Im sure by now we have all heard the disturbing information about our new Carbon laws and the Carbon footprint, or how the EPA sais that CO2 is bad for the Environment. You are killing the planet! ... B.S.
Recently we have suffered an increase on our utilities, the new tax accessed was 5% increase. our utility bill almost doubled. Let me narrow this... We pay $100 per mo for electricity, now 6% more is $105 add a $5 Administrative fee its $111 plus another 5% tax is $116. once they legaly max what they can tax you, they charge you fees. You end up paying their tax and yours.
Now WA, and OR, State have invented this Burn ban in the middle of winter! WTF? So every one that uses wood or pellet stoves to stay warm are SOL. The only exclusions to this ban is: if you have no other heating resources such as eletric, you may use the stoves.
This ban goes into effect 01/01/10.
The EPA sais that this should be done because of smog, and Carbon Dioxide.
I personally think its a way to force individuals to use utilities. increase the rates, people find alternative and cheaper resources, then convieniently create a ban preventing them from using these resources. The utility companies make a fortune, and you pay out the nose.
Saturday, December 12, 2009
Wednesday, December 9, 2009
Oxygen and Carbon dioxide
Oxygen (pronounced /ˈɒksɨdʒɨn/, OK-si-jin, from the Greek roots ὀξύς (oxys) (acid, literally "sharp", from the taste of acids) and -γενής (-genēs) (producer, literally begetter) is the element with atomic number 8 and represented by the symbol O. It is a member of the chalcogen group on the periodic table, and is a highly reactive nonmetallic period 2 element that readily forms compounds (notably oxides) with almost all other elements. At standard temperature and pressure two atoms of the element bind to form dioxygen, a colorless, odorless, tasteless diatomic gas with the formula O2. Oxygen is the third most abundant element in the universe by mass after hydrogen and helium[1] and the most abundant element by mass in the Earth's crust. Diatomic oxygen gas constitutes 20.9% of the volume of air.
All major classes of structural molecules in living organisms, such as proteins, carbohydrates, and fats, contain oxygen, as do the major inorganic compounds that comprise animal shells, teeth, and bone. Oxygen in the form of O2 is produced from water by cyanobacteria, algae and plants during photosynthesis and is used in cellular respiration for all complex life. Oxygen is toxic to obligately anaerobic organisms, which were the dominant form of early life on Earth until O2 began to accumulate in the atmosphere 2.5 billion years ago. Another form (allotrope) of oxygen, ozone (O3), helps protect the biosphere from ultraviolet radiation with the high-altitude ozone layer, but is a pollutant near the surface where it is a by-product of smog. At even higher low earth orbit altitudes atomic oxygen is a significant presence and a cause of erosion for spacecraft.
Oxygen was independently discovered by Carl Wilhelm Scheele, in Uppsala, in 1773 or earlier, and Joseph Priestley in Wiltshire, in 1774, but Priestley is often given priority because his publication came out in print first. The name oxygen was coined in 1777 by Antoine Lavoisier,[6] whose experiments with oxygen helped to discredit the then-popular phlogiston theory of combustion and corrosion. Oxygen is produced industrially by fractional distillation of liquefied air, use of zeolites to remove carbon dioxide and nitrogen from air, electrolysis of water and other means. Uses of oxygen include the production of steel, plastics and textiles; rocket propellant; oxygen therapy; and life support in aircraft, submarines, spaceflight and diving.
