Nitrogen monoxide and water react to form ammonia and oxygen, like this: 4 NO(g) + 6 H,O(g) → 4 NH3(g) + 50,(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of nitrogen monoxide, water, ammonia, and oxygen has the following composition: compound concentration at equilibrium NO 0.94 M H,O 1.5 M NH3 1.2 M 02 0.90 M Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits.
Nitrogen monoxide and water react to form ammonia and oxygen, like this: 4 NO(g) + 6 H,O(g) → 4 NH3(g) + 50,(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of nitrogen monoxide, water, ammonia, and oxygen has the following composition: compound concentration at equilibrium NO 0.94 M H,O 1.5 M NH3 1.2 M 02 0.90 M Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits.
Introductory Chemistry: A Foundation
8th Edition
ISBN:9781285199030
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter17: Equilibrium
Section: Chapter Questions
Problem 20QAP
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Transcribed Image Text:Nitrogen monoxide and water react to form ammonia and oxygen, like this:
4 NO(g) + 6 H,O(g) → 4 NH3(g) + 50,(g)
Also, a chemist finds that at a certain temperature the equilibrium mixture of nitrogen monoxide, water, ammonia, and oxygen has the following composition:
compound concentration at equilibrium
NO
0.94 M
H,O
1.5 M
NH3
1.2 M
02
0.90 M
Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits.
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