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Bioscience > Gas Laws/State Of Matter CH 6 & 7 > Flashcards

Gas Laws/State Of Matter CH 6 & 7 Flashcards

1
Q

What are the laws that make up the Empirical gas laws

A

Boyle’s law, Charle’s Law, and Avogadro’s Law

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2
Q

What does Boyle’s Law state

A

When temperature is constant, Volume is inversely proportional to pressure

As pressure goes up, volume goes down
As pressure goes down, volume goes up

P1V1=P2V2

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3
Q

What does Charle’s Law state

A

When pressure and amount of gas are constant, volume is directly proportional to temperature

As temp goes up, volume goes up
As temp goes down, volume goes down

V1/T1 = V2/T2

*note: Not really true. Gas in a contained cylinder will have an increase in pressure as the temp goes up and VOLUME remains constant.

*Gay Lussc’s Law is a variation of Charles law which addresses this discrepancy (P1/T1=P2/T2)

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4
Q

What does Avogadro’s Law state

A

When temperature is constant, the volume of gas is directly proportional to the number of moles of gas

Volume goes up, #moles goes up
Volume goes down, #moles goes down

V1/n1=V2/n2

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5
Q

What does Gay-Lussac’s Law state

A

It is a variation of Charle’s law and states that when volume is constant, the pressure of a gas is directly proportional to the absolute temperature

Temp goes up, pressure goes up
Temp goes down, pressure goes down

P1/T1 = P2/T2

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6
Q

What is the combined gas laws?

A

It combines Boyles, Charles, and Avogadro’s Law

P1V1/n1T1 = P2V2/n2T2

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7
Q

What is the Ideal Gas Law

A

It describes the behavior of an ideal gas under all conditions, but it does not account for real gases that we deal with in real life.

PV=nRT

R is constant
n = # moles
P = pressure
V = volume
T = temp in kelvin

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8
Q

What is the universal gas constant?

A

R is the universal gas constant
R = PV/nT

R = 0.08206 Latm/molK

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9
Q

What does R equal

A

R = 0.08206 Latm/molK

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10
Q

What is STP

A

The Standard Temperature and Pressure

It is a commonly cited set of conditions that helps determine R when conditions are specified

STP is defined to be exactly zero degrees C or 273.15K with a standard pressure 1 Bar

1Bar = 100kPa = 1atm = 760 torr = 101325 Pa or 101.325 kPa

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11
Q

What is the standard molar volume of a gas

A

The volume that exactly 1 mole of ideal gas occupies under STP conditions

1 mol = 22.71 L

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12
Q

What do we need to know in order to calculate gas density

A

mass and volume
Density = m/V

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13
Q

How do we calculate density if we have known temperature and pressure

A

use the ideal gas law (n=PV/RT) to get moles of each component

then obtain the molecular mass of each component

Multiply n by the molecular mass of each component to get the fraction of mass

Substitute those fractions into the Density = m/v

Volume should be given and remember gas is non-reactive and their volumes are additive (so if N2=0.79L and O2=0.21L the the V=0.79+0.21=1.0L)

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14
Q

What does Dalton’s law state

A

the total pressure of a gas mixture is equal to the sum of partial pressures of each component of gas

Ptotal = P1 + P2…..+Pn

To calculate partial pressure,
Pi = Xi * Ptotal

where Xi is the mole fraction in a mixture

And Ptotal = nRT/V

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15
Q

What is relative humidity

A

the measure of the saturation of water in the air

One way to calculate relative humidity is to divide the amount of water in the air by the solubility of water in the air

Relative humidity is a function of temperature
as temp goes up solubility of water in air goes up

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16
Q

What is the solubility of water in the air

A

It is the maximum amount of water that a given volume of air can accommodate

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17
Q

How much N2 and O2 are in the air?

