Nitrogen and water react to form nitrogen monoxide and hydrogen, like this: N2(9) + 2 H,O(g) - 2 NO(g) + 2 H,(9) Also, a chemist finds that at a certain temperature the equilibrium mixture of nitrogen, water, nitrogen monoxide, and hydrogen has the following composition: compound concentration at equilibrium N2 0.78M H,O 1.5M NO 1.0M H, 1.6M Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = 0

Nitrogen and water react to form nitrogen monoxide and hydrogen, like this: N2(9) + 2 H,O(g) - 2 NO(g) + 2 H,(9) Also, a chemist finds that at a certain temperature the equilibrium mixture of nitrogen, water, nitrogen monoxide, and hydrogen has the following composition: compound concentration at equilibrium N2 0.78M H,O 1.5M NO 1.0M H, 1.6M Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = 0

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter12: Gaseous Chemical Equilibrium

Section: Chapter Questions

Problem 34QAP: At 500C, k for the for the formation of ammonia from nitrogen and hydrogen gases is 1.5105....

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At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g) (a) Analysis shows that the concentrations of N2 and O2 are both 0.25 M, and that of NO is 0.0042 M under certain conditions. Is the system at equilibrium? (b) If the system is not at equilibrium, in which direction does the reaction proceed? (c) When the system is at equilibrium, what are the equilibrium concentrations?
. Ammonia. a very important industrial chemical. is produced by the direct combination of the following elements under carefully controlled conditions: N2(g)+3H2(g)2NH3(g)Suppose. in an experiment, that the reaction mixture is analyzed after equilibrium is reached, and it is found, at a particular temperature. that [NH3]=0.25M,[H2]=3.4103M, and [N2]=5.3105M. Calculate the value of K at this temperature.
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The atmosphere consists of about 80% N2 and 20% O2, yet there are many oxides of nitrogen that are stable and can be isolated in the laboratory. (a) Is the atmosphere at chemical equilibrium with respect to forming NO? (b) If not, why doesnt NO form? If so, how is it that NO can be made and kept in the laboratory for long periods?
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