Pyrophoric
April 16th, 2004, 04:45 AM
Having recently made KClO3 quite successfully by electrolysis (another story) I was looking around for some basic compositions on the PFP that would give results indeed proving that I had made KClO3....I found three charcoal/sulfur/chlorate mixtures listed - all with quite different reactant ratios. I simply chose one, specifically KClO3:60% S:30% C:10% I was quite unimpressed by the burn rate of this comp produced by mixing the reactants that had beforehand been crushed by a spoon. The mix also had much residue left over after burning, however it did explode when given a firm whack with a hammer. I decided that this mixture could be improved.
So in an effort to optimise the mixture I assumed the greatest amount of energy would be released when the products of the reaction consisted of CO, KCl, SO2 - that is species with the highest possible inter-atomic bond strength. [Not knowing the exact bond enthalpies I may be wrong! Can someone correct me on this?]
Using this information I came up with a few equations describing the mass ratio of the reactants required to produce only the before mentioned products (not in any particular ratio though). Below is a table of selected values taken from the graph generated from the equations. An infinite number of combinations are possible by basically varying the ratio of carbon to sulfur. X is just an arbitrary value used to define different mole ratios. Ratios are expressed as a fraction of unity.
graph can be found here (http://www.geocities.com/pyrophoric_me/KClO3z.gif) (right click and save as)
Equation(s):
(18x-36)/(79x+12)=y (1)
(48)/(79x+12)=y (2)
(61*x)/(79x+12)=y (3)
x.............Carbon....Sulfur.....KClO3
---------------------------------------------
2.0..........0...........0.28235..0.71765
3.0..........0.07229..0.19277..0.73494
4.0..........0.10976..0.14634..0.7439
5.0..........0.13268..0.11794..0.74939
6.0..........0.14815..0.09877 0.75309
7.0..........0.15929..0.08496..0.75575 <=chosen mix
8.0..........0.1677....0.07453..0.75776
9.0......... 0.17427..0.06639..0.75934
10.0........0.17955...0.05985..0.7606
11.0........0.18388...0.05448..0.76163
12.0........0.1875.....0.05.......0.7625
13.0........0.19057...0.0462....0.76323
14.0........0.1932.....0.04293 0.76386
15.0........0.19549...0.0401....0.76441
---------------------------------------------
You can see the mix ranges from zero carbon and a large quantity of sulfur, to (when x = infinity) zero sulfur and a large proportion of carbon. Change in enthalpy is going to be increasing as x increases due to a greater proportion of the fuel being in the form of carbon. I simply picked one result which "looked" like it still had enough sulfur to catalyse the reaction, while still maintaining a large portion of carbon - which is going to release more energy per atom of oxygen than sulfur. This assumption had to be made as there is no other way, other than by experiment to determine which is the optimum tradoff between reaction rate and change in reaction entahlpy. The measured reactants were crushed up with the back of a spoon and mixed. The resulting meal powder burnt MANY times faster than the original comp (couldn't get a quantitative measurement as only was a 2 gram sample) it infact flashed like fine grain commercial black powder and left very little residue (just a thin white coating). Surprisingly this mixture, despite it's fierce burn rate, failed to explode when struck with a hammer - only quietly deflagrated - probably due to comparatively low sulfur content. If I ever get around to it I might measure the burn rates of some other points on the graph to find the optimal value. Both test mixtures were made from the same batch of chemicals and all reactants were measured down to 1/10mg.
After the success of my method of analysis I then tried it on KNO3/S/C mix (black powder)
Graph here (http://www.geocities.com/pyrophoric_me/KNO3z.gif) (right click and save as)
Equation(s):
(30x-72)/(131x+24)=y (1)
(96)/(131x+24)=y (2)
(101x)/(131x+24)=y (3)
x...........Carbon.....Sulfur......KNO3
--------------------------------------------
3.0.........0.04317..0.23022..0.72662
4.0.........0.08759..0.17518..0.73723
5.0.........0.11487..0.14138..0.74374
6.0.........0.13333..0.11852..0.74815
7.0.........0.14665..0.10202..0.75133 <=common formulation :D
8.0.........0.15672..0.08955..0.75373
9.0.........0.16459..0.0798....0.75561
10.0.......0.17091..0.07196...0.75712
11.0.......0.17611..0.06553...0.75836
12.0.......0.18045..0.06015...0.7594
13.0.......0.18413..0.05559...0.76028
14.0.......0.1873....0.05167...0.76103
15.0.......0.19005..0.04827...0.76169
---------------------------------------------
To my surprise one of my datapoints matched very closely to the common 75:15:10 mix.
Now you may be asking what the purpose of all these graphs were? Well if you had a composition from a database that could not be fitted to graph generated for that mixture you would know that the products of the reaction cannot be solely the products with the highest possible bond enthalpies used to generate the graph. Hence the mixture is not optimised, as some of the energy generated during the reaction would be going into decomposing/vaporising material that would not add to the energy produced during the reaction. We can see that a common formulation for blackpowder agrees very well with the graph and therefore it must be close to optimal. These graphs would also simplify the task of finding the optimal ratio as only one vaiable has to be changed - namely x. The original composition pulled from the PFP database does not even approximate the graph at any point and therefore it must be quite far from optimal.
