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Thread: Aluminothermic Reactions

  1. #1 Aluminothermic Reactions 
    Forum Isotope
    Join Date
    Feb 2009
    Reading up a bit on the fantastic pyrotechnic reaction, I'm terribly curious, how do you calculate the amount of energy produced by the reaction, given different compositions?
    Quote Originally Posted by wiki
    Thermites can be a diverse class of compositions. The fuels are often aluminium, magnesium, calcium, titanium, zinc, silicon, and boron. The oxidizers can be boron(III) oxide, silicon(IV) oxide, chromium(III) oxide, manganese(IV) oxide, iron(III) oxide, iron(II,III) oxide, copper(II) oxide, and lead(II,III,IV) oxide.[1]
    The fact that there are multiple fuel-oxidizer combinations has given me a lot to be curious about, and it made me wonder how you would go about figuring out how much energy is produced from, say, silicon and iron(II,III) oxide.

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  3. #2  
    Forum Professor
    Join Date
    May 2005
    You should be able to figure it out easily by looking at the standard enthalpies of formation for the metal oxide and silicon (or whatever). I would try googling for "stand enthalpy of formation tables" or something similar. Just subtract the standard enthalpy of formation of the products from that of the reactant, and you get the energy released.

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