**Consider the reaction:**\[ 3\text{Fe}_2\text{O}_3 (s) + \text{H}_2 (g) \rightarrow 2\text{Fe}_3\text{O}_4 (s) + \text{H}_2\text{O} (g) \]Using standard absolute entropies at 298 K, calculate the entropy change for the system when 1.58 moles of Fe₂O₃(s) react at standard conditions.| Substance | \( S^\circ \) (J/K·mol) ||------------|-------------------------|| Fe₂O₃(s) | 87.4 || H₂(g) | 130.7 || Fe₃O₄(s) | 146.4 || H₂O(g) | 188.8 |\[ \Delta S^\circ_{\text{system}} = \boxed{} \text{J/K} \]**Explanation:**The provided table lists the standard absolute entropies (\( S^\circ \)) for each substance involved in the reaction. The task is to calculate the entropy change of the system (\( \Delta S^\circ_{\text{system}} \)) using the given entropies at 298 K when 1.58 moles of Fe₂O₃(s) react.

Answered: Image /qna-images/answer/aa2aeedb-8ed9-4754-a461-eab54f9d1b6d.jpg

the reaction: 3Fe2O3 (s) + H₂(g) → 2Fe3O4 (s) + H₂O(g) Using standard absolute entropies at 298 K, calculate the entropy change for the system when 1.58 moles of Fe2O3 (8) react at standard conditions. AS⁰ Substance S (J/K mol) Fe₂O3 (8) 87.4 H₂(g) 130.7 Fe3O4(s) 146.4 H₂O(g) 188.8 system J/K 4

the reaction: 3Fe2O3 (s) + H₂(g) → 2Fe3O4 (s) + H₂O(g) Using standard absolute entropies at 298 K, calculate the entropy change for the system when 1.58 moles of Fe2O3 (8) react at standard conditions. AS⁰ Substance S (J/K mol) Fe₂O3 (8) 87.4 H₂(g) 130.7 Fe3O4(s) 146.4 H₂O(g) 188.8 system J/K 4

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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