Elements Unearthed Podcast Script and Notes

 

Overview

This page is for students working on the Air Separation video podcast. It will have the following features:

• Student notes from their individual research, edited into a draft script 
• Revisions by team members and the Subject Matter Expert
• Questions to ask the SME and others during the interviews at the sites
• Transcripts of video clips of the interviews and tours
• Final approval by the SME and company PR people 

 

Team

• Chris Cox: Air composition and chemicals 
• David Shelanskey: Processes for air separation 
• Brett Bertola: Uses of liquid nitrogen, oxygen, and argon
• Carlos Kidman: Hazards of liquid air

 

Timeline

• Initial Research: November, 2008 
• Detailed Research/Draft of Script: Dec. 15-16, 2008 
• Contact with SME: By Dec. 19, 2009
• Tour of Companies (Videotaping): Jan. 6-8, 2009
• Capture and Transcription/B-Roll Creation: Jan. 9-23, 2009 
• Final Script Complete with Approval of SME: Jan. 23, 2009 
• Video Editing - Draft: Jan. 26-30, 2009 
• Alpha Testing/Revisions: Feb. 2-6, 2009
• Beta Test/SME Checkoff: Feb. 9-13, 2009
• Export to Podcast/Add Metadata: Feb. 17-20
• Post to Blog, Upload to iTunes: Monday, Feb. 23

 

Editor's Comments:

 

 

 

Script Sections:

 

Lead In:

 

 

Air Composition:

 

A Brief History of the Atmosphere

 

   Five billion years ago, the Earth’s first atmosphere was composed of hydrogen and helium. Because of the planet’s lack of mass, most of the hydrogen and helium drifted into space.

 

   4.4 billion years ago, volcanic activity expelled additional gases – carbon dioxide, methane, ammonia, and water vapor – into the ancient atmosphere. This volcanic activity helped create the second atmosphere.

 

   The second atmosphere began to more fully develop 3.5 to 3.3 billion years ago as carbon dioxide became a major gas component, estimated to be as much as 96.5% of the atmosphere, followed by nitrogen and other gases. Early aquatic organisms – cyanobacteria, also known as blue/green algae – used the sun’s energy to split molecules of water and carbon dioxide and recombine them into organic compounds and oxygen, a process we know as photosynthesis. This early atmosphere was also much hotter than the modern one and extremely dense, about 100 times more than today’s. As it cooled a lot of the carbon dioxide dissolved into the oceans.

 

   Due to the increased production of oxygen, the atmosphere began to change again during the time between 2.7 and 2.2 billion years ago. After oxidizing the planet's surface, the extra oxygen began to accumulate in the atmosphere.

 

   As oxygen levels high in the atmosphere increased, sunlight energy was absorbed and double oxygen (O₂) atoms split forming single oxygen atoms. These free oxygen atoms combined with pairs to form O₃, known as ozone. This newly formed ozone would eventually creat a shielding layer protecting the earth’s surface from harmful ultraviolet radiation and allowing more complex organisms to form. Evolving plant life continued using carbon dioxide and created more oxygen, and, over time, excess carbon became locked in fossil fuels and sedimentary rock. This transformation of the earth’s atmosphere from an anoxic to oxic state is often referred to as the Great Oxygen Catastrophe as many carbon dioxide dependent organisms died off.

 

   By 600 million years ago, sufficient ozone was in the atmosphere to protect advanced biological life on the surface. Prior to this time life was restricted to the ocean. Oxygen became a key gas player and made up 10% of the atmosphere. The nitrogen content in the atmosphere also increased as oxygen molecules reacted with ammonia and released nitrogen gas. Bacteria also converted ammonia into nitrogen.

 

   250 to 200 million years ago, the Earth’s third atmosphere is established where oxygen makes up 35% of the gases. This oxygen-nitrogen atmosphere is the beginning of our modern atmosphere. In this new atmosphere, oxygen is consumed by inorganic chemical reactions, animals and bacteria. Carbon dioxide is produced by respiration, decomposition, and the oxidation of organic matter. Both carbon dioxide and oxygen levels are maintained primarily by biological activity and geologic forces which keep the present day atmosphere fairly steady.

