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CRNA CHEM & PHYS > Test 2 > Flashcards

Test 2 Flashcards

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1
Q

Define Work? What is the formula for work?

A

Work is defined as a measurement of force displacing an object:
W = F x d (Work is equal to force x distance)

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2
Q

What is the SI unit of measurement for Work?

A

Joules

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3
Q

Other ways of expressing 1J?

A

1) 1J = N x m

2) 1J = kg x m^2/s^2

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4
Q

If you have 1kg mass you want to accelerate at 1m/s^2 over a distance of 1m. How much energy do you need?

A

Since W = F x d and F = m x a;
Then W = (m x a) x d
W = (1kg x 1m/s^2) x 1m = 1J or 1kg/m^2/s^2

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5
Q

How much work was done in Joules lifting a 100kg patient up to a distance of 0.02m straight up to place him onto the operating table?

A

Since W = F x d;
1st change weight into newtons because weight is acted upon by gravity which is newtons. So, 100kg = 981N, (1kg = 9.81N)
Now, w = 981 X .02 = 19.62J (rounding up gives you 20J or 2 x 10^1J

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6
Q

Define Kinetic Energy? what is the formula for it?

A

Kinetic Energy is described as energy of motion or the energy a mass has by virtue of being in motion.
KE = 1/2 mass x velocity (KE = 1/2kg x (m^2/s^2))

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7
Q

What is the SI unit of measurement for Kinetic Energy?

A

Joules or (kg/m^2/s^2); same as Force

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8
Q

What is the KE of a 55kg mass moving at 3.87 meters per second?

A 
KE = 1/2m x velocity^2
KE = 0.5 x 55kg x (3.87m/s^2)
KE = 27.5kg x 14.97m^2/s^2
KE = 411.675J
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9
Q

What is the formula used to find the Work done by expanding gas?

A

W = P x ΔV

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10
Q

What is the formula used to find the volume of a cylinder?

A

V = A x h (Volume = area x height)

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11
Q

What is the SI units of measurement for volume?

A

m^3

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12
Q

How many Liters in 1 m^3?

A

1000L

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13
Q

How much work is done when 2.5L of gas expands to 3L against 600 Pa?

A

Since W = P x ΔV or W = P x (final volume - initial volume). Since 3L = .003m^3 and 2.5L = .0025m^3; then
W = 600 Pa x (3 x 10^-3m^3 - 2.5 x 10^-3m^3)
W = 600 Pa x (.0005)
W = 0.3 Pa x m^3
W = 0.30J (1J is equal to 1 Pa x m^3)

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14
Q

How much work is done when a ventilator increases the volume of air in the body by 500mL using 600Pa of pressure?

A 
W = P x ΔV
W = 600Pa x .0005m^3 = .3J
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15
Q

Define Calorie?

A

A calorie is the amount of energy necessary to raise 1 gram of water 1 degree Celsius.

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16
Q

Whats the difference between a calorie and a Calorie?

A

Food Calories are actually kilocalories, written with a capitalized “C”. So, one Calorie = 1 kilocalorie or 1000 calories.

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17
Q

How many Joules are in 1 calorie?

A

1kcal (1000 calories) = 4184J or

1J = .239 calories

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18
Q

How many Joules in a 2000kcal daily diet?

A 
.239cal/1J = 2000kcal/xJoules. -->
.239x = 2000kcal (2,000,000 calories) --> x = 8,368,200J or 8.368 x 10^6J
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19
Q

If a 1500kg truck is traveling down the highway, how fast (v) must it be going to have the same energy as 2000kcal?

A 
KE = 1/2m x v^2 --> V^2 = 2KE/m
v = sq. root of 2KE/m
v = sq. root of 2(8.37 x 10^6J)/1500kg
v = 106m/s or 237mph
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20
Q

Convert 106m/s to mph

A 
1609m = 1 mile and 3600 secs in and hr
1690/106 = 15.17miles
3600secs/15.17miles = 237mph
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21
Q

Define Potential Energy? Give examples?

