Module 5

Question 1

The temperature of a gas depends on its average _____ energy

Answer 1

Kinetic

Question 2

Increased pressure of a gas = ______ volume

Answer 2

decreased

Question 3

Boyle’s Law

Answer 3

Volume is inversely related to pressure with a gas

Question 4

Law that explains pressure gradient in lungs during respiration

Answer 4

Boyle’s Law

Question 5

As pressure of a gas decreases, volume _______

Answer 5

Increases

Question 6

Pressure and volume of a gas are ______ proportional

Answer 6

inversely

Question 7

P1V1 = P2V2

Answer 7

Boyle’s Law

Question 8

At 36 Degrees Celcius,
Vt is 500mL @ sea level

What is Vt @ 730mmHg?

Answer 8

500(760) = V2(730)
500(760)/730 = V2
so,

520mL

Question 9

Volume of a gas is _____ proportional to its absolute temperature when pressure and amount of gas are constant (flexible container)

Answer 9

Directly

Question 10

Charles’ Law

Answer 10

Volume of gas and temperature are directly proportional

Question 11

As temperature of a gas increases, volume _____

Answer 11

increases

Question 12

V1/T1 = V2/T2

Answer 12

Charles’ Law

Question 13

When performing gas calculations, temperature must be converted to ______

Answer 13

Kelvin

Question 14

Volume of a gas _______ when heated

Answer 14

Increases

Question 15

When a pt is febrile, what do you need to watch for with their ETT?

Answer 15

Increase in cuff volume

Question 16

At sea level,
balloon w/ helium contains 200mL in 19 degree C room,

Volume @ 38 degrees C?

Answer 16

200/292 = V2/311
(200/292)(311) = V2
so,

213mL

Question 17

At a constant volume (rigid container), the pressure of a gas is _____ proportional to the temperature

Answer 17

Directly

Question 18

At constant volume (rigid container), as temperature increases, pressure ______

Answer 18

increases

Question 19

Does Gay-Lussac’s Law pertain to gas in a rigid or flexible container?

Answer 19

Rigid

Question 20

Does Charles’ Law pertain to gas in a rigid or flexible container?

Answer 20

Flexible

Question 21

P1/T1 = P2/T2

Answer 21

Gay-Lussac’s Law

Question 22

Full cylinder of O2 has 2200psi in 20 degrees C,

What is the pressure in 32 degrees C?

Answer 22

2200/293 = P2/305
(2200/293)(305) = P2
so,

2290psi

Question 23

What is the number of molecules in 1 mole of gas?

Answer 23

6.023x10^23

Question 24

Avogadro’s number is ______?

Answer 24

6.023x10^23

Question 25

Avogadro's hypothesis?

Answer 25

1 mole of any gas @ STP (standard temperature pressure) occupies a volume of 22.4L

Question 26

How much volume does 1 mole of gas occupy?

Answer 26

22.4L

Question 27

Avogadro's Law

Answer 27

Volume of gas is directly proportional to the number of gas molecules at STP (standard temperature pressure)

Question 28

Quantity of gas is expressed in _____ units

Answer 28

mole

Question 29

V1/n1 = V2/n2

Answer 29

Avogadro's Law

Question 30

What volume does 2 moles of N2O occupy at STP?

Answer 30

22. 4L x 2 = | 44. 8L

Question 31

Balloon has 1.9L of 0.0920 mol of helium, 0.0210 mol of helium is added, What is new volume of balloon?

Answer 31

1.9/0.092 = V2/0.113 (1.9/0.092)(0.113) = V2 so, 2.33L

Question 32

This theory was created to explain the ideal gas law

Answer 32

Kinetic Molecular Theory

Question 33

Combination of the empirical gas laws

Answer 33

Ideal Gas Law

Question 34

Name the three empirical gas laws

Answer 34

Boyle's Law Charles' Law Gay-Lussac's Law

Question 35

Ideal Gas Law equation

Answer 35

PV=nRT | Pressure)(Volume)=(moles)(Gas constant)(Temp

Question 36

Gas constant for Ideal Gas Law

Answer 36

0.0821 atm/K/mol

Question 37

5g of neon at 256mmHg & 35 degrees C What is the volume?

Answer 37

256mmHg = 0.3368atm 5g Ne = 0.25mol (1mol of Ne = 20.1797)(molecular weight) 35C = 308K 0.3368(V) = 0.25(0.0821)(308) so, 19L

Question 38

_________ equation corrects the Ideal Gas Law & accounts for molecular volume and molecular interactions in a gas

Answer 38

Van der Waal's Equation

Question 39

Dalton's Law of Partial Pressure

Answer 39

Total pressure = sum of each gas' partial pressures

Question 40

Approximate percent of O2 in RA @ sea level?

Answer 40

21%

Question 41

Approximate percent of N2 in RA @ sea level?

Answer 41

79%

Question 42

Partial pressure of O2 at sea level?

Answer 42

0.21 x 760 = 160mmHg

Question 43

Partial pressure of N2 at sea level?

Answer 43

0.79 x 760 = 600mmHg

Question 44

Dalton's Law of Partial Pressure equation

Answer 44

Pt = P1 + P2 + P3 + P4 + .....

Question 45

What are the partial pressures of N2O & O2 if they are delivered in a 70/30% mixture at sea level?

Answer 45

``` PN2O = 0.70(760) = 532mmHg PO2 = 0.3(760) = 228mmHg ```

Question 46

At STP, what is the partial pressure of O2 if the fresh gas flow from the anesthesia machine is 50/50% air/O2 mixture?

Answer 46

``` PO2 = 0.50(760) = 380mmHg Pair = 0.50(760) = 380mmHg but, PO2 in air = 0.21(380) = 79.8mmHg so, ``` 380 + 79.8 = 459.8mmHg

Question 47

This process explains why it is important to slowly open gas cylinders and pipes

Answer 47

Adiabatic Process

Question 48

Opening a cylinder fast = adiabatic process or not?

Answer 48

Yes, adiabatic process

Question 49

Opening a cylinder slowly = adiabatic process or not?

Answer 49

No, not an adiabatic process (has time to equilibrate)

Question 50

Joule-Thompson Effect

Answer 50

Rapid expansion of gas causes the temp to decrease

Question 51

This effect happens when you rapidly open a gas valve

Answer 51

Joule-Thompson effect