 

The Modern Day Atmosphere

 

   Earth’s present day atmosphere has two main gases, nitrogen and oxygen, which together make up about 99% of the atmosphere. The remaining one percent consists of other gases – argon, carbon dioxide, neon, helium, methane, krypton, and hydrogen. Water vapor is also found in the atmosphere, making up 1% - 4% of the typical atmosphere near the surface.

 

   Compared to ancient carbon dioxide levels (up to 96.5%), this gas is less than .036% of the modern atmosphere. Hydrogen and helium are, respectively, .00005 and .0005 percent of the atmospheric gases.

 

Composition of Dry Atmosphere

 

Gas	Volume (ppmv parts per million by volume)
Nitrogen (N2)	780,840 ppmv (78.084%)
Oxygen (O2)	209,460 ppmv (20.946%)
Argon (Ar)	9,340 ppmv (0.934%)
Carbon Dioxide (CO2)	383 ppmv (0.0383% some references show as low as .0314%)
Neon (Ne)	18.18 ppmv (0.001818% some references round up to .00182%)
Helium (He)	5.24 ppmv (0.000524%)
Methane (CH4)	1.745 ppmv 0.0001745%, other references vary from .00015 to .0002%
Krypton (Kr)	1.14 ppmv (0.000114%)
Hydrogen (H2)	0.55 ppmv (0.000055%)

 

   Water vapor (H₂O) is approximately .040% over the full atmosphere, with it averaging between 1% to 4% near the surface.

 

Where Atmospheric Gases Come From

 

   Nitrogen makes up 78% of the atmosphere by volume. It is also found in protein matter of all life forms, in natural gas-hydrogen deposits, and other compounds. Most of the nitrogen in the atmosphere is the result of photolysis of ammonia released from volcanic activity over millennia. Oxygen reacts with ammonia producing nitrogen, and bacteria can also convert ammonia into nitrogen.

 

   While oxygen is only 21% of the atmosphere by volume, it is the most abundant of Earth elements. "Oxygen comprises 85% of [the] oceans and, as a component of most rocks and minerals, 46% of [Earth’s] solid crust. In addition it constitutes 60% of the human body." (http://praxair.com/praxair.nsf/AllContent/0D925DC826435C1E8525656200823F2E?OpenDocument&URLMenuBranch=EE3D8AD2DB9A09858525706F0027D95E). It also reacts with elements to form oxides and enhances combustion of materials. Oxygen is primarily created by photosynthesis, where plant life uses the sun’s energy to split molecules of water and carbon dioxide.

 

   Argon makes up 1.3 percent of the atmosphere by weight and 0.94 percent by volume, and it’s also found occluded in rocks. The decay of the potassium-40 in potassium containing minerals produces most of the naturally occurring argon. This gas then leaks into the atmosphere

 

   Carbon Dioxide was initially expelled into the atmosphere by volcanic out-gassing. While volcanic activity still produces alot of carbon dioxide, it is also produced by respiration, decomposition, and the oxidation of organic matter.

 

   Neon occurs in small quantities in the atmosphere where it has escaped after being trapped within rocks inside the Earth’s crust. It is more abundant in the universe than on Earth. It is about 3.5 times more plentiful than helium on Earth.

 

   Helium found on earth is the product of the decay of radioactive materials. It doesn’t accumulate in large quantities because the Earth’s gravity is too low and helium gradually escapes into space. It is the second most abundant element in the universe, making up about 23% of the universe’s mass.

 

   Methane is a primary component of natural gas, which contains 50 to 90 percent methane. It is also produced by “destructive distillation [http://www.answers.com/topic/destructive-distillation] of bituminous coal [http://en.wikipedia.org/wiki/Bituminous_coal] and by coal carbonization [http://en.wikipedia.org/wiki/Carbonization].” (http://www.c-f-c.com/specgas_products/methane.htm)

 

   Traces of krypton are found in certain minerals and meteorites. Although it is also formed by nuclear fission of uranium, most the atmospheric krypton is the result of the gas leaking into the atmosphere from minerals in the Earth.

