Re: chemistry class problem

From: Abast44 (abast44_at_aol.com)
Date: 11/07/04 

Date: 07 Nov 2004 19:00:21 GMT

>From the information you've given me, it looks like you're just supposed to
apply Le Chatlier's principle to each case, not grind out numerical answers.
Obviously, it would have been nice to have values of K...but that would have
rendered the problem completely trivial. As you know, for a system at
equilibrium, adding more reactant will cause the conversion to product to
increase and vice versa until said equilibrium is reestablished.

For the first case (eq. conc. of D), the order should be II,I,III. You'll get
the most amount from rxn. III as the 2 moles of A (and the lack of any products
to start with) will drive the reaction strongly to the right. Rxn I is just
like the last case, but won't go to the right as stongly, due to decreased
amount (well, technically concentration...but you know that M = mol/L) of A. II
will form the least amount of D, as now you have some product initially, so
equilibrium will have to be established with the initial 0.2 moles of C, which
will drive down the total amount of D that is formed. The second case is just
like the first, but reversed (III,I,II). Just apply similiar reasoning as I did
for that one and you'll have your explanation.

Also, I just found a webpage that has a java applet that'll let you play with
conditions for a reaction. Maybe it'll help you get more of a grasp on chemical
equilibrium.
http://www.chm.davidson.edu/java/lechatelier/lechatelier.html

Hope this helps!
-Shane

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