Wednesday
April 16, 2014

Homework Help: Chemistry

Posted by Scott L. on Sunday, May 23, 2010 at 9:07pm.

At a particular temp, K = 1.6 x 10^-5 for the reaction:
2SO3(g) <-> 2SO2(g) + O2 (g)
If 4 mol of SO2 and 2 mol of O2 are placed into a 2.0L flask, calculate the equilibrium concentrations of all species.

I set up an ICE table with SO3 to start with 0M and SO2 to start with 2M and O2 with 1M.
At equilibrium, I got SO3 = 2x, SO2 = 2-2x, and O2 = 1-x.
After I got:
1.6 x 10^-5 = [(2-2x)^2 (1-x)]/(2x)^2

After that do I just solve for x? If so, is there an faster way to determine x because that looks a bit complex. Thanks

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