A

79%N2 and 21% O2

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18
Q

We usually measure water vapor pressure in air as

A

47mmHg

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19
Q

What is the dew point temperature

A

it is the condensation formed when a sample is cooled to a temperature where the actual concentration of water exceeds the solubility of water in air

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20
Q

How can we calculate of relative humidity using vapor pressure and partial pressures

A

RH = partial pressure of water/vapor pressure of water all times 100%

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21
Q

what is the Kinetic Molecular Theory of Gases

A

It describes ideal gases based on 4 tenents

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22
Q

what are the 4 tenants of the kinetic molecular theory of gases

A

1) Gases consist of small particles while volume is negligible compare to the volume of gas
- not really true: real gas at high pressures crows more gas molecules into same volume

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 Collins are elastic
- not really true: real gases do have an attractive force as seen in liquid state & low temperatures

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23
Q

The average KE is dependent on what

A

Temperature

KE = 3/2kT

k= Boltzmann’s constant

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24
Q

Boltzmann’s constant (k) equals

A

1.38 x10^-23 J/K

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25
Q

1 mi = meters (m)?

A

1,609m

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26
Q

1hr = sec?

A

3600s

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27
Q

What is the difference between Diffusion and Effusion

A

Diffusion is the movement of a substance from an area of high to low concentration

Effusion is the movement of gas through a small opening

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28
Q

What does Graham’s Law state

A

The rate of effusion is inversely proportional to the square root of the molecular mass (M)

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29
Q

What does the Vander de Waals Equation do

A

It corrects for the intermolecular attractions between gaseous molecules and for the finite volume of the gas molecules

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30
Q

What does The Molecular Theory of Matter describe

A

it describes all states of matter and the conversion between the states by considering the structures of molecules comprising matter and how those molecules interact

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31
Q

What are the 3 commonly encountered states and what characterizes them?

A

Solid: characterized by shape and volume

Liquid: characterized by a definite volume, but NOT shape. It conforms to the shape of the canister.

Gas: Have neither Definite shape or volume. Gas will expand to fill available space.

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32
Q

Do gases have intermolecular forces?

A

No

the move freely and collide freely

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33
Q

Which states are compressible

A

Liquids and Solids

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34
Q

Which states are considered fluids

A

Gases and Liquids

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35
Q

Melting is

A

the conversion of a solid into a liquid

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36
Q

Freezing is

A

the conversion of a liquid into a solid

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37
Q

Vaporization is

A

when a liquid vaporizes into a gas

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38
Q

Condensation is

A

when a gas condenses into a liquid

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39
Q

Deposition is

A

when a gas converts into a solid

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40
Q

Sublimation is

A

when a solid converts into a gas without having to become a liquid first

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41
Q

What are intermolecular forces

A

Forces the determine how molecules interact with one another. They arise because of the attraction of opposite charges and produce an inherent repulsion.

Determined by chemical bonds that hold atoms together

They are electrostatic in nature

4 types of IMF: dipole-dipole, hydrogen bonding, London forces, and ion-dipole interactions

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42
Q

What are Dipole-Dipole interactions

A

Dipole attractions between the opposite (partial) charges of POLAR molecules

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43
Q

What are Hydrogen Bonding interactions

A

Special type of dipolar interaction only possible when a hydrogen atom is directly bonded to F, O or N.

Stronger than Dipole-Dipole interactions

It is the most important intermolecular force

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44
Q

What are London forces

A

It is the result of an instantaneous dipole that is created whenever electrons in a molecule are unevenly distributed.

All molecules and atoms that have electrons, exhibit London forces.

Larger molecules show more London forces because larger molecule have more electrons

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45
Q

What are Ion-Dipole attractions

A

Attraction between an ION and POLAR molecule

This attractions allows ionic solids to dissolve in water

46
Q

What are valence electrons

A

electrons in partially filled shells.

electrons in the highest energy or valence (shell).

8 total valence electrons for a stable element

47
Q

Noble gases

A

have 8 valence electrons in outer shell. Most stable

48
Q

What are isoelectric species

A

elements that are only one or two atomic numbers away from a noble gas form

49
Q

What are core (kernel) electrons

A

electrons in filled shells.

virtually inert because they represent complete collections of electrons, very energetically expensive to break up a complete set

50
Q

Which bonds are stronger, covalent or ionic

A

Ionic and for this reason every ionic compound is solid at room temperature and pressure.

