Mercury(II) oxide decomposes to form mercury and oxygen, like this: 2HgO(s)Hg(l) + O2(g)
At a certain temperature, a chemist finds that a reaction vessel containing a mixture of mercury(II) oxide, mercury, and oxygen at equilibrium has the following composition:
compound amount
HgO 24.0g
Hg 23.6g
O2 22.7g
Calculate the value of the equilibrium constant for this reaction. Round your answer to significant digits.

Explanation:

Hello,

In this case, since the equilibrium constant is written including gaseous and aqueous species only, for this reaction, it is:

Thus, since the volume is missing, we are going to assume 1 L, but you can change it based on the one you are given, thus, the concentration of oxygen at equilibrium is:

It means, that the equilibrium constant, with two significant figures is:

Best regards.

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