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Given the following thermochemical equations with hypothetical ΔH values: 2NH3 (g) + 3N2O (g) → 4N2 (g) + 3H2O (l)                  ΔH = -1,056 kJ 4NH3 (g) + 3O2 (g) → 2N2 (g) + 6H2O (l)                     ΔH = -1,549 kJ Calculate the value of ΔH (in kJ) for the reaction:       N2 (g) + ½ O2 (g) → N2O (g)

Given the following thermochemical equations with hypothetical ΔH values: 2NH3 (g) + 3N2O (g) → 4N2 (g) + 3H2O (l)                  ΔH = -1,056 kJ 4NH3 (g) + 3O2 (g) → 2N2 (g) + 6H2O (l)                     ΔH = -1,549 kJ Calculate the value of ΔH (in kJ) for the reaction:       N2 (g) + ½ O2 (g) → N2O (g)

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
Chapter8: Thermochemistry
Section: Chapter Questions
Problem 36QAP: Given the following thermochemical equations: 4B(s)+3O2(g)2B2O3(s)H=2543.8kJ H2(g)+12...
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Given the following thermochemical equations with hypothetical ΔH values:

2NH3 (g) + 3N2O (g) → 4N2 (g) + 3H2O (l)                  ΔH = -1,056 kJ

4NH3 (g) + 3O2 (g) → 2N2 (g) + 6H2O (l)                     ΔH = -1,549 kJ

Calculate the value of ΔH (in kJ) for the reaction:       N2 (g) + ½ O2 (g) → N2O (g)

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