what is the manufacture of ammonia and its salts?
822172
the Haber process is used for the manufacture of ammonia. It's named after the German scientist, Fritz Haber, who discovered it. u can check out this site:\n\nhttp://www.ausetute.com.au/haberpro.html
696413
1. Diamonds and graphite are a form of carbon.\n\n2. Ammonia is made using the Haber process.\n\nLook here for details\nhttp://www.ausetute.com.au/haberpro.html\n\nIt is used as a fertilizer, explosives, chemicals\n\n3. Ozone in the upper atmosphere act as a filter for UV rays, which are harmful to life.\n\n4. Halogens have an outer orbital that will be filled if they add one electron\n\n5. Noble gases have an outer orbital that is completelly filled.
839202
Last week I wrote a detailed answer to a very similar question.  Try looking at that first, and follow the same procedure for your ammonia oxidation question.
319335
It's liquid hydrogen and oxygen.  I imagine they just make it in a factory by cooling down those gases to very low temperatures.
1033934
Nitric acid is made by mixing nitrogen dioxide (NO2) with water. Creating a very pure nitric acid usually involves distillation with sulfuric acid, as nitric acid forms an azeotrope with water with a composition of 68% nitric acid and 32% water. Commercial grade nitric acid solutions are usually between 52% and 68% nitric acid. Commercial production of nitric acid is via the Ostwald process after Wilhelm Ostwald.\n\nNitric acid can be made from Copper(II) nitrate or by reacting 200 g of potassium nitrate (KNO3) in 106 ml of 96% sulfuric acid (H2SO4), and distilling this mixture at nitric acid's boiling point of 83 °C until only a white crystalline mass, potassium hydrogen sulfate (KHSO4), remains in the reaction vessel. The obtained red fuming nitric acid may be converted to the white nitric acid. Note that in a laboratory setting, it is necessary to use all-glass equipment, ideally a one-piece retort, because nitric acid attacks cork and rubber, and leaks can be extremely dangerous.\n\nThe dissolved NOx are readily removed using reduced pressure at room temperature (10-30 min at 200 mmHg or 27 kPa). Obtained white fuming nitric acid has density 1.51 g/cm³. This procedure can also be performed under reduced pressure and temperature in one step in order to produce less nitrogen dioxide gas.\n\nThe acid can also be synthesized by oxidizing ammonia, but the product is diluted by the water also formed as part of the reaction. However, this synthesization method is important in producing ammonium nitrate from ammonia derived from the Haber process, because the final product can be produced from nitrogen, hydrogen, and oxygen as the sole feedstocks.\n\nWhite fuming nitric acid, also called 100% nitric acid or WFNA, is very close to the anhydrous nitric acid product. One specification for white fuming nitric acid is that it has a maximum of 2 % water and a maximum of 0.5 % dissolved NO2. Red fuming nitric acid, or RFNA, contains substantial quantities of dissolved nitrogen dioxide (NO2) leaving the solution with a reddish-brown color. One formulation of RFNA specifies a minimum of 17% NO2, another specifies 13% NO2. In either event, an inhibited fuming nitric acid (either IWFNA, or IRFNA) can be made by the addition of 0.6 to 0.7% hydrogen fluoride, HF. This fluoride is added for corrosion resistance in metal tanks (the fluoride creates a metal fluoride layer that protects the metal)
185385
Basically you need to oxidise ammonia and then  adsorb the gases into water.\n\nSee the site below.
711078
Acid used is ethanoic acid, hence the salt produced is ethanoate (in this case, the exact salt is sodium ethanoate CH3COONa). Since this is an acid-base titration, products are salt and water.\nCH3COOH + NaOH --> CH3COONa + H2O
1104610
Ammonia is shipped as a liquified gas under its own vapor pressure of 114 psig. The oldest commercial refrigerant known and still in use today. Most extensive use is in soil fertilization. This application is used in the form of salts, nitrates and urea.\n\nIt is the simplest stable compound of these elements and serves as a starting material for the production of many commercially important nitrogen compounds. Pure ammonia was first pre-pared by Joseph Priestley in 1774, and its exact composition was determined by Claude-Louis Berthollet in 1785.
1152760
You can buy houshold grade ammonia (that's about 2% w/v ammonia) from Bi-Low, Coles or Woolworths. Look in the cleaning section.\n\nIf you want more concentrated solutions (eg 25% w/v sometimes known as "880") it may be obtained from specialty chemical companies or some industrial cleaning manufacturers. Expect them to check out your credentials to ensure you have a legitimate use - they will want Drivers Licence/Photo ID, Name, Address, etc. This is required under the "Substance Diversion" requirements of the PACIA agreement which operates in Australia and also under the Health Dept Poisons Regulations in Queensland.\n\nFor cleaning purposes the 2% solution will suffice. If you wish to clean mold of a fish tank, I'm assuming the fish tank is empty - use 3% hydrogen peroxide solution (available from pharmacies) and rinse well.
656515
I hate it too. By the way it's NH3 - Ammonia that is formed. I got little time left. I'll answer later.
514565
Main Entry: am·mo·nia \nPronunciation: &-'mO-ny&\nFunction: noun\nEtymology: New Latin, from Latin sal ammoniacus sal ammoniac, literally, salt of Ammon, from Greek ammOniakos of Ammon, from AmmOn Ammon, Amen, an Egyptian god near one of whose temples it was prepared\n1 : a pungent colorless gaseous alkaline compound of nitrogen and hydrogen NH3 that is very soluble in water and can easily be condensed to a liquid by cold and pressure
771931
Starting material:\nCH3CH2CHBrCH2Br ?\n\nProduct wanted:\nCH3CH2CH2CH=CHCH3 ?  Cis or Trans?\n\nIf the starting material is 1,2 Dibromobutane, then treating it with base (eg. NaNH2) will give:\n\n CH3CH2CHBr–CH2Br   +   base   ——>  CH3CH2CH=CHBr   +   base   ——>  CH3CH2C≡CH\n\nIf this is done with excess NaNH2 in liquid ammonia or dry diethyl ether, then the sodium salt will be produced:\n\n(CH3CH2C≡C)- Na+\n\n(CH3CH2C≡C)- Na+ + BrCH2CH3  ——>  CH3CH2C≡CCH2CH3 \n\nCH3CH2C≡CCH2CH3 when heated gives the more stable compound CH3CH2CH2C≡CCH3  (this is 2-hexyne).  The path will be different from here depending on if you want a cis or trans product.  A controlled catalytic addition (Lindlar catalyst) of H2 will give the Cis form.  Na in liquid ammonia will give the Trans.\n\nThere might be an easier way, but this path is a classic.
1080354
NaCl IS A MOLECULE CALLED TABLE SALT!\nNH3 is not a molecule because the nitrogen atom is not bonded to another atom/atoms using all of its valence electrons and is therefore not a molecule, it is an ion.
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...   :)
436267
http://www.lloydminsterheavyoil.com/nitrogen.jpg\nhttp://www.tcm.phy.cam.ac.uk/castep/MD/img43.png
904363
(NH4)2CO3+MgSO4->(NH4)2SO4+MgCO3
829049
Ammonia (NH3) is the catalyst. Are u in 10th class?