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65-490: [REDACTED] Look up O₃ in Wiktionary, the free dictionary. O3 may refer to: O 3 , the molecular formula for ozone O , the ozonide anion O 3 , the 1993 debut album by the techno band Sunscreem O3 A Trilogy , a 2008 concept album trilogy by progressive metal band Dominici O3 star, in stellar classification, a subclass of type O stars O-3,

130-500: A Turkish motorway from Edirne to Istanbul Oskarshamn 3, unit 3 at Oskarshamn Nuclear Power Plant in Sweden O3 (album) , a 2008 album by Son of Dave LNER Class O3 , a class of British steam locomotives See also [ edit ] 03 (disambiguation) Ö3 , Austrian radio station 3O (disambiguation) [REDACTED] Topics referred to by the same term This disambiguation page lists articles associated with

195-500: A VOC whose atmospheric concentration has increased tremendously during the last century, contributes to ozone formation but on a global scale rather than in local or regional photochemical smog episodes. In situations where this exclusion of methane from the VOC group of substances is not obvious, the term Non-Methane VOC (NMVOC) is often used. Indoors ozone is produced by certain high-voltage electric devices (such as air ionizers ), and as

260-531: A by-product of other types of pollution. Outdoor air used for ventilation may have sufficient ozone to react with common indoor pollutants as well as skin oils and other common indoor air chemicals or surfaces. Particular concern is warranted when using "green" cleaning products based on citrus or terpene extracts, because these chemicals react very quickly with ozone to form toxic and irritating chemicals as well as fine and ultrafine particles . The chemical reactions involved in tropospheric ozone formation are

325-444: A constituent of smog . Its levels have increased significantly since the industrial revolution, as NOx gasses and VOCs are some of the byproducts of combustion. With more heat and sunlight in the summer months, more ozone is formed which is why regions often experience higher levels of pollution in the summer months. Although the same molecule, ground-level ozone can be harmful to human health, unlike stratospheric ozone that protects

390-499: A dark blue liquid . It is dangerous to allow this liquid to warm to its boiling point, because both concentrated gaseous ozone and liquid ozone can detonate. At temperatures below 80 K (−193.2 °C; −315.7 °F), it forms a violet-black solid . Most people can detect about 0.01 μmol/mol of ozone in air where it has a very specific sharp odour somewhat resembling chlorine bleach . Exposure of 0.1 to 1 μmol/mol produces headaches, burning eyes and causing irritation to

455-734: A destructive action". Schönbein himself reported that chest pains, irritation of the mucous membranes and difficulty breathing occurred as a result of inhaling ozone, and small mammals died. In 1911, Leonard Hill and Martin Flack stated in the Proceedings of the Royal Society B that ozone's healthful effects "have, by mere iteration, become part and parcel of common belief; and yet exact physiological evidence in favour of its good effects has been hitherto almost entirely wanting ... The only thoroughly well-ascertained knowledge concerning

520-484: A maximum concentration at the tropopause . About 90% of total ozone in the atmosphere is in the stratosphere, and 10% is in the troposphere. Although tropospheric ozone is less concentrated than stratospheric ozone, it is of concern because of its health effects . Ozone in the troposphere is considered a greenhouse gas , and as such contribute to global warming . as reported in IPCC reports. Actually, tropospheric ozone

585-456: A potent respiratory hazard and pollutant near ground level , a higher concentration in the ozone layer (from two to eight ppm) is beneficial, preventing damaging UV light from reaching the Earth's surface. The trivial name ozone is the most commonly used and preferred IUPAC name . The systematic names 2λ -trioxidiene and catena-trioxygen , valid IUPAC names, are constructed according to

650-404: A process called ozonolysis , giving alcohols, aldehydes, ketones, and carboxylic acids, depending on the second step of the workup. Ozone can also cleave alkynes to form an acid anhydride or diketone product. If the reaction is performed in the presence of water, the anhydride hydrolyzes to give two carboxylic acids . Usually ozonolysis is carried out in a solution of dichloromethane , at