It would be interesting to see how the overall change in enthapy ranges as the mixture varies (need data for that).
Now all we need is a way to predict rate of reaction and we could predict the optimum mix for any reactants!
Apologies if this was all a waste of time.
So in an effort to optimise the mixture I assumed the greatest amount of energy would be released when the products of the reaction consisted of CO, KCl, SO2 - that is species with the highest possible inter-atomic bond strength. [Not knowing the exact bond enthalpies I may be wrong! Can someone correct me on this?]
Using this information I came up with a few equations describing the mass ratio of the reactants required to produce only the before mentioned products (not in any particular ratio though). Below is a table of selected values taken from the graph generated from the equations. An infinite number of combinations are possible by basically varying the ratio of carbon to sulfur. X is just an arbitrary value used to define different mole ratios. Ratios are expressed as a fraction of unity.
graph can be found here (http://www.geocities.com/pyrophoric_me/KClO3z.gif) (right click and save as)
Equation(s):
(18x-36)/(79x+12)=y (1)
(48)/(79x+12)=y (2)
(61*x)/(79x+12)=y (3)
x.............Carbon....Sulfur.....KClO3
---------------------------------------------
2.0..........0...........0.28235..0.71765
3.0..........0.07229..0.19277..0.73494
4.0..........0.10976..0.14634..0.7439
5.0..........0.13268..0.11794..0.74939
6.0..........0.14815..0.09877 0.75309
7.0..........0.15929..0.08496..0.75575 <=chosen mix
8.0..........0.1677....0.07453..0.75776
9.0......... 0.17427..0.06639..0.75934
10.0........0.17955...0.05985..0.7606
11.0........0.18388...0.05448..0.76163
12.0........0.1875.....0.05.......0.7625
13.0........0.19057...0.0462....0.76323
14.0........0.1932.....0.04293 0.76386
15.0........0.19549...0.0401....0.76441
---------------------------------------------
You can see the mix ranges from zero carbon and a large quantity of sulfur, to (when x = infinity) zero sulfur and a large proportion of carbon. Change in enthalpy is going to be increasing as x increases due to a greater proportion of the fuel being in the form of carbon. I simply picked one result which "looked" like it still had enough sulfur to catalyse the reaction, while still maintaining a large portion of carbon - which is going to release more energy per atom of oxygen than sulfur. This assumption had to be made as there is no other way, other than by experiment to determine which is the optimum tradoff between reaction rate and change in reaction entahlpy. The measured reactants were crushed up with the back of a spoon and mixed. The resulting meal powder burnt MANY times faster than the original comp (couldn't get a quantitative measurement as only was a 2 gram sample) it infact flashed like fine grain commercial black powder and left very little residue (just a thin white coating). Surprisingly this mixture, despite it's fierce burn rate, failed to explode when struck with a hammer - only quietly deflagrated - probably due to comparatively low sulfur content. If I ever get around to it I might measure the burn rates of some other points on the graph to find the optimal value. Both test mixtures were made from the same batch of chemicals and all reactants were measured down to 1/10mg.
After the success of my method of analysis I then tried it on KNO3/S/C mix (black powder)
Graph here (http://www.geocities.com/pyrophoric_me/KNO3z.gif) (right click and save as)
Equation(s):
(30x-72)/(131x+24)=y (1)
(96)/(131x+24)=y (2)
(101x)/(131x+24)=y (3)
x...........Carbon.....Sulfur......KNO3
--------------------------------------------
3.0.........0.04317..0.23022..0.72662
4.0.........0.08759..0.17518..0.73723
5.0.........0.11487..0.14138..0.74374
6.0.........0.13333..0.11852..0.74815
7.0.........0.14665..0.10202..0.75133 <=common formulation :D
8.0.........0.15672..0.08955..0.75373
9.0.........0.16459..0.0798....0.75561
10.0.......0.17091..0.07196...0.75712
11.0.......0.17611..0.06553...0.75836
12.0.......0.18045..0.06015...0.7594
13.0.......0.18413..0.05559...0.76028
14.0.......0.1873....0.05167...0.76103
15.0.......0.19005..0.04827...0.76169
---------------------------------------------
To my surprise one of my datapoints matched very closely to the common 75:15:10 mix.
Now you may be asking what the purpose of all these graphs were? Well if you had a composition from a database that could not be fitted to graph generated for that mixture you would know that the products of the reaction cannot be solely the products with the highest possible bond enthalpies used to generate the graph. Hence the mixture is not optimised, as some of the energy generated during the reaction would be going into decomposing/vaporising material that would not add to the energy produced during the reaction. We can see that a common formulation for blackpowder agrees very well with the graph and therefore it must be close to optimal. These graphs would also simplify the task of finding the optimal ratio as only one vaiable has to be changed - namely x. The original composition pulled from the PFP database does not even approximate the graph at any point and therefore it must be quite far from optimal.
It would be interesting to see how the overall change in enthapy ranges as the mixture varies (need data for that).
Now all we need is a way to predict rate of reaction and we could predict the optimum mix for any reactants!
Apologies if this was all a waste of time.