N2(g) +O2(g) 2NÓ(g) The equilibrium constant K for this reaction is 0.857 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places.
N2(g) +O2(g) 2NÓ(g) The equilibrium constant K for this reaction is 0.857 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places.
General Chemistry - Standalone book (MindTap Course List)
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ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter14: Chemical Equilibirum
Section: Chapter Questions
Problem 14.19QP: During an experiment with the Haber process, a researcher put 1 mol N2 and 1 mol H2 into a reaction...
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![Suppose a 500. mL flask is filled with 1.5 mol of O, and 1.7 mol of NO. The following reaction becomes possible:
N,(g) +O,(g) - 2NO (g)
The equilibrium constant K for this reaction is 0.857 at the temperature of the flask.
Calculate the equilibrium molarity of NO. Round your answer to two decimal places.
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Transcribed Image Text:Suppose a 500. mL flask is filled with 1.5 mol of O, and 1.7 mol of NO. The following reaction becomes possible:
N,(g) +O,(g) - 2NO (g)
The equilibrium constant K for this reaction is 0.857 at the temperature of the flask.
Calculate the equilibrium molarity of NO. Round your answer to two decimal places.
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Continue
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