text:
Modern Family (season 10)
From Wikipedia, the free encyclopedia
Jump to navigation Jump to search
Modern Family (season 10)
Promotional poster
Starring
Ed O'Neill
Sofía Vergara
Julie Bowen
Ty Burrell
Jesse Tyler Ferguson
Eric Stonestreet
Sarah Hyland
Ariel Winter
Nolan Gould
Rico Rodriguez
Aubrey Anderson-Emmons
Jeremy Maguire
Country of origin
United States
No. of episodes
5
Release
Original network
ABC
Original release
September 26, 2018 (2018-09-26) – present
Season chronology
← Previous
Season 9
List of Modern Family episodes
The tenth season of Modern Family debuted on September 26, 2018 on ABC.[1] The show is scheduled on Wednesday nights and is produced by 20th Century Fox Television, Steven Levitan Prods., and Picador Productions, with creators Steven Levitan and Christopher Lloyd as showrunners. Modern Family was renewed for its tenth season in May 2017.[2]
In January 2018, creators Levitan and Lloyd stated that the tenth season would most likely be the series' final[3] although later in August 2018, it was reported that ABC were in discussions to renew the series for a potential 18-episode eleventh and final season.[4][5]
Contents
1 Cast
1.1 Main
1.2 Recurring
1.3 Guest
2 Episodes
3 Reception
3.1 Live + SD ratings
3.2 Live + 7 Day (DVR) ratings
4 References
5 External links
Cast[edit]
See also: List of Modern Family characters
Main[edit]
Ed O'Neill as Jay Pritchett
Sofía Vergara as Gloria Pritchett
Julie Bowen as Claire Dunphy
Ty Burrell as Phil Dunphy
Jesse Tyler Ferguson as Mitchell Pritchett
Eric Stonestreet as Cameron Tucker
Sarah Hyland as Haley Dunphy
Ariel Winter as Alex Dunphy
Nolan Gould as Luke Dunphy
Rico Rodriguez as Manny Delgado
Aubrey Anderson-Emmons as Lily Tucker-Pritchett
Jeremy Maguire as Joe Pritchett
Recurring[edit]
Chris Geere as Arvin Fennerman[6]
Reid Ewing as Dylan Marshal[7]
Guest[edit]
Dan Levy as Jonah
Ben Schwartz as Nick
Marcello Reyes as Cal
Hillary Ann Matthews as Sherry
Jimmy Tatro as Bill
Shelley Long as Dede Pritchett
Sherian Pierce as Paige
Rosa Blasi as Florence
Episodes[edit]
See also: List of Modern Family episodes
No.
overall
No. in
season
Title
Directed by
Written by
Original air date
Prod.
code
US viewers
(millions)
211
1 "I Love a Parade" James Bagdonas Paul Corrigan & Brad Walsh September 26, 2018 (2018-09-26) 10ARG01 5.40[8]
The family gets together for the annual Fourth of July parade where Jay acts as the grand marshal; Haley's farewell to Arvin doesn't go as well as expected and she is distracted by the return of an old flame.
212
2 "Kiss and Tell" Steven Levitan Abraham Higginbotham & Jon Pollack October 3, 2018 (2018-10-03) 10ARG02 5.39[9]
The family gets together at Jay's house but nobody knows what the occasion is. Phil plans to flip the script on Jay Mean Girls-style after watching the movie with Alex. Manny returns from his road trip and tells them he has Canadian girlfriend, but nobody really believes him because he doesn't have any picture of her. Hayley feels conflicted about kissing Dylan, and looks for advice, but her uncles and later her parents give her conflicting opinions.
213
3 "A Sketchy Area" Jeffrey Walker Elaine Ko October 10, 2018 (2018-10-10) 10ARG03 5.10[10]
Phil stumbles into an exciting new career after dropping by Luke's college. Claire deals with her dad, Jay, and the merger of Pritchett's Closets with a tech-savvy, hipper company. Mitch's new high-profile case as an assistant district attorney is marred by an unflattering courtroom sketch by the resident artist.
214
4 "Torn Between Two Lovers" Beth McCarthy-Miller Jeffrey Richman & Danny Zuker October 17, 2018 (2018-10-17) 10ARG04 5.03[11]
Haley can't seem to choose between her past and present relationships. Manny returns to college and dorm life while his girlfriend, Sherry, continues to stay at Jay and Gloria's, and might be overstaying her welcome.
215
5 "Good Grief" Beth McCarthy-Miller Vali Chandrasekaran & Stephen Lloyd October 24, 2018 (2018-10-24) 10ARG06 5.27[12]
During the Halloween, Jay, Mitchell and Claire receives a call revealing that his mother DeDe has died in her sleep, the family must dealing about her recent news.
216
6 "On the Same Paige"[13] Ryan Case Ryan Walls October 31, 2018 (2018-10-31) 10ARG05 TBD
217
7 "Did the Chicken Cross the Road?"[14] Eric Dean Seaton Bill Wrubel November 7, 2018 (2018-11-07) 10ARG07 TBD
Reception[edit]
Live + SD ratings[edit]
No. in
series
No. in
season
Episode
Air date
Time slot (EST)
Rating/share (18–49)
Viewers
(millions)
18–49 rank
Viewership rank
211 1 I Love a Parade September 26, 2018 (2018-09-26) Wednesdays
9:00 p.m. 1.6/7[8] 5.40[8] 22[15] N/A
212 2 Kiss and Tell October 3, 2018 (2018-10-03) 1.4/6[9] 5.39[9] 18[16] N/A
213 3 A Sketchy Area October 10, 2018 (2018-10-10) 1.4/6[10] 5.10[10] TBA TBA
214 4 Torn Between Two Lovers October 17, 2018 (2018-10-17) 1.3/6[11] 5.03[11] TBA TBA
215 5 Good Grief October 24, 2018 (2018-10-24) 1.5/6[12] 5.27[12] TBA TBA
216 6 On the Same Paige October 31, 2018 (2018-10-31) TBA TBA TBA TBA
217 7 Did the Chicken Cross the Road? November 7, 2018 (2018-11-07) TBA TBA TBA TBA
Live + 7 Day (DVR) ratings[edit]
No. in
series
No. in
season
Episode
Air date
Time slot (EST)
18–49 rating increase
Viewers
(millions) increase
Total 18-49
Total viewers
(millions)
Ref.
211 1 "I Love a Parade" September 26, 2018 (2018-09-26) Wednesdays
9:00 p.m.
1.2
3.20
2.8
8.60
[17]
212 2 "Kiss and Tell" October 3, 2018 (2018-10-03)
1.2
2.90
2.6
8.29
[18]
213 3 "A Sketchy Area" October 10, 2018 (2018-10-10)
214 4 "Torn Between Two Lovers" October 17, 2018 (2018-10-17)
215 5 "Good Grief" October 24, 2018 (2018-10-24)
216 6 "On the Same Paige" October 31, 2018 (2018-10-31)
217 7 "Did the Chicken Cross the Road?" November 7, 2018 (2018-11-07)
References[edit]
Jump up ^ "ABC Fall Premiere Dates 2018: See the Complete Schedule!". ABC. ABC. Retrieved 25 July 2018.
Jump up ^ Goldberg, Lesley. "'Modern Family' Renewed for Seasons 9 and 10 as Cast Inks Rich New Deals to Return". The Hollywood Reporter. The Hollywood Reporter. Retrieved 16 September 2017.
Jump up ^ "Modern Family Showrunners Are Already Plotting the Series Finale — and It's Soon!". TVGuide.com. 2018-01-10. Retrieved 2018-01-11.
Jump up ^ Andreeva, Nellie (August 7, 2018). "'Modern Family': ABC In Talks For Season 11 Of Comedy Series – TCA". Deadline. Retrieved September 20, 2018.
Jump up ^ Andreeva, Nellie (September 19, 2019). "'Modern Family': Optimism Grows For Season 11 Of ABC Comedy Series". Deadline. Retrieved September 20, 2018.
Jump up ^ @cwgeere (August 2, 2018). "First read of season 10! Such an honour to be a part of this national treasure..." (Tweet) – via Twitter.
Jump up ^ "(#1001) I Love a Parade". TheFutonCritic.com. Retrieved September 17, 2018.
^ Jump up to: a b c Welch, Alex (September 27, 2018). "'Chicago Fire' and 'Survivor' adjusts up, 'Star' adjusts down: Wednesday final ratings". TV by the Numbers. Retrieved September 27, 2018.
^ Jump up to: a b c Welch, Alex (October 4, 2018). "'Single Parents,' 'Empire,' everything else unchanged: Wednesday final ratings". TV by the Numbers. Retrieved October 4, 2018.
^ Jump up to: a b c Welch, Alex (October 11, 2018). "'Survivor,' 'Empire,' and 'Chicago Fire' adjust up: Wednesday final ratings". TV by the Numbers. Retrieved October 11, 2018.
^ Jump up to: a b c Welch, Alex (October 18, 2018). "'Chicago P.D.' and 'Single Parents' adjust down: Wednesday final ratings". TV by the Numbers. Retrieved October 18, 2018.
^ Jump up to: a b c Welch, Alex (October 25, 2018). "'Survivor,' 'Chicago Fire,' and 'World Series' adjust up, 'Single Parents' and 'Chicago Med' adjust down: Wednesday final ratings". TV by the Numbers. Retrieved October 25, 2018.
Jump up ^ "(#1005) "On the Same Paige"". The Futon Critic. Retrieved October 15, 2018.
Jump up ^ "(#1007) "Did the Chicken Cross the Road?"". The Futon Critic. Retrieved October 22, 2018.
Jump up ^ Welch, Alex (2018-10-02). "'This is Us' and 'The Big Bang Theory' lead premiere week: Broadcast top 25 and network rankings for Sept. 24-30". TV By The Numbers. Retrieved 2018-10-12.
Jump up ^ Welch, Alex (2018-10-11). "'This is Us' and Sunday Night Football stay on top: Broadcast top 25 and network rankings for Oct. 1-7". TV By The Numbers. Retrieved 2018-10-12.
Jump up ^ Pucci, Douglas (October 11, 2018). "Live+7 Weekly Ratings: 'Manifest' is Most-Watched NBC Drama Series Premiere in 19 Years". Programming Insider. Retrieved October 20, 2018.
Jump up ^ Welch, Alex (October 18, 2018). "'A Million Little Things' and 'Manifest' score biggest viewer gains in broadcast Live +7 ratings for Oct. 1-7". TV by the Numbers. Retrieved October 20, 2018.
External links[edit]
List of Modern Family episodes on IMDb
hide
v
t
e
Modern Family
Awards and nominations
Characters
Episodes
1
2
3
4
5
6
7
8
9
10
Adaptations
Familia moderna
Haft Sang
Category
Retrieved from "https://en.wikipedia.org/w/index.php?title=Modern_Family_(season_10)&oldid=866454125"
Categories:
2018 American television seasons
Modern Family seasons
Navigation menu
Personal tools
Not logged in
Talk
Contributions
Create account
Log in
Namespaces
Article
Talk
Variants
Views
Read
Edit
View history
More
Search
Navigation
Main page
Contents
Featured content
Current events
Random article
Donate to Wikipedia
Wikipedia store
Interaction
Help
About Wikipedia
Community portal
Recent changes
Contact page
Tools
What links here
Related changes
Upload file
Special pages
Permanent link
Page information
Wikidata item
Cite this page
Print/export
Create a book
Download as PDF
Printable version
Languages
Español
Français
Italiano
Edit links
This page was last edited on 30 October 2018, at 12:50 (UTC).
Text is available under the Creative Commons Attribution-ShareAlike License; additional terms may apply. By using this site, you agree to the Terms of Use and Privacy Policy. Wikipedia® is a registered trademark of the Wikimedia Foundation, Inc., a non-profit organization.
Privacy policy
About Wikipedia
Disclaimers
Contact Wikipedia
Developers
Cookie statement
Mobile view
Enable previews

