What is the chemical equation for fire?
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Fire is not a chemical, so there is no chemical symbol to represent it. However, numerous things burn, and these can be adequately described by a reaction. For example, wood is primarily cellulose: \n(C6H12O6)n + O2 --> H20 + C02 + heat + light\nPS. The above reaction is unbalanced. This is what happens when wood is burned - it turns into water and carbon dioxide. Note that "normal" fire only happens in the presence of oxygen. I say "normal" because there are other types of fire that don't involve oxygen.\nWe don't see any water because it evaporates from the heat of the fire as soon as it is formed. \nThe heat given off is the heat of the fire (obviously). \nThe light produced is what you see as fire.
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Fires need oxygen to burn.
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When silane burns, SiO2 is formed (and water). You can now draw up the balanced equation.\n\nManganese(IV) oxide catalyses the decomposition of hydrogen peroxide:\n\n2H2O2 ----> 2H2O + O2
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no oxygen is required\nthe equation for burning is:\nCxHy + CO2 --> O2 + H2O\n\nthe product is oxygen.. meaning you don't need oxygen in the first place to burn\nand on the sun, there are already zillions of carbon and hydrogen compounds which can burn with it, and you're forgetting CO2 is different than just O2.
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The burning of fossil fuels containing sulphur and nitrogen:\n\nS + O2 ---> SO2\n\nN2 + 2O2 ---> 2NO2
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the answer is fire because if you give fire something to burn it will live, maybe even get bigger, but if you put water on it, it will go out... so the answer is... FIRE!
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heat of combustion = -(enthalpy change for reaction )\n          \n = -(heats of formation of products - reactants)\n \n1 mole of ethanol, when burnt completely, produces 2 moles of CO2 and 3H2O i.e delta H = 2(heat of formation of CO2) + 3(heat of formation of H2O ) \n\n= 2(-394 kJ/mol ) + 3(-286 kJ/mol)\n\n= -1646 kJ/mol\n\nheat of formation of ethanol = -277 kJ/mol\n\nso\n\nheat of combustion = - (-1646 - (-277) )\n                   \n                   = - (-1646 + 277 )\n\n                   = 1369 kJ mol
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Fe2O3(s) + 3 CO(g) ----> 2 Fe(l) + 3 CO2(g)\n\nCount up the oxygens; the left side and right side oxygens should match.
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CH4 + 2O2-> CO2 + 2H2O
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States are solid, liquid, gas and plasma...there is no fire state.  Fire is a chemical reaction that occurs when an object is going from one state to another.  A physical reaction is like the melting of ice...it goes from a solid state to a liquid state.  Fire actually changes the chemical makeup of a substance, therefore it is a chemical reaction.\n\nAnd it definitely does NOT have "plasma in it"!  Plasma is extremely rare on earth.
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Fire is the rapid combination of oxygen with fuel in the presence of heat, typically characterized by flame, a body of incandescent gas that contains and sustains the reaction and emits light and heat. (from www.straightdope.com)\n\nThe typical, bright, yellowish-orange upper part of a flame is due to the heating of unburned carbon particles.\n\nThe temperature of the fire and the material being burned are the factors that determine the color of the flame. The various colors of flames in a wood fire are due to the different substances in the flames.
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ever 1 mole of CO2 and one mole of H20 produces 1 mole of O2 for plants. A fire needs only one molecule of H20 to create a fire
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This is a complete combustion.\nReaction:            aX + bO2 --> dCO2 + eH2O\nd = 0.811818182, derived from mass of CO2 and its Mr.\n\nX has 0.811818182 mol of C.\n\nOriginal sample has 0.811818182/ 1.626 x 60.095\n                                  = 30.00382143mol of C
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For example, hydrogen burns in oxygen to form water vapor. \n\n2H2(g) + O2(g) -> H2O(g) \nHow much hydrogen must be burned to form 1.00 L of water vapor at 1.00 atm pressure and 3000C? \nTo work this problem, we need to figure out how many moles of water vapor we need to form. Use the ideal gas equation to compute this: \n\nPV = nRT \n1.00 atm * 1.00 L = n*0.0821 (L*atm/mol*K)* 473 K \nn = 0.0258 moles \nThus, we need to form 0.0258 moles of water. Now it's just a basic stoichiometry problem: for each mole of water formed, you need 2 moles of hydrogen gas, so 0.0258 moles water * 2 moles H2/1 mole water = 0.0516 moles of hydrogen \n\n=====================================================\n\nthis will help you a lot\n\nhttp://www.chem.hawaii.edu/asato161/Ch10NotesP2.pdf#search='Gas%20Stoichiometry%20PV%3DnRT'\n\nhttp://members.aol.com/profchm/gasstoic.html
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Vinegar is acetic acid,  CH3COOH\n\nCH3COOH + NaHCO3 ---> CH3COONa + H2CO3 (carbonic acid)\n\nThen H2CO3  gives CO2 + H2O  and CO2 will extinguish flame...Many fire extinguishers are made with compressed CO2.
