Ammonia and oxygen react to form nitrogen monoxide and water, like this: 4 NH3(g) + 50,(9) → 4 NO(9) + 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 34.1 atm O2 99.2 atm NO 98.5 atm H,0 34.4 atm Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K, = 0
Ammonia and oxygen react to form nitrogen monoxide and water, like this: 4 NH3(g) + 50,(9) → 4 NO(9) + 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 34.1 atm O2 99.2 atm NO 98.5 atm H,0 34.4 atm 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 38QAP: Nitrogen dioxide can decompose to nitrogen oxide and oxygen. 2NO2(g)2NO(g)+O2(g) K is 0.87 at a...
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