Contents
1 Characteristics
1.1 Structure
1.2 Allotropes
1.3 Physical properties
1.4 Isotopes and stellar origin
1.5 Occurrence
2 Biological role
2.1 Photosynthesis and respiration
2.2 Build-up in the atmosphere
3 History
3.1 Early experiments
3.2 Phlogiston theory
3.3 Discovery
3.4 Lavoisier's contribution
3.5 Later history
4 Industrial production
5 Applications
5.1 Medical
5.2 Life support and recreational use
5.3 Industrial
5.4 Scientific
6 Compounds
6.1 Oxides and other inorganic compounds
6.2 Organic compounds and biomolecules
7 Safety and Precautions
7.1 Toxicity
7.2 Combustion and other hazards
8 See also
9 Notes and citations
10 References
11 Further reading
12 External links
Photosynthesis and respiration
Photosynthesis splits water to liberate O2 and fixes CO2 into sugar
In nature, free oxygen is produced by the light-driven splitting of water during oxygenic photosynthesis. Green algae and cyanobacteria in marine environments provide about 70% of the free oxygen produced on earth and the rest is produced by terrestrial plants.[40]
A simplified overall formula for photosynthesis is:[41]
6 CO2 + 6 H2O + photons → C6H12O6 + 6 O2 (or simply carbon dioxide + water + sunlight → glucose + dioxygen)
Photolytic oxygen evolution occurs in the thylakoid membranes of photosynthetic organisms and requires the energy of four photons.[42] Many steps are involved, but the result is the formation of a proton gradient across the thylakoid membrane, which is used to synthesize ATP via photophosphorylation.[43] The O2 remaining after oxidation of the water molecule is released into the atmosphere.[44]
Molecular dioxygen, O2, is essential for cellular respiration in all aerobic organisms. Oxygen is used in mitochondria to help generate adenosine triphosphate (ATP) during oxidative phosphorylation. The reaction for aerobic respiration is essentially the reverse of photosynthesis and is simplified as:
C6H12O6 + 6 O2 → 6 CO2 + 6 H2O + 2880 kJ·mol-1
In vertebrates, O2 is diffused through membranes in the lungs and into red blood cells. Hemoglobin binds O2, changing its color from bluish red to bright red.[19][45] Other animals use hemocyanin (molluscs and some arthropods) or hemerythrin (spiders and lobsters).[36] A liter of blood can dissolve 200 cm3 of O2.[36]
Reactive oxygen species, such as superoxide ion (O−2) and hydrogen peroxide (H2O2), are dangerous by-products of oxygen use in organisms.[36] Parts of the immune system of higher organisms, however, create peroxide, superoxide, and singlet oxygen to destroy invading microbes. Reactive oxygen species also play an important role in the hypersensitive response of plants against pathogen attack.[43]
An adult human in rest inhales 1.8 to 2.4 grams of oxygen per minute.[46] This amounts to more than 6 billion tonnes of oxygen inhaled by humanity per year.[47]
You will notice after reading this and my previous post: epa-and-carbon-dioxide How natural and important these things are to life of all living creatures on our planet.
but our representatives rely on us to be stupid and not pay attention to what they are doing. They continue to write stupid laws and create rediculous mandates and uncomprehensable legislations... Swine Flu was a Bio-test, and Martial Law is around the corner. This Carbon footprint is a scam just like H1N1 to scare you and tax you into submission.
These actions are Terrorist actions.
Please read the Def of Terrorist via Dictionary and compare that to the protocols that our Presidential Administrations have been subjecting us to for the past 12 years but more relative the past 2 years.
Remove the HEAD the body will fall- Q: X = ? X is the head The head controls the admin. Obama and members of congress are only the arms and legs Who is moving Obama?
Your true enemy is not Obama, nor is it congress.
Your true enemy is not Military or Law enforcement.
To Capture the enemy you MUST follow the money. WallStreet, Globalists, World Bankers, Memebers of the N.W.O. W.H.O. Bilderburgers, Rothchilds, Rockefellers Etc.. Those who possess the largest sum of money control the Economy. Ignoring it WILL NOT make it go away!
All major classes of structural molecules in living organisms, such as proteins, carbohydrates, and fats, contain oxygen, as do the major inorganic compounds that comprise animal shells, teeth, and bone. Oxygen in the form of O2 is produced from water by cyanobacteria, algae and plants during photosynthesis and is used in cellular respiration for all complex life. Oxygen is toxic to obligately anaerobic organisms, which were the dominant form of early life on Earth until O2 began to accumulate in the atmosphere 2.5 billion years ago. Another form (allotrope) of oxygen, ozone (O3), helps protect the biosphere from ultraviolet radiation with the high-altitude ozone layer, but is a pollutant near the surface where it is a by-product of smog. At even higher low earth orbit altitudes atomic oxygen is a significant presence and a cause of erosion for spacecraft.