715-464: A repercussion on climate, as well. Also, since climate change is causing sea ice to melt, what occurs is the sea ice releases molecular chlorine , which reacts with UV radiation to produce chlorine radicals. Because chlorine radicals are highly reactive, they can expedite the degradation of methane and tropospheric ozone and the oxidation of mercury to more toxic forms. Ozone production rises during heat waves , because plants absorb less ozone. It

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780-428: A series of complex cycles in which carbon monoxide and VOCs are oxidised to water vapour and carbon dioxide. The reactions involved in this process are illustrated here with CO but similar reactions occur for VOC as well. The oxidation begins with the reaction of CO with the hydroxyl radical ( OH). The radical intermediate formed by this reacts rapidly with oxygen to give a peroxy radical HO 2 An outline of

845-481: A spark and can occur in ozone concentrations of 10 wt% or higher. Ozone can also be produced from oxygen at the anode of an electrochemical cell. This reaction can create smaller quantities of ozone for research purposes. This can be observed as an unwanted reaction in a Hoffman gas apparatus during the electrolysis of water when the voltage is set above the necessary voltage. Ozone will oxidize most metals (except gold , platinum , and iridium ) to oxides of

910-853: A temperature of −78 °C. After a sequence of cleavage and rearrangement, an organic ozonide is formed. With reductive workup (e.g. zinc in acetic acid or dimethyl sulfide ), ketones and aldehydes will be formed, with oxidative workup (e.g. aqueous or alcoholic hydrogen peroxide ), carboxylic acids will be formed. All three atoms of ozone may also react, as in the reaction of tin(II) chloride with hydrochloric acid and ozone: Iodine perchlorate can be made by treating iodine dissolved in cold anhydrous perchloric acid with ozone: Ozone could also react with potassium iodide to give oxygen and iodine gas that can be titrated for quantitative determination: Ozone can be used for combustion reactions and combustible gases; ozone provides higher temperatures than burning in dioxygen ( O 2 ). The following

975-457: A warming climate alters humidity and wind conditions in some parts of the world, resulting in a reduction in the frequency of surface cyclones. Changes in air temperature and water content affect the air's chemistry and the rates of chemical reactions that create and remove ozone. Many chemical reaction rates increase with temperature and lead to increased ozone production. Climate change projections show that rising temperatures and water vapour in

1040-559: Is 116.78°. The central atom is sp ² hybridized with one lone pair. Ozone is a polar molecule with a dipole moment of 0.53  D . The molecule can be represented as a resonance hybrid with two contributing structures, each with a single bond on one side and double bond on the other. The arrangement possesses an overall bond order of 1.5 for both sides. It is isoelectronic with the nitrite anion . Naturally occurring ozone can be composed of substituted isotopes ( O, O, O). A cyclic form has been predicted but not observed. Ozone

1105-486: Is a trace gas in the troposphere (the lowest level of the Earth's atmosphere ), with an average concentration of 20–30 parts per billion by volume (ppbv), with close to 100 ppbv in polluted areas. Ozone is also an important constituent of the stratosphere , where the ozone layer (2 to 8 parts per million ozone) exists which is located between 10 and 50 kilometers above the Earth's surface. The troposphere extends from

1170-486: Is a reaction for the combustion of carbon subnitride which can also cause higher temperatures: Ozone can react at cryogenic temperatures. At 77 K (−196.2 °C; −321.1 °F), atomic hydrogen reacts with liquid ozone to form a hydrogen superoxide radical , which dimerizes : Ozone is a toxic substance, commonly found or generated in human environments (aircraft cabins, offices with photocopiers, laser printers, sterilizers...) and its catalytic decomposition

