Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

1-Physics Exam 1 > Kinetic Molecular Theory > Flashcards

Kinetic Molecular Theory Flashcards

You may prefer our related Brainscape-certified flashcards:
Physics 101 flashcards AP® Physics flashcards
1
Q

What is matter?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What form can matter take?

A

solid, liquid, or gas

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What is a solid?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What is a liquid?

A

Molecules in a liquid are held together by intermolecular forces

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What is the movement of solids?

A

They may move about slightly and vibrate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What is the movement of a liquid?

A

May slide or flow by one another

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What is the movement of a gas?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What is kinetic energy?

A

Studies the movement of molecules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What is the focus of kinetic molecular energy?

A

Molecular movement (energy) and forces between these molecules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

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

A

Charles, Boyle, and Gay-Lussac

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

General assumptions of the KMT: Molecules have no ______.

A

Volume

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

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

A

Collide

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

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

A

Constant; Random

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

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

A

Temperature

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

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

A

Kinetic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What is the formula for Charles Law?

A

V1/T1=V2/T2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What is the formula for Gay Lussac’s Law?

A

P1/T1=P2/T2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What is the formula for Boyle’s Law?

A

P1V1=P2V2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

What remains constant in Boyle’s Law?

A

Temperature

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

What remains constant in Charles’s Law?

A

Pressure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

What remains constant in Gay-Lussac’s Law?

A

Volume

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

What is Charles’s Law?

A

Studied the relationship of volume and temperature at constant pressure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

What is the relationship described in charles’s law?

A

Found that the volume-to-temperature relationship is directly proportional.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

What is Boyle’s Law?

A

Studied the relationship of pressure and volume at a constant temperature

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

What is the relationship described in Boyle’s law?

A

Found that the pressure-to-volume relationship is indirectly proportional

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

What is Gay-Lussac Law?

A

Studied the relationship of pressure and temperature at constant volume.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

What is the relationship described in Gay-Lussac Law?

A

Found that the pressure-to-temperature relationship is directly proportional

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

What is the Universal Gas Law?

A

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
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

What is the Universal Gas Law allow us to do?

A

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?

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

What is mole?

A

Is the gram molecular weight of a gas.

36
Q

What is molecular weight?

A

Atomic (or molecular) weight is the additive weight of all of the atomic particles, protons, neutrons, and electrons in an atom or molecule.

37
Q

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.

A

One mole of any gas at 0°C will expand to 22.4 liters

38
Q

which _____ of a gas will expand at any given temperature or pressure.

A

1 mole

39
Q

What can be used to explain the relationship of Universal Gas Law?

A

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
Q

What conditions must be met in the Universal Gas Law?

A

Represents ideal gas

41
Q

When the Universal Gas Law not occur?

A

Adiabatic changes

42
Q

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.

A

156 min

43
Q

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?

A

2.6 hr

44
Q

What does the universal gas law allow us to calculate?

A

The universal gas law allows us to calculate the amount of gas in an E-cylinder based on the current pressure.

45
Q

For an E-cylinder of O2 assume it equals _____ L on the exam

A

660 L

46
Q

For an E-cylinder of O2 assume it equals _____ Psig on the exam

A

1900

47
Q

How is nitrous oxide different then other gases?

A

Stored as a liquid because it has a different boiling point and temperature

48
Q

What is important to known about calculating nitrous oxide?

A

Can’t use the regular gas equations to figure this out (stored at liquid)

49
Q

What happens to the nitrous oxide tank when it reaches 1/4 or 400L full?

A

Rapidly empty

50
Q

Amedeo Avogadro was able to show that in a mole of any gas, there are __________molecules

A

6.022 x 10^23 molecules

51
Q

How much does a mole of helium weigh? Number of molecules contained?

A

4 g; 6.022 × 10^23 molecules

52
Q

How much does a mole of oxygen weigh? Number of molecules contained?