values: mw-page-base noprint

values: mw-head-base noprint

values: firstHeading firstHeading en

values: siteSub noprint

values: mw-jump-link #mw-head

values: mw-jump-link #p-search

values: text-align:center;font-size:125%;font-weight:bold;background: #F4F3F9; color: black; padding: 0.25em 1em; line-height: 1.5em;

values:
row
white-space: nowrap

values: text-align:center;background: #F4F3F9; color: black; padding: 0.25em 1em; line-height: 1.5em;

values:
/wiki/Christopher_Lloyd_(screenwriter)
mw-redirect
Christopher Lloyd (screenwriter)

values: checkbox button toctogglecheckbox toctogglecheckbox display:none

values:
description
8
border-bottom:solid 3px #F4F3F9

values: background: #ececec; color: #2C2C2C; vertical-align: middle; font-size: smaller; text-align: center;

values:
wikitable
text-align:center; width: 100%;

values: Edit section: Live + 7 Day (DVR) ratings

values: font-size:90%; text-align:center; width: 100%; margin-left: auto; margin-right: auto;

values: List of awards and nominations received by Modern Family

values:
/wiki/Haft_Sang_(television_series)
mw-redirect
Haft Sang (television series)

values: nowraplinks hlist collapsible autocollapse navbox-inner mw-collapsible mw-made-collapsible

values: Category:2018 American television seasons

values:
catlinks mw-normal-catlinks
catlinks mw-normal-catlinks
interface

values: Discussion about edits from this IP address [ctrl-alt-n]

values: A list of edits made from this IP address [ctrl-alt-y]

values: You are encouraged to create an account and log in; however, it is not mandatory

values: You're encouraged to log in; however, it's not mandatory. [ctrl-alt-o]

values:
/wiki/Modern_Family_(season_10)
View the content page [ctrl-alt-c]
c

values: Discussion about the content page [ctrl-alt-t]

values: p-namespaces navigation vectorTabs p-namespaces-label

values:
p-variants
navigation
vectorMenu emptyPortlet
p-variants-label

values: Past revisions of this page [ctrl-alt-h]

values: p-views navigation vectorTabs p-views-label

values:
p-cactions
navigation
vectorMenu emptyPortlet
p-cactions-label

values:
mw-wiki-logo
/wiki/Main_Page
Visit the main page

values:
/wiki/Main_Page
Visit the main page [ctrl-alt-z]
z

values: Featured content – the best of Wikipedia

values: Find background information on current events

values:
/wiki/Special:Random
Load a random article [ctrl-alt-x]
x

values: portal navigation p-navigation p-navigation-label

values: Guidance on how to use and edit Wikipedia

values: Anexo:Décima temporada de Modern Family – Spanish

values: Episodi di Modern Family (decima stagione) – Italian

values: mediawiki ltr sitedir-ltr mw-hide-empty-elt ns-0 ns-subject page-Modern_Family_season_10 rootpage-Modern_Family_season_10 skin-vector action-view


text:
Adiabatic process
From Wikipedia, the free encyclopedia
Jump to: navigation, search
Thermodynamics
The classical Carnot heat engine
Branches[show]
Classical
Statistical
Chemical
Equilibrium / Non-equilibrium
Laws[show]
Zeroth
First
Second
Third
Systems[show]
State
Equation of state
Ideal gas
Real gas
State of matter
Equilibrium
Control volume
Instruments
Processes
Isobaric
Isochoric
Isothermal
Adiabatic
Isentropic
Isenthalpic
Quasistatic
Polytropic
Free expansion
Reversibility
Irreversibility
Endoreversibility
Cycles
Heat engines
Heat pumps
Thermal efficiency
System properties[show]
Note: Conjugate variables in italics
Property diagrams
Intensive and extensive properties
Functions of state
Temperature / Entropy (introduction)
Pressure / Volume
Chemical potential / Particle number
Vapor quality
Reduced properties
Process functions
Work
Heat
Material properties[show]
Property databases
Specific heat capacity c = {\displaystyle c=}
T {\displaystyle T} ∂ S {\displaystyle \partial S}
N {\displaystyle N} ∂ T {\displaystyle \partial T}
Compressibility β = − {\displaystyle \beta =-}
1 {\displaystyle 1} ∂ V {\displaystyle \partial V}
V {\displaystyle V} ∂ p {\displaystyle \partial p}
Thermal expansion α = {\displaystyle \alpha =}
1 {\displaystyle 1} ∂ V {\displaystyle \partial V}
V {\displaystyle V} ∂ T {\displaystyle \partial T}
Equations[show]
Carnot's theorem
Clausius theorem
Fundamental relation
Ideal gas law
Maxwell relations
Onsager reciprocal relations
Bridgman's equations
Table of thermodynamic equations
Potentials[show]
Free energy
Free entropy
Internal energy
U ( S , V ) {\displaystyle U(S,V)}
Enthalpy
H ( S , p ) = U + p V {\displaystyle H(S,p)=U+pV}
Helmholtz free energy
A ( T , V ) = U − T S {\displaystyle A(T,V)=U-TS}
Gibbs free energy
G ( T , p ) = H − T S {\displaystyle G(T,p)=H-TS}
History
Culture
[show]
History
General
Heat
Entropy
Gas laws
"Perpetual motion" machines
Philosophy
Entropy and time
Entropy and life
Brownian ratchet
Maxwell's demon
Heat death paradox
Loschmidt's paradox
Synergetics
Theories
Caloric theory
Theory of heat
Vis viva ("living force")
Mechanical equivalent of heat
Motive power
Key publications
"An Experimental Enquiry
Concerning ... Heat"
"On the Equilibrium of
Heterogeneous Substances"
"Reflections on the
Motive Power of Fire"
Timelines
Thermodynamics
Heat engines
Art
Education
Maxwell's thermodynamic surface
Entropy as energy dispersal
Scientists[show]
Bernoulli
Boltzmann
Carnot
Clapeyron
Clausius
Carathéodory
Duhem
Gibbs
von Helmholtz
Joule
Maxwell
von Mayer
Onsager
Rankine
Smeaton
Stahl
Thompson
Thomson
van der Waals
Waterston
Book:Thermodynamics
v
t
e
This article is about adiabatic processes in thermodynamics. For the adiabatic theorem in quantum mechanics, see adiabatic theorem.
In thermodynamics, an adiabatic process is one that occurs without transfer of heat or matter between a thermodynamic system and its surroundings. In an adiabatic process, energy is transferred to its surroundings only as work.[1][2] The adiabatic process provides a rigorous conceptual basis for the theory used to expound the first law of thermodynamics, and as such it is a key concept in thermodynamics.
Some chemical and physical processes occur so rapidly that they may be conveniently described by the term "adiabatic approximation", meaning that there is not enough time for the transfer of energy as heat to take place to or from the system.[3]
By way of example, the adiabatic flame temperature is an idealization that uses the "adiabatic approximation" so as to provide an upper limit calculation of temperatures produced by combustion of a fuel. The adiabatic flame temperature is the temperature that would be achieved by a flame if the process of combustion took place in the absence of heat loss to the surroundings.
Contents
[hide]
1 Description
1.1 Various applications of the adiabatic assumption
2 Adiabatic heating and cooling
3 Ideal gas (reversible process)
3.1 Example of adiabatic compression
3.2 Adiabatic free expansion of a gas
3.3 Derivation of P–V relation for adiabatic heating and cooling
3.4 Derivation of P–T relation for adiabatic heating and cooling
3.5 Derivation of discrete formula
4 Graphing adiabats
5 Etymology
6 Conceptual significance in thermodynamic theory
7 Divergent usages of the word adiabatic
8 See also
9 References
10 External links
Description[edit]
A process that does not involve the transfer of heat or matter into or out of a system, so that Q = 0, is called an adiabatic process, and such a system is said to be adiabatically isolated.[4][5] The assumption that a process is adiabatic is a frequently made simplifying assumption. For example, the compression of a gas within a cylinder of an engine is assumed to occur so rapidly that on the time scale of the compression process, little of the system's energy can be transferred out as heat to the surroundings. Even though the cylinders are not insulated and are quite conductive, that process is idealized to be adiabatic. The same can be said to be true for the expansion process of such a system.
The assumption of adiabatic isolation of a system is a useful one, and is often combined with others so as to make the calculation of the system's behaviour possible. Such assumptions are idealizations. The behaviour of actual machines deviates from these idealizations, but the assumption of such "perfect" behaviour provide a useful first approximation of how the real world works. According to Laplace, when sound travels in a gas, there is no time for heat conduction in the medium and so the propagation of sound is adiabatic. For such an adiabatic process, the modulus of elasticity (Young's modulus) can be expressed as E = γP, where γ is the ratio of specific heats at constant pressure and at constant volume (γ = Cp/Cv ) and P is the pressure of the gas .
Various applications of the adiabatic assumption[edit]
For a closed system, one may write the first law of thermodynamics as : ΔU = Q + W, where ΔU denotes the change of the system's internal energy, Q the quantity of energy added to it as heat, and W the work done on it by its surroundings.
If the system has rigid walls such that work cannot be transferred in or out (W = 0), and the walls of the system are not adiabatic and energy is added in the form of heat (Q > 0), and there is no phase change, the temperature of the system will rise.
If the system has rigid walls such that pressure–volume work cannot be done, and the system walls are adiabatic (Q = 0), but energy is added as isochoric work in the form of friction or the stirring of a viscous fluid within the system (W > 0), and there is no phase change, the temperature of the system will rise.
If the system walls are adiabatic (Q = 0), but not rigid (W ≠ 0), and, in a fictive idealized process, energy is added to the system in the form of frictionless, non-viscous pressure–volume work, and there is no phase change, the temperature of the system will rise. Such a process is called an isentropic process and is said to be "reversible". Fictively, if the process is reversed, the energy added as work can be recovered entirely as work done by the system. If the system contains a compressible gas and is reduced in volume, the uncertainty of the position of the gas is reduced, and seemingly would reduce the entropy of the system, but the temperature of the system will rise as the process is isentropic (ΔS = 0). Should the work be added in such a way that friction or viscous forces are operating within the system, then the process is not isentropic, and if there is no phase change, then the temperature of the system will rise, the process is said to be "irreversible", and the work added to the system is not entirely recoverable in the form of work.
If the walls of a system are not adiabatic, and energy is transferred in as heat, entropy is transferred into the system with the heat. Such a process is neither adiabatic nor isentropic, having Q > 0, and ΔS > 0 according to the second law of thermodynamics.
Naturally occurring adiabatic processes are irreversible (entropy is produced).
The transfer of energy as work into an adiabatically isolated system can be imagined as being of two idealized extreme kinds. In one such kind, there is no entropy produced within the system (no friction, viscous dissipation, etc.), and the work is only pressure-volume work (denoted by P dV). In nature, this ideal kind occurs only approximately, because it demands an infinitely slow process and no sources of dissipation.
The other extreme kind of work is isochoric work (dV = 0), for which energy is added as work solely through friction or viscous dissipation within the system. A stirrer that transfers energy to a viscous fluid of an adiabatically isolated system with rigid walls, without phase change, will cause a rise in temperature of the fluid, but that work is not recoverable. Isochoric work is irreversible.[6] The second law of thermodynamics observes that a natural process, of transfer of energy as work, always consists at least of isochoric work and often both of these extreme kinds of work. Every natural process, adiabatic or not, is irreversible, with ΔS > 0, as friction or viscosity are always present to some extent.
Adiabatic heating and cooling[edit]
The adiabatic compression of a gas causes a rise in temperature of the gas. Adiabatic expansion against pressure, or a spring, causes a drop in temperature. In contrast, free expansion is an isothermal process for an ideal gas.
Adiabatic heating occurs when the pressure of a gas is increased from work done on it by its surroundings, e.g., a piston compressing a gas contained within a cylinder and raising the temperature where in many practical situations heat conduction through walls can be slow compared with the compression time. This finds practical application in diesel engines which rely on the lack of heat dissipation during the compression stroke to elevate the fuel vapor temperature sufficiently to ignite it.
Adiabatic heating occurs in the Earth's atmosphere when an air mass descends, for example, in a katabatic wind, Foehn wind, or chinook wind flowing downhill over a mountain range. When a parcel of air descends, the pressure on the parcel increases. Due to this increase in pressure, the parcel's volume decreases and its temperature increases as work is done on the parcel of air, thus increasing its internal energy, which manifests itself by a rise in the temperature of that mass of air. The parcel of air can only slowly dissipate the energy by conduction or radiation (heat), and to a first approximation it can be considered adiabatically isolated and the process an adiabatic process.
Adiabatic cooling occurs when the pressure on an adiabatically isolated system is decreased, allowing it to expand, thus causing it to do work on its surroundings. When the pressure applied on a parcel of air is reduced, the air in the parcel is allowed to expand; as the volume increases, the temperature falls as its internal energy decreases. Adiabatic cooling occurs in the Earth's atmosphere with orographic lifting and lee waves, and this can form pileus or lenticular clouds.
Adiabatic cooling does not have to involve a fluid. One technique used to reach very low temperatures (thousandths and even millionths of a degree above absolute zero) is via adiabatic demagnetisation, where the change in magnetic field on a magnetic material is used to provide adiabatic cooling. Also, the contents of an expanding universe can be described (to first order) as an adiabatically cooling fluid. (See heat death of the universe.)
Rising magma also undergoes adiabatic cooling before eruption, particularly significant in the case of magmas that rise quickly from great depths such as kimberlites.[7]
Such temperature changes can be quantified using the ideal gas law, or the hydrostatic equation for atmospheric processes.
In practice, no process is truly adiabatic. Many processes rely on a large difference in time scales of the process of interest and the rate of heat dissipation across a system boundary, and thus are approximated by using an adiabatic assumption. There is always some heat loss, as no perfect insulators exist.
Ideal gas (reversible process)[edit]
Main article: Reversible adiabatic process
For a simple substance, during an adiabatic process in which the volume increases, the internal energy of the working substance must decrease
The mathematical equation for an ideal gas undergoing a reversible (i.e., no entropy generation) adiabatic process can be represented by the polytropic process equation[3]
P V n = constant {\displaystyle PV^{n}=\operatorname {constant} \qquad }
where P is pressure, V is volume, and for this case n = γ where
