Sulfur Dioxide and Oxides of Nitrogen

mho Dioxide and Oxides of NitrogenAlan ChanSince the Industrial revolution, in that respect were great increases in emissions of southward dioxide and particulates, deteriorating breeze qualities much dominantly in industrial cities but besides suburban beas and surrounds sloshed by. Two of the truly evident and dominant gases which ca substance ab utilisation much deterioration to our Earth accommodate some(prenominal) entropy dioxides and oxides of north which when reacted with body of water unblock virulent through biting rain much(prenominal) that SO2(g) + H2O(l) H2SO3(aq) and 2NO2(g) + H2O(l) HNO2(aq) + HNO3(aq).As shown, the reply between the sec dioxides and oxides of newton mixed bag blisteryic solutions when reacted with water as they release hydronium ions which indicate their doseic natures.There are much of both ( second dioxide and oxides of nitrogen) produced by nature and excessively industrially.Natural sources of mho dioxide lead to of the total sulfur dioxide released to the atmosphere where it reacts with water and causes acid raid gains from activities of geothermal hot springs and volcanoes and the cut down of organic matter, eg bushfires and decomposition of organic matter.Natural sources of the oxides of nitrogen, much(prenominal) as azotic oxide is lightning. These oxides of N2 are generated by lightning such that atmospheric oxygen and nitrogen gases accept to radiation pattern nitric oxideO2(g) + N2(g) 2NO(g)Then the nitric oxide slowly reacts with oxygen to form nitrogen dioxide2NO(g) + O2(g) 2NO2(g)The above is the major internal source of nitrogen dioxide.And finally, nitrous oxide is organize naturally by the action of certain bacteria on nitrogenous material in soils.Main industrial origins of sulfur dioxide come from the combustion of fossil fuels ( in particular in power plants and motor vehicles). Smelting of sulphide ores during conversions of minerals to metals (such as lead, coppe r and zinc) incineration of garbage petroleum refineries and industries using sulfur dioxide for production of sulphuric acid, production of paper, viands processing and sewage treatment all contribute to the oxide of sulfur in the air.The main industrial origins of oxides of nitrogen include the blown-up amounts of nitric oxide and nitrogen dioxide is combustion, both in stationary sources (power stations) and moving ones (motor vehicles). At amply temperatures in combustion chambers, oxygen and nitrogen from air flow to form nitric oxide, and thusly nitric oxide is slowly converted to nitrogen dioxide. Releases of nitrous oxides to the atmosphere include the increased uses of nitrogenous fertiliser which provides to a greater extent raw material for the bacteria.In terms of concern for their release into the environment, there are manyEffects of sulfur dioxide and nitrogen oxides on benevolent health ie sulfur dioxide irritates the respiratory system and causes breathing dif ficulties at concentrations as low as 1ppm. Effects of sulfur dioxide are exaggerated if particulates are cede also. Nitrogen dioxide irritates the respiratory tract and causes breathing botheration at concentration levels of about 3-5ppm and greater that causes tissue damage.Effects of sulfur dioxide and nitrogen oxides on the environment - formation of acid rainH2O(l) + SO2 H2SO3(g) and 2NO2(g) + H2O(l) HNO2(aq) + HNO3(aq) which contributes to the change magnitude tartness of lakes (aquatic animals hence), damage to forests (such as pine forests in parts of europium and North America), erosion of the marble and limestone of building surfaces and decorations and severe damage to plant especially around mine and smelter sites.Even though this has happened very slowly over a desire period of time, it is greatly concerning as these releases of gases testament only increase as industries and mining in token grows for the future. In the long term, these effects will become e ven more evident and greater and may be very difficult to deposit or even slow down.As mentioned before, the main contributor to high sulfur dioxide levels comes from the combustion of fossil fuels in power plants and motor vehicles. scorch and petroleum products contain sulfur, which combines with oxygen in air to form sulfur dioxide.S(s) + O2(g) SO2(g)Smelting of metal sulfides, eg copper sulphide, also produces sulfur dioxide.CuS(s) + O2(g) SO2(g) + Cu(s)Nitrogen undergoes combustion to form nitrogen monoxide and dinitrogen monoxide. Fossil fuels and biomass contain nitrogen (in proteins), so they also burn to produce these oxides.N2(g) + O2(g) 2NO(g)2N2(g) + O2(g) 2N2O(g)N2(g) + 2O2(g) 2NO2(g)Nitrogen monoxide burns to produce nitrogen dioxide.2NO(g) + O2(g) 2NO2(g)Although we may fall upon a lot about the effects of sulfur dioxides and oxides of nitrogen when reacted with water (acid rain), it is difficult to quantitatively state that oxides of sulfur and nitrogen have been increase in the atmosphere because these oxides occur in relatively low concentrations, such as 0.01ppm, and the instruments utilize to bankers bill these very low concentrations such as for SO2 have only been commercially avail satisfactory since the 1970s, so there is no reliable date for these gases before this time.However, analysis of gases assemble in polar ice core samples by the CSIRO and the Australian Antarctic Division showed that levels of N2O in the atmosphere has increased by about 10%.Also, the increased importunate of fossil fuels after the Industrial Revolution lead to a get up in oxides of sulfur, and evidence for this is the air quality of major industrial cities that deteriorated greatly. ex scarper in acid rain, which is mainly caused by acidic oxides of nitrogen and sulfur dissolved in water, eg SO2(g) + H2O(l) H2SO3(aq) which is acidic and 2NO2(g) + H2O(l) HNO2(aq) + HNO3(aq), of which both are acidic.This lead to the change magnitude damage to buildings, forests and aquatic organisms. Also, it was found that higher atmospheric concentrations of sulfur dioxide and nitrogen oxides in industrial areas than in non-industrial areas.Although we do not have ideal measures of atmospheric oxides of sulfur and nitrogen interpreted over a long period of