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PHYS-575/CSI-655 Introduction to Atmospheric Physics and Chemistry Lecture Notes #3 – Part 1: Thermodynamics. Thermodynamics Review/Tutorial - Ideal Gas Law - Heat Capacity - 1 st & 2 nd Laws of Thermodynamics - Adiabatic Processes - Energy Transport - PowerPoint PPT Presentation
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04/20/2304/20/23 11
PHYS-575/CSI-655PHYS-575/CSI-655Introduction to Atmospheric Physics and ChemistryIntroduction to Atmospheric Physics and Chemistry
Lecture Notes #3 – Part 1: Lecture Notes #3 – Part 1: ThermodynamicsThermodynamics
1. Thermodynamics Review/Tutorial - Ideal Gas Law - Heat Capacity - 1st & 2nd Laws of Thermodynamics - Adiabatic Processes - Energy Transport2. Hydrostatic Equilibrium3. Adiabatic Lapse Rate – DRY4. Adiabatic Lapse Rate - WET5. Static Stability6. SLT and the Atmosphere
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What is Thermodynamics?What is Thermodynamics?
"Now, in the second law of thermodynamics...""Department of Entropy"
Thermodynamics is the study of heat and its transformation from a macroscopic point of view.
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1. Thermodynamics Tutorial1. Thermodynamics TutorialThermodynamics is the study of heat and its transformation to andfrom other sources of energy, from a macroscopic point of view.
Statistical Mechanics connects thermodynamics to the microscopic world through the statistical description of an ensemble of atoms ormolecules that constitute a macroscopic system.
The transfer of heat, in turn, is driven by differences in temperatureor potential differences associated with chemical reactions.
In the interest of crafting a brief tutorial for applications to the atmosphere, I haveglossed over some of the finer (but yet important) points of thermodynamics.
For more complete treatment:General: Fundamentals of Statistical and Thermal Physics (McGraw-Hill Series in Fundamentals of Physics) by Frederick Reif, 1965.Atmospheric: Atmospheric Thermodynamics, by C.F. Bohren and B.A. Albrecht, Oxford University Press, Oxford, 1998.
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Defining TemperatureDefining Temperature
Temperature is a measure of the mean kinetic energy of gas molecules.
The temperature of an ideal monatomic gas is related to the average kinetic energy of its atoms as they move. In this animation, the size of helium atoms relative to their spacing is shown to scale under 1950 atmospheres of pressure. These room-temperature atoms have a certain, average speed (slowed down here two trillion fold).
kTmv2
3
2
1 2
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Measure of TemperatureMeasure of Temperature
dvevdvvf cv 2)/(2)(
kTdvvfvm
vmmv2
3
22
1
2
1
0
222
Temperature of a measure of the mean kinetic energy of gas molecules.
m
kTc 2
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Temperature ScalesTemperature Scales
The The FahrenheitFahrenheit Scale: Scale: • we are most familiar with this one we are most familiar with this one • water freezes at 32 degrees F. water freezes at 32 degrees F. • water boils at 212 degrees F. water boils at 212 degrees F. • when we cool to the absolute lowest when we cool to the absolute lowest
temperature we reach -459 degrees temperature we reach -459 degrees (this is referred to as Absolute Zero) (this is referred to as Absolute Zero)
The The CelsiusCelsius Scale: Scale: • water freezes at 0 degrees C. water freezes at 0 degrees C. • water boils at 100 degrees C. water boils at 100 degrees C. • Absolute Zero is at -273 degrees C. Absolute Zero is at -273 degrees C.
The The Kelvin Kelvin ScaleScale • Absolute Zero is 0 K Absolute Zero is 0 K • a temperature change of 1 degree K is a temperature change of 1 degree K is
the same as a temperature change of 1 the same as a temperature change of 1 degree C. degree C.
• water freezes (or melts) at 273 K water freezes (or melts) at 273 K • water boils at 373 K water boils at 373 K
The Kelvin is scale is the more useful scale The Kelvin is scale is the more useful scale for our course since it refers to Absolute for our course since it refers to Absolute Zero in a direct way. Zero in a direct way.
Temperature is a measure of the random kinetic energy of atoms and/or molecules
<1/2 mv2> = 3/2 k T
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The Ideal Gas LawThe Ideal Gas LawLaboratory experiments show that the pressure, volume, and temperature ofany material may be related by an Equation of State (EOS). These variablesare known as State Variables. All atmospheric gasses follow an equation of state known as the Ideal Gas Law (IGL) to a very high degree of accuracy. We assume the IGL to be exact in atmospheric science.