γ = C P C V = f + 2 f , {\displaystyle \gamma ={C_{P} \over C_{V}}={\frac {f+2}{f}},}
CP being the specific heat for constant pressure, CV being the specific heat for constant volume, γ is the adiabatic index, and f is the number of degrees of freedom (3 for monatomic gas, 5 for diatomic gas and collinear molecules e.g. carbon dioxide).
For a monatomic ideal gas, γ = 5/3, and for a diatomic gas (such as nitrogen and oxygen, the main components of air) γ = 7/5.[8] Note that the above formula is only applicable to classical ideal gases and not Bose–Einstein or Fermi gases.
For reversible adiabatic processes, it is also true that
P 1 − γ T γ = constant {\displaystyle P^{1-\gamma }T^{\gamma }=\operatorname {constant} } [3]
V T f 2 = constant {\displaystyle VT^{\frac {f}{2}}=\operatorname {constant} }
where T is an absolute temperature. This can also be written as
T V γ − 1 = constant {\displaystyle TV^{\gamma -1}=\operatorname {constant} } [3]
Example of adiabatic compression[edit]
The compression stroke in a gasoline engine can be used as an example of adiabatic compression. The model assumptions are: the uncompressed volume of the cylinder is one litre (1 l = 1000 cm3 = 0.001 m3 ); the gas within is the air consisting of molecular nitrogen and oxygen only (thus a diatomic gas with five degrees of freedom and so γ = 7/5); the compression ratio of the engine is 10:1 (that is, the 1 l volume of uncompressed gas is reduced to 0.1 l by the piston); and the uncompressed gas is at approximately room temperature and pressure (a warm room temperature of ~27 °C or 300 K, and a pressure of 1 bar = 100 kPa, i.e. typical sea-level atmospheric pressure).
P V γ = constant 1 = 100 , 000 Pa × ( 0.001 m 3 ) 7 5 {\displaystyle PV^{\gamma }=\operatorname {constant} _{1}=100,000\operatorname {Pa} \times (0.001\operatorname {m} ^{3})^{\frac {7}{5}}}
= 10 5 × 6.31 × 10 − 5 Pa  m 21 / 5 = 6.31 Pa  m 21 / 5 {\displaystyle =10^{5}\times 6.31\times 10^{-5}\operatorname {Pa} \operatorname {m} ^{21/5}=6.31\operatorname {Pa} \operatorname {m} ^{21/5}}
so our adiabatic constant for this example is about 6.31 Pa m4.2.
The gas is now compressed to a 0.1 l (0.0001 m3) volume (we will assume this happens quickly enough that no heat can enter or leave the gas through the walls). The adiabatic constant remains the same, but with the resulting pressure unknown
P V γ = constant 1 = 6.31 Pa  m 21 / 5 = P × ( 0.0001 m 3 ) 7 5 {\displaystyle PV^{\gamma }=\operatorname {constant} _{1}=6.31\operatorname {Pa} \operatorname {m} ^{21/5}=P\times (0.0001\operatorname {m} ^{3})^{\frac {7}{5}}}
so solving for P:
P = 6.31 Pa  m 21 / 5 ( 0.0001 m 3 ) 7 5 = 6.31 Pa  m 21 / 5 2.5 × 10 − 6 m 21 / 5 = 2.51 × 10 6 Pa {\displaystyle P={\frac {6.31\operatorname {Pa} \operatorname {m} ^{21/5}}{(0.0001\operatorname {m} ^{3})^{\frac {7}{5}}}}={\frac {6.31\operatorname {Pa} \operatorname {m} ^{21/5}}{2.5\times 10^{-6}\operatorname {m} ^{21/5}}}=2.51\times 10^{6}\operatorname {Pa} }
or 25.1 bar. Note that this pressure increase is more than a simple 10:1 compression ratio would indicate; this is because the gas is not only compressed, but the work done to compress the gas also increases its internal energy which manifests itself by a rise in the gas's temperature and an additional rise in pressure above what would result from a simplistic calculation of 10 times the original pressure.
We can solve for the temperature of the compressed gas in the engine cylinder as well, using the ideal gas law, PV=nRT (n is amount of gas in mol and R the gas constant for that gas). Our initial conditions being 100 kPa of pressure, 1 l volume, and 300 K of temperature, our experimental constant (=nR) is:
P V T = constant 2 = 10 5 Pa × 10 − 3 m 3 300 K = 0.333 Pa  m 3  K − 1 {\displaystyle {PV \over T}=\operatorname {constant} _{2}={{10^{5}\operatorname {Pa} \times 10^{-3}\operatorname {m} ^{3}} \over {300\operatorname {K} }}=0.333\operatorname {Pa} \operatorname {m} ^{3}\operatorname {K} ^{-1}}
We know the compressed gas has V = 0.1 l and P = 7006251000000000000♠2.51×106 Pa, so we can solve for temperature:
T = P V constant 2 = 2.51 × 10 6 Pa × 10 − 4 m 3 0.333 Pa  m 3  K − 1 = 753 K {\displaystyle T={PV \over {\operatorname {constant} _{2}}}={{2.51\times 10^{6}\operatorname {Pa} \times 10^{-4}\operatorname {m} ^{3}} \over {0.333\operatorname {Pa} \operatorname {m} ^{3}\operatorname {K} ^{-1}}}=753\operatorname {K} }
That is a final temperature of 753 K, or 479 °C, or 896 °F, well above the ignition point of many fuels. This is why a high-compression engine requires fuels specially formulated to not self-ignite (which would cause engine knocking when operated under these conditions of temperature and pressure), or that a supercharger with an intercooler to provide a pressure boost but with a lower temperature rise would be advantageous. A diesel engine operates under even more extreme conditions, with compression ratios of 20:1 or more being typical, in order to provide a very high gas temperature which ensures immediate ignition of the injected fuel.
Adiabatic free expansion of a gas[edit]
See also: Free expansion
For an adiabatic free expansion of an ideal gas, the gas is contained in an insulated container and then allowed to expand in a vacuum. Because there is no external pressure for the gas to expand against, the work done by or on the system is zero. Since this process does not involve any heat transfer or work, the first law of thermodynamics then implies that the net internal energy change of the system is zero. For an ideal gas, the temperature remains constant because the internal energy only depends on temperature in that case. Since at constant temperature, the entropy is proportional to the volume, the entropy increases in this case, therefore this process is irreversible.
Derivation of P–V relation for adiabatic heating and cooling[edit]
The definition of an adiabatic process is that heat transfer to the system is zero, δQ = 0. Then, according to the first law of thermodynamics,
(1) d U + δ W = δ Q = 0 , {\displaystyle {\text{(1)}}\qquad dU+\delta W=\delta Q=0,}
where dU is the change in the internal energy of the system and δW is work done by the system. Any work (δW) done must be done at the expense of internal energy U, since no heat δQ is being supplied from the surroundings. Pressure–volume work δW done by the system is defined as
(2) δ W = P d V . {\displaystyle {\text{(2)}}\qquad \delta W=P\,dV.}
However, P does not remain constant during an adiabatic process but instead changes along with V.
It is desired to know how the values of dP and dV relate to each other as the adiabatic process proceeds. For an ideal gas the internal energy is given by
(3) U = α n R T , {\displaystyle {\text{(3)}}\qquad U=\alpha nRT,}
where α is the number of degrees of freedom divided by two, R is the universal gas constant and n is the number of moles in the system (a constant).
Differentiating Equation (3) and use of the ideal gas law, PV = nRT, yields
(4) d U = α n R d T = α d ( P V ) = α ( P d V + V d P ) . {\displaystyle {\text{(4)}}\qquad dU=\alpha nR\,dT=\alpha \,d(PV)=\alpha (P\,dV+V\,dP).}
Equation (4) is often expressed as dU = nCV dT because CV = αR.
Now substitute equations (2) and (4) into equation (1) to obtain
− P d V = α P d V + α V d P , {\displaystyle -P\,dV=\alpha P\,dV+\alpha V\,dP,}
factorize −P dV:
− ( α + 1 ) P d V = α V d P , {\displaystyle -(\alpha +1)P\,dV=\alpha V\,dP,}
and divide both sides by PV:
− ( α + 1 ) d V V = α d P P . {\displaystyle -(\alpha +1){dV \over V}=\alpha {dP \over P}.}
After integrating the left and right sides from V0 to V and from P0 to P and changing the sides respectively,
ln  ( P P 0 ) = − α + 1 α ln  ( V V 0 ) . {\displaystyle \ln \left({P \over P_{0}}\right)={-{\alpha +1 \over \alpha }}\ln \left({V \over V_{0}}\right).}
Exponentiate both sides, and substitute α + 1/α with γ, the heat capacity ratio
( P P 0 ) = ( V V 0 ) − γ , {\displaystyle \left({P \over P_{0}}\right)=\left({V \over V_{0}}\right)^{-{\gamma }},}
and eliminate the negative sign to obtain
( P P 0 ) = ( V 0 V ) γ . {\displaystyle \left({P \over P_{0}}\right)=\left({V_{0} \over V}\right)^{\gamma }.}
Therefore,
( P P 0 ) ( V V 0 ) γ = 1 {\displaystyle \left({P \over P_{0}}\right)\left({V \over V_{0}}\right)^{\gamma }=1}
and
P 0 V 0 γ = P V γ = constant . {\displaystyle P_{0}V_{0}^{\gamma }=PV^{\gamma }=\operatorname {constant} .}
Derivation of P–T relation for adiabatic heating and cooling[edit]
Substituting the ideal gas law into the above, we obtain
P ( n R T P ) γ = constant . {\displaystyle P\left({\frac {nRT}{P}}\right)^{\gamma }=\operatorname {constant} .}
which simplifies to
P ( 1 − γ ) T γ = constant . {\displaystyle P^{(1-\gamma )}T^{\gamma }=\operatorname {constant} .}
Derivation of discrete formula[edit]
The change in internal energy of a system, measured from state 1 to state 2, is equal to
(1) Δ U = α R n T 2 − α R n T 1 = α R n Δ T {\displaystyle {\text{(1)}}\qquad \Delta U=\alpha RnT_{2}-\alpha RnT_{1}=\alpha Rn\Delta T}
At the same time, the work done by the pressure-volume changes as a result from this process, is equal to
(2) W = ∫ V 1 V 2 P d V {\displaystyle {\text{(2)}}\qquad W=\int _{V_{1}}^{V_{2}}P\,dV}
Since we require the process to be adiabatic, the following equation needs to be true
(3) Δ U + W = 0 {\displaystyle {\text{(3)}}\qquad \Delta U+W=0}
By the previous derivation,
(4) P V γ = constant = P 1 V 1 γ {\displaystyle {\text{(4)}}\qquad PV^{\gamma }={\text{constant}}=P_{1}V_{1}^{\gamma }}
Rearranging (4) gives
P = P 1 ( V 1 V ) γ {\displaystyle P=P_{1}\left({\frac {V_{1}}{V}}\right)^{\gamma }}
Substituting this into (2) gives
W = ∫ V 1 V 2 P 1 ( V 1 V ) γ d V {\displaystyle W=\int _{V_{1}}^{V_{2}}P_{1}\left({\frac {V_{1}}{V}}\right)^{\gamma }\,dV}
Integrating,
W = P 1 V 1 γ V 2 1 − γ − V 1 1 − γ 1 − γ {\displaystyle W=P_{1}V_{1}^{\gamma }{\frac {V_{2}^{1-\gamma }-V_{1}^{1-\gamma }}{1-\gamma }}}
Substituting γ = α + 1/α,
W = − α P 1 V 1 γ ( V 2 1 − γ − V 1 1 − γ ) {\displaystyle W=-\alpha P_{1}V_{1}^{\gamma }\left(V_{2}^{1-\gamma }-V_{1}^{1-\gamma }\right)}
Rearranging,
W = − α P 1 V 1 ( ( V 2 V 1 ) 1 − γ − 1 ) {\displaystyle W=-\alpha P_{1}V_{1}\left(\left({\frac {V_{2}}{V_{1}}}\right)^{1-\gamma }-1\right)}
Using the ideal gas law and assuming a constant molar quantity (as often happens in practical cases),
W = − α n R T 1 ( ( V 2 V 1 ) 1 − γ − 1 ) {\displaystyle W=-\alpha nRT_{1}\left(\left({\frac {V_{2}}{V_{1}}}\right)^{1-\gamma }-1\right)}
By the continuous formula,
P 2 P 1 = ( V 2 V 1 ) − γ {\displaystyle {\frac {P_{2}}{P_{1}}}=\left({\frac {V_{2}}{V_{1}}}\right)^{-\gamma }}
Or,
( P 2 P 1 ) − 1 γ = V 2 V 1 {\displaystyle \left({\frac {P_{2}}{P_{1}}}\right)^{-1 \over \gamma }={\frac {V_{2}}{V_{1}}}}
Substituting into the previous expression for W,
W = − α n R T 1 ( ( P 2 P 1 ) γ − 1 γ − 1 ) {\displaystyle W=-\alpha nRT_{1}\left(\left({\frac {P_{2}}{P_{1}}}\right)^{\frac {\gamma -1}{\gamma }}-1\right)}
Substituting this expression and (1) in (3) gives
α n R ( T 2 − T 1 ) = α n R T 1 ( ( P 2 P 1 ) γ − 1 γ − 1 ) {\displaystyle \alpha nR(T_{2}-T_{1})=\alpha nRT_{1}\left(\left({\frac {P_{2}}{P_{1}}}\right)^{\frac {\gamma -1}{\gamma }}-1\right)}
Simplifying,
T 2 − T 1 = T 1 ( ( P 2 P 1 ) γ − 1 γ − 1 ) {\displaystyle T_{2}-T_{1}=T_{1}\left(\left({\frac {P_{2}}{P_{1}}}\right)^{\frac {\gamma -1}{\gamma }}-1\right)}
Simplifying,
T 2 T 1 − 1 = ( P 2 P 1 ) γ − 1 γ − 1 {\displaystyle {\frac {T_{2}}{T_{1}}}-1=\left({\frac {P_{2}}{P_{1}}}\right)^{\frac {\gamma -1}{\gamma }}-1}
Simplifying,
T 2 = T 1 ( P 2 P 1 ) γ − 1 γ {\displaystyle T_{2}=T_{1}\left({\frac {P_{2}}{P_{1}}}\right)^{\frac {\gamma -1}{\gamma }}}
Graphing adiabats[edit]
An adiabat is a curve of constant entropy in a diagram. Some properties of adiabats on a P–V diagram are indicated. These properties may be read from the classical behaviour of ideal gases, except in the region where PV becomes small (low temperature), where quantum effects become important.
Every adiabat asymptotically approaches both the V axis and the P axis (just like isotherms).
Each adiabat intersects each isotherm exactly once.
An adiabat looks similar to an isotherm, except that during an expansion, an adiabat loses more pressure than an isotherm, so it has a steeper inclination (more vertical).
If isotherms are concave towards the north-east direction (45°), then adiabats are concave towards the east north-east (31°).
If adiabats and isotherms are graphed at regular intervals of entropy and temperature, respectively (like altitude on a contour map), then as the eye moves towards the axes (towards the south-west), it sees the density of isotherms stay constant, but it sees the density of adiabats grow. The exception is very near absolute zero, where the density of adiabats drops sharply and they become rare (see Nernst's theorem).[clarification needed]
