Mercury(II) oxide decomposes to form mercury and oxygen, like this: 2 HgO(s)→2 Hg(1) + O₂(g) At a certain temperature, a chemist finds that a 7.5 L reaction vessel containing a mixture of mercury(II) oxide, mercury, and oxygen at equilibrium has the following composition: compound amount HgO 20.7 g Hg 7.7 g 0₂ 10.5 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. =0 K = x10 X

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Mercury(II) oxide decomposes to form mercury and oxygen, like this:
2 HgO(s) 2 Hg(1) + O₂(g)
At a certain temperature, a chemist finds that a 7.5 L reaction vessel containing a mixture of mercury(II) oxide, mercury, and oxygen at equilibrium has the
following composition:
K
compound amount
HgO
20.7 g
7.7 g
10.5 g
Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits.
с
с
Hg
0₂
0
x10
X
S
Transcribed Image Text:Mercury(II) oxide decomposes to form mercury and oxygen, like this: 2 HgO(s) 2 Hg(1) + O₂(g) At a certain temperature, a chemist finds that a 7.5 L reaction vessel containing a mixture of mercury(II) oxide, mercury, and oxygen at equilibrium has the following composition: K compound amount HgO 20.7 g 7.7 g 10.5 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. с с Hg 0₂ 0 x10 X S
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