The Ideal Gas Law may be written: pV = mRT where
p = pressureV = volumem = mass T = temperature (absolute Kelvin; K = oC + 273.15)R = gas constant
The gas constant R depends upon the particular gas under consideration.Since m/V = ρ (density of the gas), the IGL may be written:
p = ρRT
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We can also define α = 1/ρ, known as the specific volume,to write the IGL as:
pα = RTBoyle’s Law: For fixed temperature, the pressure of a gas is inverselyproportional to its volume, i.e., P ~ 1/V.
Additional forms of the Ideal Gas Law:
A mole (gram-molecular weight) of any substance is the molecular weight M of the substance expressed in grams. For example, the molecular weight of water is 18.015 gm, so 1 mole of water is 18.015 gm of water. The number of moles (N) in a mass m (in grams) of a substance is given by:
N = m/M
The number of molecules in 1 mole of any substance is a universalconstant called Avogadro’s number, NA.
NA = 6.022 x 1023 molecules per mole.
Ideal Gas Law (IGL) - continued
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The Ideal Gas Law for 1 mole of any gas can be written:
pV = R*T
Where R* is the universal gas constant = 8.3145 J K-1 mol-1.So for N moles of any gas, the IGL will be:
pV = NR*T
The gas constant for 1 molecule of any gas is also a universal constantknown as Boltzmann’s constant, k = 1.38 x 10-23 J K-1 molecule-1
So for a gas with n gas molecules per unit volume V, the IGL is then
p = nkT
Ideal Gas Law (IGL) – continued again
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Ideal Gas Law - SummaryIdeal Gas Law - Summary
Ideal Gas Law: P = nkT = ρRT= RT/α
PV = R*T/MP = pressurem = mass per gas particlen = number density of gas particles ρ = mn = mass densityα = 1/ρ = specific volumeV = volume of one mole of gask = Boltzmann’s constantR = gas constant (gas specific) = R*/ΜM = molar massR* = universal gas constantT = temperature
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Heat CapacityHeat Capacity
dT
dQC
The Heat Capacity of a material is a measure of its ability to absorb and retain heat.
More precisely, the Heat Capacity is the energy (dQ) required to increase the temperature of a unit volume of any substance from T to T+dT (in Kelvin)
The Heat Capacity depends upon the nature of the material and its temperature.
The Heat Capacity also depends upon exactly how the energy is added. If theheat is added to a gas at constant volume the heat capacity is lower than if theheat is added at constant pressure. The reason is that heat performs work if the volume changes.
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Heat Capacity - continuedHeat Capacity - continued
Heat capacity is related to the ability of a substance to store energy. Energy can be stored in a variety of ways. For a gas, the most obviousway to store energy is in random kinetic energy of the gas molecules.
kTmv2
3
2
1 2
The 1/2mv2 is the kinetic energy of a molecule of mass m moving with avelocity v. There is ½ kT of energy “per degree of freedom” of the molecule.For a molecule moving in 3-dimensions, there are 3 degrees of freedomand thus the average kinetic energy is stored as 3/2kT.
If there are other ways for a molecule to store energy, then the heat capacitywill be higher.
Thus the Heat Capacity depends upon the phase of the substance.
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Heat Capacity of WaterHeat Capacity of Water
http://www.ac.wwu.edu/~vawter/PhysicsNet/Topics/Thermal/gifs/HeatCapacity02.gif
The Heat Capacity of water makesan excellent example.
When frozen, water molecules do nothave translational kinetic energy andthus its heat capacity is low. Moleculescan only vibrate.
Thawing requires heat and thus isa portion of its heat capacity.
Upon thawing, water molecules canhave kinetic energy of translation andthe heat capacity increases with temperature.
Evaporation requires heat and thus increases the heat capacity.
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Heat Capacity - continuedHeat Capacity - continued
As can be seen with water, the Heat Capacity is a function of only temperature.
Thus we define the Internal Energy, U, of a unit volume of material to be the measure of the amount of thermal energy stored in the material. The Internal Energy thus depends only upon temperature.
For a gas, the distribution of speeds is a strong function of temperature.
So the internal energy increases as the temperature increase.
U = ρCvT
If you add heat (dq) to a gas, you can cause the internal energy (U) toincrease and/or cause the gas to expand and do work on its environment.
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Specific HeatsSpecific Heats
dT
dq
constvv dT
dqC
Suppose a small quantity of heat dq is added to a unit mass of material andthis causes the material to rise in temperature from T to T+dT.
Then is the specific heat of the material.