1235-551: Is among the most powerful oxidizing agents known, far stronger than O 2 . It is also unstable at high concentrations, decaying into ordinary diatomic oxygen. Its half-life varies with atmospheric conditions such as temperature, humidity, and air movement. Under laboratory conditions, the half-life will average ~1500 minutes (25 hours) in still air at room temperature (24 °C), zero humidity with zero air changes per hour. This reaction proceeds more rapidly with increasing temperature. Deflagration of ozone can be triggered by

1300-412: Is considered the third most important greenhouse gas after CO 2 and CH 4 , as indicated by estimates of its radiative forcing . Photochemical and chemical reactions involving ozone drive many of the chemical processes that occur in the troposphere by day and by night. At abnormally high concentrations (the largest source being emissions from combustion of fossil fuels ), it is a pollutant , and

1365-650: Is known to have the following health effects at concentrations common in urban air: It was observed in the 1990s that ground-level ozone can advance death by a few days in predisposed and vulnerable populations. A statistical study of 95 large urban communities in the United States found significant association between ozone levels and premature death. The study estimated that a one-third reduction in urban ozone concentrations would save roughly 4000 lives per year (Bell et al., 2004). Tropospheric ozone causes approximately 22,000 premature deaths per year in 25 countries in

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1430-457: Is measured in a column from the surface to the top of the atmosphere, and is dominated by high concentrations of stratospheric ozone. Typical units of measure for this purpose include the Dobson unit and millimoles per square meter (mmol/m ). The majority of tropospheric ozone formation occurs when nitrogen oxides (NOx), carbon monoxide (CO), and volatile organic compounds (VOCs), react in

1495-420: Is oxidized to lead(II) sulfate : Sulfuric acid can be produced from ozone, water and either elemental sulfur or sulfur dioxide : In the gas phase , ozone reacts with hydrogen sulfide to form sulfur dioxide: In an aqueous solution, however, two competing simultaneous reactions occur, one to produce elemental sulfur, and one to produce sulfuric acid : Alkenes can be oxidatively cleaved by ozone, in

1560-464: Is reminiscent of chlorine , and detectable by many people at concentrations of as little as 0.1  ppm in air. Ozone's O 3 structure was determined in 1865. The molecule was later proven to have a bent structure and to be weakly diamagnetic . In standard conditions , ozone is a pale blue gas that condenses at cryogenic temperatures to a dark blue liquid and finally a violet-black solid . Ozone's instability with regard to more common dioxygen

1625-446: Is specifically for the troposphere. LIDAR is a common ground-based remote sensing technique that uses laser to measure ozone. The Tropospheric Ozone Lidar Network (TOLNet) is the network of ozone observing lidars across the United States. Ozonesondes are a form of in situ , or local ozone measuring instruments. An ozonesonde is attached to a meteorological balloon, so that the instrument can directly measure ozone concentration at

1690-561: Is such that both concentrated gas and liquid ozone may decompose explosively at elevated temperatures, physical shock, or fast warming to the boiling point. It is therefore used commercially only in low concentrations. Ozone is a powerful oxidant (far more so than dioxygen) and has many industrial and consumer applications related to oxidation. This same high oxidizing potential, however, causes ozone to damage mucous and respiratory tissues in animals, and also tissues in plants, above concentrations of about 0.1 ppm . While this makes ozone

1755-432: Is then: The amount of ozone produced through these reactions in ambient air can be estimated using a modified Leighton relationship . The limit on these interrelated cycles producing ozone is the reaction of •OH with NO 2 to form nitric acid at high NOx levels. If nitrogen monoxide (NO) is instead present at very low levels in the atmosphere (less than 10 approximately ppt), the peroxy radicals (HO 2 • ) formed from

1820-407: Is very important to reduce pollution. This type of decomposition is the most widely used, especially with solid catalysts, and it has many advantages such as a higher conversion with a lower temperature. Furthermore, the product and the catalyst can be instantaneously separated, and this way the catalyst can be easily recovered without using any separation operation. Moreover, the most used materials in