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The creation and or discovery of fire.
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The explanations of fire in most standard reference works, not to put too fine a point on it, suck. The Encyclopaedia Britannica, for example, takes the following ineffectual stab: "rapid burning of combustible material with the evolution of heat and usually accompanied by flame." No wonder people have lost faith in science. Time to let a professional show how it's done. We'll start by reviewing the defects of the EB definition.\n\n(1) Rapid burning. OK, fire burns rapidly. Slow combustion, also known as oxidation, includes such nonfiery processes as rusting and digestion. However, to say that fire involves burning is to embark on a circular definition: What is fire? When something burns. What is burning? When something is on fire. We need to address the matter in more basic terms.\n\n(2) Combustible materials. Redundant. If a material is capable of rapid burning, by definition it's combustible. Also, "materials" is needlessly vague. One specific material, oxygen, is always involved.\n\n(3) Evolution of heat. I don't know what this is supposed to mean either.\n\n(4) Usually accompanied by flame. "Usually accompanied by" my arse. Flame is the quintessential pyrolytic phenomenon, not a mere by-product.\n\nNow for a proper definition, devised by myself: "Fire is the rapid combination of oxygen with fuel in the presence of heat, typically characterized by flame, a body of incandescent gas that contains and sustains the reaction and emits light and heat." Let's go through this bit by bit:\n\n(1) Rapid combination of oxygen with fuel in the presence of heat. Oxygen, fuel, and heat are the essential ingredients of fire. \n\n(2) Typically characterized by flame. The pup qualifier "typically" allows me to sidestep the issue of apparently nonflaming fires, like you get with burning charcoal. I suspect charcoal fires do create flame--you just can't see it due to the lack of impurities or incompletely burned fuel in the plume. (You can't see a fuel fire at an Indy or CART race either, because the cars run on clean-burning methanol.) But that's a matter we can leave for another day.\n\n(3) Body of incandescent gas. Flame defined. Most encyclopedia and dictionary definitions blow past this entirely, allowing persons such as yourself to imagine that fire is "pure energy" or similar nonsense. We say "body" because the gas has a characteristic structure and composition. We say "incandescent" because (a) it sounds scientific, (b) it means "luminous with intense heat," precisely what we are attempting to convey, and (c) if the Teeming Millions are going to learn one vocabulary word today, by God "incandescent" should be it.\n\n(4) Contains and sustains the reaction. Flame isn't just the result of fire; it is the fire. What's more, without the flame's heat the fire would go out.\n\n(5) Emits light and heat. Duh. However, we mustn't overlook the obvious.  \n\n>>>why do things that are put in it come out totally destroyed?\n\nOf course most things that go into fire aren’t totally destroyed. Most metals, glass, ceramic and so forth all emerge unscathed from fire. Even wood and paper aren’t totally destroyed, they leave an ash and charcoal residue as well as fine particles that we can see as soot and smoke.\n\nFire will ‘destroy’ anything organic that can be completely oxidised at the temperature that it burns at, but that is simply because the oxidation process converts the organic material to carbon dioxide,  and water. IOW the material isn’t destroyed it is just converted to gas and that gas blows away.\n\n>>>>>what fuel does it need from say, paper,\n\nThe paper IS the fuel the fire needs. The fire converts the paper into gases and ash. Or more accurately fire is the process of converting paper into gases and ash.