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

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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

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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5. Note: Please don't write on a paper. I can't understand handwrittens.
2 NH3 (g) + 2 O2 (g) → N20 (g) + 3 H2O (g) Is this reaction spontaneous only at low temperatures, only at high temperatures, at all temperatures? AH°r, kJ/mol s°, J/mol·K NH3(g) -46.1 192.5 0:(g) 205.0 N 20 (g) 82.1 219.9 H2O(g) |-241.8 188.7 AH°i, kJ/mol s°, J/mol·K What is the lowest temperature at which the following reaction is spontaneous? H2O (g) + C (s) → H2 (g) + CO (g) Co(g) H2(g) C (s) -110.5 | 197.7 130.6 5.7 H2O(g) |-241.8 188.7
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