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1-Physics Exam 1 > Kinetic Molecular Theory > Flashcards

Kinetic Molecular Theory Flashcards

1
Q

What is matter?

A

Composed of small particles called molecules, and molecules are composed of atoms.

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2
Q

What form can matter take?

A

solid, liquid, or gas

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3
Q

What is a solid?

A

Molecules in a solid are held together closely by intermolecular forces.

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4
Q

What is a liquid?

A

Molecules in a liquid are held together by intermolecular forces

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5
Q

What is gases?

A

Molecules in a gas move linearly, and the attractive forces between molecules are less than their kinetic energy. They move almost completely free of one another.

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6
Q

What is the movement of solids?

A

They may move about slightly and vibrate

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7
Q

What is the movement of a liquid?

A

May slide or flow by one another

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8
Q

What is the movement of a gas?

A

They move almost completely free of one another. Move in chaos

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9
Q

What is kinetic energy?

A

Studies the movement of molecules

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10
Q

What is kinetic molecular theory?

A

Describes the actions of gases. This theory explains how molecules behave as they follow the laws of thermodynamics.

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11
Q

What is the focus of kinetic molecular energy?

A

Molecular movement (energy) and forces between these molecules

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12
Q

Who’s finding have made up the the kinetic molecular theory?

A

Charles, Boyle, and Gay-Lussac

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13
Q

General assumptions of the KMT: Molecules have no ______.

A

Volume

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14
Q

General assumptions of the KMT: Gas molecules exert no force on each other unless they ________.

A

Collide

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15
Q

General assumptions of the KMT: Collisions of molecules with each other or the walls of the container do not decrease the ____ of the system

A

Energy

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16
Q

General assumptions of the KMT: The molecules of a gas are in ______and random _____.

A

Constant; Random

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17
Q

General assumptions of the KMT: The _______ of a gas depends entirely on its average kinetic energy.

A

Temperature

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18
Q

General assumptions of the KMT: The energy of a gas is entirely ________.

A

Kinetic

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19
Q

What is gas law?

A

Allow us to calculate the behavior of gases when one of the three factors of pressure, volume, or temperature remains unchanged.

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20
Q

What is the clinical significant of gas law?

A

Expressed by the ability to calculate the available volume of oxygen from a known cylinder of any known pressure.

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21
Q

What is the formula for Charles Law?

A

V1/T1=V2/T2

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22
Q

What is the formula for Gay Lussac’s Law?

A

P1/T1=P2/T2

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23
Q

What is the formula for Boyle’s Law?

A

P1V1=P2V2

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24
Q

What remains constant in Boyle’s Law?

