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Course Review Flashcards

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1
Q

1: 200,000 =
1: 100,000 =
1: 10,000 =

A

5 mcg/mL
10 mcg/mL
100 mcg/ml

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2
Q

Ratios are expressed in

A

g/mL

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3
Q

What is the concentration in mcg/mL of

epinephrine 1:200,000?

A

5 mcg/mL

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4
Q

What is the final concentration in mcg/ml when 4 mg of a drug is placed in 250 ml?

A

16 mcg/ml

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5
Q

Fresh Gas in the OR

A

– Oxygen
– Air
– Nitrous Oxide (N2O)

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6
Q

What is the percent of inspired O

2 when flows are 2 L/min O 2 and 2 L/min N2O?

A

50%

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7
Q

What is the percent O

2 when 2 L/min O2 and 2 L/min air are flowing?

A

60.5%

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8
Q

What is the percent O2 when 1 L/min O2 and 2

L/min N2O are flowing?

A

– 33%

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9
Q

ABL Equation

ABL =

A

((Original H - Final H)/ Original H) x EBV

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10
Q

Estimated Blood Volume, these values are calculated based

A

upon: Age, Sex, Weight

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11
Q

EBV =

A

body wt (kg) x average blood volume (ml/kg)

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12
Q

Given: initial Hgb 14, male blood volume 75 ml/kg, weight

70 kg, minimum Hgb 8, determine the EBV and ABL.

A

EBV = 75 * 70 ml/kg = 5250 ml

ABL = ((14-8)/14)) * 5250 = 2250 ml

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13
Q

Moles used in chemistry to identify or measure

A

how much of a substance is present.

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14
Q

Uses Avogadro’s number:

A

6.02x10^23

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15
Q

Avocadro’s number is based on

A

Carbon

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16
Q

Convert a.m.u.s to grams =

A

12 grams for one “mole” of Carbon

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17
Q

One mole of ANYTHING contains

A

6.02x10^23 particles

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18
Q

What is the Molar Mass of Oxygen?

A

16g/mol

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19
Q

What is the Molar Mass of H2O?

A

18g/mol

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20
Q

Cations (+)

Anions (-)

A

have positive electrical charge, example (Na+)

Anions (-) have negative electrical charge,

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21
Q

Ionic Compounds

A

A metal donates its electron to a non-metal

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22
Q

The number of Electrons should equal the number of

A

Protons

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23
Q

1 N/m2 =

A

1 pascal = 1 Pa

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24
Q

Pressure Defined as force per unit area

A

P = Force/Area

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25
Q

How much pressure is created when you apply a 5.00 N force on a syringe plunger that has a diameter of 1.00 cm? in KPA

A

63.7 kPa

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26
Q

Area of a circle =

A

π r ²

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27
Q

How much pressure is created when you apply a 5.00 N force on a syringe plunger that has a diameter of 2.00 cm?

A

15.9 kPa

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28
Q

Pressure is __________to the square of the Area when the area is increased.

A

inversely proportional

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29
Q

Doubling the diameter of the syringe decreased the pressure

A

by a factor of 4.

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30
Q

__________syringes have the capacity to develop very

high pressures!

A

Smaller

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31
Q

1 atm = _______mmHg =______kPa

A

760 ; 101. 3

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32
Q

101 kPa = psi

A

14.7

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33
Q

Bourdon gauge =

A

gauge pressure – atmospheric pressure

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34
Q

At zero pressure the pressure in the cylinder is equal to

A

atmosphere

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35
Q

O2 tank gauge reads 45 psi. What is the total (absolute) pressure in the tank?

A

59 psi

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36
Q

Dalton’s Law of Partial Pressures

A

The total pressure exerted by a gaseous mixture is equal
to the sum of the partial pressures of each individual
component: P1 + P2 + P3 + ….. = Ptotal

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37
Q 
Calculating partial pressures for nitrogen and oxygen at 1
atmosphere (at sea level)
Nitrogen 78%
 Oxygen 21%
answer in mmhg andKpa
A

593 (79 kpa)

159 (21.2 Kpa)

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38
Q

Denver, altitude 5,183 ft above sea level, atmospheric
pressure 635 mmHg (85kPa)
What are the partial pressures of N2O and O2 during a 70:30 induction?

A

445

191

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39
Q

Formula:work W =

A

F xD

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40
Q

It is measured in units called joules ( J )

A

Work

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41
Q

newton and meter combination

A

Joule

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42
Q

J is

A

kg/m²/s²

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43
Q

How much work is done (in Joules) lifting a 100kg patient
up a distance of 0.02 m straight up to place him onto the
operating table? W= first find weight
How much work is done lifting a 100kg patient up a
distance of 0.02 m straight up to place him onto the
operating table?