 

   Hydrogen is the most abundant element in the universe constituting about 75% of the universe’s mass, and on Earth it is the 9^th most abundant. It is found in the form of compounds, combined with carbon and other elements, in all animal and vegetable substances. It also found in hydrocarbons and makes up about 11% of the mass of sea water (http://www.c-f-c.com/specgas_products/hydrogen.htm). Atmospheric hydrogen content remains low because of the continual escape of the gas into space.

 

   Water Vapor was initially injected into the atmosphere by volcanic activity during the formation of the second atmosphere. Today most water vapor in the atmosphere is the result of the water cycle, also known as the hydrologic cycle. In this cycle heat from the sun evaporates water and the vapor enters the atmosphere, from which it cools and precipitates back to the surface.

 

Atmospheric Composition Table References

 

http://en.wikipedia.org/wiki/earth%27s_atmosphere

 

http://www.ux1.eiu.edu/~cfjps/1400/atmos_origin.html , (figure and table on website attributed to Lutgens and Tarbuck, The Atmosphere, 8^th Edition)

 

http://www.physlink.com/reference/AirComposition.cfm

 

References

 

Wikipedia, http://www.wikipedia.org,  http://en.wikipedia.org/wiki/earth%27s_atmosphere

 

WiseGEEK, http://www.wisegeek.com/what-is-the-history-of-the-earths-atmosphere.htm

 

Georgia Louviere, http://teachertech.rice.edu/Participants/louviere/struct.html, http://teachertech.rice.edu/Participants/louviere/comp.html, http://teachertech.rice.edu/Participants/louviere/history.html

 

Eastern Illinois University, http://www.ux1.eiu.edu/~cfjps/1400/atmos_origin.html

 

Manchester Metropolitan University, http://www.ace.mmu.ac.uk/eae/Atmosphere/Older/Thermosphere.html

 

CFC StarTec LLC, http://www.c-f-c.com

 

Praxair,http://www.praxair.com

 

 

 

 

Uses of Air Components:

 

   Liquid nitrogen is used to freeze things fast or to keep them frozen. Trucks use it for transporting food or other goods that need to be kept cold. Another way it is used is for Subzero ice cream. They mix the milk and cream right in front of you. They blast the mixture with liquid nitrogen and freeze the ice cream right in front of you in seconds. It is as fresh as you can get. It’s pretty good to. We might have to check the place out and film there for an example in the movie.         

 

   Liquid nitrogen is used for medical purposes as well for keeping embryonic stem cells frozen so they can later be used for research. There is even a company that when you die they will preserve your body in liquid nitrogen so if technology every can bring people back from the dead they will unfreeze you. I think that is crazy but people do it.

 

   It is used for medical things as well. Doctors use it to freeze of warts, moles, acne and other thing on the skin. It is used as a coolant to make sure big machines that are constantly running don’t over heat.

 

  There are many cool experiments you can do with liquid nitrogen. Some are very dangerous. But some look really cool and we should try some of them out to put in the movie. For example there is one of a spinning ping pong ball, you can make a levitating magnet, and it can suck the helium out of o balloon.  If you look on you tube there are many videos of experiments we could try. They are very simple.

 

Here are some links to videos:

http://www.youtube.com/watch?v=MvatmPlKOYQ&NR=1 This is the spinnig ping pong ball

http://www.youtube.com/watch?v=Olt9-r6IXz0 This is the balloon

http://www.youtube.com/watch?v=c3asSdngzLs&feature=related This is the floating magnet

 

   Photo by Jeffrey M. Vinocur; 4/21/06

 

 

Air Liquification and Distillation Processes:

 

 

   In order to attain liquid oxygen, argon and nitrogen, you need to take air and put it thought a distillation process. Distillation is a method of separating based on differences in their volatilities in a boiling liquid mixture. Distillation is a unit operation, or a physical separation process, and not a chemical reaction.

 

Commercially, distillation has a number of uses. It is used to separate crude oil into more fractions for specific uses such as transport, power generation, and heating. Water is distilled to remove impurities, such as salt from seawater. Air is distilled to separate its components—notably oxygen, nitrogen, and argon—for industrial use.