A

Energy that is stored by virtue of position (expressed in Joules). i.e.:

1) An airplane in the air
2) Chemical energy stored in food, glucose, or fat

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22
Q

Define Internal Energy? How is Internal Energy represented in an equation?

A

The sum of all the kinetic energy and potential energies of the particles in a system. It results from the state of the particles at the molecular level.
Represented by the letter “U”

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23
Q

Define Thermodynamics?

A

The study of how energy is converted from one form to another, and how it flows into and out of a system. A system could be a test tube, a gas cylinder, a patient, etc.

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24
Q

What are the 4 Laws of Thermodynamics?

A

1) The Zeroth Law of Thermodynamics
2) The First Law of Thermodynamics
3) The Second Law of Thermodynamics
4) The Third Law of Thermodynamics

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25
Q

What is the Zeroth Law of Thermodynamics?

A

Says that if 2 systems are in a thermal equilibrium with a third system, then they are thermal equilibrium with each other.
Therefore, if the temperature of A = B, and B = C, then A =C.

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26
Q

What is the First Law of Thermodynamics?

A

The change in Internal Energy (U) of a system of heat (Q) flowing in or out of the system; and work (W) done by or on the system. (ΔU = Q - W) but is written as (ΔU = Q + W)

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27
Q

Why is the 1st Law of thermodynamics written as ΔU = Q - W instead of ΔU = Q + W?

A

Because heat and work can be added into or taken out of the system.
If Q > 0, the process is endothermic and heat flows into the system (+Q is used).
If Q < 0, the process is exothermic and heat flows into the system (-Q is used).
If W > 0, work done by system on surroundings aka expansion (-W is used).
If W < 0, work done by system on surroundings aka compression (-W is used).

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28
Q

What is the 2nd Law of Thermodynamics?

A

Says that entropy of the universe is constantly increasing. It does not become spontaneously more organized.

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29
Q

Give an example of the 2nd Law of Thermodynamics?

A

A mixture of oxygen and nitrous oxide in an anesthesia induction will not spontaneously separate and send only one gas to the patient.

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30
Q

What is the Third Law of Thermodynamics?

A

Says that it is not possible to lower the temperature of an object to absolute zero.

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31
Q

We have a gas in a cylinder with a frictionless piston. 3J of energy is absorbed in the system. The gas expands to 500mL greater than the original volume against a constant pressure of 600Pa. What are the work, heat, and internal energy changes?

A

ΔU = Q + W
1st convert SI units for volume ml to m^3
500mL or .5L = .0005m^3,
Since W = P x ΔV,
W = 600Pa x .0005) = .3J
Since there is expansion, the system is doing work and we use (-W) or -0.3 to indicate energy lost from the system.
Q wil be positive (+3) because energy was absorbed into the system.
ΔU = Q + W –> ΔU = +3J - 0.3J –> ΔU = 2.7J
The internal energy of the system increased by 2.7J

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32
Q

Define Specific Heat?

A

The amount of heat per unit mass required to raise the temperature of something by one degree Celsius.

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33
Q

What is the formula for Specific Heat?

A

c = Q/m(ΔT).

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34
Q

Hydrostatics

A

Study of fluids that are not moving

35
Q

Hydrodynamics

A

Study of fluids in motion

36
Q

A beaker with a diameter of 10cm is filled to 20cm with water. If the density of water is 1000km/m^3, how much pressure does the water exert on the bottom of the beaker?

