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Chemistry & Physics > Gas Laws > Flashcards

Gas Laws Flashcards

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1
Q

Name 8 Empirical Gas Laws

A
  • Graham’s
  • Gay-Lussacs
  • Ideal
  • Fick’s
  • Boyle’s
  • Charles
  • Dalton’s
  • Henry’s
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2
Q

What does 0 degrees C = in Kelvin?

A

0 C = 273.15 K

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3
Q

What does 1 atm equal?

A

760 torr

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4
Q

What does one molar volume equal?

A

22.414L (or 22.7L)

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5
Q

What are the 4 quantities that describe the state of a gas

A
  • Pressure
  • Temperature
  • Volume
  • Number of moles
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6
Q

Boyle’s Law

A

P1V1=P2V2

  • Volume is inversely related to pressure
  • Pressure > as Volume
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7
Q

Charles’s Law

A

V1/T1=V2/T2

  • Volume is directly proportional to temperature (K).

V > as Temp (K) >

If temp doubles, Volume doubles
If temp is 1/2, volume is 1/2

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8
Q

Avogadro’s Law

A
  • The volume of a gas is directly proportional to the number of gas molecules. (P and T must be constant)
    6. 022 x 10 ^ 23rd

V % = Mole %

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9
Q

Will an ET cuff > or < after being in a patient?

A

> . Room temp (70), body temp (98). Cuff will > due to Charles’ Law.

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10
Q

Gay-Lussacs Law

A

P1/T1=P2/T2

  • Pressure is directly proportional to temperature.

If volume is constant, temp goes up, pressure goes up.

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11
Q

Triangle GBC

A

G (p) B (v) C (t) G

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12
Q

Combined Gas law are what combined laws?

A

Boyle’s
Charle’s
Gay-Lussacs

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13
Q

The Ideal Gas Law

A
  • Combines the elements of the empirical gas laws to formulate a state function to completely describe the state of a gas under a given set of conditions.

PV=nRT

(R=constant) (T+Kinetic energy relationship).
(N=# of moles)

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14
Q

Gas density depends on ____ and ____.

A

Temperature and Pressure

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15
Q

Dalton’s Law

A

Law of partial pressures

  • The total pressure of a mixture of gases = the sum of the partial pressures of the component gases.
  • Ptot=P1+P2+P3…
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16
Q

How to calculate the mole fraction?

A

Divide # of moles of a particular gas by total # of moles in the mixture.

Mole fraction = (Mol A)/(Mol A + Mol B…Mol N)

17
Q

Relative Humidity

A

RH=(mass of H20 that is in air)/(Mass of H2O that will fit in air)

18
Q

What is Dew Point?

A

The temperature at which the moisture content in the air saturates.

19
Q

Kinetic Theory of Gases

A

Assumes that the molecules are very small relative to the distance between molecules.

Density: sum of the mass of molecules / Volume

Pressure: Force / Area

Temperature: a measure of the mean kinetic energy of the gas. Energy = Mass x Volume ^2

Temp and Kinetic Energy are directly proportional

20
Q

Graham’s Law

A

(Effusion)
Rate of effusion is inversely proportional to the the square root of the molecular mass.

Diffusion: the movement of a substance from high concentration to low concentration.

Effusion: the movement of a gas through a small opening.

21
Q

Fick’s Law

A 
(Diffusion)
Rate of diffusion of a gas is determined by the chemical nature of the membrane itself.
-surface area
-partial pressure of gradient
-thickness of membrane
22
Q

What is Gas Diffusion rate proportional to?

A
  • Partial pressure gradient
  • membrane area
  • solubility of gas in membrane
23
Q

What is Gas Diffusion inversely proportional to?

A
  • Membrane thickness

- Square root of the molecular weight

24
Q

Henry’s Law

A

Amount of a non-reacting gas which dissolves in liquid is directly proportional to the PP of the gas

The amount of gas dissolved is inversely proportional to the temperature. (The colder the liquid, the more gas that will dissolve in the liquid) (Temperature effect).

25
Q

Ostwald’s Solubility Coefficient

A

The > the coefficient the more readily the gas dissolves in the liquid.

This blood/gas partition describe how the gas will partition itself between the two phases after equilibrium has been reached.

> coefficient = > lipophilicity, > potency, > solubility

> solubility = > anesthetic needed to be dissolved = < onset time

26
Q

Meyer Overton

A

> oil solubility = > potency

27
Q

Gander Waals Equation

A

Assumes that gas molecules have finite volumes and that gas molecules attract on another

28
Q

Joule-Thompson Effect

A

Thermodynamic process that causes cooling of the fluid when it expands from high pressure to low pressure.

29
Q

Adiabetic Compression

A

“If you 1/2 the volume you double the pressure.

30
Q

Carbon Dioxide Absorber yields…(reaction of CO2 in soda lime)

A
  • Heat

- Calcium Bicarbonate

Chemistry & Physics (4 decks)

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