Oxygen was independently discovered by Carl Wilhelm Scheele, in Uppsala, in 1773 or earlier, and Joseph Priestley in Wiltshire, in 1774, but Priestley is often given priority because his publication came out in print first. The name oxygen was coined in 1777 by Antoine Lavoisier,[6] whose experiments with oxygen helped to discredit the then-popular phlogiston theory of combustion and corrosion. Oxygen is produced industrially by fractional distillation of liquefied air, use of zeolites to remove carbon dioxide and nitrogen from air, electrolysis of water and other means. Uses of oxygen include the production of steel, plastics and textiles; rocket propellant; oxygen therapy; and life support in aircraft, submarines, spaceflight and diving.
Contents
1 Characteristics
1.1 Structure
1.2 Allotropes
1.3 Physical properties
1.4 Isotopes and stellar origin
1.5 Occurrence
2 Biological role
2.1 Photosynthesis and respiration
2.2 Build-up in the atmosphere
3 History
3.1 Early experiments
3.2 Phlogiston theory
3.3 Discovery
3.4 Lavoisier's contribution
3.5 Later history
4 Industrial production
5 Applications
5.1 Medical
5.2 Life support and recreational use
5.3 Industrial
5.4 Scientific
6 Compounds
6.1 Oxides and other inorganic compounds
6.2 Organic compounds and biomolecules
7 Safety and Precautions
7.1 Toxicity
7.2 Combustion and other hazards
8 See also
9 Notes and citations
10 References
11 Further reading
12 External links
Photosynthesis and respiration
Photosynthesis splits water to liberate O2 and fixes CO2 into sugar
In nature, free oxygen is produced by the light-driven splitting of water during oxygenic photosynthesis. Green algae and cyanobacteria in marine environments provide about 70% of the free oxygen produced on earth and the rest is produced by terrestrial plants.[40]
A simplified overall formula for photosynthesis is:[41]
6 CO2 + 6 H2O + photons → C6H12O6 + 6 O2 (or simply carbon dioxide + water + sunlight → glucose + dioxygen)
Photolytic oxygen evolution occurs in the thylakoid membranes of photosynthetic organisms and requires the energy of four photons.[42] Many steps are involved, but the result is the formation of a proton gradient across the thylakoid membrane, which is used to synthesize ATP via photophosphorylation.[43] The O2 remaining after oxidation of the water molecule is released into the atmosphere.[44]
Molecular dioxygen, O2, is essential for cellular respiration in all aerobic organisms. Oxygen is used in mitochondria to help generate adenosine triphosphate (ATP) during oxidative phosphorylation. The reaction for aerobic respiration is essentially the reverse of photosynthesis and is simplified as:
C6H12O6 + 6 O2 → 6 CO2 + 6 H2O + 2880 kJ·mol-1
In vertebrates, O2 is diffused through membranes in the lungs and into red blood cells. Hemoglobin binds O2, changing its color from bluish red to bright red.[19][45] Other animals use hemocyanin (molluscs and some arthropods) or hemerythrin (spiders and lobsters).[36] A liter of blood can dissolve 200 cm3 of O2.[36]
Reactive oxygen species, such as superoxide ion (O−2) and hydrogen peroxide (H2O2), are dangerous by-products of oxygen use in organisms.[36] Parts of the immune system of higher organisms, however, create peroxide, superoxide, and singlet oxygen to destroy invading microbes. Reactive oxygen species also play an important role in the hypersensitive response of plants against pathogen attack.[43]
An adult human in rest inhales 1.8 to 2.4 grams of oxygen per minute.[46] This amounts to more than 6 billion tonnes of oxygen inhaled by humanity per year.[47]
You will notice after reading this and my previous post: epa-and-carbon-dioxide How natural and important these things are to life of all living creatures on our planet.
but our representatives rely on us to be stupid and not pay attention to what they are doing. They continue to write stupid laws and create rediculous mandates and uncomprehensable legislations... Swine Flu was a Bio-test, and Martial Law is around the corner. This Carbon footprint is a scam just like H1N1 to scare you and tax you into submission.
