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?

Answers

Answer 1

Answer:

[IBr] = 0.049 M.

Explanation:

Hello there!

In this case, according to the balanced chemical reaction:

[tex]I_2+Br_2\rightarrow 2IBr[/tex]

It is possible to set up the following equilibrium expression:

[tex]K=\frac{[IBr]^2}{[I_2][Br_2]} =0.0110[/tex]

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

[tex]0.0110=\frac{(2x)^2}{(0.50-x)^2}[/tex]

Which can be solved for [tex]x[/tex] to obtain two possible results:

[tex]x_1=-0.0277M\\\\x_2=0.0245M[/tex]

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

[tex][IBr]=2x=2*0.0249M=0.049M[/tex]

Regards!


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