Ammonia and oxygen react to form nitrogen monoxide and water, like this: 4 NH3(9) + 50,(g) → 4 NO(g) + 6 H,O(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of ammonia, oxygen, nitrogen monoxide, and water has the following composition: compound pressure at equilibrium NH3 23.4 atm O2 40.2 atm NO 87.8 atm H,O 63.4 atm Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits.

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Ammonia and oxygen react to form nitrogen monoxide and water, like this:
4 NH3(g) + 502(g) →
4 NO(g) + 6H,O(g)
Also, a chemist finds that at a certain temperature the equilibrium mixture of ammonia, oxygen, nitrogen monoxide, and water has the following composition:
compound pressure at equilibrium
NH3
23.4 atm
O2
40.2 atm
NO
87.8 atm
H,0
63.4 atm
Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits.
Transcribed Image Text:Ammonia and oxygen react to form nitrogen monoxide and water, like this: 4 NH3(g) + 502(g) → 4 NO(g) + 6H,O(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of ammonia, oxygen, nitrogen monoxide, and water has the following composition: compound pressure at equilibrium NH3 23.4 atm O2 40.2 atm NO 87.8 atm H,0 63.4 atm Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits.
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