These actions are Terrorist actions.
Please read the Def of Terrorist via Dictionary and compare that to the protocols that our Presidential Administrations have been subjecting us to for the past 12 years but more relative the past 2 years.
Remove the HEAD the body will fall- Q: X = ? X is the head The head controls the admin. Obama and members of congress are only the arms and legs Who is moving Obama?
Your true enemy is not Obama, nor is it congress.
Your true enemy is not Military or Law enforcement.
To Capture the enemy you MUST follow the money. WallStreet, Globalists, World Bankers, Memebers of the N.W.O. W.H.O. Bilderburgers, Rothchilds, Rockefellers Etc.. Those who possess the largest sum of money control the Economy. Ignoring it WILL NOT make it go away!
The E.P.A. and Carbon Dioxide
The EPA sais Carbon Dioxide is Bad for the Environment. And our Representatives want to tax us on this "Carbon Foot print" in other words Taxing you to breath.
But here are the FACTS: http://en.wikipedia.org/wiki/Carbon_dioxide
Carbon dioxide (chemical formula CO2) is a chemical compound composed of two oxygen
atoms covalently bonded to a single carbon atom. It is a gas at standard temperature and pressure and exists in Earth's atmosphere in this state. CO2 is a trace gas being only 0.038% of the atmosphere.
Carbon dioxide is used by plants during photosynthesis to make sugars, which may either be consumed in respiration or used as the raw material to produce other organic compounds needed for plant growth and development. It is produced during respiration by plants, and by all animals, fungi and microorganisms that depend either directly or indirectly on plants for food. It is thus a major component of the carbon cycle. Carbon dioxide is generated as a by-product of the combustion of fossil fuels or the burning of vegetable matter, among other chemical processes. Small amounts of carbon dioxide are emitted from volcanoes and other geothermal processes such as hot springs and geysers and by the dissolution of carbonates in crustal rocks.
As of March 2009[update], carbon dioxide in the Earth's atmosphere is at a concentration of 387 ppm by volume.[1] Atmospheric concentrations of carbon dioxide fluctuate slightly with the change of the seasons, driven primarily by seasonal plant growth in the Northern Hemisphere. Concentrations of carbon dioxide fall during the northern spring and summer as plants consume the gas, and rise during the northern autumn and winter as plants go dormant, die and decay. Carbon dioxide is a greenhouse gas as it transmits visible light but absorbs strongly in the infrared and near-infrared.
Carbon dioxide has no liquid state at pressures below 5.1 atmospheres. At 1 atmosphere (near mean sea level pressure), the gas deposits directly to a solid at temperatures below −78 °C and the solid sublimes directly to a gas above −78 °C. In its solid state, carbon dioxide is commonly called dry ice.
CO2 is an acidic oxide: an aqueous solution turns litmus from blue to pink. It is the anhydride of carbonic acid, an acid which is unstable and is known to exist only in aqueous solution. In organisms carbonic acid is produced by the enzyme, carbonic anhydrase.
CO2 + H2O ⇌ H2CO3
CO2 is toxic in higher concentrations: 1% (10,000 ppm) will make some people feel drowsy.[2] Concentrations of 7% to 10% cause dizziness, headache, visual and hearing dysfunction, and unconsciousness within a few minutes to an hour.[3]
Contents[hide]
1 Chemical and physical properties
2 History of human understanding
3 Isolation and production
3.1 Industrial production
4 Uses
4.1 Drinks
4.2 Foods
4.3 Pneumatic systems
4.4 Fire extinguisher
4.5 Welding
4.6 Caffeine removal
4.7 Pharmaceutical and other chemical processing
4.8 Agricultural and biological applications
4.9 Lasers
4.10 Polymers and plastics
4.11 Oil recovery
4.12 As refrigerants
4.13 Coal bed methane recovery
4.14 Wine making
4.15 pH control
5 In the Earth's atmosphere
6 In the oceans
7 Biological role
7.1 Role in photosynthesis
7.2 Toxicity
7.3 Human physiology
8 See also
9 References
10 Further reading
11 External links
Chemical and physical properties
For more details on this topic, see Carbon dioxide (data page).