1885-523: The pay grade for the following officer ranks in the U.S. uniformed services: Captain in the Army, Marine Corps, Air Force, and Space Force Lieutenant in the Navy, Coast Guard, Public Health Service Commissioned Corps, and NOAA Commissioned Officer Corps Haplogroup O3 (Y-DNA) , a Y-DNA Haplogroup Oldershaw O-3 , glider USS O-3 (SS-64) , a 1917 United States O class submarine Otoyol 3 ,

1950-493: The substitutive and additive nomenclatures , respectively. The name ozone derives from ozein (ὄζειν), the Greek neuter present participle for smell, referring to ozone's distinctive smell. In appropriate contexts, ozone can be viewed as trioxidane with two hydrogen atoms removed, and as such, trioxidanylidene may be used as a systematic name, according to substitutive nomenclature. By default, these names pay no regard to

2015-421: The 1920s, it was not certain whether small amounts of oxozone , O 4 , were also present in ozone samples due to the difficulty of applying analytical chemistry techniques to the explosive concentrated chemical. In 1923, Georg-Maria Schwab (working for his doctoral thesis under Ernst Hermann Riesenfeld ) was the first to successfully solidify ozone and perform accurate analysis which conclusively refuted

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2080-604: The Clean Air Act Amendments. In 2024, the Lung Association ranked Fort Collins 16th in the nation for high ozone days out of 228 metropolitan areas, 38 for 24-hour particle pollution out of 223 metropolitan areas, and 136 for annual particle pollution out of 204 metropolitan areas. In monitoring air quality, Boulder County , Colorado is classified by the EPA as part of a nine-county group that includes

2145-745: The Denver metro area and North Front Range region. This nine-county zone has recorded ozone levels that exceed the EPA's ozone standard since 2004. Attempts have been made under the Early Action Compact to bring the area's air quality up to the EPA's standards. However, since 2004 ozone pollution in Boulder County has regularly failed to meet federal standards set by the Environmental Protection Agency. The County of Boulder continues trying to alleviate some of

2210-492: The European Union. (WHO, 2008) The United States Environmental Protection Agency has developed an Air Quality index to help explain air pollution levels to the general public. 8-hour average ozone mole fractions of 76 to 95 nmol/mol are described as "Unhealthy for Sensitive Groups", 96 nmol/mol to 115 nmol/mol as unhealthy and 116 nmol/mol to 404 nmol/mol as very unhealthy. The EPA has designated over 300 counties of

2275-673: The United States, clustered around the most heavily populated areas (especially in California and the Northeast), as failing to comply with the National Ambient Air Quality Standards . In 2000, the Ozone Annex was added to the U.S.–Canada Air Quality Agreement . The Ozone Annex addresses transboundary air pollution that contributes to ground-level ozone, which contributes to smog. The main goal

2340-488: The atmosphere in the presence of sunlight, specifically the UV spectrum. NOx, CO, and VOCs are considered ozone precursors. Motor vehicle exhaust, industrial emissions, and chemical solvents are the major anthropogenic sources of these ozone precursors. Although the ozone precursors often originate in urban areas, winds can carry NOx hundreds of kilometers, causing ozone formation to occur in less populated regions as well. Methane,

2405-431: The atmosphere will likely increase surface ozone in polluted areas like the eastern United States. In particular, the degradation of the pollutant peroxyacetylnitrate (PAN), which is a significant reservoir species for long-range transport of ozone precursors, is accelerated by rising temperatures. As a result, as the temperature rises, the lifetime of PAN reduces, changing the long-range transport of ozone pollution. Second,

2470-436: The catalytic decomposition of ozone in the gas phase are noble metals like Pt, Rh or Pd and transition metals such as Mn, Co, Cu, Fe, Ni or Ag. There are two other possibilities for the ozone decomposition in gas phase: The first one is a thermal decomposition where the ozone can be decomposed using only the action of heat. The problem is that this type of decomposition is very slow with temperatures below 250 °C. However,