If the volume of the material is kept constant, then the specific heatat constant volume Cv is defined as:
However, if the volume of the material is kept constant, then dq = du(heat changes internal energy and does no work on the environment)and:
constvv dT
duC
For an ideal gas u depends only upon temperature (T), so Cv depends only upon T.
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We can also define a specific heat at constant pressure Cp as:
constpp dT
dqc
But when heat is added to a parcel of gas at constant pressure, some energy can be used in expanding the gas.
So more heat must be added to a given mass of material at constant pressure to raise it to a given temperature than if the material was kept at constant volume.
Specific Heats - continued
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The 3 Laws of ThermodynamicsThe 3 Laws of Thermodynamics
First Law:First Law: You can You can’’t win.t win. Second Law:Second Law: You can You can’’t break even.t break even. Third Law:Third Law: You can You can’’t get out of the game.t get out of the game.
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The Three Laws of ThermodynamicsThe Three Laws of Thermodynamics
1) Conservation of Energy: Energy is neither created nor destroyed, it is merely converted from one form to another.
2) The Entropy of an isolated system increases when a system undergoes a spontaneous change.
3) The Entropy of all substances approaches zero as the temperature (in Kelvin) approaches zero. All substances have zero energy at absolute zero.
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The First Law of Thermodynamics Conservation of Energy: Energy is neither created
nor destroyed, it is only changed from one form to another.
What is Energy?Forms of Energy:-- Gravitational Potential-- Kinetic Energy-- Chemical Energy-- Electromagnetic Energy-- Rest mass energy
For any system (e.g. a specific collection of matter), the changein energy of the system is equal to the energy transferred by workplus the energy transferred by heat.
Heat is the transfer of energy to or from a system associated with a temperature difference.Work is the transfer of energy to a system by the application of a force.
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The first law of thermodynamics is the The first law of thermodynamics is the application of the application of the conservation of energyconservation of energy principle to thermodynamic processes:principle to thermodynamic processes:
http://hyperphysics.phy-astr.gsu.edu/hbase/thermo/firlaw.html
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The First Law and WorkThe First Law and Work
http://www.grc.nasa.gov/WWW/K-12/airplane/thermo1.html
04/20/2304/20/23 2222http://www.fas.org/irp/imint/docs/rst/Sect14/stability2.jpg
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Useful Forms of the Useful Forms of the First Law of ThermodynamicsFirst Law of Thermodynamics
PdVdTCdU
PdVdQdU
dWdQdU
p
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Second Law of ThermodynamicsSecond Law of Thermodynamics
Entropy is the heat added (or subtracted), ΔQ, to a system divided by its temperature in Kelvin (T). It is a measure of the disorderof a system; a measure of the unavailability of a system’s energy todo work; a measure of the disorder of the molecules in a system;a measure of the number of possible states of a system.
The Entropy of an isolated system increases when the system undergoes a spontaneous change.
dQ is the heat absorbed in an isothermal and reversible process.
T
QS
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Implications of the Second LawImplications of the Second Law
It is impossible for any process (e.g., engine), working in It is impossible for any process (e.g., engine), working in a cycle, to completely convert surrounding heat to work.a cycle, to completely convert surrounding heat to work.
Dissipation will always occur.Dissipation will always occur. Entropy will always increase.Entropy will always increase.
The Second Law of Thermodynamics states that it is impossible to completely convert heat energy into mechanical energy. Another way to put that is to say that the level of entropy (or tendency toward randomness) in a closed system is always either constant or increasing.
The Second Law of Thermodynamics
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Work and Heat DissipationWork and Heat Dissipation
No matter how efficient the system (engine) is, dissipation will always occur.This usually appears as heat released from the system to its surroundings
04/20/2304/20/23 2727
Work and HeatWork and Heat
http://physics.uoregon.edu/~courses/dlivelyb/ph161/heat_engine_schem.gif
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Work and EfficiencyWork and Efficiency
The Second Law of Thermodynamics states that it is impossible for any heat engine to be 100 % efficient: No process is possible which results in the extraction of an amount of heat from a reservoir and its conversion to an equal amount of mechanical work.
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Efficiency of AutomobilesEfficiency of Automobiles
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The Second Law and Heat Dissipation The Second Law and Heat Dissipation for a Automobilefor a Automobile
04/20/2304/20/23 3131
The Atmosphere as an Engine with The Atmosphere as an Engine with Associated DissipationAssociated Dissipation
04/20/2304/20/23 3232
Atmospheric Circulation acts an Engine transferring Atmospheric Circulation acts an Engine transferring
heat from a hot region to a cold regionheat from a hot region to a cold region..
