A sealed 1.0L flask is filled with 0.500 mols of I_2 and 0.500 mols of Br_2. When the container achieves equilibrium the equilibrium constant is 1.10x10^{-2}. What is the equilibrium concentration of the product, IBr?

[IBr] = 0.049 M.

Explanation:

Hello there!

In this case, according to the balanced chemical reaction:

It is possible to set up the following equilibrium expression:

Whereas the the initial concentrations of both iodine and bromine are 0.50 M; and in terms of (reaction extent) would be:

Which can be solved for to obtain two possible results:

Whereas the correct result is 0.0245 M since negative results does not make any sense. Thus, the concentration of the product turns out:

Regards!

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