2535-494: The chain reaction that occurs in oxidation of CO, producing O 3 : The reaction begins with the oxidation of CO by the hydroxyl radical ( OH). The radical adduct (•HOCO) is unstable and reacts rapidly with oxygen to give a peroxy radical , HO 2 : Peroxy-radicals then go on to react with NO to produce NO 2 , which is photolysed by UV-A radiation to give a ground-state atomic oxygen, which then reacts with molecular oxygen to form ozone. The net reaction in this case

2600-436: The decomposition rate can be increased working with higher temperatures but this would involve a high energy cost. The second one is a photochemical decomposition, which consists of radiating ozone with ultraviolet radiation (UV) and it gives rise to oxygen and radical peroxide. The process of ozone decomposition is a complex reaction involving two elementary reactions that finally lead to molecular oxygen, and this means that

2665-443: The earth from excess UV radiation. Photolysis of ozone occurs at wavelengths below approximately 310–320 nanometres . This reaction initiates a chain of chemical reactions that remove carbon monoxide , methane , and other hydrocarbons from the atmosphere via oxidation . Therefore, the concentration of tropospheric ozone affects how long these compounds remain in the air. If the oxidation of carbon monoxide or methane occur in

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2730-422: The focus of the next cycle of scientific concern. In several parts of the northern hemisphere, tropospheric ozone levels have been rising. On various scales, this may have an impact on moisture levels, cloud volume and dispersion, precipitation, and atmospheric dynamics. A rising environment, on the other hand, favours ozone synthesis and accumulation in the atmosphere, owing to two physicochemical mechanisms. First,

2795-497: The gaseous chemical and named it "ozone", from the Greek word ozein ( ὄζειν ) meaning "to smell". For this reason, Schönbein is generally credited with the discovery of ozone. He also noted the similarity of ozone smell to the smell of phosphorus, and in 1844 proved that the product of reaction of white phosphorus with air is identical. A subsequent effort to call ozone "electrified oxygen" he ridiculed by proposing to call

2860-502: The ground up to a variable height of approximately 14 kilometers above sea level . Ozone is least concentrated in the ground layer (or planetary boundary layer ) of the troposphere. Ground-level or tropospheric ozone is created by chemical reactions between NOx gases (oxides of nitrogen produced by combustion) and volatile organic compounds (VOCs). The combination of these chemicals in the presence of sunlight form ozone. Its concentration increases as height above sea level increases, with

2925-868: The higher elevations beneficial because of their ozone content. "There is quite a different atmosphere [at higher elevation] with enough ozone to sustain the necessary energy [to work]", wrote naturalist Henry Henshaw , working in Hawaii. Seaside air was considered to be healthy because of its believed ozone content. The smell giving rise to this belief is in fact that of halogenated seaweed metabolites and dimethyl sulfide . Much of ozone's appeal seems to have resulted from its "fresh" smell, which evoked associations with purifying properties. Scientists noted its harmful effects. In 1873 James Dewar and John Gray McKendrick documented that frogs grew sluggish, birds gasped for breath, and rabbits' blood showed decreased levels of oxygen after exposure to "ozonized air", which "exercised

2990-683: The metals in their highest oxidation state . For example: Ozone also oxidizes nitric oxide to nitrogen dioxide : This reaction is accompanied by chemiluminescence . The NO 2 can be further oxidized to nitrate radical : The NO 3 formed can react with NO 2 to form dinitrogen pentoxide ( N 2 O 5 ). Solid nitronium perchlorate can be made from NO 2 , ClO 2 , and O 3 gases: Ozone does not react with ammonium salts , but it oxidizes ammonia to ammonium nitrate : Ozone reacts with carbon to form carbon dioxide , even at room temperature: Ozone oxidizes sulfides to sulfates . For example, lead(II) sulfide