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Energy Flow in the Biosphere as an Engine with Energy Flow in the Biosphere as an Engine with DissipationDissipation
Visible light contains most energy from the sun (per wavelength interval) and overlaps the region where the atmosphere is most transparent, and also is the region where most photosynthesis occurs in the biosphere.
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Usable EnergyUsable Energy
http://trc.ucdavis.edu/biosci10v/bis10v/week2/2webimages/figure-06-03b.jpg
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The Third Law of ThermodynamicsThe Third Law of Thermodynamics
The Entropy of all substances approaches zero as the temperature (in Kelvin) approaches zero. All substances have zero energy at absolute zero.
04/20/2304/20/23 3636
The Use of The Use of Thermodynamic Thermodynamic
DiagramsDiagrams
A pair of variables:(P, V) or (P,T) or (V,T) or…denote a state of the system.
A P-V diagram shows the possible states that the system can have.
dW = PdV = Force x Displacement
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Parcel ConceptsParcel ConceptsBelow approximately 100 km altitude, Below approximately 100 km altitude, air is relatively well mixed. air is relatively well mixed.
Virtually all mixing is accomplished Virtually all mixing is accomplished by the exchange of air by the exchange of air ““parcelsparcels”” which which have horizontal dimensions ranging have horizontal dimensions ranging from mm to the scale of the Earth.from mm to the scale of the Earth.
An air An air ““parcelparcel”” of infinitesimal of infinitesimal dimensions is assumed to be:dimensions is assumed to be:
(1)(1) Thermally insulated from the Thermally insulated from the environment (no energy exchange)environment (no energy exchange)
(2)(2) Moving slowly so that kinetic energy Moving slowly so that kinetic energy of motion is much smaller than itof motion is much smaller than it’’s s total energy.total energy.
In reality, both of these assumptions are violated to some extent. But for small displacements over small time intervals they can be excellent approximations.
04/20/2304/20/23 3838
Thermodynamic Descriptions of the AtmosphereThermodynamic Descriptions of the Atmosphere
During any atmospheric process, the state of a parcel of atmospheric gas (P, V, T, S, etc) will change. The Laws of Thermodynamics determine exactly how these changes can occur. Phase Diagrams describe these changes in the state variables describing the gas.
04/20/2304/20/23 3939
Thermodynamic Descriptions of the AtmosphereThermodynamic Descriptions of the Atmosphere
During any atmospheric process, the state of a parcel of atmospheric gas (P, V, T, S, etc) will change.
Any pair of variables can be used to describe the state of the system: (P,V) or (T, S) or (P, S), etc.
04/20/2304/20/23 4040
Example: Adiabatic Process - No Energy In/OutExample: Adiabatic Process - No Energy In/Out
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Parcel Concepts: Applications of the laws of Parcel Concepts: Applications of the laws of thermodynamics to air parcelsthermodynamics to air parcels
First Law of Thermodynamics: dQ = dU + PdV
Internal Energy: dU = CpdT
Second Law of Thermodynamics: dS = dQ/T
Adiabatic means dQ = 0. dQ implies dS = 0.
Thus an adiabatic process is also an isentropic process.
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Energy TransportEnergy Transport
(1) (1) Conduction:Conduction: is the transfer is the transfer of energy by collisions of energy by collisions between particles (generally between particles (generally atoms or molecules). Also atoms or molecules). Also known as diffusive transport known as diffusive transport of energy.of energy.
(2) (2) Convection:Convection: is the motion of is the motion of a fluid caused by density a fluid caused by density gradients which are a result of gradients which are a result of temperature differences.temperature differences.
(3) (3) Radiation:Radiation: is the transport of is the transport of energy by photons.energy by photons.
There are three primary ways that energy is transported in planetary atmospheres.
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Diffusion of Mass and HeatDiffusion of Mass and Heat
Diffusion can be driven by concentration gradients, temperature gradients,and pressure gradients. When diffusion is produced by temperature gradientsthis is known as thermal conduction and leads to the transfer of heat.
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Thermal ConductionThermal Conduction is the transfer of heat by collisions is the transfer of heat by collisions between particlesbetween particles
QQ = heat flux (erg cm = heat flux (erg cm-2-2 s s-1-1))
dT/dzdT/dz = temperature gradient in z direction = temperature gradient in z direction
κκTT = thermal conductivity is a measure of a material= thermal conductivity is a measure of a material ’’s physical ability to s physical ability to conduct heat.conduct heat.