The following diagram is a P–V diagram with a superposition of adiabats and isotherms:
The isotherms are the red curves and the adiabats are the black curves.
The adiabats are isentropic.
Volume is the horizontal axis and pressure is the vertical axis.
Etymology[edit]
Look up adiabatic in Wiktionary, the free dictionary.
The term adiabatic (/ˌædiəˈbætɪk/) is an anglicization of the Greek term ἀδιάβατος "impassable" (used by Xenophon of rivers). It is used in the thermodynamic sense by Rankine (1866),[9][10] and adopted by Maxwell in 1871 (explicitly attributing the term to Rankine).[11] The etymological origin corresponds here to an impossibility of transfer of energy as heat and of transfer of matter across the wall.
The Greek word ἀδιάβατος is formed from privative ἀ- ("not") and διαβατός, "passable", in turn deriving from διά ("through"), and βαῖνειν ("to walk, go, come").[12]
Conceptual significance in thermodynamic theory[edit]
The adiabatic process has been important for thermodynamics since its early days. It was important in the work of Joule, because it provided a way of nearly directly relating quantities of heat and work.
For a thermodynamic system that is enclosed by walls that do not allow mass transfer, energy can pass in and out only as heat or work. Thus a quantity of work can be related almost directly to an equivalent quantity of heat in a cycle of two limbs. The first is an isochoric adiabatic work process that adds to the system's internal energy. Then an isochoric and workless heat transfer returns the system to its original state. The first limb adds a definite amount of energy and the second removes it. Accordingly, Rankine measured quantity of heat in units of work, rather than as a calorimetric quantity .[13] In 1854, Rankine used a quantity that he called "the thermodynamic function" that later was called entropy, and at that time he wrote also of the "curve of no transmission of heat",[14] which he later called an adiabatic curve.[9] Besides it two isothermal limbs, Carnot's cycle has two adiabatic limbs.
For the foundations of thermodynamics, the conceptual importance of this was emphasized by Bryan,[15] by Carathéodory,[1] and by Born.[16] The reason is that calorimetry presupposes a type of temperature as already defined before the statement of the first law of thermodynamics, such as one based on empirical scales. Such a presupposition involves making the distinction between empirical temperature and absolute temperature. Rather, the definition of absolute thermodynamic temperature is best left till the second law is available as a conceptual basis.[17]
In the eighteenth century, the law of conservation of energy was yet to be fully formulated or established, and the nature of heat was debated. One approach to these problems was to regard heat, measured by calorimetry, as a primary substance that is conserved in quantity. By the middle of the nineteenth century, it was recognized as a form of energy, and the law of conservation of energy was thereby also recognized. The view that eventually established itself, and is currently regarded as right, is that the law of conservation of energy is a primary axiom, and that heat is to be analyzed as consequential. In this light, heat cannot be a component of the total energy of a single body because it is not a state variable, but, rather, is a variable that describes a process of transfer between two bodies. The adiabatic process is important because it is a logical ingredient of this current view.[17]
Divergent usages of the word adiabatic[edit]
This present article is written from the viewpoint of macroscopic thermodynamics, and the word adiabatic is used in this article in the traditional way of thermodynamics, introduced by Rankine. It is pointed out in the present article that, for example, if a compression of a gas is rapid, then there is little time for heat transfer to occur, even when the gas is not adiabatically isolated by a definite wall. In this sense, a rapid compression of a gas is sometimes approximately or loosely said to be adiabatic, though often far from isentropic, even when the gas is not adiabatically isolated by a definite wall.
Quantum mechanics and quantum statistical mechanics, however, use the word adiabatic in a very different sense, one that can at times seem almost opposite to the classical thermodynamic sense. In quantum theory, the word adiabatic can mean something perhaps near isentropic, or perhaps near quasi-static, but the usage of the word is very different between the two disciplines.
On the one hand, in quantum theory, if a perturbative element of compressive work is done almost infinitely slowly (that is to say quasi-statically), it is said to have been done adiabatically. The idea is that the shapes of the eigenfunctions change slowly and continuously, so that no quantum jump is triggered, and the change is virtually reversible. While the occupation numbers are unchanged, nevertheless there is change in the energy levels of one-to-one corresponding, pre- and post-compression, eigenstates. Thus a perturbative element of work has been done without heat transfer and without introduction of random change within the system. For example, Max Born writes "Actually, it is usually the 'adiabatic' case with which we have to do: i.e. the limiting case where the external force (or the reaction of the parts of the system on each other) acts very slowly. In this case, to a very high approximation
c 1 2 = 1 , c 2 2 = 0 , c 3 2 = 0 , . . . , {\displaystyle c_{1}^{2}=1,\,\,c_{2}^{2}=0,\,\,c_{3}^{2}=0,\,...\,,}
that is, there is no probability for a transition, and the system is in the initial state after cessation of the perturbation. Such a slow perturbation is therefore reversible, as it is classically."[18]
On the other hand, in quantum theory, if a perturbative element of compressive work is done rapidly, it randomly changes the occupation numbers of the eigenstates, as well as changing their shapes. In that theory, such a rapid change is said not to be adiabatic, and the contrary word diabatic is applied to it. One might guess that perhaps Clausius, if he were confronted with this, in the now-obsolete language he used in his day, would have said that "internal work" was done and that 'heat was generated though not transferred'.[citation needed]
In classical thermodynamics, such a rapid change would still be called adiabatic because the system is adiabatically isolated, and there is no transfer of energy as heat. The strong irreversibility of the change, due to viscosity or other entropy production, does not impinge on this classical usage.
Thus for a mass of gas, in macroscopic thermodynamics, words are so used that a compression is sometimes loosely or approximately said to be adiabatic if it is rapid enough to avoid heat transfer, even if the system is not adiabatically isolated. But in quantum statistical theory, a compression is not called adiabatic if it is rapid, even if the system is adiabatically isolated in the classical thermodynamic sense of the term. The words are used differently in the two disciplines, as stated just above.
See also[edit]
Cyclic process
First law of thermodynamics
Heat burst
Isobaric process
Isenthalpic process
Isentropic process
Isochoric process
Isothermal process
Polytropic process
Entropy (classical thermodynamics)
Quasistatic process
Total air temperature
Magnetic refrigeration
References[edit]
^ Jump up to: a b Carathéodory, C. (1909). "Untersuchungen über die Grundlagen der Thermodynamik". Mathematische Annalen. 67: 355–386. doi:10.1007/BF01450409. . A translation may be found here. Also a mostly reliable translation is to be found in Kestin, J. (1976). The Second Law of Thermodynamics. Stroudsburg, PA: Dowden, Hutchinson & Ross.
Jump up ^ Bailyn, M. (1994). A Survey of Thermodynamics. New York, NY: American Institute of Physics Press. p. 21. ISBN 0-88318-797-3.
^ Jump up to: a b c d Bailyn, M. (1994), pp. 52–53.
Jump up ^ Tisza, L. (1966). Generalized Thermodynamics. Cambridge, MA: MIT Press. p. 48. (adiabatic partitions inhibit the transfer of heat and mass)
Jump up ^ Münster, A. (1970), p. 48: "mass is an adiabatically inhibited variable."
Jump up ^ Münster, A. (1970). Classical Thermodynamics. Translated by Halberstadt, E. S. London: Wiley–Interscience. p. 45. ISBN 0-471-62430-6.
Jump up ^ Kavanagh, J. L.; Sparks, R. S. J. (2009). "Temperature changes in ascending kimberlite magmas". Earth and Planetary Science Letters. Elsevier. 286 (3–4): 404–413. Bibcode:2009E&PSL.286..404K. doi:10.1016/j.epsl.2009.07.011. Retrieved 18 February 2012.
Jump up ^ Adiabatic Processes
^ Jump up to: a b Rankine, W.J.McQ. (1866). On the theory of explosive gas engines, The Engineer, July 27, 1866; at page 467 of the reprint in Miscellaneous Scientific Papers, edited by W.J. Millar, 1881, Charles Griffin, London.
Jump up ^ Partington, J. R. (1949), An Advanced Treatise on Physical Chemistry., volume 1, Fundamental Principles. The Properties of Gases, London: Longmans, Green and Co., p. 122
Jump up ^ Maxwell, J. C. (1871), Theory of Heat (first ed.), London: Longmans, Green and Co., p. 129
Jump up ^ Liddell, H.G., Scott, R. (1940). A Greek-English Lexicon, Clarendon Press, Oxford UK.
Jump up ^ Rankine, W. J. M. (1854). "On the geometrical representation of the expansive action of heat, and theory of thermodynamic engines". Proc. Roy. Soc. 144: 115–175. Miscellaneous Scientific Papers p. 339
Jump up ^ Rankine, W. J. M. (1854). "On the geometrical representation of the expansive action of heat, and theory of thermodynamic engines". Proc. Roy. Soc. 144: 115–175. Miscellaneous Scientific Papers p. 341.
Jump up ^ Bryan, G. H. (1907). Thermodynamics. An Introductory Treatise dealing mainly with First Principles and their Direct Applications. Leipzig: B. G. Teubner.
Jump up ^ Born, M. (1949). "Natural Philosophy of Cause and Chance". London: Oxford University Press.
^ Jump up to: a b Bailyn, M. (1994). "Chapter 3". A Survey of Thermodynamics. New York, NY: American Institute of Physics. ISBN 0-88318-797-3.
Jump up ^ Born, M. (1927). "Physical aspects of quantum mechanics". Nature. 119: 354–357. Bibcode:1927Natur.119..354B. doi:10.1038/119354a0. (Translation by Robert Oppenheimer.)
General
Silbey, Robert J.; et al. (2004). Physical chemistry. Hoboken: Wiley. p. 55. ISBN 978-0-471-21504-2.
Broholm, Collin. "Adiabatic free expansion." Physics & Astronomy @ Johns Hopkins University. N.p., 26 Nov. 1997. Web. 14 Apr. *Nave, Carl Rod. "Adiabatic Processes." HyperPhysics. N.p., n.d. Web. 14 Apr. 2011. [1].
Thorngren, Dr. Jane R.. "Adiabatic Processes." Daphne – A Palomar College Web Server. N.p., 21 July 1995. Web. 14 Apr. 2011. [2].
External links[edit]
Media related to Adiabatic process at Wikimedia Commons
Article in HyperPhysics Encyclopaedia
Retrieved from "https://en.wikipedia.org/w/index.php?title=Adiabatic_process&oldid=803845095"
Categories:
Thermodynamic processes
Atmospheric thermodynamics
Entropy
Hidden categories:
Wikipedia articles needing clarification from March 2015
All articles with unsourced statements
Articles with unsourced statements from December 2015
Navigation menu
Personal tools
Not logged in
Talk
Contributions
Create account
Log in
Namespaces
Article
Talk
Variants
Views
Read
Edit
View history
More
Search
Navigation
Main page
Contents
Featured content
Current events
Random article
Donate to Wikipedia
Wikipedia store
Interaction
Help
About Wikipedia
Community portal
Recent changes
Contact page
Tools
What links here
Related changes
Upload file
Special pages
Permanent link
Page information
Wikidata item
Cite this page
Print/export
Create a book
Download as PDF
Printable version
In other projects
Wikimedia Commons
Languages
العربية
Azərbaycanca
Беларуская
Български
Bosanski
Català
Čeština
Dansk
Deutsch
Eesti
Ελληνικά
Español
Esperanto
Euskara
فارسی
Français
Gaeilge
Galego
한국어
Հայերեն
हिन्दी
Hrvatski
Bahasa Indonesia
Italiano
עברית
Қазақша
Latviešu
Lëtzebuergesch
Magyar
Македонски
Nederlands
日本語
Norsk
Norsk nynorsk
Oʻzbekcha/ўзбекча
Polski
Português
Română
Русский
Simple English
Slovenčina
Slovenščina
Српски / srpski
Srpskohrvatski / српскохрватски
Suomi
Svenska
தமிழ்
ไทย
Türkçe
Українська
Tiếng Việt
中文
Edit links
This page was last edited on 5 October 2017, at 00:37.
Text is available under the Creative Commons Attribution-ShareAlike License; additional terms may apply. By using this site, you agree to the Terms of Use and Privacy Policy. Wikipedia® is a registered trademark of the Wikimedia Foundation, Inc., a non-profit organization.
Privacy policy
About Wikipedia
Disclaimers
Contact Wikipedia
Developers
Cookie statement
Mobile view