51
Q

What is the valence bond theory

A

theory that explains how covalent bond form through the sharing of valence electrons and the electron structure of those molecules

52
Q

What amount of energy makes you stable

A

less energy

53
Q

What are isomers

A

compounds that different but have the same molecular formula

54
Q

What is the VSEPR theory

A

Valence Shell Electron Pair Repulsion explains that atoms are bound into molecules by shared pairs of electrons.

Electrons dislike each other because like charges repel each other

Whether they are lone pairs of electrons or bonding pairs of electrons, the pairs try to get as far apart in space as geometrically possible

55
Q

What angle does a linear molecule form

A

Angle between bonds is 180 degrees

56
Q

What angle does trigonal planar molecule form

A

Angle between bonds is 120 degrees

57
Q

What angle does a tetrahedral molecule form

A

Angle between bonds is just over 109 degrees

58
Q

What angle does a bent molecule form

A

Angle varies, but mainly know it is non linear

59
Q

What angle does a pyramidal molecule form

A

It is like trigonal (120 degrees) the only difference is it has a point the forms that “pyramid” shape

60
Q

What element is the most electronegative

A

Fluorine

61
Q

Describe a non polar bond

A

two atoms of IDENTICAL electronegativity bonded together

62
Q

Describe a polar bond

A

two atoms of DIFFERENT electronegativity bonded together

63
Q

What are some non polar elements we will work with

A

Nitrogen, Oxygen, Carbon Dioxide

64
Q

Substances that have greater intermolecular attractions will have what kinds of surface tension

A

Greater surface tensions

65
Q

What is surface tension

A

the force acting on the surface of a liquid cause by the attraction of molecules in the surface later; makes liquid surface act as it were elastic-like

66
Q

What is the IM force of water

A

hydrogen bonding

67
Q

Does water have high or low surface tension

A

High

68
Q

What is capillary rise (capillary action)

A

it is a second effect caused by surface tension. It is the tendency of fluid ratio to rise into a narrow-diameter tube.

the rise will depend of the diameter of the narrowest tube.

69
Q

What is Laplace’s Theory

A

Theory used to calculate the distance a fluid will rise in a capillary.

When a liquid is in contact with another surface, it has a curling the creates a pressure difference, this theory has formulas to calculate that

70
Q

What is the surface tension of water

A

0.072 N/m

71
Q

The radius (R) in the Laplace formula represents

A

(R) is a function of the contact angle and the radius of the tube, r. Since r and R form two side of a right triangle, R is give by

R = radius (r)/ cosign of angle

72
Q

What do we use to calculate upward pressure of a liquid

A

Laplace forumla

73
Q

What do we use to calculate downward pressure of a liquid

A

P=pgh

p=density
g=gravity
h=height

74
Q

Surface tension is proportional to

A

the radius

75
Q

What is a physical advantage of having an aneurysm?

A

Lowers surface tension on a blood vessel

76
Q

What is a surfactant

A

A soap or detergent used to reduce the surface tension of a solvent

77
Q

Surfactant molecules will strike to get the greasy non polar hydrocarbon tails away from the polar water molecules via 3 strategies, what are they

A

Formation of:

monolayers
bilayers
micelles

78
Q

Soaps are derived from

A

fats or oils (triglycerides) through chemical process called saponification

79
Q

Detergents are synthesized from

A

soaps

The molecular structure of detergents can be tweaked to optimize the physical properties of the detergent

Detergents can be cationic, anionic, or nonionic

80
Q

What is the structural feature of soaps and detergents

A

both have a polar (hydrophilic) HEAD and a non polar (hydrophobic, greasy) TAIL

81
Q

Describe monolayer surfactants

A

In forming a monolayer, surfactant molecules stick their polar heads onto the water, while their greasy tails stick out of the surface of the water

increasing surfactant will decrease surface tension of water

82
Q

What is an example of how we use monolayer surfactants to reduce surface tension

A

We give premature babies monolayer surfactants to decrease the surface tension of the lungs