A

mg

=980 N
19.6N

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44
Q

How much work was done by the expanding

gas?

A

W = P x change in V

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45
Q

How much work is done when 2.5L of gas expands to

3L against 600 Pa?

A

W=0.3J

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46
Q

Ventilator doing work for the body, operating at a constant pressure of 600 Pa is used to increase the volume of air in the lungs by 500ml (5.00x10^-4m³).

A

W=0.300

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47
Q

volume of a cylinder =

A

area * height

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48
Q

Q =

A

volume/time)

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49
Q

If water is moving at a speed of 0.20 m/s through a tube
with a cross-sectional area of 0.02 m2, what is the flow
rate?

A

Q = a * v
Q = a*d/t,
4 L /s

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50
Q

Poiseuille’s Law

A

The Hagen-Poiseuille equation defines the flow through a tube and how this flow is affected by the attributes of the tube; the length and radius, and the attributes of the fluid; the viscosity. The equation only applies to fluids
undergoing laminar flow through tubes.

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51
Q

Poiseuille’s law formula

A

Pir^4 change in Pressure / 8 n l

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52
Q

Calculate aortic blood flow. Blood viscosity =

0.0015Pas. Pressure of 13,000 Pa (or 100mmHg) is applied to the aorta (r = 0.010m; l = 1.0m)

A

3.4 x 10 -2 m 3 /s

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53
Q

Blood Flow =

A

Rate of uptake or excretion ml/min

/

arterial – venous concentration

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54
Q

Boyle’s Law Qs ask you to find

A

Volume or Pressure

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55
Q

Charles’s Law Qs ask you to find

A

Volume or Temp

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56
Q

Gay-Lussac Law Qs ask you to find Lussac Law Qs

A

ask you to find Pressure or Temp

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57
Q

Avogadro’s law ask you to find

A

Volume or moles

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58
Q

P1/T1 = P2/T2

A

Gay Lussacs’

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59
Q

Ideal

A

PV=nRT

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60
Q

Combined gas law

A

P1V1 / T1 = P2V2/T2

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61
Q

R is a known gas constant =

A

8.31

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62
Q

An increase in temperature causes an

A

increase in Vapor Pressure and in “Volatility”.

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63
Q

Volatility is the tendency of

A

a liquid to change into gas.

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64
Q

Higher volatility =________evaporation (ie. ROH vs. H2O)

Higher volatility =_______ vapor pressure

A

higher higher

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65
Q

Define Vapor pressure

A

When molecules of a liquid escape into the gas phase,
they collide with the walls of the container, exerting a
force on the walls. This is called Vapor Pressure.

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66
Q

Dipole-dipole, ex:________
_______molecule
Boiling point________, _____(what is the state @ room temp)

A

acetone; Polar 56C

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67
Q

*Hydrogen bonding, ex._______
_______ molecule
_______type of dipole bond
Boiling point, _____(what is the state @ room temp)

A

Water; Polar
Strongest
100C
liquid

68
Q

London dispersion forces, ex:______
_______molecule
________ type of intermol. bond
Boiling pt.______ , ____state at room temperature

A

CH4
Non-polar
Weakest
-164C

69
Q

Liquid to gas

A

Vaporization

70
Q

Gas to liquid

A

Condensation

71
Q

Gas to solid

A

deposition

72
Q

Solid to Gas

A

Sublimation

73
Q

Solid to liquid

A

melting

74
Q

Liquid to solid

A

Freezing

75
Q

Clausius-Capeyron Equation

A

logP = A + B/T

76
Q

Clausius-Capeyron Equation used

A

This equation is used to calculate the Vapor

Pressure of a liquid

77
Q

For Ex: For enflurane enflurane, A = 7.967 , A = 7.967 torr, B = -1678 torr•K
What is the vapor pressure of enflurane at 25C?

A

logP = 2.34

217 torr

78
Q

Molarity (M) is

A

moles of solute per liter of solution.

79
Q

Molarity: If you dissolved

A

1 mol of glucose in enough
water to give you a total of 1 L of solution, you
would have 1 molar solution of glucose.

80
Q

Calculate the molarity of a D5W solution prepared by

dissolving 1 g of glucose (C6H12O6) in enough water to give a total volume of 20 ml.

A

180g

0.28 M

81
Q

Moles of solute (m) per kilogram of solvent

A

MolaLITY

82
Q

Calculate the molality of a solution prepared by dissolving 1 gof glucose in 20 g of water

A

M= 0.28

83
Q

Percent by Weight to Volume (% w/v)
• Allows you to measure out a volume of medicine in a syringe andcalculate the mass of the drug.
• Defined as____________

A

grams of solute per 100 ml solution

84
Q

What is the concentration of a solution prepared by dissolving 25g of glucose in enough water to give a total volume of 500 ml?