key: html

type: local

value: div

attrs: id class

values: mw-page-base noprint

values: mw-head-base noprint

attrs: id class style

value: a

attrs: id class lang

values: firstHeading firstHeading en

values: siteSub noprint

values: jump-to-nav mw-jump

attrs: href title

value: th

values: padding:0.2em 0.4em 0.2em;font-size:145%;line-height:1.2em;padding-bottom:0.3em;border-bottom:1px solid #aaa;

value: tr

value: img

attrs: alt src width height srcset data-file-width data-file-height

value: td

values: padding:0.2em 0 0.4em;display:block;margin:0.3em 0 0.4em;

attrs: class id href

values: NavToggle NavToggle1 #

attrs: class style

value: li

values: font-size: 105%; padding: 0.2em 0px 0.4em; text-align: center; display: none;

values: float:right;clear:right;width:22.0em;margin:0 0 1.0em 1.0em;background:#f9f9f9;border:1px solid #aaa;padding:0.2em;border-spacing:0.4em 0;text-align:center;line-height:1.4em;font-size:88%;border-collapse:collapse; border-spacing:0px; border:none; width:100%; margin:0px; font-size:100%; clear:none; float:none;margin-top:0.4em;

values: Thermodynamic databases for pure substances

values: vertical-align: -0.338ex; width:3.481ex; height:1.676ex;

values: vertical-align: -0.338ex; width:1.647ex; height:2.176ex;

values: vertical-align: -0.338ex; width:2.838ex; height:2.343ex;

values: vertical-align: -0.338ex; width:2.074ex; height:2.176ex;

values: vertical-align: -0.338ex; width:2.975ex; height:2.343ex;

values: vertical-align: -0.671ex; width:6.27ex; height:2.509ex;

values: vertical-align: -0.338ex; width:1.173ex; height:2.176ex;

values: vertical-align: -0.338ex; width:3.126ex; height:2.343ex;

values: vertical-align: -0.338ex; width:1.798ex; height:2.176ex;

values: vertical-align: -0.671ex; width:2.508ex; height:2.676ex;

values: vertical-align: -0.338ex; width:3.962ex; height:1.676ex;

values: vertical-align: -0.838ex; width:7.975ex; height:2.843ex;

values: vertical-align: -0.838ex; width:18.369ex; height:2.843ex;

values: vertical-align: -0.838ex; width:18.982ex; height:2.843ex;

values: vertical-align: -0.838ex; width:18.729ex; height:2.843ex;

values: Philosophy of thermal and statistical physics

values: List of important publications in physics

values: An Experimental Enquiry Concerning the Source of the Heat which is Excited by Friction

values: On the Equilibrium of Heterogeneous Substances

values: padding:0.3em 0.4em 0.3em;font-weight:bold;border-top: 1px solid #aaa; border-bottom: 1px solid #aaa;

values: display:block; line-height:1em; margin:0 0.1em;

values: display:block; line-height:1em; margin:0 0.1em; border-top:1px solid;

values: display:inline-block; vertical-align:-0.5em; font-size:85%; text-align:center;

values: Edit section: Various applications of the adiabatic assumption

values: Edit section: Adiabatic heating and cooling

values:
/wiki/Diesel_engines
mw-redirect
Diesel engines

values:
/wiki/Earth%27s_atmosphere
mw-redirect
Earth's atmosphere

values:
/wiki/Orographic_lifting
mw-redirect
Orographic lifting

values:
/wiki/Adiabatic_demagnetization
mw-redirect
Adiabatic demagnetization

values:
/wiki/Expanding_universe
mw-redirect
Expanding universe

values:
/wiki/Hydrostatic_equation
mw-redirect
Hydrostatic equation

values: Edit section: Ideal gas (reversible process)

values:
/wiki/Reversible_adiabatic_process
mw-redirect
Reversible adiabatic process

attrs: alt src width height class srcset data-file-width data-file-height

values: vertical-align: -0.338ex; width:21.415ex; height:2.343ex;

values: P V^{n} = \operatorname{constant} \qquad

values: vertical-align: -2.505ex; width:18.309ex; height:6.176ex;

values:
/wiki/Specific_heat
mw-redirect
Specific heat

values:
/wiki/Adiabatic_index
mw-redirect
Adiabatic index

values: Degrees of freedom (physics and chemistry)

values: vertical-align: -0.338ex; width:19.803ex; height:2.676ex;

values: vertical-align: -0.338ex; width:17.197ex; height:3.843ex;

values: vertical-align: -0.338ex; width:18.682ex; height:2.676ex;

values: TV^{\gamma - 1} = \operatorname{constant}

values: Edit section: Example of adiabatic compression

values:
/wiki/Gasoline_engine
mw-redirect
Gasoline engine

values: vertical-align: -0.838ex; width:46.603ex; height:4.176ex;

values: vertical-align: -0.338ex; width:45.8ex; height:2.843ex;

values: vertical-align: -0.838ex; width:55.263ex; height:4.176ex;

values: vertical-align: -4.005ex; width:56.262ex; height:7.843ex;

values: vertical-align: -2.005ex; width:57.671ex; height:5.843ex;

values: vertical-align: -2.171ex; width:52.065ex; height:6.009ex;

values: Edit section: Adiabatic free expansion of a gas

values: Edit section: Derivation of P–V relation for adiabatic heating and cooling

values: vertical-align: -0.838ex; width:27.979ex; height:2.843ex;

values: \text{(1)} \qquad d U + \delta W = \delta Q = 0,

values: vertical-align: -0.838ex; width:20.086ex; height:2.843ex;

values: vertical-align: -0.838ex; width:19.532ex; height:2.843ex;

values:
/wiki/Universal_gas_constant
mw-redirect
Universal gas constant

values: vertical-align: -0.838ex; width:53.598ex; height:2.843ex;

values:
 \text{(4)} \qquad d U = \alpha n R \, dT
                  = \alpha \, d (P V)
                  = \alpha (P \, dV + V \, dP).