By adding this type of detergent, the water in the lungs becomes less cohesive and the surfaces in the lungs are less likely to stick together

83
Q

Describe bilayer surfactants

A

The tail of the surfactant molecules can dissolve in each other to form a double layer (bilayer)

84
Q

What is an example of a bilayer surfactant we use

A

For bactericidal properties

85
Q

Describe micelles surfactants

A

the greasy tails can dissolve in each other forming a spherical structure

86
Q

What happens with increased viscosity

A

it increases with increasing molecular forces

it increases the resistance to flow

87
Q

What is viscosity

A

a measure of a fluid’s resistance to flow

88
Q

What is the relationship of vapor pressure and temperature

A

directly proportional as temperature rises, vapor pressure will rise and so will the volatility of a liquid

89
Q

What is the relationship of vapor pressure and IM forces

A

Substances that have greater IM forces will have lower vapor pressure

90
Q

What is volatility

A

it is an non-quantitative term used to describe the tendency of a liquid to evaporate

91
Q

What is the Clausis-Clapeyron Equation

A

Formula that relates the vapor pressure of a liquid (P) to the kelvin temperature (T)

where A & B depend on the liquid

To free log (P) use the antilog (P)

92
Q

What does the vapor pressure of a volatile liquid determine

A

the maximum mole fraction of that substance in a gas phase in contact with that volatile liquid

93
Q

With a gas, the mole fraction equals

A

mole fraction = volume fraction = pressure fraction

94
Q

What is the relationship between boiling point and IM forces

A

with increasing IM forces, the boiling point will increase

95
Q

what is boiling point

A

boiling point of a liquid substance is the temperature at which the vapor pressure of a liquid is equal to 1 atm pressure

96
Q

What does boiling point correspond to

A

The average KE sufficient enough o overcome the IM forces that hold a molecule in the liquid state

97
Q

What is the relationship between boiling point and pressure

A

because gases respond strongly to pressure, the boiling point of a liquid is highly dependent on pressure

As the boiling point increases, the pressure will increase

98
Q

What is the normal boiling point of water

A

100 degrees C or 373K at 101kPa

99
Q

Calusius-Clapeyron Equation can be used to quantify the relationship between boiling point and temperature, what is the formula for that

A
100
Q

What is the relationship between melting point and IM forces

A

as IM forces increase the melting temperature increases too

101
Q

What is melting point

A

temperature at which the solid state reversibly passes into the liquid state, also known as the freezing point

102
Q

The melting point corresponds to

A

the average KE sufficient to overcome the IM forces that hold the molecules in the solid state

103
Q

What is molar enthalpy of fusion (Hfus)

A

the heat necessary to convert 1 mole of a SOLID into a LIQUID at its normal MELTING point

104
Q

What is molar enthalpy of vaporization (Hvap)

A

the heat required to convert 1 mole of a LIQUID into a GAS at its normal BOILING point

105
Q

What is the relationship between Hfus and Hvap

A

they both are endothermic and represent a amount of energy that must be added to a sample in oder for the phase transition to occur

Hvap > Hfus and this is true fore all substances

106
Q

Heat of fusion represents

A

the amount of energy necessary to overcome the IM forces to the point that the molecules can start to move around each other

107
Q

Heat of vaporization represents

A

the amount of energy necessary to overcome all the IM forces that the molecule can escape into the gas phase

108
Q

Triple point on the phase diagram represents

A

the single temperature and pressure combination where all three phases can exist in equilibrium with each other

109
Q

the solid-liquid equilibrium line defines

A

the melting point of the solid into the liquid state

110
Q

the liquid-gas equilibrium line defines

A

the boiling point of the liquid at various pressures. it terminates at a point known as the critical piont

111
Q

The solid-gas equilibrium line defines

A

sublimation of solid into gas state without become a liquid first

112
Q

supercritical fluids

A

have the flow properties of gases but densities similar to liquids and have no surface tension. make for terrific solvents

Ex; carbon dioxide, excellent solvent for extracting caffeine from coffee

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