A

5%

85
Q

How many liters of D5W are required to deliver 100g of

glucose?

A

2000 ml D5W

86
Q

• g of solute/g of solution x 100%

A

% w/w Problem

87
Q

What is the percent by weight conc. Of glucose in a solution prepared by dissolving 25 g glucose in 475 g of water?

A

5%

88
Q

One Eq of a substance contains

A

one mole of chemical

reactivity.

89
Q

Na+ cation has

Ca2+ cation has

A

1 Eq/mol

2 Eq/mol

90
Q

Pt.s blood work says calcium ion content is 40 mEq/L.

Calculate moles per Liter?

A

0.02mol/L

91
Q

Henry’s Law gives relationship

A

Gives relationship between pressure and solubility

92
Q

S =

A

k(H) * Pgas

93
Q

The Henry’s Law constant for oxygen in water is 0.042 g/L/atm at 25C. What is the solubility (in mg/L) of O2 in pure water at 740 torr room air?

A

first convert to atm

8.6 mg/L

94
Q

Calculate [H+] for pH of 7.4?

A

0.00004 mEq/L

95
Q

shortcut for nEq/L

A

[H+] = 10 ^(9 - 7.3)

96
Q

Calculate pH of a solution when the [H+] is 1.0 x

10^-3 M

A

pH = -log (1.0 x 10^-3 M) = 3.00

97
Q

Kassirer-Bleich equation:

A

(allows calculation of [H+] and pH if PCO2 and

HCO3 are known)

98
Q

Kassirer-Bleich equation: is

A

[H+] = 24 x PCO2/HCO3 ¯

99
Q

Organic compounds only containing Carbon

and Hydrogen are called

A

Hydrocarbons

100
Q

One single Carbon

A

Alkanes

101
Q

one double bonded carbon

A

Alkenes

102
Q

One triple bonded carbon

A

Alkynes

103
Q

Methane, Ethane, Propane, Butane

A

Men Eat pussy big time

104
Q

Alkyl Halides – ‘

A

RX’

105
Q

Alkyl group (ex. CH3-) bonded with a

A

Halogen

• F, Cl, Br, I

106
Q

Example: Fluoromethane

A

C3 and one F

107
Q

Amines – RNH2

A

An amine is an organic compound formed by
replacing one or more of the hydrogen atoms
in the ammonia molecule (NH3) by an Alkyl
group

108
Q

Structure of amine group

Examples

A

Has the structure R-NH2

• Example: methylamine (CH3NH2)

109
Q

Esters formula

A

R(C=O)OR

110
Q

Amides

A

R(C=O)NH2

111
Q

Amide definition

A

NH2 bound to carbonyl

112
Q

Amino Esters – metabolized in the

PCT CB

A

Blood

– Procaine
– Cocaine
– Tetracaine
– Chloroprocaine
– Benzocaine
113
Q

Amino Am-i-des - metabolized in the liver
LEMB
–

A

Lidocaine
– Mepivacaine
– Bupivacaine
– Etidocaine

114
Q

• Conductors

A

– Any substance that permits the flow of electrons (or current)

115
Q

Electricity is the

A

flow of electrons

116
Q

Current:

A

Flow of electrically charged particles

117
Q

Circuit: Electrons flow

A

around a closed path.

118
Q

There are two types of circuits:

•

A

Direct Current (DC), and alternating current (AC) circuits. –

119
Q

DC circuits:

A

Parallel

series

120
Q

Direct Current (DC) –

A

The flow of electrons in one direction

121
Q 
Alternating Current (AC)
–
A

Electrons flow switches directions at regular intervals (120 times per second for 60
Hz wall current)

122
Q

Voltage (V) =

A

pressure behind electrons

123
Q

• Amps (I) =

A

current: number of electrons

flowing past a given point per unit of time

124
Q

• Ohms

A

Ω (R) = resistance to the flow

125
Q

Voltage =

A

Current x Resistance V = I x R

126
Q

Macroshock –

A

large current flows that can cause harm

127
Q

Microshock microamps
____________Ventricular Fibrillation.
–

A

– small amounts of current flow
only dangerous to susceptible individuals (ex.
Pacing wires and central lines)
– 100

128
Q

V-Fib

A

100 (0.1 A)

129
Q

_______is the maximum recommended leakage current.

A

10 microamps:

130
Q

V-Fib in humans (direct contact w/ heart)

A

100 microshock

131
Q

Line isolation monitor Continuously monitors the

A

potential for current flow from the isolated power supply to the ground

132
Q

The Line Isolation Monitor

A

• A safety device that monitors for Leakage current from internal faults

133
Q

The line monitor Alarm between

A

2 – 5 mA potential leak (5 mA = maximal harmless current)

134
Q

• If the alarm sounds, the______ piece of equipment should be

A

last ; disconnected and inspected.

