Shared Flashcard Set

Details

gas laws
test questions
71
Physics
Graduate
11/12/2007

Additional Physics Flashcards

 


 

Cards

Term
pressure is measured in?
Definition
pascals
Term
volume is measured in?
Definition
liters
Term
temperature measured in?
Definition
Kelvin=Celcius + 273
Term
what generates pressure?
Definition
particles bombarding a container wall (think of particles hitting against a cylinder wall)
Term
what is molecular theory?
Definition
inside a lattice chain of a solid there is a "static" state, but when heat is added the vibrations and excitement of the molecules increase. as heat is added, solids change statesto liquids and then to gases.
Term
what are Van de Wealts Forces?
Definition
the increasing movement and forces of molecules that are related to an increase in heat.
Term
what is an ideal gas?
Definition

a perfect gas-but only in theory. a hypothetical gas. consists of identicle particles of zero volume and no intermolecular forces.

+molecules undergo perfectly elastic collisons with walls

+molecules are far apart

+real gasses do not exibit these exact properties.

+this approximation model breaks down at high pressure and low temperatures where intermolecular forces play a greater role related to gas properties.

Term
what  is Boyle's Law?
Definition

1st ideal gas law.    Temperature is constant!

 

pressure is inversely proportional  to volume.

 

equation:  pV=K  or  P1V1=P2V2

 

 

Term
What is Charles' Law?
Definition

2nd ideal gas law.

 

Pressure is constant.

 

volume is directly proportional to temperature.

 

equation: V/T= P so V1/T1= V2/T2       

Term
1 ATM IS EQUAL TO:
Definition
760 mmhg, 100Kpa, 100,000 p, 14.7 psi
Term
what is Gay Lussac's Law?
Definition

3rd ideal gas law.

 

volume is constant.

 

pressure is directly proportional to temperature.

 

equation: P/T=K or V  so  P1/T1 = P2/T2

 

+MUST USE kELVIN WHEN DOING TEMP GAS EQUATIONS

Term
WHAT IS THE COMBINED GAS LAW?
Definition

It combines Charles', Boyles, and GayLussac's Laws.

Changes in pressure, volume, or temp. can be found mathemtically.

 It states that the product of a gasses volume and its pressure over temperature is equal to a constant.

 

P1V1/T1 = P2V2/T2

Term

What is Avogadro's Hypothesis or Law?

Definition

equal volumes of gases, at the same temp and pressure, contain the same number of particles or molucules.

 

+the ideal gas constant has the same value for all the gases.

 

one mole of gas occupies 22.4 Liters. or molar volume.

 

Avogadro's number= 6.022 x 1023 particles per mole

Term

Avogadro's law and the combined gas law make the ideal Gas Law.

What is the equation and its components?

Definition

equation:  pv=nRt

p=pressure   1 atm= 100Kpa, 100,000 pa or 760 mmhg

v=volume    1000L = m3

n=#of moles

R=gas constant 0.0821 (L, atm, mol, K) or 8.314472 (m3,pa, K, mol)

t=temp in Kelvin (9C= 5F-160)

 

most acurate for monatomic gases.

+favored at high temps and low pressures.

Term

What is Dalton's Law?

Definition

also called Dalton's Law of Partial Pressures.

 

states that the total pressure exerted by a gaseous mixture is equal to the sum of the partial pressure of each individual component in a gas mixture.

 

It assumes that the gases do not react with each other.

Term
critical temperature
Definition

Temperature above which a

substance cannot be liquefied no

matter how much pressure is applied.

 Especially important for N2O. Critical temperature for Nitrous is 36.5°c .

 

Term
adiabitic process
Definition

Adiabatic heating and cooling are processes that

commonly occur due to a change in the pressure

of a gas.

�� Adiabatic heating occurs when the pressure of a

gas is increased. An example of this is what goes

on in a bicycle pump.

�� i.e. - bicycle pump to inflate a pneumatic tire the barrel

of the pump is found to have heated up as a result of

adiabatic heating.

�� Adiabatic cooling occurs when the pressure of a

gas is decreased, such as when it expands into a

larger volume.

�� i.e. - when the air is released from a pneumatic tire; the

outlet air will be noticeably cooler than the tire, and after

all the air has escaped the valve stem will be cold to the

touch.

Term

What is the Joule Thompson effect?

Definition

an example of adiabatic cooling.

Gas from a high pressure cylinder is allowed to escape into space. As the gas expands, it cools adiabatically.

