posted by Katie on .
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?
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.
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.