135
Q

• Equipment that activates a line isolation monitor alarm may still be ______, but increases

A

.operational ; the potential risk of shock

136
Q

• Equipment that activates a line isolation monitor alarm may still be ______, but increases

A

operational ; the potential risk of shock

137
Q

Types of radiation

A

Electromagnetic and particulate

138
Q

Electromagnetic (EM) -_______
–
–
–

A

photons
Gamma rays
X-rays
UV

139
Q

Particulate
–
–

A

Alpha (He2+ nucleus)

Beta (electron or positron)

140
Q

β−

A

decay (electron emission) – neutron is converted into a proton, an electron, and an antineutrino
n → p + e- + oῡe

141
Q

β+

A

decay (positron emission) – proton is converted into a neutron, a positron, and a neutrino
p → n + e+ + υe

142
Q

Electron Capture Decay

A

When an inner shell e- is drawn into the nucleus
and combines with a proton, forming a neutron
and a neutrino.
The neutrino is ejected from the atom’s nucleus

143
Q

In electron Capture Decay if the nucleus is left in

A

If the new nucleus is left in an excited state, gamma rays (γ) will also be emitted.
•p+ + e- → n + υe + γ

144
Q

Coherent scatter

• a.k.a. “___________

A

Thompson scatter”

145
Q

Coherent scatter Occurs when an
– The atom.
– The atom then

A

incident photon collides with an atom.
momentarily absorbs the energy and moves into an excited states
releases the same energy as another
photon traveling in a different direction as scatter rad.

146
Q

Compton scatter

A

• Occurs when incident photon collides with outer
orbital e-.
The e- is ejected from its orbit.
The photon is deflected from its original path and
continues with decreased energy in a new direction
as a scatter radiation

147
Q

Photoelectric Scatter

A

Occurs when an incident photon collides with an
inner shell orbital e-.
The e- is ejected.
When an outer orbital e- moves to the inner orbit to fill the vacated space, the difference in binding energy
between the 2 electron shells is emitted in the form of a new scatter photon.

148
Q

Somatic effects

A

– Short-term

– Long-term (“latent”)

149
Q

Short Term EFFECT Further categorized according to body system affected:
–
• Observed within
• Involve very

A

Hematologic (dysplastic anemia)
– GI (“radiation sickness” damaged mucosal lining w/ infx)
– CNS (seizures, coma, death)

3 months of exposure
high doses (unlike medical imaging)
150
Q

Long term effects
observed?
3 effects

A

Long-term Effects
• Observed at 5 – 30 years, avg. at 10 – 15 years
Latent effects of long term low dose ionizing radiation
– Cataracts (with extensive fluoroscopy)
– Cancer (skin, thyroid, breast & leukemia)
– Shortened Life span

151
Q

Rem (rem) is a

A

unit of Equivalent Dose (EqD

152
Q

Biologic effects of radiation vary

A

according to the type of radiation involved.

153
Q

Rem stands

A

for “radiation equivalent man”

154
Q

To calc. occupational dose, a

A

radiation weighting factor (WR) is assigned to each type of radiation.

155
Q

WR values are based on

A

variation of biologic damaged produced by each type of radiation

156
Q

Type of radiation vs weighing factor (WR)

Xray, gamma, beta

A

1

157
Q

Type of radiation vs weighing factor (WR)

Slow neurons

A

5

158
Q

Type of radiation vs weighing factor (WR)

Fast neurons

A

10

159
Q

Type of radiation vs weighing factor (WR)

Alpha particles

A

20

160
Q

Worker receives 10rads alpha particles and 5rads
x-rays. what is the EqD?
How many Sv did the worker in the previous
problem receive?

A

10(20) + 5 (1) = 205 rem

1 Sv =100 rem = 2.05

161
Q

EqD

A

EqD = D x W(R)

162
Q

Corresponding SI unit of a rem is

A

the Sievert (Sv)

163
Q

1 Sv

A

100 rem

164
Q

In addition to monitoring doses, radiation safety
practices are employed.
• ALARA -acronym:

A

As Low As Reasonably Achievable

165
Q

• 3 Factors of ALARA: –

A

Time – Distance – Shielding

166
Q

________L in one m ³

A

1000

SRNAChem&Physics (13 decks)

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