 

 

   How does this works? 

 

   The processes for most distillation methods are:

 

* Intake a large volume of atmosphere air.

* Filtering and cleaning out all of the undesired materials (solid, liquid and other extraneous materials).

* Compressing the air, cool it, and then expand it rapidly. This tremendous expansion of the air causes a huge drop in the air temperature by releasing heats.

* Removing the water vapor (H2O) and carbon dioxide (CO2).

* The remaining parts of air is then cool to somewhere around -300 F,

* It will then enter a distillation chamber (tower) where it is heated to differ boiling point for oxygen, argon, and nitrogen. The elements turn into vapor, float to trays base on the elements boiling point.  Oxygen (-183 degrees C) goes to the lower end of the tower, argon (-186 degrees C) in the middle, and nitrogen (-196 degrees C) to the higher end of the tower. The vapors are then cooled to liquid on the trays and transfer to storage tanks

   There are many different methods being employed to attain the same result in the industry today. 

Trays inside distillation tower

 

Questions to be asked:

- What method is being used at this plant? 

- How are the finished products stored? 

- What, if anything, needs to go through the process more than once?

 

http://en.wikipedia.org/wiki/Fractionating_column 

http://www.uigi.com/cryodist.html 

http://www.industrialgasplants.com/cryogenic-air-separation.html

http://www.process-cooling.com/CDA/Archives/ebde76fc3c5b7010VgnVCM100000f932a8c0

 

 

Hazards of Liquid Air:

 

     “Cryogenic” means  “producing, or relating to, low temperatures.” All cryogenic liquids are extremely cold. Most having a boiling point below -150 degrees Celsius (-238 degrees Fahrenheit). At normal temperatures and pressures, they are all a gas. All cryogenic liquids have to common properties: they are extremely cold, and small amounts of liquid can expand into very large volumes of gas. They are classified as “compressed gases” because they must undergo a combination of a large amount of temperature depression, and pressure, “compressing” the gas into a liquid.

 

   There are three groups of health hazards that are associated with cryogenic liquids: extreme cold, asphyxiation, and toxicity.

 

Extreme Cold Hazard:

 

   Cryogenic liquids are so cold that any brief exposure can damage delicate tissues such as the eyes. Any further exposure or contact can cause frostbite. The skin appears a waxy yellow. There is no initial pain, but there is intense pain when the frozen tissue thaws. If the skin contacts with any surface that has been cooled by cryogenic liquids, it can stick and be torn when pulled away. Breathing of extremely cold air can damage the lungs.

 

Asphyxiation Hazard:

 

  The gases that are formed by the liquids are heavier than oxygen and do not disperse or expand. Thus, they accumulate and displace air. Depleting of oxygen can cause suffocation and/or asphyxiation which can lead to death. The risk is higher in enclosed rooms. When the liquids evaporate, they make large amounts of gas, creating a health hazard.

 

Toxic Hazards:

 

    Cyrogenic liquids can release large amounts of toxic gas. Any inhalation (or in some cases just any contact) can cause intoxication, permanent damage, or even death.

      

There are three types of cryogens:

 

   Inert Gases: Inert gases do not react chemically to any great extent. They do not burn or support combustion. (Ex: nitrogen, helium, neon, argon and krypton.)

 

   Flammable Gases: Some cryogenic liquids produce a gas that can burn in air. (Ex: hydrogen, methane, and liquefied natural gas.)

 

   Oxygen: Many materials are considered as non-combustible can burn in the presence of liquid oxygen. Organic materials can react explosively with liquid oxygen. The hazards and handling precautions of liquid oxygen must be considered separately from other cryogenic liquids.

 

Questions:

1. What is the safest way to contain, and then transport these cyrogens?
2. How do you contain a rapid expansion of the liquid if the temperature shifts dramatically at a very rapid rate?
3. What would happen if you solidified the liquids?

 

  <http://www.ccohs.ca/oshanswers/chemicals/cryogenic/cryogen1.html>

 

 

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