A 
P = dhg (Pressure = density x height x gravity)
P = 1000kg/m^3 x 0.20m x 9.81m/s^2 = 1.96 x 10^3Pa
37
Q

Difference between P= dhg and P2 = P1 +dhg

A

P2 = P1 + dhg adds the pressure of a gas above a liquid to the equation

38
Q

What’s the pressure at a depth of 1000m below the surface of the ocean if the density of sea water = 1.03 x 10^3kg/m^3? (remember 1 atm = 101kPa)

A

P2 = P1 + dhg
P2 = 101,000Pa + (1.03 x 10^3kg/m^3 x 1000m x 9.81) =
1.02 x 10^7Pa

39
Q

Define Flow? What is the formula for Flow?

A

Flow is the quantity of fluid passing a point per unit of time.
F = V/t (F = flow; V = volume; t = time)

40
Q

Formula for Pressure?

A

P = F x R (P= pressure; F = flow; R = resistance)

41
Q

How is change in flow annotated?

A

Q dot (Q̇)

42
Q

Viscosity

A

The resistance a liquid offers to motion of a solid through it. (represented by symbol η)

43
Q

Turdbulence is dependent of what?

A

Density

44
Q

Reynolds Number

A

The point when laminar flow changes to turbulent flow.
< 2000 = laminar flow
2000 to 3000 = a mix btw laminar and turbulent flow
> 3000 = turbulent flow

45
Q

Describe Laminar Flow

A

The relationship of flow to pressure. Laminar Flow is steady and smooth without eddies or turbulence.

46
Q

Turbulent Flow occurs with what?

A

1) High velocity
2) When tubes are rough
3) At bends or kinks in tubing

47
Q

(T/F?)Turbulent flow is density dependent, not fluid dependent?

A

True

48
Q

Poiseuille’s Law

A

Describes flow through a tube and how this flow is affected by tube length, radius and fluid viscosity.

49
Q

Poiseuille’s Law Formula

A 
F =  (πr^4ΔP)/8ηl; where
F = flow in L/s
η = viscosity in Pa/s
r = radius of tube in meters
l = length of tube in meters
50
Q

Effect on flowrate when you increase the radius of the tube by 19%?

A

Doubles the flow rate

51
Q

Effect on flowrate when you double the radius of the tube?

A

Increases flow rate by a factor of 16

52
Q

How do changes in pressure and viscosity affect flow rate?

A

1) Changes in pressure are directly proportional

2) Changes in viscosity or length are inversely proportional

53
Q

Using Poiseuille’s Law Formula, calculate aortic blood flow, if blood viscosity = .0015Pas, pressure = 13,000Pa (or 100mmHg) misapplied to the aorta (r - 0.010m; l = 1m).

A

F = (π x 0.01^4 x 1.3x10^4Pa)/8 x 1.5x10^-3Pas x 1m =.034m^3/s

54
Q

How does the body apply Poiseuille’s Law to affect BP when needed?

A

Smaller vessels provide most of the resistance to flow, so arterioles just prior to the capillaries can provide a controlling influence on flow rate, thereby meeting the changing demands for oxygen.

55
Q

Define Bernoulli’s Principle?

A

For a non-compressible, non-viscous fluid undergoing laminar flow, the sum of the pressure, kinetic and potential energies per unit volume remains a constant at all points along the line.

56
Q

Bernoulli’s Principle Formula

A

ΔP = 1/2d (V2^2 -V1^2)

57
Q

What is the pressure differential across a flat roof having an area of 240m^2 when the wind blows at 25m/s. (density of air =

A 
ΔP = 1/2d ((V2^2 -V1^2)
ΔP = 1/2d (1.29) (25^2-0^2) = 403Pa
Since F = P x A
F = (403Pa)(240m^2)
F = 96,700N or 10.9 Tons of force on the roof from the air inside the house
58
Q

Fick’s Principle

A 
VO2 = CO x (aO2 - vO2) same as CO = VO2/(aO2 - vO2) 
VO2 = uptake of O2 by the body
CO = cardiac output
aO2 = arterial oxygen concentration
vO2 = venous oxygen concentration
59
Q

3 Variables in the Gas Law Equations?

A

1) Pressure
2) Temperature
3) Volume

60
Q

Boyle’s Law

A

V1 x P1 = V2 X P2
V = volume
P = pressure

61
Q

Charles’ Law

A 
V1/T1 = V2/T2
V = volume
T = temperature
62
Q

Avagadro’s Law

A 
V1/n1 = V2/n2
V = volume
n = number of moles
63
Q

Gay-Lussac’s Law

A 
P1/T1 = P2/T2
P = pressure
T = temperature
64
Q

Ideal Gas Law

A
  • PV = nRT

- R = known gas constant (8.31)

65
Q

Combined Gas Law

A

V1xP1/T1 = V2xP2/T2

66
Q

How is the value for R determined?

A
  • Under a set of standard conditions called “standard temperature and pressure” or STP.
    -standard temp = 0c or 273K
    R = .0821atm/L/mol/K (old way using atm)
    R = 8.31kPa/L/mol/K (new way using kPa)
67
Q

Based on Avogadro’s Law at STP, what is the volume of 1 mole on any gas?

A

22.7L

68
Q

Relationship between volume of gas and the pressure exerted on it (Boyle’s Law)

A
  • Gas is inversely proportional to pressure, if temperature and moles are constant.
  • If you increase pressure on the gas, its volume decreases and vice versa
69
Q

Boyle’s Law Applications

A
  • Ambubag being squeezed
  • Pushing syringe against resistance
  • Inspiration
  • O2 cylinder
70
Q

Relationship between volume of gas and its temperature (Charles’ Law)

A
  • Volume of gas is directly proportional to temperature

- By increasing the temperature, a gas expands to increase its volume and vice versa

71
Q

Relationship between volume of gas and number of moles (Avogadro’s’ Law)

A
  • There is a direct relationship

- As number of moles increases, so does the volume of the gas, and vice versa

72
Q

Avogadro’s number

A
  • The number of molecules in one mole of

- 6.022 x 10^23

73
Q

Calculate the volume of 12 moles of N2O would occupy at STP?

A

1mol/22.7L = 12mol/xL –> x = 272.4L

74
Q

Ideal Gas

A
  • aka perfect gas
  • hypothetical gas that consists of particles of zero volume and intermolecular forces
  • Real gasses do not exhibit these characteristics
  • These characteristics break down at high pressures and low temperatures
75
Q

Vapor

A
  • When a gas coexist in equilibrium with its liquid
  • Molecules are moving from liquid to gas and vice versa at the same rate
  • A gas is in equilibrium with its associated liquid
  • Follows Dalton’s law of Partial Pressure
76
Q

Dalton’s law of Partial Pressure

A

Ptotal = P1 + P2 + P3……

77
Q

Tripple Point

A

The temperature and pressure at which it exists simultaneously, in thermodynamic equilibrium, as a solid, liquid, and gas.
- Tripple Point for water = 273.16K or 0.01C

78
Q

Van der Waals forces

A

Include attraction and repulsions between atoms, molecules, and surfaces, as well as other intermolecular forces

79
Q

How many meters in 1 mile

A

I mile = 1609 meters

80
Q

Difference between Work and Energy

A
  • Work is the expenditure of Energy

- Energy is the ability to do Work

81
Q

Units of measurement for work when calculation pressure and changing volume?

A
  • Pressure units = Pascals

- Volume units = Liters

82
Q

The average kinetic energy of a sample of gas molecules is most closely related to ______?

A

The temperature of the sample

83
Q

Official SI units of measurement for Flow

A

m^3/s

84
Q

What is the flow rate for the following gauges of IV:

1) 24G
2) 22G
3) 20G
4) 18G
5) 16G
6) 14G

A

1) 24G - 20mL/min
2) 22G - 35mL/min
3) 20G - 60mL/min
4) 18G - 105mL/min
5) 16G 220mL/min
6) 14G - 330mLmin

CRNA CHEM & PHYS (2 decks)

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