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Chem/Phys EXAM 2 > Chapter 6 > Flashcards

Chapter 6 Flashcards

Gas laws

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1
Q

Volume & Pressure are

A

Inversely proportional

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2
Q

Volume & Temperature are

A

Directly Proportional

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3
Q

The volume of gas is directly proportional to

A

The number of moles

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4
Q

Boyle’s Law explains the relationship between

A

Volume & pressure

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5
Q

In Boyle’s Law, as the pressure increases,

A

The volume decreases & vice versa

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6
Q

At a higher pressure, gas is more

A

Concentrated & vice versa

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7
Q

Charle’s Law explains the relationship between

A

Volume & temperature

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8
Q

With Charle’s Law, volume of a gas is

A

Proportional to its absolute temperature, as long as the pressure 7 amount of gas are held constant

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9
Q

What is Boyle’s Law equation?

A

P1V1=P2V2

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10
Q

What is the equation for Charle’s Law?

A

V1/T1=V2/T2

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11
Q

With Charle’s Law, temperature must be expressed in

A

Kelvin

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12
Q

How else can you write Charles’s Law?

A

V=mT

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13
Q

Avogadro’s Law explains

A

The relationship between Volume & Mole

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14
Q

At equal temperatures & pressures, equal volumes of gas

A

Contain equal numbers of particles

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15
Q

With Advogadro’s number, the volume of a gas is

A

Directly proportional to the number of gas molecules, as long as temperature & pressure are held constant

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16
Q

What is the Combined Gas Law

A

P1V1/n1T1=

P2V2/n2T2

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17
Q

For gases & only for gases, the volume

A

Percent of each component is always equal to the mole percent

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18
Q

What is the equation for ideal gas law?

A

PV=nRT

P=pressure
V=volume
n=moles
T=absolute temperature
R=constant

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19
Q

Ideal gas does

A

Not exist

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20
Q

Volume is inversely proportional to ________ & directly proportional to_______

A

Pressure; Absolute temperature & to Moles

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21
Q

The standard temperature= is

A

Exactly 0 degree Celsius

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22
Q

The standard pressure is

A

1 bar or 100kPa

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23
Q

1 atm=

A

101.325 kPa=760 torr

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24
Q

What is the standard molar volume of a gas?

A

Is the volume that exactly 1 mole of an ideal gas occupied under STP conditions

22.71 L

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25
Q

R is called the

A

Universal gas constant because it appears in several seemingly unrelated physical relationship

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26
Q

The density of a gas depends very strongly on the

A

Temperature & pressure

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27
Q

Dalton’s Law states the

A

Total pressure of a gaseous mixture is the sum of the partial pressures of each of the component gases

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28
Q

The partial pressure of a gas in a mixture is the

A

Pressure the gas would exert by itself under identical conditions of temperature & volume

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29
Q

The partial pressure of each component is

A

Proportional to the moles of that component in the sample

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30
Q

The partial pressure of each component in a

A

Gaseous mixture is equal to the mole fraction of the component times the total pressure

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31
Q

Relative humidity measures

A

The saturation of water in the air

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32
Q

How do you calculate relative humidity?

A

Concentration of water in the air sample/solubility of water in the air TIMES 100%

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33
Q

The solubility of water in air is the

A

Maximum amount of water that a given volume of air can accommodate, & the solubility of water in air increases with increasing temperature

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34
Q

Relative humidity is also a

A

Function of temperature

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35
Q

If the sample is cooled to a temperature where the actual concentration of water exceeds the solubility of water in air,

A

Dew will form

(dew point temperature)

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36
Q

What another way to calculate relative humidity

A

Partial pressure of water/vapor pressure of water

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37
Q

What is it called when gaseous water molecules exert a pressure

A

Vapor pressure

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38
Q

At higher temperatures, more. water vaporizes into the air &

A

Exerts higher pressure

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39
Q

If the vapor pressure is higher at higher temperatures, then

A

The air has a greater capacity for water at that temperature

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40
Q

The maximum solubility of water in air is directly related to

A

The vapor pressure of water

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41
Q

Increasing humidity decreases

A

Partial pressure of oxygen available for breathing

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42
Q

What are the 4 components of the Kinetic Molecular Theory of Gases?

A
  1. gases consist of small particles whose volume is negligible compared to the volume of the gas
  2. Gas molecules are in constant, random motion
  3. The molecules in the sample show a range of kinetic energies, but the average KE depends only on the temperature
  4. There are no attractive or repulsive forces between the gas particles, so all collisions are elastic
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43
Q

In any sample of gas, the molecules are in

A

Constant random motion, but they do not move all at the same speed

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44
Q

What is the internal energy of a system?