FickFick’’s First Law of Diffusions First Law of Diffusion
The rate of change of energy per unit volume is given by:The rate of change of energy per unit volume is given by:
FickFick’’s Second Law of Diffusions Second Law of Diffusion
dz
dTQ T
dz
dQ
dt
dU
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Thermal ConductionThermal Conduction is the transfer of heat by collisions is the transfer of heat by collisions between particlesbetween particles
UU = internal energy = = internal energy = ρρCCPPTT, where, where
ρρ = mass density = mass density
CCPP = heat capacity at constant = heat capacity at constant
pressure (it can also occur at pressure (it can also occur at constant v)constant v)
TT = temperature = temperature
Where Where κκD D = thermal diffusivity = thermal diffusivity
= = κκTT//ρρCCPP
2
2
z
T
dt
dTC Tp
2
2
z
T
t
TD
Or
04/20/2304/20/23 4646
ConvectionConvectionConvection is the motion of a fluid caused by density gradients which result from temperature differences.
Examples:Boiling waterCloud formation Plate tectonics
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Convection in the AtmosphereConvection in the AtmosphereConvection is the motion of a fluid caused by density gradients which result from temperature differences.
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The Atmospheric General CirculationThe Atmospheric General Circulationis a Manifestation of Convective Currentsis a Manifestation of Convective Currents
04/20/2304/20/23 4949
Quantifying Convective Energy TransportQuantifying Convective Energy Transport
dz
dTQ eFirst Law of Diffusion
The rate of change of energy per unit volume is given by:
Second Law of Diffusion
Ke = Eddy Diffusion Coefficient
The Convective Energy Flux can be quantified analogous to the thermal conduction flux, if the thermal diffusion coefficient is replaced by an Eddy Diffusion Coefficient, Ke.
The key problem in convection and mixing is the choice of Ke. It is usuallydetermined by observations of tracer motions in the atmosphere.
2
2
z
T
t
Te
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Energy Transport by RadiationEnergy Transport by Radiation
kc
c = 2.998 x 108 ms-1 speed of electromagnetic radiationλ = wavelength (wavenumber = k = 1/λ)
ν = frequency, such that: Energy:
h = Planck’s Constant
hE
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Radiation: EmissionRadiation: Emission
Thermal Blackbody Emission
The Sun is a near-blackbody at 5770 K
The Spectrum of Solar Radiation
04/20/2304/20/23 5252
Radiation: Absorption and Emission by MatterRadiation: Absorption and Emission by Matter
Line emission and absorptionLine emission and absorption
Line wavelengths correspond to energy changes in absorbing/emitting atoms.
04/20/2304/20/23 5353
Atomic Structure: Photon Absorption & EmissionAtomic Structure: Photon Absorption & Emission
04/20/2304/20/23 5454
SpectroscopySpectroscopy Each element (and molecule) has a unique spectroscopic signature. Each element (and molecule) has a unique spectroscopic signature. This is due to their unique structure and energy level distributions.This is due to their unique structure and energy level distributions.
04/20/2304/20/23 5555
Atmospheric Absorption by MoleculesAtmospheric Absorption by Molecules
04/20/2304/20/23 5656
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The Greenhouse EffectThe Greenhouse Effect:: A Consequence of A Consequence of Radiation Absorption and Emission by Radiation Absorption and Emission by
Greeenhouse Gases in the AtmosphereGreeenhouse Gases in the Atmosphere
04/20/2304/20/23 5858
The Greenhouse Effect and Global WarmingThe Greenhouse Effect and Global Warming
Sunlight brings energy into the climate system; most of it is absorbed by the oceans and land.
THE GREENHOUSE EFFECT: Heat (infrared energy) radiates outward from the warmed surface of the Earth.
Some of the infrared energy is absorbed by greenhouse gases in the atmosphere, which emits the energy in all directions.
Some of this infrared energy further warms the Earth.
GLOBAL WARMING:Increasing concentrations of CO2 and other "greenhouse" gases trap more infrared energy in the atmosphere than occurs naturally. The additional heat further warms the atmosphere and Earth’s surface.
04/20/2304/20/23 5959
Vertical Structure of the EarthVertical Structure of the Earth’’s Atmosphere: s Atmosphere: Illustration of Heat Transport MechanismsIllustration of Heat Transport Mechanisms
Convection: The steepvertical temperature gradient produces unstable air parcels.
Radiation: Stratosphericozone (O3) absorb solar ultraviolet photons which cause local heating.
Conduction: Solar extreme ultraviolet (EUV) photons absorbed in the upper atmosphere deposit energy which is conducted downwards.