time, there is enough indirect evidence to conclude that fundamental increases in atmospheric concentrations of oxides of sulfur and nitrogen have indeed taken devote, especially since industrial revolutionWith the aforementioned much dangerous particulates, sulfur dioxides and oxides of nitrogen especially when reacted with water forming acid rain, it is very important to use indicators to determine if levels of pH in the environment are at electronegative levels for organisms and growth of nature. A few of many every day uses of indicators include testing the pH (acidity/basicity) of water in aquariums and swimming pools, chemical wastes and soils.The testing of pH in the wate r of aquariums is extremely important as ocean life are sensitive to changes in their water. If the water becomes too acidic or alkaline/basic, organisms including fish and plants may not be able to survive. A few drops of indicator can be modeld in a sample of the water, or a pH paper already soaked in indicator can be used to measure the pH of the water.As swimming pools are wide used by the public, the pH of the water also needs to be monitored regularly as it needs to be kept at almost neutral to countermand skin and eye irritations. Adding chlorine (hypochlorite ion) is one way to control acidity and stop algae from growing. The testing of pH will be exchangeable to that of the testing of pH of water in aquarium. different than the public interactional environments, there are also chemical wastes which are produced industrially. The waste solutions from industries are tested before they are pumped into rivers or seas as they tend to be highly acidic. The pH of the wastes m ust be neutralised or they can be very harmful to the environment. The pH of chemical wastes is also measured by indicators, and substances are added to neutralise it.Many plants only plunk for a narrow pH range, so the soil has to be tested regularly to ensure its survival. A way of testing the pH is to place a neutral white powder (such as barium sulphate or calcium sulfate) on top of moist soil, and then place a few drops of universal indicator on it. The powder then absorbs the moisture from the soil allowing the colour of the indicator to be clearly seen.Other than sulfur dioxides and oxides of nitrogen when reacted with water which produces acid rain eg SO2(g) + H2O(l) H2SO3(aq) and 2NO2(g) + H2O(l) HNO2(aq) + HNO3(aq) and hence poignant bon ton and environment, there are many other naturally occurring acids and bases. rough commonly known naturally occurring acids include hydrochloric acid, acetic acid, citric acid and ascorbic acid.Hydrochloric acid HCl is produced by the glands in the lining of our stomachs to form an acidic environment for the breaking of complex food molecules by the enzymes.acetic acid CH3-COOH such that vinegar is about 4% solution of acetic acid and helps to relieve food. It is produced naturally by the bacterial action on alcohol in air.Citric acid C6H8O7 is widespread in plant and animal tissue, especially in citrus fruit. It is also formed in our bodies during cellular respiration.Ascorbic acid C6H8O6 also known as vitamin C is present in pert fruits and vegetables. It is involved in many metabolic pathways and has an important role in healing, blood cell formation and tissue growth.There are also many naturally occurring bases which may include ammonia, metallic oxides and carbonates.Ammonia NH3 is present in the stale urine of humans and other animals. It is also formed through the anaerobic decay of organic matter.Metallic Oxides such as iron(III) oxide, copper oxide and titanium (IV) oxides are insoluble and are so lid bases found in minerals.Carbonates such as calcium carbonate CaCO3 is found naturally as limestones.As shown, there are many naturally occurring acids and this has been used to our benefit in homes such as using them as food additives. Acids are used as food additives to improve the taste and/or to conduct them. This is because many bacteria cannot survive in acidic conditions and if the acid used is weak enough and not harmful for human consumption, this will allow food to last over a period of time. popular acids for this use include acetic acid, citric acid and phosphoric acid.Acetic acid(vinegar), phosphoric acid and citric acid is used to improve taste.Propanoic acid is used as a preservative in bread.Another advantage of having many acids is the use of them to make esters, which are compounds formed when alkanoic acids react with alkanols, or more generally, when carboxylic acids combine with alcohols. Esters have pleasant, fruity odours and occur widely in nature as pe rfumes and flavouring agents, hence its use as food additives, artificial fruit essences and in the manufacture of perfumes and cosmetics. As flavours, it is a combination of crude taste (sweet, salt, bitter) and odour, and it is these odours which contribute to flavours. It is easier to mass-produce these synthetic esters for use as flavours and perfumes in processed foods and cosmetics than to use naturally occurring ones and they represent weensy health hazards as they contain only substances that occur in natural flavours.Overall, our environment is acidic as shown through the need to test the pH in our waters and soils, which was caused by sulfur dioxide, oxides of nitrogen and particulates released into the atmosphere where it reacts with water releasing hydronium ions through acid rain. These acids are very damaging to our society and environment in the long term as discussed through their leaden pH levels in waters, soils and corrosion of buildings. However, advantages of having acids were also discussed being used to preserve foods, improve their tastes and using them as esters. The negative effects of acids may attend to outweigh the positive effects on a much wider exceed but there are nonetheless both many advantages alongside the disadvantages which benefit our society and are essential to our everyday lives.BibliographyExcel HSC interpersonal chemistry Jim Stamell Reprinted 2012 P69-70Conquering Chemistry HSC Course Fourth Edition Roland Smith P121-126,131-133. mental faculty 3 The Acidic Environment Theory Notes HSC Chemistry Johnson for Irwins Atoms 2003