Na 640A

Front 1

Three basic states of matter

Back 1

-Gas
-Solid
-Liquid

Front 2

Categorical Characteristics Gas/Solid/Liquid

Back 2

Volume and shape
Density
Compressability
Particle Motion
Intermolecular Distance

Front 3

Characteristics of a Gas

Back 3

Volume and shape- Expands to fill the volume of its container; consequently, it takes the shape of the container
Density- Low (10^-3g/ml)
Compressability- High
Particle Motion- Virtually free
Intermolecular Distance- Very Large

Front 4

Characteristics of a Liquid

Back 4

Volume and Shape- Has a fixed volume at a given mass and temp; volume principally dependent on its mass and secondarily on temp; it assumes the shape of its container
Density- High (1g/ml)
Compressibility- Very low
Particle Motion- Molecules or atoms "slide" past each other
Intermolecular Distance- Molecules or atoms are close to each other

Front 5

Characteristics of a Solid

Back 5

Volume and Shape- Has fixed volume; volume principally dependent on its mass and secondarily on temp; it has a definite shape
Density- High (1-10g/ml)
Compressibility- Virtually incompressible
Particle Motion- Vibrate about a fixed position
Intermolecular distance- molecules, ions, or atoms are close to each other

Front 6

Solids

Back 6

-comprised of particles that are held close to one another and have limited ability to move around.
-because of the attractive forces, solids behave as a single unit when acted upon external forces
-solids may be classified based on the arrangement of the particles (crystalline vs amorphous)

Front 7

Crystalline solid

Back 7

have particles that are ordered

Front 8

Amorphous

Back 8

have particles that are not ordered

Front 9

Types of Crystalline solids

Back 9

-Ionic
-Covalent
-molecular
-metallic

Front 10

Ionic

Back 10

Particles- cations, anions
Forces- electrostatic
MP- High
Characteristics- Hard, brittle
Examples- NaCL, KBr, MgCl2

Front 11

covalent

Back 11

Particles-atoms
Forces- covalent bonds
MP- Highest, sharing = strong bond in regards to crystalline
Characteristics- Extremely hard
Examples- Diamond, graphite

Front 12

molecular

Back 12

Particles- Molecules
Forces- Various noncovalent interactions
MP= Low
Characteristics- usually soft
Examples- H20, CH3CH2OH
Vanderwaals- dipole dipole & London forces

Front 13

Metallic

Back 13

Particles- Metal ions
Forces- Shared electron cloud (metallic bond, formed by orbital overlap)
MP- Varies
Characteristics- Hard, brittle, soft, malleable (pound flat), ductile (put into wire)
Examples- Na, Fe, Cu, Ag, Au

Front 14

Amorphous

Back 14

Particles- Molecules, atoms, or ions
Forces- Covalent or noncovalent
MP- Varies
Examples- rubber glass

Front 15

Melting points

Back 15

is proportional to the strength of the attactive forces (cohesion) holding the substance in the solid state
-typically the higher the attractive forces, the more energy required to disrupt the solid state, thus the higher MP

Front 16

Liquid

Back 16

is one type of fluid

Front 17

What is a fluid?

Back 17

-a system of particles loosley held together by their own cohesive forces (intermolecular), or by the restraining forces exerted by the walls of the container
- gases are generally compressible whereas liquids are generally incompressible

Front 18

A "perfect" fluid

Back 18

-offers no resistance to flow, except through its intertia
-gases at low density and higher temps will behave more like perfect fluids
-most fluids we will encounter will have an internal friction ("stickiness")that resists flow- viscosity

Front 19

density

Back 19

-amount of mass per unit volume
-symbol rho(p)
-p=M/V
-units are kg/m^3

Front 20

conversion unit to meters^3

Back 20

1 liter= 10^-3 m^3

Front 21

Gases- Definition

Back 21

is one type of fluid

Front 22

fluid

Back 22

a continous amorphous substance whose molecules move freely past one another and that has the tendency to assume the shape of its container; a liquid or gas

Front 23

Elastic

Back 23

resist change in shape, snaps back, recoil

Front 24

shear stress

Back 24

sliding motion, when molecules rub past each other

Front 25

Gas-the state of matter distinguished from the solid and liquid states by:

Back 25

-relatively low density and viscosity
-relatively great expansion and contraction with changes in pressure and temp
-the ability to diffuse (mix) readily
-the spontaneous tendency to become distributed uniformly throughout any container

