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The first step in HNO3 production is the catalyzed oxidation of NH3. Without a catalyst, a different reaction predominates: 4NH3(g) + 30,(g) = 2N2(g) + 6H₂O(g) When 0.0150 mol of NH3 (g) and 0.0150 mol of O2 (g) are placed in a 1.00-L container at a certain temperature, the N₂ concentration at equilibrium is 1.58 x 10 M.

The first step in HNO3 production is the catalyzed oxidation of NH3. Without a catalyst, a different reaction predominates: 4NH3(g) + 30,(g) = 2N2(g) + 6H₂O(g) When 0.0150 mol of NH3 (g) and 0.0150 mol of O2 (g) are placed in a 1.00-L container at a certain temperature, the N₂ concentration at equilibrium is 1.58 x 10 M.

Chemistry: Principles and Reactions
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 32QAP: Consider the following reaction at 75C: 3R(s)+2Q(g)A(g)+5B(l)K=9.4 A 10.0-L sample contains 0.30 mol...
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Calculate Kc using correct significant figures. Information is in the image.

The first step in HNO3 production is the catalyzed oxidation of NH3. Without a catalyst, a different reaction predominates: 4NH3(g) + 302(g) = 2N2(g) + 6H₂O (g) When 0.0150 mol of NH3 (g) and 0.0150 mol of O2 (g) are placed in a 1.00-L container at a certain temperature, the N2 concentration at equilibrium is 3 1.58 × 10 M.
Transcribed Image Text:The first step in HNO3 production is the catalyzed oxidation of NH3. Without a catalyst, a different reaction predominates: 4NH3(g) + 302(g) = 2N2(g) + 6H₂O (g) When 0.0150 mol of NH3 (g) and 0.0150 mol of O2 (g) are placed in a 1.00-L container at a certain temperature, the N2 concentration at equilibrium is 3 1.58 × 10 M.
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