A

V1/T1 = V2/T2
- at constant pressure!!
- let V1 & T1 represent the initial volume and temp (in K)
- let V2 & T2 represent the final volume and temperature
- temperature MUST be measured in kelvins

22
Q

why must temperature be measured in kelvin for Charles’s Law

A
  1. 0°C would make the fractions undefined
  2. Negative temps do not work mathematically
23
Q

lussac’s law

A

relationship between temperature and pressure of a gas at a constant volume

  • as temperature increases, pressure exerted by the gas increases

P1/T1 = P2/T2

24
Q

combined gas law equation

A
  • when ALL variables (temperature, pressure, & volume) change; nothing is held constant

(P1V1) / T1 = (P2V2) / T2

25
Q

SIGFIG for this question: “convert 2.75 atm to Kpa”

A

2.75 atm x 101.3 Kpa/1 atm = 279 Kpa
^
only look at
2.75 atm for
sigfig!!

26
Q

dalton’s law of partial pressure: mixture of gases

A
  • dalton found that the TOTAL PRESSURE exerted by the mixture of gases is equal to the sum of the Partial Pressures of each gas in the mixture
  • Total Pressure = P1 + P2 + P3
27
Q

Law of Partial Pressure Example

A

If 5.0 moles of O2 and 7.0 moles of N2 together exert a total pressure of 200.0 Kpa, what is the partial pressure of O2?

5.0/12.0 x 200.0 Kpa = 83.33 Kpa
^
don’t use
this ratio
for sigfigs

28
Q

Graham’s Law of Diffusion

A
  • the rate at which gases diffuse is inversely proportional to their molar mass
  • at STP, gases with a smaller molar mass will diffuse the fastest
29
Q

graham’s law of diffusion example

A

Which gas at STP will diffuse the slowest?
1) O2 2) H2 3) Xe 4) Ar
32g/mol 2g/mol 131g/mol 40g/mol

Xenon will diffuse the slowest at STP

30
Q

Graham’s Diffusion Formula

A

V1/V2 = sqrt (m2/m1)

KE = 1/2 mv^2

(V1/V2) <- relative velocity

31
Q

at the same temperature, the KE of two different gases is the…

A

same

chemistry (11 decks)

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