Term

What is a cryoprobe and how does it work?

Definition

An example of adiabatic coolong and the joule Thompson effect.

A small tube is attatched to a pressure source, as the gas escapes, it cools an area rapidly.

Term
What is in Nitrous Oxide Cylinders?
Definition
liquid and gas due to the critical temp of N2O.
Term
What happens in Nitrous oxide Cylinders?
Definition
pressure is constant in cylinder until the liquid disappears then the pressure decreases linearly as the cylinder empties.
Term
temp drop may cause moderate decrease in pressure in cylinders due to what 2 things?
Definition
latent heat evaporation (occurs as liquid vapoizes in the atm as it cools)
and Joule thompson effect-cools the cylinder as gas escapes
Term
Gas cylinder Specs:
Definition

Gas           color             psi            liters     

oxygen       green         2,200           660

 

nitrous       blue            745             1590

 

air             yellow         1900             625

Term

oxygen and nitrous oxide

differences when emptying

Definition

Pressure in the nitrous cylinder is steady until the liquid is gone then drops exponentially.

 

oxygen pressure drops at a steady rate.

Term
At what pressure and amt of liters will all the liquid of nitrous oxide be gone and the pressure drop off linearly?
Definition
745 psi and 400 liters
Term
describe the difference between O2 and N2O when emptying the cylinders?
Definition
with O2, the pressure drops as the amt of O2 declines. With N2O, the pressure remains the same until the tank has 400 liters.
Term
what is an exponential function?
Definition
a special form of non-linear change encountered in nature. (dependent upon natural process that we see daily)
Term
what is an exponential process?
Definition
rate of change of a quantity at any time is proportional to the qua ity at that time. ++as the quantity changes-it effects the rate of change.
Term
exponential function and process equation?
Definition
y = mx + b
y=vertical axis or volume
m=slope of the lie on the graft
x=horizontal axis or time
b=constant that you can add to the baseline toincrease or decrease.
Term
example of an exponential process.
Definition

flow is proportional to pressure, and pressure is proportional to volume, therefore flow is proportional to the volume at the time.

Q∞P, P∞V, therefore Q∞V

Term
SWhat types of things in anesthesia would apply the washout curve?
Definition
+basis of dye dilution technique
+thermo dilution technique
+used to measure cardiac output
+measures concentrations of drugs
+nitrogen washout curve
Term
What is the dye washout curve and what does it test?
Definition
cardiac output=dose of dye injected/area under the curve.
concentration of dye=vertical axis
time=horizontal axis
the concentration peaks, then goes down and peaks again. presumably because the dye does not clear the blood stream in one cycle. (big hill, then little hill)
Term
What two alternativemethods developed to track the exponential process?
Definition
half life and time constant
Term
What is half life and what is it useful for?
Definition
time it takes the quantity to reach 50%.
useful in radioactvity measurements.
Term
What is the time constant and what is it used for?
Definition
time it takes for the process to end assuming the first rate of change continues. The processis linear;where the linear line is and come back up to the curve-this is where pt has one time constant. Tau
Term
equation for time constant?
Definition
time constant x 0.693 = half life
69% of drug cleared
Term
What is the time constant for the lungs and the equation?
Definition
time constant = C x R (C is compliance and R is resistance) Compliance should remain the constant.
Term
time constant formula for a washout curve?
Definition
T (time constant) = volume undergoing washout/flow of perfusing fluid
Term

exponential formula for the lung?

Definition

when K = 2.718 it is given the symbol é

 

Vt=Vo (2.718) -t/cr or Voe -t/cr

 

 

