Nitrogen dioxide and water react to form nitric acid and nitrogen monoxide, like this: 3 NO,(9)+H2O(1)→2 HNO3(aq)+NO(9) At a certain temperature, a chemist finds that a 6.4 L reaction vessel containing a mixture of nitrogen dioxide, water, nitric acid, and nitrogen monoxide at equilibrium has the following composition: compound amount NO, 24.5 g H,O 67.1 g HNO3 7.8 g NO 9.2 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K. %D

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Nitrogen dioxide and water react to form nitric acid and nitrogen monoxide, like this:
3 NO,(9)+H,O(1)→2 HNO3(aq)+NO(g)
At a certain temperature, a chemist finds that a 6.4 L reaction vessel containing a mixture of nitrogen dioxide, water, nitric acid, and
nitrogen monoxide at equilibrium has the following composition:
compound amount
NO2
24.5 g
H,O
67.1 g
HNO3
7.8 g
NO
9.2 g
Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits.
K
= ]
C
Transcribed Image Text:Nitrogen dioxide and water react to form nitric acid and nitrogen monoxide, like this: 3 NO,(9)+H,O(1)→2 HNO3(aq)+NO(g) At a certain temperature, a chemist finds that a 6.4 L reaction vessel containing a mixture of nitrogen dioxide, water, nitric acid, and nitrogen monoxide at equilibrium has the following composition: compound amount NO2 24.5 g H,O 67.1 g HNO3 7.8 g NO 9.2 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K = ] C
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