Top topic this week
Back to FAQs
Related FAQs
Frequently Asked Question
Questions asked by users might not always be phrased in the clearest way.
The equilibrium constant for the following reaction is 1.29×10-2 at 600k.rnrncocl2(g) CO(g) + Cl2(g)rnrnIf an equilibrium mixture of the three gases in a 11.4 l container at 600k contains 0.499 mol of COCl2(g) and 0.266 mol of CO, the equilibrium concentration of Cl2 is rn m.
Accepted Answer
The equilibrium constant expression for the given reaction is:
Kc = [CO][Cl2]/[COCl2]
Substituting the given values into the equilibrium constant expression:
1.29×10-2 = [CO][Cl2]/[COCl2]
1.29×10-2 = (0.266 M )[Cl2]/(0.499 M )
[Cl2] = (1.29×10-2)(0.499 M )/0.266 M
[Cl2] = 2.50×10-2 M
Therefore, the equilibrium concentration of Cl2 is 2.50×10-2 M.
Articles you might like