Carbon dioxide is colorless. At low concentrations, the gas is odorless. At higher concentrations it has a sharp, acidic odor. It will act as an asphyxiant and an irritant. When inhaled at concentrations much higher than usual atmospheric levels, it can produce a sour taste in the mouth and a stinging sensation in the nose and throat. These effects result from the gas dissolving in the mucous membranes and saliva, forming a weak solution of carbonic acid. This sensation can also occur during an attempt to stifle a burp after drinking a carbonated beverage. Amounts above 5,000 ppm are considered very unhealthy, and those above about 50,000 ppm (equal to 5% by volume) are considered dangerous to animal life.[4]
At standard temperature and pressure, the density of carbon dioxide is around 1.98 kg/m3, about 1.5 times that of air. The carbon dioxide molecule (O=C=O) contains two double bonds and has a linear shape. It has no electrical dipole, and as it is fully oxidized, it is moderately reactive and is non-flammable, but will support the combustion of metals such as magnesium.
At -78.51° C or -109.3° F, carbon dioxide changes directly from a solid phase to a gaseous phase through sublimation, or from gaseous to solid through deposition. Solid carbon dioxide is normally called "dry ice", a generic trademark. It was first observed in 1825 by the French chemist Charles Thilorier. Dry ice is commonly used as a cooling agent, and it is relatively inexpensive. A convenient property for this purpose is that solid carbon dioxide sublimes directly into the gas phase leaving no liquid. It can often be found in grocery stores and laboratories, and it is also used in the shipping industry. The largest non-cooling use for dry ice is blast cleaning.
Liquid carbon dioxide forms only at pressures above 5.1 atm; the triple point of carbon dioxide is about 518 kPa at -56.6 °C (See phase diagram, above). The critical point is 7.38 MPa at 31.1 °C.[5]
An alternative form of solid carbon dioxide, an amorphous glass-like form, is possible, although not at atmospheric pressure.[6] This form of glass, called carbonia, was produced by supercooling heated CO2 at extreme pressure (40–48 GPa or about 400,000 atmospheres) in a diamond anvil. This discovery confirmed the theory that carbon dioxide could exist in a glass state similar to other members of its elemental family, like silicon (silica glass) and germanium. Unlike silica and germania glasses, however, carbonia glass is not stable at normal pressures and reverts back to gas when pressure is released.
But here are the FACTS: http://en.wikipedia.org/wiki/Carbon_dioxide
Carbon dioxide (chemical formula CO2) is a chemical compound composed of two oxygen
atoms covalently bonded to a single carbon atom. It is a gas at standard temperature and pressure and exists in Earth's atmosphere in this state. CO2 is a trace gas being only 0.038% of the atmosphere.
Carbon dioxide is used by plants during photosynthesis to make sugars, which may either be consumed in respiration or used as the raw material to produce other organic compounds needed for plant growth and development. It is produced during respiration by plants, and by all animals, fungi and microorganisms that depend either directly or indirectly on plants for food. It is thus a major component of the carbon cycle. Carbon dioxide is generated as a by-product of the combustion of fossil fuels or the burning of vegetable matter, among other chemical processes. Small amounts of carbon dioxide are emitted from volcanoes and other geothermal processes such as hot springs and geysers and by the dissolution of carbonates in crustal rocks.
As of March 2009[update], carbon dioxide in the Earth's atmosphere is at a concentration of 387 ppm by volume.[1] Atmospheric concentrations of carbon dioxide fluctuate slightly with the change of the seasons, driven primarily by seasonal plant growth in the Northern Hemisphere. Concentrations of carbon dioxide fall during the northern spring and summer as plants consume the gas, and rise during the northern autumn and winter as plants go dormant, die and decay. Carbon dioxide is a greenhouse gas as it transmits visible light but absorbs strongly in the infrared and near-infrared.