04/20/2304/20/23 6060
Applications of Thermodynamics to Applications of Thermodynamics to Atmospheric ProcessesAtmospheric Processes
What is a Storm?What is a Storm? Parcel ConceptsParcel Concepts Hydrostatic EquilibriumHydrostatic Equilibrium Vertical Temperature ProfileVertical Temperature Profile Adiabatic Lapse RateAdiabatic Lapse Rate Dry vs. Wet AtmosphereDry vs. Wet Atmosphere Static StabilityStatic Stability The Second Law of Thermodynamics and the The Second Law of Thermodynamics and the
AtmosphereAtmosphere
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What is a Storm?What is a Storm?
http://www.noaanews.noaa.gov/stories2005/images/ivan091504-1515zb.jpg
1. Do all storms have the same cause?
2. Do all storms have the same ending?
3. Are there aspects that all storms have in common?
04/20/2304/20/23 6262
Storm Definitions:Storm Definitions: behave violently, as if in state of a great anger behave violently, as if in state of a great anger take by force; "Storm the fort" take by force; "Storm the fort" rain, hail, or snow hard and be very windy, often with rain, hail, or snow hard and be very windy, often with
thunder or lightning; "If it storms, we'll need shelter" thunder or lightning; "If it storms, we'll need shelter" a violent weather condition with winds 64-72 knots (11 a violent weather condition with winds 64-72 knots (11
on the Beaufort scale) and precipitation and thunder and on the Beaufort scale) and precipitation and thunder and lightning lightning
blow hard; "It was storming all night" blow hard; "It was storming all night" a violent commotion or disturbance; "the storms that had a violent commotion or disturbance; "the storms that had
characterized their relationship had died away"; "it was characterized their relationship had died away"; "it was only a tempest in a teapot" only a tempest in a teapot"
attack by storm; attack suddenly attack by storm; attack suddenly a direct and violent assault on a strongholda direct and violent assault on a stronghold
04/20/2304/20/23 6363
What Causes a Storm?What Causes a Storm?
http://systhread.net/pics/storm/jpegs-orig/10.jpg
04/20/2304/20/23 6464
How Long Can a Storm Last?How Long Can a Storm Last?
Jupiter’s Giant Red Spot
04/20/2304/20/23 6565
Baby Red Spots?Baby Red Spots?
04/20/2304/20/23 6666
Review: Parcel ConceptsReview: Parcel ConceptsBelow approximately 100 km altitude, Below approximately 100 km altitude, air is relatively well mixed. air is relatively well mixed.
Virtually all mixing is accomplished Virtually all mixing is accomplished by the exchange of air by the exchange of air ““parcelsparcels”” which which have horizontal dimensions ranging have horizontal dimensions ranging from mm to the scale of the Earth.from mm to the scale of the Earth.
An air An air ““parcelparcel”” of finite dimension is of finite dimension is assumed to be:assumed to be:
(1)(1) Thermally insulated from the Thermally insulated from the environment (no energy exchange)environment (no energy exchange)
(2)(2) Moving slowly so that kinetic energy Moving slowly so that kinetic energy of motion is much smaller than itof motion is much smaller than it’’s s total energy.total energy.
In reality, both of these assumptions are violated to some extent. But for small displacements over small time intervals they can be excellent approximations.
04/20/2304/20/23 6767
Ideal Gas Law - SummaryIdeal Gas Law - Summary
Ideal Gas Law: P = nkT = ρRT=RT/α PV = R*T/M
P = pressurem = mass per gas particlen = number density of gas particles ρ = mn = mass densityα = 1/ρ = specific volumeV = volume of one mole of gask = Boltzmann’s constantR = gas constant (gas specific) = R*/ΜM = molar massR* = universal gas constantT = temperature
How do you describe air Parcels?
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Parcel Concepts: Applications of the laws of Parcel Concepts: Applications of the laws of thermodynamics to air parcelsthermodynamics to air parcels
constvpvp dT
dqC
,,
Internal Energy (kinetic energy):
Internal Energy (general): U = ρCpT
Internal Energy Change: dU = CpdT; Work=PdV
First Law of Thermodynamics: dQ = dU + PdV
Second Law of Thermodynamics: dS = dQ/T
Hydrostatic Equilibrium: dP = -ρgdz
Adiabatic means dQ = 0. dQ implies dS = 0.
Thus an adiabatic process is also an isentropic process.
Specific Heats (Constant P,V)
kTmv2
3
2
1 2
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Hydrostatic EquilibriumHydrostatic Equilibrium
Hydrostatic Balance:ρg dAdz = P(z) dA – P(z+dz) dAP(z+dz) = P(z) + (dP/dz) dz
Thus dP/dz = -ρg
Air pressure at any height in theatmosphere is due to the force per unit area exerted by the weight of all of the air lying above that height.