Front 26

Working definition for Gas

Back 26

will completely fill a container or volume in which it is confined

Front 27

macroscopic properties of gases

Back 27

those properties that reflect the average condition of the gas: moles, volume, density, pressure, and temperature

Front 28

Gas Laws- Overview

Back 28

Boyle's, Charles', and Gay-Lussac's Laws are actually limited (constrained) versions of the Ideal Gas Law
-the Ideal Gas Law is a combination of Boyle's and Charles' laws

Front 29

Boyle's Law

Back 29

if temp is constant, relates volume and pressure
-volume and pressure are inversely related when T constant
-usually states "at fixed temp, volume times pressure is constant"
-moles are constant

Front 30

Boyle's Law formula

Back 30

P1V1=P2V2

Front 31

Applications of Boyle's Law in Anesthesia

Back 31

1. Squeezing BVM increases pressure and decreases volume
2. release of gas from compressed cylinder into atmosphere
3. Body plethysmography
4. Inspiration of gases into lung (increase V of thorax > decreased P) negative pressure breathing > spont vent

Front 32

Charles' Law

Back 32

-sometimes lumped with Gay-Lussac since they are related
-relates volume and temp at fixed pressure
-"at fixed pressure that ratio of volume to temp is constant"

Front 33

Charles' Law- formula

Back 33

V1/T1 = V2/T2

-direct relationship

Front 34

Application of Charles Law in Anethesia

Back 34

the inflatable cuff of an ETT or LMA in the autoclave- as temp increases so does volume

Front 35

Gay-Lussac's Law

Back 35

-often lumped with Charles' law since they are similar
-Relates pressure and temp at fixed volume
-Pressure is directly proportional to temp at fixed volume
-"at fixed volume the ration of pressure to temp is constant"

Front 36

Gay-Lussac's Law- formula

Back 36

P1/T1=P2/T2

Front 37

Applications of Gay-Lussac's Law in anesthesia

Back 37

1. When the temp of a closed cylinder increases the pressure increases
2. as the cylinder containing liquid N20 empties, the temp decreases
3. Wood's metal blows when the temp of a cylinder increases substantially

Front 38

Avogardo's Law

Back 38

equal volume of gases at the same temp and pressure, contained the same number of particles, or molecules.
-the number of molecules in a specifc volume of gas is independent of the size or mass of the gas molecules.

Front 39

The ideal gas constant

Back 39

-has the same value for all gases:

P1V1/T1n1=P2V2/T2n2

Front 40

Molar Volume and Gas Density

Back 40

The volume occupied by 1 mol of any gas is called its molar volume.
-at standard temp and pressure, dry (STPD) the molar volume of any gas is 22.4 L
-able to calculate the mass density for any gas by relating the gas's gram-molecular wt to its molar volume, which is always 22.4l/mol @ STPD

Front 41

Ideal Gas Law

Back 41

-Combination of Boyle's, Charles' and Avogardo's law

-PV=nRT

Front 42

R

Back 42

R= 0.0821 L*atm*mol^-1*K^-1

Or

R= 8.31 J*mol^-1*K^-1

where J = N*M

Front 43

Pascal conversion

Back 43

1pa = N/M^2

Front 44

Conversion of atm to Pa

Back 44

1 atm = 1.013 x 10^5 pa

Front 45

Conversion of atm to torr

Back 45

1 atm = 760 torr

Front 46

Kinetic theory of gases

Back 46

-describe molecules in a gas as a collection of elastic balls in free, random motion inside of a container
-collisions are perfectly elastic= no energy lost in collision

Front 47

Newtons's Laws

Back 47

the result of each collision of a molecule with the wall of a container creates a tiny force (f) acting on the wall of the container
-the average force exerted in 1 second over a unit area of one wall of the vessel volume (V) is the average force per unit area, which is the definition of pressure (P)

Front 48

Gas triangle memory device

Back 48

Can these guys possibly be violinists

Front 49

Graphic summary of Gas Laws

Back 49

The relationship of the gas laws

Front 50

Summary of gas Pressure
1

Back 50

the pressure of a gas is proportional to the average force per unit area that gas molecules exert on the walls of the conatiner

Front 51

Summary of gas Pressure
2

Back 51

-the total pressure exerted by all gas molecules in the atmosphere is the barometric pressure, Pb. Units of pressure are millimeter mercury (mmHg), or the kilopascal (kPa)

