how to manufacture balloon gas?
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There is very little helium on earth as nearly all present during and immediately after the earth's formation has long since been lost as it is so light. Just about all the helium remaining on the planet is the result of radioactive decay. While there is some helium in the atmosphere, currently its isolation from that source by liquefaction and separation of air is not normally economic. This is bacause it is easier, and cheaper, to isolate the gas from certain natural gases. Concentrations of helium in natural gas in the USA are as high as 7% and other good sources include natural gas from some sources in Poland. It is isolable from these gases by liquefaction and separation of from the natural gas. This would not normally be carried out in the laboratory and helium is available commercially in cylinders under pressure.
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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)
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http://www.airliquide.com/en/business/products/gases/gasdata/index.asp?GasID=25
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It is theoretically possible to make anything a gas (including that).  It would take way too much energy to do so though.
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Hydrogen and nitrogen react to form ammonia in what is called the Haber process.\n\nThe reaction is as follows:\nN2 + 3 H2 <--> 2 NH3\n\nThis reaction will give about a 85% yield at 200°C (473 °K) and 200 atm of pressure.  This is typically what is done in industry.\n\nWith special considerations to safety, you can get about 100% yield at 200°C and 750 atm of pressure.\n\nThe only remaining question is, how much do you want to make?\nI will assume 100 kg per batch.  You can recalculate for different amounts.\n\nThe molecular weight of ammonia is 17 g/mol, so 100 kg will have 100 kg / 0.017 kg/mol = 5882 mol\n\nTo produce 5882 mol of NH3, you need 2941 mol of N2 and 17646 mol of H2\nSo, the maximum number of moles of gas will be at the beginning of the reaction: 2941 + 17646 mol = 20587 mol\n\nUsing the ideal gas law:\nPV = nRT, where R is the gas constant and n is the number of moles\nV = nRT/P = 20587 mol * .082057 L*atm / mol*K * 473°K / 750 atm = 1065 L = 1.065 m3
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Make Your Own Gelled Alcohol Fuel - Canned Heat\n \nExtreme do it yourselfers can make their own gelled fuel at home with by mixing alcohol and calcium acetate (C4H6CaO4).\n \nThe following instructions and measurements are from the Montville High School Science Departmental.\n \nAdd 25g of crushed chalk or egg shells (calcium carbonate-CaCO3) to 100ml of vinegar (water and acetic acid - CH3CO2H) and stir for about 5 minutes.\nThis should produce carbon dioxide (CO2), calcium acetate (C4H6CaO4) and water (H2O) plus leave you with some left over chalk (CaCO3).  If you are guessing on how much chalk to add, just make sure that there is a little extra after 5 minutes of stirring.\n \nRemove the excess chalk by filtering your mix through some filter paper (coffee filter or napkin can be used).\nSet a funnel in a jar, place your filter in it and pour your suspension through it.\n \nMark the level of your solution in its container and allow your solution to evaporate off about half that volume to remove the excess water.\nPlace your solution in an oven set on low heat or place it out in the sun to dry.  If you went to far - just add the missing water.\nNote - if you like, you can dry out your solution completely and store the remaining dried calcium acetate for future use.\n \nIf your solution isn't already in the container you want your gel in, then pour it in there now.\n \nAdd 30ml of alcohol (ethanol, methanol, or isopropanol) to your solution and watch the gel form.  Do not stir.\n \nOnce the reaction in complete, pour off any extra fuel.\n \n \nY2kSurvivor suggests:\nDissolved calcium acetate solution ratio:\n1 part dry calcium acetate (by volume) to 2 parts water\n \nSolution to fuel ratio:\n1 part dissolved calcium acetate solution to 4 parts alcohol\n \nAlso see:\nCanned Heat: Alcohol Gels - University of Wisconsin\nCanned Heat An Alcohol Gel - Chem Matters\nCanned Heat: Sterno - Normal Community High school