A

Temperature

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25
What remains constant in Charles's Law?
Pressure
26
What remains constant in Gay-Lussac's Law?
Volume
27
What is Charles's Law?
Studied the relationship of volume and temperature at constant pressure
28
What is the relationship described in charles's law?
Found that the volume-to-temperature relationship is directly proportional.
29
What is Boyle's Law?
Studied the relationship of pressure and volume at a constant temperature
30
What is the relationship described in Boyle's law?
Found that the pressure-to-volume relationship is indirectly proportional
31
What is Gay-Lussac Law?
Studied the relationship of pressure and temperature at constant volume.
32
What is the relationship described in Gay-Lussac Law?
Found that the pressure-to-temperature relationship is directly proportional
33
What is the Universal Gas Law?
Unified the findings of Charles, Boyle, and Gay-Lussac to develop the ideal gas law: PV=nrT ``` P = Pressure V = Volume N = Number of moles r = Constant (0.0821 liter-atm/K/mole) T = Temperature ```
34
What is the Universal Gas Law allow us to do?
How much oxygen is available to be released from a partially full oxygen cylinder? At what temperature will a full oxygen cylinder exceed its recommended pressure when heated?
35
What is mole?
Is the gram molecular weight of a gas.
36
What is molecular weight?
Atomic (or molecular) weight is the additive weight of all of the atomic particles, protons, neutrons, and electrons in an atom or molecule.
37
In the example given, we calculate the volume in liters that 1 mole of oxygen will expand to at 1 atmosphere pressure at standard temperature (0°C). Celsius is converted to Kelvin.
One mole of any gas at 0°C will expand to 22.4 liters
38
which _____ of a gas will expand at any given temperature or pressure.
1 mole
39
What can be used to explain the relationship of Universal Gas Law?
To simplify the concept, we can view the universal gas law as: - PV = T - T/P = V - T/V = P when a constant is present
40
What conditions must be met in the Universal Gas Law?
Represents ideal gas
41
When the Universal Gas Law not occur?
Adiabatic changes
42
If an oxygen tank reads 900 PSI how long in minutes before it runs out if the flow rate is set at 2 L/min.
156 min
43
If an oxygen tank reads 900 PSI how long in minutes before it runs out if the flow rate is set at 2 L/min. How many hours before it runs out?
2.6 hr
44
What does the universal gas law allow us to calculate?
The universal gas law allows us to calculate the amount of gas in an E-cylinder based on the current pressure.
45
For an E-cylinder of O2 assume it equals _____ L on the exam
660 L
46
For an E-cylinder of O2 assume it equals _____ Psig on the exam
1900
47
How is nitrous oxide different then other gases?
Stored as a liquid because it has a different boiling point and temperature
48
What is important to known about calculating nitrous oxide?
Can't use the regular gas equations to figure this out (stored at liquid)
49
What happens to the nitrous oxide tank when it reaches 1/4 or 400L full?
Rapidly empty
50
Amedeo Avogadro was able to show that in a mole of any gas, there are __________molecules
6.022 x 10^23 molecules
51
How much does a mole of helium weigh? Number of molecules contained?
4 g; 6.022 × 10^23 molecules
52
How much does a mole of oxygen weigh? Number of molecules contained?
Weighs 32 g and contains 6.022 × 1023 molecules;
53
Oxygen is a molecule composed of two oxygen atoms bonded together, and therefore the molecular weight of the diatomic oxygen molecule is ______
32 g
54
The universal gas law is also called the ideal gas law because it explains the __________ if they were “ideal.”
Behavior of gases
55
What are the components of an ideal gas?
Would possess molecules that occupy no volume and never interact with other molecules.
56
What is important regarding the gas molecules?
Do have volume and do occupy space, and therefore the volume they occupy must be taken into account when calculating a gas's expansion or contraction.
57
The universal gas law does not account for _________ because Charles, Boyle, and Gay-Lussac did not account for this in their studies.
gas molecule volume
58
The simplicity of the universal gas law and molecular kinetic theory are ________ for describing the behavior of gases used for anesthesia
immensely valuable
59
What is vander waal's equation?
Corrects the universal gas law and accounts for molecular volume and molecular interaction in a gas
60
An ideal gas assumes ___________ forces.
intermolecular forces.
61
What does dalton's law state?
That the total pressure of a system is the additive pressure of each individual gas in a mixture.
62
What type of pressure will be exerted when multiple gases are in a mixture?
A pressure in proportion to its percentage in the mixture. (Summative effect of all the forces)
63
What is the formula for Dalton's law?
Pt=P1+p2+p2+p3+p4+p5
64
The total pressure is the summation of individual | __________ with the walls of a container
Molecular collisions
65
What is partial pressure?
Describes the amount of pressure exerted by one particular gas in a mixture of gases
66
What is the relationship between pressure and gas concentration according to Dalton's Law?
The higher the concentration of a gas, the higher the pressure it will exert
67
This principle governs the way that gases, such as oxygen and carbon dioxide are picked up and transported in the circulatory system.
Dalton’s Law of Partial Pressures
68
What is the partial pressure of 79% Nitrogen?
0.79 × 760 mm Hg = 600.4 mm Hg partial pressure of nitrogen
69
What is the partial pressure of 21% Oxygen?
0.21 × 760 mm Hg = 159.6 mm Hg partial pressure of oxygen
70
Partial pressures added up will always equal ________.
Total atmospheric pressure- 760 mmHg
71
Equilibration of energy takes ________.
Time
72
What can happen from the rapid expansion or compression of gases?
May exceed the speed of energy/heat equilibration with the surrounding environment
73
What is an adiabatic process?
Rapid expansion or compression of a gas without equilibration of energy/heat with the surrounding environment
74
What happens to energy in an adiabatic process?
There is NO increase or decrease in a system’s energy.
75
What are examples of adiabatic process?
Freezing and explosions
76
What is an example of an adiabatic change in anesthesia?
When a gas cylinder is connected to the anesthesia machine and opened quickly, the pressure of the gas in the connecting pipes and gauges rises rapidly. Risk of fire
77
What is the relationship of temperature and gas cylinders?
The gas in the pipe system is compressed adiabatically and a large temperature increase can occur.
78
What does adiabatic demonstrate in relationship to ideal gas laws?
This quick increase does not allow time for energy equilibration pushed it beyond these laws
79
What types of adiabatic processes are there?
Heating and cooling effect
80
Who explained the Adiabatic cooling effect?
Joule-Thompson Effect
81
What happens in the cooling process of adiabatic effect?
When we lower the pressure of a gas (i.e., increase its volume) quickly, we lower the energy per area. The temperature measurement will be lower when the volume is rapidly expanded.
82
What is the relationship of energy and volume according to the Joule-Thompson Effect?
The total energy of the gas has not changed, but the expression (or thermal measurement) is decreased related to the increased volume.
83
What may happen to the cylinder outlet during the Joule-Thompson Effect?
Frosting
84
What is an example of medical purposes that use the Joule-Thompson Effect?
Cryoprobe
85
What is Cryoprobe?
Used for rapid freezing of tissues in the treatment of skin lesions, cardiac ablations, or when applied to nerves it causes local degeneration of nerve bundles with resulting long term (3-6 months) local analgesia.

1-Physics Exam 1 (4 decks)

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