Can you create magnesium oxide  with magnesium and oxygen without the use of flame?
923645
No, it's an endothermic reaction meaning you need to add heat (but no necessarily a flame) to drive the reaction. The only way it would react with oxygen in the atmosphere is if the outside temperature where hot enough to drive the reaction. Of course, we'd all be dead, so we couldn't see it.
110024
haven't you seen magnesium burning. sodium burns, potassium burns.\n\nthese metals are very reactive metals owing to the valence electrons in their atoms. they are one electron short of stable octet structure (mg- 2 elec), and so they easily burn\n\nbut other metals are much stable and the oxides of those metals are formed at very high temp and long exposure time but not accompanied by emission of flames.\n\nwood is made of cellulose, which is organic in nature i.e carbon and hence burns to form carbon di oxide (chiefly present in smoke)
659725
Magnesium will react with any gas except noble gases when heated, because of its low electronegativity. In vacuum or noble gas atmosphere it can be heated up to melting point of 625°C, just at or below red glow.\n\nWhile red or white hot iron will oxidize on the surface, the heat released by that process is not sufficient to start a chain reaction like in burning magnesium. The higher melting point of iron depends mostly on the crystal lattice of iron.
372779
Assuming you mean in a vacuum.\nAs long as you could create a delivery system that would spray both the oxidant and the combustive material in a constant stream it would work.  The problem is that if you are spraying both the chemical accelerant and the oxygen it needs to burn from the same appliance, you have to be careful that one of both of the chemicals don't mix inside the delivery mechanism or the fire will follow the path and explode inside the device.\nNASA has torches and similar devices for welding but they are extremely short range (inches).  The flame wouldn't look like one here on Earth as any particles that strayed from the main spray of oxident would immediatly stop burning.\nAlso, you wouldn't be able to cause any other combustable things to burn once the flame was removed.  If you concentrated it on a piece of wood, for instance, it would burn until you pulled the "flamethrower" away and would immediately stop burning.
377534
errr, grind metals to a fine powder and mix them together and press them and you can get alloys physically impossible to make by forging.\n\numm, grind metal very fine so the oxidise and use them to make metal fires, such as "thermalite" for welding traintracks.
326922
Another easy reaction:\n\nMg(s) + HNO3 ===========> Mg(NO3)2 + H2 (g)\n\nMagnesium reacts rapidly with nitric acid to make magnesium nitrate and hydrogen gas
421578
Doesn't work with magnesium. Get some and start it burning with a torch. Then hit it with a super soaker from a distance. You'll get an instant sunburn from the radiation.\n\nWhen magnesium burns, it takes the oxygen and hydrogen out of the water, and flares up that much more. You need a D type fire extinguisher to put it out. Never heard of a D? It sprays sand. It's designed specifically for flammable metals, like magnesium and titanium.\n\nBy the way, do you know how to make water out of pure hydrogen and oxygen? Burn them together.
412358
You could skip the Nitrogen Oxide and use Nitrous Oxide.   :o)
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.
734862
HgO ------> Hg + O2 at about 400 C\n\nMg + CuCl2 ---------->  MgCl2 + Cu(solid)\n\nMg, being higly electropositive than Cu, replaces Cu.
518561
Mg(OH)2 n then Al(OH)3 gel
893183
Magnesium oxide, also known as magnesia.\nFormula: MgO\nFormula weight: 40.32\nColorless\nSpecific gravity: 3.65\nMelting point: 2800 Deg. C.\nBoiling point: 3600 Deg. C.\n\nHope this helps
728971
(The) second experiment was to observe the reaction when a magnesium ribbon was ignited. The ribbon was put to the flame of a burner (delete ,) and was ignited. The reaction was very (intensive) (change to intense), and (burned with a) (delete was with) very bright white light. Usually when a substance is ignited in air, it reacts with H2 or O. In this case, because the Mg was the positive ion, it must have reacted with oxygen, (which is a ?)negative ion. In this experiment, because Mg was joined to O2 to make 2MgO of different composition, this was a combination reaction.\nThe third experiment 0.1 M CuSO4 and 6 M NH3 were used. CuSO3, a Sky blue liquid,  was place in a test tube, and then 1 drop of 6 M NH3 was added. Right after NH3 was added, the top of (the) liquid changed to navy color.  After the liquid was stirred the color of the liquid changed to a blue that was darker than the color of CuSO3. Ten more drops (of CuSO4?) were added to the contents, and the color of (the) contents changed to a violet color.
346788
Mg(s) + H20(l) -----> MgOH2 + 1/2 H2\n\nThe magnesium reacts with water in a violently exothermic reaction.  It forms a compound of magnesium hydroxide consisting of one Mg(2+) ion and two hydroxyl ions OH(-) and one half mole of H2 gas is evolved, which is where the sparks and flames come from.
106182
Actually its MgO. Magnesium is a bivalent metal Mg(2+) and Oxygen has a charge of O(2-) so they form a very strong 1:1 bond.
863957
combustion means oxidation with oxygen. it is done by burning in air.\nHence Mg + heat is combustion reaction. It gives MgO upon reacting with oxygen. But it also reacts with the Nitrogen in the air by giving Mg3N2. That is the side reaction, ofcourse.
48024
Your question doesn't make sense.  No metal would produce heat by being put in hot water--heat is only produced by a chemical change.  Perhaps sodium metal, which would conbust if the water had any oxygen in it, but it wouldn't need to even be hot water.  Also, water wouldn't be water at 400 degrees.