Re: How are explosions proportional?
basically what I was wondering how the proportions of an explosion are related to scale.
Oooh! Oooh! I know! I know!!
For the rant in this post, we'll be considering an overidealized detonation - a shockwave traveling in perfect vacum (itself a self-contradiction, but meh), always arising from the detonation of a mathematical point of zero volume. Also impossible, but hey - the simplified crap makes the basics easier.
Now... there are two factors at play here.
The first, of course, is starting energy. The arrangement of a molecule from a less-stable form to more-stable byproducts tends to release a fixed amount of energy, and if you're really damned lucky, it may even do this over a fairly-reproducible period of time.
It's that last which is a doozy, and why dustbombs explode for substances which barely smoulder - moar surface area = less time of combustion.
But... just for the fuck of it, let's say that degradation occurs simultaneously across all parts of a sample in a known and reproducible time frame. In this case, you're getting a given unit of energy in a given time period for each molecule of said substance, 'n it's going to basically scale exactly like that... in the ideal sense, anyways.
The other factor you mentioned was, well... distance. 'n for that, you've got to recognize that the energy calculated from the first factor - let's assume it was released instantaneously - is spread out across a given area, and that area is the surface area of a three-dimensional sphere of the radius between one's point of measurement and the theoretical point of detonation.
So... let's take a theoretical "explosive"... the conversion of 2(HNO3) into H2 + N2 + 3(O2), shall we?
Looking (http://www.cem.msu.edu/~reusch/VirtualText/react2.htm) at the bond energies, we find that the N=O bond, for which we have two of the buggers per molecule, is 143kcal/mol, or 143 * 2 * 2 = 572kcal for both of 'em, while the N-O bond is 55kcal, or 110kcal for both, and the H-O bond is 110kcal, or 220 for both.
This leaves a starting bond energy of 572 + 110 + 220, or 902kcal for 2 mol of H-O-N(=O)2.
So, what are the ending products? Well, like a bastard, we're not even calculating the 2(H2) + O2 -> H2O exothermogenesis, because... we suck. Yeah. So, O2 is 119kcal, or 357kcal for all three, H2 is 104.2kcal, and we'll just call it 104, and N2 is probably the 226kcal n=n configuration, but who knows?
902-687 = 215kcal per 2 mols degradation of nitric acid, or 107.5kcal/mol... not counting the formation of H2O. Continuing senselessly to ignore that, the theoretical energy per square unit in a truly-instantaneous degredation from a theoretical zero-volume point of detonation would end up being somewhere along the lines of (107.5 * mol)/(4pi*r^2) kcal/unit_of_volume_squared.
Plus the ensuing hydrogen explosion... but hey, we're not counting that.
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