Front 52

Pressure conversions

Back 52

-at sealevel Pb (1 atm) = 760mm Hg = 101 kPa

-1 kPa = 7.50mmHg = 7.50 torr = 0.295 inches

Front 53

Summary of gas Pressure
3

Back 53

for low pressures, centimeters of water (cm H20) are often used.
-1mm Hg = 1.35 cm H20, this is derived from the ratio of densities of mercury (13.6gm *cm^-3) and water (1gm*cm^-3)

Front 54

Dalton's Law of Partial Pressures

Back 54

Gas molecules are assumed to act independently, which is a good approximation for low pressure gases
this assumption is the basis for Dalton's law: THE TOTAL PRESSURE OF A GAS MIXTURE (Ptot) IS EQUAL TO THE ALGABRAIC SUM OF THE PARTIAL PRESSURES (TENSIONS) OF ALL THE GASES IN THE MIXTURE.

DALTON'S LAW: Ptotal = P1+P2...Pn

Front 55

Dalton's law semantics

Back 55

Chemistry = lower case p for partial and upper case for total

Physiology= pO2, so PO2

Front 56

Fractional Concentration (percent concentration)

Back 56

-the partial pressure (tension) of a gas is equal to the fractional concentration of a specific gas times the total pressure of the mixture
-relationship derived from Dalton's law

Front 57

Fractional/Percent Concentration formula

Back 57

Pgas= Fgas X Ptotal

-Only holds true for molecules that are "free", that is not chemically combined

Front 58

Applications of Dalton's Laws

Back 58

1. Permits calculation of the % concentration of a gas by dividing the partial pressure of the gas by the total pressure
2. Permits calculation of the partial pressure of a gas by multiplying % contration by the total pressure

Front 59

Vapor Pressure

Back 59

is the partial pressure exerted by gas molecules when there is equilibrium between the liquid and gas phases of the molecules
-if the container is open to air, then the vapor pressure of the molecules is a partial pressure, along with the other gas molecules in the air

Front 60

saturated vapor pressure

Back 60

if the liquid is in a closed container with no other gases, the pressure of the vapor at equilibrium is specifically calleld the saturated vapor pressure

Front 61

Boiling point of a liquid

Back 61

is the temperature at which the vapor pressure and atmospheric pressure are equal

Front 62

Important point about boiling point and vapor pressure

Back 62

-BP of a liquid is not constant, the BP is a function of pressure
-the vapor pressure is a functiuon of the temp of the system

Front 63

Gas solubility and Henry's Law

Back 63

-describes the same equilibrium as does saturated vapor pressure, but from the perspective of the fluid rather than the gas.
-at equilibrium, the liquid is saturated with all of the gas molecules that is can hold
-Henry's law states that the amt of gas (conc) that can dissolve in a liquid is directly proportional to the partial pressure of the gas above the liquid

Front 64

Henry's Law eqauation

Back 64

Cgas= B(beta) x Pgas

B= solubility coefficient
Pgas= partial pressure

Front 65

Solubility coefficient

Back 65

the solubility coeffcient is inversly proportional to temp- increased temp = decreased B
-the concentration is usually expressed per 100ml (deciliter) of fluid, and thus called volume percent

Front 66

B(beta)C02

Back 66

0.067ml CO2 * dl^-1 mmHg @ 37C

Front 67

B(beta) 02

Back 67

0.003ml O2 *dl^-1 mmHg @ 37C

Front 68

How much oxygen is dissolved in each deciliter of blood when Po2 = 90mm HG

Back 68

Co2 = Bo2 x Po2

0.003 ml 02/ dl*mm Hg x 90mmHG

=0.27

CO2 was 2.6
-o2 does not dissolve in blood very well, good thing we have hemoglobin

Front 69

Absolute Humidity

Back 69

-the mass of water vapor present in a given volume of air
-the values of absolute humidity are usually expressed as mg/L or g/m^3, which are numerically equivalent
-the maximum amount of water vapor that can be present in a given volume of aire is a function of the system temperature

Front 70

relative humidity

Back 70

is a ratio of the measured partial pressure of water in the air to the saturated vapor pressure of water, which is determined soley by the temp of the air
-in other words it is the ration of how much water vapor is in the air, compared to the maximum(saturated) amt of h20 that the air could hold at that temp

Front 71

relative humidity formula

Back 71

actual vapor pressure/ saturated vapor pressure

-usually expressed as a percentage

Front 72

Summary of gases

Back 72

-easily compressible
-expand to fill any available volume
-have low density
-readily diffuse through each other
-exert pressure on their containers
-behave most ideally at low pressure and high temps