The air is in hydrostatic balance if thenet upward force on a thin slab of airis equal to the net downward force onthe slab.
Thus the change in pressure between thetop and bottom of the thin slab is equalto the weight (dM g = ρdV g) of the slab per unit area, where dV = dAdz.
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Hydrostatic EquilibriumHydrostatic Equilibrium
gdzdP
gkT
mPg
dz
dP
Hydrostatic Balance: dP = - ρgdz Ideal Gas Law: P = nkT = (ρ/m) kT = ρRT
P = pressurem = mass per gas particlen = number density of gas particlesρ = mn = mass densityk = Boltzmann constantR = gas constantT = temperature dz
kT
mg
P
dP
H
ZZ
P
Pdz
kT
mg
P
dP o
o
Z
Z
P
P oo
ln
mg
kTH
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Hydrostatic EquilibriumHydrostatic Equilibrium
H
ZZ
P
P o
o
ln
This means that pressure falls off exponentially with altitude z.H = kT/mg is the Atmospheric Scale Height, and is also the equivalent thickness of the atmosphere for constant temperature.
Near the Earth’s surface, H ~ 7-8 km.
Hzzo
oezPzP /)()()(
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Atmospheric Scale HeightAtmospheric Scale Height
Hzzo
oezPzP /)()()(
This means that pressure falls off exponentially with altitude z, with a e-folding “distance” in the vertical of H. For an isothermal atmosphere (T = constant), density would have the same functional form.
H is also the equivalent “thickness” of the atmosphere. If the entire atmosphere was compressed to sea level pressure (Po), then the atmosphere would extend to a height of H.
Near the Earth’s surface, H ~ 7-8 km.
H is also roughly the altitude to which an atom moving vertically can reach. This can be seen by equating an atom’s kinetic to gravitational potential energy:
½ mv2 = 3/2 kT = 3/2 mgH
mg
kTH where
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Geopotential HeightGeopotential Height
z
gdzz0
)(
dpgdzd
The Geopotential, Φ, at any point in the Earth’s atmosphere is defined asthe work that must be done against the Earth’s gravitational field to raisea mass of 1 kg from sea level to that point. Units are J kg-1 or m2s-2.
The force (in newtons) acting on 1kg at height z above sea level is numericallyequal to g. The work (in joules) done in raising 1 kg from z to z+dz is:
From hydrostatic equilibrium (dp = -ρgdz) we get:
The Geopotential at height z is then:
gdzd
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We can also define a quantity called theWe can also define a quantity called the Geopotential HeightGeopotential Height, , Z, as:Z, as:
z
gdzgg
zZ
00
1)(
Where go is the globally averaged acceleration due to gravity at the Earth’s surface.
Geopotential Height is used as the vertical coordinate in most atmospheric applications in which energy plays an important role (e.g., large scale motions). In the lower atmosphere, there is only a small difference between the physical height z and the geopotential height Z.
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Thickness of Layer Between Pressure LevelsThickness of Layer Between Pressure Levels
RT
pg
z
p
p
dpRTgdzd
2
1
2
1
p
p p
dpRTd
2
1
12
p
p p
dpTR
1
2012
p
p p
dpT
g
RZZ
In meteorological applications it is not convenient to deal with density, as itis difficult to measure. Pressure makes a more convenient vertical variable.
Hydrostatic equilibrium:
Geopotential:
Integrate the geopotential between two pressure levels, p1 and p2.
implies:
From the definition of geopotential height:
This is known as the thickness of the layerbetween two pressure layers.
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Scale Height for an Isothermal AtmosphereScale Height for an Isothermal Atmosphere
1
2012
p
p p
dp
g
RTZZ
1
2012
p
p p
dpT
g
RZZ
1
2012
p
p p
dpT
g
RZZ
If T = constant, OR if the meantemperature is used in this expression,then we get:
)/ln( 2112 ppHZZ
H
ZZpp
)(exp 12
12
Which can be integrated exactly:
Or, by raising e to the power of each side:Scale Height: H = RT/go
H ~ 7-8 km in lower atmosphere
Thickness:
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Thickness and Heights of Constant Pressure SurfacesThickness and Heights of Constant Pressure Surfaces
H
ZZpp
)(exp 12
12
Note that there is a uniquerelationship between P & Z.
Thus pressure can (and is)used as a vertical coordinate.
Lines of constant pressure areknown as isobars.