A

Weighs 32 g and contains 6.022 × 1023 molecules;

53
Q

Oxygen is a molecule composed of two oxygen atoms bonded together, and therefore the molecular weight of the diatomic oxygen molecule is ______

A

32 g

54
Q

The universal gas law is also called the ideal gas law because it explains the __________ if they were “ideal.”

A

Behavior of gases

55
Q

What are the components of an ideal gas?

A

Would possess molecules that occupy no volume and never interact with other molecules.

56
Q

What is important regarding the gas molecules?

A

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
Q

The universal gas law does not account for _________ because Charles, Boyle, and Gay-Lussac did not account for this in their studies.

A

gas molecule volume

58
Q

The simplicity of the universal gas law and molecular kinetic theory are ________ for describing the behavior of gases used for anesthesia

A

immensely valuable

59
Q

What is vander waal’s equation?

A

Corrects the universal gas law and accounts for molecular volume and molecular interaction in a gas

60
Q

An ideal gas assumes ___________ forces.

A

intermolecular forces.

61
Q

What does dalton’s law state?

A

That the total pressure of a system is the additive pressure of each individual gas in a mixture.

62
Q

What type of pressure will be exerted when multiple gases are in a mixture?

A

A pressure in proportion to its percentage in the mixture. (Summative effect of all the forces)

63
Q

What is the formula for Dalton’s law?

A

Pt=P1+p2+p2+p3+p4+p5

64
Q

The total pressure is the summation of individual

__________ with the walls of a container

A

Molecular collisions

65
Q

What is partial pressure?

A

Describes the amount of pressure exerted by one particular gas in a mixture of gases

66
Q

What is the relationship between pressure and gas concentration according to Dalton’s Law?

A

The higher the concentration of a gas, the higher the pressure it will exert

67
Q

This principle governs the way that gases, such as oxygen and carbon dioxide are picked up and transported in the circulatory system.

A

Dalton’s Law of Partial Pressures

68
Q

What is the partial pressure of 79% Nitrogen?

A

0.79 × 760 mm Hg = 600.4 mm Hg partial pressure of nitrogen

69
Q

What is the partial pressure of 21% Oxygen?

A

0.21 × 760 mm Hg = 159.6 mm Hg partial pressure of oxygen

70
Q

Partial pressures added up will always equal ________.

A

Total atmospheric pressure- 760 mmHg

71
Q

Equilibration of energy takes ________.

A

Time

72
Q

What can happen from the rapid expansion or compression of gases?

A

May exceed the speed of energy/heat equilibration with the surrounding environment

73
Q

What is an adiabatic process?

A

Rapid expansion or compression of a gas without equilibration of energy/heat with the surrounding environment

74
Q

What happens to energy in an adiabatic process?

A

There is NO increase or decrease in a system’s energy.

75
Q

What are examples of adiabatic process?

A

Freezing and explosions

76
Q

What is an example of an adiabatic change in anesthesia?

A

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
Q

What is the relationship of temperature and gas cylinders?

A

The gas in the pipe system is compressed adiabatically and a large temperature increase can occur.

78
Q

What does adiabatic demonstrate in relationship to ideal gas laws?

A

This quick increase does not allow time for energy equilibration pushed it beyond these laws

79
Q

What types of adiabatic processes are there?

A

Heating and cooling effect

80
Q

Who explained the Adiabatic cooling effect?

A

Joule-Thompson Effect

81
Q

What happens in the cooling process of adiabatic effect?

A

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
Q

What is the relationship of energy and volume according to the Joule-Thompson Effect?

A

The total energy of the gas has not changed, but the expression (or thermal measurement) is decreased related to the increased volume.

83
Q

What may happen to the cylinder outlet during the Joule-Thompson Effect?

A

Frosting

84
Q

What is an example of medical purposes that use the Joule-Thompson Effect?

A

Cryoprobe

85
Q

What is Cryoprobe?

A

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)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions