sprains and strains. It cools the local tissue and reduces bleeding‚ swelling and pain. It also aids in a speedy recovery. The most commonly used chemical in instant cold packs is ammonium nitrate which will be tested in the investigation along with four other chemicals in water. These other chemicals include potassium nitrate‚ potassium chloride‚ sodium acetate and sodium chloride. The two lowest chemicals will then be mixed together at different concentration ratios to see if this drops the temperature
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considerable damage • sulfuric acid in the rain chemically reacts with the calcium compounds in the stones (limestone‚ sandstone‚ marble and granite) to create gypsum‚ which then flakes off • commonly seen on old gravestones where the acid rain can cause the inscription to become completely illegible • causes an increased rate of oxidation for iron • Visibility is also reduced by sulfate and nitrate in the atmosphere Solutions: • many coal-burning power plants use Flue gas
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------------------------------------------------- The Processes of the nitrogen cycle Nitrogen fixation Atmospheric nitrogen must be processed‚ or "fixed" (see page on nitrogen fixation)‚ in order to be used by plants. Some fixation occurs in lightning strikes‚ but most fixation is done by free-living or symbiotic bacteria. These bacteria have the nitrogenase enzyme that combines gaseous nitrogen with hydrogen to produce ammonia‚ which is then further converted by the bacteria to make their own organic
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carbonate formula | CaCO3 | 10 | Ammonium sulfate formula | (NH4)2SO4 | 11 | Carbonic acid formula | H2CO3 | 12 | Sodium bicarbonate formula | NaHCO3 | 13 | Sodium hydroxide formula | NaOH | 14 | Calcium hydroxide formula | Ca(OH)2 | 15 | Ethanol formula | C2H5OH | 16 | Hydrobromic acid formula | HBr | 17 | Hydrosulfuric acid formula | H2SO4 | 18 | Nitrous acid formula | HNO2 | 19 | Potassium phosphate formula | KH2PO4 | 20 | Silver nitrate formula | AgNO3 | 21 | Sodium carbonate
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Centre Number Surname Other Names Candidate Signature Candidate Number For Examiner’s Use Examiner’s Initials Question Mark General Certificate of Secondary Education Foundation Tier June 2011 1 2 3 4 5 6 7 TOTAL Additional Science Unit Chemistry C2 CHY2F Chemistry Unit Chemistry C2 Wednesday 25 May 2011 For this paper you must have: the Data Sheet (enclosed). You may use a calculator. F 9.00 am to 9.45 am Time allowed 45 minutes Instructions Use
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soluble in water and some are insoluble. The reason some ionic compounds are insoluble in water is given here. All NITRATE compounds are soluble in water e.g. * sodium nitrate * ammonium nitrate * copper (II) nitrate * lead (II) nitrate * zinc nitrate * potassium nitrate All POTASSIUM‚ SODIUM and AMMONIUM compounds are soluble in water e.g. * ammonium chloride * sodium sulphate * potassium carbonate * sodium hydroxide * potassium oxide Table I showing
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oxides. Rain dissolves the nitrogen oxides‚ turning them into nitrates‚ which is carried to the earth. The second form of nitrogen fixation is Industrial fixation‚ which is a process that converts nitrogen to ammonia (NH3). Ammonia can be used directly as a fertilizer‚ but most of it is further processed to urea and ammonium nitrate (NH4NO3) . The usable nitrogen will take 2 forms: nitrate and ammonium. Plants then take up nitrate and ammonium‚ get lost in the subsoil or atmosphere‚ or are changed in
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a) To manufacture nitrogenous fertilizers such as ammonium sulphate‚ ammonium nitrate and urea b) The liquid form is used as a cooling agent (refrigerant) in refrigerators c) As a raw material for the manufacture of nitric acid in the Ostwald process d) To be converted into nitric acid used for making explosives e) As an alkali to prevent the coagulation of latex so that latex can remain in the liquid form f) To produce ammonium chloride used as an electrolyte in dry cells
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metal ions or by ammonium ions. Compounds in which the H+ ions in an acid have been replaced by ammonium ions (NH4+) are called ammonium salts. NOTE: •An anion is a negatively charged ion. Hence:•Hydrochloric acid gives chlorides. E.g. sodium chloride‚ ammonium chloride. •Nitric acid gives nitrates. E.g. barium nitrate‚ copper nitrate. •Sulphuric acid gives sulphates. E.g. silver sulphate‚ iron (ii) sulphate. •Phosphoric acid gives phosphates. E.g. sodium phosphate‚ ammonium phosphate. •Each acid
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(NOx). 4.Other processes: In addition‚ the formation of NO from N2 and O2 due to photons and especially lightning‚ can fix nitrogen. Assimilation Plants take nitrogen from the soil‚ by absorption through their roots in the form of either nitrate ions or ammonium ions. All nitrogen obtained by animals can be traced back to the eating of plants at some stage of the food chain. Ammonification When a plant or animal dies‚ or an animal expels waste‚ the
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