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Chemistry > Gas Laws > Flashcards

Gas Laws Flashcards

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1
Q

Empirical Gas Laws

A

Describe the 4 quantities that describe the state of a gas

  1. Pressure
  2. Temperature
  3. Volume
  4. Number of moles
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2
Q

Boyle’s Law

A

Volume is inversely related to pressure

Forms the basis of the relationship between the 3 important parameters of a gas: volume, pressure, and temperature

Increasing the pressure of a gas at a constant temperature, the volume decreases, and vice versa

breathing

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3
Q

Charle’s Law

A

AKA: the law of volumes

Volume is directly proportional to temperature

  • gases expanded in volume when heated
  • his work was the basis of the ideal gas law

cuff volume increases in an ETT placed in a pt bc its warmed by pt

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4
Q

Avogadoro’s Law

A

The volume-mole relationship

The volume of a gas is directly proportional to the number of gas molecules as long as temp and pressure are constant

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5
Q

Gay-Lussacs Law

A

Pressure is directly proportional to temperature
-temperature goes up, then pressure goes up if volume constant

Example: N2O. Liquid in a tank. As gas is release, liquid vaporizes. Heat is lost. Temperature in the cylinder falls and the pressure drops

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6
Q

How to remember gas Law

A

Triangle

Boyles law (corner B), relates to pressure and volume (adjacent sides)

Can These Guys Possibly Be Violinists

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7
Q

Avogadro’s Number

A

6.022 x 10 the the 23rd

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8
Q

Combined Gas Law

A

Combining Boyle’s, Charles, and Gay-Lussacs laws

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9
Q

Standard Molar Volume

A

At STP, one mole (of an ideal) gas has a volume of 22.4L

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10
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

*no such thing as an ideal gas

PV = nRT

P: pressure
V: volume
-n: number of moles
T: absolute temperature
R: is a constant -describes the relationship between temperature and kinetic energy
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11
Q

What is standard temperature and pressure?

A

STP

standard temperature is 0 celsius or 273.17K

Standard pressure is 1 atm, or 1 bar, or 100 kPa

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12
Q

Gas density depends on what?

A

Temperature and pressure

Can calculate density if you now temperature and pressure

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13
Q

Dalton’s Law of Partial Pressure

A

The total pressure of a mixture of gases is equal to the sum of the partial pressure of the component gases

The pressure exerted by an individual gas in a mixture is known as its partial pressure

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14
Q

Mole fraction

A

A way of expressing the relative proportion of one particular gas within a mixture of gases

Divide the number of moles of a particular gas by the total number of moles in the mixture

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15
Q

Relative humidity

A

Measures the saturation of water in air

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16
Q

Kinetic molecular theory of gases

A

Assumes that the molecules are very small relative to the distance between molecules. The molecules are in constant, random motion and frequently colliding with each other and with the walls of any container

-Based on four basic tenets which exactly describe an ideal gas

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17
Q

Density of a gas

A

Sum of he mass of the molecules divided by the volume which the gas occupies

18
Q

Pressure of a gas

A

A measure of the linear momentum of the molecules

19
Q

Temperature of a gas

A

Measure of the mean kinetic energy of the gas

20
Q

Internal energy

A

The sum of the kinetic energy and potential energy

21
Q

Temperature is __________ proportional to the average kinetic energy

A

Directly

22
Q

Graham’s Law of Effusion

A

The rate of effusion is inversely proportional to the square root of the molecular mass

23
Q

Diffusion

A

The movement of a substance from an area of higher concentration to an area of lower concentration

Diffusion rate of a gas is directly proportional to the:

  • partial pressure gradient
  • membrane area
  • solubility of gas in membrane

Diffusion rate is inversely proportional to:

  • membrane thickness
  • the square root of the molecular weight.
24
Q

Effusion

A

The movement of gas through a small opening

The rate of effusion depends on the speed of the molecules

25
Q

Fick’s Law

A

The rate of diffusion of a gas across a permeable membrane is determined by the chemical nature of the membrane itself, the surface area of the membrane, the partial pressure gradient of the gas across the membrane, and the thickness of the membrane

26
Q

Boltzmann constant

A

Is equal to the ideal gas constant R divined by AN

AN is the number of molecules in a mole

27
Q

Diffusion-limited Gas Exchange

A

The scenario in which the rate at which gas is transported away from functioning alveoli and into tissues is principally limited by the diffusion rate of the gases across the alveolar membrane

28
Q

Perfusion-limited Gas Exchange

A

The rate at which gas is transported away from functioning alveoli and into tissues is principally limited by the rate of blood flow through the pulmonary capillaries and thus across the alveolar membrane

29
Q

Fick’s law of diffusion

A

The rate of diffusion of a substance across unit area (such as a surface or membrane) is proportional to the concentration gradient

Fick’s law of diffusion for gases explains:

  • the concentration effect
  • the second gas effect
  • diffusion hypoxia
  • why N2O leads to increase in volume or increase in pressure in gas spaces in the body
30
Q

CO2 is how much more soluble than O2

A

20x

31
Q

Henry’s Law

A

The amount of a non reacting gas which dissolves in liquid is directionally proportional to the partial pressure of the
gas, provided the temperature remains constant

-permits the calculation of dissolved O2 and CO2 in blood

32
Q

How much O2 is dissolved in blood?

A

0.003mL/100mL

33
Q

How do you calculate the dissolved O2 in blood?

A

Multiply the partial pressure of O2 by 0.003

34
Q

How much CO2 is dissolve in blood?

A

0.067mL/100mL

35
Q

How do you calculate how much CO2 is dissolved in blood?

A

Multiply the partial pressure of CO2 by 0.067

36
Q

Temperature effect

A

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

37
Q

Ostwald’s solubility coefficient

A

The quantity of solvent needed to dissolve a quantity of gas at a given temperature and pressure

-the higher the coefficient the more readily the gas dissolves in the liquid (blood:gas)

38
Q

Blood Gas Partition Coefficient

A

The ratio of the concentration of a compound in one solvent to the concentration in another solvent at equilibrium. It describes how well the gas will partition itself between the two phases after equilibrium has been reached

  • higher partition coefficient = higher lipophillicity = higher potency = higher solubility
  • higher solubility = more anesthetic needs to be dissolved = slower onset
  • MAC decreases as blood gas coefficient increases
39
Q

Meyer Overton

A

Agents with increased oil solubility have greater potency

40
Q

Ideal gases vs real gases

A

Ideal gases obey gas laws at all temperature and pressures. There are no ideal gases.

Real gases deviate at high pressure and/or low temperatures

  • Van der Waals equation deals with this deviation
  • Van der Waals relationship assumes that gas molecules have finite volumes and that gas molecules attract one another
41
Q

Joule-Thomson effect

A

A thermodynamic process that occurs when a fluid expands from high pressure to low pressure at constant enthalpy. Under the right conditions that can cause cooling of the fluid.

  • as a cylinder of compressed gas empties, the cylinder cools*
  • Joule’s Cool’s*
42
Q

Adiabatic Compression

A

Compression in which no heat is added to or subtracted from the air and the internal energy of the air is increased by an amount equivalent to the external work done on the air.

The increase in temperature of the air during adiabatic compression tends to increase the pressure on account of the decrease in volume alone.

Chemistry (7 decks)

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