Posted by **Katie** on Thursday, May 17, 2012 at 11:25pm.

4. 5.6 x 10-6 mol of A and 5 x 10-5 mol of B are mixed in a 200 mL flask. The system is represented by the equation:

2A + B --> 3C

I 2.8x10-5 M 2.5x10-4 0

C -2x -x +3x

E 2.8x10-5-2x 2.5x10-4-x 3x10-5

B = 2.5x10-4-x = 2.4x10-4

x = 1x10-5

A = 2.8x10-5-2(1x10-5) = 8x10-6

C = 3x10-5 + 3(1x10-5) = 6x10-5

(6x10-5)3/ (8x10-6)2(2.4x10-4) = 14.1

At equilibrium, there is 4.8 x 10-5 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 = 5.6E-5 mols and B = 5E-5 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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