linked - Investigating the Terror
linked - Investigating the Terror
linked - Investigating the Terror
Create successful ePaper yourself
Turn your PDF publications into a flip-book with our unique Google optimized e-Paper software.
pounds of urea and 1694 pounds of nitric acid were missing. See G.Ex.<br />
862. Using <strong>the</strong>se figures and Jourdan's basic methodology, a proper<br />
stoichiometric calculation would be as follows: Jourdan assumed, as we<br />
will do here, that <strong>the</strong> concentration of <strong>the</strong> urea was 100% and <strong>the</strong> average<br />
concentration of <strong>the</strong> nitric acid was 68.7%. A quantity of 1694 pounds of<br />
68.7% nitric acid is <strong>the</strong> equivalent of 1164 (1694 x .687) pounds of 100%<br />
nitric acid. Since, as noted above, 63 pounds of nitric acid is needed for<br />
every 60 pounds of urea, 1164 pounds of 100% nitric acid is inadequate<br />
to achieve a complete reaction of 1200 pounds of 100% urea. Accordingly,<br />
<strong>the</strong> nitric acid was <strong>the</strong> limiting reagent.<br />
For every 63 pounds of completely reacted nitric acid, 123 pounds of urea<br />
nitrate is <strong>the</strong>oretically (100% yield) produced. Therefore, with a 100%<br />
yield, 1164 pounds of nitric acid would produce 2273 pounds of urea<br />
nitrate. A 97% yield, as obtained by Molnar, would produce 2205 pounds<br />
of urea nitrate.<br />
c. Williams' Salameh Testimony<br />
In his testimony in <strong>the</strong> Salameh trial, Williams was asked to calculate how<br />
much urea nitrate could be produced from <strong>the</strong> missing urea and nitric<br />
acid. Williams first addressed <strong>the</strong> concept of a limiting reagent:<br />
Whenever you have a reaction like this, <strong>the</strong>re is a limiting<br />
reagent when you mix two things toge<strong>the</strong>r. You can only go so<br />
far because one of <strong>the</strong> components limits <strong>the</strong> quantities that<br />
you're going to have.<br />
In <strong>the</strong> case of manufacturing urea nitrate, urea is <strong>the</strong> limiting<br />
factor. So, you'd always want to add a little bit more nitric acid<br />
than <strong>the</strong> recipe calls for to make sure that you've reacted all <strong>the</strong><br />
urea.<br />
Next, Williams addressed <strong>the</strong> issue of yield. He testified that in a<br />
laboratory type environment <strong>the</strong> [b]est case scenario would be in <strong>the</strong><br />
neighborhood of 90 percent. He <strong>the</strong>n testified: