29. A researcher fills a 1.00 L reaction vessel with 1.84 x 10-4 mol of BrCl gas and heats it to 500 K. At equilibrium, only 18.3 % of the BrCl gas remains. Calculate the equilibrium constant, assuming the following reaction is taking place.
2BrCl(g) ⇌ Br2 (g) + Cl2(g)
I keep getting 1.68 x 10^-4, but it's wrong. Can someone explain what the right answer is and how to get it?
Chem Equilibrium Module 3 #29 [ENDORSED]
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