Consider the reaction:2NH3(g) + 3N₂O(g) → 4N₂ (g) + 3H₂O(g)Using standard absolute entropies at 298 K, calculate the entropy change for the system when 1.54 moles of NH3(g) react at standardconditions.AS⁰⁰systemSubstance So (J/K mol)NH3 (9)192.5219.9191.6188.8N₂O(g)N₂ (9)H₂O(g)J/K Consider the reaction:2BrF3 (9) → Br₂(g) + 3F2 (g)Using standard absolute entropies at 298 K, calculate the entropy change for the system when 2.27 moles of BrF3 (g) react at standardconditions.AsosystemSubstance SoBr₂(g)F₂(g)BrF3 (9)J/KJK. mol245.5202.8292.5

Answered: Image /qna-images/answer/c4ee690b-78f3-4dee-b592-26940d5e2e15.jpg

Consider the reaction: 2NH3(g) + 3N₂O(g) → 4N2₂ (g) + 3H₂O(g) Using standard absolute entropies at 298 K, calculate the entropy change for the system when 1.54 moles of NH3(g) react at standard conditions. AS⁰ system Substance So (J/K mol) NH3 (9) 192.5 N₂O(g) 219.9 N₂ (9) 191.6 H₂O(g) 188.8 J/K

Consider the reaction: 2NH3(g) + 3N₂O(g) → 4N2₂ (g) + 3H₂O(g) Using standard absolute entropies at 298 K, calculate the entropy change for the system when 1.54 moles of NH3(g) react at standard conditions. AS⁰ system Substance So (J/K mol) NH3 (9) 192.5 N₂O(g) 219.9 N₂ (9) 191.6 H₂O(g) 188.8 J/K

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter17: Chemcial Thermodynamics

Section: Chapter Questions

Problem 17.70QE: What is the sign of the standard Gibbs free-energy change at low temperatures and at high...

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