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I know of at least 4 ways.  I think that the distillation or membrane separation are the most practical.\n\n(1)Distillation\nOxygen and nitrogen have different boiling points.\noxygen: 90 K\nnitrogen: 77 K\nIf you cool the mixture to a temperature between the boiling points of each you will be in a two-phase region.  There will be a gas phase rich in nitrogen (because it has a lower boiling point) and a liquid phase rich in oxygen.  A distillation column can be used to separate the phases and collect them in a continuous, pretty efficient process.  I think you have to do something special about the argon in air when you do this (like have more than one separation step, more than one distillation column).\n\n(2)Adsorption\nOxygen and nitrogen gases may adsorb to (stick to) the surfaces of certain compounds (like metal surfaces).  If you make a series of tubes lined with a substance that preferentially adsorbs (for example) oxygen, you will get a gas output that has less oxygen in it.  In a well-designed case, the adsorption is reversible.  Increasing the temperature of the substance will causes the oxygen to leave the solid surface and once again become a gas, giving you a relatively pure oxygen stream.  If the purity is not good enough, you can collect the streams and repeat the process (use a longer tube).  I don't know of an example of an adsorption material off-hand.\n\n(3)Stripping\nStripping is the process of passing a gas through a liquid and may involve chemically removing one of the components of the gas.  If you bubbled air through a liquid that had a chemical in it that reacted with oxygen to form a compound then the gas that reaches the top will be nitrogen-rich.  For example, your blood contains hemoglobin, so that when it is in contact with the air in your lungs the oxygen sticks to the hemoglobin, forming a chemical complex.  This is a lot more effective than limiting yourself to an oxygen supply based on whatever gases can dissolve in your blood. \n\n(4)Membrane Separation\nOxygen and nitrogen have different permeability in membranes.  They can diffuse through solids, but at different rates.  I think oxygen typically has high permeability.  If you pressurize the gas mixture and pass the gases through a bundle of tubes (high surface area is key) then some gas will pass through the tubes axially and some will diffuse through the walls radially.  The stream that passed through the tubes will be richer in nitrogen, since it is less permeable.  The stream that diffused through the walls of the tube will be richer in oxygen, becuase it is more permeable.  Repeat the process to get the desired purity.\n\nAn artificial lung can be made by passing blood through a long set of tubes that have oxygen on the outside of the tubes.  The oxygen diffuses into the blood through the permeable tubes.
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Nitrous Oxide (laughing gas) is most commonly made by the thermal decomposition of ammonium nitrate (NH4NO3). \n\nHowever, unless you are a chemistry professional with access to professional equipment, I would strongly discourage to try this at home.\n\na)The synthetic process frequently employed may lead to an EXPLOSION.\n\nb) Other oxides of nitrogen may be obtained as byproducts of the synthetic process.  One of these, nitrogen dioxide, is extremely toxic and can lead to rapid destruction of lung tissue, even if inhaled in small quantities (i.e. DEATH).
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Take 2 hard glass boiling tubes.In one of the tubes put small pieces of wood, and some water in the other tube.Heat the first tube with burner.First heat gently and then strong heating.Through a delivery tube collect all the gases produced in the first tube under water in the second tube.By means of another delivery tube the gases over water in the second tube is taken out. This gas is simply called wood gas.Though we call it wood gas it is not a simple gas but a mixture of many.You will see  drops of black liquid at the bottom of the second tube .This black liquid is called tar.Usually methanol and acetic acid is produced which mix with water in the second tube.Residue left in the first tube is charcoal.\n\n\nBoiling point of methanol is abt 65 degree celcius and boiling point of acetic acid is 118 degree celcius. Acetic acid is a high boiling liquid then methanol. On the other hand, water has a boiling point of 100 degree celcius.Now apply fractional distillation to separate the three. For fractional distillation visit:\nhttp://en.wikipedia.org/wiki/Fractional_distillation
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Hot air balloons have  heaters that heat the air.\n\nSo, to lower air density in a balloon without losing air pressure, you simply need to increase the speed of the air particles. You can do this very easily by heating the air. The air particles absorb the heat energy and become more excited. This makes them move faster, which means they collide with a surface more often, and with greater force.