Pressure decreases monotonically with height, thus pressure surfacesnever intersect.
Pressure is a principle driver of atmospheric motions, and thus characterizingthe variation of pressure can provide insight into atmospheric dynamics.
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First Law of Thermodynamics, Once AgainFirst Law of Thermodynamics, Once Again
dQ = dU + PdV
Heat Flow (in/out) = change in internal energy + work done by parcel
Using the specific heat relationship we have
dU = Cv dT
So we can write: dQ = Cv dT + PdV
as equivalent statement of the First Law of Thermodynamics.
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Derivation of the Dry Adiabatic Lapse Rate (DALR)Derivation of the Dry Adiabatic Lapse Rate (DALR)
Hydrostatic Equilibrium: dP = -ρg dz, or VdP = -g dz(where V = specific volume = 1/ρ)Ideal Gas Law: P = ρRT = RT/ VFirst Law of Thermodynamics: dQ = CvdT + P dVRewrite IGL PV = RTDifferentiate the IGL P dV + V dP = RdT = (Cp-Cv) dT(For an ideal gas Cp – Cv = R)Combine FLT & IGL dQ = Cv dT + (Cp-Cv) dT – V dP dQ = CpdT – V dPBut for an adiabatic process (no energy flow into or out of the parcel) dQ = 0
So CpdT = V dP = -g dz dT/dz = -g/Cp DALR
Note that the DALR doesn’t say anything about the actual value of T,but it provides a very strong constraint on how T varies with altitude.
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Adiabatic Processes for ParcelsAdiabatic Processes for Parcels
If we slowly move a parcel of dry air vertically, such that there is no energyflow with its environment (dQ=0), then its temperature will change withaltitude following the Dry Adiabatic Lapse Rate (DALR).
pd C
g
dz
dTDALR
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The Dry Adiabatic Lapse RateThe Dry Adiabatic Lapse Rate
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Dry Adiabatic Lapse Rate and the PV DiagramDry Adiabatic Lapse Rate and the PV Diagram
The (P,V) curve in a thermodynamic diagram of vertical motion in the atmosphere following the DALR will be an Adiabat.
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Dry Adiabatic Lapse RateDry Adiabatic Lapse Rate
For the Earth:DALR ~ -7-8 K/km
If we know the temperature ofthe atmosphere are any level,and we know that the heat fluxis zero, i.e. adiabatic, then wecan deduce the temperature atany other level.
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Entropy and Potential TemperatureEntropy and Potential Temperature
First Law of Thermodynamics: dQ = dU + PdV = dU - VdPInternal Energy: dU = Cp dTSecond Law of Thermodynamics: dS = dQ/T
S = Entropy of the system
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Entropy and Potential TemperatureEntropy and Potential Temperature
VdPdUPdVdUdWdUdQ
dPPRTdTCVdPdTCTdS pp )/(
P
dPR
T
dTCdS p
Where κ =R/Cp (approximately 2/7 for a diatomic gas)So is the constant of integration.
oopo P
PR
T
TCSS lnln
'ln op STpCS
FLT
SLT
Integration
Rewrite:
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Adiabatic Processes: dQ = 0Adiabatic Processes: dQ = 0Constant Entropy Processes: dS = 0Constant Entropy Processes: dS = 0
P
dPR
T
dTC p
P
dPR
T
dTCdS p
oP
PT
p P
dPR
T
dTC
From the Second Law of Thermodynamics dS = dQ/T, an adiabaticprocess is thus an isentropic process.
dS=0
P
PR
TC o
p lnln
Integrate:
P
PT o
Potential Temperature
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Potential TemperaturePotential Temperature
If we take a parcel of gas at If we take a parcel of gas at T,P and change it T,P and change it adiabatically to standard adiabatically to standard pressure Ppressure Poo, it will have a , it will have a temperature of temperature of θθ..
Why do airplanes needWhy do airplanes needair conditioners?air conditioners?
http://dewx.easternuswx.com/Figures/Figure_2.jpg
kmP(mbar)
Slanted blue lines are adiabats
P
PT o
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Parcel Concepts: Key IdeasParcel Concepts: Key Ideas
constvv dT
dqC
kTmv2
3
2
1 2 Internal Energy (kinetic energy):
Internal Energy (general): U = ρ CpT
Internal Energy Change: dU = CpdT; Work=PdV
First Law of Thermodynamics: dQ = dU + PdV
Second Law of Thermodynamics: dS = dQ/T
Hydrostatic Equilibrium: dP = -ρ gdz
Specific Heats (at constant P)
Specific Heats (at constant V)
constpp dT
dqC