Posted by Katie on Thursday, May 17, 2012 at 11:25pm.
4. 5.6 x 106 mol of A and 5 x 105 mol of B are mixed in a 200 mL flask. The system is represented by the equation:
2A + B > 3C
I 2.8x105 M 2.5x104 0
C 2x x +3x
E 2.8x1052x 2.5x104x 3x105
B = 2.5x104x = 2.4x104
x = 1x105
A = 2.8x1052(1x105) = 8x106
C = 3x105 + 3(1x105) = 6x105
(6x105)3/ (8x106)2(2.4x104) = 14.1
At equilibrium, there is 4.8 x 105 mol of B. Calculate the value of the equilibrium constant.
Where have I gone wrong?

Chemistry  DrBob222, Thursday, May 17, 2012 at 11:31pm
The problem tells you that A = 5.6E5 mols and B = 5E5 mol. You've changed both. Why do that? You didn't do it on the other problem.

Chemistry  Katie, Thursday, May 17, 2012 at 11:35pm
I did a rough answer to this question with my tutor earlier today and I see what you're saying with the switching, I'm having issues understanding how to do this one properly.
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