magnesium reacts with water, what are the products?
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.
40274
The magnesium metal buried nearby provides protection from corrosion.  “Corrosion” is the technical name for the chemical reaction that takes place when a metal combines with oxygen.  Magnesium acts as an anode and protects the iron or steel tank by corroding in preference to the iron or steel tank.  This means that instead of Iron giving up electrons that attach to the oxygen atoms(which causes corrosion), the Magnesium releases the electrons.  The Magnesium and Oxygen atoms combine to form magnesium oxide while Iron does not take part in the chemical reaction and is thus protected.\n\nThe corrosion of a magnesium anode in preference to steel is an example of galvanic protection.
532841
Minerals such as calcium, phosphorus, and magnesium.
832783
e.g. of formula: Magnesium+oxygen=magnesium oxide\ne.g. of Mixture: Air\ne.g. of Compound: Magnesium oxide
782516
a) 3SiO2 +2 Al --->3 Si + 2Al2O3\n\nb)AgNO3 +HCl---> AgCl +HNO3\n\nc) Mg + CuSO4 ---> MgSO4 + Cu\n\nd) Pb(NO3)4 +4 NaI --->4 NaNO3 + PbI4 (s)
323084
Hardness is typically classified as calcium and magnesium.  The method I propose would demonstrate all of the dissolved solids, as well as the Ca and Mg.\n\nTake a pyrex container, fill it with drinking water, and evaporate the water off by placing it on a hot plate.  This will take awhile if you use too much water, but the 'hardness' will all remain in the container as visible evidence of the solids contained in the water.  \n\nYou can remove the deposited minerals with vinegar, or a stronger acid if you're in a hurry, just be careful.
978387
You should have gotten elemental copper via the following equation:\n\n3CuCl2 + 2Al ---> 3Cu + 2AlCl3\n\nThe water is not part of the reaction.
110757
both MgCl2·6H2O and MgCl2·(H2O)6 are correct formula for hydrated magnesium chloride
644715
Epsom salts, MgSO4. It forms a heptahydrate.
1017794
your kidding right, in water??  All you would end up with is very strong bleach if you use chlorine.  Both are used in keeping pools (which are full of water) from having molds and other harmful substances.  Ignite, don't make me laugh.  \n\nThe line of elements that react violently with water is Sodium, Potassium, Rubidium, Cesium, and Francium.  Each reaction is stronger as you head down the periodic table.
290781
MgSO4(s) + 2HCL(aq) ---> H2SO4(aq) + MgCl2 (aq)
1169882
No.  \n\nMilk of magnesia's main ingredient is magnesium hydroxide in very low concentrations.  Mg(OH)2 is a non flammable, non explosive material.  You'd need to react all the Mg ouf of the hydroxide and then you'd have something to work from.\n\nCheers.
69722
The solid product is calcium carbonate, which is chalk :)\n\nHere's the balanced reaction if you're interested:\nCaCl2 (aq) + Na2CO3 (aq) ----> 2 NaCl(aq) + CaCO 3(s)
810526
when metal react with acid, you will get hydrogen and salt...\nfor example, Zink (Zn) react with hydrochloric acid (HCl):\nZn + 2HCl --> ZnCl2 + H2\n\ni'm sorry i cant give you ALL possible ways in getting H2...\nbut this acid-metal reaction should be easy and cheap enough...
429367
It doesn't form into anything. You said it yourself, it's soluble. The hydroxide part of the milk of magnesia (magnesium hydroxide) and the hydrogen of the sulfuric acid combine to form water, but then you're left with Mg+2 and HSO4- ions. It's just a clear liquid.
488199
Potassium is SO flammable, that if it is dropped in WATER it will rip the oxygen away from the hydrogen and burst into flames! \n\nThat is why it is kept in oil or kerosene, to avoid the possibility that it will come into contact with any moisture. Lithium and sodium will also burn with water this way. Magnesium will spontaneously burn with steam, not liquid water.
248591
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)