Term
Positive exponential processes.
Definition
  1. positive exponential-ie bacterial growth upwards slope
  2. build up exponential-looks like a hill
Term
what is solubility?
Definition
the ability of a solute to dissolve in a solvent. a saturated solution is when the maximum amt of solute has been dissolved.
Term
Henry's law
Definition
at a particular temp the amt of a given gas dissolves in a given liquid is directly proportional to the partial pressure of the gas in equilibrium with the liquid.
Term
Henry's law applied to scuba divers.
Definition
-at depth the body absorbs nitrogen
-ascend too quickly and it comes out of the solution and in the joints and tissues. "THE BENDS"
+++Henry's law only applis for constant temperatures.
Term
What is Cason's disease?
Definition
The Bends!
Term
The solubility of a gas is dependent upon what?
Definition
temperature, gas, liquuid, and partial pressure.
Understand that different gases dissolve differently and different liquids can effect the how a gas dissolves.
Term
What are the two solubility coefficients?
Definition
Bunsen solubility coeffiecient (not r/t anesthesia) and oswald solubility- it is the V of a gas which dissolves in 1 unit of liquid at the temp concerned. (PRESSURE INDEPENDENT!)
Term
When temp increases gases dissolve ________?
Definition
less
Term
compare solubility of N2 and Nitrous at same pressure and temp?
Definition
N2 dissolves at the rate of 0.014L,
N2O dissolves at the rate of O.39L
Term
What are partial coefficients?
Definition
the ratio of the amt of substance present in one phase compared with another, the two phases being of equal volume and equilibrium.
+temp and phase must be specified
+applied to 2 liquids
Term
Solubility and uptake of anesthetics
Definition
ether is more soluble in blood (12) than nitrous (.47) or halothane (2.3)
Term
How do gases that are soluble in blood effect anesthesia?
Definition
gases that are more soluble in blood are less effective in anesthesia, insoluble gases have their effect on the brain more quickly.
Term
second gas effect
Definition
the second gas makes the gradient steeper which helps for absorption of other gas during inspiration, but during expiration the gas comes outmore quickly than oxygen and the gradient can cause hypoxemia.
Term
Oil solubility and anesthetic potency.
Definition
Fat(neurons/brain) is analogous to oil.
Oil Gas partition coefficient means more soluble=more potent.
Term

application of Henry's Law.

  • know that O2dissolves in blood at 0.003cc/100cc/mmHg partial pressure.
  • know that CO2dissolves at   0.067/100cc/mmHg partial pressure
Definition

When PaO2 is 300mmHg, how much is dissoled in the blood?

  • O2=300mmHg x 0.003cc/100cc/mmHg =0.9/100cc blood
  • CO2= 300mmHg x 0.067/100cc/mmHg= 20.1/100cc blood 
Term
Diffusion definition and example.
Definition
-process by which the molecules of a substance transfer through a layer or area such as the surface of a solution.
-lungs diffuse anesthetic gases
-drugs diffuse in liquids ie:spinals
Term
factors that effect diffusion?
Definition
molecular size, tension gradient, membrane thickness and area, +concentration gradient effects rate of diffusion
Term
What is Fick's Law?
Definition

rate of diffusion of a substance across a unit area is proportional to the concentration gradient.

 

↑ gradient = ↑ rate of diffusion

Term
rate of diffusion affected by
Definition
concentration gradient and solubility of a gas ie:diffusing into a liquid
Term
rates of diffusion of gas are different. compare O2 and CO2.
Definition
more likely to become hypoxemic than hypercarbic.
Term
Graham's Law
Definition
diffusion rate = reciprocal of the square root of the molecular weight.
Term

diffusion equation=

  • proportional to tension gradient
  • proportional to solubility
  • inversly proportional to membrane thickness
  • inversely proportional to the √molecular wt.
  • proportional to membrane area
  • liquids diffuse less rapidly than gases
Definition

Diffusion= (P1-P2)(area)(solubility)

           (Membrane thickness)(√molecular weight)

Term
Osmosis
Definition
occurs with a semi-permeable membrane and 2 liquids. larger molecules unable to diffuse through membrane, but smaller molecules go through membrane due to gradient, so that side of the membrane has more pressure, which is called osmotic pressure.
Term
osmolarity
Definition
moles per liter
Term
osmolality
Definition
moles per kilogram
Term
oncotic pressure
Definition
osmotic pressure related to proteins
Term
components of normal saline
Definition
Na+, K+, Ca+, lactate, Cl-; total osmolarity=278 mmol/liter
body osmolarity=300 mmol/liter
therefore almost isotonic solution which has little oncotic pressure.
Term
increased hydrostatic pressure=
Definition
cells exploding
Term
increased oncotic pressure=
Definition
edema because there is no oncotic pressure to drive fluid back into the veins.
Term
principle of operation for capillaries.
Definition
-interstitial fluid has no proteins!
-plasma has proteins
-capillaries act as semi-permiable membranes(filters proteins)
-difference in osmolar gradient called oncotic pressure
Term
colligative properties=
Definition
osmotic pressure
freezing point depression
vapor pressure reduction
boiling point evaluation
Term
azeotropes
Definition
a mixture which vaporizes in the same proportion as its constituent volume proportions ie: alcohol 96% & H2O 4% always evaporate at same rate.
(application of Raoult's law)
Supporting users have an ad free experience!