Pharmacology 2 Uiuc Grimm Inhaled

Front 1

Understand the difference between the terms vapor and gas

Back 1

Gas - phase of matter which expands to fill container
Vapor gaseous phase below boiling point temperature

Front 2

Define vapor pressure and partial pressure. Understand the factors which do and don’t influence vapor and partial pressure.

Back 2

Vapor pressure is the pressure exerted by a gas: affected by heat, other gasses present
Partial pressure is the part of the total pressure of a mix of gasses that is exerted by one component of the mix: not affected by other gasses

Front 3

What physical measurement must be stated along with vapor pressure.

Back 3

Temperature

Front 4

Describe the difference between vapor pressure and vapor concentration. Which is used to describe how much anesthetic is
being administered? Which is best correlated to the clinical effect?

Back 4

vapor concentration is the percent of the mixture that is a particular gas: Concentration is most often used(vapor% or %): partial pressure

Front 5

Define partition coefficient.

Back 5

A partition coefficient is the ratio of the concentration of a substance in one medium relative to another at equilibrium.

Front 6

Know what the Meyer-Overton theory relates to.

Back 6

correlation b/w lipid solubility of an inhaled anesthetic and minmum alveolar concentration (MAC)

Front 7

Understand the effect of blood:gas partition coefficient, cardiac output, alveolar ventilation, and tissue perfusion effect the uptake and elimination of anesthetic gases

Back 7

increasing inspired concentration, alveolar ventilation, or DECREASING cardiac output can all increase the speed of induction, the
opposite effect is generally seen at recovery

Front 8

Know what government agencies set guidelines for waste anesthetic exposure limits and what agency can enforce those
regulations.

Back 8

NIOSHA sets limitations, enforced by OSHA

Front 9

Know the limits for waste anesthetic gas exposure.

Back 9

Halogenated agents alone 2 ppm
Nitrous oxide alone 25 ppm
Halogenated agents with nitrous oxide
• 0.5 ppm for halogenated agent
• 25 ppm for nitrous oxide

Front 10

Define MAC

Back 10

Minimum Alveolar Concentration 1 MAC - 50% of patients respond to noxious stimuli/50% dont
Measure of potency

Front 11

Know the factors which can increase MAC

Back 11

Duration Of Anesthesia
Type Of Stimulation
Gender
Hypocarbia (P CO< 21 mmHg)
Hypercarbia (P CO > 95 mmHg)
Metabolic Alkalosis
Hyperoxia
Isovolemic Anemia
Arterial Hypertension
Thyroid Function
Magnesium
Hyperkalemia
Hyperosmolality
Propranolol
Naloxone

Front 12

Know the factors which can decrease MAC

Back 12

Metabolic Acidosis
Hypoxia (P < 38 mmHg)
Induced Hypotension (MAP < 50 mmHg)
Decreased Central Neurotransmitter
Levels
Hypothermia
Hyponatremia
Lithium
Hypoosmolality
Pregnancy
Ethanol Intoxication
Neuromuscular Junction Blockers
Local Anesthetics
Opioids
Barbiturates
Verapramil

Front 13

What is Dalton's Law of paartial pressure?

Back 13

The partial pressure exerted by a gas is independent of other gases in the mixture; therefore the partial pressure exerted by an
anesthetic gas in an inspired gas mixture is the is the same as it would be if the gas were by itself.

Front 14

What is Boyle's Law?

Back 14

If the temperature is kept constant and the volume of the container is reduced, the molecules of gas will have the same kinetic energy, but collide with the walls
of the container more often. Boyle Law - PV = Constant. When used to examine the effect of changes in pressure or volume it is commonly written as
P1V1=P2V2.

Front 15

What is Charle's Law?

Back 15

If heat energy is added to a system, kinetic energy will increase. That will cause the gas molecules to collide with the walls more
frequently. If the pressure is kept constant, the volume of the container must increase. This is expressed as Charles as Law: V/T =Constant.
A more common expression when considering the effect of a change in temperature or volume is V1/T /T1=V =V2/T /T2. Temperature is in Kelvin.

Front 16

What is Henry's Law?

Back 16

The general definition of Henry's law is: the solubility of a gas in a liquid is proportional tothe pressure of the gas over the solution.
From it you can derive the following formula: c=kP Henry's Law constant is dependent only on temperature.