A

The sum of the kinetic & potential energies of the molecules

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45
Q

If you increase the temperature of the sample, the added energy goes

A

Into increasing the average KE of the molecules

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46
Q

Temperature is directly proportional to the

A

Average KE

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47
Q

The distribution of kinetic energies among the molecules in a sample is given by

A

The Maxwell-Boltzmann speed of distribution

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48
Q

No molecule have

A

Zero KE

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49
Q

The number of molecules at a given KE increases to a maximum & then

A

Asymptotically approach zero again

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50
Q

A higher temperature means a

A

Higher average KE

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51
Q

Different gases have the same

A

Average KE if their temperature is the same

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52
Q

Boltzmann constant treats

A

Individual molecules

53
Q

The ideal gas constant deals with

A

Moles of molecules

54
Q

What is diffusion?

A

The movement of a substance from high to low concentration

55
Q

What is Effusion?

A

The movement of a gas through a small opening

56
Q

What is Graham’s Law of Effusion?

A

States the rate of effusion is inversely proportional to the square root of the molecular mass

57
Q

The rate of effusion depends on the

A

Speed of the molecules

58
Q

There are no attractive or repulsive forces between the gas particles so

A

All collisions are elastic

59
Q

Which equation corrects the non-ideal behavior of real gases

A

The Van der Waals equation

60
Q

What is Henry’s Law?

A

At a constant temperature, the amount of gas dissolved in a liquid is directly proportional to the partial pressure of that gas at equilibrium above the gas-liquid interface

61
Q

Increasing the partial pressure of a gas above a liquid will increase the

A

Amount of gas that dissolves in the liquid

62
Q

In Graham’s Law, the rate of effusion of a gas is inversely proportional to the square root of

A

Its molecular weight

63
Q

Diffusion of a fluid through a permeable membrane is dependent on what 5 five factors

A
  1. Concentration Gradient
  2. Tissue Area
  3. Fluid tissue solubility
    4.Directly proportional to diffusion; membrane thickness & molecular weight are inversely proportional to diffusion
64
Q

Diffusion is a

A

Passive process driven by entropy

65
Q

A mole is the

A

Gram molecular weight of gas

66
Q

The atomic (or molecular) weight is the

A

Additive weight of all the atomic particles, protons, neutrons & electrons in an atom or molecule

67
Q

A mole of gas is equal to the

A

Molecular weight of the gas expressed in grams

68
Q

The universal gas law is also called the

A

Ideal gas law

69
Q

Pressure is purely the result of

A

Molecular collisions with the walls of a container

70
Q

What is solubility?

A

The maximum amount of one substance (solute) that is able to dissolve into another (solvent)

71
Q

What factors affect the solubility of solutes in solvents?

A

The intermolecular interactions between the substances, temperature & pressure

72
Q

Gas solubility in liquids is inversely

A

Related to temperature; As temperature increases, less gas is able to dissolve into a liquid

73
Q

Greater kinetic energy allows

A

Dissolved gas molecules to escape & prevents further dissolving

74
Q

Gas solubility in a liquid is directly proportional to

A

Pressure (Henry’s Law)

75
Q

What is Henry’s Law?

A

At a constant temperature, the amount of gas dissolved in a liquid is directly proportional to the partial pressure of that gas at equilibrium above the gas-liquid interface

76
Q

Increasing the partial pressure of a gas above a liquid will

A

Increase the amount of gas that dissolves in the liquid

77
Q

What is Osmosis

A

The movement of water across a semipermeable membrane to equilibrate a concentration gradient

78
Q

What is osmotic pressure?

A

The force needed to stop osmosis from occurring; exerted by plasma proteins & electrolytes in capillaries

79
Q

What is Fick’s Law?

A

Diffusion of a gas across a semipermeable membrane is directly proportional to the partial pressure gradient, the membrane solubility of the gas, & the membrane area & is inversely related to the membrane thickness & molecular weight of the gas

80
Q

Atmospheric gases are

A

Less concentrated at altitude & more concentrated at sea level

81
Q

Atmospheric pressure is the

A

Gravitational force on gases in a given area

82
Q

What is heat loss in decreasing order?

A

Radiation
Convection
Conduction
Evaporation

83
Q

Which is the most significant mechanism of heat loss?

A

Radiation (from areas that receive the highest amount of blood flow)

84
Q

What is convection?

A

Heat creates air currents (body transfer kinetic energy to air molecules on the surface of the skin-think currents)

85
Q

What is conduction?

