What do we get of we mix MgO with H2O2?
101127
You get Mg2O2 (magnesium peroxide) and water H2O.
712912
BaI2(aq) + MgSO4(aq)  --> BaSO4(s) + MgI2(aq)\n\nSo BaSO4 will precipitate.
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HgO ------> Hg + O2 at about 400 C\n\nMg + CuCl2 ---------->  MgCl2 + Cu(solid)\n\nMg, being higly electropositive than Cu, replaces Cu.
866210
2NO+O2--->2NO2\n\nCaO+H2O--->Ca(OH)2\n\nCaCO3--->CaO+CO2
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CaO + H2O => Ca(OH)2\n\ncalcium oxide + water => calcium hydroxide\n\nThis is a great site for this - the reaction between CaO and water is an exothermic reaction (1)\n\nthe second reference is even better - not simply a diagram but a torn apart "self-heating" can\n\ngood luck!\n\nSomething else you might want to looking - MRE's (meals ready to eat)
504628
you'll have a mixture of hydrogen and oxygen
277253
MgCl + H2O = MgO + H2Cl
106159
Yes,mixing two or more items together will creat a chemical reaction with alot of different substances. I suggest you read up on what your mixing toghether. Your involed with substacnces that could help creat a recipe for a bomb. I suggest you go back to the kitchen and make a new creation by trying some of your cooking skills until your sure of what your mixing together.
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(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.
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Cu + 2H2SO4 --> 2H2O + SO2 + CuSO4\nDouble the H2SO4 and the H2O.
937834
Well, you are getting in to a bit more complicated chemistry. For the question you are asking, the simple answer is No. However there are multi-valence ions, such as Oxygen. Normally Oxygen would gain 2 electrons making it O(2-) but it has another valence of 1 where it only gains one electron and becomes O(1-). By the sounds of it you are not at this point so don't worry about but you will get there eventually. In order to understand multi-valence you need a Periodic Table of Elements that lists all the valences of each element. This makes bonding harder, etc,etc so I wouldn't worry about it if I were you, yet.\n\nSo to simply answer your question, No, it is impossible for Magnesium
131743
The formation of PhMgBr is a redox reaction.  The two electrons of magnesium metal are added to the PhBr bond to make Ph-Mg-Br.  Then you added this in solution to the dry ice (solid O=C=O).  The electrons between Ph and Mg add to the carbon of the CO2.  The electrons from one of the pi bonds moves out to the oxygen so that you have PhC(O)O- where the (O) is still doubled bonded to the C.  After the reaction was complete, you added water to protonate the O minus.  This completes the reaction.  Since you are in organic lab, you should still have an organic textbook.  There is likely a mechanism drawn out in any organic textbook you can find.
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D. Mg, because it will oxidize instead of the iron.
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1. highter since given weight of magnesium looks to be a larger percent of finished product.\n2.It would depend on molecular weight of other reactants.  If they were heavier than Oxygen the Mg would seem to be a lower percentage.  If only other possibility for Rx was with nitrogen and ratio of recatants was the same as with Oxygen(unlikely) then the resulting compound would be lighter than MgO making the Mg percent higher.\n3.  Mg oxydizes in air at room temp.  This white film was MgO already oxydized which would interfere with your results, raising the calculated percentage of Mg.
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depends if the mixture is bonded by a physical or chem bond....there is magnetic separation,distillation,fractional distillation,evaporation,crystallization...etc...why dont u look up a chemistry book
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Explain. You mean the one shown in science lessons or in nature?\nIf it's mountains, that's not a reaction. It's simply molten rock or gas escaping from the pressurised chamber under the rock cap we call a mountain.\nIf it's the reaction in the lab, there are two.\n1) Tha Ammonium dichromate reaction \nsee this link: http://jchemed.chem.wisc.edu/JCESoft/CCA/CCA3/MAIN/VOLCANO/PAGE1.HTM\n2) Sulphuric acid and sugar (not really intended to be a volcano reaction though)\n3) Potassium permanganate and glycerol. Link: http://www.chem.ed.ac.uk/chemcon/electron/volcano.htm \nThere are other variations on chemicals or fuses to start it (commonly magnesium).\nThe principle behind all of them is once you have supplied enough heat to get the reaction over the activation hump, it is exothermic (produces heat) and so is self sustaining, taking oxygen either from the air or one of the compounds acting as an oxidising agent.
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MgCO3 + 2HCl ---> MgCl2 + CO2 + H2O\n\n2HCl + MgO ---> H2O + MgCl2\n\nBarium hydroxide is a base so can be neutralised with any acid.  An example being HCl.\n\nBa(OH)2 + 2HCl ---> BaCl2 + 2H2O\n\nor H2SO4\n\nBa(OH)2 + H2SO4 ---> BaSO4 + 2H2O