what is the main scource for ammonium nitrate?
814902
The main source for ammonium nitrate  is high-nitrogen fertilizers. Ammonium nitrate is industrially produced through an acid-base reaction of ammonia with nitric acid using anhydrous ammonia gas and concentrated nitric acid.  It is commonly used in agriculture, and it has also been used as an oxidizing agent in explosives, especially improvised explosive devices.♥
381305
ammonia is NH3, ammonium is NH4+.  \n\nAmmonia, if this is what you meant is inorganic, as it does not contain carbon.\n\nAmmonium can be either.  For example ammonium carbonate can be classed as organic, whereas ammonium chloride cannot.  Thinking again though I think carbon dioxide, carbonates etc are not classed as organic even though they contain carbon, so I don't think ammonium can be either.\n\nAmmonium nitrate/nitrite are undoubtedly inorganic.  The source of the material is irrelevent to its designation.\n\nHope this helps.
980281
Go to google or wikipidia and type in nitrogen regulators and tons of available info will pop up.....word....take care and good luck
626009
It makes them grow too fast and bloom.\n\nNitrates such as potassium nitrate (saltpeter) and ammonium nitrate are important nitrogen carriers in fertilizers; lesser amounts of calcium nitrate, magnesium nitrate and sodium nitrate are applied. These nitrates must be used quickly by plants because they are easily lost through leaching or denitrification by bacteria. Nitrate pollution has become an environmental issue in rivers and oceans.  High levels of nitrate in water can potentially cause the death of fish. Over 30PPM of nitrate can inhibit growth, impair the immune system, cause stress, and reduce energy levels. The principal pathway of entering aquatic systems is through surface runoff from agriculatural or landscaped areas which have received excess nitrate fertilizer. After entering the receiving waters nitrates also can induce algal blooms and eutrophication, causing other ecosystem modification in addition to the mortality effects stated above.
947511
no there isn't but it will last about 1-2 hours. ammonium nitrate and water it the reaction.
864694
Tin floride\nAmmonium sulfate\nMagnesium hydroxide\nBarium carbonate\nSodium sulfate\nCarbon chloride
875082
a. N2O4\nb.PCl5\nc.NF3\nd.S2Cl2
590452
(NH4)2 SO4  + (FeSO4)2 + 2H2O____(\nNH4)2SO4Fe2(SO4)3.24H2O\n\nAmmonium ferric sulphate
706351
KCl(aq) + AgNO3(aq)  --> KNO3(aq) + AgCl(s)\n\nNet ionic: Cl-(aq) + Ag+(aq)  --> AgCl(s)\n\nNa2SO4(aq) + Ba(NO3)2  --> 2NaNO3(aq) + BaSO4(s)\n\nnet ionic: SO4(-2)(aq) + Ba(+2)(aq)  --> BaSO4(s)
374732
i think it may be that SO2 will react with water to give sulphurous acid (H2SO3).  This is the common acid found in acid rain.  The concentrated ammonia may be to neutralise the acid should it be formed from the SO2 leak.\n\nPossibly anyway....
175298
this some link about u ask\nwww.basf.com/businesses/chemicals/pdfs/ammsulf.pdf\nwww.epa.gov/ttn/chief/ap42/ch08/final/c08s04.pdf\nwww.intlsteel.com/PDFs/ammoniumsulfate.pdf\nwww.bio.mtu.edu/campbell/ bl4820/lectures/lec5/482lec5.pdf\nwww.dakotagas.com/Products/MSDS/AMMSULMSDS.pdf
168132
Making of Fertilizers:\nBasically, fertilizers are made from ammonia..I will take you through four stages that are basically followed in order to make ammonia..mind it that I am talking about artificial fertilizers not natural ones like cow dung which is not man-made...Alright then,\n\nSTAGE 1: Haber Process\n\nThis is a reversible reaction and an exothermic reaction thats used to make Nitrogen and Hydrogen under low temperatures (about 750 degrees celcius) and high pressures (about 30 atmospheres with a catalyst of nickel)..The reaction for this equation is:\n\nN2 + 3H2 <---> 2NH3  (-92kJmol -1)\nNitrogen + Hydrogen <---> Ammonia\n\nNow we have got our ammoina..which is the raw material in the production of fertilizers..Lets move on to the 2nd step...\n\nSTAGE 2: Ammonia being converted into Nitrogen Monoxide..\n\nIn this stage, we are going to let ammonia (which we got from the Haber process) react with oxygen to form nitrogen monoxide and water..\nFor this reaction to take place..we need to apply heat and catalyst (not so sure of which catalyst). We need to apply 230 degrees celcius of heat for heating air and ammonia). So, here's the reaction equation for that:\n\n4NH3(g)  +  5O2(g)  --->  4NO(g)  +  6H20(l)\n\nWe've got our Nitrogen monoxide now..so let's move on..\n\n\nSTAGE 3: Converting Nitrogen Monoxide into Nitric Acid\n\nIn this reaction we are going to react Nitrogen Monoxide with Oxygen and Steam to obtain Nitric Acid like this:\n\n4NO(g) + 3O2(g) + 2H2O(g) ---> 4NO3(aq)\n\nSTAGE 4: Converting this Nitric Acid into Ammonium Nitrate\n\nSo, Now nitric acid is going to be reacted with Ammonia (from Haber Process again..) in an addition reaction. Ammonium Nitrate in this case, will be our fertilizer..So, this is the final stage.. <Phweks!!> Here we go:\n\nNH2(g)  +  HNO3(aq)  --->  NH4NO3(aq)\nAmmonia gas + Nitric Acid ---> Ammonium Nitrate!!!\n\n\nUses:\nThe ions these fertilizers contain enrichen the soil very much..Ions like the nitrates and phosphates are absorbed by the plants through osmosis from the soil..These ions then help the plant in various stuff like synthesising the chlorophyll molecule..some like nitrates are converted into plant proteins...\n\nOk, I guess I have exhausted everything I know about fertilizers...\n\nI really hope it was of some help for u...   :)
457812
Ammonia, baking soda.
1112820
Please restate, nitrogen 4 oxide N4O is not a common species or do you mean NO2?  For that go to\n\nhttp://www.epa.gov/ttn/emc/promgate.html
284896
One bit to add.  The only exception to this is the polyatomic ion, ammonium. (NH4+) It acts like the cation.
787213
Ammonium (NH4+) is a polyatomic ion.  That means that it is composed of a group of atoms that are covalently bound together.  As a whole, that group has a charge of +1.  \n\nBecause this group of atoms has a charge, it is an ion, and can form ionic bonds with other ions.  So in summary, ammonium itself is a covalent compound, but it is able to form ionic bonds with other substances.
341863
ammonium nitrate and aluminum hydroxide\n\nNH4NO3 + Al(OH)3\n\nThe aluminum hydroxide is insoluble when formed and will precipitate out of the solution as a solid powder.