values: vertical-align: -0.671ex; width:26.933ex; height:2.509ex;

values: -P \, dV = \alpha P \, dV + \alpha V \, dP,

values: vertical-align: -0.838ex; width:24.769ex; height:2.843ex;

values: - (\alpha + 1) P \, dV = \alpha V \, dP,

values: vertical-align: -2.005ex; width:22.113ex; height:5.509ex;

values: -(\alpha + 1) {d V \over V} = \alpha {d P \over P}.

values: vertical-align: -2.505ex; width:29.798ex; height:6.176ex;

values: \ln \left( {P \over P_0} \right) = {-{\alpha + 1 \over \alpha}} \ln \left( {V \over V_0} \right).

values: vertical-align: -2.505ex; width:19.732ex; height:6.176ex;

values: \left( {P \over P_0} \right) = \left( {V \over V_0} \right)^{-{\gamma}},

values: vertical-align: -2.505ex; width:18.447ex; height:6.176ex;

values: \left( {P \over P_0} \right) = \left( {V_0 \over V} \right)^{\gamma}.

values: vertical-align: -2.505ex; width:19.349ex; height:6.176ex;

values: \left( {P \over P_0} \right) \left( {V \over V_0} \right)^{\gamma} = 1

values: vertical-align: -1.005ex; width:26.066ex; height:3.176ex;

values: P_0 V_0^{\gamma} = P V^\gamma = \operatorname{constant}.

values: Edit section: Derivation of P–T relation for adiabatic heating and cooling

values: vertical-align: -2.505ex; width:24.51ex; height:6.176ex;

values: vertical-align: -0.338ex; width:21.754ex; height:2.843ex;

values: P^{{(1-\gamma )}}T^{\gamma }=\operatorname {constant}.

values: Edit section: Derivation of discrete formula

values: vertical-align: -0.838ex; width:42.942ex; height:2.843ex;

values: \text{(1)} \qquad \Delta U = \alpha R nT_2 - \alpha R nT_1 = \alpha Rn \Delta T

values: vertical-align: -2.671ex; width:23.267ex; height:6.676ex;

values: vertical-align: -0.838ex; width:20.966ex; height:2.843ex;

values: vertical-align: -1.005ex; width:33.057ex; height:3.176ex;

values: \text{(4)} \qquad P V^\gamma = \text{constant} = P_1 V_1^\gamma

values: vertical-align: -2.505ex; width:15.267ex; height:6.176ex;

values: P = P_1 \left(\frac{V_1}{V} \right)^\gamma

values: vertical-align: -2.671ex; width:24.265ex; height:6.676ex;

values: W = \int_{V_1}^{V_2}P_1 \left(\frac{V_1}{V} \right)^\gamma\, dV

values: vertical-align: -2.338ex; width:25.215ex; height:6.843ex;

values: vertical-align: -1.838ex; width:30.88ex; height:4.843ex;

values: W = - \alpha P_1 V_1^{\gamma} \left( V_2^{1-\gamma} - V_1^{1-\gamma} \right)

values: vertical-align: -3.171ex; width:31.929ex; height:7.509ex;

values: W = - \alpha P_1 V_1 \left( \left( \frac{V_2}{V_1} \right)^{1-\gamma} - 1 \right)

values: vertical-align: -3.171ex; width:32.547ex; height:7.509ex;

values: W = - \alpha n R T_1 \left( \left( \frac{V_2}{V_1} \right)^{1-\gamma} - 1 \right)

values: vertical-align: -2.505ex; width:15.633ex; height:6.176ex;

values: vertical-align: -2.505ex; width:16.001ex; height:7.343ex;

values: vertical-align: -3.838ex; width:33.338ex; height:8.843ex;

values: W = - \alpha n R T_1 \left( \left( \frac{P_2}{P_1} \right)^{\frac{\gamma-1}{\gamma}} - 1 \right)

values: vertical-align: -3.838ex; width:43.292ex; height:8.843ex;

values: \alpha n R (T_2 - T_1) = \alpha n R T_1 \left( \left( \frac{P_2}{P_1} \right)^{\frac{\gamma-1}{\gamma}} - 1 \right)

values: vertical-align: -3.838ex; width:32.106ex; height:8.843ex;

values: T_2 - T_1 =  T_1 \left( \left( \frac{P_2}{P_1} \right)^{\frac{\gamma-1}{\gamma}} - 1 \right)

values: vertical-align: -2.505ex; width:24.781ex; height:7.509ex;

values: vertical-align: -2.505ex; width:18.327ex; height:7.509ex;

values: T_2 = T_1 \left( \frac{P_2}{P_1} \right)^{\frac{\gamma-1}{\gamma}}

values:
/wiki/Nernst%27s_theorem
mw-redirect
Nernst's theorem

values: No quantitative formula is identified in that article as Nernst's theorem, only a qualitative "Impossibility Principle" (March 2015)

values:
noprint Inline-Template
margin-left:0.1em; white-space:nowrap;

attrs: alt src width height data-file-width data-file-height

values:
/wiki/Privative_a
mw-redirect
Privative a

values: Edit section: Conceptual significance in thermodynamic theory

values: Edit section: Divergent usages of the word adiabatic

values: vertical-align: -1.005ex; width:28.328ex; height:3.176ex;

values: This claim needs references to reliable sources. (December 2015)

values:
noprint Inline-Template Template-Fact
white-space:nowrap;

values:
/wiki/Cyclic_process
mw-redirect
Cyclic process

values:
nofollow
external text
//doi.org/10.1007%2FBF01450409

values:
nofollow
external text
//doi.org/10.1016%2Fj.epsl.2009.07.011

values:
/wiki/J.R._Partington
mw-redirect
J.R. Partington

values:
nofollow
external text
//doi.org/10.1038%2F119354a0

values: -moz-column-width: 30em; -webkit-column-width: 30em; column-width: 30em; list-style-type: decimal;

values: Category:Wikipedia articles needing clarification from March 2015

values: Category:All articles with unsourced statements

values: Category:Articles with unsourced statements from December 2015

values: Discussion about edits from this IP address [ctrl-alt-n]

values: A list of edits made from this IP address [ctrl-alt-y]

values: You are encouraged to create an account and log in; however, it is not mandatory

values: You're encouraged to log in; however, it's not mandatory. [ctrl-alt-o]

values:
/wiki/Adiabatic_process
View the content page [ctrl-alt-c]
c

values: About the project, what you can do, where to find things

values: A list of recent changes in the wiki [ctrl-alt-r]

values: portal navigation p-interaction p-interaction-label

values: List of all English Wikipedia pages containing links to this page [ctrl-alt-j]

values: Recent changes in pages linked from this page [ctrl-alt-k]

values:
/wiki/Wikipedia:File_Upload_Wizard
Upload files [ctrl-alt-u]
u

values: A list of all special pages [ctrl-alt-q]

values: Permanent link to this revision of the page

values: Link to connected data repository item [ctrl-alt-g]

values: Printable version of this page [ctrl-alt-p]

values: portal navigation p-wikibase-otherprojects p-wikibase-otherprojects-label

values:
uls-settings-trigger
Language settings
0
button
true

values: عملية كظومة – Arabic

values: Адыябатны працэс – Belarusian

values: Адиабатен процес – Bulgarian

values: Αδιαβατική μεταβολή – Greek

values: فرایند بی‌دررو – Persian

values: Ադիաբատական գործընթաց – Armenian

values: रुद्धोष्म प्रक्रम – Hindi

values: תהליך אדיאבטי – Hebrew

values: Адиабаттық процестер – Kazakh

values: Адиабатски процес – Macedonian

values: Sistema adiabático (física) – Portuguese

values: Адиабатический процесс – Russian

values: interlanguage-link interwiki-ru badge-Q17437798 badge-goodarticle

values: Адијабатски процес – Serbian

values: மாறாவெப்பச் செயல்முறை – Tamil

values: กระบวนการอะเดียแบติก – Thai

values:
https://tr.wikipedia.org/wiki/Adyabatik
Adyabatik – Turkish
tr
tr
interlanguage-link-target

values: Адіабатичний процес – Ukrainian

values: /static/images/wikimedia-button-1.5x.png 1.5x, /static/images/wikimedia-button-2x.png 2x

values: /static/images/poweredby_mediawiki_132x47.png 1.5x, /static/images/poweredby_mediawiki_176x62.png 2x

values:
suggestions
display: none; font-size: 13px;

values: mediawiki ltr sitedir-ltr mw-hide-empty-elt ns-0 ns-subject page-Adiabatic_process rootpage-Adiabatic_process vector-nav-directionality skin-vector action-view