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There are a couple of things you need to think about so you can work this out for yourself. \n\n1. Gases expand when they are heated. This is easily seen from the ideal gas law, PV=nRT, where P is pressure, V is volume, n is number of moles, R is a constant and T is temperature. Most gases roughly follow this law. As T increases, so does V, at constant P (of course, in the case of a balloon, P does not remain constant). \n\n2. When the volume of a gas increases, its density D=mass/V  decreases.\n\n3. By Archimedes principle, the buoyant force on an object is equal to the weight of the fluid displaced. The net buoyant force is the difference between the buoyant force on the object and the weight of the object. \n\nSo in the case of your balloon, if it displaces air of greater density (since it is colder), then there is going to be a net buoyant force upwards on the balloon. The weight of the air of density Da displaced by a balloon of volume V is V*Da*g, where g is the acceleration of gravity. \n\nI could go into more detail, but you might enjoy working this out for yourself. If you need more help, then ask.
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First off get a bunch of balloons and a funnel. Try going to a garden center (if there are any open) and see if they have sand or potting soil you can use. Flour would work pretty well. You can use hair gel. Get small, rounded beads. Sugar would probably work well. Just make sure you get something that is not going to rot. \n\nYou fill the balloon with the material of choice and tie it off.
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Check this link:\n\nhttp://72.14.203.104/search?q=cache:Hb_4_LKfVd4J:www.hydrogen.energy.gov/pdfs/progress05/vi_b_1_wu.pdf+how+to+make+sodium+borohydride%3F&hl=en&gl=in&ct=clnk&cd=7&client=firefox-a
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A n energy related project:\n\n1.  Ethanol production, ferment and distill - very easy.  Ethanol is used in gasoline, made from fermented sugar or starch.  Combine sugar, water, and yeast, covered so no air gets in (a plastic bottle with a balloon over the neck).  Let ferment 3 -5 days, balloon will go up then down.  Then in a small pot, put in 3/4 inch of the liquid and a small glass in the middle.  Invert the pot cover and put ice and water in it.  Boil very slowly till about 1/4 of the liquid is gone.  Cool down and you'll have ethanol in the small glass.  Repeat distillation to increase concentration of ethanol.
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1.Since Volume is proportional to Temperature, it could also be written with a constant(k): V = k x T , V/T = k , k = 0.923L/ (25+273)K = 3.10x10^-3 L/K\n2.I'm not too sure about this one, but here is my best shot.\nUsing the ideal gas law PV=nRT, same Temp & Pressure, let Va be the volume of the first baloon and Vb be the volume of the second balloon. Va = 1.25Vb, Let na be the number of moles in baloon 'a' and nb be the number of moles in balloon 'b'.\n\nBalloon a: PVa = naRT\nBalloon b: PVb = nbRT\nsolve for P,T or R.\nThis case I solved for T:\nT = PVa/naR  & T = PVb/nbR, since same temp (or pressure or constant) which is PVa/naR = PVb/nbR. Divide by P & R, Va/na = Vb/nb\nVa x nb = Vb x na, Va = 1.25 Vb, @75%\n1.25(.75)Vb nb = 0.75Vb x na, divide by .75Vb\n1.25nb = na\nSo there is 25% more moles (or mass) in baloon A.
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Add some baking soda first and then pour on some vinegar. You will observe some bubble forming and the bublbles will rise very quickly. If you want to make fire instead, add some glycerine to potassium permagnate. Be very careful if you want to do this.
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Trying to make nitroglycerin, eh?\n\nWon't find out how to do it from me.  And beware of some of the other sources out there -- they're deliberately miswritten so that you'll blow yourself up.