how can be sulphur obtained from sulphur dioxide?
405797
heat the pure gas in a sealed tube in absence of air. it breaks up into its components. you've got solid yellow sulphur.
163000
there is really no way of controlling the sulphur. is it the smell that you are trying to control, or the amount of these emmissions that are escaping?
832156
This is what actually happens:\n\nCaCO3 + H2SO4=H20+CO2+CaSO4\n\nIn short, you get carbon dioxide, water and CaSO4. CaSO4 is better known as gypsum:\nhttp://www.galleries.com/minerals/sulfates/gypsum/gypsum.htm\n\nGypsum is used to create plaster of paris.\n\nWhoever said acid rain needs to go back to class.
578806
The full reactions are:\n\nSulfur dioxide reacts with water in the air to form sulfurous acid:\n\nSO2(g) + H2O(l)  H2SO3(aq)\n\nSulfur dioxide (SO2) can also be oxidized gradually to form sulfur trioxide:\n\n2SO2(g) + O2(g) -----> 2SO3(g)\n\nSulfur trioxide then reacts with water to form sulfuric acid:\n\nSO3(g) + H2O(l) -----> H2SO4(aq)
901432
first, balance your equation\n2SO2 + O2 --> 2SO3\n\nnow convert grams SO2 to moles of SO2\n\n(256.24 g SO2) X(1 mole SO2/32.06 g) =  7.99 moles SO2\n\nconvert from moles SO2 to Moles O2\n\n(7.99 mol SO2) X (1 mol O2/2 mol SO2) = 3.99 mol O2\n\nconvert from moles O2 to grams O2\n\n(3.99 mol O2) X (32.00g / 1 mol O2) = 127.68 g O2 needed (ans)\n\nI hope this helps!
953754
Of course, it is a chemical reaction that causes ths to happen naturally.\n\nExpose the silver article to sulphur. SO2 would do the job most admiarably. Dipping it in egg yolk too - it is the sulphur that does the job.
521349
Nitric acid is a very strong oxidizing agent, so on reaction with metals, it gives salt (nitrate), nitrogen dioxode and oxygen.\n\nE.g: Cu + HNO3 ---> Cu(NO3)2 + NO2 + O2\n\nHNO3 self undergoes reduction to NO2 and metals reacting are oxidized.\n\nMetal with HCl give salt and hydrogen and with dilute sulphric acid give salt and hydrogen too, but if you use concentrated sulphuric acid with some metals, then SO2 can be released, because again with more concentration, sulphuric acid becomes a stronger oxidizing agent and gets reduced to SO2 in a redox reaction.\n\nEDIT: The reaction above for copper occurs with concentrated nitric acid; if dilute nitric acid is used, NO would be released instead of NO2.
482177
SO2.\n\nS202 would be Disulfur dioxide.
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=
761151
first you must calculate the number of moles for oxygen, with its molar mass of 32.00g/mol.\n\nonce you have that value, you know from the balanced equation that the number of moles of SO3 will be equivalent to twice the number of moles of oxygen.\nusing this value for moles of SO3, you can then find the mass, knowing that SO3's molar mass is equivalent to 80.07g\nthe mass of SO3 produced will then be 0.9280*mass of SO3. (92.8% yield means only 92.8% of expected was produced)
543308
Reacting a Sulphurous Compounds with a Carbonate generally does the trick.\n\nI hope you like eggy smells!\n\nTom Walvin\nChemist
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.
725443
d) basic\n\n[Non-metal oxides do the opposite and form acidic solutions if they are soluble e.g. sulphur dioxide dissolves to form sulphurous acid)
907925
8. SO3 + H2O --> H2SO4 (sulphuric acid)\n9. Nitric acid - reducing agent\n    Sulphuric acid - concentrated H2SO4 can be used a drying agent, catalyst (in esterification); otherwise, in manufacturing of fertilizers, detergents, and as a battery acid in cars\n    Phosphoric acid - no idea...\n    Carbonic acid - in making carbonated drinks\n\nHope this helps :)
159504
You know, I answered exactly the same question not 2 days ago.\n\nAnhydrous copper sulfate and water would be the easiest two. \n\nYou can buy copper sulfate at any good garden supply shop and most larger hardware stores. The copper sulfate usually sold is hydrated, and is already blue in colour.\n\nYou can make it anhydrous by putting it the oven, uncovered on a sheet of tin foil at 160oC or hotter. You will know when it has become anhydrous beause it goes white. This is quite safe to do in your kitchen oven, all you are doing is driving off the water. No nasty fumes or residues are produced.\n\nStore the crystals in an airtight jar to stop them absorbing water from the air. When you are ready add some water to a few crystals they will retrun to their original blue colour.\n\nThe other possibility is to manufacture your own cabbage indicator. That will make a bluish purple colour when mixed with baking soda. I've included a link with instruction on how to do this.
774704
S + O2 --> SO2\n\nmole of S needed to be converted = 5.00 / 32 = 0.15 mole\nmole of O2 = 0.15 mole\nBy using ideal gas theory:\nP * V = n * R * T\n5.15 * V = 0.15 * 0.082 * 310\nV = 0.74 litre\n\npeace\nvixklen
105753
First you must find the number of moles of 12.6 Liters of SO2 gas at STP.\n\nAt STP an ideal gas (we will assume SO2 is an ideal gas) has a volume of 22.4 Liters.\nSo how many moles would be in 12.6 Liters?\n\nAfter you obtain the number of moles of SO2, then figure out how many moles of Sulfur there are in 1 mole of SO2.\nFor every 1 molecule of SO2, there is 1 Sulfur atom, so for every 1 mole SO2, there is 1 mole of Sulfur.  Knowing this, you can calculate the number of moles of Sulfur needed.\n\nBy multiplying tbe number of moles of Sulfur needed by the molar mass of Sulfur (32.07 g/mol) you can find the mass of the Sulfur required.