Why is it necessary to heat the heat the solutions in the preparation of ammonia and sulphur dioxide?
413924
They are endothermic reactions and need energy for the forward reaction to take place.
225436
Here is one :\n\nAn aqueous solution of hydrazine can be prepared by reacting ammonia with a solution of sodium hypochorite:\n\nthe net ionic equation:\n\n2NH3(aq) + OCl-(aq) ---> N2H4(aq) +  H2O(l) + Cl-(aq)\n\n""" CAUTION""""\n\nMixing these chemicals together is very dangerous. Please on paper  analysis only .
860331
NH4Cl has an enthalpy of solution of +14.8kJ/mol, meaning the reaction is endothermic.
97767
Uh, your question is miscategorized\nthe metabolic process is not fire \njust because it shares a single characteristic\ninterestingly the products of hydrocarbon combustion \nare CO2 + H2O\n\nIf you get a 90% efficient furnace it will condense water in the exhaust stack
125270
A gas refrigerator uses ammonia as the coolant, and it uses water, ammonia and hydrogen gas to create a continuous cycle for the ammonia. The refrigerator has five main parts: \n\nGenerator - generates ammonia gas \nSeparator - separates ammonia gas from water \nCondenser - where hot ammonia gas is cooled and condensed to create liquid ammonia \nEvaporator - where liquid ammonia evaporates to create cold temperatures inside the refrigerator \nAbsorber - absorbs the ammonia gas in water \n\nThe cycle works like this: \n1. Heat is applied to the generator. The heat comes from burning something like gas, propane or kerosene. \n2.  In the generator is a solution of ammonia and water. The heat raises the temperature of the solution to the boiling point of the ammonia. \n3.  The boiling solution flows to the separator. In the separator, the water separates from the ammonia gas. \n4.  The ammonia gas flows upward to the condenser. The condenser is composed of metal coils and fins that allow the ammonia gas to dissipate its heat and condense into a liquid. \n5.  The liquid ammonia makes its way to the evaporator, where it mixes with hydrogen gas and evaporates, producing cold temperatures inside the refrigerator. \n6.  The ammonia and hydrogen gases flow to the absorber. Here, the water that has collected in the separator is mixed with the ammonia and hydrogen gases. \n7.  The ammonia forms a solution with the water and releases the hydrogen gas, which flows back to the evaporator. The ammonia-and-water solution flows toward the generator to repeat the cycle.
1087032
try Vogel's "Qualitative Inorganic Analysis", I'm pretty sure it has all the answers 4 u.\n\ndont care editions, but for 7th ed, ISBN is 0582218667\n\n****\nokey then, from Vogels\n\n1) when heated, lead nitrate decomposes to white solid lead oxide (PbO), brown gas (NO2) and oxygen gas. Brown gas decolorizes when contact with water. \n\n2) ammonia odur. ammonium compounds are all volatile towards heat and decomposes to ammonia and an acid but quickly recombine if the acid, in this case, hydrochloric acid, is a strong acid.\n\n3) anhydrate copper sulphate is white, hydrate copper sulphate is blue. I have no idea which one you actually heated. If it's anhydrate, no change; if hydrate, blue ---> white.\n\n4) blue precipitate forms initally, but resolve upon excess reagent, clear blue soln results due to the formation of copper complex [blue precipitate: Cu(OH)2*CuSO4, complex: [Cu(NH3)4]^2+]\n\n5) brown precipitates froms [Cu(OH)2], no change with excess reagents.\n\n6) metal-gray stipe (magnesium stipe) gains a redish brown color due to formation of copper metal. Possible decolorization of the soln (depends on how much magnesium u actually put in)\n\n7) volatile reaction, solid metal solves,ignitable gas is formed. (if phenolphthalein is added to water initally, soln becomes pink)
948757
The concentrations of all the components: the reactants, the products, the catalyst.\nYou will also need the temperature.\nIf it's a gas-phase reaction, the pressure..\nIf it's a solid-liquid reaction, the surface area; or if the catalyst is a solid, the surface area of the catalyst.
394775
2Cu(NO3)2 ----> 2CuO + 4NO2 + O2\nOBSERVATION: brown, choking fumes of NO2 evolved; black solid i.e CuO settles at the bottom\n\n2FeSO4 ----> Fe2O3 + SO2 + SO3 \nOBSERVATION: white fumes of SO3 evolved and reddish brown solid i.e. Fe2O3 formed\n\nEDIT: The above equation for iron(II)sulphate may be a supposed characteristic for its thermal decomposition relating to that of copper(II)nitrate above, but Chaos, O2 will not be evolved here, because SO3 will not get reduced to O2, even on strong heating.
995093
It is used to heat fluids and chemicals when the heat has to be uniform and fast.
896646
"The final experiment was to observe the reaction when one small crystal of NH4SCN was added to 0.1 M FeCl3. The color of FeCl3 was yellow, but after NH4SCN was added, the color of contents changed to red.\nIn second experiment, when the Mg was ignited, the resulting flame was hot. Therefore, the release of thermal energy through the interaction of Mg and O was shown.\nFiguring out the type of the last two reactions was difficult, because the chemical equations were not given. However, the possibility that the type of both reactions were replacement reactions was high. The reason being that the chemical reactions were observed as a color change and this means that the composition of the substance is changed.\nThis experiment was very successful, and it was a good opportunity to observe chemical reactions directly."\n\nI would change your paragraph to that.  I would also expand on the other experiments if you know more about them.
957199
If you are doing it in a laboratory setting, you can mix it with carbon and reduce it to the metal. You will need high temperatures, though.
876129
The Claus process is catalytic reaction of hydrogen sulfide with sulfur dioxide to give elemental sulfur.\n2H2S + SO2 ===> 3S + 2H2O\nSome of the H2S is oxidized in air to SO2. The elemental sulfur is isolated in pure form. This makes it suitable for re-oxidation to SO2, further catalytic oxidation to SO3, and passage through the contact process to make pure, concentrated H2SO4. Amine sweetening refers to reaction of H2S innatural gas with amines, R3N, to give ammonium sulfides, 2R3NH+ + S=
530330
Ice melting\nWater freezing\nWater boiling\nAmmonium chloride subliming
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
431802
You are not going to be able to buy nitric acid above 70% pure.  Nitric acid pretty much dissolves anything it comes in contact with which causes for its low purity.  I would not suggest heating concentrated acid since the fumes it will produce are very dangerous.  The fumes at room temperature will even cause burns. Depending on what you are trying to do, the acid will need some oxygen to dissolve metals.  With stainless steel, a small scratch on the surface will be enough.
216099
Yes if you react NH4NO3(aq) with something SO4 you can make it.
1157378
If you mean the generation of ammonia, it is called the haber process:\n\nN2 + 3H2 > 3NH3\n\nNitrogen + Hydrogen > Ammonia\n\nIt is a reversible process requiring high temperatures and pressures.