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AFN Chem & Physics > Module 5 > Flashcards

Module 5 Flashcards

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1
Q

The temperature of a gas depends on its average _____ energy

A

Kinetic

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2
Q

Increased pressure of a gas = ______ volume

A

decreased

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3
Q

Boyle’s Law

A

Volume is inversely related to pressure with a gas

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4
Q

Law that explains pressure gradient in lungs during respiration

A

Boyle’s Law

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5
Q

As pressure of a gas decreases, volume _______

A

Increases

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6
Q

Pressure and volume of a gas are ______ proportional

A

inversely

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7
Q

P1V1 = P2V2

A

Boyle’s Law

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8
Q

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

What is Vt @ 730mmHg?

A

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

520mL

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9
Q

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

A

Directly

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10
Q

Charles’ Law

A

Volume of gas and temperature are directly proportional

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11
Q

As temperature of a gas increases, volume _____

A

increases

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12
Q

V1/T1 = V2/T2

A

Charles’ Law

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13
Q

When performing gas calculations, temperature must be converted to ______

A

Kelvin

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14
Q

Volume of a gas _______ when heated

A

Increases

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15
Q

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

A

Increase in cuff volume

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16
Q

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

Volume @ 38 degrees C?

A

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

213mL

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17
Q

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

A

Directly

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18
Q

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

A

increases

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19
Q

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

A

Rigid

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20
Q

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

A

Flexible

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21
Q

P1/T1 = P2/T2

A

Gay-Lussac’s Law

22
Q

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

What is the pressure in 32 degrees C?

A

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

2290psi

23
Q

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

A

6.023x10^23

24
Q

Avogadro’s number is ______?

A

6.023x10^23

25
Q

Avogadro’s hypothesis?

A

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

26
Q

How much volume does 1 mole of gas occupy?

A

22.4L

27
Q

Avogadro’s Law

A

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

28
Q

Quantity of gas is expressed in _____ units

A

mole

29
Q

V1/n1 = V2/n2

A

Avogadro’s Law

30
Q

What volume does 2 moles of N2O occupy at STP?

A
  1. 4L x 2 =

44. 8L

31
Q

Balloon has 1.9L of 0.0920 mol of helium,
0.0210 mol of helium is added,

What is new volume of balloon?

A

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

2.33L

32
Q

This theory was created to explain the ideal gas law

A

Kinetic Molecular Theory

33
Q

Combination of the empirical gas laws

A

Ideal Gas Law

34
Q

Name the three empirical gas laws

A

Boyle’s Law
Charles’ Law
Gay-Lussac’s Law

35
Q

Ideal Gas Law equation

A

PV=nRT

Pressure)(Volume)=(moles)(Gas constant)(Temp

36
Q

Gas constant for Ideal Gas Law

A

0.0821 atm/K/mol

37
Q

5g of neon at 256mmHg & 35 degrees C

What is the volume?

A

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

38
Q

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

A

Van der Waal’s Equation

39
Q

Dalton’s Law of Partial Pressure

A

Total pressure = sum of each gas’ partial pressures

40
Q

Approximate percent of O2 in RA @ sea level?

A

21%

41
Q

Approximate percent of N2 in RA @ sea level?

A

79%

42
Q

Partial pressure of O2 at sea level?

A

0.21 x 760 = 160mmHg

43
Q

Partial pressure of N2 at sea level?

A

0.79 x 760 = 600mmHg

44
Q

Dalton’s Law of Partial Pressure equation

A

Pt = P1 + P2 + P3 + P4 + …..

45
Q

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

A 
PN2O = 0.70(760) = 532mmHg
PO2 = 0.3(760) = 228mmHg
46
Q

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

A 
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

47
Q

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

A

Adiabatic Process

48
Q

Opening a cylinder fast = adiabatic process or not?

A

Yes, adiabatic process

49
Q

Opening a cylinder slowly = adiabatic process or not?

A

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

50
Q

Joule-Thompson Effect

A

Rapid expansion of gas causes the temp to decrease

51
Q

This effect happens when you rapidly open a gas valve

A

Joule-Thompson effect

AFN Chem & Physics (21 decks)

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