Reactive Metal Fires?
925364
Definitely not water, as those three metals will burn on contact with water (and potassium will explode.) Liquid CO2 might do, as it would cool the burning material extensively, possibly below the ignition point. The sand (SiO2) would be a smothering agent. I'm not sure about the carbon tet.\n\n5 NOV 06, 1522 hrs, GMT.
31832
Any metal will melt on heating (unless burning up before), but for pure lead the melting point is fairly low with 600K (327°C, or 621°F). The melting point for lead alloys (with tin and/or antimon) is even lower.\n\nEven candle flames emit sufficient heat to melt down lead placed on a spoon in reasonable time.
1097960
Dynamic flash combustion the sudden and complete oxidation of a small sample at a high temperature.  Check out this site:\n\nhttp://www.ruc.dk/inst1/research/equipment/chnsEquip/
779894
AlthoughO2 is a strong oxidizing agent, its oxidizing reactions are usually slow kinetically. Many flammable materials will exist in the presence of air until a flame or spark starts the reaction. The very electronegative nonmetals are poor reducing agents. \n\nF2 will oxidize all metals and most other substances. It must be stored in either nickel or copper containers because the fluorides of these metals form a film passivating the metal surface. \n\nFor more please visit:\nhttp://www.wou.edu/las/physci/ch412/nonmetal.htm
419109
I don't remember the ordering, but there's probably some metal out there that won't react?  Gold, maybe?  For regular metal, that sounds a bit iffy.
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.
967480
flammable , orderless, colorless . have low frozen point ,reactive
81060
Almost all of them actually. The rusting of iron forms a red colour,  the burning of a match forms a black color and so forth. Think of any chemical reaction and it will most likely include a colour change.
151070
Accidentally putting foil and metal in the microwave can cause a fire.
155392
One method is using bimetallic strips of metals that can stand very high temperature. Bimetallic strips bend when the temperature changes.
1179262
It's too reactive. Since you have a tungsten filament blazing away at thousands of degrees, you need a totally nonreactive invironment. Hence the noble gas.\n\nIt's noble gas, by the way, not Nobel. Nobel was the inventor of dynamite.
147861
Fires need oxygen to burn.
97864
yes, with an alloy or equal or lower melting point
315090
Exremely high. In its pure form strontium is extremely reactive with air and spontaneously combusts. It is therefore considered to be a fire hazard.\n\nDue to its extreme reactivity to air, strontium always naturally occurs combined with other elements and compounds, as in the minerals strontianite, celestite, etc. It burns in air to produce both strontium oxide and strontium nitride. It should be kept under kerosene to prevent oxidation. Finely powdered strontium metal will ignite spontaneously in air.\n\nHeat capacity (25 °C) 26.4 J/(mol·K)
900859
If the metal not in the compound is higher on the activity series than the metal in the compound then a reaction will occur and the metals will switch spots. If the metal not in the compound isn't higher on the activity series than the metal in the compound then no reaction will take place. You got to be joking if you think I'm going to be doing 20 problems for you. The only way to learn these is to do them on your own. Just so you know in #6 a reaction will not occur.\n\nHere is an activity series:\nhttp://en.wikipedia.org/wiki/Reactivity_series\n\nREACH doesn't know how to do these, don't listen to his answer.
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.
445950
As the metal flexes, the molecules which make up the compound are temporarily displaced and generate kinetic energy which is dissipated as heat.   The process can be demonstrated in reverse i.e. when metal is heated, the molecules are displaced and the metal becomes pliable