text:
The Devil in the White City
From Wikipedia, the free encyclopedia
Jump to navigation Jump to search
This article's tone or style may not reflect the encyclopedic tone used on Wikipedia. See Wikipedia's guide to writing better articles for suggestions. (April 2017) (Learn how and when to remove this template message)
The Devil in the White City
Cover of The Devil in the White City
Author
Erik Larson
Country
United States
Language
English
Genre
History, Historical Fiction
Publisher
Crown Publishers
Publication date
2003
Media type
Print (hardcover and paperback)
Pages
447
ISBN
0-609-60844-4
OCLC
54397544
The Devil in the White City: Murder, Magic, and Madness at the Fair That Changed America (Crown Publishers, ISBN 0-609-60844-4) is a 2003 historical non-fiction book by Erik Larson presented in a novelistic style. The book is based on real characters and events. It tells the story of the 1893 World’s Columbian Exposition in 1893 in Chicago from the viewpoint of the designers, including Daniel Burnham, and also tells the story of H. H. Holmes, a criminal figure in that same time.
Leonardo DiCaprio purchased the film rights in 2010.[1]
Contents
1 Plot
2 Burnham and the architects
3 Holmes and associates
4 Other figures
5 Film adaptation
6 Honors
7 References
8 External links
Plot[edit]
The book is set in Chicago in 1893, interweaving the true tales of Daniel H. Burnham, the architect behind the 1893 World's Fair, and Dr. H. H. Holmes, pharmacist and serial killer who lured his victims to their deaths in his elaborately constructed "Murder Castle". The Devil in the White City is divided into four parts, the first three happening in Chicago between 1890-1893. Part four of the book takes place in Philadelphia circa 1895. The story of Daniel Burnham, his building of the fair and the struggles he overcomes forms one plot line. The other, vividly different plot line is that of H.H. Holmes, a mentally unstable pharmacist/doctor who forms a plan to use an abandoned lot across from his pharmacy to lure in and kill multiple victims.
Burnham and the architects[edit]
Daniel Burnham: the chief architect behind the World's Columbian Exposition (also known as the Chicago World's Fair)
John Root: Burnham's partner
Charles B. Atwood: Burnham's head of design after Root's death
George Washington Gale Ferris Jr.: inventor of the Ferris wheel
Frank Millet
Louis Sullivan
Richard Morris Hunt
Charles McKim
Frederick Law Olmsted (designer of New York City's Central Park): landscape architect in charge of the World's Fair landscape.
George B. Post
Sophia Hayden Bennett
Holmes and associates[edit]
1895 newspaper image of Dr. Henry Howard Holmes
Herman Webster Mudgett (aka Dr. H. H. Holmes): a serial killer who used the fair to lure his victims to their deaths. Dr. Holmes had built his "World's Fair Hotel" complete with a gas chamber, dissection table, and a crematorium to dispose of the bodies. Holmes would have the skeletons of his victims removed and sell them for medical and scientific study.
Clara A. Lovering: Holmes's first wife
Myrta Z. Belknap: Holmes's second wife
Lucy Holmes: Holmes's daughter with Myrta
Georgiana Yoke: Holmes's third wife
Julia Smythe: employee and lover of Holmes; wife of Ned Connor
Ned Connor: employee of Holmes; husband of Julia Smythe
Emeline Cigrand: fiancée (and murder victim) of Holmes
Benjamin Pietzel: business associate (and murder victim) of Holmes
Carrie Pietzel: wife of Benjamin Pietzel
Howard, Nellie and Alice Pietzel: son and two daughters (respectively) of Benjamin and Carrie Pietzel.
Frank Geyer: detective in charge of finding Pietzel's children after Holmes was jailed for fraud
Thomas W. Barlow: assistant district attorney who prosecuted Holmes
Other figures[edit]
External media
Author Erik Larson
Audio
The Devil in the White City, Weekend Edition, National Public Radio, Larson interviewed by Scott Simon, 10:01, April 5, 2003
Video
Booknotes - The Devil in the White City, C-SPAN, 58:00, September 14, 2003.
Mayor Carter Harrison, Sr.: Mayor of Chicago who was assassinated on the last day of the fair
Patrick Prendergast: assassin who killed Mayor Harrison under the delusional belief that he had helped Harrison win re-election
Film adaptation[edit]
Leonardo DiCaprio purchased the film rights to the book in 2010; the movie is to be produced by Paramount Pictures, Stacey Sher and Michael Shamberg's Double Feature Films, and DiCaprio's own production company Appian Way Productions.[2] Writer Graham Moore was originally hired to adapt the book into a screenplay, but it was later reported that Billy Ray would be writing the script.[3] Martin Scorsese is signed to direct.[4]
Honors[edit]
2003 New York Times best seller (nonfiction)
2003 International Horror Guild Award (Nonfiction)
2003 San Francisco Chronicle Best Book of the Year
2003 National Book Award (Nonfiction), finalist
2003 CWA Gold Dagger for Non-Fiction, shortlist
2003 Great Lakes Book Award (Nonfiction), finalist
2004 Washington State Book Award
2004 Pacific Northwest Booksellers Association Award
2004 Edgar Award (Best Fact Crime), winner
2004 Book Sense Book of the Year Honor Book, winner
2009 ALA Outstanding Books for the College Bound (History & Cultures)
References[edit]
Jump up ^ "Leonardo DiCaprio secures rights to book of first serial killer in the US", The Guardian newspaper (November 2, 2010). Accessed Nov. 2, 2010.
Jump up ^ "Leonardo DiCaprio Teams With Martin Scorsese for 'Devil in the White City'". The Hollywood Reporter. Retrieved 2017-09-03.
Jump up ^ Fleming, Jr., Mike (December 16, 2011). "Warner Bros Sets Black List Top Scribe Graham Moore For 'Devil In The White City'; Leonardo DiCaprio To Play Serial Killer". Deadline Hollywood.
Jump up ^ McNary, Dave (August 10, 2015). "Leonardo DiCaprio, Martin Scorsese Reunite for 'Devil in the White City'". Variety. Retrieved January 15, 2017.
External links[edit]
Official Random House page for the book
Chicago Historical Society
Retrieved from "https://en.wikipedia.org/w/index.php?title=The_Devil_in_the_White_City&oldid=852665165"
Categories:
2003 books
Architecture books
History of Chicago
Non-fiction books about serial killers
World's Columbian Exposition
Hidden categories:
Wikipedia articles needing style editing from April 2017
All articles needing style editing
Navigation menu
Personal tools
Not logged in
Talk
Contributions
Create account
Log in
Namespaces
Article
Talk
Variants
Views
Read
Edit
View history
More
Search
Navigation
Main page
Contents
Featured content
Current events
Random article
Donate to Wikipedia
Wikipedia store
Interaction
Help
About Wikipedia
Community portal
Recent changes
Contact page
Tools
What links here
Related changes
Upload file
Special pages
Permanent link
Page information
Wikidata item
Cite this page
Print/export
Create a book
Download as PDF
Printable version
Languages
Français
Nederlands
中文
Edit links
This page was last edited on 30 July 2018, at 14:55 (UTC).
Text is available under the Creative Commons Attribution-ShareAlike License; additional terms may apply. By using this site, you agree to the Terms of Use and Privacy Policy. Wikipedia® is a registered trademark of the Wikimedia Foundation, Inc., a non-profit organization.
Privacy policy
About Wikipedia
Disclaimers
Contact Wikipedia
Developers
Cookie statement
Mobile view
Enable previews

values: mw-page-base noprint

values: mw-head-base noprint

value: i

values: firstHeading firstHeading en

values: siteSub noprint

attrs: class href

values: mw-jump-link #mw-head

values: mw-jump-link #p-search

value: b

value: span

value: small

value: tbody

values: plainlinks metadata ambox ambox-style ambox-Tone

values:
/wiki/Historical_Fiction
mw-redirect
Historical Fiction

values:
nofollow
external text
https://www.worldcat.org/oclc/54397544

values:
/wiki/Historical_non-fiction
mw-redirect
Historical non-fiction

values: checkbox button toctogglecheckbox toctogglecheckbox display:none

values: Edit section: Burnham and the architects

values:
/wiki/Sophia_Hayden_Bennett
mw-redirect
Sophia Hayden Bennett

values:
/wiki/National_Public_Radio
mw-redirect
National Public Radio

values: width:22em;width: 210px; float: right; clear: right; margin:0 0 1.0em 1.0em

values:
/wiki/Carter_Harrison,_Sr.
mw-redirect
Carter Harrison, Sr.

values:
/wiki/Double_Feature_Films
mw-redirect
Double Feature Films

values: Great Lakes Book Award (page does not exist)

values:
reflist mw-references-wrap
list-style-type: decimal;

values:
nofollow
http://www.chicagohs.org/
external text

values: Category:Non-fiction books about serial killers

values: Category:Wikipedia articles needing style editing from April 2017

values: Category:All articles needing style editing

values: Discussion about edits from this IP address [ctrl-alt-n]

values: A list of edits made from this IP address [ctrl-alt-y]

values: You are encouraged to create an account and log in; however, it is not mandatory

values: You're encouraged to log in; however, it's not mandatory. [ctrl-alt-o]

values:
/wiki/The_Devil_in_the_White_City
View the content page [ctrl-alt-c]
c

values: Discussion about the content page [ctrl-alt-t]

values: p-namespaces navigation vectorTabs p-namespaces-label

values:
p-variants
navigation
vectorMenu emptyPortlet
p-variants-label

values: Past revisions of this page [ctrl-alt-h]

values: p-views navigation vectorTabs p-views-label

values:
p-cactions
navigation
vectorMenu emptyPortlet
p-cactions-label

values:
mw-wiki-logo
/wiki/Main_Page
Visit the main page

values:
/wiki/Main_Page
Visit the main page [ctrl-alt-z]
z

values: Featured content – the best of Wikipedia

values: Find background information on current events

values:
/wiki/Special:Random
Load a random article [ctrl-alt-x]
x

values: portal navigation p-navigation p-navigation-label

values: Guidance on how to use and edit Wikipedia

values: About the project, what you can do, where to find things

values: A list of recent changes in the wiki [ctrl-alt-r]

values: portal navigation p-interaction p-interaction-label

values: Le Diable dans la ville blanche – French

values: 白城魔鬼：奇蹟與謀殺交織的博覽會 – Chinese

values: mediawiki ltr sitedir-ltr mw-hide-empty-elt ns-0 ns-subject page-The_Devil_in_the_White_City rootpage-The_Devil_in_the_White_City skin-vector action-view