A

Transfer of heat via contact

86
Q

What is evaporation?

A

Moisture evaporation from the patient’s skin as well as exhaled water vapor

87
Q

What is vaporization

A

process of converting liquids or solids into vapors & requires energy

88
Q

What happens when gas particles encounter container wall

A

Momentum is transferred to the wall

89
Q

Solids are

A

Lattus

90
Q

Force is

A

Change in momentum per unit time

91
Q

Matter is composed of

A

Atoms & molecules that are in constant/chaotic movement

92
Q

Volume is proportional to

A

The number of moles

93
Q

As temperature of a substance increases, atoms & molecules

A

Vibrate with greater strength

94
Q

When volume decreases, pressure

A

Increases

95
Q

In Boyles Law is

A

Volume & pressure are inversely related; When volume decreases, pressure increases

96
Q

What is Charles Law

A

Volume is directly proportional to Temperature

As temp increases, volume increases

97
Q

What is Gay-Lussac’s Law?

A

Pressure directly related to temperature

98
Q

What is Avogadro’s Law?

A

At equal temperature & pressure, equal volumes of gas contain an equal number of particles

Volume of gas is directly proportional to the number of gas molecules

99
Q

A mole of any gas weighs

A

6.023 x 10 to the 23rd power

100
Q

A mole of gas is equal to the

A

Molecular weight of the gas in grams

101
Q

What is the memory device for gas laws?

A

P B V C T G

102
Q

What is the constant in the ideal gas law?

A

8.314 Joules/Mole Kelvin

103
Q

What is Dalton’s Law of partial pressure?

A

The partial pressure of a gas in a mixture is the pressure of a gas will exerts by itself under identical conditions of temperature & volume

total pressure of a gas is the sum of all the partial pressures of each of the component gases

104
Q

What happens when your elevation increases?

A

The number of moles & partial pressure will decrease, while the percentage stays the same

105
Q

What does Henry’s Law describe?

A

How the total of gas molecules dissolved in a liquid carries directly with the partial pressure of a gas overlying a liquid

106
Q

As the temperature increases, what happens to the liquid & gas?

A

The liquid rejects the gas molecules, making them less soluble

107
Q

What is Oswald coefficient?

A

Ratio used

Gas dissolved in a solvent (blood: tissue)

108
Q

When a volatile liquid has low solubility,

A

It will equilibrate faster
rapid on/off

109
Q

What is relative humidity?

A

Measure of saturation of water in the air

As temperature increases, air can hold more water

110
Q

What is dew point?

A

Point at which the partial pressure of water & the solubility of the air are equal

Air can no longer hold anymore water & its current temperature & dew qill form

111
Q

Partial pressure of water is equivalent to

A

The concentration of water & vapor pressure is equivalent to solubility of water of the air

112
Q

Oxygen in the lungs

A

Is decreased due to the humidity provided as we breath in air

113
Q

When gas is compressed, pressure will

A

Increase & volume is decreased

Causes temperature to rise= Adiabatic changes

114
Q

With Adiabatic change, no energy is exchanged, only

A

Redistributed

Unequal heating causes weather

115
Q

What is the Joule Thompson effect?

A

Gas compressed at high pressure & is suddenly released causing molecules to push away, decreasing temperature

116
Q

Energy concentration effect

A

Think of a diesel engine

117
Q

Pressure is the result of

A

Molecular collisions with the walls of the container

118
Q

All molecules are moving but

A

Not at the same speed

119
Q

The fraction of molecules is a function of

A

The mass, speed & temperature

120
Q

Boltzmann constant provides

A

A measurement of the amount of energy corresponding to the random thermal motion of particles

121
Q

Different gases will have the same

A

KE if temperature is the same

122
Q

KE is directly proportional to the

A

Mass of an object & square of its velocity

123
Q

Fick’s law of diffusion

A

Rate of diffusion across an area is greater where the concentration changes most rapidly

Diffusion is directly proportional to the concentration gradient

124
Q

Diffusion is a passive process driven by

A

Entropy

125
Q

What is directly proportional to diffusion

A

Concentration gradient

Tissue area

Fluid tissue solubility

126
Q

What is indirectly proportional to diffusion

A

membrane thickness

Molecular weight

127
Q

What is effusion

A

The movement of gas particles from one compartment to another through a small opening or porous membrane

Proportional to the square root of the molecular weight

Depends on the speed of molecules

larger molecule=slower speed

128
Q

What is the Van Der Walls Equation

A

Corrects for the intermolecular attractions between the molecules & for the volume of the gas molecules

Chem/Phys EXAM 2 (3 decks)

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