3055-607: The oxidation will instead react with themselves to form peroxides , and not produce ozone. Health effects depend on ozone precursors, which is a group of pollutants, primarily generated during the combustion of fossil fuels. Ground-level ozone is created by nitrous oxides reacting with organic compounds in the presence of sunlight. There are many man-made sources of these organic compounds including vehicle and industrial emissions, along with several other sources. Reaction with daylight ultraviolet (UV) rays and these precursors create ground-level ozone pollution (tropospheric ozone). Ozone

3120-481: The oxozone hypothesis. Further hitherto unmeasured physical properties of pure concentrated ozone were determined by the Riesenfeld group in the 1920s. Ozone is a colourless or pale blue gas, slightly soluble in water and much more soluble in inert non-polar solvents such as carbon tetrachloride or fluorocarbons, in which it forms a blue solution. At 161 K (−112 °C; −170 °F), it condenses to form

3185-786: The oxygen from the first step is an intermediate because it participates as a reactant in the second step, which is a bimolecular reaction because there are two different reactants (ozone and oxygen) that give rise to one product, that corresponds to molecular oxygen in the gas phase. Step 1: Unimolecular reaction     O 3 ⟶ O 2 + O {\displaystyle {\ce {O3 -> O2 + O}}} Step 2: Bimolecular reaction     O 3 + O ⟶ 2 O 2 {\displaystyle {\ce {O3 + O -> 2 O2}}} Ground level ozone Ground-level ozone ( O 3 ), also known as surface-level ozone and tropospheric ozone ,

3250-444: The ozone decomposition follows a first order kinetics, and from the rate law above it can be determined that the partial order respect to molecular oxygen is -1 and respect to ozone is 2, therefore the global reaction order is 1. The ozone decomposition consists of two elementary steps: The first one corresponds to a unimolecular reaction because one only molecule of ozone decomposes into two products (molecular oxygen and oxygen). Then,

3315-536: The ozone from white phosphorus "phosphorized oxygen". The formula for ozone, O 3 , was not determined until 1865 by Jacques-Louis Soret and confirmed by Schönbein in 1867. For much of the second half of the 19th century and well into the 20th, ozone was considered a healthy component of the environment by naturalists and health-seekers. Beaumont, California , had as its official slogan "Beaumont: Zone of Ozone", as evidenced on postcards and Chamber of Commerce letterhead. Naturalists working outdoors often considered

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3380-401: The ozone pollution through programming that encourages people to drive less, and stop ozone polluting activities during the heat of the day. Ground-level ozone is both naturally occurring and anthropogenically formed. It is the primary constituent of urban smog, forming naturally as a secondary pollutant through photochemical reactions involving nitrogen oxides and volatile organic compounds in

3445-594: The physiological effect of ozone, so far attained, is that it causes irritation and œdema of the lungs, and death if inhaled in relatively strong concentration for any time." During World War I , ozone was tested at Queen Alexandra Military Hospital in London as a possible disinfectant for wounds. The gas was applied directly to wounds for as long as 15 minutes. This resulted in damage to both bacterial cells and human tissue. Other sanitizing techniques, such as irrigation with antiseptics , were found preferable. Until

3510-453: The presence of nitrogen monoxide (NO), this chain of reactions has a net product of ozone added to the system. Ozone in the atmosphere can be measured by remote sensing technology , or by in-situ monitoring technology. Because ozone absorbs light in the UV spectrum, the most common way to measure ozone is to measure how much of this light spectrum is absorbed in the atmosphere. Because

3575-418: The presence of bright sunshine with high temperatures. Regardless of whether it occurs naturally or is anthropogenically formed, the change in ozone concentrations in the upper troposphere will: As a result, photochemical smog pollution at the earth's surface, as well as stratospheric ozone depletion, have received a lot of attention in recent years. The disruptions in the "free troposphere" are likely to be

