When mixed, how is it that Oxygen and Hydrogen, two volatile chemicals, put fire out?
94473
a compound has diferent properties to the elements thet make it up(usually)\n\nlike table salt, sodium- a slightly harmful reactive metal\n                 chlorine- a poisenous gas\n\nbut put them together and it flavours you food and you eat it\n\nwater stops the combustion reaction
817151
Water is just a liquid gas isn't it? Hydrogen and Oxygen mixed makes water. That's how.
1181278
When atoms (elements) are chemically combined to form molecules the combination makes an new substance with characteristics very different than each separate element.  Water extinguishes fire because it reduces heat and oxygen.  The fire does not break up the water molecules to form free hydrogen and oxygen.
677158
Well the obvious one about explosions and fires.\n\nThen you have that some of the propellants used can be pretty nasty to handle.  Liquid Oxygen, Liquid Hydrogen, etc are very cold and if you spill on yourself you won't live very long.  Liquid Oxygen (along with pretty much any other oxidizer) will allow things to burn very well.\n\nThe hypergolics are the really nasty ones though.  They tend to be toxic and if you mix them they burn (which is why they're called hypergolic and is an advantage in many cases) and some of them are known carcinogens.
1068258
If you mix a hydrocarbon gas/vapor with oxygen, nothing will happen. \n\nHowever, if you then add a spark or flame (which provides the activation energy needed for the reaction to proceed), you will wind up with a fire or an explosion as the hydrocarbon combusts (burns), changing into water and carbon dioxide.
772976
Combustion generally gives off CO2 and H2O vapor.
131453
Fire needs three things fuel, oxygen, and heat.  If you put sand over a fire it cuts off its oxygen.  If you put water over fire it cuts of its heat or energy.  If you reach in and take out all the fuel it will distingusih.  I wouldn't try the last one though lol.
288042
Petroleum fuels are made of Hydrocarbons (molecules made up out of Hydrogen and Carbon).  When you combust/burn a Hydrocarbon in excess Oxygen you produce Carbon Dioxide and Water (incomplete combustion also produces Carbon Monoxide).\n\nTake gasoline for instance, mostly Octane (C8H18), the reaction shown below is the complete cobustion reaction which occurs,\n2 C8H18 + 25 O2 --> 16 CO2 + 18 H2O\nThe fuel is chemically changed into Carbon Dioxide (which is not considered a fuel) and Water.  If we assume complete combustion, there is no fuel left over.\n\nIf you were to split up the Carbon Dioxide (or in your case CO that is produced through incomplete combustion), you will obtain elemental Carbon and Oxygen gas.  Carbon could be considered a fuel since it could then undergo further combustion with Oxygen however, it is not a Hydrocarbon fuel since it has no Hydrogen (all the Hydrogen went into water).
674853
Exhaled air is only about 3% carbon dioxide and is still around 18% oxgyen.  This is not the reason.  If it were, blowing air with a fan or high wind would not blow it out.\nIt blows it out because you are separating the heat from the fuel source.  The bigger the fire, the harder you need to blow.  If they are separated and the fuel source is not hot enough to re-ignite, it blows out.
1153182
Heats of Combustion are quoted in kJ/mole. However, the amount of Carbon and Hydrogen that you have in bigger molecules is larger for 1 mole. \n\nHeat is released because Carbon - Oxygen and Hydrogen - Oxygen bonds are more stable than  Carbon - Carbon or Carbon - Hydrogen bonds. When you burn an alkane, you break the Carbon - Carbon and Carbon - Hydrogen bonds and form Carbon - Oxygen and Hydrogen - Oxygen bonds. A way of thinking of this is that because these  Carbon - Oxygen and Hydrogen - Oxygen bonds are more stable, less energy is required to hold the pieces together. The energy you no longer need is released as heat.\n\nSo why release more when you have longer chains? 1 mole is a set number of molecules, but the longer the carbon chain is, the more Carbon and Hydrogen you have. \n\nAs a result, more Carbon - Carbon and Carbon - Hydrogen bonds are being converted to Carbon - Oxygen and Hydrogen - Oxygen bonds. Result, you have to get rid of more heat.\n\nSo the Heat of Combustion becomes more negative, that is to say you release more heat to the surroundings.\n\nAny help?
311126
I'm not exactly sure what you're talking about, but yes, water can be separated into hydrogen gas (H2) and oxygen gas(O2). It's the following redox reaction.\n\nreduction: 2e- + 2H+ + H2O --> H2 + H2O\noxidation: 2H2O --> O2 + 4H+ + 4e-\n\nMultiply the reduction reaction by two and add the two together to get the final reaction.\n\n2H2O --> 2H2 + O2\n\nThe hydrogen goes down from a +1 state to a 0 state, and the oxygen goes up from a -2 state to a 0 state.
722191
the fire needs oxyegen to burn.  There is no oxygen in the tube as the pressure of the gas forces the contents to flow out towards the flame.
570402
Nothing...unless you light a match, then...BOOM!  In the case of Oxygen and Hydrogen, you'll get pure water afterwards...that should put out the fire you just started :)\n(Not really)
679431
I think you mean why does water extinguish fir. Because it forms a layer of water over the combustable material which prevents oxygen getting at it. Fire needs heat, oxygen and a combustable material to continue. No oxygen-no fire.
1147489
Fire is supposed to be a plasma and/or energy. It goes up because the expanded gasses in the flame "weigh" less than cool air (like a hot air baloon). It doesnt have a shape. it adapts to the shape of the container. It looks like a drop because of the hot air "pulling" it up.
147861
Fires need oxygen to burn.
46564
VTNomad is right.  Hydrogen gas is H:H (two hydrogen atoms sharing a covalent bond) and molecular oxygen is O=O (two oxygen atoms sharing two covalent bonds).\n\nOxidation results from electronegativity, or the affinity of atoms for electrons.  Oxygen is very electronegative, which means it really, really wants to have it's own electrons, and it hates to share them (metaphorically speaking, of course).  Hydrogen is not very electronegative, and its pretty content to walk around as a positive ion with no electrons at all.  It is the weakling on the school playground who will get beaten up and have its electrons stolen by the big kids, like oxygen and chlorine.\n\nTwo oxygen atons don't like having to share electrons, but they can't take them from one another.  But if an oxygen molecule sees two hydrogen molecules, then the two oxygen atoms will part ways, and each will beat up the hydrogen weakling and take both of its electrons.  The "fight" that ensues is fire, where the rapid loss of energy (O=O bonds and H-H bonds have a lot of energy, while H-O-H bonds are low in energy) becomes heat and light, aka fire.\n\nAn oxygen atom, though it likes electrons, will have a negative charge of -2 if it has the eight total electrons needed for Nobel configuration.  Likewise, Hydrogen will have a positive charge if denied its electrons.  So oxygen will let two little hydrogens tag along, and the H2O molecule is charge neutral.  But in water, the electrons are almost always around the oxygen, while the hydgrogen has very little chance of any electrons being around it for very long.  These bonds are low energy.\n\nOther things that burn--coal, gas, methane--these are things where carbon shares electrons with either more carbon or with hydrogen.  O2 will come along and steal electrons.  But O2 can't steal electrons from water, because the oxygen atom in water is just as tough (electronegative) as the oxygen in O2, so it won't win that fight.  But oxygen can take electrons from carbon (giving CO2, or carbon dioxide) or hydrogen, and it does.