Carbon dioxide has no liquid state at pressures below 5.1 atmospheres. At 1 atmosphere (near mean sea level pressure), the gas deposits directly to a solid at temperatures below −78 °C and the solid sublimes directly to a gas above −78 °C. In its solid state, carbon dioxide is commonly called dry ice.
CO2 is an acidic oxide: an aqueous solution turns litmus from blue to pink. It is the anhydride of carbonic acid, an acid which is unstable and is known to exist only in aqueous solution. In organisms carbonic acid is produced by the enzyme, carbonic anhydrase.
CO2 + H2O ⇌ H2CO3
CO2 is toxic in higher concentrations: 1% (10,000 ppm) will make some people feel drowsy.[2] Concentrations of 7% to 10% cause dizziness, headache, visual and hearing dysfunction, and unconsciousness within a few minutes to an hour.[3]
Contents[hide]
1 Chemical and physical properties
2 History of human understanding
3 Isolation and production
3.1 Industrial production
4 Uses
4.1 Drinks
4.2 Foods
4.3 Pneumatic systems
4.4 Fire extinguisher
4.5 Welding
4.6 Caffeine removal
4.7 Pharmaceutical and other chemical processing
4.8 Agricultural and biological applications
4.9 Lasers
4.10 Polymers and plastics
4.11 Oil recovery
4.12 As refrigerants
4.13 Coal bed methane recovery
4.14 Wine making
4.15 pH control
5 In the Earth's atmosphere
6 In the oceans
7 Biological role
7.1 Role in photosynthesis
7.2 Toxicity
7.3 Human physiology
8 See also
9 References
10 Further reading
11 External links
Chemical and physical properties
For more details on this topic, see Carbon dioxide (data page).
Carbon dioxide is colorless. At low concentrations, the gas is odorless. At higher concentrations it has a sharp, acidic odor. It will act as an asphyxiant and an irritant. When inhaled at concentrations much higher than usual atmospheric levels, it can produce a sour taste in the mouth and a stinging sensation in the nose and throat. These effects result from the gas dissolving in the mucous membranes and saliva, forming a weak solution of carbonic acid. This sensation can also occur during an attempt to stifle a burp after drinking a carbonated beverage. Amounts above 5,000 ppm are considered very unhealthy, and those above about 50,000 ppm (equal to 5% by volume) are considered dangerous to animal life.[4]
At standard temperature and pressure, the density of carbon dioxide is around 1.98 kg/m3, about 1.5 times that of air. The carbon dioxide molecule (O=C=O) contains two double bonds and has a linear shape. It has no electrical dipole, and as it is fully oxidized, it is moderately reactive and is non-flammable, but will support the combustion of metals such as magnesium.
At -78.51° C or -109.3° F, carbon dioxide changes directly from a solid phase to a gaseous phase through sublimation, or from gaseous to solid through deposition. Solid carbon dioxide is normally called "dry ice", a generic trademark. It was first observed in 1825 by the French chemist Charles Thilorier. Dry ice is commonly used as a cooling agent, and it is relatively inexpensive. A convenient property for this purpose is that solid carbon dioxide sublimes directly into the gas phase leaving no liquid. It can often be found in grocery stores and laboratories, and it is also used in the shipping industry. The largest non-cooling use for dry ice is blast cleaning.
Liquid carbon dioxide forms only at pressures above 5.1 atm; the triple point of carbon dioxide is about 518 kPa at -56.6 °C (See phase diagram, above). The critical point is 7.38 MPa at 31.1 °C.[5]
An alternative form of solid carbon dioxide, an amorphous glass-like form, is possible, although not at atmospheric pressure.[6] This form of glass, called carbonia, was produced by supercooling heated CO2 at extreme pressure (40–48 GPa or about 400,000 atmospheres) in a diamond anvil. This discovery confirmed the theory that carbon dioxide could exist in a glass state similar to other members of its elemental family, like silicon (silica glass) and germanium. Unlike silica and germania glasses, however, carbonia glass is not stable at normal pressures and reverts back to gas when pressure is released.
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