3640-453: The radicality of the ozone molecule. In an even more specific context, this can also name the non-radical singlet ground state, whereas the diradical state is named trioxidanediyl . Trioxidanediyl (or ozonide ) is used, non-systematically, to refer to the substituent group (-OOO-). Care should be taken to avoid confusing the name of the group for the context-specific name for the ozone given above. In 1785, Dutch chemist Martinus van Marum

3705-540: The reaction order and the rate law cannot be determined by the stoichiometry of the fitted equation. Overall reaction: 2 O 3 ⟶ 3 O 2 {\displaystyle {\ce {2 O3 -> 3 O2}}} Rate law (observed): V = K ⋅ [ O 3 ] 2 [ O 2 ] {\displaystyle V={\frac {K\cdot [{\ce {O3}}]^{2}}{[{\ce {O2}}]}}} It has been determined that

3770-420: The respiratory passages. Even low concentrations of ozone in air are very destructive to organic materials such as latex, plastics and animal lung tissue. The ozone molecule is diamagnetic. According to experimental evidence from microwave spectroscopy , ozone is a bent molecule, with C 2v symmetry (similar to the water molecule). The O–O distances are 127.2  pm (1.272  Å ). The O–O–O angle

3835-459: The same CO 2 radiative forcing that causes global warming would chill the stratosphere. This cooling is projected to result in a relative rise in ozone (O 3 ) depletion in the polar region, as well as an increase in the frequency of ozone holes. Ozone depletion, on the other hand, is a radiative forcing of the climate system. Two opposite effects exist: Reduced ozone causes the stratosphere to absorb less solar radiation, cooling it while warming

3900-505: The same title formed as a letter–number combination. If an internal link led you here, you may wish to change the link to point directly to the intended article. Retrieved from " https://en.wikipedia.org/w/index.php?title=O3&oldid=1218801437 " Category : Letter–number combination disambiguation pages Hidden categories: Short description is different from Wikidata All article disambiguation pages All disambiguation pages Ozone Ozone's odor

3965-439: The stratosphere has higher ozone concentration than the troposphere, it is important for remote sensing instruments to be able to determine altitude along with the concentration measurements. A total ozone mapping spectrometer-earth probe (TOMS-EP) aboard a satellite from NASA is an example of an ozone layer measuring satellite, and the tropospheric emission spectrometer (TES) is an example of an ozone measuring satellite that

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4030-402: The troposphere; as a result, the stratosphere emits less long-wave radiation downward, cooling the troposphere. The IPCC believes that "measured stratospheric O3 losses over the past two decades have generated a negative forcing of the surface-troposphere system" of around 0.15 0.10 watts per square metre (W/m ). Furthermore, rising air temperatures often improve ozone-forming processes, which has

4095-550: The varying altitudes along the balloon's upward path. The information collected from the instrument attached to the balloon is transmitted back using radiosonde technology. NOAA has worked to create a global network of tropospheric ozone measurements using ozonesondes. Ozone is also measured in air quality environmental monitoring networks. In these networks, in-situ ozone monitors based on ozone's UV-absorption properties are used to measure ppb-levels in ambient air. Total atmospheric ozone (sometimes seen in weather reports)

4160-399: Was conducting experiments involving electrical sparking above water when he noticed an unusual smell, which he attributed to the electrical reactions, failing to realize that he had in fact created ozone. A half century later, Christian Friedrich Schönbein noticed the same pungent odour and recognized it as the smell often following a bolt of lightning . In 1839, he succeeded in isolating

4225-644: Was to attain proper ozone air quality standards in both countries. The North Front Range of Colorado has been out of compliance with the Federal Air Quality standards. The U.S. EPA designated Fort Collins as part of the ozone non-attainment area in November 2007. This means that the U.S.’s environmental law considers the air quality to be worse than the National Ambient Air Quality Standards, which are defined in

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